Chapter 5: Ionic and Molecular Compounds Flashcards
(200 cards)
1
Q
Atoms form ____ ions when they lose electrons
A
positively charged
2
Q
Atoms form ____ ions when they gain electrons
A
Negatively charged
3
Q
____ are formed by the strong attractive forces between positive
and negative ions
A
Ionic bonds
4
Q
____ are formed when atoms lose, gain,
or share valence electrons to acquire an octet of eight valence electrons (octet rule).
A
Chemical bonds
5
Q
____ occur when valence electrons of a metal atom are transferred to the atom of a
nonmetal.
A
Ionic bonds
6
Q
Ionic bonds occur when valence electrons of a
_____ are transferred to the atom of a
____
A
metal atom, nonmetal
7
Q
____ occur when nonmetal atoms
share electrons to attain a noble gas arrangement
A
Covalent bonds
8
Q
Covalent bonds occur when ____
share electrons to attain a noble gas arrangement.
A
nonmetal atoms
9
Q
Metals, Group 1A (1),Group 2A (2), and Group 3A (13) have:
A
- have low ionization energies.
- readily lose one or more of their valence electrons to form ions with a positive charge.
- lose electrons until they have the same number of valence electrons as the nearest noble gas, usually eight valence electrons.
10
Q
Metals ___ until they have the same number of valence electrons
A
lose electrons
11
Q
Sodium will ___ lose its electrons to form the octet rule
A
lose
12
Q
Magnesium atoms in Group 2A (2) are neutral, will ___ electrons
A
lose 2
13
Q
Nonmetals, Group 5A (15), Group 6A (16), andGroup 7A (17) have:
A
- have high ionization energies.
- readily gain one or more valence electrons to form
ions with a negative charge. - gain electrons until they have the same number of
valence electrons as the nearest noble gas, usually eight valence electrons.
14
Q
Nonmetals are the following group :
A
Group 5A (15), Group 6A (16), and
Group 7A (17)
15
Q
Nonmetals readily gain one or more valence electrons to form
ions with ____
A
a negative charge.
16
Q
Metal group that has 3+ charge
A
Group 3A
17
Q
Metal group that has 2+ charge
A
Group 2A
18
Q
Metal group that has 1+ charge
A
Group 1A
19
Q
Nonmetal group that has 2- charge
A
group 6A
20
Q
Nonmetal group that has 3- charge
A
group 5A
21
Q
Nonmetal group that has 1- charge
A
group 7A
22
Q
ca 2+ name
A
Calcium ion
23
Q
Cl- name
A
chloride
24
Q
____ consist of
positive and negative charges
held together by the strong
electrical attractions between
oppositely charged ions
A
Ionic compounds
25
_____ are important in regulating body function
ions
26
Na+ function in the body
Regulation and control of
body fluids
27
K+ function in the body
Regulation of body fluids
and cellular functions
28
Ca2+ function in the body
Major cation in bones,
needed for muscle
contractions
29
Mg2+ function in the body
Essential for certain
enzymes, muscles, and
nerve control
30
Na+ occurrence
Principal cation
outside the cell
31
K+ occurrence
Principal cation
outside the cell
32
Ca2+ occurrence
Major cation in bones,
needed for muscle
contractions
33
Mg2+ occurrence
Cation outside the
cell; found in bones
34
Na+ food source
Salt, cheese,
pickles
35
K+ Food source
Bananas, potatoes,
orange juice, milk
36
Ca2+ Food source
Milk, yogurt,
cheese, greens,
spinach
37
Mg2+ food source
Chlorophyll, nuts,
grains
38
A compound that consist of positive and negative ions.
Ionic compounds
39
Ionic compounds have attractions called ____ between
positively and negatively charged ions.
ionic bonds
40
Ionic compound physical characteristics:
* have high melting points.
* are solids at room temperature
41
___ is
more commonly
known as table salt.
