final Flashcards
(141 cards)
1
Q
matter
A
anything that has mass and occupies space
2
Q
chemistry
A
the study of the composition of matter and the changes that matter undergoes.
3
Q
what is chemistry also known as?
A
the central science
4
Q
What are the 5 traditional areas of chemistry?
A
organic, inorganic, biochemistry, analytical, and physical.
5
Q
What is organic chemistry?
A
the study of all chemicals containing carbon
6
Q
What is inorganic chemistry?
A
study of chemicals in general
7
Q
What is biochemistry?
A
the study of the processes that take place in living organisms.
8
Q
What is analytical chemistry?
A
the area of study that focuses on the composition of matter.
9
Q
What is physical chemistry?
A
the area that deals with the mechanism, rate, and energy transfer that occurs when matter undergoes a change.
10
Q
pure chemistry
A
is the pursuit of chemical knowledge for its own sake
11
Q
applied chemistry
A
research that is directed toward a practical goal or application.
12
Q
What are chemistry big main ideas?
A
chemistry as a central science electrons and structure of atoms bonding and interactions reactions kinetic theory the mole and quantifying matter matter and energy carbon chemistry
13
Q
what are elements composed of?
A
particles called atoms
14
Q
what are chemical compounds?
A
collections of two or more elements held together by relatively strong attractive forces.
15
Q
What can chemistry be useful in doing?
A
explaining the natural world, preparing people for career opportunities, and producing informed citizens.
16
Q
technology
A
is the means by which a society provided its members with those things needed and desired.
17
Q
What can modern research lead to?
A
technologies that aim to benefit the environment, conserve and produce energy, improve human life, and expand our knowledge of the universe.
18
Q
what does the word chemistry come from?
A
the word alchemy
19
Q
what was the alchemists’ goal in their study?
A
searching how to turn metals into gold.
20
Q
what did Lavoisier do?
A
helped to transform chemistry from a science of observation to the science of measurement.
21
Q
scientific methodology
A
is a general style of investigation with a logical systematic approach to the solution of a scientific problem. involves making observations, proposing and testing hypotheses, and developing theories.
22
Q
hypothesis
A
is a proposed explanation for an observation.
23
Q
experiment
A
a procedure that is used to test a hypothesis
24
Q
independent variable
A
the variable that you change during an experiment
25
dependent variable
the variable that is observed during the experiment
26
theory
a well-tested explanation for a broad set of observations.
27
scientific law
a concise statement that summarizes the results of many observations and experiments.
28
gas increases with a change in what
temperature.
29
what are the steps for solving a numeric word problem:
analyze, calculate, evaluate.
30
what are the steps to solve a non-numeric word problem?
analyze and solve.
31
mass
is a measure of the amount of matter the object contains.
32
volume
is a measure of the space occupied by the object.
33
extensive property
a property the depends on the amount of matter in a sample
34
intensive property
is a property that depends on the type of matter in a sample, not the amount of matter
35
substance
matter that has uniform and definite composition
36
what does every sample of a given substance have?
identical intensive properties because every sample has the same composition
37
malleable
means they can be hammered into sheets
38
physical property
is a quality or condition of a substance that can be observed or measured without changing the substances composition.
39
what are the three states of matter
liquid, gas, solid
40
solid
a form of matter that has a definite shape and volume.
expand when heated
orderly arrangement
incompressible
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liquid
```
a form of matter of a liquid is fixed or constant
not rigid or orderly
shape of container
foxed or constant
expend slightly when heated
incompressible
```
42
gas
a form of matter that take both the shape and volume of its container.
shape of container
gas can expand to fill any volume
easily compressed
43
what is the term gas used for
substance, like oxygen, that exist in the gaseous state at room temp.
44
vapor
describes the gaseous state of a substance that is generally a liquid or solid at room temp
45
physical change
some properties of a material change, but the composition of the material does not change.
46
how can physical changes be classified
reversible or irreversible
47
mixture
a physical blend of two or more components
48
how can mixtures be classified
heterogenous or homogenous
49
heterogenous
a mixture in which the composition is not uniform throughout
50
homogenous mixture
a mixture in which the composition is uniform thoughout
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solution
another name for a homogenous mixture
52
phase
descibe any part of a sample with uniform composition and properties
53
how many phases does a homogenous mixture consist of?
single phase
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how many phases does a hetrogenous mixture consist of?
two or more phases.
55
what can be used to seperate mixtures
differences in physical properties
56
filtration
the process that seperates a solid from the liquid in a heterogenous mixture.
57
distillation
liquid is boiled to produce a vapor that is then condensed into a liquid.
58
element
is the simpliest form of matter that has a unique set of properties
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compound
a substance that contains two or more elements chemically combined in a fixed proportion.
60
chemical change
a change that produces matter with different composition than the original matter.
61
What is one of the way to break down compounds into simpler substances
heating
62
what element cannot be broken down into simpler substances
carbon.
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in general the properties of compounds are quite different from those of their component elements.
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64
physical methods that are used to sperate mixtures be used to break a compound into simpler substances
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65
if the composition of a material is fixed, the material is a substance. if the composition of a material may vary, the material is a mixture
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66
what do chemists use to represent elements? compounds?
chemical symbols
| chemical formulas
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chemical symbol
each element is represented by a one or two letter symbol
68
because a compound has a fixed composition, the formula for a compound is always the same.
.......
69
periodic table
an arrangement of elements in which the elements are separated into groups based on a set of repeating properties.
70
What does the periodic table allow you to compare
the properties of one element to another element
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period
each horizontial row of the period table. 7
72
group
each vertical column of the periodic table or family. elements within a group have similar chemical and physical properties.
