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Gen Chemistry 1 > Gen Chem Exam 1 > Flashcards

Gen Chem Exam 1 Flashcards

1
Q

Chemistry

A

The study of the composition, structure, properties, and reactions of matter.

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2
Q

Chemical

A

A substance that always has the same composition and properties wherever it is found.

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3
Q

Elements

A

Pure substances from which all other things are built.

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4
Q

Elements can not…

A

be broken down into simpler substances

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5
Q

What are examples of elements?

A

ALL elements on the periodic table!

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6
Q

Chemical Symbol

A

Represents the names of the elements (1-2 letters)

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7
Q

What is the chemical symbol for gold?

A

Au

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8
Q

What is the chemical symbol for aluminum?

A

Al

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9
Q

How many elements are on the periodic table?

A

118

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10
Q

Elements on the periodic table are in order of…

A

Increasing atomic mass

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11
Q

What is the difference between periods and groups?

A

Periods: Horizontal rows
Groups: Vertical columns

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12
Q

What does group A on the periodic table represent?

A

Representative Elements

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13
Q

What does group B on the periodic table represent?

A

Transition Elements

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14
Q

What is group 1A?

A

Alkali Metals (metals) - VERY reactive

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15
Q

What is group 2A?

A

Alkaline Earth Metals (metals) - Reactive

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16
Q

Is group 1A or 2A more reactive?

A

1A

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17
Q

What is group 7A?

A

Halogens (metalloids and nonmetals)

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18
Q

What is group 8A?

A

The Noble Gases (gases)

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19
Q

Metals

A

Shiny, ductile, and conduct heat/electricity

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20
Q

What is the one metal that is not a solid?

A

Mercury (Hg) = Liquid

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21
Q

Metalloids

A

-Contain properties of metals and nonmetals.
-Used/modified as semiconductors and insulators

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22
Q

What is the order of best conductors?

A
  1. Metal
  2. Metalloids
  3. Nonmetals
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23
Q

Nonmetals

A

-Dull, brittle, and poor conductors
-Good insulators

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24
Q

Nonmetals have low…

A

densities and melting points

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25
Q

Atom

A

The smallest particle of an element that retains the characteristics of the same element.

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26
Q

Daltons Atomic Theory

A
  • All matter is made up of atoms.
  • Atoms in one element are the same/different than those in another element.
  • Atoms can be combined to form compounds.
  • Atoms can be combined, separated, and rearranged in chemical reactions.
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27
Q

Compounds have a constant…

A

Composition

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28
Q

JJ Thompson’s Cathode Ray

A
  • Cathode ray contains negative charged particles.
  • The particles have a smaller mass than an atom
    = electrons
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29
Q

Was JJ Thompson’s Cathode Ray experiment accepted?

A

Yes, but was controversial at first.

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30
Q

Thompson’s Plum Pudding Model

A
  • The plum pudding modeled an atom
  • Electrons are protons are randomly distributed in a positively charged cloud.
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31
Q

Alike charges ___, while opposite charges___

A

Repel, Attract

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32
Q

Rutherford’s Gold Foil Experiment (1911)

A
  • Positive charged particles were aimed at gold foil
  • Most particles went straight though the foil
  • Some particles were occasionally deflected
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33
Q

Gold Foil Experiment conclusion….

A

There must be a small, dense, (+) charged nucleus in the atom that deflects the (+) charged particles when close.

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34
Q

Nucleus

A

Center of the atom that contains protons and neutrons

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35
Q

What does the nucleus represent?

A

The mass of the atom

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36
Q

Atomic Mass Unit (amu)

A

1 amu = 1/12 the mass of a carbon12 atom
or
1 Dalton in biology

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37
Q

Proton

A

-p or p+
-charge of 1+
- mass = 1
- Located in the nucleus

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38
Q

Neutron

A
  • n or n0
  • charge of 0
  • mass = 1
  • Located in the nucleus
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39
Q

Electron

A
  • (e-)
  • charge of 1-
  • mass = 0
  • Located outside the nucleus
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40
Q

What do all atoms of the same element have?

