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A&P 1 Chapters 1-4 > Chapters 2-3 > Flashcards

Chapters 2-3 Flashcards

1
Q

Term relating to the characteristics of having mass

and occupying space

A

Matter

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2
Q

Three forms of matter

A

Solid, liquid, gas

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3
Q

A measure of the amount of matter in an atom

A

Mass

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4
Q

Determination of atomic mass

A

The number of protons plus number of

neutrons

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5
Q

The charge on an electron

A

negative

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6
Q

The charge on a proton

A

Positive

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7
Q

Based on the atomic number the elements in the

Periodic Table are arranged

A

In consecutive order, in rows, beginning at the

upper left corner

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8
Q

The number of protons will equal the number of

_____ in a neutral atom.

A

electrons

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9
Q

Atomic mass minus atomic number determines the

number of _____

A

neutrons

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10
Q

The number of protons determines this for each

element

A

Atomic Number

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11
Q

Location of electrons in an atom

A

around the nucleus, located in specific orbitals

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12
Q

Number of electrons to fill the first 3 orbitals of an

atom

A

2, 8, 8

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13
Q

For any orbital, it is most stable in one of these 2

states

A

either completely full or completely empty

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14
Q

Region in the middle of an atom, where the mass

is centered; composed of protons and neutrons

A

Nucleus

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15
Q

Basic rule on electrons: do they like to be

separate, in pairs, or in other groups?

A

Pairs

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16
Q

True or false: the basic rule on electrons is fill the
first orbital before putting electrons in the second, and
fill the second before putting electrons in the third.

A

True

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17
Q

Basic rule on how atoms react: atoms react to

become stable by…

A

having full valence shells (orbitals)

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18
Q

An isotope is an atom that has the same number of

protons and electrons but a different number of…

A

Neutrons

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19
Q

Elements are naturally composed of a variety of
______ and that makes their ______ is a weighted
average of these found in nature

A

Isotopes, Atomic Mass

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20
Q

Unstable atoms, or ______, contain an excess of
neutrons and lose nuclear components as high energy
radiation

A

radioisotopes

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21
Q

The high energy radiation lost by radioisotopes

may be

A

Alpha particles, beta particles or gamma rays

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22
Q

The physical half life of a radioisotope (time for
50% of the element to become stable) is usually _____
the biological half life (time for 50% of the element to
be eliminated from the body.

A

longer than

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23
Q

Based on the valence electron number the

elements in the Periodic Table are arranged

A

In 8 columns, each column indicating how

many electrons are in the valence shell

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24
Q

The ______ is the outermost electron orbital
containing those electrons available for chemical
reactions

A

Valence shell

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25
Q

What does the column number in the Periodic

Table mean?

A

number of electrons in the valence shell

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26
Q

What’s so special about the elements in column

VIII?

A

Their valence shells are filled

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27
Q

The fact that elements tend to lose, gain or share

electrons in the valence shell is the

A

Octet rule

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28
Q

Composed of individual particles that have the

same properties.

A

element

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29
Q

An atom or molecule with an electrical charge

A

Ion

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30
Q

These are formed when atoms either give up or

take electrons to have full and stable valence shells

A

Ions, Ionic Bonds

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31
Q

Ions that have given up electrons; they have a

positive charge.

A

Cations

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32
Q

Ions that have taken extra electrons; they have a

negative charge.

A

Anions

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33
Q

While cations are named the same as the element,
anions often take a different word ending. The
element chlorine forms the ion _____.

A

Chloride

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34
Q

When an element has lost 2 electrons, the charge

on the resulting ion will be

A

Positive two (2+ or ++)

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35
Q

When an element gains 1 electron, the charge on

the resulting ion will be

A

negative one (-)

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36
Q

Atoms with 1, 2 or 3 electrons in the valence shell

will tend to

A

Donate the electrons acquiring a positive

charge

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37
Q

Atoms with 5, 6 or 7 electrons in the valence shell

will tend to

A

Accept electrons acquiring a negative charge

38
Q

Using the Periodic Table, elements on the left side
(Groups IA through
III A) tend to

A

Donate electrons

39
Q

Using the Periodic Table, elements on the right
side (Groups VA through
VIIA) tend to

A

Accept electrons

40
Q

The mutual attraction between a cation and an

anion forms this kind of bond.

A

Ionic Bond

41
Q

In a crystalline mixture of Na+ and Cl- the smallest

repeating unit is NaCl, defining this as an …

A

Ionic Compound

42
Q

How many chloride ions are in CaCl2?

A

2

43
Q

MgCl2

A

The formula for magnesium chloride

44
Q

An ionically bonded molecule in which the cation is

hydrogen is called…

A

acid

45
Q

HCO3- and PO4– are both

A

polyatomic anions

46
Q

A combination of 2 or more atoms.

A

Molecule

47
Q

The atoms, along with their ratios, (such as H2O)

are called the ____ _____ of a molecule

A

Molecular formula

48
Q

The arrangement of each atom in a molecule

represents a …

A

Structural formula

49
Q

A _____ formula allows visualization of the

molecule as it is arranged in space.

