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Atoms and
Electronic Structure
Atomic Structure and
Subatomic Particles
Protons and neutrons in
nucleus
Electrons move about
is the remaining space
of the atom.
1
Protons Neutrons Electrons
Note:
atomic mass unit (amu)
Relative
Charge
Charge
(C)
Mass
(amu)
Mass
(g)
Proton +1 +1.602181019 1.00727 1.672611024
Neutron 0 0 1.00866 1.674931024
Electron -1 1.602181019 0.00055 0.000911024
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Elements: Defined by their
number of protons
Atomic number (Z)
This number identifies the element. (See the
numbers on the periodic table.)
Mass number (A)
So, if given the Z and A, how will you determine
the number of neutrons?
Some questions.
What is the atomic number of Chlorine?
How many protons does chlorine have?
11A
188A
1H
1.008 22A
133A
144A
155A
166A
177A
2He
4.003
3Li
6.941
4Be
9.012
5B
10.81
6C
12.01
7N
14.01
8O
16.00
9F
19.00
10Ne
20.18
11Na
22.99
12Mg
24.31 3
3B4
4B5
5B6
6B7
7B 89
8B1 0 11
1B122B
13Al26.98
14Si
28.09
15P
30.97
16S
32.06
17Cl
35.45
18Ar39.95
19K
39.10
20Ca
40.08
21Sc
44.96
22Ti
47.87
23V
50.94
24Cr
52.00
25Mn
54.94
26Fe
55.85
27Co
58.93
28Ni
58.69
29Cu
63.55
30Zn
65.39
31Ga
69.72
32Ge
75.59
33As74.92
34Se
78.96
35Br
79.90
36Kr
83.80
37Rb
85.47
38Sr
87.62
39Y
88.91
40Zr
91.22
41Nb
92.91
42Mo
95.96
43Tc
(98)
44Ru
101.1
45Rh
102.9
46Pd
106.4
47Ag
107.9
48Cd
112.4
49In
114.8
50Sn
118.7
51Sb
121.8
52Te
127.6
53I
126.9
54Xe
131.3
55Cs
132.9
56Ba
137.3
57La
138.9
72Hf
178.5
73Ta
180.9
74W
183.8
75Re
186.2
76Os
190.2
77Ir
192.2
78Pt
195.1
79Au197.0
80Hg
200.6
81Tl
204.4
82Pb
207.2
83Bi
209.0
84Po
(209)
85At(210)
86Rn(222)
87Fr
(223)
88Ra
(226)
89Ac(227)
104Rf
(261)
105Db(262)
106Sg
(266)
107Bh
(264)
108Hs
(269)
109Mt
(268)
110Ds
(271)
111Rg
(272)
112Cn
(285)
113 114Fl
(289)
115 116Lv
(292)
117 118
Lanthanide series
58Ce
140.1
59Pr
140.9
60Nd
144.2
61Pm(145)
62Sm150.4
63Eu
152.0
64Gd
157.3
65Tb
158.9
66Dy
162.5
67Ho
164.9
68Er
167.3
69Tm168.9
70Yb
173.0
71Lu
175.0
Actinide series
90Th
232.0
91Pa
231.0
92U
238.0
93Np
(237)
94Pu
(244)
95Am(243)
96Cm(247)
97Bk
(247)
98Cf
(251)
99Es
(252)
100Fm(257)
101Md(258)
102No(259)
103Lr
(262)
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If the mass number is 37, how
many neutrons does the atom
have?1. 372. 17
3. 20
4. 27
5. 30
How many electrons does an atom of chlorine
have?
What element has an atomic number of 12?
Isotopes
Isotopes
Most elements have two or more isotopes. Symbols can be used to distinguish the different
isotopes:
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Isotope symbols
XA
Z
Determine the number of
protons, neutrons and electrons.
1. p=5, n=6, e=6
2. p=5, n=6, e=5
3. p=6, n=5, e=5
4. p=5, n=11, e=5
5. p=6, n=5, e=5
B115
Example
B115
Is the 5 necessary ?
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More about isotopes:
Hydrogen is the only element in which the
different isotopes has their own names.
1H
2H
3H
Ions: Losing and Gaining
Electrons
Ions -
Cation - positive charged ion.
Anion - negative charged ion.
