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Chem 1115 > Unit 3 > Flashcards

Unit 3 Flashcards

1
Q

Triple bond

A

A covalent bond involving three electron pairs.

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2
Q

Single bond

A

A covalent bond involving one electron pair.

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3
Q

Resonance structure

A

Individual Lewis structures in cases where two or more Lewis structures are equally good descriptions of a single molecule. The resonance structures are averaged.

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4
Q

Polar molecule

A

A molecule that possesses a nonzero dipole moment.

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5
Q

Polar covalent bond

A

A covalent bond in which the electrons are not shared equally.

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6
Q

Octet rule

A

A rule stating that bonded atoms tend to possess or share a total of 8 valence electrons.

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7
Q

Nonpolar covalent bond

A

A covalent bond in which the electrons are shared equally.

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8
Q

Metallic bond

A

Bonding, usually in solid metals, in which the bonding electrons are relatively free to move throughout the 3D structure.

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9
Q

Lewis symbol

A

(electron dot symbol)

The chemical symbol for an element with a dot for each electron valence electron.

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10
Q

Lattice energy

A

The energy required to separate completely the ions in an ionic solid.

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11
Q

Ionic bond

A

A bond between oppositely charged ions. The ions are formed from atoms by transfer of one or more electrons.

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12
Q

Formal charge

A

The number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the Lewis structure.

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13
Q

Electronegativity

A

A measure of the ability of an atom that is bonded to another atom to attract electrons to itself.

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14
Q

Double bond

A

A covalent bond involving two electron pairs.

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15
Q

Dipole moment

A

A measure of the separation & magnitude of the positive & negative charges in polar molecules.

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16
Q

Dipole

A

A molecule with one end having a partial negative charge & the other end having a partial positive charge.

A polar molecule.

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17
Q

Covalent bond

A

A bond formed between two or more atoms by a sharing of electrons.

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18
Q

Chemical bond

A

A strong attractive force that exists between atoms in a molecule.

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19
Q

Born-Haber cycle

A

A thermodynamic cycle based on Hess’ Law that relates the lattice energy of ionic substance to its enthalpy of formation & to other measurable quantities.

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20
Q

Bond polarity

A

A measure of the degree to which the electrons are shared unequally between two atoms in a chemical bond.

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21
Q

Bond enthalpy

A

The enthalpy change, [delta] H, required to break a particular bond when the substance is in the gas phase.

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22
Q

*There are 3 exceptions to the octet rule*

A ___ atom is surrounded by enough ___ electronegative atoms that it has more than an octet of electrons around it.

A

A large atom is surrounded by enough small electronegative atoms that it has more than an octet of electrons around it.

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23
Q

*There are 3 exceptions to the octet rule*

It is not possible to complete an octet without forcing ___.

A

It is not possible to complete an octet without forcing an unfavorable distribution of electrons.

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24
Q

*There are 3 exceptions to the octet rule*

A molecule has a(n) ___ number of electrons.

A

A molecule has an odd number of electrons.

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25
Q

The ___ the electronegativity difference between elements, the ___ polar the bond.

A

The greater the electronegativity difference between elements, the more polar the bond.

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26
Q

Electronegativity generally ___ from left to right across periods and ___ going down a group.

A

Electronegativity generally increases from left to right across periods and decreases going down a group.

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27
Q

Deca-

A

10

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28
Q

Nona-

A

Nine

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29
Q

Octa-

A

Eight

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30
Q

Hepta-

A

Seven

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31
Q

Hexa-

A

Six

32
Q

Penta-

A

Five

33
Q

Tetra-

A

Four

34
Q

Tri-

A

Three

35
Q

Di-

A

Two

36
Q

Mono-

A

One

37
Q

For naming binary molecular compounds:

If both elements are in the same group, the ___ one is written first.

A

If both elements are in the same group, the lower one is written first.

38
Q

For naming binary molecular compounds:

The ___ element is given an -ide suffix.

A

The second element is given an -ide suffix.

39
Q

For naming binary molecular compounds:

The element farthest ___ on the periodic table is usually written ___.

A

The element farthest left on the periodic table is usually written first.

40
Q

Acids whose anions end in -ate or -ite are named by changing -ate to ___ and -ite to ___. Any prefixes are retained.

A

Acids whose anions end in -ate or -ite are named by changing -ate to -ic and -ite to -ous. Any prefixes are retained.

41
Q

Acids containing anions whose names end in -ide are named by changing -ide to ___ and adding what prefix?

A

Acids containing anions whose names end in -ide are named by changing -ide to -ic and adding the prefix hydro-.

42
Q
A

trigonal planar

43
Q
A

Trigonal bipyramidal

44
Q
A

Linear

45
Q
A

Tetrahedral

46
Q
A

Octahedral

47
Q
A

Bent

48
Q
A

T-shaped

49
Q
A

Seesaw

50
Q
A

Pyramidal

51
Q
A

Square planar

52
Q
A

Square pyramidal

53
Q

If the acid does not contain O and is a gas (g):

Name the acid as if it was an ______.

A

Name the acid as if it was an ionic bond; start with “hydrogen” and add the anion

H2S (g) hydrogen sulfide

HBr (g) hydrogen bromide

54
Q

if the acid does not contain O and is dissolved in water (aq):

Start with ___, add the ___, change -ide to ___.

A

Start with “hydro,” add the anion, change -ide to -ic.

HBr (aq) hydrobromic acid

HI (aq) hydroiodic acid

55
Q

HF (aq)

A

hydrofluoric acid

56
Q

HCl (aq)

A

hydrochloric acid

57
Q

HBr (aq)

A

hydrobromic acid

58
Q

HI (aq)

A

hydroiodic acid

59
Q

HClO4

A

perchloric acid

60
Q

HClO3

A

chloric acid

61
Q

H2SO4

A

sulfuric acid

62
Q

HNO3

A

nitric acid

63
Q

H3PO4

A

phosphoric acid

64
Q

HC2H3O2

A

acetic acid

65
Q

H2CO3

A

carbonic acid

66
Q

H2S (g)

A

hydrogen sulfide

67
Q

HCN (g)

A

hydrogen cyanide

68
Q

HF (g)

A

hydrogen fluoride

69
Q

HCl (g)

A

hydrogen chloride

70
Q

HBr (g)

A

hydrogen bromide

71
Q

HI (g)

A

hydrogen iodide

72
Q

Ammonia

A

NH3

73
Q

Hydrogen peroxide

A

H2O2

74
Q

Vinegar

A

acetic acid

HC2H3O2

75
Q

Drinking alcohol

A

ethanol

C2H5OH

76
Q

Rubbing alcohol

A

isopropyl alcohol

C3H7OH

77
Q

Nail polish remover

A

acetone

C3H6O

Chem 1115 (6 decks)

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