Unit 3: Bonding Flashcards
(67 cards)
1
Q
polyatomic ions
A
ions which consist of more than one atom
2
Q
CO3 2-^
A
carbonate
3
Q
carbonate
A
CO3 2-
4
Q
bicarbonate
A
HCO3 1-
5
Q
HCO3 1-
A
bicarbonate
6
Q
phosphate
A
PO4 3-
7
Q
PO4 3-
A
phosphate
8
Q
hydroxide
A
OH 1-
9
Q
OH 1-
A
hydroxide
10
Q
peroxide
A
O2 2-
11
Q
O2 2-
A
peroxide
12
Q
cyanide
A
CN 1-
13
Q
CN 1-
A
cyanide
14
Q
sulfate
A
SO4 2-
15
Q
SO4 2-
A
sulfate
16
Q
sulfite
A
SO3 2-
17
Q
SO3 2-
A
sulfite
18
Q
nitrate
A
NO3 1-
19
Q
NO3 1-
A
nitrate
20
Q
nitrite
A
NO2 1-
21
Q
NO2 1-
A
nitrite
22
Q
ammonium
A
NH4+
23
Q
NH4+
A
ammonium
24
Q
acetate
A
CH3COO 1-
25
CH3COO 1-
acetate
26
C2H3O2 1-
acetate
27
acetate
C2H3O2 1-
28
NH3
ammonia
29
ammonia
NH3
30
effective nuclear charge
the attraction to the nucleus felt by the outermost electrons in an atom
z (atomic number) - s (# of inner shell electrons)
increases as you go right on the periodic table
31
ionization energy
the energy required to remove an electron from an atom in the gas phase; energy required to form the cation
endothermic (energy is absorbed or used)
M(g) --> M+(g) + e-
32
lattice energy
energy required to transform crystalline solid into gas phase ions
MX(s) + energy --> M+(g) + X-(g)
E is proportional to q1q2/r
33
electron affinity
energy that is gained by forming the anion
exothermic (energy is released)
X(g) + e- --> X-(g)
34
crystallization
energy that is gained by bringing the cation and anion together
M+(g) + X-(g) --> MX(s)
exothermic (energy is released)
35
M(g) --> M+(g) + e-
ionization energy
36
MX(s) + energy --> M+(g) + X-(g)
lattice energy
37
X(g) + e- --> X-(g)
electron affinity
38
M+(g) + X-(g) --> MX(s)
crystallization
39
covalent bonds
between nonmetals, high electronegativity
electrons are shared
40
ionic bonds
metal + nonmetal, cation + anion
electrons are transferred
41
which bond is longest? why?
single bond is longest as there are less shared electrons (2 e-)
42
which bond is shortest and strongest? why?
triple bond is shortest and strongest as there are more shared electrons (6 e-), relatively maximizing the attractive forces between these electrons and the nuclei
43
which bond is weakest? why?
single bond is weakest as there are less shared electrons, thus lowest amount of attractive forces between the nuclei
44
which bond is most stable? why?
triple bonds are most stable as it has the most attractive forces, thus needs the greatest amount of energy to break the bond
45
forming a bond is always an __________ process
exothermic
46
breaking a bond is always an __________ process
endothermic
47
resonance occurs...
when we can draw two or more valid Lewis structures for the same molecule; there is at least one double or triple bond
48
radicals
molecules that have an uneven number of electrons
49
Lewis Structure for NO
nitrogen has the extra electron because oxygen is more electronegative
50
electrons are _________ in Molecular Orbital theory
delocalized
51
VSEPR
model for 3-D shapes
52
Valence Bond Theory
model for bonding between atoms
53
Molecular Orbital Theory
model for bonding throughout the molecule
54
electrons are _________ in Valence Bond Theory
localized
55
atomic orbitals form __________ orbitals in Valence Bond Theory
hybridized
56
atomic orbitals form __________ orbitals in Molecular Orbital Theory
molecular
57
in VB and MO, the number of orbitals is __________
conserved
58
VB and MO both form _______ and _______ bonds
sigma, pi
59
an antibonding orbital is formed when....
the overlap of the corresponding atomic orbitals leads to destructive interference
60
bond polarity is the result of _________ electronegativities, causing electrons to not be _________________ across the bond
differing, equally distributed
61
can you have a polar molecule with nonpolar bonds? why or why not?
no, there will be no dipole moments, thus the molecule is nonpolar
62
can you have a nonpolar molecule with polar bonds?
yes, certain geometries of a molecule can "cancel out" dipole moments, especially with symmetrical molecules
63
ionic compounds ____ prefixes
do not use
64
Fe
iron
65
IV
4
66
higher the bond order = more ____________________
stable (stronger), shorter
67
VI
6
