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final Flashcards

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1
Q

Mass

A

All the substances that make up our world

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2
Q

Organic Chemistry

A

The study of substances that contain the element carbon.

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3
Q

Inorganic Chemistry

A

The study of all other substances except those that contain carbon.

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4
Q

General Chemistry

A

The study of the composition, properties, and reactions of matter.

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5
Q

Geochemistry

A

The study of the chemical composition or ores, soils, and minerals of the surface of earth and other planets.

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6
Q

Biochemistry

A

The study of the chemical reactions that take place in biological systems.

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7
Q

Physical Chemistry

A

The study of the physical nature of chemical systems including energy changes.

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8
Q

Chemical

A

A substance that always has the same composition and properties wherever it is found.

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9
Q

Every day you use products containing substances that were prepared by chemists.

A

Yep!

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10
Q

Sunlight

A

Energy given off by the sun. Thus, sunlight does not contain matter, which means it is not a chemical.

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11
Q

Metric system

A

System of measurement that scientists and health professionals throughout the world use.

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12
Q

International system of units (SI)

A

Modification of the metric system, which is now the official system of measurement throughout the world except for the U.S.

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13
Q

Units of measurement (metric)

A 
Length: meter (m)
Volume: liter (L)
Mass: gram (g)
Temp: degree Celsius (C)
Time: seconds (s)
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14
Q

Units of measurement (SI)

A 
Length: meter (m)
Volume: cubic meter (m^3)
Mass: kilogram (kg)
Temp: kelvin (K)
Time: seconds (s)
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15
Q

Length

A

1m = 100 cm.
1m = 39.4 in.
1m = 1.09 yd.
2.54 cm = 1 in.

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16
Q

Volume

A

The amount of space a substance occupies.
1 L = 1000 mL
1 L = 1.06 qt.
946 mL = 1 qt.

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17
Q

Mass

A

A measure of the quantity of material it contains.
1 kg = 1000 g
1 kg = 2.20 lb.
454 g = 1 lb.

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18
Q

kilo-

A

1 thousand

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19
Q

centi-

A

1 hundredth

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20
Q

mili-

A

1 thousandth

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21
Q

Measured numbers

A

The numbers you obtain when you measure a quantity such as your height, weight, or temperature.

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22
Q

Significant figures

A

In a measured number, all the digits including the estimated digit.

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23
Q

A number is a significant figure if it is…

A
  • Not a zero
  • A zero between nonzero digits
  • A zero at the end of a decimal number
  • In the coefficient of a number written in scientific notation.
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24
Q

A zero is not significant if it is…

A
  • At the beginning of a decimal number

- Used as a placeholder in a large number without a decimal point

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25
Q

Exact numbers

A

Numbers obtained by counting items or using a definition that compares 2 units in the same measuring system.

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26
Q

Significant figures in multiplication or division

A

The final answer is written so it has the same number of significant figures as the measurement with the FEWEST SIGNIFICANT FIGURES.

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27
Q

Significant figures in addition or subtraction

A

The final answer is written so it has the same number of decimal places as the measurement with the FEWEST DECIMAL PLACES.

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28
Q

micro-

A

one millionth

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29
Q

Cubic centimeter

A

The volume of a cube whose dimensions are 1 cm on each side.

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30
Q

1 cm^3 = 1 cc = 1 mL

A

that’s it

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31
Q

Conversion factor

A

one of the quantities is the numerator, and the other is the denominator.

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32
Q

Ex. of a conversion factor: 1 hr = 60 min

A

60min/1hr and 1hr/60min

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33
Q

When is it exact vs significant figures

A

English to English = exact
Metric to Metric = exact
English to Metric= significant figures
Metric to English= significant figures

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34
Q

Density

A

Comparing the mass of the object to its volume.

  • D=M/V
  • Sink = more dense
  • Float = less dense
35
Q

Guide to calculating density

A
  1. State the given and needed quantities
  2. Write the density expression
  3. Express the mass in grams and the volume in mL
  4. Substitute mass & volume into the density expression and calculate the density.
36
Q

Matter

A

Anything that has mass and occupies space.

37
Q

Pure Substance

A

Matter that has a fixed or definite composition. 2 kinds: element or compound.

38
Q

Element

A

The simplest type of a pure substance, is composed of only one type of material such as silver, or iron.

