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AP Chem > Summer Packet > Flashcards

Summer Packet Flashcards

1
Q

Reactions are ____________.

A

Reversible

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2
Q

What can you pass through an atom to separate it into different molecules?

A

An electric current

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3
Q

What is defined as the study of matter and energy and the change between them?

A

Chemistry

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4
Q

What do we use to explain natural phenomenon?

A

Models

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5
Q

What did Robert Boyle experiment with?

A

Air

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6
Q

Who created the first vacuum pump?

A

Robert Boyle

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7
Q

In a ___________ there is no air resistance.

A

Vacuum

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8
Q

How did Robert Boyle define elements?

A

Anything that cannot be broken down into simpler substances

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9
Q

What is Boyle’s gas law?

A

P1V1=P2V2

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10
Q

What is a summary of observed behavior?

A

A scientific law

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11
Q

Explain the Law of Conservation of Mass.

A

Mass remains constant, what goes in must equal what comes out

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12
Q

Explain the law of conservation of energy.

A

Energy cannot be created, nor destroyed. It is only able to change forms.

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13
Q

What is another name for the Law of Conservation of Energy?

A

First law of thermodynamics

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14
Q

Which force caused Galileo to recant his astronomical observations?

A

Strong religious resistance

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15
Q

Who is the Father of Modern Chemistry?

A

Lavoisier

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16
Q

Why was Lavoisier beheaded?

A

Political affiliations

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17
Q

What is the term for rapid change of solid or liquid to gas where molecules become ~2,000 diameters farther apart and therefore exert massive force?

A

Explosion

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18
Q

The need for better explosives has led to nuclear devices and _______.

A

Fertilizer that uses nitrogen.

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19
Q

What are the two parts of a quantitative observation?

A

A number and a unit

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20
Q

What are the two major measurement systems?

A

English and Metric

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21
Q

Where is the English measurement system used?

A

America and parts of Africa

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22
Q

When was the SI system created?

A

1960

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23
Q

The SI system is based off of the __________ system.

A

Metric

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24
Q

Who uses the SI system?

A

Scientists worldwide

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25
Q

What is the term for mass in the SI system?

A

Kilogram

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26
Q

What is the SI unit for time?

A

Seconds

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27
Q

What is the SI system for electric current?

A

Ampere

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28
Q

What is the SI term for the amount of a substance?

A

Mole

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29
Q

What is the SI term for luminous intensity?

A

Candela

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30
Q

What is the SI term for temperature?

A

Kelvin

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31
Q

What is the SI term for length?

A

Meter

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32
Q

What is the abbreviation for a candela?

A

cd

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33
Q

What is the abbreviation for a kilogram?

A

kg

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34
Q

What is the abbreviation for a second?

A

s

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35
Q

What is the abbreviation for a meter?

A

m

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36
Q

What is the abbreviation for a kelvin?

A

K

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37
Q

What is the abbreviation for an ampere?

A

A

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38
Q

What is the abbreviation for a mole?

A

mol

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39
Q

How thick is a dime?

A

1mm thick

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40
Q

What is the diameter of a quarter?

A

2.5 cm

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41
Q

What is the average height of an adult male?

A

1.8m

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42
Q

What is the mass of a nickel?

A

5g

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43
Q

A 120 lbs person has a mass of ________.

A

55kg

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44
Q

What is the volume of a 12-oz can of soda?

A

360mL

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45
Q

Exa is the opposite of Atto. What are they in scientific notation?

A

10^18; 10^-18

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46
Q

A giga is the opposite of a nano. What are they in scientific notation?

A

10^9; 10^-9

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47
Q

A mega is the opposite of a micro. What are they in scientific notation?

A

10^6; 10^-6

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48
Q

A kilo is the opposite of a milli. What are they in scientific notation?

A

10^3; 10^-3

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49
Q

A hecto is the opposite of a centi. What are they in scientific notation?

A

10^2; 10^-2

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50
Q

A deka is the opposite of a deci. What are they in scientific notation?

A

10^1; 10^-1

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51
Q

What takes up space, has mass, and exhibits inertia?

