Chemistry Ionic Compounds and Formulas Flashcards
1
Q
Sulfate
A
SO42-
2
Q
Phosphate
A
PO43-
3
Q
Chlorate
A
ClO3-
4
Q
Carbonate
A
CO32-
5
Q
Hydroxide
A
OH-
6
Q
Hydride
A
H-
7
Q
Silver ion
A
Ag+
8
Q
Zinc ion
A
Zn2+
9
Q
Peroxide
A
O22-
10
Q
Chromate
A
CrO42-
11
Q
Dichromate
A
Cr2O72-
12
Q
Permanganate
A
MnO4-
13
Q
Cyanide
A
CN-
14
Q
Acetate
A
CH3COO-
15
Q
Nitrate
A
NO3-
16
Q
Ammonium
A
NH4+
17
Q
Mono-
A
1
18
Q
Di-
A
2
19
Q
Tri-
A
3
20
Q
Tetra-
A
4
21
Q
Penta-
A
5
22
Q
Hexa-
A
6
23
Q
Hepta-
A
7
24
Q
Octa-
A
8
25
Nona
9
26
Deca-
10
27
To name an acid for an anion that ends in -ide, replace -ide with _____.
Hydro- -ic acid
28
To name an acid for an anion that ends in -ite, replace -ite with _____.
-ous acid
29
To name an acid for an anion that ends in -ate, replace -ate with _____.
-ic acid
30
Molecular compounds are formed between
Nonmetals
31
Ionic compounds are formed between
Metals and nonmetals
32
Perchlorate
ClO4-
33
Chlorite
ClO2-
34
Hypochlorite
ClO-
35
Chloride
Cl-
36
Bromate
BrO3-
37
Bromide
Br-
38
Iodide
I-
39
Sulfide
S2-
40
Density equation
D=m/V
41
Percent error equation
% error = 100|(observed value - expected value)|/expected value
42
Group 1A Name
Alkali metals
43
Group 1A Charge
1+
44
Group 2A Name
Alkaline earth metals
45
Group 2A Charge
2+
46
Group 3A Charge
3+
47
Group 5A Charge
3-
48
Group 6A Name
Chalcogens
49
Group 6A Charge
2-
50
Group 7A Name
Halogens
51
Group 7A Charge
1-
52
Group 8A Name
Noble Gases
53
Group 8A Charge
No charge
54
Cm3
1 mL
55
Phosphite
PO33-
56
What are the 3 parts to the scientific method in the order they occur?
1. Observation
2. Hypothesis
3. Test
57
Concentration1Volume1 = Concentration2Volume2
C1V1 = C2V2
58
Molar mass equation
g/mol
59
Avogadro’s number
1 mole (mol) = 6.022 X 1023
60
Fe
Iron
61
K
Potassium
62
Ti
Titanium
63
S
Sulfur
64
U
Uranium
65
Sn
Tin
66
Au
Gold
67
Ag
Silver
68
Na
Sodium
69
P
Phosphorus
70
Cu
Copper
71
Pb
Lead
72
Mg
Magnesium
73
Hg
Mercury
74
The variable that the experimenter changes or manipulates
The independent variable
75
The variable that is effected and responds to the independent variable; the variable you measure
The dependent variable
76
The variables that are held constant
The control variable
77
The variable that goes on the X-axis
The independent variable
78
The variable that goes on the Y-axis
The dependent variable
79
Mixtures that vary in composition throughout a sample
Heterogeneous mixtures
80
Mixtures that have the same composition throughout the sample
Homogeneous mixtures
81
Properties that can be observed without changing a substance
Physical properties
82
Examples of physical properties
Boiling point, density, mass, or volume
83
Properties that can only be observed when a substance is changed into another substance
Chemical properties
84
Examples of chemical properties
Flammability, corrosiveness (breakdown), or reactivitiy with acid(s) (changes it into something else)
85
Properties that are independent of the amount of the substance that is present
Intensive properties
86
Examples of intensive properties
Density (as long as substances are in the same state of matter), boiling point, or color
87
Properties that depend upon the amount of the substance present
Extensive properties
88
Examples of extensive properties
Mass, volume, or energy (it would take more energy to boil a gallon of water than it would to boil 10 mL of water)
89
Changes in matter that do *not* change the composition of a substance
Physical changes
90
Examples of physical changes
Changes of state of matter, temperature, and volume
91
Changes that result in new substances
Chemical changes
92
Examples of chemical changes
Combustion, oxidation, redox (iron rusting), and decomposition
93
Giga-
Abbreviation: G
1Gm = 109m
94
Mega-
Abbreviation: M
1Mm = 106m
95
Kilo-
Abbreviation: K
1Km = 1000m
96
Deci-
Abbreviation: d
10dm = 1m
97
Centi-
Abbreviation: c
100cm = 1m
98
Milli-
Abbreviation: m
1000mm = 1m
99
Micro-
Abbreviation: μ
1μm = 10-6m
100
Nano-
Abbreviation: n
1nm = 10-9m
101
Mass unit
g (grams)
102
Volume unit
mL or cm3
103
The freezing point of water
0°C
104
The boiling point of water
100°C
105
__________ refers to the proximity of a measurement to the true value of a quantity.
Accuracy
106
__________ refers to the proximity of several measurements to each other.
Precision
107
What are the significant figure rules?
