Unit 3 Flashcards
(120 cards)
1
Q
hydrogen
A
H+
2
Q
lithium
A
Li+
3
Q
sodium
A
Na+
4
Q
potassium
A
K+
5
Q
rubidium
A
Rb+
6
Q
cesium
A
Cs+
7
Q
beryllium
A
Be+2
8
Q
magnesium
A
Mg+2
9
Q
calcium
A
Ca+2
10
Q
strontium
A
Sr+2
11
Q
Barium
A
Ba+2
12
Q
aluminum
A
Al+3
13
Q
silver
A
Ag+
14
Q
nickel
A
Ni+2
15
Q
zinc
A
Zn+2
16
Q
cadmium
A
Cd+2
17
Q
copper (I)
A
Cu+
18
Q
copper(II)
A
Cu+2
19
Q
iron (II)
A
Fe+2
20
Q
iron(III)
A
Fe+3
21
Q
tin(II)
A
Sn+2
22
Q
tin(IV)
A
Sn+4
23
Q
lead(II)
A
Pb+2
24
Q
lead(IV)
A
Pb+4
25
cobalt(II)
Co+2
26
cobalt(III)
Co+3
27
mercury(I)
Hg2 +2
28
mercury(II)
Hg+2
29
ammonium
NH4+
30
suffix change
anions
31
ide, ite, ate
anions
32
hydride
H-
33
fluoride
F-
34
chloride
Cl-
35
bromide
Br-
36
iodide
I-
37
oxide
O-2
38
sulfide
S-2
39
selenide
Se-2
40
telluride
Te-2
41
nitride
N-3
42
phosphide
P-3
43
nitrate
NO3-
44
nitrite
NO2-
45
sulfate
SO4 -2
46
sulfite
SO3 -2
47
hydroxide
OH-
48
acetate
CH3CO2
49
cyanide
CN-
50
carbonate
CO3 -2
51
hypochlorite
CIO-
52
chlorite
CIO2-
53
chlorate
CIO3-
54
perchlorate
CIO4-
55
chromate
CrO4 -2
56
dichromate
Cr2O7 -2
57
permanganate
MnO4 -2
58
bicarbonate
HCO3-
59
bisulfate
HSO4-
60
bisulfite
HSO3-
61
phosphate
PO4 -3
62
hydrogen phosphate
HPO4 -2
63
dihydrogen phosphate
H2PO4-
64
transfer e-
ionic bonding
65
metal and nonmetal
ionic bonding
66
ionic compound
ionic bonding
67
share e-
covalent bonding
68
nonmetal and metalloid
covalent bonding
69
molecular compound
covalent bonding
70
molecular element (7 diatomic elements)
covalent bonding
71
size of an atom
atomic radii
72
we know atoms are what shape
spheres
73
t or f atoms are all the same size
false
74
as we move down a group, the atomic radius
increases
75
as we move across a period from left - right the atomic radius
decreases
76
why does atomic radius increase as we go down a group
we have a larger number of energy levels and larger atomic radius because of it
77
why does atomic radii decrease as we move left - right across a period
we have a larger number of protons and electrons
78
electrons are pulled closer to nucleus
larger attraction
79
radius smaller
larger attraction
80
size of monoatomic ions
spheres
81
what are smaller than their corresponding atoms
cations
82
what are larger than their corresponding atoms
anions
83
why are cations smaller than their corresponding atoms
with a smaller number of energy, cation has a smaller radius than its corresponding
84
extra electrons cause what
some additional repulsions between the electrons
85
what do electrons do to minimize additional repulsions
expand outward
86
when electrons expand outward the
radius increases
87
same number of electrons
isoelectronic series
88
process of removing an electron from an atom is called
ionization
89
amount of energy required to remove an electron from an isolated atom in the gas phase
ionization energy
90
in each period which elements have the largest ionization energy
noble gases
91
in each period which elements have the smallest ionization energy
alkai metals
92
in each period which elements have similar ionization energies
transition metals
93
why do the noble gases have the largest ionization energies in each period
don't want to lose their NGEC; make removing e- as difficult as possible (large ionization energy)
94
why do alkai metals have the smallest ionization energies
want to lose electron to get NGEC so make it as easy as possible; making small ionization energy
95
amount of energy absorbed when an electron is added to an isolated atom in the gas phase
electron affinity
96
why do the transition metals within a period all have similar ionization energies
lose same e- (same amount of energy, similar ionization energies)
97
tendency of an atom to attract electrons towards itself when chemically combined with other atoms
electronegativity
98
atom has a strong desire to attract electrons
large electronegativity
99
atom has little desire to attract electrons toward itself
small electronegativity
100
e- are shared equally between the 2 atoms; occurs when 2 atoms involved have the same (or similar) electronegativities
nonpolar covalent bond
101
small difference in electronegativity
nonpolar covalent bond
102
electrons are shared but aren't shared equally
polar covalent bond
103
occurs when there is a noticeable difference in the electronegativity of the 2 atoms included
polar covalent bond
104
medium size difference in electronegaitivty
polar covlanet bond
105
force of attraction between two molecules
intermolecular force
106
this particular example is an example of a hydrogen bond
intermolecular bond
107
only occurs when a hydrogen is attracted to either N,O,F
N-H O-H F-H
108
the smallest electrically neutral collection of ions
formula unit
109
no difference or very small difference in electronegativities
nonpolar covalent
110
electrons are shared equally between the two atoms
nonpolar covalent
111
no charges are present
nonpolar covalent
112
atoms are connected by covalent bonds
nonpolar covalent
113
medium size difference in electronegativities
polar covalent
114
electrons are shared unequally between the two atoms
polar covalent
115
partial charges are present
polar covalent
116
atoms are connected by covalent bonds
polar covlanent
117
large difference in electronegativities
ionic bond
118
electrons are transferred from one atom to another
ionic
119
full charges are present
ionic
120
ions are not connected
ionic bond
