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Physical Science 9th Grade > Science Chapter 13-14 > Flashcards

Science Chapter 13-14 Flashcards

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1
Q

The organized study of the composition and interactions of matter.

A

Chemistry

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2
Q

The foundation for the understanding of matter.

A

Atomic theory of matter

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3
Q

Who created the atomic theory of matter?

A

Dalton

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4
Q

Tiny particles that compose all matter.

A

Atoms

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5
Q

A substance composed of a single type of atom.

A

Element

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6
Q

A substance composed of atoms of two or more elements bonded together.

A

Compound

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7
Q

A substance that is composed of several pure substances that are physically mixed but not chemically united.

A

Mixture

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8
Q

A unique abbreviation given to each element.

A

Chemical symbol

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9
Q

Any of the smaller particles of matter of which atoms are composed.

A

Subatomic particles

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10
Q

The dense central core of an atom made of protons and neutrons.

A

Nucleus

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11
Q

Subatomic particle that carries a positive electrical charge and determines the identity of an atom.

A

Proton

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12
Q

The number of protons in the nucleus of an atom.

A

Atomic number

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13
Q

Subatomic particle that is electrically neutral with no electric charge.

A

Neutron

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14
Q

Any of a group of atoms that are the same element but have different numbers of neutrons.

A

Isotope

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15
Q

Any of the small particles that compose protons and neutrons.

A

Quarks

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16
Q

_____ quarks are needed to make a proton or a neutron.

A

Three

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17
Q

Subatomic particle that is found outside the nucleus and carries a negative electric charge equal in strength to a proton’s positive charge.

A

Electron

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18
Q

Any of the concentric layers surrounding the nucleus in which electrons can be found.

A

Electron shell

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19
Q

An atom normally has the ______ number of protons and electrons.

A

Same

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20
Q

An atom that has an electric charge because of losing or gaining electrons.

A

Ion

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21
Q

Positive ions are

A

Cations

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22
Q

Negative ions are

A

Anions

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23
Q

The total number of protons and neutrons in the nucleus of an atom or isotope.

A

Mass number

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24
Q

A unit used to measure the masses of atoms; equal to exactly 1/12 the mass of a carbon-12 atom.

A

Atomic mass unit

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25
Q

The mass of an atom in atomic mass units is approximately equal to the ________

A

Mass number

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26
Q

The average mass of all the natural isotopes of an element, calculated according to the isotopes’ relative abundances.

A

Average atomic mass

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27
Q

The theory stating that tiny particles like electrons do not absorb or release energy in a smooth flow.

A

Quantum theory

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28
Q

The most familiar model of the atom, which pictures the nucleus surrounded by electrons that move in circular orbits at specific energy levels.

A

Bohr model

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29
Q

An atomic model that describes the electrons as waves around the nucleus.

A

Wave-mechanical model

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30
Q

Electrons have characteristics of both ________ and ________.

A

particles, waves

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31
Q

The principle stating that it is impossible to measure both the position and velocity of an electron with certainty.

A

Heisenberg uncertainty principle

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32
Q

A model of the atom that interprets the mathematical equations of the wave-mechanical model representing the probability of finding an electron at a given point.

A

Electron-cloud model

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33
Q

The region within an atom in which electrons move.

A

Orbital

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34
Q

A set of numbers that mathematically represents the overall motion of an electron.

A

Quantum numbers

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35
Q

The principle stating that no two electrons in an atom can have the same four quantum numbers.

A

Pauli exclusion principle

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36
Q

The nuclei of most atoms are ______, but the nuclei of some isotopes are ______, capable of breaking up or otherwise changing into another type of atom.

A

stable, unstable

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37
Q

Particles or electromagnetic waves given off when an atomic nucleus breaks up or undergoes a change.

A

Nuclear radiation

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38
Q

Any substance that is unstable.

A

Radioactive

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39
Q

The breakup or change of an atomic nucleus from a higher energy state to a lower energy state, emitting radiation.

A

Radioactive decay

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40
Q

The length of time required for one-half of an original substance to decay into a new substance.

A

Half life

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41
Q

The half-life of radium-226 is _______ years.

A

1,600

42
Q

Radioactive decay that occurs when an unstable atom ejects a clump of 2 protons and 2 neutrons.

A

Alpha decay

43
Q

Radioactive decay that occurs when a neutron in an atom’s nucleus changes into a proton, emitting an electron.

A

Beta decay

44
Q

Radioactive decay that occurs when an excited (unusually energetic) nucleus releases energy without a change in the number of protons or neutrons.

A

Gamma decay

45
Q

Nuclear radiation that can harm living things by disrupting the chemical process within cells; includes alpha particles, beta particles, and gamma rays.

A

Ionizing radiation

46
Q

The process whereby a heavy nucleus is split into several pieces by bombarding it with neutrons.

A

Nuclear fission

47
Q

The situation in which free neutrons released by nuclear fission cause other atoms to undergo nuclear fission and release more neutrons.

A

Chain reaction

48
Q

Chain reaction is known as a ______ effect.

