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Anatomy & Physiology I > Chapter 2 > Flashcards

Chapter 2 Flashcards

Atoms, Ions, and Molecules

1
Q

matter is

A

a substance that has mass and takes up space

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2
Q

solids are

A

things that hold their shape without a container

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3
Q

liquids are

A

things that hold their shape with a container

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4
Q

gases are

A

things that have no shape, even with a container

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5
Q

matter is composed of

A

atoms

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6
Q

atoms are

A

the simplest whole particle

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7
Q

atoms create

A

elements

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8
Q

subatomic particles are found

A

within atoms

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9
Q

three main subatomic particles are

A

protons
electrons
neutrons

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10
Q

protons are _____ charged

A

positively

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11
Q

electrons are _____ charged

A

negatively

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12
Q

neutrons have a _____ charge

A

neutral

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13
Q

neutrons provide what to an atom?

A

mass

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14
Q

mass of an atom is expressed in

A

amu, atomic mass units

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15
Q

the periodic table organizes

A

elements

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16
Q

elements are organized on the periodic table by

A

mass, electronegativity, valence electron shell

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17
Q

electronegativity on the periodic table increases when

A

traveling up and right along the table

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18
Q

valence electrons are

A

the electrons on the outermost shell of the atom

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19
Q

the number of valence electrons an atom has is the same as

A

the atom’s group number

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20
Q

the octet rule applies to

A

valence electrons

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21
Q

which elements represent the octet rule?

A

group 8, noble gases

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22
Q

how many valence electrons does an atom want in its shell?

A

eight

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23
Q

six major elements of the body

A

oxygen
carbon
hydrogen
nitrogen
calcium
phosphorus

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24
Q

six minor elements of the body

A

sulfur
potassium
sodium
chlorine
magnesium
iron

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25
Q

isotopes are

A

atoms of the same elements with the same number of protons and electron, but different numbers of neutrons

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26
Q

radioisotopes are

A

isotopes that emit radioactive nuclei when they decay

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27
Q

the more neutrons an isotope has,

A

the more unstable it is and more radioactive

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28
Q

radioisotopes decay into

A

more stable versions of the isotope

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29
Q

physical half life is

A

the amount of time it takes 50% of the isotope to decay into its more stable isotope

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30
Q

biological half life is

A

the amount of time it takes half of the isotope to be eliminated from the body

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31
Q

half life calculation is important regarding

A

medication dosage and medical imaging

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32
Q

an ion is

A

an atom or group of atoms with an electric charge, either positive or negative

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33
Q

a cation is a

A

positively charged ion

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34
Q

an anion is a

A

negatively charged ion

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35
Q

five cations in the body

A

sodium
potassium
calcium
magnesium
hydrogen

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36
Q

three main anions in the body

A

chloride
bicarbonate
phosphate

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37
Q

how are ions formed? use NaCl as an example

A

When sodium and chloride meet to form sodium chloride (NaCl), table salt, sodium donates its single valence electron to chloride, which has seven. Chloride is more electronegative than sodium, which is why it attracts the electron more.

The addition of a negative charge to neutral elemental chloride gives it a -1 charge. The loss of a negative charge to neutral elemental sodium gives it a +1 charge.

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38
Q

polarity is

A

a trait of molecular bonds between atoms, based in electronegativity differences in these bonds

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39
Q

if a molecule is amphipathic

A

there are polar and nonpolar components in the same moelcule

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39
Q

if a molecule is polar

A

there is a large electronegativity difference between the bonds

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39
Q

if a molecule is nonpolar

A

there is small or no electronegativity difference between bonds

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40
Q

what is the polarity of water?

A

water is polar

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40
Q

the polar bonds in water produce

A

slightly positive and negative charges

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40
Q

the slight charges in water gives it the ability to

A

produce hydrogen bonds

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41
Q

each water molecule can create hydrogen bonds with _____ adjacent water molecules

A

four

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42
Q

four main roles of water in the body

A

transportation of molecules
lubrication to decrease friction
cushion
excretion of waste

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43
Q

solubility is

A

the degree to which a substance can be dissolved into another substance

44
Q

solutes are

A

substances that are being dissolved

45
Q

solvent is

A

the substance a solute is being dissolved in

46
Q

a solution is

A

the creation of solute + solvent

47
Q

general rule of solubility

A

like dissolves like

48
Q

universal solvent is

A

water

49
Q

hydrophobic exclusion is

A

a phenomena where the non polar molecules, when added to water, will tightly group together as far away from the water as possible

50
Q

important amphipathic molecule in the body

A

phospholipids

51
Q

ionic compounds _____ in water, producing ____

A

dissociate
ions

52
Q

ions have the ability to

A

conduct electricty

53
Q

primary ionic compound in the body

A

NaCl

54
Q

electrolytes are

A

ions in the body that can conduct electricity

55
Q

nonelectrolytes

A

are molecules that cannot conduct electricity

56
Q

nonelectrolyte example

A

glucose

57
Q

an acid is

A

a compound that dissociates in water to produce H+ and an anion

58
Q

a base is

A

a compound that accepts an H+ when added to water

59
Q

a proton acceptor is a

A

base

59
Q

a proton donor is an

A

acid

60
Q

most bases will contain

A

OH-, hydroxide ion

61
Q

pH is how

A

acidic or basic a solution is

62
Q

pH measures

A

H+ concentration

63
Q

pH is also known as

A

potential of hydrogen

64
Q

pH scale is from

A

0 to 14

65
Q

a pH of 1 would be

A

very acidic

66
Q

a pH of 13 would be

A

very basic

67
Q

the difference between each number on the pH scale is how many times different?

