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Human Anatomy and Physiology > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

anything that has mass and occupies space can eist in three states; solid, liquid, or gas (no volume or shape)

A

matter

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2
Q

study of matter and its interactions

A

chemistry

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3
Q

smallest unit of matter that retains original properties

A

atom

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4
Q

in nucleus; positive charge;

A

proton

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5
Q

in nucleus; no charge

A

neutron

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6
Q

in cloud; negative charge (these are in the shells in the clous so we can have chemical bonding)

A

electron

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7
Q

atoms are electrically ______- they have _______ ________; # of protons and electrons are ____ cancelling each others charge; number of ____ do not have to equal number of protons

A

neutral, no charge
equal
neutrons

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8
Q

regions surronding atomic nucleus where elctrons exist

A

electron shell

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9
Q

of protons that an atom has in its nucleus is

A

atomic number

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10
Q

substance that cannot be broken down into simple substance by chemical means

A

element

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11
Q

what’re the 4 chemicals that make up 96% of our bodies?

A

hydrogen
oxygen
carbon
nitrogen

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12
Q

the periodice table lists elements by their ____

A

increasing atomic numbers

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13
Q

atoms of two or more elements physically intermixed w/out changing chem nature of the elements themselves

A

mixture

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14
Q

mixture containing two or more components with large unevenly distributed particles; WILL settle out when left undisturbed

A

suspension (type of mixture)

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15
Q

2 or more components with small, evenly distributed particles; will NOT settle out

A

colloid (type of mixture)

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16
Q

2 or more components w/ extremely small, evenly distributed particles; will NOT settle out; contain a solute dissolved in a solvent

A

solutions

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17
Q

sustance that is dissolved

A

solute (sugar/ solid)

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18
Q

substance that dissolves solute

A

solvent( water/ liquid)

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19
Q

What are energy relationships based on?

A

electrons

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20
Q

matter can be combined chemically when atons are combined by ___

A

chemical bonds

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21
Q

formed by chem bonding between 2 or more atoms of same element; atoms come together to form this

A

molecule

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22
Q

formed when 2 or more atoms from diff elements combine by chem bonding

A

compound

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23
Q

very large molecules composed of many atoms

A

macromolecules

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24
Q

represent molecules symbolically w/ letters and numbers; formula giving the numbers of atoms of each of the elements present in one molecule of a specific compound

A

molecular formulas

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25
Q

Chem bonds are formed when ___ _____ of atoms interact

A

valence electrons

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26
Q

what determines how an atom interacts with other atoms and whether it will bond w/ a specific atoms

A

valence electrons

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27
Q

states thaat an atom is most stable when it has 8 electrons in its valence shell

A

octet rule

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28
Q

states that for atoms w/ 5 or fewer electrons, that the atoms are most stable when there valence elctron shell has 2 electrosn

A

duet rule

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29
Q

formed when electrons are transferred from a metal atom to a nonmetal; results in formation of ions; transfer that results in a charged molecule (cations and anions) (ex: sodium chloride)

A

ionic bond

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30
Q

positively charged ion; forms when metal loses one or more electrons

A

cation

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31
Q

negatively charged ion; forms when nonmetal gains one or more elctron

A

anion

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32
Q

form when two or more nonmetals share electrons; strongest bond

A

covalent bond

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33
Q

how many covalent bonds can we have?

A

single bond, double bond, or triple bond of electron pairs

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34
Q

all elements have protons that attract electrons; property known as…

A

electronegativity

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35
Q

the ___ electronegativity an element has the more strongly it ______, which then _____ them away from less electronegative elements

A

more, attracts, pulls

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36
Q

results when two nonmetals in a molecule w/ similar or identical electronegaticities pull with equal force. Therefore share electrons equally

A

nonpolar covalent bonds

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37
Q

what 3 situations can nonpolar molecules occur in?

A
  • atoms sharing electrons are same elements
  • arrangement of atoms makes one atom unabe to pull more stongly than another atom
  • bond is between carbon and hydrogen
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38
Q

forms polar molecules when nonmetals w/ diff electronegativities interact resulting in an unequal sharing of electrons (ex water)

A

polar covalent bonds

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39
Q

polar molecules w/ partially positive and partially negative ends are known as…

A

dipoles

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40
Q

atoms w/ higher electronegativity in polar covalent bonds become ___

A

partially negative

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41
Q

weak attractions between partially positive end of one dipole and partially negative end of another dipole

A

hydrogen bonds

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42
Q

what is respondisble for surfacce tension?

A

hydrogen bonds

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43
Q

what’s the key property of water?

