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ANAPHY LECTURE > Chapter 2 - The Chemical Basis of Life > Flashcards

Chapter 2 - The Chemical Basis of Life Flashcards

1
Q

anything that occupies space and has mass

A

matter

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2
Q

amount of matter in an object

A

Mass

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3
Q

gravitational force acting on an object of a given mass

A

weight

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4
Q

international unit for mass

A

kilogram (kg)

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5
Q

simplest type of matter, having unique chemical properties

A

element

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6
Q

About 96% of the body’s weight results
from the elements __

A

oxygen
carbon
hydrogen
nitrogen

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7
Q

majority of the body’s weight is from __, it is also the most abundant element in the earth’s crust

A

oxygen (65%)

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8
Q

plays an especially important role in the chemistry of the body, due in part to
its propensity to form covalent bonds with itself and other molecules

A

carbon

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9
Q

(T/F) Elements can have multiple roles
and exist in different states in the body.

A

true (ex. mineralized calcium contributes to the solid matrix of bones, while dissolved calcium helps regulate enzyme activities and nervous system signaling)

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10
Q

the smallest particle of an element that has the chemical characteristics of that element.

A

atom

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11
Q

composed of atoms of only one kind

A

element (ex. element carbon is composed of only carbon atoms)

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12
Q

(T/F) Atoms are composed of subatomic
particles, some of which have an electrical charge.

A

true

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13
Q

three major types of subatomic particles

A

neutrons
protons
electrons

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14
Q

has no electrical charge

A

neutron

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15
Q

has one positive charge

A

proton

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16
Q

has one negative charge

A

electron

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17
Q

Things to remember:

A
  1. The positive charge of a proton is equal in magnitude to the negative charge of an electron.
  2. The number of protons and the number
    of electrons in each atom are equal
  3. Individual charges cancel each other, therefore, each atom is electrically neutral.
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18
Q

what forms the nucleus at the center of the atom?

A

Protons and neutrons

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19
Q

what moves charge moves around the nucleus?

A

Electron

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20
Q

accounts for 99.97% of an atom’s mass but only 1 ten-trillionth of its volume

A

nucleus

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21
Q

Most of the volume of an atom is occupied by

A

electrons

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22
Q

region where electrons are most likely to be found

A

electron cloud

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23
Q

equal to the number of protons in each atom

A

atomic number (because the number of electrons is equal to the number of
protons, the atomic number is also the number of electrons

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24
Q

there are how many naturally occurring elements?

A

90

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25
Q

responsible for most of the mass of atoms

A

Protons and neutrons (have about the same mass)

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26
Q

the number of protons plus the number of neutrons in each atom

A

mass number

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27
Q

how to find the number of neutrons?

A

subtract the number of protons from the mass number

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28
Q

are two or more forms of the same element
that have the same number of protons and electrons but a different number of neutrons

A

Isotopes

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29
Q

three isotopes of hydrogen (have 1 proton
and 1 electron, but hydrogen has no neutrons in its nucleus)

A

hydrogen
deuterium
tritium

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29
Q

have the same atomic number but different mass numbers

A

Isotopes

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29
Q

can be denoted using the symbol of the element preceded by the mass number (number of protons and neutrons)

A

Isotopes

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30
Q

unified atomic mass unit (u)

A

dalton (Da)

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31
Q

the average mass of its naturally
occurring isotopes, taking into account the relative abundance of each isotope.

A

atomic mass

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32
Q

value of Avogadro’s number, or 1 mole (abbreviated mol).

A

6.022 × 10^23

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33
Q

mass of 1 mole of a substance expressed
in grams is called the

A

molar mass

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34
Q

The chemical behavior of an atom is dependent on its

A

electrons

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35
Q

concentric rings around the nucleus

A

electron shells

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36
Q

maximum number of electrons a shell can hold:

A

The innermost shell (the shell closest to the nucleus) - maximum of 2 electrons
remaining shells - maximum of 8 electrons
outermost, valence shell - 8

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37
Q

(T/F) The number of electrons in the valence shell determines an atom’s chemical nature.

