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Flashcardlet > Phy Sci 3RD NINE WEEKS EXAM > Flashcards

Phy Sci 3RD NINE WEEKS EXAM Flashcards

0
Q

Solids, liquids, and gases are three forms of matter that

A

Take up space
Have mass
Are made of atoms

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1
Q

The smallest unit of an element that maintains the properties of that element

A

Atom

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2
Q

How many atoms are there in a single molecule of Fe2O3

A

5

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3
Q

A not pure substance

A

Mixture

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4
Q

Is iron an element

A

Yes

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5
Q

Is salt an element

A

No

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6
Q

A group of atoms that act as a unit

A

Compound

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7
Q

What is the chemical compound for table sugar

A

C12H22O11

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8
Q

What is the chemical compound for water

A

H2O

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9
Q

What is the chemical compound for rust

A

Fe2O3

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10
Q

What is the chemical compound for copper

A

Cu

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11
Q

Diamond is known for its what

A

Hardness

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12
Q

Why is helium used in balloons

A

It is lighter than air

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13
Q

What kind of property is reactivity

A

Chemical

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14
Q

What kind of property is density

A

Physical

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15
Q

An object’s volume can be found by dividing its mass by its

A

Density

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16
Q

Is the ability to rust a physical property

A

No

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17
Q

What property of a substance is not affected by chemical change

A

Reactivity

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18
Q

What do the different substances in a mixture keep

A

Their properties

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19
Q

What is one example of a potential sign of chemical change

A

Change in color

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20
Q

How can chemical changes be reversed

A

By chemical changes

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21
Q

Can burning cause a chemical change

A

Yes

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22
Q

Can shattering cause a chemical change

A

No

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23
Q

Does dissolving salt result in a mixture

A

Yes

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24
Q

Does baking a cake result in a mixture

A

No

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25
Q

When does a chemical change occur

A

When new substances form

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26
Q

What tool is best for separating a mixture of sand and water

A

Filter

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27
Q

Is evaporating a physical change

A

Yes

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28
Q

What do chemical changes effect

A

Physical and chemical properties

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29
Q

What do physical changes effect

A

Physical properties

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30
Q

The chemical element that is most abundant in the human body

A

Oxygen

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31
Q

How is a molecule of water (H2O) made

A

Chemically combining 2 hydrogen atoms and 1 oxygen atom

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32
Q

A material that can be represented by a chemical formula

A

Pure substance

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33
Q

Is evaporation of water a potential sign of chemical change

A

No

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34
Q

The smallest unit of an element that maintains the properties of that element

A

Atom

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35
Q

Is a mixture a pure substance

A

No

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36
Q

A group of atoms that acts as a unit

A

Molecule

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37
Q

Is reactivity a chemical property

A

Yes

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38
Q

Is density a physical property

A

Yes

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39
Q

Anything that has mass and takes up space

A

Matter

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40
Q

The smallest unit of a substance that behaves like the substance

A

Molecule

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41
Q

What is made up of at least 2 different types of atoms

A

Compound

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42
Q

Unlike a mixture, a pure substance has

A

A fixed composition

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43
Q

Stainless steel has chemical properties such as

A

Resistance to rust

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44
Q

Digesting food is an example of

A

Chemical change

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45
Q

The science of what matter is made of and how it changes

A

Chemistry

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46
Q

A substance that cannot be broken down into simpler substances

A

Element

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47
Q

Knowing the chemical properties of a substance will tell you how the substance …

A

Reacts with other substances

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48
Q

Is dissolving salt in water a physical or chemical change

A

Physical

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49
Q

When the identity of a substance is changed

A

Chemical change

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50
Q

What kind of change can a change in color help you detect

A

Chemical

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51
Q

What is the formula for mass

A

Density
––––––––
Volume

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52
Q

What is the formula for density

A

Mass
–––––––
Volume

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53
Q

What is the formula for volume

A

Mass
–––––––
Density

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54
Q

What does the kinetic theory of matter state about matter

A

The atoms and molecules of a substance are always in motion
The higher the temperature of a substance, the faster it’s particles move
More massive particles move slower than less massive ones

