2 Basic Chemistry, Inorganic Compounds Flashcards
1
Q
matter
A
the “stuff” of the universe; anything that occupies space and has weight
2
Q
anything that occupies space and has weight
A
matter
3
Q
how can energy be measured?
A
only by its effects on matter
4
Q
the ability to do work or put matter in motion
A
energy
5
Q
energy
A
the ability to do work or put matter in motion
6
Q
how is energy different from matter?
A
has no mass and does not take up space; energy effects matter
7
Q
kinetic energy
A
energy that is being used; actually doing work like moving objects such as atoms or balls
8
Q
energy that is being used; actually doing work like moving objects such as atoms or balls
A
kinetic energy
9
Q
energy that is inactive or stored
A
potential energy
10
Q
potential energy
A
energy that is inactive or stored
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
12
Q
stored energy in the bonds of chemical substances
A
chemical energy
13
Q
electrical energy
A
energy resulting from the movement of charged particles (in your house, the flow of electrons along the wiring)
14
Q
energy resulting from the movement of charged particles
A
electrical energy
15
Q
example of electrical energy in the body
A
the nervous system uses electrical currents called nerve impulses to transmit messages
16
Q
what kind of energy does the nervous system use when nerve impulses transmit messages throughout the body?
A
electrical energy
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)
18
Q
energy directly involved in moving matter
A
mechanical energy
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
20
Q
energy that travels in waves
A
radiant energy
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
22
Q
element
A
building block of matter; unique substance that cannot be broken down into simpler by ordinary chemical methods
23
Q
building block of matter; unique substance that cannot be broken down into simpler by ordinary chemical methods
A
element
24
Q
which four elements make up about 96% of body weight?
A
C carbon
O oxygen
H hydrogen
N nitrogen
25
subatomic particles
proton
neutron
electron
26
proton
neutron
electron
subatomic particles
27
relationship of protons and neutrons
both are heavy particles and have about the same mass; protons have a positive charge and neutrons are neutral
28
both of these subatomic particles are heavy particles and have about the same mass
protons
| neutrons
29
relationship of protons and electrons
both have charges equal in strength, protons positive and electrons negative; protons have mass, neutrons mass is almost nonexistent
30
H
Hydrogen
| 1 proton, 0 neutron & 1 electron
31
atoms that have gained or lost electrons
ions
32
ions
atoms that have gained or lost electrons
33
atomic number
equal to the number of protons an element has
34
the number of protons an element has
atomic number
35
atomic mass
the sum of the masses of the protons and neutrons of an element
36
the sum of the masses of the protons and neutrons of an element
atomic mass
37
isotopes
the varieties of an element; will have same number of protons and electrons but different number of neutrons and therefor different atomic masses
38
the varieties of an element; will have same number of protons and electrons but different number of neutrons and therefore different atomic masses
isotopes
39
what determines the bonding properties of an atom?
the electrons
40
radioisotopes
the heavier isotopes of certain atoms that are unstable and tend to decompose to become more stable
41
the heavier isotopes of certain atoms that are unstable and tend to decompose to become more stable
radioisotopes
42
radioactivity
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
43
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
radioactivity
44
what can be compared to a tiny explosion in an atom?
radioactivity
45
what do all types of radioactive decay involve?
the ejection of particles (alpha or beta particles) or electromagnetic energy (gamma rays) from the atom's nucleus and is damaging to living cells
46
what type of radioactivity has the least penetrating power?
Alpha emission
47
what type of radioactivity has the most penetrating power?
gamma radiation
48
where does the damage to the atoms in the path of ionizing radiation come from?
not from the radiation itself, but from the electrons that it sends flying like a bowling ball through pins
49
molecule
two or more atoms combine chemically (bind)
50
two or more atoms combine chemically (bind)
molecule
51
when two or more atoms of the same element bond together
a molecule of that element is produced
52
how is a molecule of an element produced?
when two or more atoms of the same element bond together
53
compound
when two or more different atoms bind together to form a molecule
54
when two or more different atoms bind together to form a molecule
compound
55
occur whenever atoms combine with or dissociate from other atoms (making or breaking bonds) #of atoms stay the same
chemical reactions
56
chemical reactions
whenever atoms combine with or dissociate from other atoms (making or breaking bonds) #of atoms stay the same
57
chemical bonds
formed when atoms unite chemically
58
formed when atoms unite chemically
chemical bonds; is an energy bond not a physical one
59
the only electrons that are important when considering bonding behavior are those in this shell
valence shell, the outermost shell
60
valence shell
the outermost shell; the only electrons that are important when considering bonding behavior are those in this shell
61
rule of eights
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)
62
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)
rule of eights
63
ionic bonds
electrons are completely transferred from one atom to another (others), the resulting charged atoms, or ions, are oppositely charged and attract each other
64
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
ionic bonds
65
ion
an atom with a positive or negative electric charge
66
an atom with a positive or negative electric charge
ion
67
negatively charged ions
anions
68
anions
negatively charged ions
69
cations
positively charged ions
70
positively charged ions
cations
71
ionic compound that dissociates into charged particles (other than hydrogen or hydroxyl ions) when dissolved in water
salt
72
salt
ionic compound that dissociates into charged particles (other than hydrogen or hydroxyl ions) when dissolved in water
73
covalent bonds
bonds created when atoms share electrons
74
molecules in which atoms share electrons
covalent molecules
75
nonpolar covalently bonded molecules
molecules with covalent bonds in which the electrons have been shared equally between the atoms of the molecule
76
molecules with covalent bonds in which the electrons have been shared equally between the atoms of the molecule
nonpolar covalently bonded molecules
77
polar molecule
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
the result of covalent bonds where one atom has a stronger electron attracting ability than another (more spots needing electrons)
polar molecule
79
a molecule with two charged poles (- and +)
polar molecule
80
nonsymmetrical and electrically unbalanced molecule
polar molecule
81
what kind of molecules do polar molecules orient themselves toward?