A

true

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38
Q

full valence shell

A

inert and does not form chemical bonds with other atoms

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39
Q

not fill valence shell

A

atom is chemically reactive and forms chemical bonds with other atoms to achieve a full valence shell, called an octet.

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40
Q

tendency of atoms to combine
with other atoms until each has 8 electrons (2 electrons for hydrogen) in its valence shell

A

octet rule

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41
Q

what determines the type of chemical bond?

A

The fate of electrons as being either transferred or shared

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42
Q

2 types of chemical bond

A

ionic or covalent

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43
Q

The decision whether an electron is transferred or shared between two atoms is determined by __

A

Electronegativity

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44
Q

ability of an atom’s nucleus to attract electrons.

A

Electronegativity

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45
Q

what atoms have a strong
electronegativity?

A

atoms that lack only 1 or 2 electrons from having an octet in their valence shell

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46
Q

what atoms have a weak electronegativity

A

atoms that lack 6 or 7 electrons from
having an octet in their valence shell

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47
Q

lacks only 1 electron from its valence shell to be full

A

hydrogen

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48
Q

(T/F) Hydrogen’s pull on electrons is less than
that of other atoms with more protons (low electronegativity)

A

True

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49
Q

How are covalent bonds formed?

A

When the electronegativities of two atoms
forming a chemical bond are similar, the atoms tend to share

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50
Q

How are ionic bonds formed?

A

when electronegativities are
very different, the atoms tend to transfer electrons

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51
Q

forms when atoms share one or more pairs of
electrons.

A

covalent bond (ex. two hydrogen atoms to form
a hydrogen molecule)

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52
Q

sharing of one pair of electrons by two atoms

A

single covalent bond.

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53
Q

results when two atoms share 4 electrons,
2 from each atom

A

double covalent bond

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54
Q

When electrons are shared equally between atoms, as in a hydrogen molecule, the bonds are called

A

nonpolar covalent bonds

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55
Q

atoms bound to one another by a covalent bond do not always share their electrons equally because in these situations the
electronegativity of one atom is stronger than the electronegativity of the other atom. Bonds of this type are called

A

polar covalent bonds

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56
Q

composed of two or more atoms chemically combined to form a structure that behaves as an independent unit.

A

molecule

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57
Q

substance resulting from the chemical combination of two or more different types of atoms.

A

compound

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58
Q

can be determined by adding up the atomic masses of its atoms (or ions)

A

molecular mass

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59
Q

are the weak electrostatic attractions
that exist between oppositely charged parts of molecules, or between ions and molecules

A

Intermolecular Forces

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60
Q

are much weaker than the forces producing
chemical bonding (include hydrogen bonds
and the properties of solubility and dissociation)

A

Intermolecular forces

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61
Q

results from the attraction of the
positive end of one polar molecule to the negative end of another
polar molecule

A

Intermolecular forces

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62
Q

If the positively charged hydrogen of one molecule is attracted to the negatively charged oxygen, nitrogen, or fluorine
of another molecule, a __ forms

A

hydrogen bond

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63
Q

ability of one substance to dissolve in another

A

Solubility

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64
Q

Four representations of picturing molecules

A

Chemical Formula
Electron-Dot Formula
Bond-Line Formula
Models

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65
Q

Cations and anions that dissociate in water that have the capacity to conduct an electric current

A

electrolytes

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66
Q

a recording of electric
currents produced by the heart

A

electrocardiogram (ECG)

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67
Q

Molecules that do not dissociate form solutions that do not conduct electricity

A

nonelectrolytes

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68
Q

A complete transfer of electrons between
two atoms results in separate positively
charged and negatively charged ions.

A

Ionic Bond

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69
Q

An unequal sharing of electrons
between two atoms results in a slightly
positive charge (δ+) on one side of the
molecule and a slightly negative charge
(δ−) on the other side of the molecule

A

Polar Covalent Bond

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70
Q

An equal sharing of electrons
between two atoms results in an
even charge distribution among
the atoms of the molecule.

