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Chemistry 1 > Chapter 1 Review > Flashcards

Chapter 1 Review Flashcards

1
Q

Chemistry is the study of

A

the composition, properties, and interactions of matter.

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2
Q

What are the steps in the scientific method?

A

1) Observation and curiosity
2) Form hypothesis; make prediction
3) Perform experiment; make more observations
4) Contributes to body of knowledge.
5) Observation becomes law OR hypothesis becomes theory

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3
Q

The macroscopic domain of chemistry

A

Is familiar to us. It’s the realm of everyday things that are large enough to be sensed directly by human sight or touch.

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4
Q

The microscopic domain of chemistry

A

is often visited in the imagination. Some aspects of the microscopic domain are visible through standard optical microscopes.

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5
Q

The symbolic domain of chemistry

A

Contains the specialized language used to represent components of both the macroscopic and microscopic domains.

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6
Q

Matter is defined as:

A

anything that occupies space and has mass, and it’s all around us.

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7
Q

A solid is

A

rigid and possesses a definite shape.

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8
Q

A liquid

A

flows and takes the shape of its container, except that it forms a flat or slightly curved upper surface when acted upon by gravity.

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9
Q

What shape does liquid take in zero gravity?

A

A spherical shape

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10
Q

Gas

A

takes both the shape and volume of its container

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11
Q

A plasma is

A

a gaseous state of matter that contains appreciable numbers of electrically charged particles

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12
Q

Where can plasma be found?

A

in stars, lightning strikes, TV screens, etc.

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13
Q

The mass of an object is

A

a measure of the amount of matter in it

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14
Q

Weight refers to

A

the force that gravity exerts on an object

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15
Q

The ___ of an object changes as the force of gravity changes, but its ____ does not.

A

weight, mass

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16
Q

What does the Law of Conservation of Matter state?

A

It states that there is no detectable change in the total quantity of matter present when matter converts from one type to another or changes among solid, liquid, or gaseous states.

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17
Q

What is a pure substance?

A

A pure substance has a constant composition.

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18
Q

A pure substance has a _____ _____.

A

constant composition

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19
Q

What do all specimens of a pure substance have?

A

All specimens of a pure substance have exactly the same makeup and properties.

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20
Q

What are the two classes of pure substances?

A

Elements and compounds.

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21
Q

What are elements?

A

Pure substances that cannot be broken down into simpler substances by chemical changes.

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22
Q

What are compounds?

A

Pure substances that are comprised of two or more elements.

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23
Q

Why and how are compounds broken down?

A

Compounds may be broken down by chemical changes to yield either elements or other compounds, or both.

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24
Q

What is a mixture?

A

A mixture is composed of two or more types of matter that can be present in varying amount and can be separated by physical changes, such as evaporation.

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25
What is a heterogenous mixture?
A mixture with a composition that varies from point to point.
26
What is a homogeneous mixture (also called a solution)?
A homogenous mixture exhibits a uniform composition and appears visually the same throughout.
27
What type of mixture is a chocolate chip cookie?
A heterogeneous mixture
28
What type of mixture is black coffee?
A homogenous mixture
29
What is an atom?
The smallest particle of an element that has the properties of that element and can enter into a chemical combination
30
What is a molecule?
A molecule consists of two or more atoms joined by strong forces called chemical bonds
31
How many atoms are in a molecule?
Two or more
32
What strong forces help join atoms to form a molecule?
chemical bonds
33
How do the atoms in a molecule move around?
The atoms in a molecule move around as a unit
34
The characteristics that distinguish one substance from another are called ____.
Properties
35
Properties
The characteristics that distinguish one substance from another.
36
A physical property is
a characteristic of matter that is not associated with a change in its chemical composition.
37
What are some examples of physical properties?
Color, density, hardness, melting and boiling points, and electrical conductivity
38
A physical change is
is the state of properties of matter without any accompanying change in the chemical identities of substances contained in the matter.
39
What are some examples of a physical change?
Wax melting, when sugar dissolves in coffee, when steam condenses into liquid water
40
A chemical property is
the ability to change from one type of matter into another
41
What is an example of a chemical property?
The formation of rust
42
What two categories do properties of matter fall into?
extensive property and intensive property
43
If the property depends on the amount of matter present, it is an ____ _____.
extensive property
44
What are some examples of extensive properties?
The mass and volume of a substance
45
If the property of a sample of matter does not depend on the amount of matter present, it is an ____ ____.
intensive property
46
What is an example of an intensive property?
Temperature
47
What three classes do intensive and extensive properties use to sort elements into?
metals, nonmetals, and metalloids
48
metals
elements that conduct well
49
nonmetals
elements that conduct poorly
50
metalloids
elements that have intermediate conductivities
51
What are the three kinds of information that every measurement provides?
The size of magnitude of the measurement (a number), a standard of comparison for the measurement (a unit), and an indication of the uncertainty of the measurement.
52
Units
standards of comparison for measurements
53
What is the standard unit of length in both the SI and original metric systems?
meter (m)
54
What is the standard unit of mass in the SI system?
kilogram (kg)
55
How many pounds are equal to 1 kg?
2.2 lbs
56
How many kilograms is 1g?
0.001 kg
57
What is the SI unit of temperature?
Kelvin (K)
58
What is the SI base unit of time?
second (s)
59
What is volume?
The measure of the amount of space occupied by an object.
60
What is the standard unit for volume?
a cubic meter (m^3)
61
What is the more common name for the cubic decimeter?
A liter (l)
62
A cubic centimeter (cm^3) is
the volume of a cube with an edge length of exactly one centimeter
63
1 cm^3 is equivalent to
a milliliter (mL) and is 1/1000 of a liter
64
What is density?
The density of a substance is the ratio of the mass of a sample of the substance to its volume.
65
Density =
mass/volume
66
Every measurement has some ____, which depends on the device used.
uncertainty
67
What are significant figures?
All the digits in a measurement, including the uncertain last digit
68
precise
Measurements are said to be precise if they yield very similar results when repeated in the same manner.
69
accurate
A measurement is considered accurate if it yields a result that is very close to the true or accepted value
70
speed =
distance/time
71
time =
distance/speed
72
Dimensional analysis is based on this premise:
the units of quantities must be subjected to the same mathematical operations as their associated numbers.
73
A ratio of two equivalent quantities expressed with different measurement units can be used as a _______.
unit conversion factor
74
What refers to the hotness or coldness of a substance?
temperature
75
Exact numbers include
definitions (one dozen, 100 cm = 1 m) counted items (# of students in a classroom) Integers within formulas (the 2 in d=2r)
76
What is the only type of measurement free from uncertainty?
Counting
77
What is the size or magnitude of a measurement called?
A number
78
area =
length*width
79
volume =
length*width*height
80
What information do measurements provide?
Measurements provide the information that is the basis of most of the hypotheses, theories, and laws in chemistry.

Chemistry 1 (7 decks)

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