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55
Q

The measure of the average kinetic energy of the particles in an object

A

Thermal energy

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56
Q

All matter is made of atoms and molecules that are

A

Always in motion

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57
Q

What is matter made of

A

Atoms and molecules that are always in motion

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58
Q

The particles can slide past each other, but are still packed together

A

Liquid

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59
Q

The particles have broken down and become ionized

A

Plasma

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60
Q

The particles are in a rigid, fixed structured

A

Solid

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61
Q

The particles are in constant motion and rarely stick together

A

Gas

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62
Q

The process of a solid changing directly into a gas

A

Sublimation

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63
Q

What does the law of conservation of mass state

A

Total mass stays the same in changes of state

64
Q

What does the law of conservation of energy state

A

A substance has the same energy before and after a change of state

65
Q

What happens to energy when ice melts to form liquid

A

It is released

66
Q

The temperature at which a substance changes from a liquid to a solid

A

Freezing point

67
Q

Why does the engine of a car left running for a long period of time become hot

A

Energy is transformed from burning gasoline

68
Q

Why does a substance change from a liquid to a gas during evaporation

A

Energy is released

69
Q

What happens to the particles of a substance when it condenses

A

They slow down and clump together

70
Q

Who described the notion that an object floats if the buoyant force on the object is equal to the object’s weight

A

Archimedes

71
Q

When does an object float

A

If the buoyant force on the object is equal to the object’s wright

72
Q

What is the ability of an object to float on a fluid influenced by

A

Buoyant force of a fluid
Density of the object
Density of the fluid

73
Q

What does Pascal’s principle state

A

A contained fluid exerts pressure equally in all directions

74
Q

What is the calculation for pressure

A

Force
–––––––––––––––––––––––
Area the force is exerted

75
Q

A measure of the resistance to flow of a fluid

A

Viscosity

76
Q

What influences the speed at which fluid flows through a pipe

A

Flow rate of the fluid
Viscosity of the fluid
Cross-sectional area of the pipe

77
Q

What happens to speed as the pressure of a moving liquid increases

A

It decreases

78
Q

Who’s principle describes the property of a fluid in motion

A

Bernoulli

79
Q

What does Bernoulli’s principal describe

A

The property of a fluid in motion

80
Q

Upward force exerted on an object immersed tp floating on a liquid

A

Buoyant force

81
Q

Measure of average kinetic energy of the particles in the object

A

Temperature

82
Q

What determines the speed of the atoms and molecules of a particular substance

A

Size of the atoms and molecules

Temperature of the substance

83
Q

The change of state from a liquid to a gas

A

Evaporation

84
Q

The law of conservation of mass states that mass cannot be

A

Created or destroyed

85
Q

Why does ice float in water

A

It is less dense than water

86
Q

Gay-Lussac’s law relates what

A

The temperature of a gas to its pressure

87
Q

Whose law relates the temperature of a gas to its pressure

A

Gay-Lussac’s

88
Q

What happens to the pressure of a fixed amount of gas as it’s temperature decreases

A

It decreases

89
Q

As the volume of a fixed amount of gas decreases, what happens to its pressure

A

Increases

90
Q

Force
––––– is the calculation for what
Area

A

Preside

91
Q

Whose principle describes the property of a fluid in motion

A

Bernoulli

92
Q

As the temperature of a gas at constant volume decreases, what happens to its pressure

A

It decreases

93
Q

Why are gases unique in comparison to solids and liquids

A

They are easily compressible

94
Q

As the pressure of a gas at a constant temperature decreases, what happens to its volume

A

It increases

95
Q

What law is illustrated by the equation P1V1 = P2V2

A

Boyle’s law

96
Q

What equation illustrates Boyle’s law

A

P1V1 = P2V2

97
Q

Why does the volume of a has decrease when the pressure increases

A

Gas particles are pushed together when the pressure is increased

98
Q

What about plasma is unlike gas

A

It conducts electric current

99
Q

What two things does Charles’s law relate

A

The volume of a gas to its temperature

100
Q

Whose law relates the volume of a gas to its temperature

A

Charles

101
Q

When a fixed sample of gas increases in temperature, what happens to its pressure

A

It increases

102
Q

What does the kinetic theory help explain the difference between

A

States of matter

103
Q

A gas becomes a liquid through a process called

A

Condensation

104
Q

Boyle’s law relates what two things

A

Volume of a gas to pressure

105
Q

Who’s law relates the volume of a gas to its pressure

A

Boyle’s

106
Q

When a fixed sample of has increases in volume, it must also do what

A

Decrease in pressure

107
Q

Why was Democritus’s original atomic theory revised

A

It didn’t have a scientific basis

108
Q

What does Dalton’s atomic theory state

A

Atoms cannot be divided
Atoms of an element are alike
Atoms of different elements form compounds