A

structural

50
Q

Molecules with the same molecular formula but

different structural formulas are called …

A

Isomers

51
Q

One or more covalent bonds will form between

atoms sharing electrons until..

A

The valence electron shell is filled with 8

electrons

52
Q

When 2 atoms share electrons, this kind of bond is

formed.

A

covalent bond

53
Q

The four most common elements forming covalent

bonds in the human body are

A

Carbon, hydrogen, oxygen and nitrogen

54
Q

In a single covalent bond

A

Two electrons are shared, one from each

atom

55
Q

In a double covalent bond

A

Four electrons are shared, two from each

atom, in two pairs

56
Q

In a triple covalent bond

A

Six electrons are shared, three from each

atom, in 3 pairs

57
Q

In a nonpolar covalent bond, the electrons in the

covalent bond …

A

Are shared equally by each atom

58
Q

In a polar covalent bond, the atom attracting the

electron will have either

A

More protons in the nucleus or fewer electron

shells

59
Q

In a polar covalent bond, the electrons in the

covalent bond

A

Spend more time around one of the bonded

atoms than the other

60
Q

The main example of a polar covalent bond

A

oxygen with hydrogen, O-H

61
Q

A second example of a polar covalent bond

A

nitrogen with hydrogen, N-H

62
Q

Two examples of small polar molecules

A

water and ammonia

63
Q

A nonpolar molecule is made with

A

Nonpolar covalent bonds and usually has no

charge on the molecule

64
Q

A ____ molecule usually has a separation of
charges on the molecule itself, where one area is
more + and another is more –

A

Polar

65
Q

A molecule with one part that is polar and another
part that is nonpolar is _____; an example is
phospholipid

A

amphipathic

66
Q

Since like dissolves like, an amphipathic molecule

can simultaneously dissolve in both

A

Nonpolar solvents and polar solvents

67
Q

A weak electrical attraction between the positive
pole of one polar molecule (always a hydrogen) and
the negative pole of another

A

hydrogen bond

68
Q

Intermolecular attractions between nonpolar
molecules, involving momentary unequal distributions
of electrons, are called ____ ___ and are very weak.

A

van der Waals forces

69
Q

. Interactions of a nonpolar molecule placed in a

polar solvent like water are called

A

Hydrophobic interactions

70
Q

Substances that don’t mix well with water are

called _____.

A

hydrophobic, lipid-soluble

71
Q

The bond between the O and each H in a water

molecule is classified as a _____ _____ bond

A

polar covalent

72
Q

The bond between the O of one water molecule
and the H in a second water molecule is classified as
a _____ bond.

A

hydrogen

73
Q

The covalent bonds between the two hydrogen
atoms and the oxygen atom in water are polar
covalent bonds, with the oxygen portion of water being
more ____ and the hydrogen portions being more ____

A

Oxygen - negative, hydrogen - positive

74
Q

Water molecules can form ___ ____ bonds since
the 2 positive hydrogen ends attract the oxygen of two
nearby water molecules and the doubly negative
oxygen end can attract two hydrogens from nearby
water molecules

A

four hydrogen bonds

75
Q

The intermolecular force most responsible for the

unique properties of water is

A

Hydrogen bonding

76
Q

The layers of water molecules that surround ions,

attracted by the electrical charge

A

hydration spheres

77
Q

When two different substances attract each other,

_____ occurs

A

Adhesion

78
Q

When molecules within a substance attract each

other, _____ occurs

A

cohesion

79
Q

The cohesive force of water makes it bead up on

waxed paper; we say water has a high _____ _____.

A

surface tension

80
Q

Hydrogen bonding of water molecules provides
for the unique water properties that keeps lungs stuck
to the chest wall

A

High surface tension

81
Q

Hydrogen bonding of water molecules provides
for the unique water properties that keeps body
temperature from undergoing drastic changes

A

high specific heat

82
Q

Hydrogen bonding of water molecules provides
for the unique water properties that allows sweat to
cool the body (evaporation is cooling since it takes a
lot heat to vaporize water)

A

high heat of vaporization

83
Q

Hydrogen bonding of water molecules provides
for the unique water properties that allows many
substances (salts and nutrients) to dissolve in body
fluids

A

good solvent for polar molecules

84
Q

Molecules that dissolve in water are described as

A

Polar, hydrophilic or water-soluble molecules

85
Q

Water is almost a universal _____, because it can

dissolve ionic and polar substances.

A

solvent

86
Q

The particles dissolved in solution are called

A

solutes

87
Q

Some molecules dissolve and dissociate in water;

these include

A

Salts (NaCl) and acids (H2CO3 or HCl) and

bases (NaOH)

88
Q

Particles carrying a + or – charge will be
produced when molecules both dissolve and _____ in
water

A

dissociate

89
Q

Charged particles produced following a molecule’
s dissolution and dissociation in water are _____, as
the solution described will carry an electrical current

A

Electrolytes

90
Q

Nonpolar molecules will not dissolve in a polar

solvent like water. (T or F)

A

true

A&P 1 Chapters 1-4 (3 decks)

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