CHEM111 PRELIM REVIEWER Flashcards
(132 cards)
1
Q
field of study concerned with the characteristics, composition, and transformations of matter
A
chemistry
2
Q
Icludes all things, both living and nonliving.
A
matter
3
Q
2 types of property
A
physical , chemical
4
Q
characteristics that can be observed without changing the basic identity of the substance
A
physical property
5
Q
Color, odor, physical state, melting/boiling point, hardness
A
physical property
6
Q
describes the way the substance undergoes or resists change to form a new substance
A
chemical property
7
Q
changes its physical appearance but not is chemical composition
A
physical change
8
Q
substance undergoes a change in chemical composition. It always involve conversion of the material under consideration into one or more new substances.
A
chemical change
9
Q
composition of a substance does not change
A
physical
10
Q
properties observable without changing composition
A
physical properties
11
Q
changes observable without changing composition
A
physical change
12
Q
changes in color, shape , solid, liquid, gas, boiling point, melting point
A
physical properties
13
Q
melting, boiling, freezing
A
physical change
14
Q
changes in state of subdivision with no change in state
A
physical change
15
Q
properties that describe how a substance changes or resist change to form a new substance
A
chemical properties
16
Q
flammability
A
chemical properties
17
Q
decomposition, reaction to chlorine
A
chemical properties
18
Q
changes in which one or more new substance are formed
A
chemical change
19
Q
2 classes of matter
A
pure substance, mixtures
20
Q
2 sub of pure substances
A
elements and compounds
21
Q
2 types of mixtures
A
homo heterogenous
22
Q
2 chemical composition as a_______
A
pure substance, mixture
23
Q
CC single kind of matter that cannot be separated into other kinds of matter by any physical means
A
Pure Substance
24
Q
CC physical combination of two or more pure substances in which each substance retains its own chemical identity
A
Mixture
25
CC components can be separated using physical means
mixture
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mixture that contains visible different phases (parts), each of which has different property
hetero
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contains only one visibly distinct phase
homo
28
pure substance that cannot be broken down into simpler pure substances by chemical means
element
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pure substance that can broken down into two or more simpler pure substances by chemical means
compound
30
how many known elements in the PT
117
31
smallest particle of an element that can exist and still have the properties of the element
atom
32
rarely encountered in nature
free atoms
33
a group of two or more atoms that functions a unit because the atoms are tightly bound together
molecule
34
molecule that contains two atoms
diatomic molecule
35
`molecule that contains 3 atoms
triatomic molecule
36
molecule in which all atoms present are of the same kind.
e.g H2
homoatomic molecule
37
molecule in which two or more kinds of atoms are present.
H20
heteroatomic molecule
38
molecules made of atoms from different elements
compound
39
atoms connected by chemical bond
molecules
40
T/F
ALL COMPOUNDS ARE MOLECULES, BUT NOT ALL MOLECULES ARE COMPOUNDS
TRUE
41
notation made up of the chemical symbols of the elements present in a compound and numerical subscripts (located to the right of each chemical symbol) that indicate the number of atoms of each element present in a molecule of the compound.
CHEMICAL FORMULA
42
determination of the dimensions, capacity, quantity, or extent of something
MEASUREMENT
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two systems of measurement that is used commonly
the English system of units and the metric system of units
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inch, foot, pound, quart, and gallon
English
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gram, meter, and liter
Metric
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1 m is equivalent to ---yards
1.09 yards
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28 g =
1 ounce
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454 g=
1 pound
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1 L is equivalent to
1,06 quarts
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T/F
Measurements will always have a degree of uncertainty or error
T
51
in a measurement that are known with certainty plus one digit that is estimated
SIGNIFICANT FIGURES
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Number of significant figures = all certain digits + one estimated digit
YES
53
T/F
All nonzero digits are NOT significant
F
54
T/F
Zeros may or may not be significant
T
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Zeros at the beginning of a number are never significant
T
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Zeros between nonzero digits are always significant
T
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Zeros at the end of a number are SIGNIFICANT if a decimal point is PRESENT in the number
T
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Zeros at the end of a number are NOT SIGNIFICANT in the number LACKS an explicitly shown decimal point
T
59
0.0141
3
60
3.063
4
61
100
1
62
100.
