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Chemistry 121 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

Define chemistry

A

study of matter & how the properties are related to its composition

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2
Q

Define matter

A

has mass & occupies space

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3
Q

Define mass

A

amount of matter

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4
Q

Formula for mass in outer space

A

F=ma or m=f/a

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5
Q

4 fundamental forces

A

Gravitational, electromagnetic, strong & weak nucles

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6
Q

Define weight

A

m*a due to g

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7
Q

Force of attraction by the earth

A

F=(m)(a) or W=(m)(g)

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8
Q

Examples of why chemistry is critical in modern society

A

Electronics, materials, medical, personal & home care products, energy

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9
Q

Force of gravity on earth

A

9.8 m/s^2 at sea level

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10
Q

Force of gravity on the moon

A

1.7 m/s^2

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11
Q

Consequences of chemistry

A

Pollution, global warming, warfare, accidents

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12
Q

How much has the earth’s temp risen in the past century

A

1.5 degrees F

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13
Q

How many tons of CO2 per person from fossil fuel consumption

A

10 tons

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14
Q

Average temp of earth’s atmosphere with greenhouse gases vs without

A

With: 57 degrees F
Without: 0 degrees F

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15
Q

Sources of CO2 emission from largest to smallest percentage

A

Electricity production, cars & trucks, industry, residential heating

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16
Q

Gases contributing to global warming from largest to smalles

A

CO2, CFCs, CH4, N2O

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17
Q

Protocol that did not get put in place but would have lowered CO2 emissions dramatically

A

Kiota protocol

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18
Q

Regions of earth’s atmosphere lowest to highest

A

Troposphere, stratosphere, mesosphere, thermosphere

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19
Q

CO2 absorbs what

A

infrared radiation

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20
Q

Concentration of CO2 has risen by what percent in the past century

A

43%

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21
Q

Scientists predict the earth temperature will rise by how much in 2100

A

4-9 degrees F

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22
Q

1 CFC molecule can destroy how many ozone molecules

A

1,000s

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23
Q

Define ozone

A

elemental oxygen (O3)

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24
Q

Ozone shields us from what

A

harmful ultraviolet radiation

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25
Q

Consequences of ozone depletion

A

increased skin cancers, crop damage, cataracts

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26
Q

Define law

A

verbal statement or mathematical equation that summarizes observations & experiments (shows physical relationship, not explanation of nature)

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27
Q

Newton’s universal law of gravity

A

Gravitational force=F=(Gm1m2)/(r^2)

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28
Q

Universal gravitational force constant

A

6.67010^-11Nm^2/kg^2

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29
Q

Earth’s mass is

A

6*10^24 kg

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30
Q

Define theory

A

Hypothesis that repeatedly withstands the test of experiments & has overwhelming supportive evidence

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31
Q

Define substance

A

Matter with a definite/constant composition & distinct properties

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32
Q

Examples of physical properties

A

Melting/boiling points, density, mass, volume, color, shape

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33
Q

Examples of chemical properties

A

All chemical reactions (composition/decomposition)

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34
Q

Define extensive properties

A

Value depends on quantity of matter

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35
Q

Examples of extensive properties

A

Mass, volume, heat

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36
Q

Define intensive properties

A

Value does not depend on the quantity of matter

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37
Q

Examples of intensive properties

A

Melting/boiling point, density, temp

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38
Q

Combination reaction to form table salt is surprisingly a very

A

Violent reaction

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39
Q

Examples of quantitative measurements

A

Length, mass, time, temp

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40
Q

SI base unit for length

A

meter, m

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41
Q

SI base unit for mass

A

kilogram, kg

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42
Q

SI base unit for time

A

second, s

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43
Q

SI base unit for temp

A

kelvin, K

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44
Q

SI base unit for amount of a substance

A

mole, mol

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45
Q

Metric system first started by who

A

France

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46
Q

giga

A

G, 10^9

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47
Q

mega

A

M, 10^6

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48
Q

kilo

A

k, 10^3

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49
Q

deci

A

d, 10^-1

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50
Q

centi

A

c, 10^-2

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51
Q

milli

A

m, 10^-3

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52
Q

micro

A

μ, 10^-6

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53
Q

nano

A

n, 10^-9

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54
Q

pico

A

p, 10^-12

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55
Q

femto

A

f, 10^-15

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56
Q

Greek prefixes used when

A

value is larger than the base (kilo, mega, giga)

