AP Chemistry 2014-2015 CH 7 ATOMIC STRUCTURE AND PERIODICITY.
AP* Chemistry ATOMIC STRUCTURE - Lundquist Labs · AP* Chemistry ATOMIC STRUCTURE *AP is a...
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AP* Chemistry ATOMIC STRUCTURE *AP is a registered trademark of the College Board, which was not involved in the production of, and does not endorse, this product. © 2008 by René McCormick. All rights reserved. ELECTROMAGNETIC RADIATION James Maxwell developed an elegant mathematical theory in 1864 to describe all forms of radiation in terms of oscillating or wave-like electric and magnetic fields in space. • electromagnetic radiation —UV, visible light, IR, microwaves, television and radio signals, and X-rays • wavelength (λ) —(lambda) length between 2 successive crests. • frequency (υ) —(nu in chemistry; f in physics—either is OK), number of cycles per second that pass a certain point in space (Hz-cycles per second) • amplitude —maximum height of a wave as measured from the axis of propagation • nodes —points of zero amplitude (equilibrium position); always occur at λ/2 for sinusoidal waves velocity —speed of the wave velocity = λ υ “c”—the speed of light; 2.99792458 [just call it 3] × 10 8 m/s; ALL EM RADIATION TRAVELS AT THIS SPEED! I call it easy, you’ll call it a trick! If “light” is involved, it travels at 3 × 10 8 m/s • Notice that λ and υ are inversely proportional. When one is large, the other is small. axis of propagation
Transcript of AP* Chemistry ATOMIC STRUCTURE - Lundquist Labs · AP* Chemistry ATOMIC STRUCTURE *AP is a...
AP* Chemistry ATOMIC STRUCTURE
*AP is a registered trademark of the College Board, which was not involved in the production of, and does not endorse, this product. © 2008 by René McCormick. All rights reserved.
ELECTROMAGNETIC RADIATION James Maxwell developed an elegant mathematical theory in 1864 to describe all forms of radiation in terms of oscillating or wave-like electric and magnetic fields in space. • electromagnetic radiation—UV, visible light, IR, microwaves,
television and radio signals, and X-rays • wavelength (λ)—(lambda) length between 2 successive crests. • frequency (υ)—(nu in chemistry; f in physics—either is OK), number
of cycles per second that pass a certain point in space (Hz-cycles per second)
• amplitude—maximum height of a wave as measured from the axis of propagation
• nodes—points of zero amplitude (equilibrium position); always occur
at λ/2 for sinusoidal waves velocity—speed of the wave
velocity = λ υ “c”—the speed of light; 2.99792458 [just call it 3] × 108 m/s; ALL EM RADIATION TRAVELS AT THIS SPEED! I call it easy, you’ll call it a trick! If “light” is involved, it travels at 3 × 108 m/s
• Notice that λ and υ are inversely proportional. When one is large, the other is small.
axis of propagation
Atomic Structure 2
Exercise 1 Frequency of Electromagnetic Radiation The brilliant red colors seen in fireworks are due to the emission of light with wavelengths around 650 nm when strontium salts such as Sr(NO3)2 and SrCO3 are heated. (This can be easily demonstrated in the lab by dissolving one of these salts in methanol that contains a little water and igniting the mixture in an evaporating dish.) Calculate the frequency of red light of wavelength 6.50 × 102 nm.
υ = 4.61 × 1014 Hz THE NATURE OF MATTER At the end of the 19th century, physicists were feeling rather smug. All of physics had been explained [or so they thought]. Students were being discouraged from pursuing physics as a career since all of the major problems had been solved! Matter and Energy were distinct: Matter was a collection of particles and Energy was a collection of waves. Enter Max Planck stage left… THE QUANTIZATION OF ENERGY "Ultraviolet catastrophe"—defined as the fact that a glowing hot object did not emit UV light as predicted. • 1900--Max Planck solved the problem. He made an incredible assumption: There is a minimum
amount of energy that can be gained or lost by an atom, and all energy gained or lost must be some integer multiple, n, of that minimum. (As opposed to just any old value of energy being gained or lost.)
ΔEnergy = n(hυ) • where h is a proportionality constant, Planck's constant, h = 6.6260755 × 10-34 joule • seconds.
This υ is the lowest frequency that can be absorbed or emitted by the atom, and the minimum energy change, hυ, is called a quantum of energy. Think of it as a “packet” of E equal to hυ.
• No such thing as a transfer of E in fractions of quanta, only in whole numbers of quanta. • Planck was able to calculate a spectrum for a glowing body that reproduced the experimental
spectrum. • His hypothesis applies to all phenomena on the atomic and molecular scale. Exercise 2 The Energy of a Photon The blue color in fireworks is often achieved by heating copper(I) chloride (CuCl) to about 1200°C. Then the compound emits blue light having a wavelength of 450 nm. What is the increment of energy (the quantum) that is emitted at 4.50 × 102 nm by CuCl?
= 4.41 × 10-19 J
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THE PHOTOELECTRIC EFFECT AND ALBERT EINSTEIN In 1900 Albert Einstein was working as a clerk in the patent office in Bern, Switzerland. This left him time to work on Physics. He proposed that EM radiation itself was quantized; he was a great fan of Planck’s work! He proposed that EM radiation could be viewed as a stream of “particles” called photons. • photoelectric effect--light bombards the surface of a metal and electrons are ejected. • frequency—a minimum υ must be met or alas, no action! Once minimum is met, intensity increases
the rate of ejection. • photon--massless particles of light. Ephoton = hυ = hc λ You know Einstein for the famous E = mc2 from his second “work” as the special theory of relativity published in 1905. Such blasphemy, energy has mass?! That would mean: m = E c2 therefore,
m = E = hc/λ = h c2 c2 λc Does a photon have mass? Yep! In 1922 American physicist Arthur Compton performed experiments involving collisions of X-rays and electrons that showed photons do exhibit the apparent mass calculated above.
SUMMARY: Energy is quantized. It can occur only in discrete units called quanta [hυ]. EM radiation [light, etc.] exhibits wave and particle properties. This phenomenon is known as the dual nature of light.
Since light which was thought to be wavelike now has certain characteristics of particulate matter, is the converse also true? Enter Louis de Broglie [French physicist, 1923] stage right…
IF m = h λc substitute v [velocity] for c for any object NOT traveling at the speed of light, then rearrange and solve for lambda
Atomic Structure 4
this is called the de Broglie equation: λ = h mv Exercise 3 Calculations of Wavelength Compare the wavelength for an electron (mass = 9.11 × 10-31 kg) traveling at a speed of 1.0 × 107 m/s with that for a ball (mass = 0.10 kg) traveling at 35 m/s.
λe = 7.27 × 10-11 m λ b = 1.9 × 10-34 m
• The more massive the object, the smaller its associated wavelength and vice
versa! • Davisson and Germer @ Bell labs found that a beam of electrons was
diffracted like light waves by the atoms of a thin sheet of metal foil and that de Broglie's relation was followed quantitatively.
• ANY moving particle has an associated wavelength. • Silly physicists! We now know that E is really a form of matter, and ALL
matter shows the same types of properties. That is, all matter exhibits both particulate and wave properties.
HYDROGEN’S ATOMIC LINE SPECTRA AND NIELS BOHR • emission spectrum—the spectrum of bright lines, bands, or
continuous radiation that is provided by a specific emitting substance as it loses energy and returns to its ground state OR the collection of frequencies of light given off by an "excited" electron
• absorption spectrum—a graph or display relating how a substance absorbs electromagnetic radiation as a function of wavelength
• line spectrum--isolate a thin beam by passing through a slit then a prism or a diffraction grating which sorts into discrete frequencies or lines
• Johann Balmer--worked out a mathematical relationship that accounted for the 3 lines of longest wavelength in the visible emission spectrum of H. (red, green and blue lines)
Atomic Structure 5
• Niels Bohr connected spectra, and the quantum ideas of Einstein and Planck: the single electron of the hydrogen atom could occupy only certain energy states, stationary states
"The Mother of all Assumptions" An electron in an atom would remain in its lowest E state unless otherwise disturbed. • Energy is absorbed or emitted by a change from this ground state • an electron with n = 1 has the most negative energy and is thus the most strongly
attracted to the positive nucleus. [Higher states have less negative values and are not as strongly attracted to the positive nucleus.]
• ground state--n = 1 for hydrogen
photon = = hchE υλ
• To move from ground to n = 2 the electron/atom must absorb no more or no less than 0.75 Rhc. [that’s a collection of constants]
• So, a move of n = 2 to n = 1 emits 985 kJ of energy. • What goes up must come down. Energy absorbed must eventually be emitted. • The origin or atomic line spectra is the movement of electrons between quantized energy states. • IF an electron moves from higher to lower E states, a photon is emitted and an emission line is
observed.
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• Bohr’s equation for calculating the energy of the E levels available to the electron in the
hydrogen atom:
• where n is an integer [larger n means larger orbit radius, farther from nucleus], Z is the nuclear charge
• The NEGATIVE sign simply means that the E of the electron bound to the nucleus is lower that it world be if the electron were at an infinite distance [n = ∞] from the nucleus where there is NO interaction and the energy is zero.
• ΔE is simply the subtraction of calculating the energy of two different levels, say n=6 and n=1. If the difference is negative, E was lost. If the difference is positive, E was gained.
• TWO Major defects in Bohr's theory: 1) Only works for elements with ONE electron. 2) The one, lonely electron DOES NOT orbit the nucleus in a fixed path!!
Exercise 4 Energy Quantization in Hydrogen Calculate the energy required to excite the hydrogen electron from level n = 1 to level n = 2. Also calculate the wavelength of light that must be absorbed by a hydrogen atom in its ground state to reach this excited state.
∆E = 1.633 × 10-18 J λ = 1.216 × 10-7 m
Exercise 5 Electron Energies Calculate the energy required to remove the electron from a hydrogen atom in its ground state.
∆E = 2.178 × 10-18 J
218
22.178 10 J ZEn
− ⎛ ⎞= − × ⎜ ⎟
⎝ ⎠
Atomic Structure 7
THE WAVE PROPERTIES OF THE ELECTRON SCHRODINGER, HEISENBERG, AND QUANTUM NUMBERS • After World War I--Niels Bohr assembled a group of physicists in Copenhagen hoping to derive
a comprehensive theory for the behavior of electrons in atoms from the viewpoint of the electron as a particle
• Erwin Schrodinger--independently tried to accomplish the same thing but focused on de Broglie's eqn' and the electron as a wave. Schrodinger's approach was better; explained more than Bohr's and met with more success. Quantum mechanics was born!
• de Broglie opened a can of worms among physicists by suggesting the electron had wave properties
• the electron has dual properties • Werner Heisenberg and Max Born provided the uncertainty principle
- if you want to define the momentum of an electron, then you have to forego knowledge of its exact position at the time of the measurement
• Max Born on the basis of Heisenberg's work suggested: if we choose to know the energy of an electron in an atom with only a small uncertainty, then we must accept a correspondingly large uncertainty about its position in the space about the atom's nucleus. So What? We can only calculate the probability of finding an electron within a given space.
