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CHEM 110 > CHEM 110 - MIDTERM #1 > Flashcards

CHEM 110 - MIDTERM #1 Flashcards

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1
Q

What kind of science is Chemistry?

A

Central Science - it joins together all the sciences (physics & biology)

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2
Q

What is the scientific method?

A

Systematic approach to research (observation -> representation -> interpretation)

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3
Q

What is the difference between law and theory?

A

Law: concise statement of a relationship between phenomena that is always the same under the same conditions (F = ma)
Theory: unifying principle that explains a body of facts and/or those laws based on them (atomic theory)

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4
Q

Chemistry is the study of ______.

A

Matter

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5
Q

What is a substance?

A

Form of matter that has a definite composition and distinct properties (Ex: H2O)

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6
Q

What is a mixture?

A

Combination of 2 or more substances in which the substances retain their distinct identities

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7
Q

Difference between homogenous mixture & heterogenous mixture?

A

Homogenous mixture: mixture composition is the same throughout
Hetereogenous mixture: composition is not uniform throughout

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8
Q

What is are some examples of a homogenous mixture?

A

Air, Sea Water, Wine

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9
Q

What are some examples of heterogenous mixtures?

A

Chicken noodle soup, sand, oil & water

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10
Q

What is the physical means of separating a mixture?

A

Does not change the chemical composition of a substance (ie. distillation, ice melting, magnet)

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11
Q

What is the chemical means of separating a mixture?

A

Changing the chemical composition or identity of the substance(s) involved

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12
Q

An element cannot be separated into simpler substances by _______ means.

A

chemical

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13
Q

What is a compound?

A

A substance composed of atoms of two or more elements chemically united in fixed proportions

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14
Q

A compound can be separated into their pure elements by _____ means.

A

Chemical

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15
Q

What’s the difference between a mixture and a substance?

A

Mixture: combination of substances that can be separated by physical methods to form substances
Substances: form of matter with distinct properties composted of compounds and elements

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16
Q

Compounds can be separated via chemical methods to form ____.

A

Elements

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17
Q

3 States of Matter

A

Solid: dense shape
Liquid: more degrees of freedom
Gas: no shape, but occupy space all throughout

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18
Q

What is an example of chemical change?

A

Hydrogen burning in air to form water

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19
Q

What’s the difference between extensive and intensive properties?

A

Extensive: dependent on amount of matter
Intensive: does NOT dependent on matter

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20
Q

What are examples of extensive properties?

A

Mass, volume, length

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21
Q

What are examples of intensive properties?

A

Density, Color, Temperature

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22
Q

What is matter?

A

Anything that occupies space and has mass

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23
Q

What is weight?

A

Force that gravity exerts on an object

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24
Q

What SI unit measures the amount of substance?

A

Mole (mol)

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25
Q

Kilo-

A

1000 (10^3)

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26
Q

Milli-

A

1/1000 (10^-3)

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27
Q

Micro-

A

1/(10^6)

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28
Q

deci-

A

1/10 (10^-1)

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29
Q

centi-

A

1/100 (10^-2)

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30
Q

nano-

A

10^-9

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31
Q

mega-

A

10^6

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32
Q

pico-

A

10^-12

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33
Q

What is volume?

A

SI derived unit for volume is cubic meter (m^3) where 1 mL = 1 cm^3

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34
Q

What is density?

A

SI derived unit for density is kg/m^3
D = mass/volume

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35
Q

What are the units for density?

A

g/mL or g/cm^3

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36
Q

How do we find Kelvin (K) from using Celsius?

A

K = C + 273.15

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37
Q

What is 0 Celsius in Kelvin?

A

273.15

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38
Q

How do we find the degrees in Fahrenheit?

A

F = 9/5 x C + 32

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39
Q

What is scientific notation?

A

A convenient way of showing the # of significant figures in a value

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40
Q

When you multiply you ___ exponents.

A

add

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41
Q

When you divide exponents, you ___ exponents.

A

subtract

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42
Q

What are significant figures?

A

Any digit that is not zero ~ provides uncertainty and accuracy of a measurement

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43
Q

What is the rule for addition/subtraction with # of sig figs?

A

The answer cannot have more digits to the right of the decimal point than any of the original numbers (83.3333 + 1.1 = 90.4)

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44
Q

What is the rule for multiplication/division of sig figs?

A

The # of sig figs must be set by the original number that has the smallest number of sig figs (4.51 + 8.7777777 = 16.6)

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45
Q

What is the difference between accuracy and precision?

A

Accuracy: how close a measurement is to the true value
Precision: how close a set of measurements are to each other

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46
Q

Give an example of a compound

A

Sugar, water

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47
Q

Water boiling is an example of ___ change

A

physical

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48
Q

fertilizers help to increase agricultural production is an example of ____ change

A

chemical

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49
Q

the flashlight beam slowly gets dimmer and finally goes out is an example of ___ change

A

chemical

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50
Q

What is Dalton’s Atomic Theory?