Symbol electrons protons neutrons
24Mg
23Na+
35Cl
35Cl-
56Fe3+
15N
16O2-
27Al3+
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Give the number of electrons and
neutrons for 35Cl
1. e = 16, n = 20
2. e = 18, n = 18
3. e = 17, n = 20
4. e = 18, n = 20
5. None of the above
The Periodic Law
and the Periodic Table
11A
188A
1H
1.008
22A
133A
144A
155A
166A
177A
2He
4.003
3Li
6.941
4Be
9.012
5B
10.81
6C
12.01
7N
14.01
8O
16.00
9F
19.00
10Ne
20.18
11Na
22.99
12Mg
24.31
33B
44B
55B
66B
77B 8
98B
10 111B
122B
13Al26.98
14Si
28.09
15P
30.97
16S
32.06
17Cl
35.45
18Ar39.95
19K
39.10
20Ca
40.08
21Sc
44.96
22Ti
47.87
23V
50.94
24Cr
52.00
25Mn
54.94
26Fe
55.85
27Co
58.93
28Ni
58.69
29Cu
63.55
30Zn
65.39
31Ga
69.72
32Ge
75.59
33As74.92
34Se
78.96
35Br
79.90
36Kr
83.80
37Rb
85.47
38Sr
87.62
39Y
88.91
40Zr
91.22
41Nb
92.91
42Mo
95.96
43Tc(98)
44Ru
101.1
45Rh
102.9
46Pd
106.4
47Ag107.9
48Cd
112.4
49In
114.8
50Sn
118.7
51Sb
121.8
52Te
127.6
53I
126.9
54Xe
131.3
55Cs
132.9
56Ba
137.3
57La
138.9
72Hf
178.5
73Ta
180.9
74W
183.8
75Re
186.2
76Os
190.2
77Ir
192.2
78Pt
195.1
79Au197.0
80Hg
200.6
81Tl
204.4
82Pb
207.2
83Bi
209.0
84Po
(209)
85At(210)
86Rn
(222)
87Fr
(223)
88Ra
(226)
89Ac(227)
104Rf
(261)
105Db(262)
106Sg
(266)
107Bh(264)
108Hs
(269)
109Mt
(268)
110Ds
(271)
111Rg(272)
112Cn(285)
113 114Fl
(289)
115 116Lv
(292)
117 118
Lanthanide series58Ce
140.1
59Pr
140.9
60Nd
144.2
61Pm(145)
62Sm
150.4
63Eu
152.0
64Gd
157.3
65Tb
158.9
66Dy
162.5
67Ho
164.9
68Er
167.3
69Tm168.9
70Yb
173.0
71Lu
175.0
Actinide series90Th
232.0
91Pa
231.0
92U
238.0
93Np(237)
94Pu
(244)
95Am(243)
96Cm(247)
97Bk
(247)
98Cf
(251)
99Es
(252)
100Fm(257)
101Md(258)
102No(259)
103Lr
(262)
Elements with
similar
properties have
a repeating
pattern and are
aligned in
columns
Understanding Light
Classical Physics viewed energy as
continuous.ie. Any amount of energy could be
released. This was found to be false by Max Planck when
concerning the radiation emitted by a heated solid.
2
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Properties of Waves
Waves - a vibrating disturbance by which energy
is transmitted.
Waves are characterized by
Wavelength ()
Amplitude
Frequency ()
The speed (u) of the wave =
Propert ies of Waves
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Visible light consists of electromagnetic waves.
Electromagnetic
radiation
Energy
Units Joule
1 J = 1 kg m2/s2
Electric field component
Magnetic field component
c =
For electromagnetic radiation:
Speed of light in a vacuum: 3.00 10 8 m/s
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A photon has a frequency of 3.5 105 Hz.
Convert this frequency into wavelength (nm).
Does this frequency fall in the visible region?
What is the frequency (in Hz) of
light with a wavelength of 490 nm?
1. 6.12 1023
2. 6.12 105
3. 6.12 1014
4. 1.63 10-15
5. 1.63 10-6
Interactions of Waves
Interference
Constructive Interference
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Destructive Interference
Wave versus particle behavior
Diffraction -
Slit must be a
comparable size to
the wavelength
Interference Pattern
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Plancks Quantum Theory
When solids are heated they emit electromagnetic
radiation.
It was determined that the amount of radiation
energy emitted was related to its wavelength.
Classical physics could not account for this fact.
Planck solved the problem...
3
Plancks Quantum Theory
Plancks assumption: atoms and molecules could
emit (or absorb) energy only in discrete quantities.