other polar molecules or charged particles (ions, proteins and others)
82
hydrogen bond
weak bond in which a hydrogen atom forms a bridge between two electron-hungry atoms (nitrogen or oxygen) (surface tension)
83
what kind of bond is surface tension?
hydrogen bond
84
weak bond in which a hydrogen atom forms a bridge between two electron-hungry atoms
hydrogen bond
85
synthesis reaction
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
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
synthesis reaction
87
what kind of chemical reaction underlies all anabolic (constructive) activities that occur in body cells?
synthesis reactions
88
what kind of chemical reaction is particularly important for growth and for repair of worn-out or damaged tissues?
synthesis reactions
89
decomposition reactions
chemical reactions that occur when a molecule is broken down into smaller molecules, atoms, or ions; energy releasing reaction
AB -> A + B
90
chemical reactions that occur when a molecule is broken down into smaller molecules, atoms, or ions; energy releasing reaction
AB -> A + B
decomposition reactions
91
what reactions are essentially synthesis reactions in revers?
decomposition reactions
92
what kind of chemical reactions underlie all catabolic (destructive) processes that occur in our body cells?
decomposition reactions
93
what are the three patterns most chemical reactions have?
synthesis reactions
decomposition reactions
exchange reactions
94
chemical reactions that involve both synthesis and decomposition reactions; bond are both made and broken
AB + C-> AC + B and AB + CD -> AD + CB
exchange reactions
95
exchange reactions
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
digestion of foods is an example of what kind of chemical reaction?
decomposition reaction
97
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?
decomposition reaction
98
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?
exchange reaction
99
how is reversibility indicated in chemical equations?
by a double arrow (A+BAB
| when the arrows differ in length the longer arrow indicates the more rapid reaction
100
what does it mean when there is a double arrow in chemical equations and one arrow is longer than the other?
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
what must occur for atoms and molecules to react chemically?
they must collide forcefully so that the electrons in their valence shells can interact. Bond making and breaking cannot occur long distance.
102
what are the two major classes of molecules all chemicals found in the body fall into?
inorganic or organic
103
what determines whether the class of a compound is inorganic or organic?
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
what does the presence of carbon determine?
whether a compound is inorganic or organic
105
inorganic compounds
lack carbon and tend to be small, simple molecules
| water, salts, and many [not all] acids and bases
106
lack carbon and tend to be small, simple molecules
inorganic compounds
| water, salts, and many [not all] acids and bases
107
organic compounds
carbon-containing compounds
fairly (or very) large covalently-bonded molecules
(carbohydrates, lipids, proteins, nucleic acids)
108
between organic and inorganic compounds, which contain carbon?
organic compounds contain carbon
109
examples of inorganic compounds found in the body
water, salts, and many (but not all) acids and bases
110
water, salts, and many (but not all) acids and bases
examples of inorganic compounds found in the body
111
examples of important organic compounds found in the body
carbohydrates
lipids
proteins
nucleic acids
112
how are organic compounds bonded?
with covalent bonds
113
how do organic and inorganic compounds compare in size?
organic are bigger, inorganic tend to be small and simple
114
what are factors that increase the rate of chemical reactions?
higher temperature
higher concentration of reacting particles
smaller particle size
the presence of catalysts
115
how does a higher temperature increase the rate of chemical reactions?
increased kinetic energy of the molecules, which in turn move more rapidly and collide more forcefully
116
how does a higher concentration of reacting particles increase the rate of chemical reactions?
increases the number of collision s because of increased numbers of reacting particles
117
how does a smaller particle size increase the rate of chemical reactions?
smaller particles have more kinetic energy and move faster than larger ones, so they take part in more collisions
118
how does the presence of catalysts increase the rate of chemical reactions?
catalysts lower the amount of energy the molecules need to interact by holding the reactants in the proper position to interact
119
what is the most abundant inorganic compound in the body?
water
120
what accounts for about two-thirds of body weight?
water
121
water accounts for about how much of body weight?
two-thirds
122
what are some factors that make water so vital in the body?
high heat capacity
polarity/solvent properties
chemical reactivity
cushioning
123
what does it mean to have a high heat capacity in water?
absorbs and releases large amounts of heat before its temperature changes appreciably
124
how does having a high heat capacity make water important to the body?
prevents sudden changes in body temperature because of factors such as sun, wind, or vigorous internal activity (keeps a homeostatic body temperature)
125
"universal solvent"
water-because of its polarity, water is an excellent solvent
126
solvent
a liquid or gas in which smaller amounts of other substances (called solutes) can be dissolved or suspended
127
a liquid or gas in which smaller amounts of other substances can be dissolved or suspended
solvent
128
how does having polarity/solvent properties make water important to the body?
