Chapter 6: Ionic and Molecular Compounds Flashcards
1
Q
Chemical bonds are formed when…..
A
when atoms lose, gain, or share valence electrons to acquire an octet of eight valence electrons
2
Q
Ionic bonds occur when…
A
when the valence electrons of atoms of a metal are transferred to atoms of NONmetal
3
Q
Covalent bonds occur when…
A
form when atoms of NONmetals share valence electrons
4
Q
Best way to remember covalent vs ionic?
A
Ionic…iconic couple….metal/nonmetal…male/female
5
Q
Atoms form positively charged ions when they lose _____ and negatively charged ions when they gain _____
A
electrons; electrons
6
Q
Group 1A, 2A, and 3A readily lose one or more of their ______ electrons to form ions with a + charge
A
Valence
7
Q
What do elements in groups 1-3 have to do to end up with the same number of valence electrons as the nearest noble gas?
A
Lose electrons
8
Q
What do elements in groups 5-8 have to do to end up with an octet?
A
Gain one or more valence electrons to form ions with a negative charge
9
Q
Na+ and O^2-?
A
Na2O
10
Q
Al^3+ and Cl- ?
A
AlCl3
11
Q
Mg^2+ and N^3-?
A
Mg3N2
12
Q
Ionic compounds, which is a metal/nonmetal compound, is named how?
A
The name of the METAL is written first, and is the same name as the element. The nonmetal is the first syllable of it’s name with an -ide ending. ex: KI is Potassium iodIDE
13
Q
Name mgBr^2
A
Magnesium(metal) bromIDE (nonmetal)
14
Q
Name K2O
A
Potassium Oxide
15
Q
Name CaO
A
Calcium Oxide
16
Q
Name Al 2 S 3
A
Aluminum sulfide
17
Q
Name MgCl2
A
Magnesium Chloride
18
Q
A cation is a:
A
Metal
19
Q
An anion is a:
A
non metal (an-onion is not a metal)
20
Q
Name NaBr
A
Sodium Bromide
21
Q
Bromide is a metal or nonmetal?
A
nonmetal ation
22
Q
Sodium is a metal or nonmetal?
A
metal cation
23
Q
Aluminum is a metal or nonmetal?
A
metal cation
24
Q
Sulfur is a metal or nonmetal?
A
nonmetal ation
25
Write out Cu 2+
Copper (II)
26
Write out Cu+
Copper (I)
27
Write out Fe 2+
Iron(II)
28
Write out Fe+
Iron(I)
29
Write out Fe3+
Iron(III)
30
Write out Pb2+
Lead (II)
31
Write out Pb4+
Lead (IV)
32
Write out Cr2+
Chromium(II)
33
Write out Cr3+
Chromium(III)
34
Transition metals except for Zn2+, Cd2+ and Ag+ form two or more positive ions (cations). They have a _____ ____
Variable change
35
Transition metals are written out using:
Roman numeral equal to the ion charge and the roman n. is placed in parentheses
36
How many ions does the transitional metal Bismuth have?
3+ and 5+
37
How many ions does the transitional metal chromium have?
2+ and 3+
38
How many ions does the transitional metal cobalt have?
2+ and 3+
39
How many ions does the transitional metal copper have
Cu+ and Cu2+
40
How many ions does the transitional metal gold have?
Au+ and Au3+
41
How many ions does the transitional metal iron have?
Fe2+ and Fe 3+
42
How many ions does the transitional metal Lead have
Pb 2+ and Pb 4+
43
How many ions does the transitional metal manganese have?
2+ and 3+
44
How many ions does the transitional metal mercury have?
Hg2 2+ and Hg 2+
45
How many ions does the transitional metal nickel have?
2+ and 3+
46
How many ions does the transitional metal Tin have?
Sn2+ and Sn+4
47
balance the charge and name MnF2
Manganese(II) Fluoride
48
Name MnO
Manganese(II) Oxide
49
write the formula for Nickel(II) Sulfide
NiS
50
Write the formula for Zinc chloride
ZnCl2
51
Write the formula for iron(III) oxide
Fe2O3
52
Polyatomic ions have a negative charge except for ______, which is ammonium
NH4+
53
Polyatomic ions often consist of a nonmetal such as _____, ______, _____ or ______, covalently boned to oxygen atoms
Phosphorus, sulfur, carbon, or nitrogen
54
Polyatomic ions are _____ of ions that have an ionic charge
groups
55
Name: OH-
Hydroxide
56
Name: NH4)+
Ammonium
57
Name: NO3)-
Nitrate
58
Name: NO2)-
Nitrite
59
Name: ClO)4-
Perchlorate
60
Name: ClO)3-
Chlorate
61
Name: ClO)2-
Chlorite
62
Name ClO)-
Hypochlorite
63
Name: CO3)2-
Carbonate
64
Name: HCO3)-
Bicarbonate
65
Name: CN)-
Cyanide
66
Name: C2H3O2)-
Acetate
67
Name: SO4)2-
Sulfate
68
Name: HSO4)-
Bisulfate
69
Name: SO3)2-
Sulfite
70
Name: HSO3)-
Bisulfite
71
Name: PO4)3-
Phosphate
72
Name: HPO4)2-
Hydrogren phosphate
73
Name: H2PO4)-
Dihydrogen phosphate
74
Name: PO3)3-
Phosphite
75
Which three common polyatomic ions end in -ate?
