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Inorganic > 1B Chemical Bond > Flashcards

1B Chemical Bond Flashcards

1
Q

Effects of metallic bond

A

Isotropic bond/force causes equal atomic sizes causes simple packing

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2
Q

Packing form of 80% all metallic elements

A

HCP, FCC, BCC

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3
Q

HCP packing

A

ABABABABABAB…

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4
Q

FCC/CCP Packing

A

ABCABCABCABC

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5
Q

Different types of strong chemical bonds

A

Metallic, ionic, covalent

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6
Q

Weak chemical bonds

A

Hydrogen bonds, van der waals interactions (London, Debye, keesom)

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7
Q

Pure elements and alloys

A

Metals

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8
Q

Characteristics of metals

A

Few electrons in valence shell; low atomic ionization energies (<10 eV); not transparent, metal,ice shine, ductile, good conductor; wide range of melting points

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9
Q

Relationship btwn electric conductivity and temp for metals

A

Decreases as temp increases

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10
Q

Relationship btwn electric conductivity and temp for metalloids

A

Increases as temp increases

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11
Q

Metallic bonds form between … bc…

A

Similar metals because similar radii leads to simple packing patterns. And the metal character

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12
Q

Zintl phases form between

A

Metals with high ΔEN (s-p) because the bond character between metallic and ionic. Has metal kind character. Often polyatomic Anions with covalent scaffold

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13
Q

Ionic bonds form between

A

Metal nonmetal compounds with ΔEN > 1.5. Large nonmetal anion with small, metal cation allows complex packing. Salt character

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14
Q

Differences between metals: main group

A

S and P valence orbitals, fewer oxidation states

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15
Q

Differences between metals: transition metals

A

S and D valence orbitals have more oxidation states

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16
Q

Main group metal ions description

A

Noble gas config. Diamagnetic, colorless, not precious

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17
Q

Transition metal ion descriptions

A

Can possess partially filled d orbitals. Potentially colorful and paramagnetic and can be precious

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18
Q

Metallic Bond by Drude and Lorentz

A

Delocalized valence electron cloud around atomic cores

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19
Q

Metallic Bond by Drude and Lorentz characteristics

A

Isotropic bond/force causes equal atomic sizes leading to simple packing

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20
Q

Ductility of the packing from softest to hardest

A

FCC > HCP > BCC

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21
Q

Effect on hardness by the transition from heteroatoms to alloys

A

Increases hardness

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22
Q

Packing between condensed noble gases?

A

Similar to metal packing bc of isotropic London forces between equal atoms

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23
Q

What causes ductility

A

Layered structure

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24
Q

Direct packing

A

Band energies (electronics)

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25
Q

Can drude lorentz theory predict packing type

A

Nope

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26
Q

HCP

A

Hexagonal close packed

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27
Q

Common HCP elements

A

Zinc, magnesium, cadmium

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28
Q

FCC or CCP

A

Face centered aka cubic close. Think of a dice

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29
Q

Common FCC/CCP elements

A

Aluminum, copper, silver

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30
Q

BCC

A

Body centered cubic. Think of it floating in the middle of a box

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31
Q

Common BCC elements

A

Chromium, tungsten, iron

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32
Q

Mixing similar metals gives you

A

Alloys

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33
Q

Mixing very different metals gives you

A

Zintls

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34
Q

How to calculate ionic band

A

Coulomb force

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35
Q

Inionic Lattice vs metallic

A

Similar

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36
Q

What does it mean that Coulomb force is isotropic

A

Works in all directions

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37
Q

How many atoms are around?

A

Coordination number

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38
Q

Void for Cord 2

A

Linear

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39
Q

Void for cord 3

A

Triangular planar

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40
Q

Void for cord 4

A

Tetrahedral

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41
Q

Void for cord 6

A

Octahedral

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42
Q

Void for cord 8

A

Cubic

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43
Q

Void for cord 12

A

Close packing CCP and HCP. In metals

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44
Q

Lattice energy is true for

A

Isolated pairs

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45
Q

Madelung constant is lattice dependent or independent?

A

Lattice dependent

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46
Q

Lattice energy effect on dissolving

A

High lattice energy means harder to dissolve. Can heat to help

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47
Q

Higher Lattice energy effect on melting point

A

Higher melting point

48
Q

3 types of point defects

A

Vacancy, interstitial, substitution

49
Q

Needed to create defects?

A

Energy

50
Q

Vacancy by moving to interstitial site

A

Frenkel type defect

51
Q

Vacancy by moving to crystal surface

A

Schottky type defect

52
Q

Intrinsic lattice defect

A

Pure compound

53
Q

Extrinsic lattice defect

A

Additional of dopant

54
Q

What happens if you add a dopant with additional valence electrons

A

Changes the color!

