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Honors Chemistry > Semester 1 Final Review > Flashcards

Semester 1 Final Review Flashcards

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1
Q

What is a chemical property?

A

The ability or inability of a substance to combine with or change into one or more other substances.

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2
Q

What is a physical property?

A

A characteristic of matter that can be observed or measured without changing the sample’s composition

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3
Q

What are some physical properties?

A

Density, color, odor, hardness, melting point, and boiling point are common physical properties

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4
Q

What can physical properties be further described as?

A

Intensive or extensive properties

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5
Q

How many significant figures are there in a distance measurement of 180,200.06 cm?

A

8

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6
Q

What are the SI base units?

A

Seconds, meters, kilograms, kelvins, moles, ampere, candela

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7
Q

In addition and subtraction, the answer must not have more significant figures…

A

To the right of the decimal point

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8
Q

Accuracy pertains to?

A

Closeness of a measurement to an accepted value

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9
Q

What does precision pertain to?

A

Precision is the sameness of measurements that show little to no variation

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10
Q

What is a solution?

A

A homogeneous mixture

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11
Q

What is the law of conservation of mass?

A

Law that states that mass in neither created nor destroyed in a chemical reaction

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12
Q

What is the periodic table?

A

The grid organizing elements into periods and groups

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13
Q

What is percent by mass?

A

The ratio of the mass of each element to the total mass of the compound

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14
Q

What is the definition regarding the states of matter?

A

Three physical forms that describe the matter that exists on Earth

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15
Q

What is crystallization?

A

A separation technique that results in the formation of pure solid particles from a solution

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16
Q

What is chromatography?

A

A technique that separates that components of a mixture

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17
Q

What is the definition of a liquid?

A

A form of matter with a constant volume that takes the shape of its container

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18
Q

What is the definition of a solid?

A

A form of matter with a definite shape and volume

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19
Q

What are some chemical properties?

A

Forms with elements exposed to air, reactivity with another substance, ability to combine with another substance

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20
Q

What are some intensive physical properties?

A

Chemical formula CO, colorless, solid at room temperature, melting point, conducts electricity, density

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21
Q

What are some extensive physical properties?

A

Mass

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22
Q

What words indicate a physical change?

A

Boiling, freezing, condense, crush, vaporize

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23
Q

What words indicate a chemical change?

A

Explode, tarnish, ferment, burn, corrode

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24
Q

What mixtures can be identified as homogeneous?

A

Saline, sterling silver (silver & copper mix), black tea

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25
Q

What mixtures can be identified as heterogeneous?

A

Glass of soda, bowl of cereal, sidewalk pavement, sand, salad, mulch, chocolate chip cookies

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26
Q

Identify the technique you would use to separate two substances with different boiling points

A

Distillation or chromatography is the technique you would use to separate two substances with different boiling points

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27
Q

What is the law that states that mass cannot be created nor destroyed in ordinary chemical and physical changes?

A

The law of conservation of mass

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28
Q

What is the charge of a proton?

A

Positive

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29
Q

Where is the proton found?

A

Nucleus

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30
Q

What is the law of conservation of mass?

A

Law that states that mass cannot be created nor destroyed in ordinary chemical and physical changes

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31
Q

What is the charge of the electron?

A

Negative

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32
Q

Where is the electron found?

A

Located outside surrounding the nucleus on the electron cloud

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33
Q

What is the law of multiple proportions?

A

When two elements combine to form two or more compounds, the mass of one element that combines with a given mass of the other element is in the ratio of the small whole numbers

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34
Q

What is the charge of a neutron?

A

Neutral/no electrical charge

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35
Q

Where is the neutron found?

A

Located inside the nucleus

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36
Q

What is the law that states when two elements combine to form two or more compounds, the mass of one element that combines with a given mass of the other element is in the ratio of the small whole numbers?

A

The law of multiple proportions

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37
Q

What contributions did Aristotle make to atomic theory?

A

Halted any progression in atomic theory. Believed that matter existed of only 4 elements

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38
Q

What contributions did Democritus make to atomic theory?

A

Believed that atoms were the building blocks of matter and atoms were indivisible

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39
Q

What contributions did Dalton make to atomic theory?

A

Determined that atoms could combine to form compounds

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40
Q

What contributions did Thomson make to atomic theory?

A

Used the cathode ray tubes to discover the electron

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41
Q

What contributions did Rutherford make to atomic theory?

A

Used the gold foil experiment to discover the nucleus of the atom

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42
Q

What contributions did Bohr make to atomic theory?

A

Determined that electrons exist in energy levels at certain distance from the nucleus

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43
Q

What contributions did Newlands make to atomic theory?