3
63
0.001004
4
64
56.00
4
65
0.05050
4
66
6010
3
67
ratio that specifies how one unit of measurement is related to another unit of measurement
conversion factor
68
a general problem-solving method in which the units associated with numbers are used as a guide in setting up calculations
dimensional analysis
69
ratio of the mass of an object to the volume occupied by that object
density
70
density triangle
M/dv
71
indicator of the tendency of heat energy to be transferred
temp
72
All matter is made up of small particles called
atoms
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Atoms, in turn, are made up of even smaller particles
subatomic particle
74
Three types of subatomic particles
protons neutrons electrons
75
where does the p an n located
center
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the outer region contain
all electron
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any subatomic particle found in the nucleus of an atom
nucleon
78
An atom as a whole is electrically -----
neutral
79
the number of protons in the nucleus of an atom
atomic number
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number of protons =
number of electrons
81
The mass number is the number of
protons and the number of neutrons in the nucleus
82
number of protons + number of neutrons
mass number
83
An atom must have the same number of electrons and protons
yes
84
t/f
However, the number of neutrons do not have to be the same as the number of protons or electrons
t
85
atoms of an element that have the same number of protons and the same number of electrons but different numbers of neutrons
isotopes
86
the calculated average mass for the isotopes of an element, expressed on a scale where 126C serves as the reference point
atomic mass
87
states that when increasing atomic number, elements with similar chemical properties occur in periodic (regularly recurring) intervals
pt law
88
a tabular arrangement of the elements in order of increasing atomic number such that elements having similar chemical properties are positioned in vertical columns
pt
89
horizontal row of elements in the periodic table
period
90
vertical column of elements in the periodic table
group
91
Four Groups of elements have common (non-numerical) names
Alkali metal, Alkaline earth metal, Halogen and Noble Gas
92
an element that has the characteristic properties of luster, thermal conductivity, electrical conductivity, and malleability
metal
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an element characterized by the absence of properties of luster, thermal conductivity, electrical conductivity, and malleability
nonmetal
94
The majority of the elements are
metals
95
region of space about a nucleus that contains electrons that gave approximate the same energy and that spend most of their time approximately the same distance from the nucleus
electron shell
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region of space within an electron shell that contains electrons that have the same energy
electron subshell
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region of space within an electron subshell where an electron with a specific energy is most likely to be found
electron orbital
98
spherical in shape
s
99
have shaped similar to the “figure 8”
p
100
clover shape
d
101
pompoms
f
102
electron in the outermost electron shell of a representative or noble-gas element
valence electron
103
the chemical symbol of an element surrounded by dots equal in number to the number of valence electrons present in atoms of the element
The general practice in writing
lewis symbol
104
If an atom gains one or more electrons
it becomes a negatively charged ;
105
if an atom loses one or more electrons,
it becomes a positively charged
106
ionic bond model
+1,2,3 -1,23
107
Ionic compounds are always
NEUTRAL
108
Ionic bonds form between atoms of
dissimilar elements (metal + nonmetal).
109
Covalent bond occurs between
similar or even identical atoms (often two nonmetals are involved)
110
Ionic bond =
ELECTRON TRANSFER
111
Covalent bond =
Electron sharing
112
written statement that uses chemical symbols and chemical formulas instead of words to describe the changes that occur in a chemical reaction
chemical equation
113
written on the left side of equation,
Reactants
114
written on the right side of equation,
Product
115
a process in which at least one new substance is produced as a result of chemical change
chemical reaction
116
a reaction in which a single product is produced from two (or more) reactants
combination reaction
117
a chemical reaction in which a single reactant is converted into two (or more) simpler substances (elements or compounds
decomposition reaction
118
chemical reaction in which an atom or molecule replaces an atom or group of atoms from a compound
single-replacement
119
a chemical reaction in which two substance exchange parts with one another and form two different substances
double-replacement
120
a chemical reaction between a substance and oxygen (usually from air) that proceeds with the evolution of heat and light (usually from a flame)
combustion reaction
121
ounce to g
23 g
122
lb to g
454 g
123
l to quarts
1.06 quarts
124
inch to cm
2.54 cm
125
m to in
39.4 in
126
km to mile
o.621 mile
127
kg to lb
2.20 lb
128
oz to g
28.3 g
129
quart to liter
0.946 liter
130
liter to gallon
0.265
131
ml to fl oz
0.038
132
