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AP Chemistry > Chapter 8 > Flashcards

Chapter 8 Flashcards

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1
Q

What is Ionic Bonding?

A

Type of bonding where electrons are transferred from a metal ion to a non metal ion

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2
Q

Ionic bonding is based on?

A

differences in electronegativity and
ionization energy

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3
Q

What is Coulomb’s Law used for?

A

to calculate the amount of energy that is involved in the interaction between a pair of ions

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4
Q

In coulomb’s law, a negative sign indicates?

A

an attractive force between the ions

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5
Q

Columb’s law tells us that?

A

the ion pair has lower energy when bonded than individual ions.

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6
Q

the closer the pair is when bonded, the more _____ the process is.

A

exothermic

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7
Q

Columb’s law can also be used to calculate?

A

the repulsive forces between like charged atoms

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8
Q

In case of diatomic molecules, we can use Columb’s law to?

A

find the exact spot where bond energy favors formation of a chemical bond

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9
Q

What is Bond length?

A

the distance at which energy in the system is at a minimum

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10
Q

All systems will bond in a way that?

A

maximizes the attractive forces and minimizes the repulsive forces between atoms/ions

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11
Q

At short distances the repulsive forces _____? Why?

A

increase because of the closeness of the particles

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12
Q

At large distances the repulsive forces _____? Why?

A

decrease because atoms are unable to bond

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13
Q

What are Covalent Bonds?

A

bonds formed when non-metals share electrons

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14
Q

In a covalent bond, electrons are?

A

shared equally or unequally

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15
Q

if electrons are shared equally the bond is?

A

non-polar

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16
Q

If electrons are shared unequally the bond is?

A

polar

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17
Q

all polar covalent molecules will have?

A

partial charges

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18
Q

Partial charges means?

A

there is a positive and negative pole

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19
Q

What is electronegativity?

A

the ability of an atom to attract electrons to itself.

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20
Q

The ability of an atom to attract electrons to itself, is based on?

A

nuclear strength

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21
Q

Metals electronegativity values are _____.

A

low

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22
Q

Non-metals electronegativity values are ________.

A

high

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23
Q

Greater electronegativity difference between bonding elements leads to?

A

a less covalent bond, and more ionic bond

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24
Q

Instead of the regents electronegativity values we use?

A

% ionic character

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25
Q

If a compound is able to
conduct an electric current when melted, its?

A

ionic

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26
Q

generally the % ionic character is?

A

greater than 50%

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27
Q

what are Dipolar molecules?

A

Molecules with a slight negative end,
and a slight positive end

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28
Q

why do Dipolar molecules have a slight negative end and a slight positive end?

A

a difference in electronegativity values between atoms

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29
Q

In an electric field, dipolar molecules will do what?

A

orient themselves

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30
Q

How are molecules with polar bonds but no dipole oriented?

A

oriented so charge differences are equally distributed over the entire molecule

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31
Q

In a molecule with polar bonds but no dipole, what happens to the charges?

A

the charge differences are cancelled out

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32
Q

In a molecule with polar bonds but no dipole, no one end of the molecule is?

A

greater in charge than the other

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33
Q

What types of molecules follow the rule associated with molecules with polar bonds but no dipole?

A

Linear, tetrahedral, and planar molecules

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34
Q

What is the rule associated with molecules with polar bonds but no dipole?

A

charge differences are equally distributed over the whole molecule

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35
Q

Group 1 always ______.

A

loses one electron

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36
Q

Group 2 always ______.

A

loses two electrons

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37
Q

Group 16 mostly _____.

A

gains 2 electrons

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38
Q

Group 17 mostly ______.

A

gains 1 electron.

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39
Q

Anions gain what?

A

electrons

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40
Q

What charge do anions have?

A

negative

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41
Q

How does an anions radius change?

A

It is larger than the atom before it

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42
Q

Cations lose what?

A

electrons

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43
Q

What charge does a cation have?

A

positive

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44
Q

How does a cations radius change?

A

It is smaller than the atom before it.

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45
Q

Why are cations significantly smaller?

A

they lose an entire energy level when bonding

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46
Q

What does the Isoelectronic Series involve?

A

Ions that have the same number of electrons when done with a reaction

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47
Q

All ions in the Isoelectronic series have?

A

the same noble gas configuration when bonded to another atom

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48
Q

What happens to the size across a isoelectronic series?

A

decreases

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49
Q

What happens to the nuclear charge across a isoelectronic series?

A

increases

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50
Q

As you go up the periodic table, electronegativity _______

A

increases

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51
Q

As you go across the periodic table, electronegativity______

A

increases

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52
Q

What is polarity?

A

An entity containing two distinct and opposite poles that can either attract or repel each other

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53
Q

As attractive forces in the system are maximized, what happens to the PE?

A

it decreases

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54
Q

when bonds are broken, the energy change is?

A

positive

55
Q

when bonds are formed, the energy change is?

A

negative

56
Q

breaking of bonds is _______.

A

endothermic

57
Q

formation of bonds is __________.

A

exothermic

58
Q

Strengths of the bond model (3)

A
  1. Associates energy with the formation of bonds between elements
  2. Shows relationships between atoms in a molecule
  3. Visual tool to understanding chemical structure
59
Q

Weaknesses of the bond model (2)

A
  1. bonds are not physical structures
  2. Can not explain some of the behavior we observe in molecules
60
Q

Single bonds are the ______ bond

A

weakest

61
Q

Double and triple bonds are the _______ bonds

A

strongest

62
Q

Why are double and triple bonds so strong?

A

The bond lengths are shorter

63
Q

3 assumptions of lone electron pairs

A
  1. can be accurately drawn with Lewis dot diagram
  2. structure we draw is accurate of the geometry of the model
  3. We can illustrate the shape/ bending of a molecule
64
Q

number of electron pairs around a Linear atom?