A

Matter

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52
Q

Where do we weigh chemical quantities?

A

On a balance

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53
Q

What is the measure of the resistance of an object to a change in it’s state of motion, or the quantity of matter present?

A

Mass

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54
Q

What is the response of mass to gravity?

A

Weight

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55
Q

Where does gravity originate?

A

The center of the Earth

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56
Q

______________ has a gravitational field.

A

Everything

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57
Q

The moon has ______ the mass of Earth.

A

1/6

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58
Q

Agreement of a measurement with the true value.

A

Accuracy

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59
Q

Degree of agreement among several measures.

A

Precision

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60
Q

Equal probability of measurement being high or low.

A

Random, or indeterminate error

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61
Q

Occurs in the same direction each time.

A

Systematic or determinate error.

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62
Q

Which digits are significant?

A

Nonzero digits

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63
Q

Terminating and right of the decimal as well as if said digit is sandwiched between two numbers are the way of determining if which digit is significant?

A

A zero

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64
Q

How many significant figures does an exact number have?

A

infinity

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65
Q

How many significant figures does a continuing figure have?

A

Infinity

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66
Q

How many significant figures do fundamental constants have?

A

Infinity

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67
Q

When multiplying and dividing, the term with the _______ number of significant figures determines the __________ maximum number of significant figures in the answer.

A

Least, maximum

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68
Q

When adding and subtracting the term with the ________ number of decimal places determines the number of significant figures in the answer.

A

Least

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69
Q

What determines the number of decimal places on the pH?

A

The number of significant figures in the least accurate measurement

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70
Q

In AP chem when do you round?

A

At the end of all calculations

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71
Q

1m=_________yd

A

1.094

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72
Q

1in=________cm

A

2.54

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73
Q

1kg=_______lb

A

2.205

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74
Q

1lb=______g

A

453.6

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75
Q

1L=________qt

A

1.06

76
Q

1ft^3=________L

A

28.32

77
Q

What are the three commonly used temperature scales?

A

Fahrenheit, Celsius, and kelvin

78
Q

What is the boiling point of water in Fahrenheit?

A

212 degrees

79
Q

What is the boiling point of water in Celsius?

A

100 degrees

80
Q

What is the boiling point of water in Kelvin?

A

373.16

81
Q

What is room temperature in Celsius?

A

20 degrees

82
Q

What is room temperature in Fahrenheit?

A

68 degrees

83
Q

What is room temperature in Kelvin?

A

293.15

84
Q

What is the freezing point of water in Celsius?

A

0 degrees

85
Q

What is the freezing point of water in Fahrenheit?

A

32 degrees

86
Q

What is the freezing point of water in kelvin?

A

273.15

87
Q

What is absolute zero in Celsius?

A

-273.15 degrees

88
Q

What is absolute zero in Fahrenheit?

A

-450.67 degrees

89
Q

What is absolute zero in Kelvin?

A

0

90
Q

What is the formula for density?

A

Density = mass/volume

91
Q

Which state of matter is rigid and has a definite shape?

A

Solids

92
Q

Which state of matter has a definite volume but takes up the shape of the container?

A

Liquids

93
Q

Which state of matter has no definite volume and takes up the shape of the container?

A

Gas

94
Q

What is the gas phase of a substance that is normally solid or liquid at room temperature?

A

Vapor

95
Q

Gases and liquids can flow so they are…

A

Fluid

96
Q

Can mixtures be separated?

A

Yes

97
Q

Which mixtures have visibly indistinguishable parts, and are solutions including air?

A

Homogeneous mixtures

98
Q

What type of mixtures have visibly distinguishable parts?

A

Heterogeneous Mixtures

99
Q

List all of the types of separations for mixtures.

A

Filtering, chromatography, fractional crystallization, and distillation

100
Q

What are examples of pure substances?

A

Water, carbon dioxide, and ALL elements

101
Q

What is a common physical method for separating compounds into elements?

A

Electrolysis

102
Q

Elements can be broken down into ________.

A

Atoms

103
Q

Atoms can be broken down into ________ and __________.

