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CHM 1220 > Exam 2 > Flashcards

Exam 2 Flashcards

1
Q

fixed charges

A

group 1 & 2; Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag+

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2
Q

transition metals lose __ e- first

A

ns

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3
Q

p-block loses _ e- first

A

p

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4
Q

d-block loses __ e- first

A

s

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5
Q

e- configuration of Mn vs Mn +2

A

4s2 3d5

Mn +2: 3d5

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6
Q

e- configuration of Cu vs Cu +2

A

4s1 3d10

Cu +2: 3d9

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7
Q

e- configuration of In vs In +1 vs In +3

A

5s2 5p1
In +1: 5s2
In +3: lost whole shell (NT)

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8
Q

what are the potential charges for Sn

A

Sn: 5s2 5p2

+2 and +4

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9
Q

what are the potential charges for Pb

A

+2 and +4

Pb: 6s2 6p2

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10
Q

what are the potential charges for Sb

A

+3 and +5

Sb: 5s2 5p3

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11
Q

anion is __ than atom

A

larger

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12
Q

cation is __ than atom

A

smaller

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13
Q

lewis dot formula

A

A formula using dots to represent valence electrons

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14
Q

octet rule

A

In forming covalent bonds, atoms tend toward having a full eight electrons in their valence shell
*H is exception bc it has two electrons in its valence shell.

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15
Q

ionic radius

A

a measure of the size of the spherical region around the nucleus of an ions within which the e- are most likely to be found
- can be measured using known distances between nuclei in crystals

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16
Q

isoelectric

A

different species having the same number and configuration of electrons.

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17
Q

organize the following isoelectronic series in decreasing order:
F-, O 2-, Mg +2

A

O 2-, F-, Mg +2

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18
Q

bond length

A

The distance between the atoms when energy is at a minimum

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19
Q

polar covalent bond

A

a covalent bond in which the bonding electrons spend more time near one atom than near the other atom.

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20
Q

what elements have the highest electronegativity?

A

Cl, F, O, N

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21
Q

what are the 3 exceptions to lewis dot diagrams

A
  • odd # of e-
  • too few e-
  • too many e-
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22
Q

example of having an odd # of e-

A

NO (11)

- not stable

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23
Q

example of having too few e-

A

Be, Al, B

  • Be forms 2 bonds
  • Al and B form 3 bonds
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24
Q

example of having too many e-

A

XeF4

8 + 4(7) = 36 e-

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25
Q

formal charge

A

group # - # of bonds - # of lone pair e-

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26
Q

electronegativity

A

a measure of the ability of an atom in a molecule to draw bonding electrons to itself.

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27
Q

single bond

A

a covalent bond in which one pair of electrons is shared by two atoms.

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28
Q

double bond

A

a covalent bond in which two pairs of electrons are shared by two atoms.
*Double bonds form primarily with C, N, O, and S atoms.

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29
Q

triple bond

A

a covalent bond in which three pairs of electrons are shared by two atoms.
*Triple bonds form primarily with C and N atoms.

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30
Q

rules for formal change

A
  1. Half of the electrons of a bond are assigned to each atom in the bond.
  2. Both electrons of a lone pair are assigned to the atom to which the lone pair belongs.
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31
Q

resonance

A

the electron structure of a molecule or ion having delocalized bonding is given by writing all possible electron-dot formulas. They are connected with a double-headed arrow.

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32
Q

expanded octet

A

periods 3,4, 5,… non-metals

*P, S

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33
Q

bond order

A 
# of pairs of e- in a bond 
*larger the bond order, shorter the bond length
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34
Q

bond length

A

distance between nuclei in a bond

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35
Q

which is the shortest: C-C, O=O, N≡N

A

N≡N

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36
Q

bond energy

A

energy it takes to break a bond

  • can be used to measure ∆H
  • break multiple bonds to get a single bond
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37
Q 
2 H2 (g) + O2 (g) -> 2 H2O (g) 
using the chart, find the ∆H
A