THE WAVE MECHANICAL VIEW OF THE ATOM • Schrodinger equation: solutions are called wave functions--chemically
important. The electron is characterized as a matter-wave • sort of standing waves--only certain allowed wave functions (symbolized by
the Greek letter, ψ, pronounced “sigh”) • Each ψ for the electron in the H atom corresponds to an allowed energy
(−Rhc/n2). For each integer, n, there is an atomic state characterized by its own ψ and energy En.
• In English? Points 1 & 2 above say that the energy of electrons is quantized.
Notice in the figure to the right, that only whole numbers of standing waves can “fit” in the proposed orbits.
The hydrogen electron is visualized as a standing wave around the nucleus [above right]. The circumference of a particular circular orbit would have to correspond to a whole number of wavelengths, as shown in (a) and (b) above, OR else destructive interference occurs, as shown in (c). This is consistent with the fact that only certain electron energies are allowed; the atom is quantized. (Although this idea encouraged scientists to use a wave theory, it does not mean that the electron really travels in circular orbits.)
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• the square of ψ gives the intensity of the electron wave or the probability of finding the electron at the point P in space about the nucleus—the intensity of color in (a) above represents the probability of finding the electron in that space, the darker the color—the more probable it is we would find the electron in that region.
• electron density map, electron density and electron probability ALL mean the same thing! When we say “orbital” this image at right is what we picture in our minds.
• matter-waves for allowed energy states are also called (drum roll please…) orbitals.
• To solve Schrodinger's equation in a 3-dimensional world we need the quantum numbers n, , and mℓ
• The amplitude of the electron wave at a point depends on the distance of the point from the nucleus.
• Imagine that the space around a H nucleus is made up of a series of thin “shells” like the layers of an onion, but these “shells” as squishy (Very scientific word, that “squishy”!)
• Plot the total probability of finding the electron in each shell versus the distance from the nucleus and you get the radial probability graph you see in (b) above
• The maximum in the curve occurs because of two opposing effects. 1) the probability of finding an electron is greatest near the nucleus [electrons just can’t resist the attraction of a proton!], BUT 2) the volume of the spherical shell increases with distance from the nucleus, SO we are summing more positions of possibility, so the TOTAL probability increases to a certain radius and then decreases as the electron probability at EACH position becomes very small.
Try not to stress over this introduction stuff! Learn to do the calculations in the practice exercises & do the best you can with the “theory” stuff. It’s my moral obligation to TRY to explain it to you.
Stress over quantum numbers and electron configurations and periodicity if you must—that’s the important stuff in this chapter!
I just feel the need to give you a complete education!
Atomic Structure 9
-1 0 +1 -1 0 +1 0 0 0
QUANTUM NUMBERS & ATOMIC ORBITALS There are 4 quantum numbers that describe the “address” and “spin” of an electron. The value of n limits the possible values of ℓ, which in turn limit the values of mℓ. • n—principal energy level--1 to infinity. Determines the total energy of the electron. It indicates the
most probable [within 90%] distance of the electron from the nucleus. A measure of the orbital size or diameter. 2n2 electrons may be assigned to a shell. It’s simply the Energy level that electron is in. If it’s a 3s electron, n = 3, if it’s a 4d electron, n = 4, etc.
• ℓ--angular momentum--0,1,2,....(n-1) electrons w/in shell may be grouped into subshells [or sublevels, same thing!], each characterized by its certain wave shape. Each ℓ is a different orbital shape or orbital type. - n limits the values of ℓ to no larger than n-1. Thus, the number of possibilities for ℓ is equal to n.
(English translation: 3 sublevels for 3rd E level, 4 for 4th E level, etc.) - s,p,d,f sublevels 0,1,2,3 ℓ-values respectively (So, what do spdf stand for? Sharp, principle,
diffuse, fundamental--early days of atomic spectroscopy)
• mℓ--magnetic—assign the “blanks” in orbital notation with zero on the middle blank and then -ℓ through zero to +ℓ. I’ll bet this looks familiar for Sulfur from Chem. I!
1s 2s 2p 3s 3p
- that means that the range of orbitals is from +ℓ to - ℓ - it describes the orientation of an orbital in a given subshell - The down arrow in the 3p, -1 slot is the last electron placed [valence electron], so far it’s set
of quantum numbers is 3, 1, -1
You can keep going from g…
DON’T try to make this hard! Embrace the elegant patterns!
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Exercise 6 Electron Subshells For principal quantum level n = 5, determine the number of allowed subshells (different values of ℓ), and give the designation of each.
ℓ = 0; 5s ℓ = 1; 5p ℓ = 2; 5d ℓ = 3; 5f ℓ = 4; 5g
THE SHAPES OF ATOMIC ORBITALS There is no sharp boundary beyond which the electrons are never found!!
• s--spherical; the size increases with n. The nodes you see at left represent ZERO probability of finding the electron in that region of space. The number of nodes equals n-1 for s orbitals.
• p--have one plane that slices through the nucleus and divides the region of electron density into 2 halves. Nodal plane--the electron can never be found there!!
• 3 orientations: px, py, and pz.
• d--2 nodal planes slicing through the nucleus to create four sections; 5 orbitals.
- The dz2 orbital is really strange!
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• f--3 nodal planes slicing through the nucleus; eight
sections; 7 orbitals ELECTRON CONFIGURATIONS Chemical properties depend on the number and arrangement of electrons in an atom. Usually only the valence electrons play the reaction game. ELECTRON SPIN • 1920--chemists realized that since electrons interact with a magnetic field,
there must be one more concept to explain the behavior of electrons in atoms.
• ms--the 4th quantum number; accounts for the reaction of electrons in a magnetic field
MAGNETISM • magnetite--Fe3O4, natural magnetic oxide of iron • 1600--William Gilbert concluded the earth is also a large spherical magnet
with magnetic south at the geographic North Pole (Santa's habitat). • NEVER FORGET: opposites attract & likes repel whether it’s opposite
poles of a magnet or opposite electrical charges
PARAMAGNETISM AND UNPAIRED ELECTRONS • diamagnetic--not magnetic [magnetism dies]; in fact they are slightly repelled by a magnetic field.
Occurs when all electrons are PAIRED. • paramagnetic--attracted to a magnetic field; lose their magnetism when removed from the magnetic
field; HAS ONE OR MORE UNPAIRED ELECTRONS • ferromagnetic--retain magnetism upon introduction to, then removal from a magnetic field • All of these are explained by electron spins
o Each electron has a magnetic field with N & S poles o electron spin is quantized such that, in an external magnetic field, only two orientations of the
electron magnet and its spin are possible o +1/2 and −1/2 o H is paramagnetic; He is diamagnetic, WHY?
- H has one unpaired electron - He has NO unpaired electrons; all spins offset and cancel each other out
Atomic Structure 12
What about ferromagnetic? clusters of atoms have their unpaired electrons aligned within a
cluster, clusters are more or less aligned and substance acts as a magnet. Don't drop it!!
When all of the domains, represented by these arrows are aligned, it behaves as a magnet.
This is what happens if you drop it: The domains go in all different directions and it no longer operates as a magnet.
THE PAULI EXCLUSION PRINCIPLE In 1925 Wolfgang Pauli stated: no two electrons in an atom can have the same set of four quantum numbers. This means no atomic orbital can contain more than 2 electrons & for two electrons to occupy the same orbital, they must be of opposite spin!! ATOMIC ORBITAL ENERGIES AND ELECTRON ASSIGNMENTS
• Order of orbital energies--the value of n (E = −Rhc/n2) determines the energy of an electron • “many-electron” atoms depend on both n & ℓ • Use the diagonal rule or Aufbau series • Orbital radius changes slightly with ℓ as well as with n • subshell orbitals contract toward the nucleus as the value of ℓ
increases • contraction is partially into the volume of space occupied by
the core electrons • the energy of the electrons in these subshells is raised due to
the repulsions between the subshell electrons and the core electrons.
- a subshell's energy rises as its ℓ quantum number increases when inner electrons are present
• Order of Orbital Assignments • each electron is lazy and occupies the lowest energy space available • based on the assumption inner electrons have no effect on which orbitals are assigned to outer or
valence electrons - not exactly true (use diagonal rule)—note that the one pictured shows the lowest
energy state (1s) at the top of the diagram—some variations show 1s at the bottom of the diagram
• electron configurations (spectroscopic notation) • clump the 1's, 2's, etc. TOGETHER rather than written in the order the orbitals fill
Atomic Structure 13
HUNDS RULE The most stable arrangement of electrons is that with the maximum number of unpaired electrons; WHY?? it minimizes electron-electron repulsions (everyone gets their own room)
• all single electrons also have parallel spins to reduce e-/e- repulsions (aligns micromagnets) • When 2 electron occupy the same orbital they must have opposite spins (Pauli exclusion
principle); this also helps to minimize e-/e- repulsions Personally, I think this whole quantum number thing is easiest when we start with the electron configurations THEN write the quantum numbers. Allow me to recap: Don’t try to make this hard! It just isn’t. Energy Level 1 2 3 4 5 6 7…. # of sublevels 1 2 3 4 5 6 7…. Names of sublevels s s, p s,p,d s,p,d,f s,p,d,f,g s,p,d,f,g,h s,p,d,f,g,h,i n, principal quantum number
1 2 3 4 5 6 7….
Name of sublevel
s p d f g h i…
ℓ, angular momentum quantum number [= n-1]
0 1 2 3 4 5 6
# of orbitals [= -ℓ to +ℓ]
1 3 5 7 9 11 13
mℓ for each orbital within a sublevel
0
-1 0 +1
-2 -1 0 +1 +2
And so on, just pretend you are in second grade and make a number line with negative
numbers on the left, ZERO in the middle, and positive numbers on the right.
The first electron placed in an orbital is assigned the +1/2 and the second one is assigned the -1/2.
Atomic Structure 14
-1 0 +1
Let’s practice: Give the electron configurations for the elements within this figure. I’ll get you started! S 1s2 2s2 2p6 3s2 3p4
Cd La Hf Ra Ac
And their Orbital Notation: Sulfur 1 2 3 4 5 8 6 9 7 10 11 12 13 16 14 15 1s 2s 2p 3s 3p Cd La Hf Ra Ac There is a super cool animation that illustrates this concept. The website is from the Chief Reader of the AP Exam. This site is http://intro.chem.okstate.edu/APnew/Default.html Click on Electron Configuration Animation. You’ll need the shockwave plug-in. Once the animation comes up, click on the screen to advance from Hydrogen on up by atomic number.
As electrons enter these sublevels their wave functions interfere with each other causing the energy of these to change and separate. Do not be misled by this diagram, there ARE INDEED energy differences between all of these sublevels. See below.
