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chemistry > Unit 14-16 > Flashcards

Unit 14-16 Flashcards

(79 cards)

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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
BF3
boron is deficient of electrons, and as a result spontaneously reacts with something else:NO DOUBLE BONDS
26
3 classes of hydrocarbons
alkanes, alkenes,alkynes
27
Alkanes
CnH2n+2, all single bonds
28
Alkenes
CnH2n,one double bond, isomers with cycloalkanes
29
Alkynes
CnH2n-2,one triple bond
30
prefix for 1 carbon
Meth-
31
prefix for 2 carbons
Eth-
32
prefix for 3 carbon
Prop-
33
prefix for four carbon
But-
34
Benzene
singular carbon hydrogen ring with 3 double bonds, C6H6
35
Naphthalene
used in mothballs, two benzenes attached together, C10H8
36
Alcohol
R-OH
37
Ether
R-O-R' (' means could be different from R)
38
Methane without a hydrogen
CH3 methyl group
39
Alkane without a hydrogen
Alkyl Group(R)
40
Aldehyde
__O || R - C - H
41
Ketone
_O || R-C-R'
42
Ester
___O || R - C-O-R'
43
Carboxyl(Carboxylic acid)
O || R-C-OH
44
Amine
R-NH2
45
bond dissociation energy
amount of energy needed to break a bond
46
ΔH calculations
ΔH = sum of brokent bonds - sum of created bonds
47
what must happen for an oxyacid
H must be bonded to O
48
exceptions to polarity rules
6 effective pairs, 2 lone pairs and 5 effective pairs 3 lone pairs
49
Bond Order
#bonds/#bond groups
50
sigma bonds
head to head overlap
51
pi bonds
side to side overlap, must be parallel
52
triple bond # pi and sigma
1 sigma 2 pi
53
sigma stronger or weaker than pi
stronger
54
hybridization
orbitals mix to form degenerate orbitals
55
how to determine hybridization quick
x effective pairs means x num of bonds
56
energy of hybrid with d s and p
higher than both s and p, lower than d
57
Molecular geometry/angle of 2 effective pairs, 0 lone pairs
linear/180
58
Molecular geometry/angle of 3 effetive pairs, 1 lone pair
bent/120
59
Molecular geometry/angle of 4 effective pairs, 2 lone pairs
bent/105
60
Molecular geometry/angle of 5 effective pairs, 3 lone pairs
linear/180(exception)
61
Molecular geometry/angle of 3 effective pairs, 0 lone pairs
Trigonal planar/120
62
Molecular geometry/angle of 4 effective pairs, 1 lone pairs
Trigonal Pyramidal/107
63
Molecular geometry/angle of 5 effective pairs, 2 lone pairs
T-Shaped/90
64
Molecular geometry/angle of 4 effective pairs, 0 lone pairs
Tetrahedral/109.5
65
Molecular geometry/angle of 5 effective pairs, 1 lone pairs
See-saw/90 & 120
66
Molecular geometry/angle of 6 effective pairs, 2 lone pairs
Square Planar/90(exception)
67
Molecular geometry/angle of 5 effective pairs, 0 lone pairs
Trigonal bipyramidal/ 90 & 120
68
Molecular geometry/angle of 6 effective pairs, 1 lone pairs
Square Pyramidal/ 90
69
Molecular geometry/angle of 6 effective pairs, 0 lone pairs
Octahedral/90
70
Is charge more or less important than distance for coulumbs law
More important
71
Aromatic
Double bond in carbon ring
72
Structure of ionic compounds like table salt are unstable
False
73
Why are metals ductile
Because the cations in a piece of pure metal are insulated from one another by a sea of electrons
74
Molecular orbital that lies on axis connecting two atomic nuclei
Sigma bond
75
Network solid
A substance in which all of the atoms are covalently bonded to each other
76
Why does the overlap of one of the p orbitals form a sigma bond but the rest are pi bond
1 pair is head to head, other two pairs are parallel
77
What happens when cl2 is added to an alkane
Replaces hydrogen
78
What happens when Cl2 is added to alkene
Turns double bond into single bond and replaces hydrogens
79
What happens when Cl2 is added to an Alkyne
Triple bond turns into double bond, replaces hydrogens

chemistry (13 decks)

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