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APES > III - Matter & Energy Resources: Types & Concepts > Flashcards

III - Matter & Energy Resources: Types & Concepts Flashcards

1
Q

matter

A

anything that has mass & takes up space.

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2
Q

What forms can matter be in?

A

Elements
Isotopes
Ions
Compounds

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3
Q

Elements

A

the distinct building blocks that form matter; made

up of a single type of atom

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4
Q

Atom

A

the smallest unit of matter unique to

an element

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5
Q

How many known elements are there?

A

112 with 92 being natural and 20 being synthesized

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6
Q

Components of an atom

A 
PROTONS – positively charged
particles in nucleus
NEUTRONS – uncharged
particles in nucleus
ELECTRONS – negatively
charged particles orbiting
nucleus
other subatomic particles
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7
Q

Characteristics of an atom

A

Atomic number

Mass number

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8
Q

Atomic number

A

number of PROTONS in a nucleus; defines an element.

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9
Q

Mass number

A

total number of neutrons (mass =1) &

protons (mass =1); mass of electrons near 0

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10
Q

Periodic Table of Elements

A

Elements organized by atomic number; groups of elements in same column have SIMILAR properties.

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11
Q

Some important elements

A 
Carbon
Hydrogen
Nitrogen
Oxygen
Phosphorus
Calcium
Iron
Sodium
Potassium
Sulfur
Bromine
Chlorine
Fluorine
Aluminum
Mercury
Lead
Silicon
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12
Q

Earth’s crust composition

A 
Oxygen
Silicon
Aluminum
Iron
Calcium
Sodium
Potassium
Magnesium
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13
Q

Isotopes

A

various forms of element that have SAME number of PROTONS, but DIFFERENT numbers of NEURONS.

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14
Q

Examples of isotopes

A 
C 12
C 14
H 1
H 2
H 3
U 235
U 238
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15
Q

Ions

A

CHARGED molecules formed when atoms of some elements GAIN or LOSE one or more ELECTRONS

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16
Q

Positive ions are known as …

A

Cations

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17
Q

Positive ions examples

A

Na+
Ca+
Fe+
Al3+

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18
Q

Negative ions are known as …

A

Anions

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19
Q

Negative ions examples

A

Cl-
PO4 3-
SO3-

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20
Q

Compounds

A

TWO or more different ELEMENTS held together in

FIXED PROPORTIONS by chemical BONDS.

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21
Q

Ionic bonds

A

STRONG bonds formed by joining OPPOSITELY

charged IONS

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22
Q

ionic bonds example

A

table salt NaCl

Na+ & Cl-

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23
Q

Ionic solid structure

A

three–dimensional ARRAY of oppositely
charged ions held
together by ionic
bonds

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24
Q

Covalent bonds

A

STRONG bonds formed by joining one or more UNCHARGED atoms into MOLECULES by SHARING of
electrons

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25
Q

Covalent bonds example

A

Water molecule H2O

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26
Q

Inorganic molecule

A

compounds NOT originating from
living sources
compounds LACKING C–C & C–H bonds.

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27
Q

Inorganic molecule examples

A 
water H2O
carbon dioxide (CO2)
nitrogen gas (N2)
oxygen gas (O2)
ozone (O3)
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28
Q

Organic molecule

A

compounds CONTAINING C–C &/or C–H bonds (natural & synthetic).

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29
Q

Organic molecule examples

A 
methane (CH4) 
sugars
starch
cellulose
proteins
nucleic acids
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30
Q

Hydrogen bonds

A

WEAK bonds between molecules containing

hydrogen & nonmetallic atoms, in particular between water molecules.

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31
Q

H-bonds in water accounts for what properties of water

A

High surface tension
High heat content
Excellent solvent of ionic compounds

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32
Q

States of matter includes

A

Solid
Liquid
Gas

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33
Q

S to L

A

melting

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34
Q

L to G

A

evaporation

35
Q

G to L

A

condensation

36
Q

L to S

A

freezing

37
Q

Energy is required when going from …

A

Solid to Gas

Takes to break

38
Q

Energy is released when going from …

A

Gas to Solid

Free to form

39
Q

Matter quality

A

measure of how useful a matter resource is

for humans, based on its availability & concentration

40
Q

Energy

A

CAPACITY to do WORK (by performing mechanical,
physical, chemical, or electrical tasks), or to cause HEAT transfer
between two objects at different temperatures.