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57
Q

Latin prefixes used when

A

value is smaller than the base (centi, milli, micro)

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58
Q

Derived unit examples

A

Volume (length)^3, area (length)^2, speed (distance/time), acceleration (distance/time^2), energy, force

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59
Q

Volume unit 1m^3=

A

110^6cm^3 or 110^3dm^3

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60
Q

Volume unit 1dm^3=

A

1 liter

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61
Q

Volume 1L=

A

1000mL or 1000cm^3

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62
Q

Volume 1mL=

A

1cm^3

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63
Q

Dimensional analysis involves

A

Conversion factors

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64
Q

Celsius scale based on

A

Water boils at 100 degrees C & freezes at 0 degrees C (Anders Celsius)

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65
Q

Define temp

A

Direction of heat flow, average kinetic energy

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66
Q

Fahrenheit scale based on

A

Salt saturated water freezes at 0 degrees F & 100 degrees F was normal body temp (Gabriel Fahrenheit)

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67
Q

Pure water boils & freezes at what degree F

A

Boils 212 degrees F, freezes 32 degrees F

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68
Q

Convert degrees C to degrees F

A

(9F/5C)tC+32F

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69
Q

Convert degrees F to degrees C

A

(tF-32F)(5C/9F)

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70
Q

Define heat

A

total kinetic energy

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71
Q

Convert C to K

A

Tk=tC+273.15

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72
Q

Substances can be either

A

elements or compounds

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73
Q

Define element

A

Substance that cannot be decomposed into simpler substances by chemical means

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74
Q

How man elements

A

Roughly 115, 82 natural

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75
Q

Sodium latin name

A

Natrium (Na)

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76
Q

Potassium latin name

A

Kalium (K)

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77
Q

Iron latin name

A

Ferrum (Fe)

78
Q

Tin latin name

A

Stannum (Sn)

79
Q

Lead latin name

A

Plumbum (Pb)

80
Q

Silver latin name

A

Argentum (Ag)

81
Q

Copper latin name

A

Cuprum (Cu)

82
Q

Define mixture

A

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

83
Q

Mixtures have variable elemental composition while a pure substance has a

A

Definite composition

84
Q

Define compound

A

Substance composed of 2 or more elements combined in a fixed proportion

85
Q

Homogeneous mixture also called a

A

Solution

86
Q

Ways to separate mixtures

A

Distillation, filtration, chromatagrophy

87
Q

Law of definite proportions

A

(Proust) Compound always contains elements combined in the same proportion by mass

88
Q

Dalton’s atomic theory, 5 parts

A

1) matter composed of tiny particles (atoms) 2) all atoms of an element are identical in mass & their properties 3) Atoms of different elements differ in mass & other properties 4) compounds are composed of different elements combined in fixed proportions by mass 5) atoms are indestructable

89
Q

Who created the atomic theory

A

John Dalton

90
Q

Most renowned scientist of his time, late 1700s, early 1800s

A

Sir Humphrey Davy

91
Q

Why wasn’t Dalton’s atomic theory accepted at first

A

Cocky Sir Humphrey Davy didn’t agree with it

92
Q

Law of multiple proportions

A

2 elements combine to form 1+ compounds, masses of 1 element that combine with a fixed mass of the other element are in ratios of small whole numbers (predicted by Dalton’s atomic theory)

93
Q

Define atom

A

smallest particle of an element which retains the chemical properties of that element

94
Q

Discovery of the first subatomic particle was made by using what

A

Crookes tube

95
Q

Tool that causes gases to glow & yield a bright spot when it strikes a fluorescent screen

A

Cathode ray tube

96
Q

Scientist that found out that magnetic & electrical fields bend cathode rays

A

JJ ThOmpson

97
Q

Cathode ray experiments suggested that Cathode rays are a basic component of all matter. Why?

