Chapter 2 Flashcards
(142 cards)
1
Q
acid
A
molecule that donates hydrogen ions and increases the concentration of hydrogen ions in a solution
2
Q
molecule that donates hydrogen ions and increases the concentration of hydrogen ions in a solution
A
Acid
3
Q
adhesion
A
attraction between water molecules and other molecules
4
Q
attraction between water molecules and other molecules
A
adhesion
5
Q
aliphatic hydrocarbon
A
hydrocarbon consisting of a linear chain of carbon atoms
6
Q
hydrocarbon consisting of a linear chain of carbon atoms
A
aliphatic hydrocarbon
7
Q
anion
A
negative ion that is formed by an atom gaining one or more electrons
8
Q
hydrocarbon consisting of closed rings of carbon atoms
A
aromatic hydrocarbon
9
Q
atom
A
the smallest unit of matter that retains all of the chemical properties of an element
9
Q
aromatic hydrocarbon
A
hydrocarbon consisting of closed rings of carbon atoms
9
Q
negative ion that is formed by an atom gaining one or more electrons
A
anion
10
Q
calculated mean of the mass number for an element’s isotopes
A
atomic mass
11
Q
atomic number
A
total number of protons in an atom
11
Q
the smallest unit of matter that retains all of the chemical properties of an element
A
atom
11
Q
atomic mass
A
calculated mean of the mass number for an element’s isotopes
12
Q
total number of protons in an atom
A
atomic number
13
Q
balanced chemical equation
A
statement of a chemical reaction with the number of each type of atom equalized for both the products and reactants
14
Q
statement of a chemical reaction with the number of each type of atom equalized for both the products and reactants
A
balanced chemical equation
15
Q
base
A
molecule that donates hydroxide ions or otherwise binds excess hydrogen ions and decreases the concentration of hydrogen ions in a solution
16
Q
molecule that donates hydroxide ions or otherwise binds excess hydrogen ions and decreases the concentration of hydrogen ions in a solution
A
base
17
Q
buffer
A
substance that prevents a change in pH by absorbing or releasing hydrogen or hydroxide ions
18
Q
substance that prevents a change in pH by absorbing or releasing hydrogen or hydroxide ions
A
buffer
19
Q
calorie
A
amount of heat required to change the temperature of one gram of water by one degree
Celsius.
20
Q
amount of heat required to change the temperature of one gram of water by one degree
Celsius.
A
calorie
21
capillary action
occurs because water molecules are attracted to charges on the inner surfaces of narrow tubular structures such as glass tubes, drawing the water molecules to the sides of the tubes.
22
occurs because water molecules are attracted to charges on the inner surfaces of narrow tubular structures such as glass tubes, drawing the water molecules to the sides of the tubes.
capillary action
23
cation
positive ion that is formed by an atom losing one or more electrons
24
chemical bond
interaction between two or more of the same or different atoms that results in the
formation of molecules
24
positive ion that is formed by an atom losing one or more electrons
cation
25
interaction between two or more of the same or different atoms that results in the
formation of molecules
chemical bond
26
chemical reaction
process leading to the rearrangement of atoms in molecules
27
process leading to the rearrangement of atoms in molecules
chemical reaction
28
chemical reactivity
the ability to combine and to chemically bond with each other
29
intermolecular forces between water molecules caused by the polar nature of water; responsible for surface tension
cohesion
30
the ability to combine and to chemically bond with each other
chemical reactivity
31
cohesion
intermolecular forces between water molecules caused by the polar nature of water; responsible for surface tension
32
compound
substance composed of molecules consisting of atoms of at least two different elements
33
substance composed of molecules consisting of atoms of at least two different elements
compound
34
covalent bond
type of strong bond formed between two of the same or different elements; forms
when electrons are shared between atoms
35
type of strong bond formed between two of the same or different elements; forms
when electrons are shared between atoms
covalent bond
36
release of an ion from a molecule such that the original molecule now consists of an ion and the charged remains of the original, such as when water dissociates into H+ and OH-
dissociation
37
ion necessary for nerve impulse conduction, muscle contractions and water balance
electrolyte
37
dissociation
release of an ion from a molecule such that the original molecule now consists of an ion and the charged remains of the original, such as when water dissociates into H+ and OH-
38
electrolyte
ion necessary for nerve impulse conduction, muscle contractions and water balance
38
arrangement of electrons in an atom’s electron shell (for example,
1s22s22p6)
electron configuration
39
electron configuration
arrangement of electrons in an atom’s electron shell (for example,
1s22s22p6)
40
electron orbital
how electrons are spatially distributed surrounding the nucleus; the area where an electron is most likely to be found
41
how electrons are spatially distributed surrounding the nucleus; the area where an electron is most likely to be found
electron orbital
42
electron transfer
movement of electrons from one element to another; important in creation of ionic bonds
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movement of electrons from one element to another; important in creation of ionic bonds
electron transfer
44
electronegativity
electronegativity ability of some elements to attract electrons (often of hydrogen atoms), acquiring partial negative charges in molecules and creating partial positive charges on the hydrogen atoms.