These bundles of energy were called quantum -
the smallest quantity of energy that can be emitted.
E = h
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The Particle Nature of Light
Planck did not know the why of his discovery.
Einstein used Plancks Quantum Theory to help
explain something called the photoelectric effect
and then explained the why of Plancks theory.
The Photoelectic Effect
Light strikes the metal and ejects electrons.
What They Found
There was a certain
frequency where
below this frequencyno electrons were
ejected, no matter
how intense the light
was.
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What They Found
What They Found
Einsteins Explanation of the
Photoelectric Effect
Light is made of a stream of particles (called
photons).
Each photon has energy- Each photon, if it has enough energy, can knock
off one electron. (It must overcome the binding
energy ( BE ) of the electron.)
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h = KE + BE
Dual Nature of Light
1. Waves
2. Particles
Depending on the experiment, light behaves one
way or the other.
We will see later that matter has this nature also.
Calculations
So now you have these two equations:
c=
E=h
With these two equations if you know one of the
following, you can calculate the other two:
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When copper is bombarded with high-energy electrons, X rays
are emitted. Calculate the frequency and energy (in joules)
associated with the photons if the wavelength of the X rays is
0.154 nm.
1. 1.96 10181/s 1.29 10-15 J
2. 1.96 109 1/s 1.29 10-24 J
3. 4.62 107 1/s 3.03 10-26 J
4. 4.62 10-2 1/s 3.06 19-34 J
Frequency Energy
Bohrs Model of the
Hydrogen atom
4
Emission Spectra
The continuous or line spectra of radiation emitted
by substances.
Obtained by energizing a sample until it produces light
the light is passed through a prism
the rainbow produced is the spectrum
The spectrum is not necessarily in the visible region
of electromagnetic radiation.
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1. e- can only have specific (quantized) energy values
2. light is emitted as e- moves from one energy level to
another
Bohrs Model of the Atom (1913)
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The Dual Nature of Electrons
Electron only occupies certain fixed
distances.Why?
Louis de Broglie provided a solution.
5
Expected behavior of particles
Actual electron behavior
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h
mv
This equation is typically used to calculate the
wavelength
of a particle when the mass and velocity are
known.
Watch your units!
What is the de Broglie wavelength (in nm)
associated with a 2.5 g Ping-Pong ball traveling at
15.6 m/s?
h
mv
The Uncertainty Principle
We know electrons
have a wave nature.
We know electronshave a particle
nature.
6
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Heisenbergs Uncertainty
Principle
4hvmx
Uncertainty in position = x
Uncertainty in velocity = v
Quantum Mechanics and the
Atom
Electrons do not move as orbits about the nucleus.
Due to Heisenbergs Uncertainty Principle we can
only define regions in space where we have a high
probability of finding an electron.
Schrdinger equations -
These equations take into account the particle and
wave nature of the electron
These equations launched quantum mechanics.
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Solutions to the Schrdinger
Equation for the Hydrogen Atom
Complex mathematical functions but they give us
quantum numbers which define the orbitals.
The four quantum numbers:
The principal quantum number (n)
The angular momentum quantum number (l)
The magnetic quantum number (ml)
The spin quantum number (ms)
7
Principal Quantum number,n
n = 1, 2, 3, 4
The farther out the electron is, the larger, higher in
energy and more unstable the orbital.
All electrons with the same n value are in the same
(principal) shell.
Energy of an electron in hydrogen:
21
nRE Hn
RH= 2.181018 J
Rydberg constant
for Hydrogen
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The Angular Momentum Q.N., (l)
l= 0, 1, .(n-1)
Usually we call the subshells by the following
names.
Orbital or subshell names
l Name of
Orbital/Subshell
0
1
2
3
4
Note: Each principal quantum number has its ownallowable values of (l) because l goes up to (n-1)
In the shelln=4, what are the
names of the subshells it has?
1. s only
2. s and p3. s, p and d
4. s, p, d and f
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Magnetic Quantum Number, ml
ml= -l, .0..+
l
All electrons with the same n,l, ml are said to bein the same orbital.
Lets stop and derive a table of quantum numbers[n, l, ml].
Connections between Q.N.s
n l ml
Which of the following is not an
allowable set of quantum numbers
[n, l, ml]1. [1,0,0]
2. [2,2,-2]
3. [3,2,0]
4. [4,1,-2]
5. Both 1 and 2
6. Both 2 and 4
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Which set of quantum numbers
will identify an electron in a 4p
subshell?
