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Chem1110 > exam 2 > Flashcards

exam 2 Flashcards

(105 cards)

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1
Q

what charge does group 1 have

A

+1

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2
Q

what charge does group 2 have

A

+2

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3
Q

what charge does group 13 (3) have

A

+3

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4
Q

what charge does group 15 (5) have

A

-3

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5
Q

what charge does group 16 (6) have

A

-2

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6
Q

what charge does group 17 (7) have

A

-1

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7
Q

what charge does Zn have

A

+2

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8
Q

what charge does Ag (silver) have

A

+1

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9
Q

do metals have a positive or negative charge

A

positive

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10
Q

do nonmetals have a positive or negative charge

A

negative

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11
Q

what charge does Sc (scandium) have

A

+3

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12
Q

what metals vary in charge

A

transition, lanthanides, p block metals

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13
Q

how to name ionic bonds

A

[name of cation (metal)] (charge of cation) [base name of anion +ide]

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14
Q

how to name molecular bonds

A

[prefix] [1st element name] [prefix] [2nd element base name +ide]
ex: carbon monoxide

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15
Q

what are acids made of

A

H+ one or more nonmetals

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16
Q

how to name binary acids: two element

A

[hydro] [base name of oxyanion +ic] [acid]
ex: hydrochloric acid

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17
Q

what do oxyacids with more oxygen end with

A

ate
ex: nitrate

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18
Q

what do oxyacids with less oxygen end with

A

ite
ex: nitrite

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19
Q

how to name oxyacids with more oxygen

A

[base name of oxyanion +ic] [acid]
ex: nitric acid

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20
Q

how to name oxyacids with less oxygen

A

[base name of oxyanion +ous] [acid]
ex: nitrous acid

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21
Q

what charges does chromium have

A

Cr2+: chromium (II)
Cr3+: chromium (III)

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22
Q

what charges does iron have

A

Fe2+: iron (II)
Fe3+: iron (III)

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23
Q

what charges does cobalt have

A

Co2+: cobalt (II)
Co3+: cobalt (III)

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24
Q

what charges does copper have

A

Cu+: copper (I)
Cu2+: copper (II)

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25
what charges does tin have
Sn2+: tin (II) Sn4+: tin (IV)
26
what charges does mercury have
Hg2 2+: mercury (I) Hg2+: mercury (II)
27
what charges does lead have
Pb2+: lead (II) Pb4+: lead (IV)
28
acetate formula
C2H3O2-
29
carbonate formula
CO3 2-
30
hydroxide formula
OH-
31
nitrite formula
NO2-
32
nitrate formula
NO3-
33
chromate formula
CrO4 2-
34
dichromate formula
Cr2O7 2-
35
phosphate formula
PO4 3-
36
phosphite formula
PO3 3-
37
ammonium formula
NH4+
38
hypochlorite formula
ClO-
39
chlorite formula
ClO2-
40
chlorate formula
ClO3-
41
perchlorate formula
ClO4-
42
permanganate formula
MnO4-
43
sulfite formula
SO3 2-
44
sulfate formula
SO4 2-
45
cyanide formula
CN-
46
peroxide formula
O2 2-
47
covalent bond
when 2 nonmetals share electrons
48
molecular vs emperical formula
molecular: shows exact number of atoms in a molecule emperical: shows simplest ratio of atoms
49
hydrate equation
Z * nH2O
50
naming hydrate
[name of compound] * [prefix-hydrate]
51
molecular weight
molar mass of a molecule
52
formula weight
molar mass of an ion
53
% weight formula
(n*atomic mass/total mass of a compound)x100 n= number of given atom
54
how to determine empirical formula and molecular formula from % composition
1. change % to grams 2. convert g to mol 3. find simplest whole # ratio
55
octet rule
atoms want 8 valence electrons in a lewis strx
56
what makes a stronger covalent bond
sharing more electrons (double and triple bonds)
57
what makes a shorter covalent bond
sharing more electrons
58
does electronegativity increase or decrease across a period
increase
59
does electronegativity increase or decrease down a group
decrease
60
pure covalent
electrons shared equally between non-metals
61
polar covalent
electrons shared but pulled toward the more electronegative element
62
ionic
electrons are transferred from the metal to the non-metal
63
what atom is usually the central atom in a lewis structure
the least electronegative atom
64
resonance
multiple lewis strx of the same molecule
65
formal charge formula
(# of valence e)-[(# of nonbonding e)+(# of bonding e /2)]
66
Valence Shell VSEPR
electron groups repel one another. shape is determined by repulsion between electron groups
67
linear electron geometry
2 electron groups
68
trigonal planar electron geometry
3 electron groups
69
tetrahedral electron geometry
4 electron groups
70
trigonal bipyramidal electron geometry
5 electron groups
71
octahedral
6 electron groups
72
bent molecular geometry
linear + 1 or 2 lone pairs
73
NH3 bond angle
107.8
74
CO2 molecular geometry and bond angle
linear, 180
75
H2O molecular geometry and bond angle
bent, 104.5
76
valence bond theory
valenece electrons in are in overlapping orbitals
77
1 bond
1 sigma bond
78
double bond
1 sigma and one pi bond
79
triple bond
1 sigma and 2 pi bonds
80
sp electron geometry
1s+ 1p linear
81
sp2 electron geometry
1s+2p trigonal planar
82
sp3 electron geometry
1s+3p tetrahedral
83
sp3d electron geometry
1s+3p+1d trigonal bipyramidal
84
sp3d2 electron geometry
1s+3p+2d octahedral
85
linear bond angle
180
86
trigonal planar bond angle
120
87
tetrahedral bond angle
109.5
88
trigonal bipyramidal bond angle
120, 90
89
octahedral bond angle
90
90
see saw
tetrahedral + 1 lone pair
91
t shaped
trig plan + 2 lone pairs
92
square pyramidal
trig bipyramidal + 1 lone pair
93
square planar
tetrahedral + 2 lone pair
94
linear molecular geometry
2 electron groups or 2 electron groups with 3 lone pairs
95
Transition Metal Orbitals
The 4s orbital is filled before the 3d orbital, but listed after.
96
Free Radicals
Compounds with an odd number of electrons in their Lewis Structure. Eg. NO₂, CN-
97
Coordinate Covalent Bonding
two-electron covalent bond in which the two electrons derive from the same atom; occurs most often between Lewis acids and bases.
98
Silicon Dioxide
Has a unique structure; O-Si-O bonds are always 109.5°.
99
Isomer
contain the same number of atoms of the same elements but differ in structural arrangement and properties
100
mol to liter
1 mol=22.4 L
101
more sheilding
lower electronegativity
102
less sheilding
higher electronegativity
103
how to know if a compound has unpaired electrons
if a lewis strx has an uneven number of electrons or a paramagnetic electron configuration
104
what makes a shorter bond distance
more valence polarity smaller atomic radius
105
how to find mass needed when given % yeild
1. g-> mol 2. stoicheometry 3. (100/% yeild)

Chem1110 (6 decks)

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