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Anatomy & Physiology > 2 Basic Chemistry, Inorganic Compounds > Flashcards

2 Basic Chemistry, Inorganic Compounds Flashcards

1
Q

matter

A

the “stuff” of the universe; anything that occupies space and has weight

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2
Q

anything that occupies space and has weight

A

matter

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3
Q

how can energy be measured?

A

only by its effects on matter

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4
Q

the ability to do work or put matter in motion

A

energy

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5
Q

energy

A

the ability to do work or put matter in motion

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6
Q

how is energy different from matter?

A

has no mass and does not take up space; energy effects matter

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7
Q

kinetic energy

A

energy that is being used; actually doing work like moving objects such as atoms or balls

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8
Q

energy that is being used; actually doing work like moving objects such as atoms or balls

A

kinetic energy

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9
Q

energy that is inactive or stored

A

potential energy

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10
Q

potential energy

A

energy that is inactive or stored

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11
Q

chemical energy

A

stored energy in the bonds of chemical substances; when the chemical bonds are broken, the potential energy becomes kinetic energy

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12
Q

stored energy in the bonds of chemical substances

A

chemical energy

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13
Q

electrical energy

A

energy resulting from the movement of charged particles (in your house, the flow of electrons along the wiring)

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14
Q

energy resulting from the movement of charged particles

A

electrical energy

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15
Q

example of electrical energy in the body

A

the nervous system uses electrical currents called nerve impulses to transmit messages

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16
Q

what kind of energy does the nervous system use when nerve impulses transmit messages throughout the body?

A

electrical energy

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17
Q

mechanical energy

A

energy directly involved in moving matter (legs provide the mechanical energy to power a bicycle; the muscles in your legs shortening to MOVE your legs)

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18
Q

energy directly involved in moving matter

A

mechanical energy

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19
Q

radiant energy

A

energy that travels in waves; the energy of the electromagnetic spectrum which includes x rays, infrared radiation (heat energy), visible light, radio, and ultraviolet rays

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20
Q

energy that travels in waves

A

radiant energy

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21
Q

how are energy conversions inefficient and how does that effect the body?

A

some of the initial energy supply is always “lost” to the environment as thermal energy–all energy conversions in the body generate heat

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22
Q

element

A

building block of matter; unique substance that cannot be broken down into simpler by ordinary chemical methods

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23
Q

building block of matter; unique substance that cannot be broken down into simpler by ordinary chemical methods

A

element

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24
Q

which four elements make up about 96% of body weight?

A

C carbon
O oxygen
H hydrogen
N nitrogen

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25
Q

subatomic particles

A

proton
neutron
electron

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26
Q

proton
neutron
electron

A

subatomic particles

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27
Q

relationship of protons and neutrons

A

both are heavy particles and have about the same mass; protons have a positive charge and neutrons are neutral

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28
Q

both of these subatomic particles are heavy particles and have about the same mass

A

protons

neutrons

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29
Q

relationship of protons and electrons

A

both have charges equal in strength, protons positive and electrons negative; protons have mass, neutrons mass is almost nonexistent

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30
Q

H

A

Hydrogen

1 proton, 0 neutron & 1 electron

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31
Q

atoms that have gained or lost electrons

A

ions

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32
Q

ions

A

atoms that have gained or lost electrons

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33
Q

atomic number

A

equal to the number of protons an element has

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34
Q

the number of protons an element has

A

atomic number

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35
Q

atomic mass

A

the sum of the masses of the protons and neutrons of an element

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36
Q

the sum of the masses of the protons and neutrons of an element

A

atomic mass

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37
Q

isotopes

A

the varieties of an element; will have same number of protons and electrons but different number of neutrons and therefor different atomic masses

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38
Q

the varieties of an element; will have same number of protons and electrons but different number of neutrons and therefore different atomic masses

A

isotopes

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39
Q

what determines the bonding properties of an atom?