Sulfate [SO4)2-], Phosphate [PO4)3-], and Nitrate [NO3)-]
Sulfate4, phosphate4, and nitrate3
76
common polyatomic ions that end in -ite?
Sulfite3, Phosphite3, and nitrite2
77
Write the formula for Sodium Phosphate
Na3PO4
78
Write the formula for copper(II) nitrate
Cu(NO3)2
79
Write the formula for Iron(III) hydroxide
Fe(OH)3
80
Write the formula for aluminum nitrate
Al(NO3)3
81
Write the formula for tin(IV) hydroxide
Sn(OH)4
82
Molecular compounds (covalent) need prefixes because:
several compounds can be formed from the same two nonmetals
83
Name CO2
Carbon dioxide
84
Name CS2
Carbon disulfide
85
Name N2O
Dinitride oxide
86
Name NO
Nitrogen Oxide
87
Molecular compounds form when atoms of to or more nonmetals share _____ and form a _____ bond
electrons, covalent bond
88
Molecular compounds form when ______ electrons are shared by nonmetals to achieve stability
valence
89
A ______ forms when two ore more atoms share electrons
Molecule
90
The first nonmetal in a molecular compound is named by its _____ name
element
91
The second nonmetal in a molecular compound is named by using the first syllable of its name followed by -___
Ide
92
In a molecular compound, when a subscript indicates two or more atoms of an element, a _____ is used
Prefix
93
Name NO2 and NO3
Nitrogen dioxide and Nitrogen trioxide
94
mono =
one
95
Di =
two
96
Tri=
three
97
Tetra=
four
98
penta =
five
99
Hexa =
6
100
hepta =
7
101
octa=
8
102
nona=
nine
103
deca=
10
104
Valence electrons are shared by _____ atoms to achieve stability
nonmetal
105
A ______ forms when two or more atoms share electons
molecule
106
Exceptions to the Octet rule: Nonmetals P, S, Cl, Br, and I can form compounds with ____ or ____ valence electrons
10 or 12
107
The __ atom has an octet in many compounds but in ___, there are 12 valence electrons or six bonds to the ___ atom.
S atom, SF6, Sulfur atom
108
Shape of methane molecule:
Tetrahedral
109
Describe the VSEPR theory
The valence shell electron-pair repulsion theory describes the orientation of electron groups around the central atom.
- states that electron groups are arranged as far apart as possible around the central atom
- states that the specific shape of a molecule is determined by the number of atoms attached to the central atom
110
Shape of ammonia molecule:
Tigonal Pyrimidal
111
Shape of h2O molecule:
Bent
112
Name three common non polar molecules
H2, Cl2, and O2
113
Nonpolar molecules with polar bonds can be non polar if the _____ in the polar bonds cancel each other out in a symmetrical arrangement such as CO2 and CCl4
dipolar: O====C====O
114
Polar molecules such as HCl are polar because:
- one end of the molecule is more _____ charged than the other.
- the polar bonds in the molecule do/do not cancel each other?
- The _____ are shared unequally in the polar covalent bond
- Negatively
- Do not
- Electrons
115
Is H2O a polar molecule?
Yes
116
H2O has dipoles that do not cancel, making the molecule ______ at one and and _____ at the other
positive/negative
117
Is NH3 polar or non polar?
Polar
118
Why is NH3 polar?
- there is one lone pair and three bonds around the central atom.
- There are dipoles that do not cancel, making it neg/ at one end and + at the other end
- there is a partial negative charge on the central atom
119
In covalent compounds, polar molecules exert attractive forces called ____ ____ _______
Dipole-Dipole attractions
120
In covalent compounds, polar molecules have dipoles where the positively charged end of the dipole in one molecule is attracted to the ______ charged end of the dipole in another molecule
Negatively
121
In covalent compounds, polar molecules form strong dipole attractions called ____ ____ between hydrogen atoms bonded to F, O, or N and a lone pair on F, O, or N.
Hydrogen bonds
122
______ bonds are the strongest force between molecules and play a major role in the shape of DNA
Hydrogen
123
_____ _____ are weak attractions between non polar molecules
Dispersion forces
124
_____ _____ are caused by temporary dipoles that develop when molecules bump into each other
dispersion forces
125
____ ____ are weak but make it possible for non polar molecules to form liquids and solids
dispersion forces
126
Melting points of compounds:
| -are related to the strength of attractive forces between _____ or _____
molecules or compounds
127
Melting points of compounds are lower as a result of weak forces such as _____ _____
dispersion forces
128
Melting points of compounds are higher as a result of stronger attractive forces such as _____ ___-
hydrogen bonding
129
Melting points of compounds are highest in _____ compounds as a result of the strong attractive forces between ions in the compound
ionic
130
A double bond occurs when atoms share two ____ of electrons
pairs
131
A double bond forms when there are not enough _____ to complete octetts
electrons
132
A triple bond occurs when atoms share ____ pairs of electrons
three
133
A triple bond forms when there are not enough electrons to complete ______
octets