A

Nuclei and electrons

104
Q

Pure substances are considered _____________ mixtures.

A

Homogeneous mixtures

105
Q

The processing of ores to produce metal for weapons and ornaments as well as the use of embalming fluids happened when?

A

1000 BC

106
Q

When did the Greeks propose that all matter was made up of four elements? {water, earth, air, fire}

A

400 BC

107
Q

Who was the first to use the term atomos to describe the smallest particles of matter?

A

Democritus

108
Q

What is alchemy?

A

A pseudoscience where people sought to turn metals into gold. Knowledge came out of the mistakes that were made.

109
Q

Georg Baeur was of which nationality?

A

German

110
Q

Who refined the process of extracting metal from ores?

A

Georg Bauer

111
Q

Minerals for medicinal purposes were first used by who? When?

A

Paracelsus {Swiss}; 16th century

112
Q

Who was the first chemist to perform quantitive experiments of pressure vs. volume?

A

Robert Boyle {English}

113
Q

Who created a working definition of elements?

A

Robert Boyle {English}

114
Q

Who suggested that phlogiston {carbon dioxide} flowed out of burning material?

A

Georg Stahl {German}

115
Q

What was previously called “dephlogisticated air”?

A

Oxygen

116
Q

Who discovered oxygen?

A

Joseph Priestly {English}

117
Q

When was combustion studied extensively?

A

Late 18th century

118
Q

Who published the first modern chemistry textbook?

A

Antoine Lavoisier {French}

119
Q

When was Lavoisier executed via guillotine?

A

1794

120
Q

Who explained the true nature of natural combustion?

A

Antoine Lavoisier {French}

121
Q

Who stated the law of conservation of mass?

A

Antoine Lavoisier {French}

122
Q

Who was the first to insist on quantitative experiments?

A

Antoine Lavoisier {French}

123
Q

What is the highest honor given by the American Chemical society?

A

The Joseph Priestly

124
Q

What is the law of conservation of mass?

A

Mass is neither created nor destroyed.

125
Q

What is the law of definite proportions?

A

A given compound always contains exactly the same proportions of elements by mass.

126
Q

Who thought up the law of definite proportions and the atomic theory of matter? When?

A

John Dalton; 1808

127
Q

What is the law of multiple proportions?

A

When two elements combine to form a series of compounds, the ratios of the masses and the second element that combine with one gram of the first element can always be reduced to small whole numbers.

128
Q

All matter is made of _________. They are __________ and ___________.

A

Atoms; indivisible; indestructible

129
Q

Each element has identical _________.

A

Atoms through weight and chemical properties however if you compare two different elements the answers will not be identical

130
Q

____________ are formed by the combination of different atoms in the ratio of small whole numbers.

A

Compounds

131
Q

A _______________ involves the separation, combination, or rearrangement of atoms.

A

Chemical reaction (atoms are not created nor destroyed during a chemical reaction)

132
Q

Who performed experiments (at a constant temperature and pressure) and measured the volumes of gases that reacted with one another? When?

A

Joseph Gay-Lucas {French}; 1809

133
Q

Who proposed his hypothesis regarding Gay-Lucas’s work?

A

Avogadro {Italian}, 1811

134
Q

At the same temperature and pressure, equal volumes of different gases contain the same number of particles… This is whose hypothesis?

A

Avogadro’s Hypothesis

135
Q

Who found that when high voltage was applied to an evacuated tube, a “Ray” he called a cathode ray was produced? (A cathode ray emanates negative electrodes when you apply a voltage)

A

J. J. Thomson {English}

136
Q

A cathode ray is a stream of negative particles called _______________.

A

Electrons

137
Q

Who played a role in the development of the “plum pudding model”?

A

Lord Kelvin

138
Q

Who at the University of Chicago used gravity to help him determine what the charge of oil particles what?

A

Robert Milikan {American}; 1909

139
Q

Who found out by accident that a piece of mineral containing uranium could produce its image on a photographic plate in the absence of light?

A

Henri Becquerel {French}

140
Q

Henri Becquerel discovered ______________.