A

Nonpolar Covalent Bond

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71
Q

The attraction of oppositely charged
ends of one polar molecule to another
polar molecule holds molecules or
parts of molecules together

A

Hydrogen Bond

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72
Q

occurs when atoms, ions, molecules, or
compounds interact either to form or to break chemical bonds

A

chemical reaction

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73
Q

substances that enter into a chemical reaction

A

reactants

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74
Q

substances that result from the chemical reaction

A

products

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75
Q

three important points about chemical reactions

A
  1. less complex reactants are combined to form a larger, more complex product.
  2. a reactant can be broken
    down, or decomposed, into simpler, less complex products.
  3. atoms are generally associated
    with other atoms through chemical bonding or intermolecular forces; therefore, to synthesize new products or break down reactants, it is necessary to change the relationship between atom
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76
Q

when two or more reactants chemically
combine to form a new and larger product.

A

synthesis reaction

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77
Q

The synthesis reactions occurring in the body are collectively referred to as

A

anabolism

78
Q

These reactions produce the molecules
characteristic of life, such as

A

ATP
proteins
carbohydrates
lipids
nucleic acids

79
Q

the product of amino
acids bound together

A

water

80
Q

Synthesis reactions in
which water is a product are called

A

dehydration reactions

81
Q

How is ATP formed?

A

ATP, which is composed of adenosine and three phosphate groups, is synthesized from adenosine diphosphate (ADP), which has two phosphate groups, and an inorganic phosphate (H2PO4)

82
Q

a larger reactant is chemically broken down into two or more smaller products.

A

decomposition reaction

83
Q

decomposition reactions occurring in the body are collectively called

A

catabolism

84
Q

All of the anabolic and catabolic reactions in the body are collectively defined as

A

metabolism

85
Q

Reactions that use water in this manner are called

A

hydrolysis reactions

86
Q

the reaction can run in the opposite direction, so that the products are converted back to the original reactants

A

reversible reaction

87
Q

the amount of reactants relative to the amount of products remains constant.

A

equilibrium

88
Q

Chemical reactions that result from the exchange of electrons between the reactants

A

oxidation-reduction reactions

89
Q

The loss of an electron by an atom

A

oxidation

90
Q

the gain of an electron

A

reduction

91
Q

the capacity to do work

A

Energy

92
Q

stored energy that could do work but is not doing so

A

Potential energy

93
Q

is the form of energy that is
actually, doing work and moving matter

A

kinetic energy

94
Q

results from the position or movement of
objects

A

Mechanical energy

95
Q

a form of potential energy stored within
the chemical bonds of a substance.

A

Chemical energy

96
Q

a form of energy that flows from a hotter object
to a cooler object

A

Heat energy

97
Q

a measure of how hot or cold a
substance is relative to another substance

A

Temperature

98
Q

(T/F) A chemical reaction occurs only when molecules with sufficient kinetic energy collide with each other.

A

true

99
Q

the minimum amount of energy that the reactants must have to start a chemical reaction

A

Activation energy

100
Q

are substances that increase the rate of chemical reactions

A

Catalysts

101
Q

proteins that act as catalysts and increase
the rate of chemical reactions by lowering the activation energy necessary for the reaction to begin

A

Enzymes

102
Q

generally deals with substances that do not
contain carbon, with lack of carbon-hydrogen bonds

A

Inorganic chemistry

103
Q

the study of carbon-containing substances, with a few exceptions. (Carbon monoxide (CO), carbon dioxide (CO2), and bicarbonate ions (HCO3−)

A

Organic chemistry

104
Q

formed when an atom of oxygen forms polar covalent bonds with two atoms of hydrogen.

A

water

105
Q

attraction of water to another water molecule

A

Cohesion (ex. surface tension exhibited when water bulges over the top of a full glass without spilling over)

106
Q

the same attractive force of
hydrogen bonds of water that will also attract other molecules.