1. [4, 3, 2]
2. [4, 1, 0]
3. [4, 1, -1]
4. [4, 2, 0]
5. Both 2 and 3
Atomic Spectroscopy Explained
Atom absorbs energy, electron promoted to
higher energy level. (Excited state.)
Electron emits photon of light. (Returns to
the ground state.
8
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For
Hydrogen
Notice how the levels
get closer together as
they go farther away
from the nucleus.
E = RH( )1 1n2f n
2i
This equation can onlybe used for
the Hydrogen atom
Connection between energy of the
electron and energy of the photon.
c
hEphoton
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Calculate the E of the electron of a hydrogen
atom as the electron drops from then = 5 state to
then = 3 state.
1. +2.91 x 10-20
2. -2.91 x 10-20
3. +1.55 x 10-19
4. -1.55 x 10-19
Calculate the wavelength (in nm) of a photon
emitted by a hydrogen atom when its electron
drops from then = 5 state to then = 3 state.
1. 323
2. 456
3. 646
4. 811
5. 1280
Atomic Orbitals
Orbitals are defined by
the Schrdinger
equations.
Regions in space where
there is a high
probability of finding
an electron.
9
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p orbital l= 1
d orbitals l= 2
f orbitals l= 3
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The Phase of Orbitals
Phase
Two dimensional waves.
Three dimensional waves
1s
2s 2p
3s 3p
4s 4p 4d
3d
Energy
Energy Levels in a Hydrogen Atom
1s
2s 2p
3s3p
4s
4p
4d
3d
Energy
Energy Levels in a Multi-electron Atom
Orbital Diagram
Shows what subshells (orbitals) are occupied by
electrons.
Ground state
10
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Electron Spin and the Pauli
Exclusion Principle
Electrons spin, either one way or the other.
All electrons have the same amount of spin.
Spin Quantum number (ms)
Example of an orbital diagram for hydrogen
Arrow shows the spin
Up arrow = +; down arrow =
1s
Pauli Exclusion Principle
No two electrons in an atom can have the same
four quantum numbers.
Result
Helium has two electrons in the atom
Orbital diagram:
1s
Quantum Numbers and
Orbital Diagrams
Each electron has a set of four quantum numbers
associated with it.
The first three, give the electrons location The forth gives the spin
1s
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Electron Configuration for
Multielectron atoms
We will learn to write the configuration for
ground state atoms.
Electrons are in their lowest energy state
possible.
Aufbau principle building up from lowest to
highest energy
11
For a many electron atom:E(s orbital) < E(p orbital) < E(d orbital) < E(f orbital)
1s
2s 2p
3s 3p
4s 4p 4d
3d
Energy
Energy Levels in a Hydrogen Atom
1s
2s 2p
3s3p
4s
4p
4d
3d
Energy
Energy Levels in a Multi-electron Atom
It will be necessary for you to know the
order of orbitals from lowest in energy to
highest energy.
The following is one way to learn the order.
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Element Orbital Diagram Electron Config. Q.N.
H
He
Li
Be
B
What are the quantum numbers
of the last two electrons of Be
electron configuration?
1. [2, 0, 0, ] [2, 0, 1, ]
2. [2, 0, 0, ] [2, 0, 0, ]
3. [2, 0, 0, ] [2, 0, 0, -]
4. [2, 0, 0, ] [3, 0, 0, ]
Hunds Rule
The most stable arrangement of electrons insubshells is the one with the greatest number of
parallel spins.
Result:
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Element Orbital Diagram Electron Config. Q.N.
C
N
O
F
Ne
Q
Which Q.N.s are different for the
last two electrons placed in
oxygen?1. n
2. l
3. ml
4. ms
5. l and ms
6. ml and ms
k3
Be able to duplicate this breakdown of the Periodic Table and
you can do the configuration of any element.
