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Chemistry > Chapter 8 Review > Flashcards

Chapter 8 Review Flashcards

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1
Q

Bonds tend to form to give . . . electron configurations

A

more stable

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2
Q

Bond form to give more stable electron configurations by . . .

A

losing, sharing, and gaining electrons

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3
Q

The three types of bonds are . . .

A

Ionic bonds, Covalent bonds, and Metallic bonds

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4
Q

Ionic bonds have a . . . of electrons

A

complete transfer

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5
Q

Because ionic bonds have a complete transfer of electrons, the ions in that bond have . . .

A

opposite charges

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6
Q

The electrons in covalent bonds are ______

A

shared

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7
Q

Metallic bonding results in . . .

A

delocalized valence electrons which are
electrostatically attracted to fixed metal nuclei.

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8
Q

Ionic bonding has . . .

A

electrostatic attractions (typically between a metal and a nonmetal)

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9
Q

Covalent bonding has . . .

A

Shared electron pairs (typically between two nonmetals)

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10
Q

Metallic bonding can be referred to as a . . .

A

“sea of electrons”

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11
Q

The electrons involved in chemical bonding are called . . .

A

valence electrons

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12
Q

An element’s Lewis symbol consists of . . .

A

the element’s chemical symbol and a dot for each valence electron

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13
Q

Most ions have a . . . electron configuration

A

noble gas

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14
Q

A noble gas configuration is . . .

A

ns^2 np^6

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15
Q

Noble gases have a very ______ electron configuration

A

stable

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16
Q

The octet rule says that . . .

A

Atoms tend to lose, gain or share electrons until they are surrounded by 8 valence electrons (full s and p subshells in an atom)

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17
Q

Ions that DO NOT have noble gas configurations are . . .

A

H, He, and most transition metals

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18
Q

Because H, He, and most transition metals do not have noble gas configurations, they don’t . . .

A

follow the octet rule

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19
Q

Ionic bonding results from the electron transfer between . . .

A

positive cations and negative anions

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20
Q

Low ionization energy (metals) =

A

cations

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21
Q

High electron affinity (nonmetals)=

A

anions

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22
Q

Some characteristics of Ionic compounds include:

A
  1. Hight melting points
  2. High heats of fusion and vaporization
  3. Electrical insulators when solid
  4. Electrical conductors when molten or
    dissolved in water
  5. Hard and Brittle
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23
Q

The formation of ionic compounds is
very . . .

A

exothermic

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24
Q

Ionic compounds are . . .

A

very stable

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25
Q

The pattern that cations and anions organize themselves in is called a . . .

A

lattice

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26
Q

A crystal lattice is . . .

A

an arrangement of ions of opposite charge
surrounding one another in three dimensions

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27
Q

The strong attraction of the cations to anions in a lattice can be measured as . . .

A

lattice energy

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28
Q

Lattice energy is . . .

A

the energy (kJ/mol) needed to completely separate 1 mole of a solid ionic compound into its cations and anions

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29
Q

What would an equation for lattice energy of cation X and anion Y look like?

A

XY(s) –> X(+)(g) + Y(-)(g)

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30
Q

An equation to find lattice energy is . . .

A

Eel = (kQ1Q2)/d

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31
Q

Lattice energy, crystal stability, and ionic bond strength increase as . . .

A

Ionic charges (Q1 and Q2) increase or atomic radii (d) decrease

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32
Q

When it comes to lattice energy, between ionic charge and atomic radii, which of those two factors has a greater effect on lattice energy?

A

Ionic charge

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33
Q

What physical properties does the lattice energy affect?

A
  1. Melting Point
  2. Boiling Point
  3. heats of fusion (ΔHfus) and vaporization (ΔHvap)
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34
Q

Covalent bonding generally occurs between

A

nonmetals

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35
Q

Covalent bonds share electrons to try to get a . . . configuration

A

Noble Gas

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36
Q

Covalent bonds can be represented with . . .

A

Lewis Symbols

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37
Q

Covalent bonds form by . . .

A

sharing one or more pairs of electrons

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38
Q

Some characteristics of Covalent molecules are . . .

A
  1. Low melting points and boiling points
  2. Low heats of fusion and vaporization
  3. Poor conductors of heat and electricity
  4. More likely to be flammable
  5. Soft, brittle solids
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39
Q

When a molecular substance melts or boils, the covalent bonds . . .

A

do not break

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40
Q

when a molecular substance melts or boils, what happens is that . . .

A

intermolecular interactions are broken

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41
Q

In Lewis structures, shared electrons are drawn as . . .

A

bonds

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42
Q

In Lewis structures, nonbonding electrons are drawn as . . .

A

dots

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43
Q

In Lewis structures, the electrons that are able to be shared are . . .

A

the dots

44
Q

What happens when atoms form bonds but there’s a “scarcity” of valence electrons?

A

they form double or triple bonds

45
Q

To achieve an octet with the available valence electrons, atoms . . .

A

can share more than one pair of electrons.

46
Q

A single bond is when

A

two atoms share one electron pair

47
Q

A double bond is when

A

two atoms share two electron pairs

48
Q

A triple bond is when

A

two atoms share three electron pairs

49
Q

A single bond has a bond order of

A

1

50
Q

A double bond has a bond order of

A

2

51
Q

A triple bond has a bond order of

A

3

52
Q

When two atoms collide, but do not bond, the closest distance between the two nuclei is called . . .