39
Q

Compound

A

Also a pure substance, but it consists of atoms of 2 or more elements always chemically combined in the same proportion.

40
Q

Mixture

A

2 or more substances are physically mixed, but not chemically combined.

41
Q

Homogeneous mixture (solution)

A

The composition is uniform throughout the sample.

-ex: air, sea water

42
Q

Heterogeneous mixture

A

The components do not have a uniform composition throughout the sample.
-Ex: oil in water, raisins in a cookie.

43
Q

States of matter

A

1 of 3 physical forms (solid, liquid, or gas),

44
Q

Solid

A

Has a definite shape and volume.

45
Q

Liquid

A

Has a definite volume, but not a definite shape.

46
Q

Gas

A

Does not have a definite shape or volume.

47
Q

Physical properties

A

Those that can be observed or measured without affecting the identity of a substance.

48
Q

Physical change

A

When matter undergoes change, its state or its appearance will change, but its composition remains the same.

49
Q

Chemical properties

A

Those that describe the ability of a substance to change into a new substance.

50
Q

Chemical change

A

The original substance is converted into one or more new substances, which have different chemical and physical properties.

51
Q

Energy

A

The ability to do work.

52
Q

Kinetic energy

A

Energy of motion. An object that is moving has kinetic energy.

53
Q

Potential energy

A

Determined by the position of an object or by the chemical composition of a substance.

54
Q

Heat (Thermal energy)

A

Associated with the motion of particles.

55
Q

Joule (J)

A

The SI unit of energy and work.

56
Q

Calorie (cal)

A

the amount of energy (heat) needed to raise the temperature of 1 g of water by 1 C.

57
Q

Kelvin scale

A

This temp, called absolute zero, has the value of 0 K. 1K = 1 C.

58
Q

Celsius to Kelvin

A

Add 273

59
Q

Heat flows from hot to cold.

A

Yep!

60
Q

Specific Heat (SH)

A

The amount of heat needed to raise the temperature of exactly 1 g of a substance by exactly 1 degree C.

61
Q

Specific heat calculation

A

SH= J (or cal) / 1 g x 1 C

62
Q

Lower heat

A

Heats up faster, and cools quickly

63
Q

Heat calculation

A

Heat = mass x temp change x SH

64
Q

Guide to calculations using specific heat

A
  1. List given and needed data
  2. Calculate the temp change
  3. Write the heat equation and rearrange for unknown
  4. Substitute the given values and solve, making sure units cancel
65
Q

Energy (caloric) values

A

Of food are the kilocalories or kilojoules obtained from burning 1 g of carbohydrate, fat, or protein.

66
Q

Typical energy (caloric) values for the 3 food types

A

FOOD TYPE kJ/g kcal/g
carbohydrates 17 4
Fat 38 9
protein 17 4

67
Q

Change of state

A

Matter is converted from one state to another.

68
Q

Melting point (mp)

A

The particles of a solid gain sufficient energy to overcome the attractive forces that hold them together.

69
Q

Evaporation

A

water molecules with sufficient energy escape from the liquid surface and enter the gas phase.

70
Q

Deposition

A

Gas changes directly to a solid

71
Q

Boiling

A

Gas bubbles from throughout the liquid, then rises to the surface and escapes.

72
Q

Melting

A

Changing from a solid to a liquid.

73
Q

Sublimation

A

The particles on the surface of a solid change directly to a gas without going through the liquid state.

74
Q

Endothermic

A

Heat absorbed, reactant side

75
Q

Exothermic

A

Heat released, product side

76
Q

Solution

A

A homogeneous in which one substance is uniformly dispensed in another substance.

77
Q

Solute

A

The substance present in lesser amounts.

78
Q

Solvent

A

The substance present in greater amounts.

79
Q

Strong electrolyte pg. 251

A

There is 100% dissociation of the solute into ions.

80
Q

Weak electrolyte

A

A compound that dissolves in water mostly as molecules.

81
Q

Unsaturated solution

A

A solution that contains less solute than can be dissolved.

82
Q

Saturated solution

A

A solution containing the maximum amount of solute that can dissolve at a given temp. Any additional solute will remain in the container.

83
Q

Osmosis

A

Water molecules move through a semipermeable membrane from the solution with lower concentration of solute into a solution with higher solute concentration.

Chemistry (2 decks)

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