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NAS 2 > Chemistry PPT > Flashcards

Chemistry PPT Flashcards

1
Q

has mass; occupies space; all living things are made up of it

A

matter

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2
Q

the smallest particle of a substance that still retains its chemical properties

A

atom

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3
Q

List the 4 elements of atom structure.

A

atomic nucleus, protons, neutrons, and electrons

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4
Q

contains two subatomic particles

A

atomic nucleus

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5
Q

List the 2 subatomic particles that make up the nucleus.

A

protons and neutrons

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6
Q

subatomic particles that carry a positive charge

A

protons

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7
Q

subatomic particles that are uncharged

A

neutrons

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8
Q

negatively charged; move around the nucleus

A

electrons

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9
Q

What’s the ratio of electrons to protons in each atom?

A

1:1

same amount of each

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10
Q

number of protons; unique to each atom

A

atomic number

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11
Q

number of protons and neutrons combined

A

atomic mass

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12
Q

atoms with the same number of protons; have the same chemical properties

A

elements

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13
Q

How many known elements are there?

A

117

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14
Q

atoms with the same number of protons but a different number of neutrons; results in different mass numbers; defined by writing in superscript; does not alter the chemical behavior of an atom

A

isotope

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15
Q

isotopes that have significantly different numbers of neutrons as compared to protons; unstable; breakdown over time

A

radioactive isotopes

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16
Q

when radioactive isotopes breakdown over time and energy is released; occurs at a constant rate

A

radioactive decay

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17
Q

substance with a radioactive isotope attached to it

A

tracer

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18
Q

List 3 uses of radioactive isotopes.

A

can insert into the body,
can detect the energy emitted,
useful in other areas of biology

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19
Q

example of a biological use of radioactive isotopes; forms images of body tissue

A

PET scan

Positron-Emission Tomography

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20
Q

What determines if two atoms interact?

A
  1. Molecular Motion

2. Arrangement and Amount of Electrons

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21
Q

molecules in constant motion (speed depends on temp.); reactions occur due to random collisions

A

molecular motion

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22
Q

List what the chance of molecular collision is based on.

A

the density and speed of the molecules

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23
Q

interact with different atoms because they are the furthest out; attracted to the positive nucleus; posses energy; move in orbitals

A

electrons

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24
Q

volume of space that surrounds the nucleus where an electron is most likely to be found

A

orbital

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25
Q

Each orbital holds a maximum of ___ electrons.

A

2

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26
Q

Orbitals closest to the nucleus are ___ in energy.

A

lower

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27
Q

Atoms with full orbitals are ___ stable.

A

most

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28
Q

If there is an empty space in an atom’s orbital, what can happen to that atom?

A

It can interact with another atom.

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29
Q

What are the different shaped orbitals?

A

S, P, and D orbitals

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30
Q

spherical orbital

A

S orbital

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31
Q

dumbbell-shaped orbital

A

P orbital

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32
Q

pear-shaped orbital

A

D orbital

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33
Q

Rather than grouping orbitals by shape, what is an easier method?

A

grouping into energy levels (shells)

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34
Q

a simple way to show how electrons are placed within an atom

A

shell model

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35
Q

shell with the lowest energy; 1 orbital; can hold 2 electrons

A

1st shell

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36
Q

shell with 4 orbitals; can hold up to 8 electrons

A

2nd shell

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37
Q

Atoms with incomplete outer electron shells are ___ reactive.

A

more

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38
Q

What are the 3 ways to fill the outermost shell?

A

gain, lose, or share electrons

39
Q

atoms with a full outermost shell

A

nonreactive atoms

40
Q

another name for a nonreactive atom

A

inert

41
Q

examples of nonreactive atoms

A

Helium, Neon, Argon

42
Q

group of atoms held together by energy

A

molecule

43
Q

the force that holds the atoms in a molecule together

A

chemical bond

44
Q

What are the 3 types of chemical bonds?

A

ionic, covalent (strongest), and hydrogen (weakest)

45
Q

type of bond formed when electrons are gained and lost between two atoms

A

ionic bond

46
Q

form as a result of ionic bonds

A

ions

47
Q

atoms that have lost or gained 1/more electrons; number of protons differs from the number of electrons; have an electric charge (+ / -)

A

ions

48
Q

atom that has lost electrons (electron donor); has a positive charge; has more protons than electrons

A

cation

49
Q

atom that has gained electrons (electron acceptor); has a negative charge; has more electrons than protons

A

anion

50
Q

measure of an atom’s ability to pull electrons from other atoms; depends on atom’s size and number of vacancies

A

electronegativity

51
Q

In an ionic bond, a ___ electronegative atom will pull an electron from another atom with ___ electronegativity.

