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Chem 111 > Exam 2 (ch 4-5) > Flashcards

Exam 2 (ch 4-5) Flashcards

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1
Q

Binary Compounds (Ionic)

A

cation+anion-ide

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2
Q

Name Al2O3

A

Aluminum Oxide

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3
Q

Multivalent Cations

A

cation (charge)+anion-ide

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4
Q

Name CuO

A

Copper (II) Oxide or -ous=lower, -ic=higher

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5
Q

Oxyanions

A

Hypo-ite, -ite, -ate, Per-ate
2nd row (C, N) predict charge to O, -ate=O3
3rd row (P, S) predict to [Ar], -ate=O4

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6
Q

Molecular Compounds

A

pre(1st)+pre(2nd)-ide
Higher atomic no. goes 1st

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7
Q

Oxyacid

A

(HXO) = ate=ic, ite=ous
No O = Hydro(element)-ide

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8
Q

Acetate

A

C2H3O2 -

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9
Q

Carbonate

A

CO3 2-

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10
Q

Hydrogen carbonate/bicarbonate

A

HCO3 -

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11
Q

hydroxide

A

OH -

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12
Q

nitrite

A

NO2 -

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13
Q

nitrate

A

NO3 -

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14
Q

chromate

A

CrO4 2-

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15
Q

dichromate

A

Cr2O7 2-

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16
Q

phosphate

A

PO4 3-

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17
Q

Hydrogen phosphate

A

HPO4 2-

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18
Q

dihydrogen phosphate

A

H2PO4 -

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19
Q

Ammonium

A

NH4 +

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20
Q

Permanganate

A

MnO4 -

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21
Q

Sulfite

A

SO3 2-

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22
Q

hydrogen sulfite/bisulfite

A

HSO3 -

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23
Q

sulfate

A

SO4 2-

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24
Q

cyanide

A

CN-

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25
Q

Peroxide

A

O2 2-

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26
Q

Binary Acids

A

2 elements (H+X), Hydro+nonmetal-ic+acid

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27
Q

Lewis Structure Rules (4)

A

8 electrons per atom
lowest FC
atoms 3rd row and below may have more than 8 electrons
puts a negative charge on most electronegative atom

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28
Q

reasonance

A

more than one possible Lewis Structure

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29
Q

exceptions to octet rule

A

ions/molecules with:
- odd no. electrons
- less than octet
- expanded octet
* H = 2
* B = 6

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30
Q

Name H3PO3

A

Phosphorous acid

31
Q

Name H2CO3

A

Carbonic acid

32
Q

Chromic acid chemical formula

A

H2CrO4

33
Q

Acetic acid chemical formula

A

C2H4O2 or CH2O

34
Q

How to determine the molecular formula of a compound (acids)

A
  1. count back to the noble gas to find ionic charge
  2. butterfly with O
  3. add H to make even with O or add 2H and 1O
35
Q

2 e- areas, 0 lone pairs

A

EDG = linear
MG = linear
Angle = 180

36
Q

3 e- areas, 0 lone pairs

A

EDG= trigonal planar
MG= trigonal planar
Angle= 120

37
Q

3 e-, 1 lone pair

A

EDG= trigonal planar
MG= bent
Angle= <120

38
Q

4 e-, 0 lone pairs

A

EDG= tetrahedral
MG= tetrahedral
Angle= 109.5

39
Q

4 e-, 1 lone pair

A

EDG= tetrahedral
MG= trigonal pyramidal
Angle= <109.5

40
Q

4 e-, 2 lone pair

A

EDG= tetrahedral
MG= bent
Angle= «109.5

41
Q

5 e-, 0 lone pairs

A

EDG= trigonal bipyramidal
MG= trigonal bipyramidal
Angle= 90, 120

42
Q

5 e-, 1 lone pair

A

EDG= trigonal bipyramidal
MG= seesaw
Angle= <90, <120
*never take from axis

43
Q

5 e-, 2 lone pair

A

EDG= trigonal bipyramidal
MG= T-shape
Angle= <90

44
Q

5 e-, 3 lone pairs

A

EDG= trigonal bipyramidal
MG= linear
Angle= 180

45
Q

6 e-, 0 lone pairs

A

EDG= octahedral
MG= octahedral
Angle= 90

46
Q

6 e-, 1 lone pair

A

*take from axis
EDG= octahedral
MG= square pyramidal
Angle= <90

47
Q

6 e-, 2 lone pairs

A

*take from axis
EDG= octahedral
MG= square planar
Angle= 90

48
Q

6 e-, 3 lone pairs

A

*don’t take from axis
EDG= octahedral
MG= T-shaped
Angle= <90

49
Q

6 e-, 4 lone pairs

A

EDG= octahedral
MG= linear
Angle= 180

50
Q

How to determine polarity

A

use vectors to show electronegativity
(point towards most electronegative atom)

51
Q

nonpolar molecule

A

net dipole = 0
pulled equally in all directions = canceled

52
Q

Polar molecule

A

permanent dipole moment
unsymmetrical EDG

53
Q

VSEPR theory

A

best geometric arrangement
predicts shape and bond angles

54
Q

Valence bond theory

A

localized electron model
chemical bond = overlapped e- orbitals
hybridization

55
Q

hybridization

A

mixing of atomic orbitals
s to sp3d5 depending on no. of things going on
electrons get promoted from ground state to allow to be shared and bonded

56
Q

sigma bonds

A

head to head overlap
1 per bond
cylindrical symmetry about internuclear axis

57
Q

Pi bonds

A

side to side overlap
the rest of the bonds
e- density above/below internuclear axis

58
Q

Hypochlorite

A

ClO -

59
Q

Chlorite

A

ClO2 -

60
Q

Chlorate

A

ClO3 -

61
Q

Perchlorate

A

ClO4 -

62
Q

Difference between VSEPR and Valence bond theory

A

VBT describes chemical bonding of an atom while VSEPR describes the molecular shape based on electron clouds

63
Q

bond rotation, single bond

A

free rotation

64
Q

bond rotation, double

A

restricted

65
Q

bond rotation, same on each side

A

cis

66
Q

bond rotation, mixed

A

trans

67
Q

difference between VSEPR and VBT

A

VSEPR = shape and angles
VBT = chemical bonding

68
Q

Lewis theory prob: bond angles

A

VSEPR

69
Q

Lewis theory prob: resonance, chem bond

A

VBT, hybridization

70
Q

Lewis theory prob: magnetic behavior

A

molecular orbital theory (MO)

71
Q

diamagnetic

A

repelled, all bonded/paired e- or bond=unbond

72
Q

paramagnetic

A

unbonded e-

73
Q

bond strength

A

Hi Bond Order
shorter bonds
- Hi number of bonds
- hi difference in EN

Chem 111 (4 decks)

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