41
Q

Types of energy includes

A

Kinetic

Potential

42
Q

kinetic energy

A

Energy of motion

43
Q

potential energy

A

stored energy

44
Q

Types of kinetic energy

A

Electrical
Heat
Light

45
Q

Electrical

A

energy of

moving electrons

46
Q

Heat

A

total kinetic energy of

all moving atoms, ions, or molecules

47
Q

Electromagnetic Radiation

A

form of kinetic energy that travels as electromagnetic waves

48
Q

Types of potential energy

A

Chemical

Atomic

49
Q

Chemical energy

A

potential energy stored in chemical

bonds

50
Q

Atomic energy

A

energy
associated with nuclear
structure

51
Q

Energy quality

A

measure of how useful
an energy source is for
humans, in terms of its
CONCENTRATION & ability to perform useful WORK.

52
Q

Levels of energy quality

A

Very high
High
Moderate
Low

53
Q

Very high source of energy

A 
Electricity
Heat above 2500 C
Nuclear fission/ fusion
Concentrated sunlight
High-velocity wind
54
Q

High source of energy

A 
Heat between 1000 and 2500 C
Hydrogen gas
Natural gas
Gasoline
Coal
Food
55
Q

Moderate source of energy

A 
Normal sunlight
Moderate-velocity wind
High-velocity water flow
Concentrated geothermal energy
Moderate heat between 100 and 1000 C
Wood & Crop Wastes
56
Q

Low source of energy

A

Dispersed geothermal energy

Heat below 100 C

57
Q

Physical change

A

involves no change in

chemical composition

58
Q

Chemical change

A

changes in the composition of compounds

59
Q

Physical change example

A

Phase changes

60
Q

Chemical change example

A

Burning of wood or fossil fuel

61
Q

Law of Conservation of Matter

A

In chemical reaction
atoms are never created, destroyed, or changed one into
another; they are ONLY REARRANGED to form different molecules & compounds

62
Q

Nuclear fission

A

a nuclear change in which certain
UNSTABLE isotopes of high mass numbers split into LIGHTER
nuclei & RELEASE ENERGY in the process.

63
Q

Nuclear Chain reaction

A 
MULTIPLE FISSIONS resulting from a POSITIVE  feedback
loop in which each
fission releases
neutrons that cause
MORE fissions to
occur.
64
Q

Nuclear fusion

A

nuclear change in which two isotopes
of light elements are forced TOGETHER to form a HEAVIER
nucleus, RELEASING ENERGY in the process.

65
Q

Do nuclear reactions break the law of conservation of matter?

A

atoms can be CHANGED

energy & matter are CONSERVED because very SMALL amounts of matter converted to energy

66
Q

First law of thermodynamics

A

energy is neither created nor

destroyed, but may be converted from one form to another

67
Q

Second law of thermodynamics

A

when energy is converted from one form to another, SOME of the useful energy is always DEGRADED to LOWER–quality, more DISPERSED energy.

68
Q

Entropy

A 
measure of
DISORDER 
increased
entropy means
increased randomness
or dispersion
69
Q

Eventually unsustainable high-waste, high-throughput societies

A

High quality energy/ matter -> one way high throughput society -> low quality heat, waste

70
Q

sustainable low–waste,

low–throughput societies

A 
Energy recycled
Reduced matter throughput
Low-waste production
Pollution control
Complex
71
Q

Degraded energy generally is in the form of …

A

HEAT

72
Q

In order to maintain a system,

A

continual energy input is needed

73
Q

Nuclear fusion examples

A

Sun

H + H -> He

74
Q

Very high energy tasks

A

Industrial processes

Producing electricity to run electronics

75
Q

High energy tasks

A

Mechanical motion

Industrial processes/ Electricity production

76
Q

Moderate energy tasks

A

Industrial processes, cooking, producing steam, electricity, & hot water

77
Q

Low energy tasks

A

Space heating

78
Q

Atomic energy example

A

energy released

by fission of Uranium–235.

79
Q

Chemical energy example

A

energy in C–C & C–H

bonds of fossil fuels or foods.

80
Q

Electromagnetic radiation examples

A

radio waves, microwaves,

visible light, ultraviolet radiation, & X–rays

81
Q

Kinetic energy examples

A

Moving car

Rock rolling down hill

82
Q

Potential energy examples

A

Stretched rubber band
Rock on top of hill
Water stored behind dam

83
Q

High quality matter includes

A 
Solid
Coal
Gasoline
Salt
Aluminum can
84
Q

Low quality matter includes

A 
Automobile emissions
Gas
Solution of salt in water
Aluminum ore
Coal-fired power plant emissions

APES (26 decks)

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