A

Domino

49
Q

The minimum amount of fissionable material that must be present for a chain reaction to occur.

A

Critical mass

50
Q

A device that works by initiating an uncontrolled nuclear fission chain reaction.

A

Atomic bomb

51
Q

A device that harnesses controlled fission to produce useful energy.

A

Nuclear reactor

52
Q

A nuclear reactor that recycles spent nuclear fuel to produce more than it uses.

A

Breeder reactor

53
Q

The process of combining two nuclei to form a heavier nucleus and thereby releasing energy

A

Nuclear fusion

54
Q

A weapon that uses nuclear fusion to release a tremendous amount of energy.

A

Hydrogen bomb

55
Q

Any of the electrons in the outer shell of an atom.

A

Valence electron

56
Q

The rule stating that an atom tends to react in a way that fills its valence shell with eight electrons.

A

Octet rule

57
Q

The law that states that elements show regular and repeating, or periodic, properties when they are arranged by their increasing atomic numbers.

A

Periodic law

58
Q

A table of the elements arranged by atomic number and number of valence electrons.

A

Periodic table of the elements

59
Q

A row of the periodic table.

A

Period

60
Q

A column on the periodic table.

A

Group

61
Q

Any of the elements in groups 1,2, and 13-18.

A

Main-group element

62
Q

Any of the group of elements that are typically hard, dense, shiny solids; are good conductors of heat and electricity; and have high melting points.

A

Metal

63
Q

Any of the group of elements that are typically poor conductors of electricity and heat.

A

Nonmetal

64
Q

Any of the solid elements that have properties intermediate between metals and nonmetals.

A

Semimetal

65
Q

Any element in group 1.

A

Alkali metal

66
Q

The first most abundant element in the human body.

A

Oxygen

67
Q

The second most abundant element in the human body.

A

Carbon

68
Q

The third most abundant element in the human body.

A

Hydrogen

69
Q

Any element in group 2.

A

Alkaline earth metal

70
Q

Any element in groups 3-12.

A

Transition metals

71
Q

Any of the metals that lie beneath the main body of the periodic table, between groups 3 and 4; the Lanthanoids and Actinoids.

A

Inner transition metal

72
Q

Group 15 is referred to as the _______.

A

Pnictogens

73
Q

Group 16 is called _______.

A

Chalcogens

74
Q

Meaning “salt former” is any element in group 17.

A

Halogen

75
Q

Any element in group 18.

A

Noble gas

76
Q

a group of two or more atoms linked by chemical bonds to form distinct units

A

molecule

77
Q

a _________ is a combination of chemical symbols and numbers showing the type and number of atoms in each compound

A

chemical formula

78
Q

Oxygen and Hydrogen are _________

A

diatomic

79
Q

C60 is named after __________

A

Buckminsterfullerene

80
Q

the sum of the atomic masses of all the atoms in a molecule

A

molecular mass

81
Q

substances composed of atoms of two or more elements bonded together

A

compounds

82
Q

molecules that have the same molecular formula but different structural formulas

A

isomer

83
Q

a substance that has the same physical properties throughout and consists of only one type of atom, one type of molecule, or one nonmolecular compound; all pure substances are either elements or compounds

A

pure substances

84
Q

a substance that has the same physical properties throughout the substance

A

homogenous

85
Q

three-dimensional representation of a molecule that shows its shape and the position of its atom

A

molecular model

86
Q

a substance composed of several pure substances that are physically mixed but not chemically united.

A

mixture

87
Q

a homogeneous mixture that exists because of attraction between atoms, molecules, or ions.

A

solution

88
Q

a substance in a solution that is dissolved.

A

solute

89
Q

a substance in a solution that does the dissolving.

A

solvent

90
Q

The key difference between solutions and pure substances is that, like all mixtures, a solution is a ________ mixture, not a ________ combination.

A

physical, chemical

91
Q

describes a mixture in which the molecules of the mixed substances are not completely mixed.

A

heterogenous

92
Q

a mixture containing tiny suspended clumps or particles.

A

colloid

93
Q

the appearance of a blue-tinged milky or cloudy effect within a colloid when a light shines through it.

A

tyndall effect

94
Q

a heterogeneous mixture whose particles are large enough that they will settle.

A

suspension

95
Q

an attractive force that links atoms to form molecules and compounds.

A

chemical bond

96
Q

The most important factor affecting how chemical bonds form is the number of _______ in the valence shell of each atom involved.

A

electrons

97
Q

a chemical bond resulting from the sharing of valence electrons between atoms.

A

covalent bond

98
Q

Covalent bonds typically form between two ________.

A

nonmetals

99
Q

a covalent bond involving an electron.

A

single bond

100
Q

a covalent bond formed by the sharing of two pairs of electrons.

A

double bond

101
Q

a covalent bond in which three pairs of electrons are shared.

A

triple bond

102
Q

a diagram showing the locations of all the atoms and valence electrons in a molecule or ion.

A

lewis structure

Physical Science 9th Grade (11 decks)

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