Sodium chloride
42
In chemical formula, the symbols and subscripts are written in the _____ of the atoms or ion
lowest whole-number ratio
43
In a chemical formula, the sum of ion charges equals ___
0
44
In a chemical formula, the total positive charge = ____
total negative charge.
45
To get the ionic formula, the superscript charge of elements should be ____
criss-cross
46
Al^3+ N^3- in ionic formula
Al3N3 or AlN (simplified)
47
Li ^+ O^2- in ionic formula
Li2O
48
Pb^4+ O^2-
Pb2O4 or PbO2 (simplified)
49
Na+ and O2− correct ionic formula
Na2O
50
Al3+ and Cl− correct ionic formula
AlCl3
51
Mg2+ and N3− correct formula
Mg2N3
52
How to check if the ionic formula is correct?
if the net charge is zero
53
what is the ionic formula and net charge of Na+ and O2−?
Na2O (net charge: 2 (1+)+ 1(2-) =0)
54
what is the ionic formula and net charge of Mg2+ and N3− ?
Mg3N2 (Net charge: 3(2+) + 2(3-)= 0)
55
When naming an ionic compound, the name of the_____ is written first and is the ___ as the name of the element
metal, same (eg. Sodium chloride)
56
When naming an ionic compound, the name of the ____ is the first syllable of the nonmetal name + ____ ending and is written second.
nonmetal, ide ( eg. Sodium chloride)
57
When naming an ionic compound, a ___ is placed between the name of the metal and nonmetal ion.
space
58
What is the name of ionic compound KI?
Potassium Iodide
59
What is the name of ionic compound MgBr2?
Magnesium bromide
60
What is the name of ionic compound Al2O3?
Aluminum oxide
61
Cation is ?
Positive
62
Anion is ?
negative
63
Name the ____ by its element name
Cation
64
Name the ___ by using the first
syllable of its element name
followed by ___
Anion, -ide
65
What is the name of the ionic compound K2O?
Potassium oxide
66
What is the name of the ionic compound CaO?
Calcium oxide
67
What is the name of the ionic compound MgCl2?
Magnesium chloride
68
CaO, identify the cation and anion.
Ca2+ cation and O2- anion
69
Name the cation by its element name, Al2O3
Al3+ aluminum (cation includes the charge)
70
MgCl2: The anion is
Cl-, chloride
71
NaBr- ionic compound name
Sodium bromide
72
Na2S ionic compound name
Sodium sulfide
73
Na3N ionic compound name
Sodium nitride
74
Al2S3 ionic compound name
Aluminum sulfide
75
AlBr3 ionic compound name
Aluminum bromide
76
AlN ionic compound name
Aluminum nitride
77
Transition metals except ___, ___, ___ form 2 or more positive ions (cations)
Zn2+, Cd2+, and Ag+
78
For transition metals, ____ equal to the ion charge is placed in parentheses immediately after the metal name
Roman numeral
79
Cu2+ name
copper (ll)
80
Fe3+ name
iron(III)
81
Pb4+ name
lead (IV)
82
Cr2+ name
Chromium (II)
83
Bi3+ name
bismuth (III)
84
Bi5+ name
Bismuth(V)
85
Au+ name
Gold (I)
86
Au3+ name
Gold (III)
87
Mn2+ name
Manganese (II)
88
Mn3+ name
Manganese (III)
89
Sn2+ name
Tin (II)
90
Sn4+ name
Tin (IV)
91
Co2+ name
Cobalt (II)
92
Ni 2+ name
Nickel (II)
93
Ni3+ name
Nickel (III)
94
Hg2+ name
mercury(II)
95
Hg3+ name
Mercury (III)
96
MnF2
Manganese (II) fluoride
97
The roman numeral is based on the ___ of the transition metal