1. All nonzero digits are significant.
2. Zeros between two significant figures are themselves significant.
3. Zeroes at the beginning of a number are never significant.
4. Zeroes at the end of a number are significant if a decimal point is written in the number.
108
When you multiply or divide, the answer is rounded to the number of digits that corresponds to the _______________.
Least number of significant figures
109
When addition or subtraction is performed, answers are __________________.
Rounded to the least significant decimal place
110
What is stoichiometry?
The area of study that examines the quantities of substances consumed and produced in chemical reactions.
111
What does the Law of Conservation of Mass state?
An equal amount of matter exists both before and after the experiment.
112
In a chemical equation, (aq) means that an element or compound is
In an aqueous solution (in water)
113
We change the _________ to balance the equation.
Coefficients
114
What is a combination reaction?
When two or more substances react to form one product
A + B → C
115
What is a decomposition reaction?
When one substance breaks down into two or more substances
C → A + B
116
What is a combustion reaction?
A rapid reaction that produces a flame; these reactions most often involve hydrocarbons reacting with oxygen in the air.
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
117
What is the formula weight (for ionic compounds only)?
The sum of the atomic weights (in amu or g/mol) for the atoms in a chemical formula.
118
Atomic weight units
amu = g/mol
They are interchangeable units/measurements
119
What is the molecular weight?
The sum of the atomic weights of the atoms in a molecule (for nonmetals).
120
Percent Composition Equation
% (mass of an) Element = (number of atoms)(atomic weight of the atom) / (full weight of the compound) X 100
121
What is a empirical formula?
A formula that expresses the relative number of atoms in the smallest whole numbers possible
122
How do you find the molecular formula?
Molar mass of the molecular formula / molar mass of the empirical formula = #
You multiply the subscripts in the empirical formula by the #
123
What is the limiting reactant?
The reactant that will run out first, causing the reaction to stop.
124
What is the excess reactant?
The reactant that there will be some remaining of when the reaction stops as a result of the limiting factor running out.
125
What is the theoretical yield?
The maximum amount of product that can be made (the number we calculate using math); amount of product _predicted_ by the chemical equation.
126
What is the actual yield?
The amount of product one actually produces and measures (in a lab experiment for example); the amount of product _recovered_.
127
Equation for the percent yield
Percent yield = actual yield / theoretical yield X 100
128
What is a solution?
A homogeneous mixture of two or more pure substances.
129
What is a solvent?
The substances that dissolves the other substances and is present in the greatest abundance; usually water (aka the universal solvent)
130
What are the solutes?
The other substances that are dissolved in the solvent.
131
What is an aqueous solution?
A solution in which water is the solvent
132
How do ionic compounds dissolve in water?
By dissociation
133
What is dissociation?
Where water surrounds the separated ions
134
How do molecular compounds dissolve in water?
They interact with water, but most do NOT dissociate.
135
What is a polar covalent bond?
When electrons are shared unequally
For example, H2O. The water is slightly _negative_ on the oxygen side and _positive_ on the hydrogen side.
136
What dissolves polar solutes?
Polar solvents dissolve polar solutes
“Like dissolves like”.
137
What dissolves non-polar solutes?
Non-polar solvents dissolve non-polar solutes
“Like dissolves like”
138
What is hydration?
The binding of water to solutes
139
What is a “hydration shell”?
It is a result of hydration; it is when a molecule or ion is being surrounded by water molecules creating a “hydration shell”
140
What is an electrolyte?
A substance that dissociates into ions when dissolved in water; ionic compounds
141
What is a nonelectrolyte?
A substance that may dissolve in water, but it does not dissociate into ions when it does so; sugar, ethanol, etc.
142
What is a strong electrolyte?
An electrolyte that dissociates completely when dissolved in water
NaCl(s) → Na+(aq) + Cl-(aq)
Produce a lot of ions that can _conduct electricity_
143
What is a weak electrolyte?
An electrolyte that only dissociates partially when dissolved in water
CH3COOH ⇌ CH3COO- + H+
You have some of the reactant and a little bit of the product
144
What are the three groups of strong electrolytes?
Strong acids, strong bases, and most salts (ionic compounds)/(aq).
145
HCl
Hydrochloric acid
A **strong acid**