A

the electrons

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40
Q

radioisotopes

A

the heavier isotopes of certain atoms that are unstable and tend to decompose to become more stable

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41
Q

the heavier isotopes of certain atoms that are unstable and tend to decompose to become more stable

A

radioisotopes

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42
Q

radioactivity

A

the process of spontaneous decay seen in some of the heavier isotopes, during which particles or energy is emitted from the atomic nucleus; results in the atom becoming more stable

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43
Q

the process of spontaneous decay seen in some of the heavier isotopes, during which particles or energy is emitted from the atomic nucleus; results in the atom becoming more stable

A

radioactivity

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44
Q

what can be compared to a tiny explosion in an atom?

A

radioactivity

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45
Q

what do all types of radioactive decay involve?

A

the ejection of particles (alpha or beta particles) or electromagnetic energy (gamma rays) from the atom’s nucleus and is damaging to living cells

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46
Q

what type of radioactivity has the least penetrating power?

A

Alpha emission

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47
Q

what type of radioactivity has the most penetrating power?

A

gamma radiation

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48
Q

where does the damage to the atoms in the path of ionizing radiation come from?

A

not from the radiation itself, but from the electrons that it sends flying like a bowling ball through pins

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49
Q

molecule

A

two or more atoms combine chemically (bind)

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50
Q

two or more atoms combine chemically (bind)

A

molecule

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51
Q

when two or more atoms of the same element bond together

A

a molecule of that element is produced

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52
Q

how is a molecule of an element produced?

A

when two or more atoms of the same element bond together

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53
Q

compound

A

when two or more different atoms bind together to form a molecule

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54
Q

when two or more different atoms bind together to form a molecule

A

compound

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55
Q

occur whenever atoms combine with or dissociate from other atoms (making or breaking bonds) #of atoms stay the same

A

chemical reactions

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56
Q

chemical reactions

A

whenever atoms combine with or dissociate from other atoms (making or breaking bonds) #of atoms stay the same

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57
Q

chemical bonds

A

formed when atoms unite chemically

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58
Q

formed when atoms unite chemically

A

chemical bonds; is an energy bond not a physical one

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59
Q

the only electrons that are important when considering bonding behavior are those in this shell

A

valence shell, the outermost shell

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60
Q

valence shell

A

the outermost shell; the only electrons that are important when considering bonding behavior are those in this shell

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61
Q

rule of eights

A

key to chemical reactivity; atoms react in such a ways that they will have 8 electrons in their valence shell (except Hydrogen with it being full at 2 electrons)

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62
Q

key to chemical reactivity; atoms react in such a ways that they will have 8 electrons in their valence shell (except Hydrogen with it being full at 2 electrons)

A

rule of eights

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63
Q

ionic bonds

A

electrons are completely transferred from one atom to another (others), the resulting charged atoms, or ions, are oppositely charged and attract each other

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64
Q

in this chemical bond, electrons are completely transferred from one atom to another (or others) the resulting charged atoms, or ions, are oppositely charged and attract each other

A

ionic bonds

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65
Q

ion

A

an atom with a positive or negative electric charge

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66
Q

an atom with a positive or negative electric charge

A

ion

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67
Q

negatively charged ions

A

anions

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68
Q

anions

A

negatively charged ions

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69
Q

cations

A

positively charged ions

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70
Q

positively charged ions

A

cations

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71
Q

ionic compound that dissociates into charged particles (other than hydrogen or hydroxyl ions) when dissolved in water

A

salt

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72
Q

salt

A

ionic compound that dissociates into charged particles (other than hydrogen or hydroxyl ions) when dissolved in water

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73
Q

covalent bonds

A

bonds created when atoms share electrons

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74
Q

molecules in which atoms share electrons

A

covalent molecules

75
Q

nonpolar covalently bonded molecules

A

molecules with covalent bonds in which the electrons have been shared equally between the atoms of the molecule

76
Q

molecules with covalent bonds in which the electrons have been shared equally between the atoms of the molecule

A

nonpolar covalently bonded molecules

77
Q

polar molecule

A

a molecule with two charged poles (- and +); nonsymmetrical and electrically unbalanced; the result of covalent bonds where one atom has a stronger electron attracting ability than another (more spots needing electrons)

78
Q

the result of covalent bonds where one atom has a stronger electron attracting ability than another (more spots needing electrons)

A

polar molecule

79
Q

a molecule with two charged poles (- and +)

A

polar molecule

80
Q

nonsymmetrical and electrically unbalanced molecule

A

polar molecule

81
Q

what kind of molecules do polar molecules orient themselves toward?