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mighty close to the nucleus. “E is ZAPPED”
What are the quantum numbers for the outermost [valence] electron? S--since the last electron put in is #16 and it is in the 3p sublevel, n = 3 and ℓ = 2. It’s in the -1 slot, the mℓ = -1 and since it’s the second arrow placed [down arrow] its ms = -1/2. So the set of quantum numbers for the 16th electron in sulfur is: 3,2,-1, -1/2. You’ll find this really easy IF you draw the orbital notation for the last sublevel! Cd La Hf Ra Ac • You accepted that the sublevels had differences in energies long ago. • You even know the increasing order of energies: s < p < d < f < g…
• Now you have to be able to EXPLAIN it on the AP test. Throughout this discussion keep some fundamental scientific principles close at hand
o electrons repel each other o electrons are negative and thus, attracted by the
positive nucleus o forces (attractive & repulsive) dissipate with
increasing distance. • We need to examine the graph at the right, radial
probabilities again. o See the small hump near the origin? That’s the
distance from the nucleus that a 2s electron occupies a small but significant amount of the time—we say the 2s electron “penetrates to the nucleus” more than for the 2p orbital. This causes a 2s electron to be ATTRACTED to the nucleus more than a 2p electron making the 2s orbital LOWER in E than the 2p orbital.
o Think of the nucleus as “zapping” the energy of the electrons that penetrate closer to it. [Just don’t write that!] Imagine a hyper child—it’s on its best behavior, sitting still, being quiet, etc. when it’s close to Mom. The closer to the Mother Nucleus the hyper electron is, the less hyper or energetic it is. Don’t EVER write this as an answer to an essay question! It’s just a model to help you get your teeth into this concept!
“penetrates” closest to the nucleus
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• Same song second verse—the last hump represents the greatest probability for predicting the distance of an electron from the nucleus, BUT the first humps determine the order of the energy.
o The top graph is for 3s—note it has 2 humps close to the nucleus
o The bottom graph is for 3s, 3p and note that 3d only has one hump.
o 3s penetrates most [has least energy], then 3p [higher E than 3s, lower E than 3d] then 3d penetrates least [so it has the highest energy].
o MORAL: The greater the penetration, the less energy that orbital has. Since you already knew the order with respect to energy, s < p < d < f , the degree of penetration is s’s penetrate most and f’s penetrate least.
ION ORBITAL ENERGIES AND ELECTRON CONFIGURATIONS The dfs overlay [that thing that happens when the configurations don’t fit the pattern in transition metals and rare earth metals] does not occur in ion configurations since the valence (outermost n) electrons are the first to go! THE SHELL ENERGY RANGES SEPARATE MORE WIDELY AS ELECTRONS ARE REMOVED.
• Atoms and ions with unpaired electrons are paramagnetic (attracted to a magnetic field) • Transition metals with +2 or higher have no ns electrons • Fe+2 is paramagnetic to the extent of 4 unpaired electrons and Fe+3 is paramagnetic to the extent
of 5 unpaired electrons THE HISTORY OF THE PERIODIC TABLE
1800ish—Johann Dobereiner, triads; 1864 John Newlands octaves; 1870--Dmitrii Mendeleev & Julius Lothar Meyer--by mass; 1913 Mosley--by number of protons.
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o Group IA(1A or 1)--alkali metals o Group IIA(2A or 2)--alkaline earth metals o Group VIA(6A or 16)--Chalcogens o Group VIIA(7A or 17)—Halogens o Group VIIIA (8A or 18)—Noble gas
SOME PROPERTIES OF COMMON GROUPS:
• Alkali metals—the most reactive metal family; must be stored under oil; react with water violently!
• Alkaline-earth metals-- except for Be(OH)2, the metal hydroxides formed by this group provide basic solutions in water ; pastes of these used in batteries
• Chalcogen family – many found combined with metal ores • Halogen family – known as the “salt-formers” ; used in modern lighting • Noble Gas family – known for their disinterest in other elements; once thought to
never react; neon used to make bright RED signs • Transition metals—fill the d orbitals.
o Anomalies occur at Chromium and Copper to minimize electron/electron repulsions. If you learned that there is special stability associated with a half-filled sub-level, IT’S A LIE!! No such stability exists! NEVER, EVER write that! It’s all about lowering energy by minimizing electron/electron repulsions.
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PERIODIC TRENDS: A trend is NOT an
EXPLANATION!
• Rare Earth metals—fill the f sublevels.
Lanthanides and Actinides. These sometimes put an electron in d [just one or two electrons] before filling f. This is that dsf overlay referred to earlier—the energies of the sublevels are very similar.
This is an important section—there is almost always an essay involving this topic on the AP exam. There are several arguments you will evoke to EXPLAIN a periodic trend. Remember opposites attract and likes repel. The trick is learning which argument to use when explaining a certain trend! THE ARGUMENTS:
1. Effective nuclear charge, Zeff—essentially equal to the group number. Think of the IA’s having a Zeff of one while the VII A’s have a Zeff of 7! The idea is that the higher the Zeff, the more positive the nucleus, the more attractive force there is emanating from the nucleus drawing electrons in or holding them in place. Relate this to ENERGY whenever possible.
2. Distance—attractive forces dissipate with increased distance. Distant electrons are held loosely and thus easily removed. Relate this to ENERGY whenever possible.
3. Shielding—electrons in the “core” effectively shield the nucleus’ attractive force for the valence electrons. Use this ONLY when going up and down the table, NOT across. There is ineffective shielding within a sublevel or energy level. Relate this to ENERGY whenever possible. {I can’t help but think of dodge ball, such a barbaric ritual—since you’re the smart kids, you figured out in elementary school to stay behind the bigger kids to keep from getting hit! The electrons in the first or second energy level, shield the outer valence electrons from the Mother Nucleus’ attractive force. }
4. Minimize electron/electron repulsions—this puts the atom at a lower energy state and makes it more stable. Relate this to ENERGY whenever possible.
Here we go!
Atomic Structure 19
1. ATOMIC RADIUS--No sharp boundary beyond which the electron never strays!! • Use diatomic molecules and determine radius then react with other atoms to
determine the radius of those atoms • ATOMIC radii decreases (↓) moving across a period AND increases (↑)
moving down a row (family)
WHY ↓ across? The effective nuclear charge (Zeff) increases (more protons for the same number of energy levels) as we move from left to right across the periodic table, so the nucleus has a greater positive charge, thus the entire electron cloud is more strongly attracted and “shrinks”.
o This shrinks the electron cloud until… …the point at which electron/electron repulsions overcome the nuclear attraction and stop the contraction of the electron cloud.
WHY ↑ down? The principal level, n, determines the size of an atom—add another principal level and the atoms get MUCH larger radii
As we move down a family, the attractive force the nucleus exerts on the valence electrons dissipates.
Shielding is only a valid argument when comparing elements from period to period (up and down the table) since shielding is incomplete within a period—use this argument with extreme caution! It should NOT be your favorite!
2. IONIZATION ENERGY--energy required to remove an electron from the atom IN THE GAS PHASE. Costs Energy. • Removing each subsequent electron requires more energy:
Second IE, Third IE, etc. Some subsequent IEs cost more E than others!! A
HUGE energy price is paid if the subsequent removal of electrons is from another sublevel or, Heaven forbid, another principal E level (core).
- ↓ down a family—increased distance from the nucleus and increased shielding by full principal E levels means it requires less E to remove an electron
- ↑across a period—due to increasing Zeff. The higher the Zeff, the stronger the nucleus attracts valence electrons, the more energy required to remove a valence electron. Let’s talk EXCEPTIONS!!
Atomic Structure 20
• an anomaly occurs at “messing up a half-filled or filled sublevel” There’s nothing magical about this and electrons are not “happier” as a result. The simple truth is that when electron pairing first occurs within an orbital, there is an increase in electron/electron repulsions which makes it require less energy [easier] to remove an electron thus the IE drops. NEVER, EVER write about the fictitious stability of a ½-filled shell—even though you may see it in books!
• Look at oxygen vs. nitrogen—it requires less energy to remove an electron from oxygen’s valence
IN SPITE OF AN INCREASING Zeff because oxygen’s p4 electron is the first to pair within the orbital thus experiencing increased repulsion. The increased repulsion lowers the amount of energy required to remove the newly paired electron!
• Also, look at the drop in IE from any s2 to p1. This is also IN SPITE OF AN INCREASING Zeff. This
drop in the energy required to remove a valence electron is due to the fact that you are removing a p electron rather than an s electron. The p’s are less tightly held BECAUSE they do not penetrate the electron cloud toward the nucleus as well as an s electron. The general trend is that s is held most tightly since it penetrates more then p, d and f…
3. ELECTRON AFFINITY—an affinity or “liking” for electrons—force feeding an element an electron—Energy associated with the addition of an electron to a gaseous atom: X (g) + e− X− (g) If the addition of an electron is exothermic, then you’ll see a negative sign on the energy change and the converse is also true. The more negative the quantity, the more E is released. This matches our sign convention in thermodynamics. • ↓ down a family [that means becomes less negative a.k.a. more positive, giving off less energy]—due to increased distance from the nucleus with each increasing principal E level. The nucleus is farther from the valence level and more shielded. • ↑ across a period [that means become more negative, giving off more energy]—Again the increasing Zeff more strongly attracts the electron. The interactions of electron/electron repulsions wreaks havoc with this generalization as we shall soon see!
Atomic Structure
21
• Let’s talk EXCEPTIONS!! First the lines on the diagram below connect adjacent elements. The absence of a line indicates missing elements whose atoms do not add an electron exothermically and thus do not form stable isolated anions [remember these are all –1 ions at this point].
- an anomaly—No N− yet there is a C−--this is due to their electron/electron repulsions compared to their electron configurations. N is p3 while C is p2. C adds an electron WITHOUT PAIRING which does NOT increase the e-/e- repulsions and therefore, carbon forms a stable -1 ion while N would have to pair p electrons and the increased e-/e- repulsions overcome the increasing attractive force due to the increase in Zeff and no -1 N ion forms! [horrid sentence structure!]
- O2- doesn’t exist in isolated form [gasp] for the same reason. It’s p4, so adding the first electron causes a subsequent pairing BUT it has a greater Zeff than N, so it can form O-. BUT adding the second electron fills the p’s and that increased e-/e- repulsion overpowers the Zeff of oxygen. Never fear, oxide ions exist in plenty of compounds so we haven’t exactly been lying to you!
- F is weird, it has really strong e-/e- repulsion since the p orbitals are really small in the second level therefore repulsions are high. In subsequent halogen orbitals, it’s not as noticeable.
4. IONIC RADII • Cations—shrink big time since the nucleus is now attracting
fewer electrons • Anions—expand since the nucleus is now attracting MORE
electrons than there are protons AND there is enhanced electron/electron repulsion to boot.
• Isoelectronic—ions containing the same number of electrons - consider the # of protons to determine size. Oxide vs. Fluoride.
Fluoride has one more proton which further attracts the electron cloud, so it is smaller.
Atomic Structure
22
5. ELECTRONEGATIVITY (En)—The ability of an atom IN A MOLECULE [meaning it’s participating in a BOND] to attract shared electrons to itself. Think “tug of war”. Now you know why they teach you such games in elementary school! o Linus Pauling’s scale—Nobel Prize for Chemistry & Peace
o Fluorine is the most En and Francium is the least En o Why is F the most? Highest Zeff and smallest so that the nucleus is closest to the valence
“action”. o Why is Fr the least? Lowest Zeff and largest so that the nucleus is farthest from the
“action”. o We’ll use this concept a great deal in our discussions about bonding since this atomic
trend is only used when atoms form molecules.
Exercise 8 Trends in Ionization Energies The first ionization energy for phosphorus is 1060 kJ/mol, and that for sulfur is 1005 kJ/mol. Why?