A

Radioactivity

141
Q

What are the three types of radioactive emissions?

A

Alpha, beta, gamma

142
Q

An alpha radiation particle is equivalent to a _______________.

A

Helium nucleus

143
Q

Which particle is largest?

A

Alpha; it’s mass is 7300x that of an electron

144
Q

What is a beta radiation particle?

A

A high speed electron

145
Q

What is a gamma radiation particle?

A

No particles, just waves, penetrates deepest, therefore most dangerous

146
Q

A pioneer in radioactive studies, __________________ performed tests on the “plum pudding model”.

A

Ernest Rutherford {English}; 1911

147
Q

Rutherford directed alpha particles at a thin sheet of ________________ in order to test Thomson’s model, if Thomson was correct then the alpha particles would blast through the thin material with ease.

A

Gold foil

148
Q

What were the results of Rutherford’s experiment?

A

The alpha particles not only went through the gold foil, they were transmitted in all other directions, even reflected! This proved the plum pudding model incorrect

149
Q

The nuclear atom has a dense + core, or ______________.

A

Nucleus

150
Q

Most of an atoms mass in the _____________ while the rest is suspended within an electron cloud.

A

Nucleus

151
Q

How many naturally occurring elements are there?

A

92

152
Q

What retains the chemical properties of an element?

A

An atom

153
Q

Nuclear material is very ___________.

A

Dense

154
Q

The nucleus contains the ______________ and ______________.

A

Protons and neutrons

155
Q

What is the diameter of a nucleus? How far away from the nucleus are electrons?

A

10^-13; 10^-8

156
Q

Which subatomic particle is responsible for isotopes and can alter the atomic mass?

A

Neutrons

157
Q

Which subatomic particle is responsible for atomic number?

A

Protons

158
Q

Electrons are the same size as protons and neutrons but _____________ the mass.

A

1/2,000

159
Q

Which subatomic particle is responsible for bonding and are easily added or removed?

A

Electrons

160
Q

What is the variable for atomic number? Atomic mass?

A

Z; A

161
Q

Does atomic mass determine the element?

A

No. Just isotopes!

162
Q

What is an isotope?

A

An atom having the same atomic number but a different number of neutrons

163
Q

Which elements only have one stable isotope?

A

Aluminum, Florine, and Phosphorus

164
Q

Most elements have how many stable isotopes?

A

2

165
Q

What are the three isotopes of hydrogen and how many neutrons do they have?

A

Hydrogen {0}; deuterium {1}; tritium {3}

166
Q

What hold atoms together?

A

Chemical bonds

167
Q

What is it called when atoms share electrons to make molecules?

A

Covalent bonds

168
Q

The structural formula uses what to show bonds?

A

Lines

169
Q

What is formed when electrons are lost or gained?

A

Ions

170
Q

Metals _________ electrons to become positively charged. This ionic bond results in ____________.

A

Lose; cations

171
Q

Nonmetals _________ electrons to become positively charged. This ionic bond results in ________.

A

Gains; anions

172
Q

What hold ions together?

A

Electrostatic forces

173
Q

F=(kq1q2)/(r2)

A

Coulomb’s law

174
Q

In the periodic table where is the atomic number written?

A

Above the atom

175
Q

Which elements are malleable, ductile, and have luster? This includes most of the elements, most are cations, and can form oxides.

A

Metals

176
Q

Groups are __________

A

Vertical

177
Q

Periods are ______________

A

Horizontal

178
Q

Alkali Metals?

A

1A or IA

179
Q

Alkaline Earth Metals?

A

2A or IIA

180
Q

Halogens?

A

7A or VIIA

181
Q

Noble Gases?

A

8A or VIIIA

182
Q

No Roman numerals are used with __________, _____________, and ____________.

A

Silver, cadmium, and zinc. They only make one valence state

183
Q

NH4^+ is…

A

Ammonium

184
Q

Monatomic adds the suffix _______ to the stem of the nonmetal.

A

-ide

185
Q

Polyatomic naming goes in which order?

A

Hypo, -ite, -ate, hyper/per

AP Chem (1 decks)

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