73
chemical property
the ability of a substance to undergo a specific chemical change.
74
what can be used to identify a substance
chemical properties.
75
during a chemical change, the compostion of matter always changes.
.......
76
what is a chemical change also called
chemical reaction
77
chemical reaction
one or more substaces change into one or more new substances
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reactant
a substance present at the start of the reaction
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product
a substance produced in the reaction
80
possible clues to chemical change include a transfer of energy, a change in color, the production of gas, or the formation of a precipate.
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81
what does every chemical change involve?
a transfer of energy
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precipate
a solid that forms and settles out of a liquid mixture.
83
energy is always transfers when matter changes from one state to another.
...
84
during any chemical reaction, the mass of the products is always equal to the mass of the reactants.
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85
law of conservation of mass
states that in any physical change or chemical reaction, mass is conserved. mass never created or destroyed.
86
measurement
a quantity that has both mumber and unit
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scientific notation
a given number is written as the product of two numbers. a coefficient and 10 raised to a power.
88
in scientific notation, the coefficent is always a number greater than or equal to one and less than ten. the exponent is an integer.
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89
when writing numbers greater than ten in scientific notation, the exponent is positive and equals the number of places that the original decimal point has been moved to the left.
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90
numbers less than one have a negative exponent when written in scientific notation. the value of the exponent equals the number of places the decimal has been moved to the right.
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91
multiplying numbers in scientific notation
multiply coefficents and add exponents.
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accuracy
a measure of how close a measurement comes to the actual or true value of whatever is measured
93
precision
a measure of how close a series of measurements are to one another, irrespective of the actual value.
94
to evaulte the accuracy of the measurement, the measured value just be compared to the correct value. the evaulte the precision of the measurement, you must compare the values of two or more repeated measurements.
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95
accepted value
the correct value for the measurement based on reliable references.
96
experimental value
the value measured in the lab
97
error
difference between the experimental value and the accepted value
98
error can be positive or negetive depending on whether the experiment value is greater
.........
99
percent error
measurement is the absolute value of the error divided by the accepted value, multiplied by 100%.
100
significant figures
a measurement includes all of the digits that are known, plus the last digit that is estimated.
101
measurements must always be reported to the correct number of significant figures because calculated answers often depend on the number of significant figures in the values used in the calculation.
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102
what are the rules for determining significant figures.
1. every nonzero digit
2. zero appearing between nonzero digits.
3. leftmost zeros appearing in front of nonzero digits.
4. zeros at end of the number and to the right of the decimal point.
5. zeros at rightmost end of measurement that lie to left of the decimal point.
6. there are two situations in which numbers have an unlimited number of sig figs. defined quantities and counted numbers.
103
the position of the decimal point is not sig with the rounding of numbers when multiplying and dividing. it is important when rounding addition or subtraction.
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104
the international system of units.
a revised version of the metric system.
105
meter
the basic unit of length, or linear measure
106
volume
the space occupied by any sample of matter
107
how do you calculate the volume
the multiplying length by width and height.
108
liter
the volume of a cube that is 10 centimeters along each edge.
109
kilogram
the mass of an object is measured in comparison to a standard mass, which is the basic SI unit of mass.
110
weight
is a force that measures the pull on a given mass by gravity.
111
energy
the capacity to o work or to produce heat
112
joule
the SI unit of energy
113
calorie
the quantity of heat that raised the temperature of 1 g of pure water by 1 C.
114
temperature
a measure of how hot or cold an object is.
115
What does the temperature of an object determine?
the direction of heat transfer.
116
when two objects at different temperatures are in contact, heat moves from the object at the higher temp to the object at the lower temp.
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117
scientists commonly use two equivalent units of temp, the degree Celsius and the kelvin.
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118
Celsius scale
the freezing point of water at 0 C and the boiling point of water at 100 C.
119
kelvin scale
the freezing point of water is 273.15 kelvons and the boiling point Is 373.15 K.
120
absolute zero
equal to -273.15 C
121
density
the ratio of the mass of an object to its volume
122
density is an intensive property that depends only on the composition of a substance, not on the size of the sample.
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123
what does a gas filled balloon depend on
the density of the gas compares with the density of air.
124
the volume of most substances increases as the temperature increases.
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125
the mass remains the same despite the temperature and volume changes.
.......
126
the density decreases with what
increase in temperature.
127
what is needed for the volume of water to increase
temperature decreases
128
conversion factors
a ratio of equivalent measurements.
129
whenever two measurements are equivalent, a ratio of the two measurements will equal 1
.....
130
when a measurement is multiplied by a conversion factor, the numerical value is generally changed, but the actual size of the quantity measured remains the same.
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131
what conversion do you use to convert between Kelvin and celsius
C=K-273
132
dimensional analysis
way to analyze and solve problems using the units, dimensions, of the measurements.
133
dimensional analysis is a powerful tool for solving conversion problems in which a measurement with one unit is changed to an equivalent measurement with another unit.
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134
what is all matter composed of?
particles, called atoms
135
atom
the smallest particle of an element that retains its identity in a chemical reaction.
136
how did democritus see atoms
as indivisible and indestructible
137
what is daltons atomic theory?
all elements are composed of tiny particles called atoms
atoms of the same element are identical
atoms of different elements can physically mix together or chemically combine in simple whole number ratios to form compounds.
chemical reactions occur when atoms are separated from each other, joined, or rearranged in a different combination
138
what are three kinds of subatomic particles
electron, neutrons, and protons.
139
electrons
negatively charged subatomic particles.
140
protons
positively charged subatomic particles
141
neutrons
subatomic particles with no charge but with a mass nearly equal to that of a proton.