-482 kJ

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38
Q

VSEPR

A

valence shell electron pair repulsion model

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39
Q

molecular geometry

A

general SHAPE of a molecule

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40
Q

arrangement

A

all e- regions

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41
Q

shape

A

bonding regions

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42
Q

region

A

1 lone pair, 1 single bond, 1 double bond, 1 triple bond

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43
Q

2 e- pairs are __ apart

A

180º (linear)

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44
Q

3 e- pairs are __ apart

A

120º (trigonal planar)

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45
Q

4 e- pairs are __ apart

A

109.5º(tetrahedral)

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46
Q

5 e- pairs are arranged with 3 pairs __ and 2 pairs __ and __ to each other

A

120º; 90º and 180º (trigonal bipyramidal)

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47
Q

6 e- pairs are __ apart

A

90º (octahedral)

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48
Q

total number of valence e- in BeCl2

A

16

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49
Q

total number of valence e- in NO2-

A

18

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50
Q

lone pairs in 5 e- pairs are

A

equitorial

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51
Q

what is the shape of TeCl4?

A

trigonal bipyramid

*see-saw arrangement

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52
Q

what is the shape of SF4?

A

trigonal bipyramid

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53
Q

what is the geometry of XeF2?

A

linear

*arrangement: trigonal bipyramid

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54
Q

arrangment

A

looks at ALL regions

55
Q

shape/geometry

A

starts with arrangement and omits lone pairs (only uses bonds)

56
Q

what is the geometry of IF5?

A

square pyramidal

57
Q

predicting bond angles: 180º

A

linear

58
Q

predicting bond angles: 120º

A

trigonal planar

59
Q

predicting bond angles: 109.5º

A

tetrahedral

60
Q

lone pairs push __ closer together and tend to require more space than corresponding pair

A

bonds

61
Q

lone pairs tend to __ bond angle

A

reduce

62
Q

double bonds require __ space than single bonds & cause bond angle to constrict/reduce

A

more

63
Q

dipole moment

A

a quantitative measure of the degree of charge separation in a molecule

  • dipole moment of a molecule can affect its properties
  • indicator of polarity on molecule
64
Q

are diatomic molecules polar or non-polar?

A

non-polar

65
Q

is CO2 polar or non-polar?

A

the bonds are polar, the molecule is non-polar

66
Q

is SO2 linear or bent?

A

bent

67
Q

is PH3 trigonal planar or trigonal pyramid?

A

trigonal pyramid

68
Q

molecular geometry of AX

A

linear

69
Q

molecular geometry of AX2

A

linear, bent

70
Q

molecular geometry of AX3

A

trigonal planar, trigonal pyramidal, T-shaped

71
Q

molecular geometry of AX4

A

tetrahedral, square planar, seesaw

72
Q

molecular geometry of AX5

A

trigonal bipyramidal, square pyramidal

73
Q

molecular geometry of AX6

A

octahedral

74
Q

cis- vs trans-

A

cis- is on the same side of double bond

trans- opposite side of double bond

75
Q

valence bond theory

A

an approximate theory put forth to explain the electron pair or covalent bond by quantum mechanics

76
Q

_ hybrid orbital is required for each bond and for each lone pair

A

1

77
Q

hybrid orbitals

A

orbitals used to describe the bonding obtained by taking combinations of the atomic orbitals of the isolated atoms
- number of hybrid orbitals formed always equals the number of atomic orbitals used

78
Q

kinds of hybrid orbitals

A

of orbitals: hybrid orbitals: geometric arrangement:
2 sp linear
3 sp2 trigonal planar
4 sp3 tetrahedral
5 sp3d trigonal bipyramid
6 sp3d2 octahedral

79
Q

a multiple bond can form by the overlapping of more than _ orbital from each bonding atom

A

1

80
Q

of hybrid orbitals =

A

of atomic orbitals

81
Q

what is the hybridization of H2O

A

sp3

- sigma bond

82
Q

is C2H4 a pi bond or sigma bond?