A

The same # of protons and the same atomic #

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41
Q

Atomic Number

A

A whole number that helps locate and identify elements.

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42
Q

The atomic number =

A

The # of protons

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43
Q

Mass Number

A

The whole number that represents the total number of particles in the nucleus of an atom.

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44
Q

The mass number =

A

protons + neutrons

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45
Q

Does the mass number appear on the periodic table?

A

No

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46
Q

The number of protons =

A

The number of electrons

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47
Q

Ion

A

When the charge of an atom does not equal 0 (different number of electrons than protons).

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48
Q

Cation

A
  • Positively charged
  • More protons than electrons
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49
Q

Anion

A
  • Negatively charged
  • More electrons than protons
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50
Q

Isotopes

A

Atoms of the same element that have
- different number of neutrons
- different atomic mass number

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51
Q

What are isotopes distinguished by?

A

Atomic symbols (Mg24 vs Mg25)

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52
Q

Average Atomic Mass

A

The calculated atomic mass of all isotopes of an element.
(Mg24 + Mg25 +Mg26 = avg atomic mass)

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53
Q

Protons + Neutrons =

A

Atomic Mass

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54
Q

The energy of an atom is determined by…

A

Electrons

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55
Q

Electrical Energy

A

Energy emitted as visible light and heat
-Travels through space

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56
Q

Emitted Energy =

A

Electromagnetic Radiation

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57
Q

What is an example of electrical energy?

A

An electric stove

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58
Q

Electromagnetic Radiation

A

Energy particles that move as waves

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59
Q

Photons

A

Particles of electromagnetic radiation

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60
Q

Wavelength

A

Distance between the peaks of waves

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61
Q

High energy radiation has ___ wave lengths

A

Short

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62
Q

Low energy radiation has ___ wave lengths

A

Long

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63
Q

Electromagnetic Spectrum

A

Arrangement of wavelengths of electromagnetic radation

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64
Q

The visible range of light is…

A

700-400 nm

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65
Q

Atomic Spectrum

A

Lines of color separated by dark areas

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66
Q

How is the atomic spectrum created?

A

When light from a heated element passes through a prism.

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67
Q

Each element has it’s own ___ spectrum.

A

unique

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68
Q

Energy Level

A

Each electrons specific energy in an atom

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69
Q

As electrons move farther away from the nucleus, their energy level…

A

Increases

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70
Q

The arrangment of electrons in energy levels determine…

A

Physical and chemical properties in an element

71
Q

Energy emitted =

A

The difference between the two energy levels

72
Q

As electrons move to a higher energy level…

A

Energy is absorbed

73
Q

As electrons move to a lower energy level…

A

Light is emitted

74
Q

Orbitals

A

3D volume where electrons have the highest chance of being found

75
Q

S Orbital

A
  • Found in all energy levels
  • Holds up to 2 electrons
  • Sphere shape
76
Q

P Orbital

A
  • Starts in energy level 2
    -Holds up to 6 electrons
  • Dumbell shaped
77
Q

D Orbital

A
  • Starts in energy level 3
  • Holds up to 10 electrons
  • Two dumbells or donut shaped
78
Q

Pauli Exclusion

A

Each orbital can hold up to 2 electrons
- Magnetic spins must cancel

79
Q

Electron Configuration

A

Indicates placement of electrons in an atom.
- Fill energy and sub levels in order of increasing energy.

80
Q

“Ground State”

A

Lowest energy configuration for that atom

81
Q

Orbital Diagrams

A

Use boxes to show how electrons
- are arranged in orbitals
-fill orbitals from lowest to highest
-fill orbitals 1 sub level at a time

82
Q

Cr and Cu are…

A

half filled in last S sub level to increase stability

83
Q

Valence Electrons

A

Electrons in the outermost energy level

84
Q

What orbitals do valence electrons occupy?

