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Midterm Review Flashcards

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0
Q

Give an example of qualitative data?

A

Color of a shirt

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1
Q

What is the goal of science and it’s models?

A

Workability

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2
Q

When a hypothesis makes as few assumptions and is as simple as possible, what principle of logic has been followed?

A

Ockham’s razor

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3
Q

What is a simple, testable statement of a prediction based on available information?

A

Hypothesis

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4
Q

Who discovered the element oxygen?

A

Joseph Priestly

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5
Q

Which branch of chemistry primarily studies compounds contained carbon?

A

Organic chemistry

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6
Q

Alchemists were known for trying to convent ordinary metals into __________.

A

Gold

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7
Q

What is anything that occupies space and mass?

A

Matter

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8
Q

The Sumerians were skilled in the science of obtaining metals from ores. What is this science called?

A

Metallurgy

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9
Q

What were the four basic elements the Greeks believed made up the universe?

A

Earth
Air
Fire
Water

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10
Q

The logical thinking demanded by a course in chemistry helps Christians to further develop the ability to think critically.

T/F

A

True

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11
Q

Alchemists were known for their experimentations.

T/F

A

True

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12
Q

The Greeks desired knowledge rather than practical skills.

T/F

A

True

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13
Q

Scientific theories should be accepted without question because they have results from thorough investigation.

T/F

A

False

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14
Q

The scientific method, when used properly, can lead a person to determine absolute truth.

T/F

A

False

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15
Q

As Christians, we all believe were all created how?

A

In God’s image

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16
Q

What science explorers natural products and processes for specific purposes and applications?

A

Applied science

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17
Q

What physical property explains materials that can be drawn into long, thin wires?

A

Ductility

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18
Q

What is the most conductive metal?

A

Silver

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19
Q

The measure of disorder or randomness of particles is also known as ______________.

A

Entropy

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20
Q

What is the change from a gas to a liquid called?

A

Condensation

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21
Q

Identify each of the following chemical formula: 5H2O

A

5- coefficient
2- subscript
H&O- element
Chemical symbol

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22
Q

What is matter?

A

Is anything that takes up space and has mass

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23
Q

Identify three characteristics of a solid:

A

Definite volume
Definite shape
Difficult to compress

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24
Q

What is the study of movement and conservation of energy?

A

Thermodynamics

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25
Q

What are changes that result in changes of the identity of a material?

A

Chemical change

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26
Q

What is a pure substance that cannot be broken down into a simpler substance by ordinary chemical means?

A

Element

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27
Q

What is an example of a molecule that occurs naturally as a monatomic element?

A

Xenon

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28
Q

What is the operation definition of energy?

A

The ability to do work

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29
Q

What energy is responsible for the forming of breaking bonds with other elements?

A

Chemical energy

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30
Q

What is the sum of the kinetic energy of an objects parities?

A

Thermal energy

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31
Q

What temperature is absolute zero?

A

-273.15 C

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32
Q

What is the standard SI unit for measuring energy and work?

A

Joules (J)

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33
Q

The first professor of chemistry in the United States

A

Benjamin Rush

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34
Q

Identify the three characteristics for each of the following:
Solids
Liquids
Gases

A

Solids:
Definite shape
Definite volume
Incompressible

Gases
No definite shape
Do definite volume
Highly compressible

Liquids
Shape of container
Definite volume
Nearly incompressible

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35
Q

Give an example of quantitative data.

A

The amount of fish in a bowl

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36
Q

List 3 of the six major branches of chemistry.

A

Organic chemistry
Inorganic chemistry
Nuclear chemistry

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37
Q

What is matter?

A

Anything that takes up space and has mass

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38
Q

What distinguishes mixtures from pure substances?

A

Type of change or bonding

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39
Q

Identify two homogeneous and two heterogeneous mixtures.

A

Homogeneous- cake and air

Heterogeneous- oil&vinegar dressing and granite

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40
Q

Physical or chemical property:

Colorless

A

Physical

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41
Q

Physical or chemical property:

Flammable

A

Chemical

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42
Q

Physical or chemical property:

Freezes at 34K

A

Physical

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43
Q

Physical or chemical property:

Magnetic

A

Physical

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44
Q

Physical or chemical property:

Explosive

A

Chemical

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45
Q

Physical or chemical property:

Sinks in water

A

Physical

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46
Q

The second letter in a chemical symbol is always capitalized.

T/F
Why

A

False

The first letter is always capitalized

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47
Q

Kelvin temperatures cannot be negative.

T/F
Why

A

True

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48
Q

Reactions that release energy are exothermic.

T/F
Why

A

True

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49
Q

Everything in the universe is composed of chemicals.

T/F
Why

A

True

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50
Q

Temperature measures the total kinetic emery in a sample.

T/F
Why

A

False

Thermal energy

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51
Q

What is the base unit for the dimension of mass and length?

A

Mass- kilogram(kg)

Length- meter (m)

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52
Q

What is the comparison of the actual measurement and the numerical evaluation of the instrument?1

A

Accuracy

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53
Q

When adding and subtracting measurements, what must be taken into consideration when dealing with significant digits?