A

the apparent radii

53
Q

The apparent radii are . . .

A

the nonbonding atomic radii

54
Q

When atoms are in a chemical bond, the nuclei are closer together, this radius is referred to as . . .

A

the bonding atomic radii

55
Q

When talking about molecular radii, we use . . .

A

bonding atomic radii

56
Q

Provided we know the bonding atomic radii of two elements, we can calculate . . . between those two atoms within a molecule.

A

the bond length

57
Q

Bond strengths and bond lengths contribute to . . .

A

reactivity and thermodynamics

58
Q

Bond Enthalpy is also symbolized by . . .

A

D

59
Q

Bond Enthalpy is . . .

A

the enthalpy change (ΔH) for the breaking of a particular bond in one mole of a gaseous substance

60
Q

Since breaking bonds REQUIRES energy, bond enthalpies are always . . .

A

positive qualities

61
Q

The greater the bond enthalpy, . . .

A

the stronger the bond

62
Q

The stronger the bond, . . .

A

the greater the bond enthalpy

63
Q

Most reactions proceed with bond breakage and formation are . . .

A

simultaneous

64
Q

Bond polarity is . . .

A

a measure of how equally, or unequally, the electrons in a covalent bond are shared

65
Q

Bond polarities can be . . .

A

nonpolar covalent, polar covalent, or ionic

66
Q

What leads to an unequal sharing of electrons between two atoms?

A

Differences in electronegativity between the two atoms

67
Q

In a compound, the atom that pulls the electrons to itself the most is . . .

A

the most electronegative atom

68
Q

asymmetric charge distribution results in . . .

A

polar bond

69
Q

When two atoms share electrons unequally, a . . . results

A

bond dipole

70
Q

A dipole moment is measured in . . .

A

Debyes

71
Q

1 Debyes is equal to . . .

A

3.34 x 10^-34 C*m

72
Q

To compare and determine bond polarity, . . .

A

you can use the difference in electronegativity values (ΔEN)

73
Q

When the difference in electronegativity values is smaller than 0.5, the bond is . . .

A

usually nonpolar covalent

74
Q

When the difference in electronegativity values is between o.5 and 1.6, the bond is . . .

A

usually polar covalent

75
Q

When the difference in electronegativity values is between 1.6 and 2.0, the bond is . . .

A

polar covalent if the two atoms are nonmetals and ionic if one of the two atoms is a metal

76
Q

When the difference in electronegativity values is greater than 2, the bond is . . .

A

usually ionic

77
Q

The greater the difference in electronegativity, the larger . . .

A

the dipole moment

78
Q

The larger the dipole moment, the
more . . .

A

polar is the bond

79
Q

The first step in drawing a Lewis structure

A

count the number of valence electrons

80
Q

When counting the number of elections and accounting for a cation, . . .

A

subtract one electron from the total for each positive charge

81
Q

When counting the number of electrons and accounting for an anion, . . .

A

add one electron from the total for each negative charge

82
Q

The second step in drawing a Lewis structure

A

Look at the chemical formula and decide which atom is the CENTRAL atom

83
Q

The central atom is usually . . .

A

written first and is the least electronegative element

84
Q

Chemical formulas are often written in the order . . .

A

the atoms are connected

85
Q

The third step in drawing a Lewis structure

A

draw a molecular “skeleton” connecting all outer atoms to the central atom with single lines

86
Q

The fourth step in drawing a Lewis structure

A

complete the octets for the all of the outer atoms using lone pairs

87
Q

Because hydrogen can only make one bond, hydrogen will only have . . .

A

2 electrons

88
Q

The fifth step in drawing a Lewis structure

A

place any excess electrons (as lone pairs) on the central atom

89
Q

A central atom can have more than eight electrons if it is . . .

A

in Row 3 of the Periodic Table or below

90
Q

If there are not enough electrons to give the central atom an octet, then . . .

A

shift lone pair electrons from outer atoms to form multiple bonds and satisfy the octet rule

91
Q

The most dominant Lewis structure has . . .

A

an overall formal charge equal to 0 and when the most electronegative atom has the negative charge

92
Q

Formal charge is equal to . . .

A

Number of valence electrons - lines - dots

93
Q

When multiple correct Lewis structures can be drawn, . . .

A

the structures are called resonance structures

94
Q

The different resonance forms represent . . .

A

delocalized bonding

95
Q

Resonance indicates . . .

A

increased stability in the structure

96
Q

The first exception to the octet rule is . . .

A

Ions or molecules with an odd number of electrons

97
Q

The second exception to the octet rule is . . .

A

Ions or molecules with less than an octet

98
Q

The third exception to the octet rule is . . .

A

Ions or molecules with more than eight valence electrons (an expanded octet)

99
Q

If there is an odd number of valence electrons, one atom, usually the central atom will contain . . .

A

7 instead of 8 electrons

100
Q

The 4 atoms that can have less than 8 electrons are . . .

A

B, Be, H, and Al

101
Q

B needs _ electrons

A

6

102
Q

Be needs _ electrons

A

4

103
Q

H needs _ electrons

A

2

104
Q

Al needs _ electrons

A

6

105
Q

Atoms that can have more than an octet are . . .

A

Period 3 or below

106
Q

When atoms have more than 8 electrons, they are called . . .

A

hypervalent

107
Q

Hypervalent atoms are usually surrounded by . . .

A

small, highly electronegative atoms

Chemistry (17 decks)

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