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AP Chemistry > Chapter 9: Chemical Bonds > Flashcards

Chapter 9: Chemical Bonds Flashcards

(106 cards)

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1
Q

the … electrons form bonds

A

valence

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2
Q

a lewis-dot symbol for an atom consists of the

A

symbol for the element surrounded by dots, one for each valence electron

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3
Q

electrons are usually removed from groups 1 and 2 because they have

A

low ionization energies

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4
Q

electrons are easily added to nonmetals because their

A

electron affinities are generally favorable

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5
Q

ionic bonding is the bonding that results from

A

electrostatic attraction between positively and negatively charged ions

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6
Q

when an ionic coompound forms, the number of electrons lost in forming the cations must

A

equal the number gained to form the anions

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7
Q

born-haber cycle: a process in which the formation of an ionic compond is shown as the

A

sum of five simpler reactions

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8
Q

lattice energy is the energy required to separate

A

one mole of an ionic crystalline solid into the isolated gaseous ions

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9
Q

lattice enrgy is always

A

positive

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10
Q

E=

A

kQ1Q2/ r

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11
Q

k is a

A

constant

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12
Q

Q1 and Q2 are the

A

charges on the two particles

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13
Q

r is the

A

distance of separation in the compound

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14
Q

equation for E known as

A

coulomb’s law

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15
Q

lattice energies are greatest for compounds made from

A

highly charged small ions

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16
Q

maximize …, minimize … to get the largest E

A

Q; r

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17
Q

ionic solids are stable because of

A

high lattice energies

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18
Q

ionic compounds are typically … with …

A

brittle solids; high melting points

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19
Q

covalent compounds are typically … or … at …

A

liquids; gases; room temperature

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20
Q

when covalent compounds are solids, they are

A

low melting

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21
Q

a covalent bond is a bond that results from

A

atoms sharing electrons

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22
Q

the bond length is the … between the … in a molecule

A

minimum energy distance; nuclei of two bonded atoms

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23
Q

bond length is determined by a … observed as the two atoms move ..