A

B:2 L:0

65
Q

What are the 2 names of the electrons around a central atom?

A

Bonding and Lone

66
Q

number of electron pairs around a Trigonal Planar atom?

A

B:3 L:0

67
Q

number of electron pairs around a Trigonal Planar Bent or V shape atom?

A

B:2 L:1

68
Q

number of electron pairs around a Tetrahedral atom?

A

B:4 L:0

69
Q

number of electron pairs around a Trigonal Pyramidal atom?

A

B:3 L:1

70
Q

number of electron pairs around a Bent or V shaped Tetrahedral atom?

A

B:2 L:2

71
Q

number of electron pairs around a Trigonal Bipyramidal atom?

A

B:5 L:0

72
Q

number of electron pairs around a Seesaw atom?

A

B:4 L:1

73
Q

number of electron pairs around a T-shaped atom?

A

B:3 L:2

74
Q

number of electron pairs around a Linear Trigonal bipyramid atom?

A

B:2 L:3

75
Q

number of electron pairs around a Octahedral atom?

A

B:6 L:0

76
Q

number of electron pairs around a square pyramidal atom?

A

B:5 L:1

77
Q

number of electron pairs around a Square Planar atom?

A

B:4 L:2

78
Q

Linear geometry has how many electrons

A

2

79
Q

Trigonal planar has how many electrons

A

3

80
Q

Tetrahedral has how many electrons

A

4

81
Q

Trigonal bipyramidal has how many electrons

A

5

82
Q

Octahedral has how many electrons

A

6

83
Q

Bond angle of linear

A

180

84
Q

Bond angle of Bent or V shaped Trigonal planar

A

slightly less than 120

85
Q

Bond angle of Trigonal planar

A

120

86
Q

Bond angle of tetrahedral

A

109.5

87
Q

Bond angle of Trigonal pyramidal

A

107.5

88
Q

Bond angle of Bent or V shaped tetrahedral

A

104.5

89
Q

Bond angle of Trigonal Bipyramidal

A

120 in plane, 90 perpendicular to plane

90
Q

Bond angle of Seesaw

A

Complex

91
Q

Bond angle of T shaped

A

Approx. 90

92
Q

Bond angle of Linear Trigonal bipyramid

A

180

93
Q

Bond angle of Octahedral

A

90

94
Q

Bond angle of Square Pyramidal

A

Approx. 90

95
Q

Bond angle of Square Planar

A

90

96
Q

Atoms that are linear

A

linear, Trigonal bipyramid

97
Q

Atoms that are Trigonal planar

A

Bent or V-shaped, Trigonal Planar

98
Q

Atoms that are tetrahedral

A

tetrahedral, trigonal pyramidal, Bent or V-shaped

99
Q

Atoms that are Trigonal bipyramidal

A

Trigonal bipyramidal, Seesaw, T-shaped, Linear

100
Q

Atoms that are Octahedral

A

Octahedral, Square Pyramidal, square planar

101
Q

What are the diatomic molecules?

A

Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, and Bromide

102
Q

duet rule

A

hydrogen, helium, lithium, beryllium, and boron form stable molecules when they share 2 electrons

103
Q

Octet Rule

A

elements carbon and beyond form stable molecules when they are surrounded by 8 electrons

104
Q

Exceptions to the octet rule

A

Boron Triflouride and Sulfur Hexafluoride

105
Q

molecules with dipolar moment are ______

A

polar

106
Q

molecules without a dipole moment are _______

A

nonpolar

107
Q

Resonance

A

More than 1 valid structure exists for a molecule

108
Q

Where is resonance usually found?

A

polyatomic ions

109
Q

a bond will form if the energy in a system can?

A

lower its total energy

110
Q

the simultaneous attraction of each electron by the protons generates a force that?

A

balances the proton- proton and electron- electron repulsive forces at the distance corresponding to bond length.

111
Q

unequal sharing of electrons results in a ________ bond.

A

polar covalent

112
Q

dipole moments

A

when a molecule has a center of positive charge and a center of negative charge

113
Q

atoms in a stable compound have a _________ configuration.

A

noble gas

114
Q

In Isoelectronic ions, what determines the size?

A

number of protons

115
Q

For a series of isoelectronic ions, as size ____ the nuclear charge ________.

A

decreases, increases

116
Q

lattice energy

A

change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

117
Q

lattice energy is also defined as?

A

the energy released when an ionic solid forms from ions

118
Q

Ionic character ______ with EN difference

A

increases

119
Q

bonds result from when?

A

A system is seeking its lowest possible energy

120
Q

Localized Electron model

A

A molecule composed of atoms bound together by sharing electrons using atomic orbitals

121
Q

electron pairs are assumed to be localized on a particular atom or?

A

in space between 2 atoms

122
Q

Lone pairs

A

pair of electrons localized on the atom

123
Q

bonding pairs

A

pair of electrons in the space between atoms

124
Q

atoms want to achieve _______ configuration

A

noble gas

125
Q

second row elements are assumed to always?

A

obey the octet rule

126
Q

second row elements never?

A

exceed the octet rule

127
Q

Which two elements often have fewer than 8 electrons around them in compounds?

A

Boron and Beryllium

128
Q

When writing the Lewis structure for a molecule you do what first?

A

satisfy the octet rule

129
Q

formal charge

A

difference in # of valence electrons and valance electrons assigned to the atom in the molecule

130
Q

atoms in molecules try to achieve formal charges close to ?

A

zero

131
Q

negative formal charges are expected to reside on?

A

the most electronegative atoms

132
Q

Sigma bonds have what bonds?

A

single double and triple

133
Q

Pi bonds have what bonds?

A

double and triple

AP Chemistry (16 decks)

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