A

other polar molecules or charged particles (ions, proteins and others)

82
Q

hydrogen bond

A

weak bond in which a hydrogen atom forms a bridge between two electron-hungry atoms (nitrogen or oxygen) (surface tension)

83
Q

what kind of bond is surface tension?

A

hydrogen bond

84
Q

weak bond in which a hydrogen atom forms a bridge between two electron-hungry atoms

A

hydrogen bond

85
Q

synthesis reaction

A

chemical bond formation in which two or more atoms or molecules combine to form a larger, more complex molecule; energy absorbing reaction
A + B -> AB

86
Q

chemical bond formation in which two or more atoms or molecules combine to form a larger, more complex molecule; energy absorbing reaction
A + B -> AB

A

synthesis reaction

87
Q

what kind of chemical reaction underlies all anabolic (constructive) activities that occur in body cells?

A

synthesis reactions

88
Q

what kind of chemical reaction is particularly important for growth and for repair of worn-out or damaged tissues?

A

synthesis reactions

89
Q

decomposition reactions

A

chemical reactions that occur when a molecule is broken down into smaller molecules, atoms, or ions; energy releasing reaction
AB -> A + B

90
Q

chemical reactions that occur when a molecule is broken down into smaller molecules, atoms, or ions; energy releasing reaction
AB -> A + B

A

decomposition reactions

91
Q

what reactions are essentially synthesis reactions in revers?

A

decomposition reactions

92
Q

what kind of chemical reactions underlie all catabolic (destructive) processes that occur in our body cells?

A

decomposition reactions

93
Q

what are the three patterns most chemical reactions have?

A

synthesis reactions
decomposition reactions
exchange reactions

94
Q

chemical reactions that involve both synthesis and decomposition reactions; bond are both made and broken
AB + C-> AC + B and AB + CD -> AD + CB

A

exchange reactions

95
Q

exchange reactions

A

chemical reactions that involve both synthesis and decomposition reactions; bond are both made and broken
AB + C-> AC + B and AB + CD -> AD + CB

96
Q

digestion of foods is an example of what kind of chemical reaction?

A

decomposition reaction

97
Q

the breakdown of glycogen (a large carbohydrate molecule stored in the liver) to release glucose when blood sugar levels start to decline is an example of what kind of chemical reaction?

A

decomposition reaction

98
Q

when ATP reacts with glucose and transfers its end phosphate group to glucose, forming glucose-phosphate and ATP becomes ADP it is an example of what chemical reaction?

A

exchange reaction

99
Q

how is reversibility indicated in chemical equations?

A

by a double arrow (A+BAB

when the arrows differ in length the longer arrow indicates the more rapid reaction

100
Q

what does it mean when there is a double arrow in chemical equations and one arrow is longer than the other?

A

when the arrows differ in length the longer arrow indicates the more rapid reaction or the major direction in which the reaction is proceeding

101
Q

what must occur for atoms and molecules to react chemically?

A

they must collide forcefully so that the electrons in their valence shells can interact. Bond making and breaking cannot occur long distance.

102
Q

what are the two major classes of molecules all chemicals found in the body fall into?

A

inorganic or organic

103
Q

what determines whether the class of a compound is inorganic or organic?

A

determined solely by the presence or absence of carbon (with a few unexplained exceptions such as carbon dioxide gas [CO2] and carbon monoxide [CO])

104
Q

what does the presence of carbon determine?

A

whether a compound is inorganic or organic

105
Q

inorganic compounds

A

lack carbon and tend to be small, simple molecules

water, salts, and many [not all] acids and bases

106
Q

lack carbon and tend to be small, simple molecules

A

inorganic compounds

water, salts, and many [not all] acids and bases

107
Q

organic compounds

A

carbon-containing compounds
fairly (or very) large covalently-bonded molecules
(carbohydrates, lipids, proteins, nucleic acids)

108
Q

between organic and inorganic compounds, which contain carbon?

