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CHE 111 > Chemistry Ionic Compounds and Formulas > Flashcards

Chemistry Ionic Compounds and Formulas Flashcards

1
Q

Sulfate

A

SO42-

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2
Q

Phosphate

A

PO43-

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3
Q

Chlorate

A

ClO3-

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4
Q

Carbonate

A

CO32-

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5
Q

Hydroxide

A

OH-

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6
Q

Hydride

A

H-

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7
Q

Silver ion

A

Ag+

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8
Q

Zinc ion

A

Zn2+

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9
Q

Peroxide

A

O22-

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10
Q

Chromate

A

CrO42-

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11
Q

Dichromate

A

Cr2O72-

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12
Q

Permanganate

A

MnO4-

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13
Q

Cyanide

A

CN-

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14
Q

Acetate

A

CH3COO-

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15
Q

Nitrate

A

NO3-

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16
Q

Ammonium

A

NH4+

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17
Q

Mono-

A

1

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18
Q

Di-

A

2

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19
Q

Tri-

A

3

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20
Q

Tetra-

A

4

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21
Q

Penta-

A

5

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22
Q

Hexa-

A

6

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23
Q

Hepta-

A

7

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24
Q

Octa-

A

8

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25
Q

Nona

A

9

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26
Q

Deca-

A

10

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27
Q

To name an acid for an anion that ends in -ide, replace -ide with _____.

A

Hydro- -ic acid

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28
Q

To name an acid for an anion that ends in -ite, replace -ite with _____.

A

-ous acid

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29
Q

To name an acid for an anion that ends in -ate, replace -ate with _____.

A

-ic acid

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30
Q

Molecular compounds are formed between

A

Nonmetals

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31
Q

Ionic compounds are formed between

A

Metals and nonmetals

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32
Q

Perchlorate

A

ClO4-

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33
Q

Chlorite

A

ClO2-

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34
Q

Hypochlorite

A

ClO-

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35
Q

Chloride

A

Cl-

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36
Q

Bromate

A

BrO3-

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37
Q

Bromide

A

Br-

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38
Q

Iodide

A

I-

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39
Q

Sulfide

A

S2-

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40
Q

Density equation

A

D=m/V

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41
Q

Percent error equation

A

% error = 100|(observed value - expected value)|/expected value

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42
Q

Group 1A Name

A

Alkali metals

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43
Q

Group 1A Charge

A

1+

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44
Q

Group 2A Name

A

Alkaline earth metals

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45
Q

Group 2A Charge

A

2+

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46
Q

Group 3A Charge

A

3+

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47
Q

Group 5A Charge

A

3-

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48
Q

Group 6A Name

A

Chalcogens

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49
Q

Group 6A Charge

A

2-

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50
Q

Group 7A Name

A

Halogens

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51
Q

Group 7A Charge

A

1-

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52
Q

Group 8A Name

A

Noble Gases

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53
Q

Group 8A Charge

A

No charge

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54
Q

Cm3

A

1 mL

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55
Q

Phosphite

A

PO33-

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56
Q

What are the 3 parts to the scientific method in the order they occur?

A
  1. Observation
  2. Hypothesis
  3. Test
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57
Q

Concentration1Volume1 = Concentration2Volume2

A

C1V1 = C2V2

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58
Q

Molar mass equation

A

g/mol

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59
Q

Avogadro’s number

A

1 mole (mol) = 6.022 X 1023

60
Q

Fe

A

Iron

61
Q

K

A

Potassium

62
Q

Ti

A

Titanium

63
Q

S

A

Sulfur

64
Q

U

A

Uranium

65
Q

Sn

A

Tin

66
Q

Au

A

Gold

67
Q

Ag

A

Silver

68
Q

Na

A

Sodium

69
Q

P

A

Phosphorus

70
Q

Cu

A

Copper

71
Q

Pb

A

Lead

72
Q

Mg

A

Magnesium

73
Q

Hg

A

Mercury

74
Q

The variable that the experimenter changes or manipulates

A

The independent variable

75
Q

The variable that is effected and responds to the independent variable; the variable you measure

A

The dependent variable

76
Q

The variables that are held constant

A

The control variable

77
Q

The variable that goes on the X-axis

A

The independent variable

78
Q

The variable that goes on the Y-axis

A

The dependent variable

79
Q

Mixtures that vary in composition throughout a sample

A

Heterogeneous mixtures

80
Q

Mixtures that have the same composition throughout the sample

A

Homogeneous mixtures

81
Q

Properties that can be observed without changing a substance

A

Physical properties

82
Q

Examples of physical properties

A

Boiling point, density, mass, or volume

83
Q

Properties that can only be observed when a substance is changed into another substance

A

Chemical properties

84
Q

Examples of chemical properties

A

Flammability, corrosiveness (breakdown), or reactivitiy with acid(s) (changes it into something else)

85
Q

Properties that are independent of the amount of the substance that is present

A

Intensive properties

86
Q

Examples of intensive properties

A

Density (as long as substances are in the same state of matter), boiling point, or color

