Periodic Relationships Among the Elements Chapter 5 Copyright © The McGraw-Hill Companies, Inc....
Transcript of Periodic Relationships Among the Elements Chapter 5 Copyright © The McGraw-Hill Companies, Inc....
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Periodic Relationships Among the Elements
Chapter 5
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
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History of the Periodic Table
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•Arranged the elements by increasing ATOMIC MASS and saw a periodic repetition of properties
•Produced the first PERIODIC TABLE – 1871•The table placed elements with similar properties in the same column
•Kept “holes” for undiscovered elements, and predicted the properties in advance
Dimitri Mendeleev
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Mendeleev’s Periodic Table
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Properties of elements predicted by Mendeleev
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H.G. Moseley in 1914
• Rearranged the elements by:ATOMIC NUMBER
• This has become theMODERN PERIODIC TABLE
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Electrons and Ions on the Periodic Table
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Review: Valence Electrons
What are valence electrons?
*Remember: Elements in a group have similar properties because they have the same valence electron configuration
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Valence Electron Configuration
Group e- config Valence electrons
Expected Charges
1 ns1
2 ns2
13 ns2np1
14 ns2np2
15 ns2np3
16 ns2np4
17 ns2np5
18 ns2np6
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+1
+2
+3 -1-2-3
Charges Of Representative Elements
8.2
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Na+
Al3+
F-
O2-
N3-
What ions are isoelectronic with Neon?
Isoelectronic: Elements and ions that have the same number of electrons and therefore the same electron configuration
Mg2+
What would the electron configuration be?___________
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When a cation is formed from an atom of a transition metal, electrons are always removed first from the s orbital and then from the d orbitals.
Fe: [Ar]4s23d6
Fe2+: [Ar]4s03d6 or [Ar]3d6
Fe3+: [Ar]4s03d5 or [Ar]3d5
Mn: [Ar]4s23d5
Mn2+: [Ar]4s03d5 or [Ar]3d5
Forming Ions with Transition Metals
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Periodic Table Groups and Properties
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Periodic Table Groups
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• Very unreactive due to full valence shell
• Odorless, colorless, gases
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1
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• Extremely reactive; not found in pure form in nature
•Silverly, soft• form strong bases in water
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• less reactive than alkali, but still not found in pure form
• also form strong bases in water
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Transition Metals
• typical metallic properties• form colorful ions
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• shiny metals• similar reactivity to Group 2• filling 4f sublevel
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• mainly synthetic (created in a lab)• all radioactive
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• very reactive• volatile (exist as gases)
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1
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Properties of Metals
1. shiny (luster)2. conductors of heat and electricity3. reactive with acids4. ductile
– can be stretched into a wire
5. malleable – can be hammered or rolled into sheets
6. forms positive ions (by losing e-)
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Properties of Nonmetals
1. dull and brittle2. poor conductors of heat and
electricity3. does not react with acids4. usually gases at room temp.5. forms negative ions (by gaining e-)
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What are properties of Metalloids??
•In the middle!•Metalloids have properties of BOTH!! (metals and nonmetals)
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Periodic Trends
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PERIODIC LAW
When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic (repeating) pattern.
patterns on the periodic table are called periodic trends
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Atomic Radius
half the distance from center-center of 2 like atoms
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Atomic Radii DOWN a Group
↓As you go down there are more energy levels, the atom size gets larger
↓There are more electrons between the nucleus and the outermost energy level which increases the shielding effect
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Shielding Effect
• reduction of attraction between positive nucleus and outermost electrons
•outer electrons are not held tight and can move away
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Na
Atomic Radius: down group
P
PP
X
X
X
P
X
P
X
P
X
P
PP
P
P
X
X
X
X
X
XP
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K
Atomic Radius: down group
P
PP
X
X
X
P
X
P
X
P
X
P
PP
P
P
X
X
X
X
X
PX
X
X
X
X
X
X
X
X
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Atomic Radii DOWN a Group
↓DOWN THE GROUP ATOMIC RADIUS
INCREASES
more energy levels, the larger the size of the atom
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Atomic Radii ACROSS a Period
→ Each atom gains one proton and one electron in the same energy level
→Each added electron is the same distance from the nucleus
→The positive charge increases and exerts a greater force on the electrons pulling them closer to the nucleus
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REMEMBER!
PROTONSare bigger and stronger!
electrons are smaller and weaker!P
+ + - -
e
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Ask yourself, how effective are the positive protons pulling in the electrons?
Atomic Radii ACROSS a Period
Effective nuclear charge: “positive charge” felt by an electron.