A

potential energy minimum; closer together

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24
Q

a covalent bond forms because two atoms sharing electrons are

A

lower in energy than the two isolated atoms

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25
bonding pairs of electrons are
shared between two atoms
26
lone, or nonbonding, pairs of electrons are entirely
on one atom and are not shared
27
lewis structures show how valence electrons are
arranged among atoms in a molecule
28
lewis structures reflect the central idea that stability of a compound relates to
noble gas electron configuration
29
lewis structures show the .. and ..., not the ...
numbers; types of bonds; geometry of the molecule
30
The octet rule states that each atom in a molecule shares electrons until it is
Surrounded by eight electrons
31
In most Lewis structures oxygen makes ... bonds and has ... lone electrons; nitrogen makes ... bonds and has ... lone pair; carbon makes ... bonds
Two; two; three; one; four
32
Single bond;
Shares one electron pair
33
Double bond:
Shares two electron pairs
34
Triple bond:
Shares three electron pairs
35
Bond order: the number of
Electron pairs that are shared between two atoms
36
Skeleton structure shows which atoms are
Bonded to each other in a molecule
37
Central atom: an atom bonded to
Two or more other atoms
38
Nonpolar
Equal sharing of electrons
39
Polar
Unequal sharing of electrons
40
The polarity of a compound can be determined by
Placing the compound in an electric field
41
If a molecule is polar it will no longer have a
Random orientation In the electric field
42
dipole moment is a measure of the
unequal sharing of electrons
43
the dipole moment of a compound can be determined by placing the compound in
an electric field
44
the unequal sharing leads to a ... bond that is indicated with the symbol ... followed by a sign to show ...
polar covalent; δ; partial charges
45
electronegativity is the measure of the ability of an atom to attract the
shared electrons in a chemical bond
46
... is the most electronegative element
fluorine
47
electronegativity order of some elements
F>O>Cl=N
48
elements with low ionization energies have ... electronegativities, and elements with high ionization eneries have ... electronegativities
low; hgh
49
the polarity of a bond is proportional to the
difference in electronegativity between two covalently bonded atoms
50
electronegativities ... across a period and .. down a row
increase; decrease
51
nonpolar electronegativity diff.
up to 0.4
52
polar electronegativity diff
0.4-1.7
53
ionic electronegativity diff
>1.7
54
but to truly identify a substance as ionic, you must assess the
electrical conductance of the molten compound
55
formal charge is a charge assigned to atoms in lewis structures by assuming the shared electrons are
divided equally between the bonded atoms
56
formal charge =
#v.e- - #lonepairelectrons - #bonds
57
lewis structures that show the .... formal chages are...
smallest; favored
58
lewis structures that have adjacent atoms with formal charges of the .... are ...
same sign; much less favorable
59
lewis structures that place negative formal charges on the ... are...
more electronegative atoms; favored
60
formal charges of opposite sign are usually on
adjacent atoms
61
resonance structures: structures that differ only in the
distribution of valence electrons
62
resonance is invoked when more than one valid Lewis structure can be
written for a particular moleucle
63
resonance bonds are ... and .... than single bonds and ... and .... than double bonds
shorter; stronger; longer; weaker
64
no resonance structure is correct by itself, the correct structure is
an average of all resonance structures
65
sometimes resonance structures are not equivalent, so ... are used to determine which structure is favored
formal charges
66
four classes of molecules do not obey the octet rule:
electron-deficient; odd-electron; expanded valence shell; oxides & oxyacids
67
central atoms from groups ... and ... do not have enough valence electrons to complete an octet and are thus ...
2; 3; electron-deficient
68
electron-deficiency is typically seen with compounds containt
Be, B, Al
69
any molecule that has an odd number of valence electrons must
violate the octet rule
70
odd-electron molecules are highly ..., and are called ...
reactive; radicals
71
in the lewis structure of a molecule that contains an odd number of electrons, one atom has only
seven valence electrons
72
expanded valence shell molecules have ... about an atom in a lewis structure
more than eight electrons
73
a large class of expanded valence shell compounds have the general formula ..., where Y= ...
YFn; P, S, Cl, As, Se, Br, Te, I, or Xe
74
when more electrons are available than are needed to satisfy the octet rule for all atoms present, place the extra electrons around the
central atom as lone pairs
75
the octet rule can be exceeded for elements in ... and ... periods, but not for elements in the
third; later; second period
76
the octet rule is based on the idea that the valence s and p subshells can hold eight electrons, but atoms in the third and later periodshave ...tat can hold ....,exceeding an octet
d subshells; additional electrons
77
oxides and oxyacids of p-block elements in periods .... typically have ...
>= three; expanded valence shells
78
oxyacids have at least one ... attached to an .... and has the general formula
hydrogen atom; oxygen atom; (HO)mXOn
79
species with strong bonds are generally
stable
80
bond dissociation energy (D) is the energy required to
break one mole of bonds in a gaseous species
81
bond energies are always ...
endothermic
82
bond energies for diatomic molecules are measured ...., other bond energies are ...
directly; averages
83
triple bonds are ... than double bonds which are ... than single bonds
stronger; stronger
84
triple and double bond lengths are ... than single bond lengths
shorter
85
ΔHreaction=
ΣDbondsbroken - ΣDbondsformed
86
breaking bonds always
requires energy
87
forming bonds always
releases energy
88
to calculate ΔHreaction, the lewis structures need to be written to determine the
types and numbers of bonds broken and formed
89
in calculating, ΔHreaction .... are used
average bond energies
90
bond order=
#bonds/how many regions of bonding
91
for compounds, formal charges must add to
0
92
for polyatomic ions, formal charges should add to the
charge of the ion
93
(electronegativity) F=
4.0
94
(electronegativity) O=
3.5
95
(electronegativity) N=
3.0
96
(electronegativity) C=
2.5
97
(electronegativity) Cl=
3.0
98
(electronegativity) H=
2.1
99
(electronegativity) Br=
2.8
100
(electronegativity) I=
2.5
101
(electronegativity) S=
2.5
102
(electronegativity) P=
2.1
103
(electronegativity) Si=
1.8
104
(electronegativity) Al=
1.5
105
ionic compounds form from
metals and nonmetals;
106
nonmetal nonmetal compounds are usually
covalent bonds

AP Chemistry (24 decks)

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