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CHEM 111 05B > C1: Chemistry the Study of Change > Flashcards

C1: Chemistry the Study of Change Flashcards

1
Q

Chemistry

A

The study of matter and the changes it undergoes.

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2
Q

Matter

A

Anything that occupies space and has mass.

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3
Q

Substance

A

A form of matter that has definite composition and distinct properties.

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4
Q

Macroscopic

A

Physically Seen

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5
Q

Microscopic

A

Not physically seen

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6
Q

Scientific Method

A

A systematic approach to research. 3 Steps: Observation, Representation, and Interpretation

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7
Q

Hypothesis

A

Tentative explanation for a set of observations.

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8
Q

Observations

A

Facts obtained by observing and measuring events in nature.

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9
Q

A Scientific Method Hypothesis

A

A statement that explains the observations. This can be modified if the results of the experiments do not support it.

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10
Q

Experiments

A

Procedures that test the hypothesis

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11
Q

Theory

A

A model that describes how observations occur using experimental results. Also, a unifying principle that explains a body of facts and/or laws that are based on them.

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12
Q

Law

A

A concise statement of a relationship between phenomena that is always the same under the same conditions.

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13
Q

Mass

A

The measure of the quantity of matter

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14
Q

SI unit of mass

A

Kilogram (kg)

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15
Q

Weight

A

Force that gravity exerts on an object. (Can change from location to location) High altitude locations will have lower weight for the same mass.

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16
Q

Solid

A

Definite Shape and Volume (Compact)

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17
Q

Liquid

A

Definite volume but no definite shape. (Less Compact)

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18
Q

Gas

A

No definite shape or volume. (Least Compact)

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19
Q

Plasma

A

A gaseous state of matter that contains an appreciable amount of electrically charged particles.

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20
Q

Where is plasma found?

A

High Temp. Environments
Naturally: Stars and Lightening
Man-Made: TV Screens

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21
Q

Element

A

A substance that CANNOT be separated into simpler substances by chemical means.

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22
Q

Compound

A

A substance composed of atoms of 2 or more elements chemically united in fixed proportions. (CAN be separated by chemical means).

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23
Q

Diatomic Molecules in Their Natural State

A

Hydrogen (H2), Oxygen (O2), Nitrogen (N2), and all elements in Group 17.

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24
Q

Mixture

A

A combination of two or more substances in which the substances retain their distinct identites.

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25
Homogeneous Mixture
Composition of the mixture is the same throughout (No physical separation)
26
Heterogeneous Mixture
Composition is not uniform throughout (Physical separation)
27
Hot Fudge Sundae and Peach Pie
Heterogeneous Mixtures
28
Baby Shampoo and Sugar Water
Homogeneous Mixture
29
Pasta and Tomato Sauce // Air
Mixture
30
Aluminum Foil and Helium
Pure Subtance
31
LAW OF CONSERVATION OF MATTER
There is no detectable change in the total quantity of matter present when matter converts from one type to another. (CANNOT CREATE OR DESTROY MATTER)
32
Physical Property
A characteristic of matter that is not associated with a change in its chemical composition.
33
Examples of a Physical Property
Density, color, hardness, melting and boiling points, and electrical conductivity
34
Chemical Property
The change of one type of matter into another type (or the inability to change)
35
Examples of a Chemical Property
Flammability, toxicity, acidity, reactivity, and heat of combustion.
36
Physical Change
Does not alter the composition or identity of a substance
37
Example of a Physical Change
Ice Melting or Sugar Dissolving in Water
38
Chemical Change
Alters the composition or identity of the substance(s) involved.
39
Examples of a Chemical Change
Hydrogen burns in air to form water.
40
Extensive Property
Material depends upon how much matter is being considered.
41
Examples of an Extensive Property
Mass, Length, Volume
42
Intensive Property
Material DOES NOT depend on how much matter is being considered,
43
Examples of an Intensive Property
Density, Temperature, Color
44
Measurements
Provide the info that is the basis of most of the hypotheses, theories, and laws in chemistry
45
Measurements provide 3 kinds of info:
1. A Number 2. A Unit 3. An indication of the uncertainty of the measurement.
46
How long has the International System of Units (SI) been used for?
Since 1964`
47
What is the SI unit for length?
Meter (m)
48
What is the SI unit for mass?
kilogram (kg)
48
What is the SI unit for mass?
kilogram (kg)
49
What is the Si unit for time?
second (s)
50
What is the Si unit for temperature?
kelvin (K)
51
What is the SI unit for Electric Current?
ampere (A)
52
What is the SI unit for the amount of substance?
mole (mol)
52
What is the SI unit for the amount of substance?
mole (mol)
53
What is the SI unit for luminous intensity?
candela (cd)
54
x10^-15
femto (f)
55
x10^-3
milli (m)
56
x10^-2
centi (c)
56
x10^-2
centi (c)
57
x10^-1
deci (d)
58
x10^3
kilo (k)
59
Precise Measurements
They yield very similar results when repeated in the same manner.
60
Accurate
Yields a result that is very close to the true or accepted value.
61
Scientific Notation: | 11000
1.1 x 10^4
62
Scientific Notation: | 0.00021
2.1 x 10^-4
63
Scientific Notation: | 0.001021
1.021 x 10^-3
64
Scientific Notation: | 1730
1.73 x 10^3
65
Density
Compares the mass of an object to its volume.
66
Density Equation
Mass of Substance / Volume of Substance
67
Substances that have HIGHER densities contain particles that are...
Closely packed together
68
Substances that have LOWER densities contain particles that are...
Farther apart.

CHEM 111 05B (1 decks)

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