A

highly,

lower

52
Q

type of bond that shares a pair of electrons between two atoms; forms between 2 atoms of similar electronegativity

A

covalent bonds

53
Q

Biologically, covalent bonds are formed by which elements?

A

O, C, P, and N

54
Q

covalent bond in which 1 pair of electrons is shared

A

single covalent bond

55
Q

covalent bond in which 2 pairs of electrons are shared

A

double covalent bond

56
Q

covalent bond in which 3 pairs of electrons are shared

A

triple covalent bond

57
Q

What molecules come from the 4 covalent bonds formed by Carbon atoms?

A

ethanol, ethylene, acetylene, and caffeine

58
Q

type of covalent bond in which two identical atoms share electrons equally; atoms have identical electronegativities; nuclei of the atoms have the same number of protons

A

nonpolar covalent bonds

59
Q

type of covalent bond that occurs between atoms of different elements; no net charge on molecule (has a positive and negative end/poles)

A

polar covalent bonds

60
Q

In a polar covalent bond, electrons spend more time near the nucleus with more ___, giving it a slightly ___ partial charge.

A

protons,

negative

61
Q

In a polar covalent bond, the element with fewer protons has a slightly ___ partial charge.

A

positive

62
Q

example of a polar covalent bond

A

H₂O

63
Q

example of a nonpolar covalent bond

A

O₂

64
Q

attraction between a hydrogen atom and an electronegative atom; both involved in separate polar covalent bonds

A

hydrogen bonds

65
Q

Water molecules attract each other and hydrogen bond. Due to partial charges, this results in ___.

A

lattice

66
Q

biological significance of water’s temperature property

A

buffer: resists temperature changes in aquatic ecosystems and in body cells

67
Q

List the properties of water.

A 
temperature,
evaporation,
ice,
cohesion,
adhesion,
reactions,
solvent
68
Q

biological significance of water’s evaporation property

A

sweating in mammals

69
Q

Ice is ___ dense than liquid water.

A

less

70
Q

biological significance of water’s ice property

A

insulation for ponds and streams

71
Q

the attraction between two polar water molecules

A

cohesion

72
Q

biological significance of water’s cohesion property

A

creates surface tension on ponds

73
Q

the attraction between water and another polar molecule

A

adhesion

74
Q

biological significance of water’s adhesion property

A

allows water to carry nutrients through plants

75
Q

property of water in which water attracts and repels other polar molecules

A

reaction

76
Q

when water attracts other polar molecules it’s called

A

hydrophilic (water loving)

77
Q

when water repels nonpolar molecules it’s called

A

hydrophobic (water hating)

78
Q

example of a hydrophilic reaction with water

A

sugar

79
Q

example of a hydrophobic reaction with water

A

oil

80
Q

property of water in which ions and polar molecules dissolve easily in water

A

solvent

81
Q

in water’s solvent property, water molecules cluster around molecules forming what

A

hydration layers

82
Q

process of spontaneous ion formation

A

ionization

83
Q

covalent bonds in water can spontaneously break resulting in what

A

positively charged hydrogen ion (H+) and negatively charged hydroxide ion (OH-)

84
Q

substance that increases the concentration of H+ when dissolved in water; pH below 7

A

acid

85
Q

Stronger ___ produce more H+ and have a ___ pH.

A

acids,

lower

86
Q

a substance that combines with H+ when dissolved in water; lowers the H+ concentration; pH above 7

A

base

87
Q

Stronger ___ combine with more H+.

A

bases

88
Q

What is the pH of a cell?

A

close to 7

89
Q

Cell chemical reactions constantly produce what?

A

acids and bases

90
Q

substance that can take up or release H+ in solution as the H+ concentration changes; pair of substances (1 acid and 1 base) that interact in reversible reactions

A

chemical buffer

91
Q

buffer example

A

human blood

92
Q

What happens with the chemical buffer when blood pH rises?

A

carbonic acid dissociates to form bicarbonate and H+

93
Q

What happens with the chemical buffer when blood pH drops?

A

bicarbonate binds H+ to form carbonic acid

NAS 2 (19 decks)

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