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

C1: Chemistry the Study of Change Flashcards

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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
Q

Homogeneous Mixture

A

Composition of the mixture is the same throughout (No physical separation)

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26
Q

Heterogeneous Mixture

A

Composition is not uniform throughout (Physical separation)

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27
Q

Hot Fudge Sundae and Peach Pie

A

Heterogeneous Mixtures

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28
Q

Baby Shampoo and Sugar Water

A

Homogeneous Mixture

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29
Q

Pasta and Tomato Sauce // Air

A

Mixture

30
Q

Aluminum Foil and Helium

A

Pure Subtance

31
Q

LAW OF CONSERVATION OF MATTER

A

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
Q

Physical Property

A

A characteristic of matter that is not associated with a change in its chemical composition.

33
Q

Examples of a Physical Property

A

Density, color, hardness, melting and boiling points, and electrical conductivity

34
Q

Chemical Property

A

The change of one type of matter into another type (or the inability to change)

35
Q

Examples of a Chemical Property

A

Flammability, toxicity, acidity, reactivity, and heat of combustion.

36
Q

Physical Change

A

Does not alter the composition or identity of a substance

37
Q

Example of a Physical Change

A

Ice Melting or Sugar Dissolving in Water

38
Q

Chemical Change

A

Alters the composition or identity of the substance(s) involved.

39
Q

Examples of a Chemical Change

A

Hydrogen burns in air to form water.

40
Q

Extensive Property

A

Material depends upon how much matter is being considered.

41
Q

Examples of an Extensive Property

A

Mass, Length, Volume

42
Q

Intensive Property

A

Material DOES NOT depend on how much matter is being considered,

43
Q

Examples of an Intensive Property

A

Density, Temperature, Color

44
Q

Measurements

A

Provide the info that is the basis of most of the hypotheses, theories, and laws in chemistry

45
Q

Measurements provide 3 kinds of info:

A
  1. A Number
  2. A Unit
  3. An indication of the uncertainty of the measurement.
46
Q

How long has the International System of Units (SI) been used for?

A

Since 1964`

47
Q

What is the SI unit for length?

A

Meter (m)

48
Q

What is the SI unit for mass?

A

kilogram (kg)

48
Q

What is the SI unit for mass?

A

kilogram (kg)

49
Q

What is the Si unit for time?

A

second (s)

50
Q

What is the Si unit for temperature?

A

kelvin (K)

51
Q

What is the SI unit for Electric Current?

A

ampere (A)

52
Q

What is the SI unit for the amount of substance?

A

mole (mol)

52
Q

What is the SI unit for the amount of substance?

A

mole (mol)

53
Q

What is the SI unit for luminous intensity?

A

candela (cd)

54
Q

x10^-15

A

femto (f)

55
Q

x10^-3

A

milli (m)

56
Q

x10^-2

A

centi (c)

56
Q

x10^-2

A

centi (c)

57
Q

x10^-1

A

deci (d)

58
Q

x10^3

A

kilo (k)

59
Q

Precise Measurements

A

They yield very similar results when repeated in the same manner.

60
Q

Accurate

A

Yields a result that is very close to the true or accepted value.

61
Q

Scientific Notation:

11000

A

1.1 x 10^4

62
Q

Scientific Notation:

0.00021

A

2.1 x 10^-4

63
Q

Scientific Notation:

0.001021

A

1.021 x 10^-3

64
Q

Scientific Notation:

1730

A

1.73 x 10^3

65
Q

Density

A

Compares the mass of an object to its volume.

66
Q

Density Equation

A

Mass of Substance / Volume of Substance

67
Q

Substances that have HIGHER densities contain particles that are…

A

Closely packed together

68
Q

Substances that have LOWER densities contain particles that are…

A

Farther apart.

CHEM 111 05B (1 decks)

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