Stillwagon Test 2 Electrons & Bonding

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21 Terms

1
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metalloids on table

- divide periodic table along zig zag

- diagonal, down over, down over, diagonal

<p>- divide periodic table along zig zag</p><p>- diagonal, down over, down over, diagonal</p>
2
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principle quantum #

n= any pos integer value

- (2n)^2 = # of e- per energy level

- describes energy level of e- (1-7)

<p>n= any pos integer value</p><p>- (2n)^2 = # of e- per energy level</p><p>- describes energy level of e- (1-7)</p>
3
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angular momentum quantum number

l < or = n-1

- indicates shape of the electron's orbital

s: sphere

p: figure 8

d: clover

f: tetrahedral

<p>l < or = n-1</p><p>- indicates shape of the electron's orbital</p><p>s: sphere</p><p>p: figure 8</p><p>d: clover</p><p>f: tetrahedral</p>
4
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magnetic quantum number

m = values from l to -l (if l=2 m could = 2, 1, 0, -1, -2)

- describes shape of orbital in 3D around axes (x, y, z)

- indicates the orientation of the orbital around the nucleus

s: 1 orientation

p: 3 orientations

d: 5 orientations

f: 7 orientations

EACH ORIENTATION CAN HOLD MAX 2 ELECTRONS!!!

<p>m = values from l to -l (if l=2 m could = 2, 1, 0, -1, -2)</p><p>- describes shape of orbital in 3D around axes (x, y, z)</p><p>- indicates the orientation of the orbital around the nucleus</p><p>s: 1 orientation</p><p>p: 3 orientations</p><p>d: 5 orientations</p><p>f: 7 orientations</p><p>EACH ORIENTATION CAN HOLD MAX 2 ELECTRONS!!!</p>
5
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spin quantum number

- ms = 1/2 or -1/2

- indicates the spin orientation (+/- 1/2) of an electron in an orbital

- 2 e- in same orientation must spin in different directions (pos is upwards, neg is downwards)

<p>- ms = 1/2 or -1/2</p><p>- indicates the spin orientation (+/- 1/2) of an electron in an orbital</p><p>- 2 e- in same orientation must spin in different directions (pos is upwards, neg is downwards)</p>
6
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Aufbau Principle

electrons occupy the orbitals of lowest energy levels first

<p>electrons occupy the orbitals of lowest energy levels first</p>
7
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Pauli Exclusion Principle

- NO 2 ELECTRONS CAN BE IN SAME PLACE AT SAME TIME

- orbital may only contain 2 e- each w opposite spin directions

(no two electrons in the same atom can have the same set of four quantum numbers)

<p>- NO 2 ELECTRONS CAN BE IN SAME PLACE AT SAME TIME</p><p>- orbital may only contain 2 e- each w opposite spin directions</p><p>(no two electrons in the same atom can have the same set of four quantum numbers)</p>
8
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Hund's Rule

e- will fill up each orientation once before pairing up

<p>e- will fill up each orientation once before pairing up</p>
9
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cations and anions

cations gain e-, anions lose e-

<p>cations gain e-, anions lose e-</p>
10
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how many VSEPR models are there?

6 (or 5 with bent having 2 possible bond angles)

<p>6 (or 5 with bent having 2 possible bond angles)</p>
11
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linear

bond angle 180 degrees

<p>bond angle 180 degrees</p>
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bent 1 pair

IF 1 PAIR OF LONE ELECTRONS:

- bond angle 120 degrees

<p>IF 1 PAIR OF LONE ELECTRONS:</p><p>- bond angle 120 degrees</p>
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bent 2 pairs

IF 2 PAIRS OF LONE ELECTRONS:

- bond angle 105 degrees

<p>IF 2 PAIRS OF LONE ELECTRONS:</p><p>- bond angle 105 degrees</p>
14
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trigonal planar

3 bonds, 0 lone pairs, bond angle 120 degrees

<p>3 bonds, 0 lone pairs, bond angle 120 degrees</p>
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trigonal pyramidal

3 bonds, 1 lone pair, bond angle 107 degrees

<p>3 bonds, 1 lone pair, bond angle 107 degrees</p>
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tetrahedral

bond angle 109.5 degrees

<p>bond angle 109.5 degrees</p>
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Sheilding

core electrons partially block the attraction between the nucleus and the valence electrons

<p>core electrons partially block the attraction between the nucleus and the valence electrons</p>
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Periodicity

the repeating patterns of chemical and physical properties of the elements moving down/across periodic table

<p>the repeating patterns of chemical and physical properties of the elements moving down/across periodic table</p>
19
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atomic radius

- 1/2 distance between 2 nuclei in molecule with identical atoms

- gets bigger as you go down (energy levels increase size)

- gets smaller as you go across (adds p+, force becomes strong)

<p>- 1/2 distance between 2 nuclei in molecule with identical atoms</p><p>- gets bigger as you go down (energy levels increase size)</p><p>- gets smaller as you go across (adds p+, force becomes strong)</p>
20
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ionization energy

- energy required to lose e-

- gets smaller as you go down table (shielding makes losing e- easier)

- gets bigger as you go across table (harder to lose e- closer you are to 8)

<p>- energy required to lose e-</p><p>- gets smaller as you go down table (shielding makes losing e- easier)</p><p>- gets bigger as you go across table (harder to lose e- closer you are to 8)</p>
21
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Electronegativity

- the ability of an atom to attract shared electrons when the atom is in a compound

- gets smaller going down table

-gets larger going across table (nonmetals want to attract e-)

<p>- the ability of an atom to attract shared electrons when the atom is in a compound</p><p>- gets smaller going down table</p><p>-gets larger going across table (nonmetals want to attract e-)</p>