Atomic Structure
23
Exercise 9 Ionization Energies Consider atoms with the following electron configurations: a. 1s22s22p6 b. 1s22s22p63s1 c. 1s22s22p63s2 Identify each atom. Which atom has the largest first ionization energy, and which one has the smallest second ionization energy? Explain your choices.
A: Ne; largest IE B: Na
C: Mg; smallest IE2
Exercise 10 Trends in Radii Predict the trend in radius for the following ions: Be2+, Mg2+, Ca2+, and Sr2+.
Be2+ < Mg2+ < Ca2+ < Sr2+
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Dev
elo
pin
g t
he C
on
cep
t o
f S
hell
s, S
ub
shell
s, E
lectr
on
Co
nfi
gu
ra
tio
ns,
an
d M
ore
PA
RT
I:
Dis
cove
ring
ho
w e
lect
rons
are
‘a
rra
ng
ed’
in a
n a
tom
1.
Des
crib
e th
e n
atu
re o
f th
e in
tera
ctio
n b
etw
een
pro
ton
s an
d e
lect
ron
s in
an
ato
m?
Co
nsi
der
usi
ng
so
me
or
all
of
the
foll
ow
ing
ter
ms
in y
ou
r d
escr
ipti
on
:
•
attr
acti
on
, re
pu
lsio
n,
neu
tral
, p
osi
tiv
e, n
egat
ive,
ch
arg
e, d
ista
nce
, n
ucl
eus,
forc
e, e
ner
gy
, C
ou
lom
b’s
Law
.
2.
Fo
r ea
ch s
itu
atio
n b
elo
w,
com
par
e th
e re
lati
ve
ener
gy
nec
essa
ry t
o s
epar
ate
po
siti
ve
and
neg
ativ
e el
ectr
ical
ch
arg
es.
•
Co
mp
are
A t
o B
•
Co
mp
are
A t
o C
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
3.
Co
nsi
der
•
Ho
w m
any
ele
ctro
ns
do
yo
u s
ee i
n t
he
pic
ture
? H
ow
man
y p
roto
ns?
•
Wh
ich
of
thes
e el
ectr
on
s is
th
e ea
sies
t (r
equ
ires
th
e le
ast
amo
un
t o
f
ener
gy
) to
rem
ov
e (i
on
ize)
? Ju
stif
y y
ou
r an
swer
.
•
Co
mp
are
the
ener
gy
req
uir
ed t
o r
emo
ve
the
elec
tro
n f
rom
3 w
ith
th
e
ener
gy
in
•
2a
•
2c
Th
e fi
rst
ion
izat
ion
en
erg
y i
s d
efin
ed a
s th
e m
inim
um
en
erg
y t
hat
mu
st b
e ad
ded
to
a
neu
tral
ato
m,
in t
he
gas
ph
ase,
to
rem
ov
e an
ele
ctro
n f
rom
th
at a
tom
.
Th
is d
efin
itio
n c
an b
e re
pre
sen
ted
by
th
e fo
llo
win
g c
hem
ical
eq
uat
ion
:
ener
gy
+ A
(g) →
A+(g
) +
e–
4.
In t
he
ion
izat
ion
eq
uat
ion
ab
ov
e id
enti
fy w
hic
h s
pec
ies
is a
t lo
wer
en
erg
y,
A(g
) o
r A
+(g
) +
e–?
Ju
stif
y y
ou
r an
swer
.
5.
Exp
lain
wh
y e
ner
gy
is
req
uir
ed (
an e
nd
oth
erm
ic p
roce
ss)
to r
emo
ve
the
elec
tro
n
in a
neu
tral
ato
m.
6.
Th
e v
alu
e o
f th
e fi
rst
ion
izat
ion
en
erg
y f
or
hy
dro
gen
is
13
12
kJ
mo
l-1.
ener
gy
+ H
(g) →
H+(g
) +
e–
On
th
e g
rap
h o
n t
he
nex
t p
age
use
a s
ho
rt h
ori
zon
tal
lin
e to
in
dic
ate
the
ener
gy
of
H(g
) an
d a
sh
ort
ho
rizo
nta
l li
ne
to i
nd
icat
e th
e en
erg
y o
f H
+(g
) +
e–. B
e su
re t
o
con
sid
er y
ou
r re
spo
nse
s to
Q4
an
d Q
5 a
bo
ve.
!
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
7.
Wh
at d
oes
th
e d
iffe
ren
ce i
n e
ner
gy
in
th
e li
nes
in
yo
ur
dia
gra
m a
bo
ve
rep
rese
nt?
Th
e v
alu
es f
or
the
firs
t io
niz
atio
n e
ner
gy
fo
r a
hy
dro
gen
an
d h
eliu
m a
tom
are
pro
vid
ed i
n
the
tab
le b
elo
w.
!
Ato
m
1H
2H
e 3L
i
Ion
izat
ion
En
erg
y (
kJ
mo
l –
1)
13
12
2
37
3
!
8.
Bas
ed o
n c
om
par
iso
ns
yo
u m
ade
in Q
ues
tio
n 2
ho
w w
ou
ld y
ou
exp
lain
th
e
dif
fere
nce
in
th
e v
alu
es f
or
the
firs
t io
niz
atio
n e
ner
gy
fo
r h
yd
rog
en a
nd
hel
ium
?
9.
Ho
w d
oes
yo
ur
exp
lan
atio
n a
cco
un
t fo
r th
e re
lati
ve
char
ge
on
hy
dro
gen
an
d
hel
ium
an
d t
he
dis
tan
ce o
f th
e el
ectr
on
(s)
fro
m t
he
nu
cleu
s?
H(g
) H
+(g
) +
e–
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
In t
he
ener
gy
dia
gra
m b
elo
w l
oca
te (
dra
w a
ho
rizo
nta
l li
ne)
th
e fi
rst
ion
izat
ion
en
erg
y f
or
hy
dro
gen
an
d t
he
firs
t io
niz
atio
n e
ner
gy
fo
r h
eliu
m.
10
. H
ow
do
es t
he
dia
gra
m i
llu
stra
te t
he
rela
tiv
e ea
se w
ith
wh
ich
an
ele
ctro
n c
an b
e
rem
ov
ed f
rom
eac
h a
tom
?
11
. P
red
ict
a v
alu
e fo
r th
e fi
rst
ion
izat
ion
en
erg
y f
or
lith
ium
.
Do
no
t ad
d y
ou
r p
red
icti
on
to
th
e fi
gu
re j
ust
yet
. Ju
stif
y y
ou
r p
red
icti
on
(lo
ok
bac
k a
t Q
ues
tio
n 2
if
yo
u n
eed
gu
idan
ce).
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Th
e ac
tual
val
ue
of
the
firs
t io
niz
atio
n e
ner
gy
of
lith
ium
is
52
0 k
J m
ol-1
. A
dd
th
is v
alu
e
for
to t
he
fig
ure
on
th
e p
rev
iou
s p
age.
12
. H
ow
wo
uld
yo
u e
xp
lain
th
e io
niz
atio
n e
ner
gy
fo
r li
thiu
m c
om
par
ed t
o t
he
ion
izat
ion
en
erg
y f
or
hel
ium
? C
om
par
ed t
o h
yd
rog
en?
13
. P
red
ict
the
rela
tiv
e v
alu
e o
f th
e en
erg
y n
eces
sary
to
rem
ov
e a
seco
nd
ele
ctro
n
(cal
led
th
e se
con
d i
on
izat
ion
en
erg
y)
fro
m l
ith
ium
. S
up
po
rt y
ou
r p
red
icti
on
wit
h
an e
xp
lan
atio
n.
14
. B
ased
on
th
e fi
rst
ion
izat
ion
en
erg
ies
for
hy
dro
gen
, h
eliu
m a
nd
lit
hiu
m t
hat
yo
u
rep
rese
nte
d i
n t
he
fig
ure
on
th
e p
rev
iou
s p
age,
wh
at c
an y
ou
in
fer
abo
ut
the
dis
tan
ce o
f th
e el
ectr
on
s fr
om
th
eir
resp
ecti
ve
nu
clei
.
! ! ! ! Th
e fi
rst
ion
izat
ion
en
erg
ies
for
sele
cted
ele
men
ts f
rom
th
e se
con
d p
erio
d o
f th
e p
erio
dic
tab
le a
re p
rov
ided
in
th
e ta
ble
bel
ow
.
Ato
m
3L
i 4B
e 6C
7N
9F
1
0N
e
Ion
izat
ion
En
erg
y (
kJ
mo
l –
1)
52
0
89
9
10
86
1
30
2
16
81
2
08
1
15
. E
xp
lain
th
e tr
end
in
io
niz
atio
n e
ner
gie
s in
ter
ms
of
the
char
ge
of
the
nu
cleu
s an
d
the
rela
tiv
e lo
cati
on
of
the
elec
tro
ns.
Th
e fi
rst
ion
izat
ion
en
erg
y f
or
the
elem
ent
sod
ium
is
giv
en i
n t
he
foll
ow
ing
tab
le.
Ato
m
11N
a 1
2M
g
14S
i 1
5P
1
7C
l 1
8A
r
Ion
izat
ion
En
erg
y (
kJ
mo
l –
1)
52
0
16
. P
red
ict
the
val
ues
fo
r th
e fi
rst
ion
izat
ion
en
erg
y f
or
the
oth
er s
elec
ted
th
ird
per
iod
elem
ents
. E
xp
lain
ho
w y
ou
arr
ived
at
yo
ur
pre
dic
tio
ns.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Bel
ow
is
a ta
ble
co
nta
inin
g t
he
elec
tro
n e
ner
gie
s fo
r ea
ch o
f th
e 1
8 e
lect
ron
s in
an
arg
on
ato
m.
Th
e g
rap
h o
f th
is d
ata
is s
ho
wn
.
17
. M
ake
ob
serv
atio
ns
abo
ut
the
gra
ph
in
ter
ms
of
the
rela
tiv
e en
erg
ies
of
the
elec
tro
ns
and
th
eir
rela
tio
nsh
ip t
o e
ach
oth
er.
18
. B
ased
on
yo
ur
resp
on
ses
fro
m t
he
pre
vio
us
qu
esti
on
s h
ow
man
y ‘
gro
up
s’ (
lev
els
or
shel
ls)
of
elec
tro
ns
are
sho
wn
fo
r A
rgo
n?
19
. In
dic
ate
the
nu
mb
er o
f el
ectr
on
s in
eac
h g
roup
/lev
el t
hat
yo
u i
den
tifi
ed?
Ele
ctro
n
Rem
ov
ed
Ele
ctro
n
En
erg
y
(kJ
mo
l –
1)
1
−1
52
1
2
−2
66
6!
3
−3
93
1!
4
−5
75
1!
5
−7
23
8!
6
−8
78
1!
7
−1
19
95!
8
−1
38
42!
9
−4
07
60!
10
−
46
18
6!
11
−
52
00
2!
12
−
59
65
3!
13
−
66
19
8!
14
−
72
91
8!
15
−
82
47
2!
16
−
88
57
6!
17
−
39
76
04!
18
−
42
70
65!
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
20
. O
n t
he
gra
ph
bel
ow
dra
w a
ho
rizo
nta
l li
ne
(to
th
e ri
gh
t o
f th
e y
-ax
is)
that
rep
rese
nts
an
av
erag
e en
erg
y l
evel
fo
r ea
ch o
f th
e g
roup
s o
f el
ectr
on
s th
at y
ou
iden
tifi
ed.