A

pi bond

83
Q

sigma bond

A

has a cylindrical shape about the bond axis
- formed either when two s orbitals overlap or with directional orbitals (p or hybrid) when they overlap along their axis

84
Q

pi bond

A

has an electron distribution above and below the bond axis

  • formed by the sideways overlap of 2 parallel p orbitals
  • this overlap occurs when 2 parallel half-filled p orbitals are available after sigma bonds have formed
85
Q

formal charge

A

VE - LE - BE/2
OR
VE- LE - bonds

86
Q

draw the best lewis structure for SO2. show electron counts and formal charge on each atom and complete the following:

  • number of valence e-
  • formal charge of S
  • formal charge of O
  • hybridization of S
  • is the molecule polar?
  • is the dipole moment zero?
A
  • 18 e-
  • formal charge of S: 0
  • formal charge of O: 0
  • hybridization: sp2
  • the molecule is polar
  • the dipole moment is zero
87
Q

which element goes in the middle for lewis structures?

A

the least electronegative one

88
Q

molecular orbital theory

A
  • current best theory
  • theory of electronic structure of molecules in terms of molecular orbitals, which may spread over several atoms or the entire molecule
    • sigma σ
    • pi π
  • as atoms approach one another, their atomic orbitals overlap and form molecular orbitals
  • can describe delocalized bonding in terms of a single e- configuration
89
Q

sigma bonding orbital

A

1s + 1s –> attraction

  • most bonding is between atoms
  • high e- density
90
Q

sigma anti-bonding orbital

A

1s - 1s -> repulsion

  • not between atoms
  • low e- density
91
Q

bond order formula

A

B.O.: 1/2 (nb- na)

nb: e- bonding orbital
na: e- anti bonding orbital

92
Q

what is the molecular orbital of H

A

.

93
Q

bond order of H2

A

1

94
Q

bond order of He2

A

0

95
Q

bond order of Li

A

1

96
Q

strength of bond is determined by

A

1) energy difference between interacting orbitals
2) magnitude of overlap
- energies of the 2 orbitals must be approximately equal and the overlap must be large

97
Q

2 diff ways in which 2p orbitals interact

A

1) one set of 2p orbitals can overlap along their axes to give one bonding and one anti bonding orbital *σ orbitals
2) other 2 sets of 2p orbitals then overlap sideways to give 2 bonding and 2 anti bonding π orbitals

98
Q

bond order of NO

A

2.5

99
Q

bond order of NO+

A

3

100
Q

bond order of O2 +

A

2.5

101
Q

bond order of O2

A

2

102
Q

bond order of O2-

A

1.5

103
Q

which one is longer, O2 + or O2

A

O2

104
Q

which one is longer, O2 or O2 -

A

O2 -

105
Q

the lower the bond order, the __ the bond is for the same 2 atoms

A

longer

106
Q

is oxygen diamagnetic or paramagnetic?

A

paramagnetic

- has 2 unpaired e-

107
Q

C2H2
H - C ≡ C - H
- determine hybridization
- determine sigma vs pi bond

A

1,2 H 1s, C sp -> σ bond
3 C sp, C sp -> σ bond
4 C 2p, C 2p -> π bond
5 C 2p, C 2p -> π bond

108
Q

arrangement of e- pairs

A 
linear
trigonal planar
tetrahedral
trigonal bipyramidal
octahedral
109
Q

arrangement of e- pairs and shape of a molecule with 2 total e- pairs (2 bonding e- pairs, and 0 lone e- pairs)

A

arrangement: linear
shape: linear

110
Q

arrangement of e- pairs and shape of a molecule with 3 total e- pairs (3 bonding e- pairs and 0 lone e- pairs)

A

arrangement: trigonal planar
shape: trigonal planar

111
Q

arrangement of e- pairs and shape of a molecule with 3 total e- pairs (2 bonding e- pairs and 1 lone e- pair)

A

arrangement: trigonal planar
shape: bent

112
Q

arrangement of e- pairs and shape of a molecule with 4 total e- pairs (4 bonding e- pairs and 0 lone e- pairs)