55
Q

Nonpolar covalent bond ΔEN

A

ΔEN < 0.5 or 0.7

56
Q

Polar covalent ΔEN

A

0.5 or 0.7 < ΔEN < 1.5 or 1.7

57
Q

Ionic ΔEN

A

ΔEN > 1.5 or 1.7

58
Q

Equal shading of valence electrons

A

Nonpolar covalent

59
Q

Unequal sharing of valence electrons

A

Polar covalent

60
Q

Valence Bond theory based on

A

Orbital theory application of schrodingers wave equation

61
Q

Valence bond theory explains covalent bonding as

A

Overlap of atomic orbitals

62
Q

Orbitals according to VB theory

A

Still localized on atoms

63
Q

Interactions between 2 isolated H atoms with Ha e1 and Hb e2?

A

Core A + e1 and Core B + e2

64
Q

Interactions between 2 hydrogen atoms that approach each other

A

Core A + e1
Core B + e2
Core A + e2
Core B + e1
e1 + e2
Core A + Core B

65
Q

Total energy when no interaction between 2 hydrogen atoms

A

E total = EA + EB

66
Q

Total energy between 2 hydrogen atoms approaching each other

A

E total DOES NOT EQUAL Ea + Eb

67
Q

Heisenberg’s Uncertainty Principle

A

Electrons of close atoms cannot be differentiated. Electron 1 and e2 can both be assigned to either Ha or Hb

68
Q

ψ+ represents

A

Spin coupled state

69
Q

Does ψ+ obey Pauli?

A

Yeah

70
Q

ψ+ stable or unstable

A

Stable

71
Q

ψ- represents

A

State with parallel spins

72
Q

ψ- stability

A

Unstable

73
Q

Electrons in ψ+ or ψ- have more space?

A

ψ+ so they can get closer to cores

74
Q

Electrons that can get closer to cores leads to what kind of electron density

A

High

75
Q

The bond is located in the

A

Density between cores

76
Q

Constructive interference of different atomic orbitals

A

Attractive

77
Q

Destructive interference of different atomic orbitals

A

Repulsive

78
Q

Non constructive interference of different atomic orbitals

A

No interactions

79
Q

Can the original valence bond theory predict geometry

A

No it cannot

80
Q

Hybridization of atomic orbitals based on

A

Orbital theory. Application of schrodingers wave equatjon

81
Q

Hybridization of atomic orbitals is an expansion of

A

Valence bond theory

82
Q

Explain hybridization of atomic orbitals

A

Linear combo of atomic orbitals (LCAO)
Only AOs of the same atom are combined /hybridized

83
Q

x AOs in hybridization of AO theory become

A

x hybrid AOs

84
Q

percent s character in sp3

A

25%

85
Q

Percent s character in sp2

A

33%

86
Q

orbital geometry in sp

A

Linear. 180°

87
Q

Orbital geometry of sp2

A

Triangular planar 120°

88
Q

Orbital geometry of sp3

A

Tetrahedral 109.5°

89
Q

Orbital geometry of sp3d

A

Trigonal bipyramidal 90° and 120°

90
Q

Orbital geometry of sp3d2

A

Octahedral 90°

91
Q

MO theory orbitals and electrons placement

A

Orbitals/electrons spread over whole molecule! Not localized at single atoms

92
Q

Lewis form in MO

A

Not compatible

93
Q

MO theory AOs combination

A

AOs of all atoms in same molecule or ion are combined

94
Q

In MO theory, x AOs =

A

x MOs

95
Q

AOs symbolized with

A

Roman letters like s p d

96
Q

ΜOs are symbolized with

A

Greek letters like σ π δ

97
Q

Antibonding MOs marked by

A

An asterisk like σ*

98
Q

Bond order equation

A

BO = (#e in binding MO) - (#e in antibinding MO) divided all by 2

99
Q

Hybrids symmetry

A

Hybrids are asymmetric

100
Q

MO binding electrons

A

Not assigned to individual bonds between atoms

101
Q

VB theory explains covalent bonds as

A

Overlap of atomic orbitals

102
Q

VB Orbitals

A

Localized on atoms

103
Q

difference between main group and transition metals oxidation states

A

transition metals have more oxidation states

104
Q

smaller Madelung Constant (A) means

A

not good packing

105
Q

Which has a node? Spin couple or parallel spins?

A

parallel

106
Q

hybridization of linear

A

sp

107
Q

hybridization of triangular planar

A

sp2

108
Q

hybridization of tetrahedral

A

sp3

109
Q

hybridization of trigonal bipyrimidal

A

sp3d

110
Q

hybridization of octahedral

A

sp3d2

111
Q

destructive overlap can cause a

A

nodal plane

112
Q

What needs more space? single bond, double bond, or lone pair?

A

lone > double > single

113
Q

metal + metal =

A

metallic bond

114
Q

metal + nonmetal =

A

ionic bond

115
Q

nonmetal + nonmetal =

A

covalent bond

116
Q

metalloid + metal =

A

metallic bond

117
Q

metalloid + nonmetal =

A

covalent bond

Inorganic (16 decks)

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