Lab
el t
he
lev
els
1,
2,
etc.
… b
egin
nin
g f
rom
th
e lo
wes
t en
erg
y l
evel
.
Wh
at d
o t
hes
e li
nes
rep
rese
nt?
2
1. H
ow
wo
uld
yo
u d
escr
ibe
the
rela
tiv
e en
erg
y s
epar
atio
n o
f th
ese
ener
gy
lev
els?
22
. A
n e
lect
ron
fro
m w
hic
h l
evel
req
uir
es
•
the
least
am
ou
nt
of
ener
gy
to
rem
ov
e?
•
Th
e la
rges
t am
ou
nt
of
ener
gy
to
rem
ov
e?
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Des
crib
e th
e el
ectr
on
str
uct
ure
(lo
cati
on
of
the
elec
tro
n)
of
the
ato
m.
Co
nsi
der
usi
ng
som
e o
r al
l o
f th
e fo
llo
win
g t
erm
s in
yo
ur
des
crip
tio
n;
nu
cleu
s, e
lect
ron
, en
erg
y,
dis
tan
ce,
lev
el, p
roto
n,
shel
l, a
rran
gem
ent,
att
ract
ion
, re
pu
lsio
n, p
osi
tiv
e, n
egat
ive,
ch
arg
e,
loca
tio
n.
PA
RT
II:
Do
all
ele
ctro
ns
in t
he
sam
e le
vel
ha
ve t
he
sam
e en
erg
y?
On
e im
po
rtan
t co
ncl
usi
on
bas
ed o
n t
he
firs
t io
niz
atio
n e
ner
gy
exp
erim
enta
l d
ata
is t
hat
elec
tro
ns
in h
igh
er s
hel
ls r
equ
ire
less
en
erg
y t
o r
emo
ve.
We
hav
e ex
amin
ed e
xp
erim
enta
l
dat
a th
at r
elat
es t
he
ener
gy
req
uir
ed t
o r
emo
ve
an e
lect
ron
to
th
e sh
ell
the
elec
tro
n
occ
up
ies.
•
In w
hic
h s
hel
l d
oes
an
ele
ctro
n r
equ
ire
mo
re e
ner
gy
to
rem
ov
e, a
n e
lect
ron
in
th
e
seco
nd
sh
ell
or
the
fou
rth
sh
ell?
An i
nte
rest
ing
qu
esti
on
th
at c
ann
ot
be
answ
ered
fro
m t
he
exp
erim
enta
l d
ata
of
the
firs
t
ion
izat
ion
en
erg
y i
s…
Do
all
ele
ctro
ns
in t
he
sam
e sh
ell
req
uir
e th
e sa
me
am
ou
nt
of
ener
gy
to r
emo
ve?
We
CA
N a
nsw
er t
his
qu
esti
on
if
we
loo
k a
t p
ho
toel
ectr
on
sp
ectr
osc
op
y (
PE
S)
dat
a fo
r
the
ato
ms.
In
a p
ho
toel
ectr
on
sp
ectr
osc
op
y e
xp
erim
ent
any
ele
ctro
n c
an b
e io
niz
ed w
hen
the
ato
m i
s ex
cite
d.
Lik
e w
ith
th
e fi
rst
ion
izat
ion
, o
nly
on
e el
ectr
on
is
rem
ov
ed f
rom
th
e
ato
m.
Ho
wev
er i
n a
PE
S e
xp
erim
ent
it c
an b
e A
NY
ele
ctro
n,
no
t ju
st t
he
elec
tro
n t
hat
req
uir
es t
he
leas
t am
ou
nt
of
ener
gy
to
rem
ov
e.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Ex
amin
e th
e P
ES
sp
ectr
um
fo
r h
yd
rog
en s
ho
wn
in
th
e fi
gu
re.
Th
e la
bel
on
th
e y-a
xis
is
ener
gy
an
d t
he
un
its
are
in m
egaj
ou
les(
M J
mo
l –
1)
1.
Wh
at d
oes
th
e x-a
xis
dep
ict?
Exp
lain
.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
2.
Wh
at i
s th
e re
lati
on
ship
bet
wee
n t
he
ph
oto
elec
tro
n s
pec
tru
m a
nd
th
e fi
rst
ion
izat
ion
en
erg
y f
or
hy
dro
gen
?
Hel
ium
is
nex
t, b
ut
bef
ore
lo
ok
ing
at
its
ph
oto
elec
tro
n s
pec
tru
m a
nsw
er t
he
foll
ow
ing
qu
esti
on
s:
3.
Ho
w m
any
ele
ctro
ns
do
es h
eliu
m h
ave
in i
ts f
irst
sh
ell?
4.
Ref
er b
ack
to
Par
t I
of
this
act
ivit
y,
and
ob
tain
th
e fi
rst
ion
izat
ion
en
erg
y f
or
a
hel
ium
ato
m.
Can
yo
u p
red
ict
wh
at t
he
PE
S w
ou
ld l
oo
k l
ike
if
a.
the
sam
e am
ou
nt
of
ener
gy
is
req
uir
ed t
o r
emo
ve
each
of
the
elec
tro
ns?
b.
dif
fere
nt
amo
un
ts o
f en
erg
y a
re r
equ
ired
to
rem
ov
e ea
ch e
lect
ron
?
Go
to
bac
k t
o t
he
pre
vio
us
fig
ure
an
d s
ket
ch b
oth
sce
nar
ios.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Ex
amin
e th
e P
ES
fo
r h
eliu
m a
nd
co
mp
are
it t
o y
ou
r p
red
icti
on
fro
m t
he
pre
vio
us
qu
esti
on
.
5
. E
xp
lain
th
e re
lati
ve
ener
gy
of
the
pea
k(s
) an
d t
he
nu
mb
er o
f el
ectr
on
s re
pre
sen
ted
by
eac
h p
eak
in
th
e P
ES
fo
r h
eliu
m a
nd
fo
r h
yd
rog
en.
6.
Fo
r li
thiu
m
a.
Ho
w m
any
ele
ctro
ns
do
es l
ith
ium
hav
e?
b.
Wh
at s
hel
ls (
lev
els)
do
th
ose
ele
ctro
ns
occ
up
y?
7.
Pre
dic
t w
hat
yo
u e
xp
ect
the
PE
S f
or
lith
ium
to
lo
ok
lik
e. (
No
te:
yo
u d
o n
ot
hav
e
to p
red
ict
the
exac
t en
erg
ies
of
each
ele
ctro
n,
yo
u c
an m
ake
a re
aso
nab
le e
stim
ate
bas
ed o
n t
he
firs
t io
niz
atio
n e
ner
gie
s fo
r li
thiu
m a
nd
hel
ium
- r
efer
bac
k t
o P
art
I
of
this
act
ivit
y.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
L
oo
k a
t th
is P
ES
an
d c
om
par
e it
to
th
e p
red
icti
on
yo
u m
ade
in t
he
pre
vio
us
qu
esti
on
.
8.
Fo
r ea
ch p
eak
in
th
e P
ES
of
lith
ium
, id
enti
fy t
he
shel
l th
e el
ectr
on
s re
pre
sen
ted
by
that
pea
k o
ccup
y.
Be
sure
to
co
mm
ent
abo
ut
the
rela
tiv
e en
erg
y o
f th
e p
eak
(s)
and
the
nu
mb
er o
f el
ectr
on
s fo
r ea
ch p
eak
fo
r L
i.)
Th
e n
ext
elem
ent
in t
he
Per
iod
ic T
able
is
ber
yll
ium
.
9.
Ho
w m
any
ele
ctro
ns
do
es b
ery
lliu
m h
ave
and
wh
at s
hel
ls d
o t
ho
se e
lect
ron
s
occ
up
y?
10
. F
or
the
PE
S f
or
ber
yll
ium
pre
dic
t
a.
ho
w m
any
pea
ks
b.
the
nu
mb
er o
f el
ectr
on
fo
r ea
ch p
eak
c.
esti
mat
e th
e re
lati
ve
ener
gie
s.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
T
he
nex
t el
emen
t in
th
e P
erio
dic
Tab
le i
s b
oro
n.
11
. H
ow
man
y e
lect
ron
s d
oes
bo
ron
hav
e an
d w
hat
sh
ells
do
th
ose
ele
ctro
ns
occ
up
y?
12
. F
or
the
PE
S f
or
bo
ron
pre
dic
t
a.
ho
w m
any
pea
ks
b.
the
nu
mb
er o
f el
ectr
on
(s)
for
each
pea
k
c.
esti
mat
e th
e re
lati
ve
ener
gie
s
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Bel
ow
is
the
PE
S f
or
bo
ron
.
13
. B
rief
ly d
escr
ibe
ho
w t
o i
nte
rpre
t th
e P
ES
fo
r b
oro
n.
14
. P
red
ict
wh
at c
han
ges
in
th
e P
ES
yo
u w
ou
ld e
xp
ect
to s
ee g
oin
g a
cro
ss p
erio
d 2
of
the
per
iod
ic t
able
, fr
om
car
bo
n t
o n
eon
? L
oo
k a
t th
e P
ES
fo
r th
ese
seco
nd
per
iod
elem
ents
.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
Bel
ow
is
the
PE
S f
or
the
per
iod
2 e
lem
ents
fro
m b
oro
n t
o n
eon
.
Ad
apte
d a
nd
mo
dif
ied
fro
m J
oh
n G
eld
er’s
DR
AF
T V
ER
SIO
N.
15
. A
nsw
er t
he
foll
ow
ing
qu
esti
on
s af
ter
loo
kin
g a
t th
e P
ES
fo
r h
yd
rog
en t
hro
ug
h
neo
n. a.
Wo
uld
yo
u a
gre
e o
r d
isag
ree
wit
h t
he
foll
ow
ing
sta
tem
ent?
Exp
lain
yo
ur
answ
er.
‘Th
e el
ectr
ons
in t
he
seco
nd
sh
ell
all
ha
ve t
he
sam
e en
erg
y.’
b.
Ho
w m
any
‘su
bsh
ells
’ ar
e fo
un
d i
n t
he
seco
nd
sh
ell?
c.
Ho
w m
any
‘su
bsh
ells
’ ar
e fo
un
d i
n t
he
firs
t sh
ell?
d.
Ho
w m
any
ele
ctro
ns
are
in e
ach
sub
shel
l in
th
e se
con
d s
hel
l? I
n t
he
firs
t
shel
l?
e.
Mo
vin
g s
yst
emat
ical
ly f
rom
lit
hiu
m t
o n
eon
;
i.
Ho
w m
any
ele
ctro
ns
are
in t
he
firs
t sh
ell?
ii.
Wh
at h
app
ens
to t
he
ener
gy
req
uir
ed t
o r
emo
ve
an e
lect
ron
in
th
e
firs
t sh
ell
mo
vin
g f
rom
lef
t to
rig
ht
in t
he
seco
nd
per
iod
? S
up
po
rt
yo
ur
ob
serv
atio
n w
ith
an e
xp
lan
atio
n.
iii.
Wh
at h
app
ens
to t
he
ener
gy
of
the
elec
tro
ns
in t
he
ou
ter
mo
st
shel
l?
