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CH301 > Unit 3: Bonding > Flashcards

Unit 3: Bonding Flashcards

1
Q

polyatomic ions

A

ions which consist of more than one atom

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2
Q

CO3 2-^

A

carbonate

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3
Q

carbonate

A

CO3 2-

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4
Q

bicarbonate

A

HCO3 1-

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5
Q

HCO3 1-

A

bicarbonate

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6
Q

phosphate

A

PO4 3-

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7
Q

PO4 3-

A

phosphate

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8
Q

hydroxide

A

OH 1-

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9
Q

OH 1-

A

hydroxide

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10
Q

peroxide

A

O2 2-

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11
Q

O2 2-

A

peroxide

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12
Q

cyanide

A

CN 1-

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13
Q

CN 1-

A

cyanide

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14
Q

sulfate

A

SO4 2-

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15
Q

SO4 2-

A

sulfate

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16
Q

sulfite

A

SO3 2-

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17
Q

SO3 2-

A

sulfite

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18
Q

nitrate

A

NO3 1-

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19
Q

NO3 1-

A

nitrate

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20
Q

nitrite

A

NO2 1-

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21
Q

NO2 1-

A

nitrite

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22
Q

ammonium

A

NH4+

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23
Q

NH4+

A

ammonium

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24
Q

acetate

A

CH3COO 1-

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25
Q

CH3COO 1-

A

acetate

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26
Q

C2H3O2 1-

A

acetate

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27
Q

acetate

A

C2H3O2 1-

28
Q

NH3

A

ammonia

29
Q

ammonia

A

NH3

30
Q

effective nuclear charge

A

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
Q

ionization energy

A

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
Q

lattice energy

A

energy required to transform crystalline solid into gas phase ions
MX(s) + energy –> M+(g) + X-(g)
E is proportional to q1q2/r

33
Q

electron affinity

A

energy that is gained by forming the anion
exothermic (energy is released)
X(g) + e- –> X-(g)

34
Q

crystallization

A

energy that is gained by bringing the cation and anion together
M+(g) + X-(g) –> MX(s)
exothermic (energy is released)

35
Q

M(g) –> M+(g) + e-

A

ionization energy

36
Q

MX(s) + energy –> M+(g) + X-(g)

A

lattice energy

37
Q

X(g) + e- –> X-(g)

A

electron affinity

38
Q

M+(g) + X-(g) –> MX(s)

A

crystallization

39
Q

covalent bonds

A

between nonmetals, high electronegativity
electrons are shared

40
Q

ionic bonds

A

metal + nonmetal, cation + anion
electrons are transferred

41
Q

which bond is longest? why?

A

single bond is longest as there are less shared electrons (2 e-)

42
Q

which bond is shortest and strongest? why?

A

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
Q

which bond is weakest? why?

A

single bond is weakest as there are less shared electrons, thus lowest amount of attractive forces between the nuclei

44
Q

which bond is most stable? why?

A

triple bonds are most stable as it has the most attractive forces, thus needs the greatest amount of energy to break the bond

45
Q

forming a bond is always an __________ process

A

exothermic

46
Q

breaking a bond is always an __________ process

A

endothermic

47
Q

resonance occurs…

A

when we can draw two or more valid Lewis structures for the same molecule; there is at least one double or triple bond

48
Q

radicals

A

molecules that have an uneven number of electrons

49
Q

Lewis Structure for NO

A

nitrogen has the extra electron because oxygen is more electronegative

50
Q

electrons are _________ in Molecular Orbital theory

A

delocalized

51
Q

VSEPR

A

model for 3-D shapes

52
Q

Valence Bond Theory

A

model for bonding between atoms

53
Q

Molecular Orbital Theory

A

model for bonding throughout the molecule

54
Q

electrons are _________ in Valence Bond Theory

A

localized

55
Q

atomic orbitals form __________ orbitals in Valence Bond Theory

A

hybridized

56
Q

atomic orbitals form __________ orbitals in Molecular Orbital Theory

A

molecular

57
Q

in VB and MO, the number of orbitals is __________

A

conserved

58
Q

VB and MO both form _______ and _______ bonds

A

sigma, pi

59
Q

an antibonding orbital is formed when….

A

the overlap of the corresponding atomic orbitals leads to destructive interference

60
Q

bond polarity is the result of _________ electronegativities, causing electrons to not be _________________ across the bond

A

differing, equally distributed

61
Q

can you have a polar molecule with nonpolar bonds? why or why not?

A

no, there will be no dipole moments, thus the molecule is nonpolar

62
Q

can you have a nonpolar molecule with polar bonds?

A

yes, certain geometries of a molecule can “cancel out” dipole moments, especially with symmetrical molecules

63
Q

ionic compounds ____ prefixes

A

do not use

64
Q

Fe

A

iron

65
Q

IV

A

4

66
Q

higher the bond order = more ____________________

A

stable (stronger), shorter

67
Q

VI

A

6

CH301 (4 decks)

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