A

Adhesion

107
Q

combination of two or more substances physically blended together, but not chemically combined

A

mixture

108
Q

any mixture in which the substances are uniformly distributed

A

solution

109
Q

mixture containing materials that separate
from each other unless they are continually, physically blended together

A

suspension (ex. blood)

110
Q

a mixture in which a dispersed substance
or particle is unevenly distributed throughout the mixture.

A

colloid

111
Q

indicate the number of particles in a solution.

A

osmoles

112
Q

reflects the number, not the type, of particles
in a solution

A

osmolality

113
Q

1/1000 of an osmole

A

milliosmole

114
Q

can alter body functions by releasing and binding protons

A

acids and bases

115
Q

maintained by homeostatic mechanisms involving buffers, the respiratory system,
and the kidneys

A

normal balance of acids and bases

116
Q

defined as a proton donor

A

acid

117
Q

defined as a proton acceptor

A

base

118
Q

dissociate almost completely when dissolved in water

A

Strong acids or bases

119
Q

only partially dissociate in water

A

Weak acids or bases

120
Q

a means of referring to the H+ concentration in a solution

A

pH scale

121
Q

has equal concentrations of H+ and OH−;

A

neutral solution

122
Q

Solutions with a pH less than 7

A

acidic

123
Q

Solutions with a pH greater than 7 a

A

alkaline or basic

124
Q

results if blood pH drops below 7.35, in which case the nervous system becomes depressed and the individual may become disoriented and possibly comatose

A

Acidosis

125
Q

results if blood pH rises above 7.45. Then the nervous system becomes overexcitable, and the individual may become extremely nervous
or have convulsions.

A

Alkalosis

126
Q

a compound consisting of a cation other than H+ and an anion other than OH−.

A

salt

127
Q

are chemicals that resist changes in pH when either acids or bases are added to a solution.

A

buffers

128
Q

Buffers prevent large changes in pH values by acting as

A

conjugate acid-base pairs

129
Q

(T/F) The greater the buffer concentration, the more effectively it can resist a change in pH

A

true

130
Q

an inorganic molecule consisting of two oxygen atoms bound together by a double covalent bond.

A

oxygen

131
Q

consists of one carbon atom bound to two
oxygen atoms.

A

Carbon dioxide

132
Q

four major groups of organic molecules essential to living organisms

A

carbohydrates
lipids
proteins
nucleic acids

133
Q

organic molecules composed primarily of carbon, hydrogen, and oxygen atoms and range in size from small to very
large.

A

carbohydrates

133
Q

Large carbohydrates are composed of numerous, relatively simple
building blocks called

A

monosaccharides

134
Q

molecules that have the same number and types of atoms but differ in their three-dimensional arrangement

A

isomers (ex. glucose, fructose, galactose)

135
Q

are composed of two
monosaccharides bound together through a dehydration reaction.

A

Disaccharides

136
Q

glucose and fructose combine to form a disaccharide called

A

sucrose

137
Q

glucose combined with galactose

A

Lactose

138
Q

two glucose molecules joined together

A

Maltose

139
Q

are long chains of monosaccharides

A

Polysaccharides

140
Q

a multibranched polysaccharide
composed of many glucose molecules

A

Glycogen

141
Q

main storage form of glucose in humans that is also an important energy-storage molecule.

A

Glycogen

142
Q

two important polysaccharides
found in plants

A

Starch and cellulose

143
Q

is an important
structural component of plant cell walls

A

cellulose

144
Q

can be broken down and used as an energy
source when humans ingest
plants

A

Starch

144
Q

can be broken down and used as an energy
source when humans ingest
plants

A
145
Q

eliminated in the feces, where it provides bulk as humans, do not have the digestive enzymes necessary to break down such

A

Cellulose

146
Q

a major group of organic molecules that are relatively insoluble in water.

A

Lipids

147
Q

broken down by hydrolysis reactions in cells
to release energy for use by those cells.

A

fats

148
Q

constitute 95% of the fats in l
the human body.