16
. L
oo
k a
t th
e P
ES
fo
r th
e el
emen
ts i
n t
he
thir
d p
erio
d (
sod
ium
– a
rgo
n)
and
des
crib
e y
ou
r ob
serv
atio
ns.
An
y s
urp
rise
s? E
xp
lain
.
A n
ota
tio
n h
as b
een
ag
reed
up
on
fo
r w
riti
ng
an
ele
ctro
n c
on
fig
ura
tio
n t
o i
den
tify
th
e
loca
tio
n o
f th
e sh
ell
and
sub
shel
l o
f ea
ch e
lect
ron
in
an
ato
m.
Sh
ells
are
lab
eled
wit
h a
nu
mb
er;
1,
2,
3,
etc.
an
d s
ub
shel
l ar
e la
bel
ed w
ith
let
ters
; s,
p, d
, an
d f
. E
ver
y s
hel
l
con
tain
s an
s s
ub
shel
l.
17
. W
rite
th
e co
mp
lete
ele
ctro
n c
on
fig
ura
tio
n f
or
the
firs
t te
n e
lem
ents
in
th
e p
erio
dic
tab
le?
Lo
ok
at
the
PE
S f
or
po
tass
ium
, ca
lciu
m a
nd
sca
nd
ium
.
18
. E
xp
lain
wh
at h
app
ens
in t
he
PE
S f
or
scan
diu
m t
hat
has
no
t o
ccu
rred
in
an
y
elem
ent
pri
or.
19
. If
on
e el
ectr
on
is
rem
ov
ed f
rom
sca
nd
ium
, w
hic
h e
lect
ron
(id
enti
fy t
he
shel
l an
d
sub
shel
l) r
equ
ires
th
e le
ast
amo
un
t o
f en
erg
y t
o r
emo
ve?
AP
* A
tom
ic S
tru
ctu
re &
Pe
rio
dic
ity F
ree
Re
sp
on
se
Qu
estio
ns
page 1
(1)
AP
® i
s a
regi
ster
ed t
rade
mar
k of
the
Col
lege
Boa
rd. T
he C
olle
ge B
oard
was
not
inv
olve
d in
the
pro
duct
ion
of a
nd d
oes
not
endo
rse
this
pro
duct
. (2)
Tes
t Q
uest
ions
are
Cop
yrig
ht ©
198
4-20
08 b
y C
olle
ge E
ntra
nce
Exa
min
atio
n B
oard
, Pri
ncet
on, N
J. A
ll r
ight
s re
serv
ed. F
or f
ace-
to-f
ace
teac
hing
pur
pose
s, c
lass
room
te
ache
rs a
re p
erm
itte
d to
rep
rodu
ce t
he q
uest
ions
. Web
or
Mas
s di
stri
buti
on p
rohi
bite
d.
19
80
(a)
Wri
te t
he g
roun
d st
ate
elec
tron
con
figu
rati
on f
or a
n ar
seni
c at
om, s
how
ing
the
num
ber
of e
lect
rons
in
each
su
bshe
ll.
(b)
Giv
e on
e pe
rmis
sibl
e se
t of
fou
r qu
antu
m n
umbe
rs f
or e
ach
of t
he o
uter
mos
t el
ectr
ons
in a
sin
gle
As
atom
w
hen
it i
s in
its
gro
und
stat
e.
(c)
Is a
n is
olat
ed a
rsen
ic a
tom
in
the
grou
nd s
tate
par
amag
neti
c or
dia
mag
neti
c? E
xpla
in b
rief
ly.
(d)
Exp
lain
how
the
ele
ctro
n co
nfig
urat
ion
of t
he a
rsen
ic a
tom
in
the
grou
nd s
tate
is
cons
iste
nt w
ith
the
exis
tenc
e of
the
fol
low
ing
know
n co
mpo
unds
: N
a 3A
s, A
sCl 3
, and
AsF
5.
19
81
The
em
issi
on s
pect
rum
of
hydr
ogen
con
sist
s of
sev
eral
ser
ies
of s
harp
em
issi
on li
nes
in th
e ul
trav
iole
t (L
yman
ser
ies)
in
the
vis
ible
(B
alm
er s
erie
s) a
nd i
n th
e in
frar
ed (
Pas
chen
ser
ies,
Bra
cket
t se
ries
, etc
.) r
egio
ns o
f th
e sp
ectr
um.
(a)
Wha
t fe
atur
e of
the
ele
ctro
nic
ener
gies
of
the
hydr
ogen
ato
m e
xpla
ins
why
the
em
issi
on s
pect
rum
con
sist
s of
di
scre
te w
avel
engt
h ra
ther
tha
n a
cont
inuu
m w
avel
engt
h?
(b)
Acc
ount
for
the
exis
tenc
e of
sev
eral
ser
ies
of li
nes
in th
e sp
ectr
um. W
hat q
uant
ity
dist
ingu
ishe
s on
e se
ries
of l
ines
fr
om a
noth
er?
(c)
Dra
w a
n el
ectr
onic
ene
rgy
leve
l dia
gram
for
the
hydr
ogen
ato
m a
nd in
dica
te o
n it
the
tran
siti
on c
orre
spon
ding
to
the
line
of
low
est
freq
uenc
y in
the
Bal
mer
ser
ies.
(d
) W
hat
is t
he d
iffe
renc
e be
twee
n an
em
issi
on s
pect
rum
and
an
abso
rpti
on s
pect
rum
? E
xpla
in w
hy th
e ab
sorp
tion
sp
ectr
um o
f at
omic
hyd
roge
n at
roo
m t
empe
ratu
re h
as o
nly
the
line
s of
the
Lym
an s
erie
s.
19
87
Use
the
det
ails
of
mod
ern
atom
ic t
heor
y to
exp
lain
eac
h of
the
fol
low
ing
expe
rim
enta
l ob
serv
atio
ns.
(a)
Wit
hin
a fa
mil
y su
ch a
s th
e al
kali
met
als,
the
ion
ic r
adiu
s in
crea
ses
as t
he a
tom
ic n
umbe
r in
crea
ses.
(b
) T
he r
adiu
s of
the
chl
orin
e at
om i
s sm
alle
r th
an t
he r
adiu
s of
the
chl
orid
e io
n, C
l- . (R
adii
: C
l at
om =
0.
99Å
; C
l i
on =
1.8
1Å)
(c)
The
fir
st i
oniz
atio
n en
ergy
of
alum
iniu
m i
s lo
wer
tha
n th
e fi
rst
ioni
zati
on e
nerg
y of
mag
nesi
um.
(Fir
st
ioni
zati
on e
nerg
ies:
12M
g =
7.6
ev;
13A
l =
6.0
ev)
(d
) F
or m
agne
sium
, the
dif
fere
nce
betw
een
the
seco
nd a
nd th
ird
ioni
zati
on e
nerg
ies
is m
uch
larg
er th
an th
e di
ffer
ence
bet
wee
n th
e fi
rst a
nd s
econ
d io
niza
tion
ene
rgie
s. (I
oniz
atio
n en
ergi
es fo
r Mg:
1st =
7.6
ev;
2nd
=
14 e
v; 3
rd =
80
ev)
19
87
Tw
o im
port
ant
conc
epts
tha
t re
late
to
the
beha
viou
r of
ele
ctro
ns i
n at
om s
yste
ms
are
the
Hei
senb
erg
unce
rtai
nty
prin
cipl
e an
d th
e w
ave-
part
icle
dua
lity
of
mat
ter.
(a
) S
tate
the
Hei
senb
erg
unce
rtai
nty
prin
cipl
e as
it r
elat
ed to
the
dete
rmin
ing
the
posi
tion
and
mom
entu
m o
f an
obj
ect.
(b
) W
hat
aspe
ct o
f th
e B
ohr
theo
ry o
f th
e at
om i
s co
nsid
ered
uns
atis
fact
ory
as a
res
ult
of t
he H
eise
nber
g un
cert
aint
y pr
inci
ple?
(c
) E
xpla
in w
hy th
e un
cert
aint
y pr
inci
ple
or th
e w
ave
natu
re o
f par
ticl
es is
not
sig
nifi
cant
whe
n de
scri
bing
the
beha
viou
r of
mac
rosc
opic
obj
ects
, but
it
is v
ery
sign
ific
ant
whe
n de
scri
bing
the
beh
avio
ur o
f el
ectr
ons.
AP
* A
tom
ic S
tru
ctu
re &
Pe
rio
dic
ity F
ree
Re
sp
on
se
Qu
estio
ns
page 2
19
90
T
he d
iagr
am s
how
s th
e fi
rst
ioni
zati
on e
nerg
ies
for
the
elem
ents
fro
m L
i to
Ne.
Bri
efly
(in
one
to
thre
e se
nten
ces)
exp
lain
eac
h of
the
fol
low
ing
in t
erm
s of
ato
mic
str
uctu
re.
(a
) In
gen
eral
, the
re i
s an
inc
reas
e in
the
fir
st i
oniz
atio
n en
ergy
fro
m L
i to
Ne.
(b
) T
he f
irst
ion
izat
ion
ener
gy o
f B
is
low
er t
han
that
of
Be.
(c
) T
he f
irst
ion
izat
ion
ener
gy o
f O
is
low
er t
han
that
of
N.
(d)
Pre
dict
how
the
fir
st i
oniz
atio
n en
ergy
of
Na
com
pare
s to
tho
se o
f L
i an
d of
Ne.
Exp
lain
. 1
99
3
Acc
ount
for
eac
h of
the
fol
low
ing
in t
erm
s of
pri
ncip
les
of a
tom
str
uctu
re, i
nclu
ding
the
num
ber,
pr
oper
ties
, and
arr
ange
men
ts o
f su
bato
mic
par
ticl
es.
(a)
The
sec
ond
ioni
zati
on e
nerg
y of
sod
ium
is
abou
t th
ree
tim
es g
reat
er t
han
the
seco
nd i
oniz
atio
n
ener
gy o
f m
agne
sium
. (b
) T
he d
iffe
renc
e be
twee
n th
e at
omic
rad
ii o
f N
a an
d K
is
rela
tive
ly l
arge
com
pare
d to
the
dif
fere
nce
betw
een
the
atom
ic r
adii
of
Rb
and
Cs.
(c
) A
sam
ple
of n
icke
l ch
lori
de i
s at
trac
ted
into
a m
agne
tic
fiel
d, w
here
as a
sam
ple
of s
olid
zin
c ch
lori
de
is n
ot.
(d)
Pho
spho
rus
form
s th
e fl
uori
des
PF
3 an
d P
F5,
whe
reas
nit
roge
n fo
rms
only
NF
3.
AP
* A
tom
ic S
tru
ctu
re &
Pe
rio
dic
ity F
ree
Re
sp
on
se
Qu
estio
ns
page 3
19
94
D
Use
pri
ncip
les
of a
tom
ic s
truc
ture
and
/or
chem
ical
bon
ding
to
answ
er e
ach
of t
he f
ollo
win
g.
(a)
The
rad
ius
of t
he C
a at
om i
s 0.
197
nano
met
er;
the
radi
us o
f th
e C
a2+ i
on i
s 0.
099
nano
met
er.