A

surface tension

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44
Q

occurs every time a chemical bond is formed, broken, or rearranged, or when electrons are transferred between two or more atoms

A

chemical reaction

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45
Q

series of symbols and abbreviations used to demonstrate what occurs in a reaction

A

chemical notation

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46
Q

in a chemical equation, _____ are on the left side, are startgin ingridients; will undergo reaction

A

reactants

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47
Q

in a chem euqation, ___ are on the right side, are the results of the reaction

A

products

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48
Q

reactions can proceed in either direction as denoted by 2 arrows tht run in opposite directions

A

reversible reactions

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49
Q

capacity to do work or put matter into motion or fuel chemical reactions

A

energy

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50
Q

stored energy; can be released to do work at some later time

A

potential energy

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51
Q

potential energy that has been released or set in motion to perform work; all atoms have this energy b/c they are constantly in motion

A

kinectic energy

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52
Q

energy found in bonds between atoms; drives nearly all chem process

A

chem energy

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53
Q

generated by movement of charged particles or ions

A

electrical energy

54
Q

energy directly transferred from one object to another

A

mechanical energy

55
Q

reactions that require input of energy from another source; products contain more energy than reactants b/c energy was inversted so reaction could proceed

A

endergonic reactions

56
Q

reactions release excess energy (heat) so products have less energy than reactants

A

exergonic reactions

57
Q

when a large substance is broken down into smaller substances; uses ____ energy

A

catobolic reactions
exergonic
AB- A + B

58
Q

one or more atoms form reactants are exchanged for another; rearranging atoms

A

exchange reactions

AB + CD- AD + BC

59
Q

special kind of exchange reaction; occurs when electros and energy are exchanged instead of atoms

A

oxidation-reduction reactions

60
Q

special kind of exchange reaction; occurs when electros and energy are exchanged instead of atoms; this reaction is a ____ reaction

A

oxidation-reduction reactions

exergonic

61
Q

reactant that loses electrons is

A

oxidized

62
Q

reactant that gains electrons is

A

reduced

63
Q

reactions that occur when small subunits are united by chemical bonds to make large more complex substances (take small and make it big); this reaction is a ____ reaction

A

anabolic reaction

A + B- AB
endergonic

64
Q

the energy required to overcome the repulsion of their own electrons is called

A

activation energy

65
Q

why must activation energy be used?

A

so that the reactants reach their transition states (ready to form new bonds) in order to react and form products (hill ex on page 11)

66
Q

which factors increase reaction rate by reducing activation energy or increasing likelihood of strong collisions between reactants (4)

A
  • concentration
  • temperature
  • reactant properties
  • presence or absense of catalyst
67
Q

how will concentration increase reaction rate by reducing activation energy or increasing likelihood of strong collisions between reactants

A

the more concentrated it is the more likely it’ll increase the chances of a sucessful collisions

68
Q

how will temperature increase reaction rate by reducing activation energy or increasing likelihood of strong collisions between reactants

A

heat a substance up, atoms move more, so it will collide.

69
Q

how will reactant properties increase reaction rate by reducing activation energy or increasing likelihood of strong collisions between reactants

A

size and phase influence reaction rates:

small atoms have more energy and move faster; gasses are faster than solids

70
Q

substance that increases reaction rate by lowering activation energy w/out being consumed or altered in reaction

A

catalyst

71
Q

biological catalysts; most are proteins

A

enzymes

72
Q

describes enzyme’s interaction w/ its substrates; binding of a substance causes a small shape change that ___ energy of activation (shape of active site on enzyme, directly matches shape of reactants)

A

induced-fit mechanism

reduces

73
Q

the chemistry of life

A

biochemistry

74
Q

____ ____ do not contain carbon bonded to hydrogen; include ____ ( 4 exjs)

A

include water, acids, bases, and salts

75
Q

those compounds that do contain carbon bonded to hydrogen

A

organic compounds

76
Q

___ makes up 60-80% of mass of human body and has several key properties vital to our existence (4)

A

water (polar covalent bond)

  1. high heat capacity- able to absorb hear w/out significantly changing temp itself ( lake takes long time to warm up)
  2. carries heat w/ it when it evaporates
  3. cushions and protects body structures because of relatively high density
  4. acts as a lubricants between 2 adjacent surfaces (reduces friction)
77
Q

___ is the body’s primary solvent or the universal solvent? why?

A

water

b/c so many solutes will dissolve in it entirely or to some degree

78
Q

water is only able to dissolve what?

A

hydrophillic solutes
“like dissolves like”
water dissolves ionic and polar covalent structures

79
Q

solutes that do not have fully or partially charged ends are…; do not dissolved in water; includes uncharged nonpolar covalent molecules like ___ and ____

A

hydrophobic

oils and fats

80
Q

___ recive/ accept H while _____ donate H

A

bases

acids donate

81
Q

hydrogen ion or proton donor; # of hydrogen ions increases in water when its is added; pH less than 7

A

acid

82
Q

hydrogen ion acceptor; # of hydrogen ions decreases in water when its addded; pH is greater than 7

A

base

83
Q

chemical system that resists changes in pH; prevents large swings in pH when acid or base is added to a solution

A

buffer

84
Q

any metal cation and nonmetal anion held together by ionic bonds

A

salt

85
Q

salts can dissolved in water to form cations and anions called ….; These are capable of what?