charge
98
this also includes to the transition metal
Al3+, Sn2+, Sn4+, Pb 2+, Pb4+, Bi3+, Bi 5+
99
Name the ionic compound SnO2
Tin (IV) oxide
100
Chromium charges:
Cr2+ and Cr3+
101
Manganese charges:
Mn2+ and Mn3+
102
Iron charges:
Fe2+ and Fe3+
103
Cobalt charges:
Co2+ and Co3+
104
Nickel charges:
Ni2+ and Ni3+
105
Copper charges
Cu1+ and Cu2+
106
Zinc charges:
Zn2+
107
Silver charges:
Ag1+
108
gold charges:
Au1+ and Au3+
109
cadmium charges
Cd2+
110
Mercury charges:
Hg2^2+ and Hg2+
111
Aluminum charges:
Al3+
112
Tin charges:
Sn2+ and Sn4+
113
Lead charges:
Pb2+ and Pb4+
114
Bismuth charges:
Bi3+ and Bi5+
115
Name the FeCl2
Iron(II) chloride
116
SnO2 name
Tin (IV) oxide
117
Name of the PbS2
Lead (IV) sulfur
118
Formula for the nickel(ii) sulfide
Ni2S2
119
Formula of the ionic compound Zinc chloride
ZnCl
120
Formula for the Iron(III) oxide
FeO3
121
based the __ of the element for the last number of the electronic configuration
charge
122
What is the electronic configuration of the Na2+
1s2 2s2 2p6 = [Ne]
123
___ are a group of atoms with an overall charge
Polyatomic ions
124
____ often consist of a nonmetal such as phosphorus, sulfur, carbon, or nitrogen and
oxygen.
Polyatomic ions
125
Polyatomic ions often consist of a nonmetal such as
phosphorus, sulfur, carbon, or nitrogen and
oxygen
126
Polyatomic ions usually have _,_, or _ charge
1−, 2−, or 3− charge
127
Polyatomic ions have a negative charge, except for _____, which has a positive charge
NH4+
ammonium
128
Many products contain _____, which are groups of ions that have an ionic charge.
polyatomic ions
129
Nonmetal: Hydrogen
formula of Ion: OH-
What is the name of the ion?
Hydroxide
130
Nonmetal: Nitrogen
formula of Ion: Cl04-
What is the name of the ion?
Perchlorate
131
Nonmetal: Nitrogen
formula of Ion: Cl03-
What is the name of the ion?
Chlorate
132
Nonmetal: Nitrogen
formula of Ion: Cl02-
What is the name of the ion?
Chlorite
133
Nonmetal: Nitrogen
formula of Ion: Cl0-
What is the name of the ion?
Hypochlorite
134
Nonmetal: carbon
formula of Ion: CO3^2-
What is the name of the ion?
Carbonate
135
Nonmetal: carbon
formula of Ion: HCO3-
What is the name of the ion?
Hydrogen carbonate or bicarbonate
136
Nonmetal: carbon
formula of Ion: CN-
What is the name of the ion?
Cyanide
137
Nonmetal: carbon
formula of Ion: C2H3O2
What is the name of the ion?
Acetate
138
Nonmetal: Sulfur
formula of Ion: SO4^2-
What is the name of the ion?
Sulfate
139
Nonmetal: Sulfur
formula of Ion: HSO4-
What is the name of the ion?
Hydrogen sulfate (or bisulfate)
140
Nonmetal: Sulfur
formula of Ion: SO3^2-
What is the name of the ion?
Sulfite
141
Nonmetal: Sulfur
formula of Ion: HSO3-
What is the name of the ion?
Hydrogen sulfite or bisulfite
142
Nonmetal: Phosphorus
formula of Ion: PO4^3-
What is the name of the ion?
Phosphate
143
Nonmetal: Phosphorus
formula of Ion: HPO4^2-
What is the name of the ion?
Hydrogen phosphate
144
Nonmetal: Phosphorus
formula of Ion: H2PO4
What is the name of the ion?
Dihydrogen phosphate
145
Nonmetal: Phosphorus
formula of Ion: PO3^3-
What is the name of the ion?