A

S and P

85
Q

What does the A group number represent?

A

The number or valence electrons.

86
Q

Lewis Symbol

A

Represent the valence electrons as dots placed on sides of the element symbol.

87
Q

Atomic size

A

Increases down, decreases right

88
Q

Atomic Radius

A

Distance between nucleus and outermost electrons

89
Q

Ionization Energy

A

Energy required to remove one of the outermost electrons

90
Q

Ionization energy decreases___ and increases ____.

A

down, right

91
Q

Ionization energy is low for ___ and high for ___

A

metals, nonmetals

92
Q

Metallic Character

A

increases down, decreases right (more prevalent for metals)

93
Q

Matter

A

The material that makes up all things.
- Has mass and occupies space

94
Q

How is matter classified?

A

According to it’s composition.

95
Q

Pure Substance

A

Fixed/definite composition

96
Q

What are the two types of pure substances?

A

Elements and Compounds

97
Q

Element

A

Composed of 1 type of atom

98
Q

What are examples of elements?

A

Any element on the periodic table.

99
Q

Compound

A

Composed of 2+ elements, always combined in the same proportion

100
Q

What are examples of compounds?

A

H20 (water), H2O2 (hydrogen peroxide), and NaCl (table salt)

101
Q

Mixture

A

A type of matter that consists of
- 2+ physically mixed substances but not chemically combined
- 2+ substances in different proportions
- Can be separated in physical methods

102
Q

What are the types of mixtures?

A

Homogenous and Heterogenous

103
Q

Homogenous Mixture

A

A mixture with a composition that is uniform throughout

104
Q

Are the different parts in a homogenous mixture visible?

A

No

105
Q

A homogenous mixture can also be called a…

A

Solution

106
Q

What are examples of homogenous mixtures?

A

Helium and aluminum foil

107
Q

Heterogenous Mixture

A

A mixture whose composition varies from one part to another.

108
Q

Are the different parts in a heterogenous mixture visible?

A

Yes

109
Q

What are examples of heterogenous mixtures?

A

Pasta with sauce and the air we breath

110
Q

What are the three types of matter?

A

Solid, liquid, gas

111
Q

Solids have ___ shape and ___ volume

A

definite, definite

112
Q

The particles in a solid are…

A

close together and have a fixed arrangment

113
Q

What is the speed of particles in a solid?

A

Very slow

114
Q

Liquids have a ___ shape and ___ volume

A

indefinite, definite

115
Q

True or false: Liquids take on the shape of their container.

A

TRUE

116
Q

The particles in a liquid are…

A

close together and mobile

117
Q

What is the speed of particles in a liquid?

A

Moderatley fast

118
Q

Gases have ___ shape and ___ volume.

A

indefinite, indefinite

119
Q

True or false: Gases take on the same shape and volume as it’s container.

A

TRUE

120
Q

The particles in a gas are…

A

Far apart and not uniform

121
Q

What is the speed of particles in a gas?

A

VERY fast

122
Q

Physical Properties

A

Characteristics observed/measured without changing the identity of a substance

123
Q

What are examples of physical properties?

A

Shape, color, density, boiling/freezing points

124
Q

Physical Change

A
  • No change in identity/composition
  • Change in state of matter
  • Change in physical shape
125
Q

What are examples of physical change?

A

Water boiling to form water vapor

126
Q

Chemical Properties

A

Describe the ability of a substance to…
- Interact with other substances
- Change into a new substance

127
Q

Chemical Change

A

An original substance is turned into a one or more new substances with
- New composition
- New chemical properties
- New physical properties

128
Q

What are examples of chemical change?

A

Digesting food or fireworks exploding

129
Q

Temperature

A

Measures how hot/cold an object is compared to another object

130
Q

What does temperature indicate?