A

Triglycerides

149
Q

Triglycerides consist of two different types of
building blocks:

A

one glycerol and three fatty acids

150
Q

3-carbon molecule with a hydroxyl group attached to each carbon atom

A

Glycerol

151
Q

consists of both an oxygen atom
and a hydroxyl group attached to a carbon atom

A

carboxyl group

152
Q

contains only single covalent bonds between
the carbon atoms

A

saturated fatty acid

153
Q

one or more double
covalent bonds between carbon atoms (

A

unsaturated fatty acid

154
Q

one double covalent bond
between carbon atoms

A

Monounsaturated fats

155
Q

two or more double covalent
bonds between carbon atoms

A

Polyunsaturated fats

156
Q

unsaturated fats that have been chemically altered by the addition of hydrogen

A

Transfats

157
Q

similar to triglycerides,
except that one of the fatty acids bound to the glycerol is replaced by a phosphate-containing region

A

Phospholipids

158
Q

water-loving

A

hydrophilic

159
Q

water-fearing

A

hydrophobic

160
Q

composed of carbon atoms bound together into
four ringlike structures

A

steroid

161
Q

an especially important steroid because other steroid molecules are synthesized from it.

A

Cholesterol

162
Q

organic macromolecules that contain carbon,
hydrogen, oxygen, and nitrogen bound together by covalent bonds

A

Proteins

163
Q

The basic building blocks for proteins

A

20 amino acid

164
Q

Covalent bonds formed between amino acid molecules during protein synthesis

A

peptide bonds

165
Q

determined by the sequence of the amino acids bound by peptide bonds

A

primary structure

166
Q

results from the folding or bending of the polypeptide chain caused by the hydrogen bonds between amino acids

A

secondary structure

167
Q

change in shape caused by the breaking of
hydrogen bonds.

A

denaturation

168
Q

results from large-scale folding of
the protein driven by interactions within the protein and with the immediate environment

A

tertiary structure

169
Q

results from the association of two
or more proteins to form a functional unit

A

quaternary structure

170
Q

a protein catalyst that increases the
rate at which a chemical reaction proceeds without the enzyme being permanently changed

A

Enzymes

171
Q

region of the enzyme that binds reactants and catalyzes their conversion
to products.

A

active site

172
Q

an enzyme that catalyzes the breakdown of lipids

A

lipase

173
Q

an enzyme that breaks down proteins

A

protease

174
Q

are large molecules
composed of carbon, hydrogen, oxygen, nitrogen, and phosphorus

A

Nucleic Acids

175
Q

genetic material of cells

A

Deoxyribonucleic acid (DNA)

176
Q

contains the
information that determines the structure of proteins

A

DNA

177
Q

play important roles in protein synthesis.

A

Ribonucleic acid (RNA)

178
Q

The basic building blocks of DNA and RNA

A

nucleotides

179
Q

Each nucleotide is composed of a
a __ to which a nitrogenous base and a phosphate
group are attached

A

monosaccharide

180
Q

5-carbon monosaccharide for DNA; for RNA

A

deoxyribose; ribose

181
Q

Consist of carbon and nitrogen atoms organized into rings.

A

Nitrogenous
bases

182
Q

nitrogenous bases (5)

A

cytosine
thymine
uracil
guanine
adenine

183
Q

two strands of nucleotides joined together to form a twisted, ladderlike structure

A

double helix

184
Q

. Single-ringed bases

A

pyrimidines

185
Q

double-ringed bases

A

purines

186
Q

nucleotide of DNA

A

adenine
thymine
cytosine
guanine

187
Q

e bases held together by
hydrogen bonds

A

Complementary base pairs

188
Q

Complementary base pairs

A

Adenine and thymine
Cytosine and guanine

189
Q

A sequence of DNA bases that directs the synthesis of proteins or RNA molecules

A

gene

190
Q

nucleotide of RNA

A

thymine is replaced by uracil and can only be paired with adenine

191
Q

an especially important molecule for storing and providing energy
in all living organisms. I

A

Adenosine triphosphate

ANAPHY LECTURE (10 decks)

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