Dissolves and Distributes
Facilitate chemical reactions
Transports
Lubricates
129
the importance of water's polarity/solvent properties dissolving chemicals
small reactive chemicals (salts, acids, bases) dissolve easily in water and become evenly distributed
130
the importance of water's polarity/solvent properties in chemical reactions
molecules cannot react chemically unless they are in a solution--virtually all chemical reactions that occur in the body depend on water
131
the importance of water's polarity/solvent properties in transport
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
the importance of water's polarity/solvent properties in lubrication
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
hydrolysis reactions
chemical reaction using water to split substance into smaller particles; water molecules are added to the bonds of larger molecules; like digesting food
134
chemical reaction using water to split substance into smaller particles
hydrolysis reaction
135
salt
an ionic compound containing cations other than H+ and anions other than the hydroxyl ion (OH-)
136
an ionic compound containing cations other than H+ and anions other than the hydroxyl ion (OH-)
salt
137
salts of many metal elements are found in the body, the most plentiful salts are those containing these
calcium and phosphorus, found chiefly in bones and teeth
138
when dissolved in body fluids, what happens to salts?
easily separate into their ions (dissociate)
139
dissociation
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
because ions are charged particles, all salts are this
electrolytes
141
substances that conduct an electrical current in solution
electrolytes
142
electrolytes
substances that conduce an electrical current in solution
143
what happens in the body when ionic (electrolyte) balance is severely disturbed
virtually nothing in the body works
144
which ions are essential for nerve impulses?
sodium and potassium ions
145
salts acids and bases are all what?
electrolytes; ionize then dissociate in water and can then conduct an electrical current
146
OH-
hydroxyl ion
147
H+
hydrogen ion
148
substance that can release hydrogen ions (H+) in detectable amounts
acid
149
proton donors
acids; a hydrogen ion is essentially a hydrogen nucleus (naked proton)
150
acid
have a sour taste
substance that can release hydrogen ions (H+) in detectable amounts
dissolves many metals and "burns"
151
what happens when acids are dissolved in water?
they release hydrogen ions and some anions; it's the releases of the protons that determines the effects on it's environment
152
acids found or produced in the body
```
hydrochloric acid (acid produced by stomach)
acetic acid (vinegar)
carbonic acid
```
153
strong acids
acids that ionize completely and liberate all of their protons (like hydrochloric acid)
154
acids that ionize completely and liberate all of their protons
strong acids
155
weak acids
acids that ionize incompletely (like carbonic acid)
156
acids that ionize incompletely
weak acids
157
a substance that can release hydroxide ions (OH-) in detectable amounts
base
158
bases
have a bitter taste, feel slippery
| proton acceptors
159
what happens when bases are dissolved in water?
they release hydroxyl ions and some cations
160
strong base
any base containing the hydroxyl ion (OH-) because it is a strong proton (H+) seeker
161
what happens when acids and bases mix?
they react with each other (in an exchange reaction) to form water and salt; called neutralization reaction
162
neutralization reaction
exchange reaction in which acids and bases react and form water and salt
HCl + NaOH --> H2O + NaCl
163
pH
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
what does a pH scale of seven indicate?
the scale midpoint, means the number of hydrogen ions (H+) exactly equals the number of hydroxyl ions; the solution is neutral
165
pH below 7
solution is acidic; the hydrogen ions (H+) outnumber the hydroxyl ions (OH-) the number goes down, the concentration of H+ gets higher
166
pH above 7
solution is alkaline, or basic; the hydroxyl ions (OH-) outnumber the hydrogen ions (H+) number goes up, the concentration of H+ gets smaller
167
living cells are sensitive to change in pH; what regulates the acid-base balance in the body?
kidneys
lungs
chemicals called buffers, present in body fluid
168
what is an important part of the body's buffer system?
weak bases and acids which help maintain stability by taking up excess hydrogen or hydroxyl ions
169
what is the pH of blood?
close to neutral (7.4)
170
a hydrogen ion H+ is the same as a
proton
171
acidic foods can be determined by what taste?
sour
172
OH- is called the _____
hydroxide ion
173
acids increase the concentration of what in water?
H+ ions
174
bases can be referred to as
proton acceptors
175
NaOH sodium hydroxide
bleach
176
bleach
NaOH sodium hydroxide, basic
177
chemical reactions that cause things to get colder
endothermic
178
endothermic
chemical reactions that cause things to get colder
179
chemical reactions that cause things to get hotter
exothermic
180
exothermic
chemical reactions that cause things to get hotter
181
NaOH sodium hydroxide
bleach
182
bleach
basic; sodium hydroxide (NaOH)
183
matter exists in what three states?
gas
liquid
solid