87
Q

Properties that depend upon the amount of the substance present

A

Extensive properties

88
Q

Examples of extensive properties

A

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
Q

Changes in matter that do not change the composition of a substance

A

Physical changes

90
Q

Examples of physical changes

A

Changes of state of matter, temperature, and volume

91
Q

Changes that result in new substances

A

Chemical changes

92
Q

Examples of chemical changes

A

Combustion, oxidation, redox (iron rusting), and decomposition

93
Q

Giga-

A

Abbreviation: G
1Gm = 109m

94
Q

Mega-

A

Abbreviation: M
1Mm = 106m

95
Q

Kilo-

A

Abbreviation: K
1Km = 1000m

96
Q

Deci-

A

Abbreviation: d
10dm = 1m

97
Q

Centi-

A

Abbreviation: c
100cm = 1m

98
Q

Milli-

A

Abbreviation: m
1000mm = 1m

99
Q

Micro-

A

Abbreviation: μ
1μm = 10-6m

100
Q

Nano-

A

Abbreviation: n
1nm = 10-9m

101
Q

Mass unit

A

g (grams)

102
Q

Volume unit

A

mL or cm3

103
Q

The freezing point of water

A

0°C

104
Q

The boiling point of water

A

100°C

105
Q

__________ refers to the proximity of a measurement to the true value of a quantity.

A

Accuracy

106
Q

__________ refers to the proximity of several measurements to each other.

A

Precision

107
Q

What are the significant figure rules?

A
  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
Q

When you multiply or divide, the answer is rounded to the number of digits that corresponds to the _______________.

A

Least number of significant figures

109
Q

When addition or subtraction is performed, answers are __________________.

A

Rounded to the least significant decimal place

110
Q

What is stoichiometry?

A

The area of study that examines the quantities of substances consumed and produced in chemical reactions.

111
Q

What does the Law of Conservation of Mass state?

A

An equal amount of matter exists both before and after the experiment.

112
Q

In a chemical equation, (aq) means that an element or compound is

A

In an aqueous solution (in water)

113
Q

We change the _________ to balance the equation.

A

Coefficients

114
Q

What is a combination reaction?

A

When two or more substances react to form one product
A + B → C

115
Q

What is a decomposition reaction?

A

When one substance breaks down into two or more substances
C → A + B

116
Q

What is a combustion reaction?

A

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
Q

What is the formula weight (for ionic compounds only)?

A

The sum of the atomic weights (in amu or g/mol) for the atoms in a chemical formula.

118
Q

Atomic weight units

A

amu = g/mol
They are interchangeable units/measurements

119
Q

What is the molecular weight?

A

The sum of the atomic weights of the atoms in a molecule (for nonmetals).

120
Q

Percent Composition Equation

A

% (mass of an) Element = (number of atoms)(atomic weight of the atom) / (full weight of the compound) X 100

121
Q

What is a empirical formula?

A

A formula that expresses the relative number of atoms in the smallest whole numbers possible

122
Q

How do you find the molecular formula?

A

Molar mass of the molecular formula / molar mass of the empirical formula = #
You multiply the subscripts in the empirical formula by the #

123
Q

What is the limiting reactant?

A

The reactant that will run out first, causing the reaction to stop.

124
Q

What is the excess reactant?

A

The reactant that there will be some remaining of when the reaction stops as a result of the limiting factor running out.

125
Q

What is the theoretical yield?

A

The maximum amount of product that can be made (the number we calculate using math); amount of product predicted by the chemical equation.

126
Q

What is the actual yield?

A

The amount of product one actually produces and measures (in a lab experiment for example); the amount of product recovered.

127
Q

Equation for the percent yield

A

Percent yield = actual yield / theoretical yield X 100

128
Q

What is a solution?

A

A homogeneous mixture of two or more pure substances.

129
Q

What is a solvent?

A

The substances that dissolves the other substances and is present in the greatest abundance; usually water (aka the universal solvent)

130
Q

What are the solutes?

A

The other substances that are dissolved in the solvent.

131
Q

What is an aqueous solution?

A

A solution in which water is the solvent

132
Q

How do ionic compounds dissolve in water?

A

By dissociation

133
Q

What is dissociation?

A

Where water surrounds the separated ions

134
Q

How do molecular compounds dissolve in water?

A

They interact with water, but most do NOT dissociate.

135
Q

What is a polar covalent bond?

A

When electrons are shared unequally
For example, H2O. The water is slightly negative on the oxygen side and positive on the hydrogen side.

136
Q

What dissolves polar solutes?

A

Polar solvents dissolve polar solutes
“Like dissolves like”.

137
Q

What dissolves non-polar solutes?

A

Non-polar solvents dissolve non-polar solutes
“Like dissolves like”

138
Q

What is hydration?

A

The binding of water to solutes

139
Q

What is a “hydration shell”?

A

It is a result of hydration; it is when a molecule or ion is being surrounded by water molecules creating a “hydration shell”

140
Q

What is an electrolyte?

A

A substance that dissociates into ions when dissolved in water; ionic compounds

141
Q

What is a nonelectrolyte?

A

A substance that may dissolve in water, but it does not dissociate into ions when it does so; sugar, ethanol, etc.

142
Q

What is a strong electrolyte?

A

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
Q

What is a weak electrolyte?

A

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
Q

What are the three groups of strong electrolytes?

A

Strong acids, strong bases, and most salts (ionic compounds)/(aq).

145
Q

HCl

A

Hydrochloric acid
A strong acid

CHE 111 (2 decks)

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