11A
188A
1H
1.00
8
22A
133A
144A
155A
166A
177A
2He4.00
3
3Li
6.94
1
4Be9.01
2
5B
10.8
1
6C
12.0
1
7N
14.0
1
8O
16.0
0
9F
19.0
0
10Ne20.1
8
11Na22.9
9
12Mg24.3
1
33B
44B
55B
66B
77B 8
98B
10 111B
122B
13Al26.9
8
14Si
28.09
15P
30.97
16S
32.06
17Cl
35.45
18Ar39.9
5
19K
39.10
20Ca40.0
8
21Sc44.9
6
22Ti
47.87
23V
50.94
24Cr52.0
0
25Mn54.9
4
26Fe55.8
5
27Co58.9
3
28Ni
58.69
29Cu63.5
5
30Zn65.3
9
31Ga69.7
2
32Ge75.5
9
33As74.9
2
34Se78.9
6
35Br79.9
0
36Kr83.8
0
37Rb
85.47
38Sr
87.62
39Y
88.91
40Zr
91.22
41Nb
92.91
42Mo
95.96
43Tc
(98)
44Ru
101.1
45Rh
102.9
46Pd
106.4
47Ag
107.9
48Cd
112.4
49In
114.8
50Sn
118.7
51Sb
121.8
52Te
127.6
53I
126.9
54Xe
131.3
55Cs132.
9
56Ba137.
3
57La138.
9
72Hf
178.
5
73Ta180.
9
74W
183.
8
75Re186.
2
76Os190.
2
77Ir
192.
2
78Pt
195.
1
79Au197.
0
80Hg200.
6
81Tl
204.
4
82Pb207.
2
83Bi
209.
0
84Po
(209)
85At(210)
86Rn(222)
87Fr
(223)
88Ra
(226)
89Ac(227)
104Rf
(261)
105Db
(262)
106Sg
(266)
107Bh(264)
108Hs
(269)
109Mt
(268)
110Ds
(271)
111Rg(272)
112Cn(285)
113 114Fl
(289)
115 116Lv
(292)
117 118
Lanthanide series
58Ce140.
1
59Pr
140.9
60Nd144.
2
61Pm(145)
62Sm150.
4
63Eu152.
0
64Gd157.
3
65Tb158.
9
66Dy162.
5
67Ho164.
9
68Er
167.3
69Tm168.
9
70Yb173.
0
71Lu175.
0
Actinide series
90Th232.
0
91Pa
231.0
92U
238.0
93Np(237)
94Pu
(244)
95Am(243)
96Cm(247)
97Bk
(247)
98Cf
(251)
99Es
(252)
100Fm(257)
101Md(258)
102No(259)
103Lr
(262)
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Slide 92
k3 diagram used for the question has points to the the two paramagnetic electrons of oxygenkwoodru, 10/29/2007
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Procedure for writing the
Electron Configuration
Find the nearest noble gas which comes before the
element. Place the noble gas symbol in square brackets.
This is called the noble gas core.
Example: [He]
Now use the breakdown of the periodic table that
you learned to add electron in until you have
reached the element of interest.
Write the electron configuration of Cl.
11A
188A
1H
1.008
22A
133A
144A
155A
166A
177A
2He4.00
3
3Li
6.941
4Be9.01
2
5B
10.81
6C
12.01
7N
14.01
8O
16.00
9F
19.00
10Ne20.1
8
11Na22.9
9
12Mg24.3
1
33B
44B
55B
66B
77B 8
98B
10 111B
122B
13Al26.9
8
14Si
28.0
9
15P
30.9
7
16S
32.0
6
17Cl
35.4
5
18Ar39.9
5
19K
39.10
20Ca40.0
8
21Sc44.9
6
22Ti
47.87
23V
50.94
24Cr52.0
0
25Mn54.9
4
26Fe55.8
5
27Co58.9
3
28Ni
58.69
29Cu63.5
5
30Zn65.3
9
31Ga69.7
2
32Ge75.5
9
33As74.9
2
34Se78.9
6
35Br79.9
0
36Kr83.8
0
37Rb85.4
7
38Sr
87.62
39Y
88.91
40Zr
91.22
41Nb92.9
1
42Mo95.9
6
43Tc(98)
44Ru101.
1
45Rh102.
9
46Pd106.
4
47Ag107.
9
48Cd112.
4
49In
114.8
50Sn118.
7
51Sb121.
8
52Te127.
6
53I
126.9
54Xe131.
3
55Cs132.
9
56Ba137.
3
57La138.
9
72Hf
178.5
73Ta180.
9
74W
183.8
75Re186.
2
76Os190.
2
77Ir
192.2
78Pt
195.1
79Au197.
0
80Hg200.
6
81Tl
204.4
82Pb207.