A

organic compounds contain carbon

109
Q

examples of inorganic compounds found in the body

A

water, salts, and many (but not all) acids and bases

110
Q

water, salts, and many (but not all) acids and bases

A

examples of inorganic compounds found in the body

111
Q

examples of important organic compounds found in the body

A

carbohydrates
lipids
proteins
nucleic acids

112
Q

how are organic compounds bonded?

A

with covalent bonds

113
Q

how do organic and inorganic compounds compare in size?

A

organic are bigger, inorganic tend to be small and simple

114
Q

what are factors that increase the rate of chemical reactions?

A

higher temperature
higher concentration of reacting particles
smaller particle size
the presence of catalysts

115
Q

how does a higher temperature increase the rate of chemical reactions?

A

increased kinetic energy of the molecules, which in turn move more rapidly and collide more forcefully

116
Q

how does a higher concentration of reacting particles increase the rate of chemical reactions?

A

increases the number of collision s because of increased numbers of reacting particles

117
Q

how does a smaller particle size increase the rate of chemical reactions?

A

smaller particles have more kinetic energy and move faster than larger ones, so they take part in more collisions

118
Q

how does the presence of catalysts increase the rate of chemical reactions?

A

catalysts lower the amount of energy the molecules need to interact by holding the reactants in the proper position to interact

119
Q

what is the most abundant inorganic compound in the body?

A

water

120
Q

what accounts for about two-thirds of body weight?

A

water

121
Q

water accounts for about how much of body weight?

A

two-thirds

122
Q

what are some factors that make water so vital in the body?

A

high heat capacity
polarity/solvent properties
chemical reactivity
cushioning

123
Q

what does it mean to have a high heat capacity in water?

A

absorbs and releases large amounts of heat before its temperature changes appreciably

124
Q

how does having a high heat capacity make water important to the body?

A

prevents sudden changes in body temperature because of factors such as sun, wind, or vigorous internal activity (keeps a homeostatic body temperature)

125
Q

“universal solvent”

A

water-because of its polarity, water is an excellent solvent

126
Q

solvent

A

a liquid or gas in which smaller amounts of other substances (called solutes) can be dissolved or suspended

127
Q

a liquid or gas in which smaller amounts of other substances can be dissolved or suspended

A

solvent

128
Q

how does having polarity/solvent properties make water important to the body?

A

Dissolves and Distributes
Facilitate chemical reactions
Transports
Lubricates

129
Q

the importance of water’s polarity/solvent properties dissolving chemicals

A

small reactive chemicals (salts, acids, bases) dissolve easily in water and become evenly distributed

130
Q

the importance of water’s polarity/solvent properties in chemical reactions

A

molecules cannot react chemically unless they are in a solution–virtually all chemical reactions that occur in the body depend on water

131
Q

the importance of water’s polarity/solvent properties in transport

A

Acts as a transport since nutrients, respiratory gases (oxygen and carbon dioxide) and wastes can dissolve in water; all these substances are carried in blood plasma and are exchanged between blood and tissue through interstitial fluid

132
Q

the importance of water’s polarity/solvent properties in lubrication

A

specialized molecules that lubricate the body (like mucus) use water as their solvent, and synovial fluid “oil” the ends of bones as they move within joint cavities

133
Q

hydrolysis reactions

A

chemical reaction using water to split substance into smaller particles; water molecules are added to the bonds of larger molecules; like digesting food

134
Q

chemical reaction using water to split substance into smaller particles

A

hydrolysis reaction

135
Q

salt

A

an ionic compound containing cations other than H+ and anions other than the hydroxyl ion (OH-)

136
Q

an ionic compound containing cations other than H+ and anions other than the hydroxyl ion (OH-)

A

salt

137
Q

salts of many metal elements are found in the body, the most plentiful salts are those containing these

A

calcium and phosphorus, found chiefly in bones and teeth

138
Q

when dissolved in body fluids, what happens to salts?

A

easily separate into their ions (dissociate)

139
Q

dissociation

A

salts dissolved in water (body fluid) separating into their charged ions and dispersing; the charged elements orienting with the polar ends of the water molecules

140
Q

because ions are charged particles, all salts are this

A

electrolytes

141
Q

substances that conduct an electrical current in solution

A

electrolytes

142
Q

electrolytes

A

substances that conduce an electrical current in solution

143
Q

what happens in the body when ionic (electrolyte) balance is severely disturbed

A

virtually nothing in the body works

144
Q

which ions are essential for nerve impulses?

