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Chem 101 > exam 3: chapters 8 & 9 > Flashcards

exam 3: chapters 8 & 9 Flashcards

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1
Q

Ionic bond

A

metal + nonmetal
(cation + anion)
- EN > 1.7

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2
Q

Covalent

A

nonmetal + nonmetal
- sharing of e- b/w 2 atoms

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3
Q

Nonpolar

A

covalent b/w same element
- equal pull

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4
Q

ionic bonding

A

metal loses e-, nonmetal gains e-

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5
Q

Born-Haber Cycle (energetics of ionic bonding):

A
  1. Break into separate elements
  2. Add energy (heat) to transform Na (s)(g)
  3. Add energy (heat) to transform ½Cl2 (g)  (g)
  4. Electron is transfers/added to Cl (g)
  5. Opposites attract; Na and Cl attract
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6
Q

Lattice energy

A

energy to separate 1 mol of (s) –> 2 ions (g)
- ↑ w/ ↑ charge of ions
- ↑ w/ ↓ size of ions

charge > energy

  • consumes energy
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7
Q

Lewis’ Rule

A

Column/group # = # of valence e-
- ex: group 3A = 3 v. e-

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8
Q

Octet rule

A

atoms tend to gain, lose, or share electrons until they’re surrounded by 8 valence e-
- (full s and p subshells)

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9
Q

↑ # bonds = __ distance

A

= ↓ distance
- additional bonding e- attract nuclei more

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10
Q

Bond polarity

A

measures how equal/unequal e- shared in covalent bond

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11
Q

nonpolar covalent bond

A

e- shared equally
- EN < 0.4

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12
Q

polar covalent bond

A

1 atom exerts greater attraction for the bonding e-
- partially (+) or partially (-)
- 0.4 < EN < 1.7

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13
Q

Electronegativity (EN)

A

ability/strength of atom to attract e-
- increase left–>right, bottom–>top

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14
Q

Polar molecule

A

separation of (+) and (-) charges in molecule
- unequal pull

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15
Q

dipole

A

2 electrical charges of = magnitude but opposite sign separated by distance

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16
Q

dipole moment (μ)

A

2 equal & opposite charges (Q+/Q-) separated by distance (r)
- μ = Qr
- Unit (μ) = D

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17
Q

Formal charge =

A

= (# v.e. atom brings) – (# e- surrounding on LS)

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18
Q

Resonance structures

A

1 LS can’t accurately depict molecule
- Need multiple LS
- ex: Ozone (O3)

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19
Q

Bond angles

A

angles made by lines joining nuclei of atoms

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20
Q

Valence-Shell Electron-Pair Repulsion Model:

A

Electron pairs repel each other
- best arrangement = minimizes repulsions

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21
Q

region e- most likely to be found

A

bonding pair

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22
Q

Hypervalent

A

more than octet of e-
- break octet rule

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23
Q

Bond dipole

A

dipole moment w/ 2 atoms
- Bond dipole and dipole moments = vector quantities
- must consider 3D shape

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24
Q

nonpolar bond dipole

A

equal/opposite bond dipoles = symmetric
- Linear

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25
Q

polar bond dipole

A

bent in nature = asymmetric
- Overall dipole moment = up/towards
O (partial -) away H (partial +)

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26
Q

Valence-bond theory

A

“overlap” of orbitals
- Sharing of space b/w 2 e- of opposite spin = covalent bond
- share space b/w nuclei

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27
Q

Hybrid orbitals

A

“mixing” of 2+ atomic orbitals on the same atom

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28
Q

degenerate orbitals

A

“new orbitals” after hybridization
- 2 orbitals mix –> create 2 orbitals
- 6 e- start –> 6 e- end

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29
Q

Orbital Shape

A

orbitals in bonded molecules (molecular orbitals) have diff shape an unbonded atom (atomic orbitals)

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30
Q

Orbital Energy Level

A

energy level changes from atomic  molecular

31
Q

Sigma (σ) bond

A

to-head overlap (direct collision @ end points) ; forms covalent bond
- cylindrical symmetry of e- density about nuclear axis

32
Q

Pi (∏) bond

A

sideways overlap of p orbitals
- e- density above and below nuclear axis
- ALWAYS involves p orbitals

33
Q

localized electrons

A

σ, ∏, lone pair:
- Bonding e- shared only b/w 2 atoms

34
Q

delocalized electrons

A

∏, lone pair:
- Bonding e- shared by 3+ atoms
- Due to Resonance!