Phosphite
146
Names of most common polyatomic ions end in ____
-ate (eg. SO4^2−sulfate
PO4^3−phosphate
NO3− nitrate)
147
When a related ion has one less oxygen, its name
ends in ____
-ite. (eg. SO3^2−sulfite
PO3^3−phosphite
NO2− nitrite )
148
Exceptions to the rules in polyatomic ions rules are the following:
CN− cyanide
OH− hydroxide
149
Add an H+ to the polyatomic ion, and add ___ to its charge.
+1
150
Based on the rule #4 of Polyatomic ion, CO3^2− + H+ = HCO3−
Based on the rule #4 of Polyatomic ion, SO4^2− + H+ = HSO4−
151
____ form 4 polyatomic
ions with oxygen.
Each has a −1 charge.
Halogens
152
In writing the formula for the ionic compound that contains polyatomic ions, the ____ is placed inside the parenthesis
polyatomic ions (Eg. Mg(NO3)2 - magnesium nitrate)
153
What is the process when naming ionic compounds containing polyatomic ions?
* first write the positive ion, usually a metal.
* write the name of the polyatomic ion second (put it inside the parenthesis when the coefficient is higher than 1)
154
Na2SO4 name
Sodium sulfate
155
FePO4 name
Iron (III) phosphate
156
Al2(CO3)3 name
Aluminum carbonate
157
Ca(NO3)2 name
Calcium nitrate
158
FePO4 name
Iron (III) phosphate
159
MgSO3 name
Magnesium sulfite
160
MgSO4
Magnesium sulfate
161
Pb3(PO3)2
Lead (II) phosphite
162
Fe2(SO4)3
Iron(II) sulfate
163
Ba3(PO3)2
Barium phosphite
164
NiCO3
Nickel (II) carbonate
165
The ___ need prefixes
because several different
compounds can be formed from
the same two nonmetals.
names of molecular
compounds
166
The names of molecular
compounds need prefixes
because several different
compounds can be formed from
the ____
same two nonmetals.
167
Molecular compounds form when
atoms of two or more nonmetals share electrons and form a ____
covalent bond
168
____ form when valence electrons are shared by nonmetal atoms to achieve stability
Molecular compounds
169
A ___forms when two or more atoms share electrons.
molecule
170
A molecule forms when two or more atoms ____
share electrons
171
In naming covalent bond, the following are needed to be follow:
1. first nonmetal is named by its element name
2. Second nonmetal is named using the first syllable of the name followed by ide
172
In naming covalent compound, when a subscript indicates
two or more atoms of an
element, a ____is shown in
front of its name
prefix
173
Prefixes used in naming molecular compound:
1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca
174
Prefix for subscript 1
mono
175
Prefix for subscript 2
di
176
Prefix for subscript 3
tri
177
Prefix for subscript 4
tetra
178
Prefix for subscript 5
penta
179
Prefix for subscript 6
hexa
180
Prefix for subscript 7
hepta
181
Prefix for subscript 8
octa
182
Prefix for subscript 9
nona
183
Prefix for subscript 10
deca
184
In naming 2 nonmetals, if the vowels o and o or a and o appear
together, the first vowel is ___
omitted (eg. Carbon monooxide = carbon monoxide)
185
CS2 name
Carbon disulfide
186
CO2 name
carbon dioxide
187
N2O name
Dinitrogen oxide
188
SO3
Sulfur trioxide
189
Name the molecular compound: B2O3
Diboron trioxide
190
What is the formula for diphosphorus pentoxide
P2O5
191
If the first element is metal, it is an __ compound
ionic
192
If the first element is nonmetal, it is an __ compound
covalent
193
The ionic compound uses suffix __
-ide
194
The covalent compound uses __ depending on the subscript
prefix
195
SO3, ionic or covalent?
covalent
196
BaCl2, ionic or covalent?
ionic
197
(NH4)3PO3, ionic or covalent?
ionic
198
Cu2CO3, ionic or covalent?
ionic
199
. N2O4, ionic or covalent?
covalent
200