A

sodium and potassium ions

145
Q

salts acids and bases are all what?

A

electrolytes; ionize then dissociate in water and can then conduct an electrical current

146
Q

OH-

A

hydroxyl ion

147
Q

H+

A

hydrogen ion

148
Q

substance that can release hydrogen ions (H+) in detectable amounts

A

acid

149
Q

proton donors

A

acids; a hydrogen ion is essentially a hydrogen nucleus (naked proton)

150
Q

acid

A

have a sour taste
substance that can release hydrogen ions (H+) in detectable amounts
dissolves many metals and “burns”

151
Q

what happens when acids are dissolved in water?

A

they release hydrogen ions and some anions; it’s the releases of the protons that determines the effects on it’s environment

152
Q

acids found or produced in the body

A 
hydrochloric acid (acid produced by stomach)
acetic acid (vinegar)
carbonic acid
153
Q

strong acids

A

acids that ionize completely and liberate all of their protons (like hydrochloric acid)

154
Q

acids that ionize completely and liberate all of their protons

A

strong acids

155
Q

weak acids

A

acids that ionize incompletely (like carbonic acid)

156
Q

acids that ionize incompletely

A

weak acids

157
Q

a substance that can release hydroxide ions (OH-) in detectable amounts

A

base

158
Q

bases

A

have a bitter taste, feel slippery

proton acceptors

159
Q

what happens when bases are dissolved in water?

A

they release hydroxyl ions and some cations

160
Q

strong base

A

any base containing the hydroxyl ion (OH-) because it is a strong proton (H+) seeker

161
Q

what happens when acids and bases mix?

A

they react with each other (in an exchange reaction) to form water and salt; called neutralization reaction

162
Q

neutralization reaction

A

exchange reaction in which acids and bases react and form water and salt
HCl + NaOH –> H2O + NaCl

163
Q

pH

A

the unit measure of the relative concentration of hydrogen (and hydroxyl) ions in various fluid
based on the number of protons in terms of moles per liter
runs on a scale of 0-14 each change of pH units is a ten-fold change in hydrogen-ion
pH of 0 is hydrochloric acid (all H+)
pH of 14 is Sodium hydroxide (almost all OH-)

164
Q

what does a pH scale of seven indicate?

A

the scale midpoint, means the number of hydrogen ions (H+) exactly equals the number of hydroxyl ions; the solution is neutral

165
Q

pH below 7

A

solution is acidic; the hydrogen ions (H+) outnumber the hydroxyl ions (OH-) the number goes down, the concentration of H+ gets higher

166
Q

pH above 7

A

solution is alkaline, or basic; the hydroxyl ions (OH-) outnumber the hydrogen ions (H+) number goes up, the concentration of H+ gets smaller

167
Q

living cells are sensitive to change in pH; what regulates the acid-base balance in the body?

A

kidneys
lungs
chemicals called buffers, present in body fluid

168
Q

what is an important part of the body’s buffer system?

A

weak bases and acids which help maintain stability by taking up excess hydrogen or hydroxyl ions

169
Q

what is the pH of blood?

A

close to neutral (7.4)

170
Q

a hydrogen ion H+ is the same as a

A

proton

171
Q

acidic foods can be determined by what taste?

A

sour

172
Q

OH- is called the _____

A

hydroxide ion

173
Q

acids increase the concentration of what in water?

A

H+ ions

174
Q

bases can be referred to as

A

proton acceptors

175
Q

NaOH sodium hydroxide

A

bleach

176
Q

bleach

A

NaOH sodium hydroxide, basic

177
Q

chemical reactions that cause things to get colder

A

endothermic

178
Q

endothermic

A

chemical reactions that cause things to get colder

179
Q

chemical reactions that cause things to get hotter

A

exothermic

180
Q

exothermic

A

chemical reactions that cause things to get hotter

181
Q

NaOH sodium hydroxide

A

bleach

182
Q

bleach

A

basic; sodium hydroxide (NaOH)

183
Q

matter exists in what three states?

A

gas
liquid
solid

Anatomy & Physiology (13 decks)

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