45
one of 118 unique substances that cannot be broken down into smaller substances; each element has unique properties and a specified number of protons
element
46
negatively charged subatomic particle that resides outside of the nucleus in the electron orbital; lacks functional mass and has a negative charge of –1 unit.
electron
46
ability of some elements to attract electrons (often of hydrogen atoms), acquiring partial negative charges in molecules and creating partial positive charges on the hydrogen atoms.
electronegativity
47
electron
negatively charged subatomic particle that resides outside of the nucleus in the electron orbital; lacks functional mass and has a negative charge of –1 unit.
48
element
one of 118 unique substances that cannot be broken down into smaller substances; each element has unique properties and a specified number of protons
49
enantiomers
molecules that share overall structure and bonding patterns, but differ in how the atoms are three dimensionally placed such that they are mirror images of each other
50
molecules that share overall structure and bonding patterns, but differ in how the atoms are three dimensionally placed such that they are mirror images of each other
enantiomers
51
equilibrium
steady state of relative reactant and product concentration in reversible chemical reactions in a closed system
52
steady state of relative reactant and product concentration in reversible chemical reactions in a closed system
equilibrium
53
evaporation
separation of individual molecules from the surface of a body of water, leaves of a plant, or the skin of an organism
54
separation of individual molecules from the surface of a body of water, leaves of a plant, or the skin of an organism
evaporation
55
functional group
group of atoms that provides or imparts a specific function to a carbon skeleton
56
geometric isomer
isomer with similar bonding patterns differing in the placement of atoms
alongside a double covalent bond
57
group of atoms that provides or imparts a specific function to a carbon skeleton
functional group
58
isomer with similar bonding patterns differing in the placement of atoms
alongside a double covalent bond
geometric isomer
59
heat of vaporization of water
high amount of energy required for liquid water to turn into water vapor
60
high amount of energy required for liquid water to turn into water vapor
heat of vaporization of water
61
hydrocarbon
molecule that consists only of carbon and hydrogen
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molecule that consists only of carbon and hydrogen
hydrocarbon
63
hydrogen bond
weak bond between slightly positively charged hydrogen atoms to slightly
negatively charged atoms in other molecules
64
weak bond between slightly positively charged hydrogen atoms to slightly
negatively charged atoms in other molecules
hydrogen bond
65
hydrophilic
describes ions or polar molecules that interact well with other polar molecules such as water
66
describes ions or polar molecules that interact well with other polar molecules such as water
hydrophilic
67
hydrophobic
describes uncharged non-polar molecules that do not interact well with polar molecules such as water
68
describes uncharged non-polar molecules that do not interact well with polar molecules such as water
hydrophobic
69
inert gas (also, noble gas)
element with filled outer electron shell that is unreactive with other atoms
70
element with filled outer electron shell that is unreactive with other atoms
inert gas (also, noble gas)
71
ionic bond
chemical bond that forms between ions with opposite charges (cations and anions)
72
chemical bond that forms between ions with opposite charges (cations and anions)
ionic bond
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atom or chemical group that does not contain equal numbers of protons and electrons
ion
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ion
atom or chemical group that does not contain equal numbers of protons and electrons
75
irreversible chemical reaction
chemical reaction where reactants proceed uni-directionally to form products
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chemical reaction where reactants proceed uni-directionally to form products
irreversible chemical reaction
77
isomers
molecules that differ from one another even though they share the same chemical formula
78
isotope
one or more forms of an element that have different numbers of neutrons
79
molecules that differ from one another even though they share the same chemical formula
isomers
80
one or more forms of an element that have different numbers of neutrons
isotope
81
law of mass action
chemical law stating that the rate of a reaction is proportional to the concentration of the reacting substances
82
chemical law stating that the rate of a reaction is proportional to the concentration of the reacting substances
law of mass action
83
litmus paper (also, pH paper)
filter paper that has been treated with a natural water-soluble dye that changes its color as the pH of the environment changes so it can be used as a pH indicator
84
filter paper that has been treated with a natural water-soluble dye that changes its color as the pH of the environment changes so it can be used as a pH indicator
litmus paper (also, pH paper)
85
mass number
total number of protons and neutrons in an atom