2
83Bi
209.0
84Po
(209)
85At(210)
86Rn
(222)
87Fr
(223)
88Ra
(226)
89Ac(227)
104Rf
(261)
105Db(262)
106Sg
(266)
107Bh(264)
108Hs
(269)
109Mt
(268)
110Ds
(271)
111Rg(272)
112Cn
(285)
113 114Fl
(289)
115 116Lv
(292)
117 118
Lanthanide series
58Ce140.
1
59Pr
140.9
60Nd144.
2
61Pm(145)
62Sm150.
4
63Eu152.
0
64Gd157.
3
65Tb158.
9
66Dy162.
5
67Ho164.
9
68Er
167.3
69Tm168.
9
70Yb173.
0
71Lu175.
0
Actinide series
90Th232.
0
91Pa
231.0
92U
238.0
93Np(237)
94Pu
(244)
95Am(243)
96Cm(247)
97Bk
(247)
98Cf
(251)
99Es
(252)
100Fm(257)
101Md(258)
102No(259)
103Lr
(262)
Sn:
V: 1
1A188A
1H
1.008
22A
133A
144A
155A
166A
177A
2He4.00
3
3Li
6.941
4Be9.01
2
5B
10.81
6C
12.01
7N
14.01
8O
16.00
9F
19.00
10Ne20.1
8
11Na22.9
9
12Mg24.3
1
33B
44B
55B
66B
77B 8
98B
10 111B
122B
13Al26.9
8
14Si
28.09
15P
30.97
16S
32.06
17Cl
35.45
18Ar39.9
5
19K
39.1
0
20Ca40.0
8
21Sc44.9
6
22Ti
47.8
7
23V
50.9
4
24Cr52.0
0
25Mn54.9
4
26Fe55.8
5
27Co58.9
3
28Ni
58.6
9
29Cu63.5
5
30Zn65.3
9
31Ga69.7
2
32Ge75.5
9
33As74.9
2
34Se78.9
6
35Br79.9
0
36Kr83.8
0
37Rb85.4
7
38Sr
87.6
2
39Y
88.9
1
40Zr
91.2
2
41Nb92.9
1
42Mo95.9
6
43Tc(98)
44Ru101.
1
45Rh102.
9
46Pd106.
4
47Ag107.
9
48Cd112.
4
49In
114.
8
50Sn118.
7
51Sb121.
8
52Te127.
6
53I
126.
9
54Xe131.
3
55Cs132.
9
56Ba137.
3
57La138.
9
72Hf
178.5
73Ta180.
9
74W
183.8
75Re186.
2
76Os190.
2
77Ir
192.2
78Pt
195.1
79Au197.
0
80Hg200.
6
81Tl
204.4
82Pb207.
2
83Bi
209.0
84Po
(209)
85At(210)
86Rn
(222)
87Fr
(223)
88Ra
(226)
89Ac(227)
104Rf
(261)
105Db(262)
106Sg
(266)
107Bh(264)
108Hs
(269)
109Mt
(268)
110Ds
(271)
111Rg(272)
112Cn
(285)
113 114Fl
(289)
115 116Lv
(292)
117 118
Lanthanide series
58Ce140.
1
59Pr
140.9
60Nd144.
2
61Pm(145)
62Sm150.
4
63Eu152.
0
64Gd157.
3
65Tb158.
9
66Dy162.
5
67Ho164.
9
68Er
167.3
69Tm168.
9
70Yb173.
0
71Lu175.
0
Actinide series
90Th232.
0
91Pa
231.
0
92U
238.
0
93Np(237)
94Pu
(244)
95Am(243)
96Cm(247)
97Bk
(247)
98Cf
(251)
99Es
(252)
100Fm(257)
101Md(258)
102No(259)
103Lr
(262)
7/25/2019 Chem-01-Atoms ElectronicStructure Lecture Notes
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The electron configuration of
Antimony is1. [Kr]5s25d105p6
2. [Kr]5s2
4d10
5p3
3. [Xe]5s24d105p3
4. [Xe]5s25d105p2
A few other points to know. Transition metals - have incompletely filled d
subshells or readily give rise to cations that have
incompletely filled d subshells.
Exception to learn:
This is due to the stability achieved with half filled
or filled subshells.
Examples of the Exceptions
chromium
[Ar] 4s23d4
silver
[Kr]5s24d9
7/25/2019 Chem-01-Atoms ElectronicStructure Lecture Notes
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Lanthanides (rare earths) - incompletely filled
4f subshells or readily give rise to cations that
have incompletely filled 4f subshells.
Actinide series - most of these not found in nature
but have been synthesized.
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