109
Q

A subatomic particle that has a negative charge

A

Electron

110
Q

Who determined that atoms could be divided

A

Thomson

111
Q

What experiment did Thomson use

A

Cathode-ray

112
Q

What is Thomson responsible for discovering

A

That atoms have electrons

113
Q

What kind of charge do neutrons have

A

Neutral / none

114
Q

What is an atom’s nucleus made of

A

Protons

Neutrons

115
Q

In whose model do negative electrons orbit a positively charged nucleus

A

Rutherford

116
Q

Whose model determined that an atom’s positive charge is concentrated in the atom’s center

A

Rutherford

117
Q

What is Avogadro’s number useful for

A

Counting atoms

118
Q

What is the charge of an atom

A

Neutral

119
Q

How much effect do commonly found isotopes have on the average atomic mass of an element

A

More than rarely found isotopes

120
Q

What is an element’s atomic number equal to

A

It’s number of protons

121
Q

Two different isotopes of an element have different what

A

Number of neutrons

122
Q

What is the mass number of an element that has 19 protons, 19 electrons, and 20 neutrons

A

39

123
Q

How many electrons can fit in the first level

A

2

124
Q

How many electrons can fit in the second level

A

8

125
Q

How many electrons can fit in the third level

A

18

126
Q

How many electrons can fit in the fourth level

A

32

127
Q

After the fourth level, how many electrons can fit in each level

A

32

128
Q

A sodium atom, which has 11 electrons, has how many valence electrons

A

1

129
Q

What does Bohr’s model state that is unlike the modern model of the atom

A

Electrons move in set paths around the nucleus of an atom

130
Q

What are the four types of orbitals

A

s
d
p
f

131
Q

When does an electron jump to a new energy level

A

When the atom gains or loses energy

132
Q

The number of energy levels filled in an atom is determined by what

A

Electrons

133
Q

How many electrons can each orbital hold up to

A

2

134
Q

What determines the number of electrons each level can hold

A

Orbitals

135
Q

Found in the outer energy level of an atom

A

Valence electron

136
Q

Where electrons are likely to be found in an atom

A

Orbital

137
Q

Unit or quantum of light

A

Photon

138
Q

What happens to an electron when it gains energy

A

Excited state

139
Q

Why was Dalton’s atomic theory accepted

A

There was evidence to support it

140
Q

Why do atoms have no electric charge

A

They have an equal number of protons and electrons

141
Q

According to the new model of the atom, what do electrons behave like

A

Waves on a vibrating string

142
Q

It is nearly impossible to determine an electron’s what

A

Exact position

143
Q

Valence electrons determine an atom’s what

A

Chemical properties

144
Q

A mole is an SI base unit that describes what

A

Volume of a substance

145
Q

If the atomic mass of carbon is 12u, 1 mole of pure carbon will have a mass of what

A

12g

146
Q

Who’s original atomic theory revised because it didn’t have a scientific basis

A

It didn’t have a scientific basis

147
Q

What did Thomson determine about atoms

A

That they could be divided

148
Q

How much effect do commonly found isotopes have on the average atomic mass of an element

A

More than rarely found isotopes

149
Q

An element’s atomic number is equal to its number of

A

Protons

150
Q

An element’s atomic number is equal to its number of

A

Protons

151
Q

According to Rutherford’s model of the atom, electrons behave like what

A

Planets orbiting the sun

152
Q

According to Rutherford’s model of the atom, electrons behave like what

A

Planets orbiting the sun

153
Q

According to Bohr’s theory, an electron’s path around the nucleus defines its what

A

Energy level

154
Q

According to Bohr’s theory, an electron’s path around the nucleus defines its what

A

Energy level

155
Q

A unified atomic mass unit is equal to

A

One-twelfth her mass of a carbon-12 atom

156
Q

A unified atomic mass unit is equal to

A

One-twelfth her mass of a carbon-12 atom

157
Q

Molar mass is defined as what

A

The mass in grams of one mole of a substance

158
Q

Molar mass is defined as what

A

The mass in grams of one mole of a substance

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