A

Heat flow between an object of a high temp and another of a lower temp

131
Q

How is temperature measured?

A

Using a thermometer

132
Q

What are temperature scales based on?

A

The difference between boiling and freezing points of water

133
Q

What are temperature scales divided into?

A

Degrees

134
Q

What are the boiling and freezing points of Celcius?

A

Boiling = 100
Freezing = 0

135
Q

What are the boiling and freezing points of Fahrenheit?

A

Boiling = 212
Freezing = 32

136
Q

What is absolute zero?

A

The coldest temperature possible
- 0 Kelvin
- -273.15 Celcius

137
Q

Does Kelvin use a degree symbol or negative numers?

A

No

138
Q

Energy

A

Ability to do work
- Makes objects move and stop

139
Q

Work =

A

Force x Distance

140
Q

What are the two types of energy?

A

Kinetic and Potential

141
Q

Kinetic Energy

A

Energy of motion

142
Q

What are examples of kinetic energy?

A
  1. Working out
  2. Driving a car on a road
  3. Water flowing over a dam
143
Q

Potential Energy

A

Energy based on the position of an object or chemical composition of a substance

144
Q

What are examples of potential energy?

A
  1. Compressed spring
  2. Water at the top of a dam
  3. Chemical bonds in gas, coal or food
145
Q

Potential energy is converted into…

A

Kinetic Energy

146
Q

Heat

A

Energy associated in the movement of particles

147
Q

The faster the particles move, the ___ the heat/thermal energy

A

Higher

148
Q

What is an example of heat?

A

An ice cube melting
- Energy is needed to change from solid to liquid

149
Q

What are the SI units of energy?

A

Joule (J) or kilojoules (kJ)

150
Q

How many kilojoules are in a Joule?

A

1000 kJ

151
Q

What are the other units of energy?

A

calories (cal) or kilocalories (kcal)

152
Q

How many kilocalories are in a calorie?

A

1000 kcal

153
Q

Calorie

A

The amount of energy (heat) needed to raise the temperature of 1g H2O by 1 degree C

154
Q

C (uppercase) stands for

A

Nutritional Calorie

155
Q

How many calories are in a C?

A

1000 calories

156
Q

How many C are in a kcal?

A

1

157
Q

Calorimeters

A

Used to measure energy values of substances

158
Q

Specific Heat

A

The amount of heat that raises the temperature of exactly 1g of a substance by 1 degree C

159
Q

Specific Heat =

A

heat / mass x change in temperature

160
Q

True of False: Each substance has a unique SH.

A

TRUE

161
Q

Changes of State

A

Converting one state to another

162
Q

Evaportation

A

Liquid molecules ON SURFACE gain enough energy to convert to a gas.

163
Q

Condensation

A

Gas molecules lose energy to convert to a liquid

164
Q

Boiling

A

ALL liquid molecules acquire energy to convert to gas.
- Bubbles appear throughout the liquid

165
Q

Condensation and ___ are reversible processes.

A

Boiling

166
Q

Melting

A

Solid changes to a liquid at the melting point temperature.

167
Q

Freezing

A

Liquid changes to a solid at the freezing point temperature.

168
Q

Melting and ___ are reversible processes.

A

Freezing

169
Q

The melting and freezing point is…

A

0 degrees C

170
Q

Heat of Fusion is the amount of heat

A
  1. Released when 1g of liquid freezes.
  2. Needed to melt 1g of solid
171
Q

Heat of Vaporization is the amount of heat…

A
  1. Absorbed to change 1g of liquid to gas at the boiling point.
  2. Released when 1g of gas changes to liquid at the condensation point.
172
Q

Heating Curve

A

A digram that shows temperature increase and change of state as heat is added.

173
Q

Cooling Curve

A

A diagram that shows temperature decrease and change of state as heat is removed.

Gen Chemistry 1 (10 decks)

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