A

arrangement: tetrahedral
shape: tetrahedral

113
Q

arrangement of e- pairs and shape of a molecule with 4 total e- pairs (3 bonding e- pairs and 1 lone e- pair)

A

arrangement: tetrahedral
shape: trigonal pyramidal

114
Q

arrangement of e- pairs and shape of a molecule with 4 total e- pairs ( 2 bonding e- pairs and 2 lone e- pairs)

A

arrangement: tetrahedral
shape: bent

115
Q

arrangement of e- pairs and shape of a molecule with 5 total e- pairs (5 bonding e- pairs and 0 lone e- pairs)

A

arrangement: trigonal bipyramidal
shape: trigonal bipyramidal

116
Q

arrangement of e- pairs and shape of a molecule with 5 total e- pairs (4 bonding e- pairs and 1 lone e- pair)

A

arrangement: trigonal bipyramidal
shape: see saw

117
Q

arrangement of e- pairs and shape of a molecule with 5 total e- pairs (3 bonding e- pairs and 2 lone e- pairs)

A

arrangement: trigonal bipyramidal
shape: T-shaped

118
Q

arrangement of e- pairs and shape of a molecule with 5 total e- pairs (2 bonding e- pairs and 3 lone e- pairs)

A

arrangement: trigonal bipyramidal
shape: linear

119
Q

arrangement of e- pairs and shape of a molecule with 6 total e- pairs (6 bonding e- pairs and 0 lone e- pairs)

A

arrangement: octahedral
shape: octahedral

120
Q

arrangement of e- pairs and shape of a molecule with 6 total e- pairs (5 bonding e- pairs and 1 lone e- pair)

A

arrangement: octahedral
shape: square pyramidal

121
Q

arrangement of e- pairs and shape of a molecule with 6 total e- pairs (4 bonding e- pairs and 2 lone e- pairs)

A

arrangement: octahedral
shape: square planar

122
Q

de Broglie Rxn

A 
λ = h / mv
λ = wavelength (m)
h = planck's constant (J x s)
v = velocity (m/s)
123
Q

commonly used prefixes in metric system

A

prefix symbol meaning power of 10
giga G 10^9
mega M 1,000,000 10^6
kilo k 1000 10^3
deci d 0.1 10^-1
centi c 0.01 10^-2
milli m 0.001 10^-3
micro μ 0.000001 10^-6
nano n 0.000000001 10^-9
pico p 10^-12

124
Q

rules for sig figs

A

1) all nonzero integers ALWAYS count for significance ex: 3456 has 4 sig figs
2) zeros (3 classes of zeros)
a) leading zeros:NEVER count as sig figs
ex: 0.048 has 2 sig figs
b) captive zeros: ALWAYS count as sig figs ex: 16.07 has 4 sig figs
c) trailing zeros: only significant when # HAS A DECIMAL POINT
ex: 9.300 has 4 sig figs; 0.004020 has 4 sig figs; 150 has 2 sig figs

125
Q

how to find ∆H

A

of bonds broken - # of bonds formed

126
Q

Explain the impact on bond order when an electron is removed (a) and added (b).

A

For N2,
When an electron is removed, it is removed from a bonding orbital, giving a lower bond order, making the bond weaker and longer.
When an electron is added it goes into an antibonding orbital, also giving a lower bond order. making the bond weaker and longer.

127
Q

which has a higher boiling point, polar or non-polar molecules?

A

polar

128
Q

a molecule is considered to be polar when the electronegativity difference is at least __

A

0.5

129
Q

magnetic properties

A
  • paramagnetic substance: weakly attracted; unpaired e-

- diamagnetic substance: only paired e-

130
Q

bonding

A

forms a bond, there is a signification e- density between 2 nuclei ( σ)

131
Q

anti-bonding

A

there is no e- density between 2 nuclei ( σ*)

132
Q

exceptions for less than octet

A

Be, B, Al

133
Q

exceptions for expanded octet

A

S, P, Si, and Cl

CHM 1220 (2 decks)

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