A

1) Elements are composed of atoms
2) All atoms of an element are identical, have same size, mass and chemical properties
3) Compounds are composed of atoms of more than one element
4)A chemical reaction is the rearrangement of atoms (not creation or destruction - law of conservation of mass)

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51
Q

What is the law of conservation of mass?

A

Mass is not created or destroyed

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52
Q

What is Dalton’s Law of Multiple Proportions?

A

If 2 elements form more than one compound - the ratio of the masses of the 2nd element can be reduced to whole numbers

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53
Q

What was the finding of Rutherford’s Experiment (1908)?

A

1) Atoms positive charge is concentrated in the nucleus
2) Protons have an opposite charge (+) of an electron (-)
3) Mass of a proton = 1840 x mass of e- (1.67 x 10^-24 g) = protons are bigger than electrons

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54
Q

What is the atomic number (Z)?

A

number of protons in a nucleus and determines the identity of an element

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55
Q

What is the mass number (A)?

A

number of protons + neutrons

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56
Q

What are isotopes?

A

Atoms of the element with different numbers of neutrons in their nuclei

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57
Q

What is the first group and respective charge in the period table?

A

Alkali Metals (+1)

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58
Q

What is the second group of the periodic table with their respective charge?

A

Alkaline Earth Metals (+2)

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59
Q

What is the name of the 3rd-12th group in the periodic table?

A

Transition metals (varying charges)

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60
Q

What is the name of the 7th group of the periodic table and their respective charges?

A

Halogens (-1)

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61
Q

What is the name of the last group of the periodic table?

A

Noble gases

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62
Q

What is the difference between a period and a group?

A

period = row in the periodic table
group = column in the periodic table

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63
Q

What is a molecule?

A

Aggregate of 2 or more atoms held by chemical forces

64
Q

What is an example of a diatomic molecule?

A

N2, H2, CO, HCl (2 atoms)

65
Q

What is an example of a polyatomic molecule?

A

O3, CH4 (more than 2 atoms)

66
Q

What is an ion?

A

Atom(s) with a net positive or negative charge

67
Q

What are the two types of ions?

A

Anion and cation

68
Q

What is the difference between cation and anions?

A

Cation: net positive charge (lose an electron)
Anion: net negative charge (gain an electron)

69
Q

What is an example of a monatomic ion?

A

Na+, Cl-

70
Q

What are the two types of formulas and what are their differences?

A

Molecular (exact number of atoms of each element in the smallest unit of a substance) & empirical (simplest whole number ratio of atoms in a substance)

71
Q

An example of molecular and empirical formula

A

C6H12O6 (molecular)
CH2O (empirical)

72
Q

What are ionic compounds held together by?

A

Electrostatic forces (+) and (-) charges

73
Q

Ionic compounds are generally formed with a ____ and ____

A

metal, nonmetal

74
Q

What is an example of an ionic compound?

A

Na+Cl-

75
Q

What is the chemical nomenclature of ionic compounds?

A

The anion (nonmetal), add “‘-ide” to element name

76
Q

What is the chemical name for K2O?

A

Potassium oxide

77
Q

How do we name transition metal ionic compounds?

A

Indicate the charge on metal with roman numerals

78
Q

How do we name FeCl2?

A

Iron (II) chloride

79
Q

Name Monatomic Atom for S?

A

Sulfide

80
Q

Name Monatomic Atom for N?

A

Nitride

81
Q

Name Monatomic Atom for P?

A

Phosphide

82
Q

What is an inorganic cation?

A

NH4 (ammonium)

83
Q

Cu(NO3)2 name?

A

Copper (II) nitrate

84
Q

KH2PO4 name?

A

Potassium dihydrogen phosphate

85
Q

Calcium phosphate formula?

A

Ca3(PO4)2

86
Q

What do molecular compounds consist of?

A

Nonmetals/nonmetals + metalloids
(they are held together by covalent bonds and made up of discrete, individual molecules)

87
Q

Common molecular compound?

A

H2O, CH4, NH3

88
Q

____ compounds use Greek prefixes & the last element ends in ___ for chemical nomenclature

A

Molecular, -ide

89
Q

1

A

Mono-

90
Q

2

A

Di-

91
Q

3

A

Tri-

92
Q

4

A

Tetra-

93
Q

5

A

Penta-

94
Q

6

A

Hexa-

95
Q

7

A

Hepta

96
Q

9

A

Nona-

97
Q

Deca-

A

10

98
Q

NF3 name?

A

Nitrogen trifluoride

99
Q

N2O name?

A

dinitrogen monoxide

100
Q

SiCl4 name?

A

Silicon tetrachloride

101
Q

P4O10 name?

A

Tetraphosphorus Decoxide

102
Q

What is an acid?

A

Substance that yields H+ ions when dissolved in water

103
Q

HF name?

A

hydrofluoric acid

104
Q

HCl name?

A

Hydrochloric acid

105
Q

HBr name?

A

Hydrobromic acid

106
Q

HI name?

