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chemistry > Unit 14-16 > Flashcards

Unit 14-16 Flashcards

1
Q

what groups does the repulsion exception happen in

A

5 and 6

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2
Q

what groups does the shielding exception happen in

A

2 and 3

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3
Q

ionization energy

A

The amount of energy needed to remove an electron from a gaseous atom

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4
Q

why do jumps in ionization energy happen

A

After an entire energy level is taken away, the element becomes a pseudo-noble gas and becomes much more stable. Ionization energy jumps at group number of atom and next group number

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5
Q

electronegativity

A

attraction of a bonded atom towards electrons

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6
Q

electron affinity

A

The amount of energy associated with the addition of an electron to a gaseous atom

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7
Q

periodic trend for atomic/ionic size

A

increases downward, decreases to the right

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8
Q

periodic trend for ionization energy, electronegativity and electron affinity

A

decreases downward, increases to the right

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9
Q

metallic bond

A

attraction of free floating valence electrons for cations

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10
Q

purpose of Coulomb’s law

A

to calculate energy of attraction

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11
Q

coulomb’s law coefficient

A

2.3110^-19 Jnm

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12
Q

brass

A

copper + zinc

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13
Q

Bronze

A

Copper + tin

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14
Q

Sterling Silver

A

Copper + silver

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15
Q

Steel

A

Iron + carbon

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16
Q

any alloy of mercury

A

amalgum

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17
Q

dipole moment

A

An arrow showing which atom in bond is more electronegative

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18
Q

what atom goes in center of molecule

A

least electronegative atom

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19
Q

dipole

A

molecule that has two poles

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20
Q

can elements in p2 exceed octet rule

A

no

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21
Q

what happens to molecules with 5 atoms

A

all atoms always connect to one center atom

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22
Q

PCl5

A

5 bonds, exception to octet rule

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23
Q

SF6

A

6 bonds around central atom

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24
Q

SO2

A

exception because sulfur does not follow octet rule

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25
Q

BF3

A

boron is deficient of electrons, and as a result spontaneously reacts with something else:NO DOUBLE BONDS

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26
Q

3 classes of hydrocarbons

A

alkanes, alkenes,alkynes

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27
Q

Alkanes

A

CnH2n+2, all single bonds

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28
Q

Alkenes

A

CnH2n,one double bond, isomers with cycloalkanes

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29
Q

Alkynes

A

CnH2n-2,one triple bond

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30
Q

prefix for 1 carbon

A

Meth-

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31
Q

prefix for 2 carbons

A

Eth-

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32
Q

prefix for 3 carbon

33
Q

prefix for four carbon

34
Q

Benzene

A

singular carbon hydrogen ring with 3 double bonds, C6H6

35
Q

Naphthalene

A

used in mothballs, two benzenes attached together, C10H8

36
Q

Alcohol

37
Q

Ether

A

R-O-R’ (‘ means could be different from R)

38
Q

Methane without a hydrogen

A

CH3 methyl group

39
Q

Alkane without a hydrogen

A

Alkyl Group(R)

40
Q

Aldehyde

A

__O
||
R - C - H

41
Q

Ketone

A

_O
||
R-C-R’

42
Q

Ester

A

___O
||
R - C-O-R’

43
Q

Carboxyl(Carboxylic acid)

A

O
||
R-C-OH

44
Q

Amine

45
Q

bond dissociation energy

A

amount of energy needed to break a bond

46
Q

ΔH calculations

A

ΔH = sum of brokent bonds - sum of created bonds

47
Q

what must happen for an oxyacid

A

H must be bonded to O

48
Q

exceptions to polarity rules

A

6 effective pairs, 2 lone pairs and 5 effective pairs 3 lone pairs

49
Q

Bond Order

A

bonds/#bond groups

50
Q

sigma bonds

A

head to head overlap

51
Q

pi bonds

A

side to side overlap, must be parallel

52
Q

triple bond # pi and sigma

A

1 sigma 2 pi

53
Q

sigma stronger or weaker than pi

54
Q

hybridization

A

orbitals mix to form degenerate orbitals

55
Q

how to determine hybridization quick

A

x effective pairs means x num of bonds

56
Q

energy of hybrid with d s and p

A

higher than both s and p, lower than d

57
Q

Molecular geometry/angle of 2 effective pairs, 0 lone pairs

A

linear/180

58
Q

Molecular geometry/angle of 3 effetive pairs, 1 lone pair

59
Q

Molecular geometry/angle of 4 effective pairs, 2 lone pairs

60
Q

Molecular geometry/angle of 5 effective pairs, 3 lone pairs

A

linear/180(exception)

61
Q

Molecular geometry/angle of 3 effective pairs, 0 lone pairs

A

Trigonal planar/120

62
Q

Molecular geometry/angle of 4 effective pairs, 1 lone pairs

A

Trigonal Pyramidal/107

63
Q

Molecular geometry/angle of 5 effective pairs, 2 lone pairs

A

T-Shaped/90

64
Q

Molecular geometry/angle of 4 effective pairs, 0 lone pairs

A

Tetrahedral/109.5

65
Q

Molecular geometry/angle of 5 effective pairs, 1 lone pairs

A

See-saw/90 & 120

66
Q

Molecular geometry/angle of 6 effective pairs, 2 lone pairs

A

Square Planar/90(exception)

67
Q

Molecular geometry/angle of 5 effective pairs, 0 lone pairs

A

Trigonal bipyramidal/ 90 & 120

68
Q

Molecular geometry/angle of 6 effective pairs, 1 lone pairs

A

Square Pyramidal/ 90

69
Q

Molecular geometry/angle of 6 effective pairs, 0 lone pairs

A

Octahedral/90

70
Q

Is charge more or less important than distance for coulumbs law

A

More important

71
Q

Aromatic

A

Double bond in carbon ring

72
Q

Structure of ionic compounds like table salt are unstable

73
Q

Why are metals ductile

A

Because the cations in a piece of pure metal are insulated from one another by a sea of electrons

74
Q

Molecular orbital that lies on axis connecting two atomic nuclei

A

Sigma bond

75
Q

Network solid

A

A substance in which all of the atoms are covalently bonded to each other

76
Q

Why does the overlap of one of the p orbitals form a sigma bond but the rest are pi bond

A

1 pair is head to head, other two pairs are parallel

77
Q

What happens when cl2 is added to an alkane

A

Replaces hydrogen

78
Q

What happens when Cl2 is added to alkene

A

Turns double bond into single bond and replaces hydrogens

79
Q

What happens when Cl2 is added to an Alkyne

A

Triple bond turns into double bond, replaces hydrogens

chemistry (13 decks)

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