Within a period, every time a proton is added, the effective nuclear charge increases… so the radius decreases
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Atomic Radius: across period
P
PP
X
X
X
P
X
P
X
P
X
P
PP
P
P
X
X
X
X
X
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Atomic Radii ACROSS a Period
→ACROSS THE PERIOD ATOMIC RADIUS
DECREASES
greater effective nuclear charge (more protons), greater pull on the electrons, smaller radius
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Ionic Radii
half the distance from center-center of 2 like ions
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Ionic Radius DOWN a Group
↓As you go down a group another energy level is added, increasing the size of the atom.
(just like the atomic radius)
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Ionic Radius DOWN the Group
↓DOWN THE GROUP IONIC RADIUS
INCREASES
more energy levels, increase in atom size
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Ionic Radius ACROSS the Period
Cation: positive ion formed from losing an electron
→ A cation is always smaller than the original atom
→The more electrons lost the more protons available to attract a smaller number of electrons.
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Na +
Ionic Radius
P
PP
XP
X
X
PP
P
PP
P
P
X
X
X
X
X
X
X
X
XP
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Ionic Radius ACROSS the Period→ACROSS THE PERIOD IONIC RADIUS
DECREASES
greater effective nuclear charge, less electrons, the shorter the radius
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Ionic Radius ACROSS the Period
Anion: negative ion formed from gaining an electron
→ A anion is always larger than the original atom
→The more electrons gained, the less protons available to attract a larger number of electrons.
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F
Ionic Radius
P
PP
XP
X
X
PP
P
PP
P
P
X
X
X
X
X
X
X
X
P
-
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Ionic Radius ACROSS the Period
→ACROSS THE PERIOD IONIC RADIUS
DECREASES
As electrons are added the atom gets larger from right to left,
General trend from left to right is decreasing
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Ionic Radii
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amount of energy needed to remove an electron from an atom
Ionization Energy
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X X+ + e-
X X2++ e-
X X3++ e-
I1 first ionization energy
I2 second ionization energy
I3 third ionization energy
I1 < I2 < I3
Multiple Ionization Energies
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Ionization Energy DOWN a Group
↓As you go down a group atoms become larger
↓The more electrons in an atom between the nucleus and valence shell, the greater the shielding effect
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Ionization Energy DOWN a Group
↓DOWN THE GROUP IONIZATION ENERGY
DECREASES
greater distance from the nucleus, greater shielding effect
less energy needed to remove electron
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Ionization Energy ACROSS a Period
→As atomic radius decreases there is a greater attraction between protons and electrons. (effective nuclear charge)
→The stronger the attraction, the more energy needed to remove an electron.
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Ionization Energy ACROSS a Period
→ACROSS THE PERIOD IONIZATION ENERGY
INCREASES
greater the effective nuclear charge,more energy required to remove electron
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Electronegativity
It is a “tug of war” between the two atoms of a bond
H F :
::
Which is the more electronegative element?
.
..
ability of an atom to attract electrons
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Electronegativity DOWN the Group
↓The farther away from the nucleus, the greater the shielding effect
↓The larger the atom, the less likely it is to accept more electrons.
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Electronegativity DOWN the Group
↓DOWN THE GROUP ELECTRONEGATIVITY
DECREASES
farther the distance from the nucleus, lower ability to attract electrons
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Electronegativity ACROSS the Period
→As you go across a period atomic radius decreases because there is a greater effective nuclear charge
→Metals do not attract electrons. →Non-metals do attract electrons.
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Electronegativity ACROSS the Period
→ACROSS THE PERIOD ELECTRONEGATIVITY
INCREASES
greater effective nuclear charge, greater ability to attract electrons
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the energy change that occurs when an electron is added to an atom to form an
anion.
Increases with ability to attract and hold an electron (electronegativity)
Electron Affinity
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Electron Affinity DOWN the Group
↓The larger the atom the more difficult to accept electrons
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Electron Affinity DOWN the Group
↓DOWN THE GROUP ELECTRON AFFINITY
DECREASES
farther the distance from the nucleus,does not want to gain electrons
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Electron Affinity ACROSS the Period
→As effective nuclear charge gets stronger, it is easier to attract an electron.
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Electron Affinity ACROSS the Period
→ACROSS THE PERIOD ELECTRON AFFINITY
INCREASESgreater effective nuclear charge,
easily forms anions
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Other TrendsReactivity of Metals Video 1Reactivity of Metals Video 2
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Incr
easi
ng r
eact
ivity
METAL REACTIVITY
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Incr
easi
ng r
eact
ivity
NONMETAL REACTIVITY