A

Developed the law of octaves

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44
Q

What contributions did Moseley make to atomic theory?

A

Arranged the elements by increasing atomic number

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45
Q

What contributions did Mendeleev make to atomic theory?

A

Developed the first widely accepted periodic table of elements by arranging the elements by increasing atomic mass.

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46
Q

Why was Mendeleev’s periodic table widely accepted?

A

He predicted the existence and properties of undiscovered elements. As well, he was the first to notice a pattern of similar properties among elements

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47
Q

How do you know which elements have the same or similar chemical properties?

A

If they are in the same group

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48
Q

What is an element with chemical properties similar to Iodine?

A

Chlorine

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49
Q

What is an element with chemical properties similar to Iron?

A

Ruthantum

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50
Q

What is the group name of group 1?

A

Alkali metals

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51
Q

What is the group name of group 17?

A

Halogens

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52
Q

What is the group name of group 2?

A

Alkali earth metals

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53
Q

What is the group name of group 18?

A

Noble gases

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54
Q

What is the group name of groups 3-12?

A

Transition metals

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55
Q

What is the group name of groups 14-18?

A

Nonmetals

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56
Q

What is the group name of “stair step” between groups 13-16?

A

Metalloids

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57
Q

What is the group name of the groups to the left of metalloids?

A

Other metals

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58
Q

What do the lewis dot diagrams show?

A

The valence electrons

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59
Q

What is a extensive property?

A

Properties that depend on the amount of a substance present (mass, length, volume)

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60
Q

What is an intensive property?

A

Properties that are independent on the amount of substance present (density)

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61
Q

Can the inability of a substance to change into another substance be considered a chemical property?

A

Yes

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62
Q

What is a phase change?

A

A transition of matter from one state to another

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63
Q

How do you know a chemical change has occurred? Give evidence.

A

The observation that the product has different properties than the reactants is evidence that a chemical reaction has taken place because they always produce a change in properties

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64
Q

What is the definition of mass?

A

A measurement that reflects the amount of matter

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65
Q

What is the definition of weight?

A

A measurement of the amount of matter and the Earth’s gravitational pull on that matter

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66
Q

What is the definition of volume?

A

The space occupied by an object

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67
Q

What is the definition of density?

A

A physical property of matter defined as the amount of mass per unit volume

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68
Q

What is the definition of an atom?

A

The smallest particle of matter that retains the properties of the element

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69
Q

What is the definition of a molecule?

A

A group of atoms

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70
Q

What is the definition of a pure substance?

A

Matter with a uniform and unchanging composition

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71
Q

What is the definition of a heterogeneous mixture?

A

A mixture that does not blend smoothly throughout and in which the individual substances remain distinct

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72
Q

What is the definition of a homogeneous mixture?

A

A mixture that has constant composition throughout; it always has a single phase

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73
Q

What is a theory?

A

An explanation of a natural phenomenon based on many observations and investigations over time

74
Q

What is scientific law?

A

A relationship in nature that is supported by many experiments

75
Q

What is pure research?

A

Research for the sake of knowledge

76
Q

What is applied research?

A

Research to solve a specific problem

77
Q

What is a substance?

A

Matter that has a definite and uniform composition (a.k.a a chemical)

78
Q

What is the SI base unit of time?

A

Seconds

79
Q

What is the SI base unit of length?

A

Meters

80
Q

What is the SI base unit of mass?

A

Kilograms

81
Q

What is the SI base unit of temperature?

A

Kelvins

82
Q

What is the SI base unit of amount of a substance?

A

Moles

83
Q

What is the SI base unit of an electric current?

A

Ampere

84
Q

What is the SI base unit of luminous intensity?

A

Candela

85
Q

What is base unit?

A

A defined unit in a system of measurement that is based on an object or event in the physical world

86
Q

What is a derived unit?

A

A unit that is defined by a combination of base units

87
Q

What is dimensional analysis?

A

A systematic approach to problem solving that used conversion factors to convert from one unit to another

88
Q

What is a conversion factor?

A

A ratio of equivalent values having different units

89
Q

What must a conversion factor in dimensional analysis accomplish?

A

Must cancel one unit and introduce a new one

90
Q

What is error?

A

The difference between an experimental value and an accepted value

91
Q

What is the percent error equation?

A

%Error= |experimental value- accepted value|/ accepted value x 100

92
Q

What is percent error?

A

Expresses error as a percentage of the accepted value

93
Q

What are significant figures?

A

The reported digits indicated from the precision of a measurement

94
Q

What are the rules of significant figures?

A

Nonzero numbers are always significant.

All final zeroes to the right of the decimal are significant.

Any zero between significant figures is significant.