A

10x

68
Q

pH of blood

A

7.35 to 7.45, average 7.4

69
Q

why is blood slightly basic?

A

bicarbonate ion presence

70
Q

how does blood maintain such a tight pH range?

A

buffer systems, specifically the bicarbonate buffer system

71
Q

neutralization is when

A

an acidic or basic solution is made neutral at a pH of 7

72
Q

acidosis is

A

when blood pH is less than 7.35

73
Q

alkalosis is when

A

blood pH is greater than 7.45

74
Q

why aren’t buffers systems and neutralization the same?

A

buffer systems do not always result in a neutral pH, but work to maintain a specific pH range

75
Q

bicarbonate buffer system chemical equation

A

CO2 + H2O <-> H2CO3 <-> HCO3- + H+
carbon dioxide + water -> carbonic acid -> bicarbonate ion + hydrogen ion

75
Q

biological macromolecules are

A

large organic molecule synthesized by the body, always containing carbon, hydrogen, and oxygen

76
Q

biological macromolecules may also contain

A

nitrogen, phopshorus, sulfur

77
Q

hydrocarbons are

A

molecules that only contain hydrogen and carbon

78
Q

hydrocarbon example

A

CH4, methane

79
Q

hydrocarbons are always

A

nonpolar and hydrophobic

80
Q

functional groups are

A

two or more atoms that always exhibit the same chemical characteristics when present on a molecule

81
Q

functional group examples

A

-OH, hydroxyl
-COOH, carboxyl/carboxylic acid
-NH2, amine
- PO4 3-, phosphate

82
Q

polymers are

A

molecules made up of repeating subunits called monomers

83
Q

a dimer is

A

two monomers bound together

84
Q

polymer examples

A

glycogen, proteins

85
Q

dehydration synthesis

A

when two monomers join to form a dimer and water is lost in the process

86
Q

hydrolysis

A

when a dimer is broken into two monomers and water is used to break the dimer

87
Q

lipids are

A

a group of fatty, hydrophobic molecules

88
Q

four main types of lipids in the body

A

triglycerides - energy storage
phospholipids - cell structure
steroids - precursor to hormones
eicosanoids - inflammation and immune response

89
Q

carbohydrates are

A

hydrated carbons

90
Q

general chemical formula of carbohydrates

A

CH2On, n = number of carbons

91
Q

monosaccharides are

A

the simplest carbohydrate

92
Q

polysaccharides are

A

the most complex carbohydrate

93
Q

most common monosaccharide

A

glucose

94
Q

nucleic acids are

A

biological macromolecules within cells that store genetic information

95
Q

DNA is

A

a double stranded nucleic acid with each stand containing repeating units of deoxyribonucleotides linked together by phosphodiester bonds. Each deoxyribonucleotide contains either thymine, guanine, adenine, or cytosine nitrogenous bases

96
Q

RNA is

A

a single stranded nucleic acid formed by repeating units of ribonucleotides bound by phosphodiester bonds. Each ribonucleotide contains either uracil, guanine, adenine, or cytosine nitrogenous bases

97
Q

uracil is specific to

A

RNA

98
Q

thymine is specific to

A

DNA

99
Q

DNA and RNA are composed of

A

nucleotide monomers

100
Q

nucleotides have three components:

A

pentose sugar
phosphate
nitrogenous base

101
Q

six examples of protein function in the body

A

catalysis of reactions, through enzymes
structural support of cells
body movement
oxygen transport in the blood
membrane transport for molecules like glucose
immune protection, through antibodies

102
Q

Proteins are polymers composed of

A

one or more linear strands of amino acid monomers

103
Q

how many amino acids are there in the body that are used to form proteins?

A

20

104
Q

what are the four structural hierachy of proteins?

A

primary
secondary
tertiary
quaternary

105
Q

primary protein structure

A

single chains of peptide bonded amino acids with a carboxyl and amino terminal ends

106
Q

secondary protein structure is characterized by

A

alpha helices and beta sheets

107
Q

tertiary protein structure is

A

the final 3D shape by one protein chain

108
Q

quaternary protein structure is

A

a structure of two or more proteins in 3D structure

109
Q

denaturation is

A

when the conformation/structure of a protein is changed

110
Q

what is the result of denaturation?

A

the biological activity of a protein ends or is disrupted

111
Q

three ways denaturation can occur

A

extreme heat
extreme pH changes
addition of solvents

Anatomy & Physiology I (16 decks)

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