A

electrolytes

electrical current

86
Q

single units; makes up carbs, lipids, proteins, nucleic acid by taking out water

A

monomers

87
Q

combine single subunits that can be combined to build larger structures

A

polymers

88
Q

anabolic reaction that links monomers together and makes a molecule of water in process

A

dehydration synthesis

89
Q

catabolic reaction that uses water to break up polymers into smaller subunits

A

hydrolysis

90
Q

composed of carbon, hydrogen, and oxygen, function primarily as fuel; energy storage; important for storage

A

carbohydrates

91
Q

sugar; monomers from which all carbs are made; glucose, fructose, galactose, ribose, deoxyribose are most abundant version of this

A

monosacchrides

92
Q

What chemicals make up lactose

A

glucose + galactose

93
Q

What chemicals make up maltose

A

glucose + glucose

94
Q

formed by union of two monosaccharides by dehydration synthesis; pull water out

A

disaccharides

95
Q

What chemicals make up table salt?

A

glucose + fructose

96
Q

3 main types of carbs:

A
  • polysaccharides
  • disaccharides
  • monosaccharides
97
Q

consist of many monosaccharides joined to one another by dehydration synthesis reactions

A

polysaccharides

98
Q

____ is the storage polymer of glucose. It’s mostly in ____ and _____

A

glycogen

skeletal muscle and liver cells

99
Q

group of nonpolar hydrophobic* molecules composed primarily of carbon and hydrogen; includes fats and oils; important in _____ structure; in lipid bilayer, under your skin, around kidneys (for _____)

A

lipids
cellular
protection
*won’t do well in water; issue if we want to transport lipid molecules in blood

100
Q

lipid monomers; may have non, one, or more double bonds between carbons in hydrocarbon chain; building blocks

A

fatty acid

101
Q

solid at room temperature; have no double bonds; bad for your health (in butter and whipped cream)

A

saturated fatty acids

102
Q

generally liquid at room temperature; have 1 double bond;

A

monounsaturated fatty acids

better to commsume unsaturated fat than saturated

103
Q

liquid at room temp; have 2 or more double bonds

A

polyunsaturated fatty acids

104
Q

3 fatty acids linked by dehydration synthesis (pull out water) toglycerol; storage polymer for fatty acids

A

triglyceride

105
Q

composed of a glycerol backbone, two fatty acid tails and one phosphate head. What makes the phospholipids vital to the structure of the cell membranes?

A

phospholipid

amphiphilic nature

106
Q

molecule w/ polar head and a nonpolar tail

A

amphiphilic

107
Q

nonpolar and share a steroid nucleus; ex: vitamin D, bial salts, secretion from gall bladder

A

steroids

108
Q

steroid that forms basis for all other steroids

A

cholesterol

109
Q

What are all the functions of proteins? (5)

A
  • function as enzymes
  • play structural roles
  • involved in movement
  • function in the body’s defenses
  • can be used as fuel
110
Q

20 diff ______; can be linked by______ into polypeptides

A

amino acids

peptide bonds

111
Q

formed from 2 or more amino acids linked together by peptide bonds through dehydration synthesis

A

peptides

112
Q

consist of 2 amino acids, tripeptides (3 amino acids), and polypeptides ( 10 or more amino acids)

A

dipeptides

113
Q

long rope like stands; composed mostly of nonpolar amino acids; link things together and add strength and durability to structures; water insoluble

A

fiborous proteins

114
Q

spherical or globe-like; composed mostly of polar amino acids; function as enzymes, hormones, and other cell messangers; water soluble

A

globular proteins

115
Q

amino acid sequence of polypeptide chain

A

primary structure (complex structure of a complete protein is divided into four levels this is one)

116
Q

one or more segments of primary structure folded in specific ways; held together by hydrogen bonds

A

secondary structure

117
Q

coilded spring; part of secondary structure; assembled

A

alpha helix

118
Q

venetian blind; spontaneously; part of secondary structure

A

beta pleaded sheet

119
Q

three-dimensional shape that peptide chain assumes (twists, folds, and coils including secondary structure); stabilized by hydrogen bonding; based on 2ndary structure

A

tertiary structure

120
Q

linking together more than one polypeptide chain in a specific arrangement; critical to function of protein as a whole

A

quaternary structure

121
Q

process of destroying a protein’s shape by heat, pH changes, or exposure to chemicals; influenced by tem[, pH, # of diff chemicals; no way to put protein back together

A

protein denuturation

122
Q

monomers of nucleic acid; DNA, RNA

A

nucleotides

123
Q

how do you make up a nucleotide structure?

A

5 carbon pentose sugar, ribose or dexyribose, phosphate

124
Q

doubled ringed molecule

A

purines

125
Q

single-ringed molecule

A

pyrimidines

126
Q

energy held in bonds; major energy transfer time (main source of energy in body);

A

ATP

127
Q

how is ATP synthesized from ADP and Pi?

A

using energy from oxidation of fuels (like glucose)

128
Q

production of large quantities of ATP requires what?

A

oxygen, which is why we breathe

129
Q

an extremely large molecules found in nuclei of cells; composed of 2 long chairs that twist around each other to form a double helix

A

DNA

130
Q

what’re the bases of DNA

A

adenine, guanine, cytosine, and thymine

131
Q

What forms backbone of strand

A

pentose sugar deoxyribose

Human Anatomy and Physiology (8 decks)

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