Placeholder zeroes are not significant. To remove placeholder zeros, rewrite the number in scientific notation

Counting numbers and defined constants have an infinite number of significant figures

95
Q

What is the rule of significant figures for addition and subtraction?

A

Answer must have the same number of digits to the right of the decimal as the original value with the fewest number of digits

96
Q

What is the rule of significant figures for multiplication and division?

A

Answer must have the same number of significant figures as the value with the fewest significant figures

97
Q

What does endothermic mean?

A

Absorbs or uses heat energy

98
Q

What does exothermic mean?

A

Releases heat energy

99
Q

What is an independent variable?

A

Variable that scientists deliberately change during an experiment

100
Q

What is a dependent variable?

A

Variable whose value depends on or changes in response to the independent variable

101
Q

What does gas refer to?

A

A substance that is naturally in the gaseous state at room temperature

102
Q

What does vapor refer to?

A

The gaseous state of a substance that is a solid or a liquid at room temperatures

103
Q

True or False: A substance can often be identified by its intensive properties

A

True

104
Q

What is a physical change?

A

A change which alters a substance without changing its composition

105
Q

What is a chemical change?

A

A process that involves one or more substances changing into new substances

106
Q

What terms generally refer to chemical reactions?

A

Decompose, explode, rust, oxidize, corrode, tarnish, ferment, burn, or rot

107
Q

The starting substances in a chemical reaction are called what?

A

Reactants

108
Q

The new substances formed in a chemical reaction are called what?

A

Products

109
Q

True or False: A chemical reaction always produces a change in properties?

A

true

110
Q

What is the equation form of the law of conservation of mass?

A

Mass reactants = mass products

111
Q

What is an element?

A

A pure substance that cannot be separated into simpler substances by physical or chemical means

112
Q

Why is the periodic table called periodic?

A

The pattern of similar properties repeats from period to period

113
Q

True or False: Elements in the same group have similar chemical and physical properties.

A

True

114
Q

What is a compound?

A

Made up of two or more different elements that are combined chemically in a fixed ratio

115
Q

What is the percent by mass ratio?

A

Ratio of mass of each element to the total mass of the compound expressed as a percentage

116
Q

What is the percent by mass equation?

A

mass of element/mass of compound x 100

117
Q

What is a mixture?

A

A combination of two or more pure substances in which each pure substance retains its individual chemical properties

118
Q

True or False: Homogeneous mixtures are also referred to as solutions

A

True

119
Q

What is an alloy?

A

A homogeneous mixture of metals

120
Q

True or False: heterogeneous mixtures composed of solids and liquids are easily separated by filtration

A

True

121
Q

What is filtration?

A

A technique that uses a porous barrier to separate a solid from a liquid

122
Q

True or False: Many homogeneous mixtures can be separated by distillation

A

True

123
Q

What is distillation?

A

A physical separation technique that is based on differences in the boiling points of the substances involved

124
Q

What is sublimation?

A

The process during which a solid changes to vapor without melting without going through the liquid phase

125
Q

True or False: Sublimation can be used to separate two solids present in a mixture when one of the solids sublimates but not the other

A

True

126
Q

What is an atom?

A

Smallest particle of matter that retains the properties of the element

127
Q

Protons and neutrons have their own structures and are composed of subatomic particles called what?

A

Quarks

128
Q

What is the atomic number?

A

Refers to the number of protons in an atom

129
Q

True or False: All atoms of an element have the same number of protons and electrons, but the number of neutrons might differ.

A

True

130
Q

What is the mass number?

A

the sum of the atomic number (number of protons) and neutrons in the nucleus

131
Q

How do you write isotopes in isotope notation?

A

Write the element symbol, top number is the mass number (the number that should be different), bottom number is the atomic number (number that should always stay the same)

132
Q

True or False: Each element’s atomic emission spectrum is unique and can be used to identify an element

A

True

133
Q

What is the ground state?

A

Lowest allowable energy state of an atom, atoms normally exist with electrons at the lowest possible energy levels closest to the nucleus

134
Q

Is it true that when an atom gains energy, it is said to be in an excited state?

A

Yes

135
Q

What is the principal quantum number?

A

N

136
Q

What does the quantum number n indicate?

A

The energy level

137
Q

What is electron configuration?

A

The arrangement of electrons in an atom

138
Q

What does the aufbau principle state?

A

Electrons fill orbitals with the lowest energy first

139
Q

What does the Pauli Exclusion Principle state?

A

Only 2 electrons can be in the same orbital at a time

140
Q

What is Hund’s Rule?

A

Electrons will fill all the orbitals with the same energy level and quantum numbers singly before pairing begins

141
Q

What did DeBrogli propose?

A

Electrons act like waves in a confined space

142
Q

What is a valence electron?