A

hydroiodic acid

107
Q

HCN name?

A

hydrocyanic acid

108
Q

H2S name?

A

Hydrosulfuric acid

109
Q

What is an oxoacid?

A

An acid that contains hydrogen, oxygen, and another element

110
Q

Examples of oxoacids?

A

Nitric acid (HNO3), Carbonic Acid (H2CO3), Phosphoric acid (H3PO4)

111
Q

H2SO4 name?

A

Sulfuric acid (Oxoacid)

112
Q

HClO3- name?

A

Chloric Acid (Oxoacid)

113
Q

Naming Oxoanions?

A

1) Anion ends in “-ate” when the H ions are removed from the “ic” acid
2) Anion ends in “ite” when the H ions are removed from the “-ous” acid
3) Number of H atoms present are indicated with anion names (dihydrogen phosphate H2PO4)

114
Q

HClO4 name?

A

Perchloric acid

115
Q

HClO3 name?

A

Chloric acid

116
Q

HClO2 name?

A

Chlorous acid

117
Q

HClO name?

A

Hypochlorous acid

118
Q

Why does the nomenclature vary with perchloric acid, chloric acid, chlorous acid and hypochlorous acid?

A

of oxygens vary, corresponding anion vary

119
Q

H3PO3 name?

A

Phosphorous acid

120
Q

HIO4 name?

A

Periodate

121
Q

What is a base?

A

A substance that yields hydroxide ions (-OH) when dissolved in water

122
Q

NaOH name and ID?

A

Sodium hydroxide, base

123
Q

What is a hydrate?

A

A compound that has a specific number of water molecules attached to them

124
Q

LiCl x H2O name and ID?

A

Lithium chloride monohydrate

125
Q

BaCl2 x 2H2O name and ID?

A

Barium chloride dihydrate

126
Q

H2O name?

A

dihydrogen monoxide

127
Q

CaO name?

A

Calcium oxide

128
Q

Simplest type of organic compound?

A

Hydrocarbon

129
Q

Protons and neutrons are ____ than electrons

A

larger in mass (same with each other)

130
Q

Mg(HCO3)2 name?

A

Magnesium bicarbonate

131
Q

HBrO4 name?

A

Perbromic acid

132
Q

HrBrO3 name?

A

Bromic acid

133
Q

HBrO2 name?

A

Bromous acid

134
Q

HBrO name?

A

Hypobromous acid

135
Q

HIO4 name

A

Periodic acid

136
Q

HIO3 name

A

Iodic acid

137
Q

HIO2 name

A

Iodous acid

138
Q

HIO name

A

Hypoiodous acid

139
Q

H2SO3 name

A

Sulfurous acid

140
Q

HNO3 name

A

Nitric acid

141
Q

HNO2 name

A

Nitrous acid

142
Q

H3PO4 name

A

Phosphoric acid

143
Q

H3PO3

A

phosphorous acid

144
Q

What is atomic mass?

A

The mass of an atom in atomic mass units (1 atom C = 12 amu)

145
Q

What is average atomic mass?

A

Weighted average of all naturally occurring isotopes of the element (based on relative abundance)

To solve:
1) Convert percentage given of isotope into a decimal (60.0% -> 0.600)
2) Multiply decimal by amount of grams given of isotope
3) Add the atomic masses (products) together to find the average within the element

146
Q

What is a mole?

A

A unit to count number of particles - contains as many elementary entities as there are atoms in exactly 12 grams of 12C

147
Q

Avogadro’s number is used to find the number of ____ of a compound/element

A

atoms/particles

148
Q

What is molar mass?

A

Mass of 1 mole of anything in grams

149
Q

How do we convert from mass to atoms of an element?

A

Mass (g) –> Molar mass –> Moles –> Avogadro’s number–> Atoms

150
Q

What is the molecular mass (molecular weight)?

A

Sum of the atomic masses (in amu) in a molecule

151
Q

What is the formula mass?

A

Sum of atomic masses (in amu) in a formula unit of an ionic compound

152
Q

What is the percent composition and how do we calculate it?

A

The amount of an element in a compound; calculated by:
1) Find the atomic mass of the element with respect to its coefficient in the equation
2) Divide atomic mass by the molar mass of the compound
3) Multiply the product by 100 to find the percentage

153
Q

How would we find the empirical formula given the percent composition?

A

1) Convert the percent given into grams of an element (40.0% -> 40.0 grams of C)
2) Use the grams to find number of moles (by dividing by molar mass of compound)
3) Identify the smallest amount of moles and divide the other products by the smallest number to find a smallest compound ratio
4) If needed to achieve a whole number, multiply all the products by a common integer to achieve a whole number
5) Write out empirical formula with the subscripts :)

154
Q

We cannot use the ____ to read a chemical reaction. Only moles and molecules

A

Mass (g)

155
Q

Stoichiometric coefficients are consist with ____, not ____.

A

moles, grams

156
Q

What is the limiting reagent?

A

The reactant used up first in the reaction

CHEM 110 (4 decks)

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