Acc
ount
for
thi
s di
ffer
ence
. (b
) T
he l
atti
ce e
nerg
y of
CaO(s)
is -
3,46
0 ki
lojo
ules
per
mol
e; t
he l
atti
ce e
nerg
y fo
r K
2O(s)
is -
2,24
0 ki
lojo
ules
pe
r m
ole.
Acc
ount
for
thi
s di
ffer
ence
. Io
niza
tion
Ene
rgy
(kJ/
mol
)F
irst
Sec
ond
K41
93,
050
Ca
590
1,14
0
(c)
Exp
lain
the
dif
fere
nce
betw
een
Ca
and
K i
n re
gard
to
(i)
thei
r fi
rst
ioni
zati
on e
nerg
ies,
(i
i)
thei
r se
cond
ion
izat
ion
ener
gies
. (d
) T
he f
irst
ion
izat
ion
ener
gy o
f M
g is
738
kil
ojou
les
per
mol
e an
d th
at o
f A
l is
578
kil
ojou
les
per
mol
e.
Acc
ount
for
thi
s di
ffer
ence
. 1
99
7
Exp
lain
eac
h of
the
fol
low
ing
obse
rvat
ions
usi
ng p
rinc
iple
s of
ato
mic
str
uctu
re a
nd/o
r bo
ndin
g.
(a)
Pot
assi
um h
as a
low
er f
irst
-ion
izat
ion
ener
gy t
han
lith
ium
.
(b)
The
ion
ic r
adiu
s of
N3 ¯
is l
arge
r th
an t
hat
of O
2 ¯.
(c)
A c
alci
um a
tom
is
larg
er t
han
a zi
nc a
tom
.
(d)
Bor
on h
as a
low
er f
irst
-ion
izat
ion
ener
gy t
han
bery
lliu
m.
19
99
Ans
wer
the
fol
low
ing
ques
tion
s re
gard
ing
ligh
t an
d it
s in
tera
ctio
ns w
ith
mol
ecul
es, a
tom
s, a
nd i
ons.
(a)
The
lon
gest
wav
elen
gth
of l
ight
wit
h en
ough
ene
rgy
to b
reak
the
Cl-
Cl
bond
in
Cl 2
(g)
is 4
95 n
m.
(i)
Cal
cula
te t
he f
requ
ency
, in
s-1, o
f th
e li
ght.
(ii)
Cal
cula
te t
he e
nerg
y, i
n J,
of
a ph
oton
of
the
ligh
t.
(iii
)C
alcu
late
the
min
imum
ene
rgy,
in
kJ m
ol-1
, of
the
Cl-
Cl
bond
.
AP
* A
tom
ic S
tru
ctu
re &
Pe
rio
dic
ity F
ree
Re
sp
on
se
Qu
estio
ns
page 4
(b)
A c
erta
in l
ine
in t
he s
pect
rum
of
atom
ic h
ydro
gen
is a
ssoc
iate
d w
ith
the
elec
tron
ic t
rans
itio
n in
th
e H
ato
m f
rom
the
six
th e
nerg
y le
vel
(n =
6)
to t
he s
econ
d en
ergy
lev
el (n =
2).
(i)
Indi
cate
whe
ther
the
H a
tom
em
its
ener
gy o
r w
heth
er i
t ab
sorb
s en
ergy
dur
ing
the
tran
siti
on. J
usti
fy y
our
answ
er.
(ii)
Cal
cula
te t
he w
avel
engt
h, i
n nm
, of
the
radi
atio
n as
soci
ated
wit
h th
e sp
ectr
al l
ine.
(iii
)A
ccou
nt f
or t
he o
bser
vati
on t
hat
the
amou
nt o
f en
ergy
ass
ocia
ted
wit
h th
e sa
me
elec
tron
ic t
rans
itio
n (n
= 6
to n
= 2
) in
the
He+
ion
is
grea
ter
than
tha
t as
soci
ated
wit
h th
e co
rres
pond
ing
tran
siti
on i
n th
e H
ato
m.
20
00
Ans
wer
the
fol
low
ing
ques
tion
s ab
out
the
elem
ent
sele
nium
, Se
(ato
mic
num
ber
34).
(a)
Sam
ples
of
natu
ral
sele
nium
con
tain
six
sta
ble
isot
opes
. In
term
s of
ato
mic
str
uctu
re, e
xpla
in w
hat
thes
e is
otop
es h
ave
in c
omm
on, a
nd h
ow t
hey
diff
er.
(b)
Wri
te t
he c
ompl
ete
elec
tron
con
figu
rati
on (
e.g.
, 1s2 2s2 . .
. et
c.)
for
a se
leni
um a
tom
in
the
grou
nd
stat
e. I
ndic
ate
the
num
ber
of u
npai
red
elec
tron
s in
the
gro
und-
stat
e at
om, a
nd e
xpla
in y
our
reas
onin
g.
(c)
In t
erm
s of
ato
mic
str
uctu
re, e
xpla
in w
hy t
he f
irst
ion
izat
ion
ener
gy o
f se
leni
um i
s
(i)
less
tha
n th
at o
f br
omin
e (a
tom
ic n
umbe
r 35
), a
nd
(ii)
grea
ter
than
tha
t of
tel
luri
um (
atom
ic n
umbe
r 52
).
(d)
Sel
eniu
m r
eact
s w
ith
fluo
rine
to
form
SeF
4. D
raw
the
com
plet
e L
ewis
ele
ctro
n-do
t st
ruct
ure
for
S
eF4
and
ske
tch
the
mol
ecul
ar s
truc
ture
. Ind
icat
e w
heth
er t
he m
olec
ule
is p
olar
or
nonp
olar
, and
ju
stif
y yo
ur a
nsw
er.
AP* Atomic Structure & Periodicity Free Response Questions KEY page 1
(1) AP® is a registered trademark of the College Board. The College Board was not involved in the production of and does not endorse this product. (2) Test Questions are Copyright © 1984-2008 by College Entrance Examination Board, Princeton, NJ. All rights reserved. For face-to-face teaching purposes, classroom teachers are permitted to reproduce the questions. Web or Mass distribution prohibited.
1980
a) 2 points
1s2 2s22p6 3s23p6 4s23d104p3
b) 2 points
for the two electrons in the 4s: 4, 0, 0, +1/2 and 4, 0, 0, - 1/2
for the three electrons in the 4p: 4, 1, -1, +1/2; 4, 1, 0, +1/2 and 4, 1, +1, +1/2
c) 2 points
Paramagnetic. It has three unpaired electrons.
d) 2 points
Na3As - each Na gives up one electron to the As, the As has a complete octet and the sodium atoms are ionically bonded to the arsenic
AsCl3 - the three chlorines each have one half-filled orbital and the aresenic has three. So three covalent bonds are created and the As has one non-bonding pair to make a pyramidal structure.
AsF5 - fluorine is so eletronegative that it draws the two electrons of the non-bonding pair of AsCl3 into bonding. A 4d orbital is involved in the sp3d hydridization, yielding a trigonal bipyramidal shape.
1981
a) 1 point
Quantized energy levels or discrete energies or wave properties of electron produce discrete energy states in a gas.
b) 2 points
The excited state atoms can relax to several lower energy states (see diagram in c).
Each final state energy level produces a separate series.
c) 2 points
AP* Atomic Structure & Periodicity Free Response Questions page 2
d) 3 points
Emission spectra are photons emitted from excited state systems as they drop to lower energy states.
Absorption spectra result from the absorption of electromagnetic radiation. Electrons are excited to a highter energy state.
Hydrogen atoms are in the lowest electronic energy state at 25 °C (n = 1) so absorptions will be n = 1 to n = 2,3,4, etc.
1987
Special rules for this question:
An ambiguous 2 pt. response receives only 1 pt An incorrect statement in an otherwise correct 2 pt response will result in a score of 1 pt The answers labeled (i) below received two points; (ii) received one point.
a) two points
The radii of the alkali metal ions increase with increasing atomic number because:
(i) the principle quantum number (or shell or energy level) increases (ii) there is an increase in shielding (or the number of orbitals increases)
b) two points
The chloride ion is larger than the chlorine atom because:
AP* Atomic Structure & Periodicity Free Response Questions page 3
(i) electron- electron repulsion increases (or shielding increases or the electron-proton ratio increases or the effective nuclear charge decreases) (ii) an extra electron generally increases the size
c) two points
The ionization energy of Mg is greater than that for Al because:
(i) the 3p orbital is at a higher energy than the 3s orbital (or the electron in Al is shielded from the nucleus more completely by the 3s electron than the 3s electrons shield one another from the nucleus) (ii) a 3p electron is easier to remove than a 3s electron
d) two points
The much greater difference between the 2nd and 3rd ionization energies in Mg (relative to the difference between the 1st and 2nd) is due to the 3rd electron being removed from the 2p subshell after the first 2 were removed from the 3s subshell.
1987
a) three points
It is impossible to determine (or measure) bothe the position and momentum of any particle (or object, or body) simutaneously.
OR
The more exactly the position of a particle is known, the less exactly the position or velocity of the particle is known.
OR
([delta] x) ([delta] p) [greater than or equal to] h-bar (or h / 4pi)
h = Planck's constant [delta] x = uncertainty in position [delta] p = uncertainty in momentum
Notes:
1 point is given for the notion of simultaneous determination. (A number of students give the first sentence but omit the word simultaneously. (They got 2 out of 3.) If the second or third versions of the answer are given, simultaneity is understood. If they give the equation, they must have a > sign, not just an = sign, or they lose 1 pt. A student who gives a correct answer but adds erroneous material gets one point deducted.
AP* Atomic Structure & Periodicity Free Response Questions page 4
b) five points
Bohr postulated that the electron in a H atom travels about the nucleus in a circular orbit and has a fixed angular momentum. With a fixed radius of orbit and a fixed momentum (or energy), ([delta] x) ([delta] p) < h/4pi
and violates the uncertainty principle.
Students receive 2 pts total for the above. If they say only "the electron travels in circular orbits", they get 1 point. They also get credit for saying elliptical orbits. To receive full credit, they must describe an aspect of the Bohr theory.
The following portion of the answer is worth three points.
The wavelength of a particle is given by the deBroglie relation:
[gamma] = h/mv
For masses of macroscopic objects, h/m is so small for any v that [gamma] is so small as to be undetectable. For an electron, m is so small that h/mv yields a detectable [gamma].
OR
They may say the product of the uncertainties in postion and velocity depends on h/m and since h is so
small (h = 6.63 × 10¯34 J s) unless m is very small, as for an electron, the product of the uncertainties is too small to be detected.
Students may discuss the fact that measuring the position and momentum requires having a photon strike the particle. The photon has an energy comparable to that of an electon but small compared to that of a macroscopic object. They must stress mass rather than size as the important distinction to get full credit.
A student who says [gamma] or ([delta] x) ([delta] p) depends on "size" and not mass gets 2 points if discussion is otherwise okay.
Page 5
1990
1993
Page 6 Page 7
1997
AP® CHEMISTRY
1999 SCORING GUIDELINES
Copyright © 2001 by College Entrance Examination Board. All rights reserved. College Board, Advanced Placement Program, AP, and the acorn logo
are registered trademarks of the College Entrance Examination Board.
4
Question 2
9 points
One point deduction for mathematical error (maximum once per question)
One point deduction for error in significant figures* (maximum once per
question)
*number of significant figures must be correct within +/- one digit.