35
Q

largest lattice energy magnitude

A

large charge + small ion

36
Q

ionic size increases…

A

from top to bottom (right to left)

37
Q

polarity is based on

A

electronegativity

38
Q

acid in Lewis Structure

A

O-H

39
Q

average bond order =

A

(# of bonds)/(# of bonding domains)

40
Q

hybridization =

A

ED # - 1 (ex: N = 4 ED = sp3)

41
Q

zero dipole moment

A

nonpolar
- equal pull

42
Q

nonzero dipole moment

A

polar
- unequal pull

43
Q

When to subtract from bond angles?

A

1 lone pair = -2 degrees

44
Q

an atom with low first ionization energy and low electron affinity is more likely to form a ___.

A

more like to form a cation (than an anion)

45
Q

T/F: the most common ion for an atom of a representative element generally adopts a noble-gas electron configuration

A

true

46
Q

the stability of KBr is due to the _______ between the potassium ions and the bromide ions

A

electrostatic attraction

47
Q

the attraction b/w cations and anions increases as the ___ increase.

A

charges on the ions

48
Q

the attraction b/w cations and anions decreases as the ___ increase.

A

radii of the ions

49
Q

what happens to electron density as you increase the distance between nuclei in a covalent bond?

A
  • repulsions in nuclei decrease
  • attraction b/w nuclei and e- decrease
  • repulsions b/w e- = unaffected
50
Q

cations

A

(+), metal, smaller radius

51
Q

anions

A

(-), nonmetal, larger radius

52
Q

strength of a bond increases, as # of __ increase

A

e-
- ex: H2 > H2+

53
Q

electron affinity vs electronegativity

A

electron affinity- energy released when 1 atom gains an e- to form a (1-) ion
electronegativity- ability of atom to attract e-
- no units

54
Q

electron affinity vs electronegativity

A
  • electron affinity- energy released when 1 atom gains an e- to form a (1-) ion
  • electronegativity- ability of atom to attract e-
    - no units
55
Q

elements w/ high EN, usually also have high ____

A

first ionization energy and electron affinity

56
Q

Benzene:

A

{circles inside of hexagon}
- circle = 3 double bonded C (w/ resonance- 1 single)
- vertices on hexagon = 1 carbon atom
- H atoms = omitted
- notation = blend of 2 = resonance structures

57
Q

reaction enthalpy can be estimated by:

A
  • energy added to break bonds + energy released forming bonds
58
Q

avg bond enthalpies

A
  • Energy to break bonds
  • More bonds = more energy to break
  • # of bonds ↑, bond length ↓, bond enthalpy ↑
59
Q

dipole energy/direction of arrow is based on ___

A

Electronegativity

60
Q

in valence bond theory, bonds are formed by the overlap of ___

A

atomic orbitals in different atoms

61
Q

as two atoms are pulled apart, the overlap between their atomic orbitals ___

A

decreases

62
Q

bond order =

A

1/2 (# bonding electrons - # nonbonding electrons)

63
Q

(*) =

A

antibonding molecular orbital

64
Q

paramagnetism

A

more unpaired e- = stronger attractive force

65
Q

diamagnetism

A

no unpaired e- = weakly repelled by magnetic field

66
Q

SO3 is polar or nonpolar?

A

polar

67
Q

IF5 is polar or nonpolar?

A

polar

68
Q

PCl3 is polar or nonpolar?

A

polar

69
Q

XeF4 is polar or nonpolar?

A

nonpolar
- octahedral ; square planar

70
Q

partial charge for diatomic molecules

A

partial = (Formal Charge on atoms of interest) / (# of atoms of interest)
- ex: NO3

71
Q

partial charge for diatomic molecules

A

partial = (Formal Charge on atoms of interest) - (# of atoms of interest)
- ex: NO3
- (-1 + -1 + 0) / (3)

72
Q

sulfuric acid

A

H2SO4

73
Q

acetic acid

A

CH3COOH

74
Q

perchloric acid

A

HClO4

Chem 101 (11 decks)

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