A

Precision

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54
Q

What is the formula for density?

A

d=m/v

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55
Q

What is the scale or a measuring instrument which is the accurately subdivided measuring units?

A

Calibrated scale

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56
Q

What is the prefix that represents million? Millionth?

A

Million- mega (m)

Millionth- micro (u)

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57
Q

In order to deal with significant digits of a measurement, what two things must be present?

A

Number & unit

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58
Q

SI unit that represents the amount of particles of a substance

A

Mole

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59
Q

Your calculators answer is read from this type of screen

A

Digital

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60
Q

A fraction equal to one that contains both the original unit and it’s equivalent value in a new unit

A

Conversion factor

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61
Q

Indicates the precision of an instrument and helps scientists report measurements honestly

A

Significant digits

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62
Q

System of measurement based on a decimal scale

A

Metric

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63
Q

The accurately subdivided measuring units

A

Calibrated

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64
Q

The result of comparing an unknown quantity to a standard unit

A

Measurement

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65
Q

Any artificial device made for the purpose of refining, extending, or substituting for the human senses when measuring

A

Instrument

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66
Q

The number 0.00800 has three significant digits

T/F
Why

A

True

67
Q

When determining significant digits in multiplication and division problems, the answer cannot contain more significant digits than the measurement with the least number of significant digits.

T/F
Why

A

True

68
Q

If a scientist is extremely careful and uses precise instruments, a perfect measurement can be obtained.

T/F
Why

A

False

There is always going to be uncertainty with measurements, there is no perfect measurement.

69
Q

The unit for volume is derived from the SI unit for length, the meter.

T/F
Why

A

True

70
Q

The first step in problem solving is choosing the specific tools to use.

T/F
Why

A

False

Read the statement of problem

71
Q

When wolfing problems that involve compost calculations, it is nest to round off at each of the intermediate steps.

T/F
Why

A

False

Don’t round until the end

72
Q

Give four of the seven base units for SI and the basic dimension that each represents.

A

Length- meter (m)
Time- seconds (s)
Mass- kilogram (kg)
Temperature- kelvin (K)

73
Q

Explain the difference between accuracy and precision.

A

Accuracy is how close your measurement is to the actual measurement. Precision is how close a repeated number of measurements are to each other.

74
Q

Hundredth

A

Centi

75
Q

Million

A

Mega

76
Q

Tenth

A

Deci

77
Q

Billionth

A

Nano

78
Q

Thousandth

A

Milli

79
Q

Thousand

A

Kilo

80
Q

Millionth

A

Micro

81
Q

What is the maximum numbers of electrons that can be found in any atom’s second principle energy level?

A

8

82
Q

Who was the first to refer to the smallest particles composing matter as atoms?

A

Democritus

83
Q

What rule describes how electrons fill an orbital?

A

Hund’s rule

84
Q

The following equals the number of protons and neutrons:

A

Mass number (A)

85
Q

What charge does an atom have if it loses an electron?

A

Positive=cation

86
Q

Who discovered the electron?

A

Thompson

87
Q

An atom that gains three electrons will have a +3 charge.

T/F

A

False

88
Q

An electron can behave either as a wave of a particle.

T/F

A

True

89
Q

What are the names and values for the four sublevels?

A

S-0
P-1
D-2
F-3

90
Q

Isotopic atoms have different number of __________, while ions have a differing number of _____________.

A

Neutrons

Electrons

91
Q

Philosophical atomism

A

Democritus

92
Q

First experimental atomic model

A

John dalton

93
Q

Cathode rays

A

J. J Thomas

94
Q

X rays

A

Wilhelmina roentgen

95
Q

Neutrons

A

James Chadwick

96
Q

Protons

A

Ernest Rutherford

97
Q

God foil experiment

A

Hans Geiger

98
Q

What is the idea that any sample of water always contains 8 g of oxygen for every 1 g of hydrogen.

A

Law of definite composition

99
Q

The type of sublevel found in all principle energy levels is the ____ level.

A

S

100
Q

The s, p, d, and f sublevels are identified by _________ quantum numbers.

A

Azimuthal

101
Q

Two different isotopes of a single element will have the same number of _________ but different number of ___________.

A

Protons

Neutrons

102
Q

The general region of space where an electron is most probably found is known as it’s orbital.

T/F

A

True

103
Q

Dalton based his atomic model on both experiments and logic.

T/F

A

True

104
Q

Neutrons contribute to an atom’s mass and it’s charge.

T/F

A

False

105
Q

An electron can behave as either a wave or particle.

T/F

A

True

106
Q

Each atom can be identified by the number of protons in its nuecleus.

T/F

A

True

107
Q

The first quantum number identifies the principle energy level of an electron.

T/F

A

True

108
Q

Compare three different atomic models.

A

Dalton’s atomic model, Thompsons plum pudding model, and rutherford’s nuclear model all dealt with uncertainty and enhanced in later years.

109
Q

First model to include atoms of each element having different masses.

A

Dalton

110
Q

States that it is impossible to know both the energy and the exact position of an electron at the same time.