A

Same properties regardless of metal used

98
Q

What are cathode rays really

A

Beam of electrons

99
Q

Whats a coulumb

A

Unit of electric charge

100
Q

Robert Millikan designed what experiment which determined the charge of an electron

A

Oil drop experiment

101
Q

Rontgen used cathode rays and discovered that some rays could pass through matter, he dubbed them what

A

X rays

102
Q

Becquerel found that some compounds emitted rays spontaneously without cathode ray stimulation. This suggested what

A

Radioactivity

103
Q

Women who was unable to speak after winning a Nobel Prize in physics for helping to discover radioactivity

A

Marie Curie

104
Q

Three types of radioactivity named by Ernest Rutherford

A

Alpha, beta, & gamma rays

105
Q

Beam of positively charged particles, helium nuclei

A

Alpha rays

106
Q

Beam of negatively charged particles, electrons

A

Beta rays

107
Q

High energy radiation, no charge, does not consist of particles, similar to x rays

A

Gamma rays

108
Q

JJ ThOmpson created what model for the atom where the atom is mainly composed of protons with some electrons embedded randomly throughout

A

Plum Pudding model

109
Q

Ernest Rutherford with Geiger & Marsden studied scattering a beam of alpha particles by a thin gold foil, what were they surprised about

A

Some alpha particles had large scattering angles, a few even bounced back

110
Q

Rutherford’s new model of the atom, 2 distinct parts. Called the nuclear model for the atom

A

1) dense central core (nucleus), + charge 2) negatively charged electrons surround the nucleus & are far removed from the nucleus

111
Q

Protons discovered by who

A

Rutherford

112
Q

Neutrons discovered by who

A

James Chadwick

113
Q

Magnitude charge of protons & electrons

A

P: +1.60*10^-19C E: same, but -

114
Q

Mass of an atom

A

1*10^-23g

115
Q

Diameter of an atom

A

1*10^-10m

116
Q

Diameter of the nucleus

A

1*10^-14m

117
Q

Henry Moseley discovered that the number of what characterizes an element

A

Protons

118
Q

Letter representing atomic number (# of protons)

A

Z

119
Q

Letter representing mass number (# of protons + neutrons)

A

A

120
Q

Define isotope

A

Same element with different mass #’s

121
Q

Nucleus of a specific isotope called a

A

nuclide

122
Q

Cobalt 60 used for

A

Cancer radiation therapy

123
Q

Cesium 137 used for

A

Food sterilization

124
Q

Iodine 129 used for

A

Thyroid radiation therapy

125
Q

Technetium 99 used for

A

Medical imaging of internal organs

126
Q

Scientist who discovered isotopes

A

JJ ThOmpson

127
Q

2 in Dalton’s theory changed to what after isotopes were discovered

A

2) All atoms of a given element have the same number of protons & chemical properties

128
Q

Mendeleev & Meyer arranged elements by increasing atomic number in what kinds of a row

A

horizantal

129
Q

Elements with similar chemical properties are arranged in columns called

A

groups

130
Q

Metals are located left & center of the periodic table, they have what properties

A

good conductors of heat & electricity, luster, ductile, malleable, solid at room temp (except mercury)

131
Q

Nonmetals are located to right of the periodic table, they have what properties

A

poor conductors of heat & electricity, solids are brittle, dull surface

132
Q

Metalloids located to the right & center of the periodic table, divide nonmetals & metals, properties are

A

intermediate between metals & nonmetals

133
Q

Group A elements are called main group elements or

A

representative elements

134
Q

Group B elements are called

A

transition elements

135
Q

Two rows below table are called what, broken down into lanthanide & actinide elements

A

inner transition elements

136
Q

Group 1A called

A

alkali metals (except hydrogen)

137
Q

Group 2A called

A

alkaline earth metals

138
Q

Group 6A called

A

chalcogens

139
Q

Group 7A called

A

halogens

140
Q

Group 8A called

A

noble (rare) gases

141
Q

What are the only elements that exist in nature as free, single atoms

A

Group 8A, the noble gases

142
Q

Atoms combine in what two ways

A

1) sharing electrons- forms molecules, 2) transferring electrons- forms ionic compounds

143
Q

When nonmetals form with nonmetals or metalloids, this forms. Definite shape, constant composition applies, all are neutral

A

molecules

144
Q

Different forms of an element are called

A

allotropes

145
Q

Composed of two or more different nonmetals or metalloids

A

molecular compounds

146
Q

Chemical formula denoting the exact number of atoms of each element in a molecule

A

molecular formula

147
Q

Gives the simplest whole number ratio of atoms of each element in the compound

A

empirical formula (C6H6 becomes CH, C2H4 becomes CH2, CH4 stays the same)