A

Electrons in the atom’s outermost orbitals

143
Q

What is the law of conservation of energy?

A

Energy can neither be created nor destroyed only converted from one form of energy to another

144
Q

What is an isotope?

A

Same number of protons but different number of neutrons

145
Q

What does the mass number equal?

A

Equals the total number of protons and neutrons

146
Q

What are the names of the electron orbital shapes?

A

S, p, d, f

147
Q

How many orbitals and electrons does the s-orbital have? What’s its spherical shape?

A

1 orbital, 2 electrons max, spherical shape

148
Q

How many orbitals and electrons does the p-orbital have? What’s its spherical shape?

A

3 orbitals, 6 electrons max, dumbbell shape

149
Q

How many orbitals and electrons does the d-orbital have? What’s its spherical shape?

A

5 orbitals, 10 electrons max, clover shape & 1 donut shape

150
Q

How many orbitals and electrons does the f-orbital have? What’s its spherical shape?

A

7 orbitals, 14 electrons max, double dumbbell shape

151
Q

What is a period?

A

A horizontal row of elements in the periodic table that has increasing atomic number

152
Q

What is a group?

A

A vertical column of elements in the periodic table

153
Q

What is electron shielding?

A

Inner electrons shield outer electrons from the nucleus

154
Q

How is the periodic table organized?

A

The periodic table is organized left-to-right and top-to-bottom by increasing atomic number. This pattern of order with the periodic table is called periodicity.

155
Q

What are the general properties for the alkali metals?

A

Extremely reactive, reacts with water, very soft, easily cut, good conductor of electricity

156
Q

What are the general properties for alkali earth metals?

A

Highly reactive (not as much as group 1), reacts with oxygen in the air, higher melting points that the alkali metals

157
Q

What are the general properties for transition metals?

A

Less reactive than alkali metals and alkali earth metals, most are solid at room temperature (Hg is a liquid), good conductors of heat and electricity

158
Q

What are the general properties for halogens?

A

Most reactive group of nonmetals, reacts to form salts, likely to react with alkali metals, found in sea water and within Earth’s crust, all are liquids at room temperature (except Bromine), can be poisonous when they are not combined as compounds

159
Q

What are the general properties for noble gases?

A

Very unreactive due to stable electron configurations, only Kr, Xe, & Rn have been able to form compounds, colorless, odorless, tasteless

160
Q

What are the general properties for metals?

A

Some can react to form poisons, good conductors of heat and electricity, silver/grey in color, malleable

161
Q

What are the general properties for non-metals?

A

Easily gains electrons, exists at room temperature as a gas or a solid, poor conductors of heat and electricity

162
Q

What are the general properties for semiconductors (metalloids)?

A

Shares properties of metals and nonmetals, not typically reactive, poor conductors of heat and electricity

163
Q

What are the general properties for lanthanides?

A

Highly reactive with halogens, burns easily in air, soft, silverish color, “rare earth metals”

164
Q

What are the general properties for actinides?

A

Radioactive, highly reactive with most nonmetals, soft, silverish metals, “inner transition metals”

165
Q

What is the trend for atomic radius?

A

Increases down a group, decreases across a period

166
Q

Why does the trend for atomic radius occur?

A

Increases down due to more energy levels getting full, electron shielding remains the same across a period

167
Q

What is a trend?

A

A predictable change in a particular direction

168
Q

What is ionization energy?

A

The energy required to remove an electron from an atom or an ion

169
Q

What is the trend for ionization energy?

A

Decreases down a group, increases across a period

170
Q

What is the trend for electron shielding?

A

Increases down a group, remains the same across a period

171
Q

What is the trend for atomic radius?

A

Increases down a group, decreases across a period

172
Q

What is electronegativity?

A

A measure of the ability of an atom in a chemical compound to attract electrons

173
Q

What is electron affinity?

A

The energy change when a neutral atom gains an electron

174
Q

What is the trend for electron affinity?

A

Decreases down a group, increases across a period

175
Q

What is the trend for ionic radius?

A

Increases down a group, cations & anions decrease

176
Q

What are more physical properties of metals?

A

Luster, good conductors of heat & electricity, high density, high melting point, ductile, malleable

177
Q

What are chemical properties of metals?

A

Easily lose electrons, called electron donors, corrodes easily, react with acids

178
Q

What are the physical and chemical properties of nonmetals?

A

Gain electrons, electron acceptors, solids are dull and brittle, poor conductors, low melting and boiling points

179
Q

What is an alloy according to the note slides?

A

A homogeneous mixture of two or more metals

180
Q

When do high melting and boiling points occur?

A

When an orbital is half full

Honors Chemistry (13 decks)

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