A

Uncertainty principle

111
Q

Describes how electrons fill orbitals.

A

Hunds

112
Q

Describes now electrons fill sublevels

A

Aufbua

113
Q

Equals the numbers of protons and neutrons.

A

Mass number

114
Q

Electrons in the outermost energy level that are important in bonding.

A

Valence electrons

115
Q

Negatively charged ions.

A

Anions

116
Q

Charge of an atom if it loses an electron.

A

Positive

117
Q

What is determined by the weighted averages of isotopes on an element?

A

AMU

118
Q

What is the minimum energy required to remove the first electron form it’s outermost shell to make it a cation?

A

First ionization energy

119
Q

Helium, neon, argon, and krypton are all examples of what family of elements?

A

Noble gases

120
Q

What group of elements conduct electricity only under certain conditions therefore are known as semiconductors.

A

Metalloids

121
Q

What is the measured attraction between the nucleus and the valence electrons?

A

Electronegativity

122
Q

Who was the Nobel Prize winning chemist who devised an electronegativity scale?

A

Linus Pauling

123
Q

What states that the properties of elements vary with their atomic numbers in a periodic way?

A

Periodicity

124
Q

Which element has a larger atomic radius: potassium or helium?

A

Potassium

125
Q

Which element has a higher first ionization energies: calcium or krypton?

A

Krypton

126
Q

What is the tasteless, odorless gas that accounts for 21% of the earth’s ato sooner and is the most abundant element in the earth’s crust. It is also essential for the life of animals and humans.

A

Oxygen

127
Q

The two elements that are the major constituents of hard water and magnesium and ____________.

A

Calcium

128
Q

Mendeleev’s periodic table was arranged by elements what?

A

First mass, then atomic number

129
Q

Who arranged a number of elements in triads based on similar properties?

A

Dobreiner

130
Q

Whose work resulted in the revision in of the periodic law and the atomic number being used as the organizing factor for the elements of the periodic table?

A

Moseley

131
Q

What chemist arranged the elements according to increasing atomic masses and thereby discovered the relationship he called the law of octaves?

A

Newlands

132
Q

It is the lightest and most abundant element in the universe is extremely flammable in the air, and is used in the industrial production of ammonia.

A

Hydrogen

133
Q

Existing as diatomic molecules, this gas is tasteless, colorless, odorless and it accounts for approximately 78% of the earths atmosphere.

A

Nitrogen

134
Q

According to the Big Bang theory, the very first elements would problem have been….?

A

H and He

135
Q

The presence of calcium and magnesium ions in water makes it “hard” water.

T/F

A

True

136
Q

Graphite and diamonds are both composed of the same element, carbon.

T/F

A

True

137
Q

Halogens are easily obtainable in their elemental form.

T/F

A

False

138
Q

High electronegativity is are associated with large ionization energies and high electron affinities.

T/F

A

True

139
Q

Under normal conditions, noble gases form compounds with other elements easily.

T/F

A

False

140
Q

Mendeleev’s work sets him apart from other scientists because of his obsessiveness about his work.

T/F

A

True

141
Q

Helium, neon, argon, xenon, radon

A

Noble gases

142
Q

Oxygen, nitrogen, carbon, sulfur

A

Nonmetal

143
Q

Flourine, chlorine, iodine, bromine

A

Halogens

144
Q

Boron, silicon, arsenic, germanium

A

Metalloids

145
Q

Semiconductors

A

Metalloids

146
Q

Good conductors of heat and electricity, usually hard, lustrous, malleable, and ductile

A

Metals

147
Q

Contains characteristics of both metals and nonmetals.

A

Metalloids

148
Q

Generally gases or soft solids

A

Nonmetals

149
Q

Negative ion

A

Anion

150
Q

The minimum energy required to remove the first electron from its outermost shell to make it a cation

A

First ionization energy

151
Q

Distance from the center of an atom’s nucleus to its outermost electron.

A

Atomic radius

152
Q

Positive ion

A

Cation

153
Q

Amount of energy required to add an electron to a neutral atom to form a negative ion

A

Electron affinity

154
Q

The electron-sea theory applies to what bonds?

A

Metallic

155
Q

What bond is between the attraction of oppositely charged ions?

A

Ionic

156
Q

What is the ultimate purpose of why atoms bond?

A

Octet rule

157
Q

In the Lewis structure, how many electrons does the dash represent?

A

Two

158
Q

When one or two pairs of shared electrons bond, what bond occurs?

A

Covalent

159
Q

What is the mixture of metal atoms with another element resulting in a mixture with metallic properties?

A

Alloys

160
Q

Examples of network covalent substances

A

Diamonds
Silicate
Quartz

161
Q

Diatomic molecules

A

H2 N2 O2 Cl2 F2 Br2 I2

162
Q

What is the tendency of an object to form two localized regions of opposite character?

A

Polarity

163
Q

What are the two-dimensional diagrams that show the bonds between different atoms?

A

Lewis structures

164
Q

What is the force exerted between electrical charges of two atoms?

A

Electrostatic force

Chemistry (4 decks)

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