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total number of protons and neutrons in an atom
mass number
87
molecule
two or more atoms chemically bonded together
88
matter
anything that has mass and occupies space
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anything that has mass and occupies space
matter
90
molecule two or more atoms chemically bonded together
molecule
91
neutron
uncharged particle that resides in the nucleus of an atom; has a mass of one amu
92
uncharged particle that resides in the nucleus of an atom; has a mass of one amu
neutron
93
nucleus
core of an atom; contains protons and neutrons
93
nonpolar covalent bond
type of covalent bond that forms between atoms when electrons are shared equally between them
94
type of covalent bond that forms between atoms when electrons are shared equally between them
nonpolar covalent bond
95
core of an atom; contains protons and neutrons
nucleus
96
octet rule
rule that atoms are most stable when they hold eight electrons in their outermost shells
96
rule that atoms are most stable when they hold eight electrons in their outermost shells
octet rule
97
orbital
region surrounding the nucleus; contains electrons
98
region surrounding the nucleus; contains electrons
orbital
99
organic molecule
any molecule containing carbon (except carbon dioxide)
100
any molecule containing carbon (except carbon dioxide)
organic molecule
100
scale ranging from zero to 14 that is inversely proportional to the concentration of hydrogen ions in a solution
pH scale
101
periodic table
organizational chart of elements indicating the atomic number and atomic mass of each element; provides key information about the properties of the elements
101
pH scale
scale ranging from zero to 14 that is inversely proportional to the concentration of hydrogen ions in a solution
102
organizational chart of elements indicating the atomic number and atomic mass of each element; provides key information about the properties of the elements
periodic table
103
polar covalent bond
type of covalent bond that forms as a result of unequal sharing of electrons, resulting in the creation of slightly positive and slightly negative charged regions of the molecule
104
type of covalent bond that forms as a result of unequal sharing of electrons, resulting in the creation of slightly positive and slightly negative charged regions of the molecule
polar covalent bond
105
product
molecule found on the right side of a chemical equation
106
molecule found on the right side of a chemical equation
product
107
proton
positively charged particle that resides in the nucleus of an atom; has a mass of one amu and a
charge of +1
108
positively charged particle that resides in the nucleus of an atom; has a mass of one amu and a
charge of +1
proton
109
isotope that emits radiation composed of subatomic particles to form more stable elements
radioisotope
109
radioisotope
isotope that emits radiation composed of subatomic particles to form more stable elements
110
reactant
molecule found on the left side of a chemical equation
111
molecule found on the left side of a chemical equation
reactant
112
reversible chemical reaction
chemical reaction that functions bi-directionally, where products
may turn into reactants if their concentration is great enough
113
chemical reaction that functions bi-directionally, where products
may turn into reactants if their concentration is great enough
reversible chemical reaction
114
solvent
substance capable of dissolving another substance
115
specific heat capacity
the amount of heat one gram of a substance must absorb or lose to change its temperature by one degree Celsius
116
the amount of heat one gram of a substance must absorb or lose to change its temperature by one degree Celsius
specific heat capacity
116
sphere of hydration
when a polar water molecule surrounds charged or polar molecules thus keeping them dissolved and in solution.
117
when a polar water molecule surrounds charged or polar molecules thus keeping them dissolved and in solution.
sphere of hydration
118
substance capable of dissolving another substance
solvent
119
structural isomers
molecules that share a chemical formula but differ in the placement of their chemical bonds
120
molecules that share a chemical formula but differ in the placement of their chemical bonds
structural isomers
121
substituted hydrocarbon
hydrocarbon chain or ring containing an atom of another element in place of one of the backbone carbons
122
hydrocarbon chain or ring containing an atom of another element in place of one of the backbone carbons
substituted hydrocarbon
123
tension at the surface of a body of liquid that prevents the molecules from separating; created by the attractive cohesive forces between the molecules of the liquid
surface tension
123
valence shell
outermost shell of an atom
123
surface tension
tension at the surface of a body of liquid that prevents the molecules from separating; created by the attractive cohesive forces between the molecules of the liquid
124
outermost shell of an atom
valence shell
125
van der Waals interaction
very weak interaction between molecules due to temporary charges
attracting atoms that are very close together
126
very weak interaction between molecules due to temporary charges
attracting atoms that are very close together
van der Waals interaction