(a) (i) 114
9
817
sec1006.6)m10495
m/sec1000.3,(
nm495
nm/sec1000.3 −
−×=
×
×=
×== or
c
λν 1 pt
(ii) E = hν = (6.626 × 10−34 J sec)(6.06 × 1014 sec−1) = 4.02 × 10−19 J 1 pt
(iii) (4.02 × 10−19 J)(6.022 × 10−23 mol−1)(0.00100 kJ/J) = 242 kJ/mol 1 pt
Note: No units required if answers are numerically same as above. No penalty
if answers are correct with different units and units are explicitly indicated
(e.g., for part (ii), 4.02 × 10−22 kJ is acceptable)
(b) (i) Energy is emitted. 1 pt
The n = 6 state is at a higher energy than the n = 2 state. Going from a high energy 1 pt
state to a low energy state means that energy must be emitted.
Note: The key idea is that the energy of the n = 6 state is higher (more excited) than
the lower (less excited) n = 2 state. The argument that �e− is farther away� at
the n = 6 level is not accepted.
(ii) J1005.66
J10178.2 , J1045.5
2
J10178.2 20
2
18
619
2
18
2−
−−
−
×−=×−
=×−=×−
= EE
J104.84 J)1045.5( J1005.6 19192026
−−−×=×−−×−=−=∆ EEE
OR, 1 pt
∆E = 2.178 × 10−18( )
1
2
1
62 2− J = 2.178 × 10−18 (0.2222) J = 4.84 × 10−19 J
Note: Point earned for determining the energy of transition.
Negative energies acceptable.
Page 8
AP® CHEMISTRY
1999 SCORING GUIDELINES
Copyright © 2001 by College Entrance Examination Board. All rights reserved. College Board, Advanced Placement Program, AP, and the acorn logo
are registered trademarks of the College Entrance Examination Board.
5
Question 2 (cont.)
E = λ
hc ! λ =
E
hc
OR, 1 pt
114
34
19
sec1030.7secJ10626.6
J1084.4 −
−
−
×=×
×==
h
Eν
Note: Point earned for writing or using λ
hcE = , or for calculating the frequency, ν
nm411m10
nm1
sec1030.7
secm1000.3
9114
18
=××
×==
−−
−
νλ
c
OR, 1 pt
J1084.4
)sec nm1000.3)(sec J 10626.6(19
11734
−
−−
×
××=λ = 411 nm
Note: Point earned for correct wavelength; λ = 4.11 x 10−7 m accepted.
Negative wavelength not accepted.
(iii) The positive charge holding the electron is greater for He+, which has a 2+ nucleus,
than for H with its 1+ nucleus. The stronger attraction means that it requires more energy1 pt
for the electron to move to higher energy levels. Therefore, transitions from high energy
states to lower states will be more energetic for He+ than for H.
Note: Other arguments accepted, such as, �E is proportional to Z 2. Since Z = 2 for He+
and Z = 1 for H, all energy levels in He + are raised (by a factor of 4).� Other accepted
answers must refer to the increased charge on the He+ nucleus, and NOT the mass.
______________________________________________________________________________________
One point deduction for mathematical error (maximum once per question)
One point deduction for error in significant figures* (maximum once per question)
*number of significant figures must be correct within +/− one digit
Page 9
AP® Chemistry 2000 ! Scoring Standards
Copyright © 2000 College Entrance Examination Board and Educational Testing Service. All rights reserved.AP is a registered trademark of the College Entrance Examination Board.
Question 7
(8 points)
(a) The isotopes have the same number (34) of protons, 1 pt.
but a different number of neutrons. 1 pt.
• No comment about the number of electrons is necessary
(b) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
or 1 pt.
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4
• No point is earned for [Ar] 4s2 3d10 4p4, because the question specifically asks for a complete electron configuration.
Since there are three different 4p orbitals, there must be two unpaired electrons. 1 pt.
Notes: The second part should have some explanation of Hund’s rule, and may include adiagram. The second point can still be earned even if the first point is not IF the electronconfiguration is incorrect, but the answer for the second part is consistent with the electronconfiguration given in the first part.
(c) (i) The ionized electrons in both Se and Br are in the same energy level, but Br has more protons than Se, so the attraction to the nucleus is greater. 1 pt.
Note: There should be two arguments in an acceptable answer -- the electronsremoved are from the same (4p) orbital and Br has more protons (a greater nuclearcharge) than Se.
(ii) The electron removed from a Te atom is in a 5p orbital, while the electron 1 pt.
removed from an Se atom is in a 4p orbital. The 5p orbital is at a higherenergy than the 4p orbital, thus the removal of an electron in a 5p orbitalrequires less energy.
Page 10
AP® Chemistry 2000 ! Scoring Standards
Copyright © 2000 College Entrance Examination Board and Educational Testing Service. All rights reserved.AP is a registered trademark of the College Entrance Examination Board.
Question 7
(continued)
(d) 1 pt.
Notes: One point earned for a correct Lewis diagram and a sketch. The Lewisdiagram and the molecular structure may be combined into one sketch if bothaspects (electron pairs and structure) are correct. Dots, lines, or a mixture of bothcan be used in the Lewis diagram. The lone pair of electrons need not be shown inthe sketch -- just the atomic positions. No credit earned for just a verbal descriptionof molecular geometry (“see-saw”, “saw-horse”, or something “distorted”), becausethe question clearly asks the student to “sketch the molecular structure”.
The SeF4 molecule is polar, because the polarities induced by the bonds and 1 pt.
the lone pair of electrons do not cancel.
Se
F
F
F
F
Se
FF
F F
Page 11
AP Atomic Structure Multiple Choice Practice
1
AP Chemistry -- Atomic Structure and Periodicity
Multiple ChoiceFor the AP exam you are not allowed to use a calculator, so you should try doing as many of these as possible without one. When I grade it I will mark which ones you missed, and if you return it to me with the corrected answers BEFORE we go over it in class, I’ll give you back half the points
1. Which of the following represents a pair of isotopes? atomic number atomic massa. I. 6 14
II. 7 14
b. I. 6 7II. 14 14
c. I. 6 14II. 14 28
d. I. 7 13II. 7 14
2. Atoms of an element, X, have the electronic configuration shown below. The compound most likely formed with magnesium, Mg, is
1s2 2s22p6 3s23p3
a. MgXb. MgX2
c. Mg3X2
d. MgX3
3. Which of the following represents the ground state electron configuration for the Mn3+ ion?a. 1s2 2s22p6 3s23p63d4
b. 1s2 2s22p6 3s23p63d54s2
c. 1s2 2s22p6 3s2 3p63d24s2
d. 1s2 2s22p6 3s23p63d84s2
4. Gaseous atoms of which of the elements below are paramagnetic?
Ca, V, Co, Zn, Asa. V, Co, and Zn onlyb. Zn and As onlyc. Ca, V, and Co onlyd. V, Co, and As only
5. Given the photoelectron spectra of valence electrons below, which is a possible identity of the atom?
a. Sr c. Lib. Ga d. Br
2
6. Which of the following conclusions can be drawn from J.J Thompson’s cathode ray experiments?a. Atoms contain electronsb. Practically all the mass of an atom is contained
in its nucleus.c. Atoms contain protons, neutrons, and electrons.d. Atoms have a positively charged nucleus
surrounded by an electron cloud.
7. Which of the following is a correct interpretation of the results of Rutherford’s experiments in which gold atoms were bombarded with alpha particles?a. Atoms have equal numbers of positive and
negative chargesb. electrons in atoms are arranged in shellsc. the positive charge of an atom is concentrated
in a small regiond. neutrons are at the center of an atom
8. In which of the following properties generally decreases across the periodic table from sodium to chlorinea. First ionization energyb. Atomic massc. Electronegativityd. Atomic radius
9. The effective nuclear charged experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outmost electron of Ne. This difference best accounts for which of the following?a. Na has a greater density at standard conditions
than Ne.b. Na has a lower first ionization energy than Nec. Na has a higher melting point than Ned. Na has fewer naturally occurring isotopes than
Ne
10. The elements in which of the following have most nearly the same atomic radius?a. Be, B, C, Nb. Ne, Ar, Kr, Xec. C, P, Se, Id. Cr, Mn, Fe, Co
11. A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt ofa. Cub. Mnc. Nid. Zn
12. The ionization energies for element X are listed in the table below. On the basis of the data, element X is most likely to be
a. Na c. Alb. Mg d. Si
13. In the periodic table, as atomic number increases from 11 to 17, what happens to the atomic radius?a. It decreases, than increasesb. It increases onlyc. It increases, than decreasesd. It decreases only
14. All of the halogens in their elemental form at 25oC and 1 atm area. odorlessb. diatomic moleculesc. colorlessd. gases
15. Which of the following characteristics is common to elemental sulfur, chlorine, nitrogen, and carbon?
3
a. They are gaseous elements at room temperatureb. they have oxides that are acid anhydridesc. They have perceptible color at room
temperatured. They form ionic oxides
16. In which of the following groups are the three species isoelectronic; ie: have the same number of electrons?a. S2-, K+, Ca2+
b. Sc, Ti, V2+
c. O2-, S2-, Cl-
d. Mg2+, Ca2+, Sr2+
Consider atoms of the following elements. Assume that the atoms are in the ground state.a. Sb. Cac. Gad. Sb
17. The atom that contains exactly two unpaired electrons
18. The atom that contains only one electron in the highest occupied energy sublevel.
For the next four questions, refer to the following electron configurations.a. 1s2 2s22p5 3s23p5
b. 1s2 2s22p6 3s23p6
c. 1s2 2s22p62d10 3s23p5
d. 1s2 2s22p6 3s23p63d10 4s2
19. An impossible electronic configuration. 20. The ground-state configuration for the atoms of a transition element.
21. The ground-state configuration of a negative ion of a halogen. 22. The ground-state configuration of a common ion of an alkaline earth element.
For the next three (3) questions refer to the following orbital notations.
4
a. Ab. Bc. Cd. D
23. Represents an atom that is chemically unreactive 24. Represents an atom in an excited state
25. Represents an atom that has four valence electrons
For the next three (3) questions refer to the following elementsa. Fb. Sc. Mgd. Mn
26. Forms monatomic ions with 2- charge in solution 27. forms a compound having the formula KXO4
28. Forms oxides that are common air pollutants and that yield acidic solution in water.
For the next three (3) questions refer to the following elements.a. Ob. Mgc. Rbd. N
29. What is the most electronegative element listed above?
30. Which element exhibits the greatest number of different oxidative states?
31. Which of the elements above has the smallest ionic radius for its most commonly found ion?
For the next two (2) questions, refer to the following types of energya. Activation energyb. Free energyc. Ionization energyd. Lattice energy
32. The energy required to convert a ground-state atom in the gas phase to gaseous positive ion
33. The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions.
3/16/2015 Catpin Bubble Test Generator
http://www.catpin.com/cgibin/bubble_test.pl 1/1
AP Chemistry Atomic Structure Homework
Name: _______________________________
1. 18. 2. 19. 3. 20. 4. 21. 5. 22. 6. 23. 7. 24. 8. 25. 9. 26. 10. 27. 11. 28. 12. 29. 13. 30. 14. 31. 15. 32. 16. 33. 17.