148
Q

Shows which atoms are connected together

A

structural formulas

149
Q

Species containing a net charge either by gaining electrons or losing electrons

A

ions

150
Q

A cation is a positively charged ion that is attracted to a negative what in an electrolyte cell

A

cathode

151
Q

An anion is a negatively charged ion that is attracted to a positive what in an electrolyte cell

A

anode

152
Q

Metals tend to what

A

lose electrons- cations

153
Q

Nonmetals tend to what

A

gain electrons- anions

154
Q

Ions with only one atom are called what

A

monatomic ions

155
Q

Are monatomic metal ions formed by losing or gaining electrons

A

losing

156
Q

Are monatomic nonmetal ions formed by losing or gaining electrons

A

gaining

157
Q

Predicting charges for stable monatomic ions in Group 1A or 2A

A

of electrons the metal atoms lose is equal to the group #

158
Q

Predicting charges for the number of electrons that a nonmetal atom gains is

A

Group 7A: gain 1 electron to form X- ions, Group 6A: gain 2 electrons to form X2- ions, Group 5A: gain 3 electrons to form X3- ions

159
Q

Ions that consist of atoms chemically bonded together in a molecular sense & carry a net charge

A

polyatomic ions

160
Q

These are composed of cations & anions interacting in appropriate proportions to yield an overall neutral compound, forms a crystal lattice structure

A

ionic compounds

161
Q

Chemical formulas of ionic compounds are always represented in which fashion

A

empirical formula

162
Q

Formulas for ionic compounds

A

1) always neutral, 2) cation written first, then anion, 3) subscripts denote # of ions in each type required to yield a neutral compound (formula unit)

163
Q

For charge balance of ionic compounds, the subscript of the cation is equal to the charge on the anion, the subscript of the anion is equal to the charge of the

A

Cation (Na+ + CO3^2- turns into Na2CO3)

164
Q

How do you name ionic compounds

A

Cation first, anion second

165
Q

Transition metal ions can form stable ions with variable changes, you use what to name them

A

stock system, written as element name (charge) ion

166
Q

Naming polyatomic cations

A

name ends in -ium, + cation (ex: ammonium ion)

167
Q

Naming monatomic nonmetal anions

A

name derived from stem of element followed by -ide plus ion

168
Q

Naming polyatomic anions

A

many contain O2 & have suffixes ate & ite

169
Q

OH-

A

hydroxide ion

170
Q

CN-

A

cyanide ion

171
Q

O2^2-

A

peroxide ion

172
Q

CO3^2-

A

carbonate ion

173
Q

HcO3^-

A

hydrogen carbonate ion

174
Q

MnO4^-

A

permanganate ion

175
Q

CrO4^2-

A

chromate ion

176
Q

Cr2O7^2-

A

dichromate ion

177
Q

PO4^3-

A

phosphate ion

178
Q

SCN-

A

thiocyanate ion

179
Q

C2H3O2-

A

acetate ion

180
Q

NO2-

A

nitrite ion

181
Q

NO3-

A

nitrate ion

182
Q

SO3^2-

A

sulfite ion

183
Q

SO4^2-

A

sulfate ion

184
Q

ClO2-

A

chlorite ion

185
Q

ClO3-

A

chlorate ion

186
Q

Oxoanions are used for a homologous series with the same central atom w/ a variable number of oxygen atoms, when do you use what suffix

A

ite suffix (less oxygen), ate suffix (more oxygen). If more than two in series, hypo prefix (even less oxygen than ite) or per (even more oxygen than ate)

187
Q

Naming ionic compounds

A

Cation named first, then anion, anion not used in name

188
Q

Transition metal ionic compounds specify the charge by using what

A

stock system

189
Q

Acids are compounds that yield hydronium ions when dissolved in water, named how

A

acids based on anions whose name ends in -ide, add hydro and change -ide to -ic acid. acids from oxoanions, change the suffix…-ate suffix to -ic acid, for -ite suffix change to -ous acid

190
Q

Binary molecular compounds contain only 2 elements, name them how

A

name first as the element & second as an anion, use greek prefixes to specify the # of each element, when prefix ends in a or o & the anion name begins with a vowel, then a or o of prefix is often omitted. Acids whose anion ends in ide, if they aren’t in water they are named as molecular compounds

191
Q

Hydrates are compounds with a specific number of water molecules that are what

A

strongly adhered

Chemistry 121 (5 decks)

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