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CHEM121 > Chapter 1 Lecture > Flashcards

Chapter 1 Lecture Flashcards

1
Q

Study of matter—its composition, properties, and transformations.

A

Chemistry

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2
Q

Anything that has mass and takes up volume

A

Matter

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3
Q

Cotton, sand, digoxin: a cardiac drug

A

Naturally occurring matter

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4
Q

Nylon, Styrofoam, ibuprofen

A

Synthetic (human-made) matter

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5
Q

Has a definite volume, maintains its shape regardless of its container, and has particles that lie close together in a regular three-dimensional array.

A

Solid

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6
Q

Has definite volume, takes the shape of its container, and has particles that are close together, but they can randomly move around, sliding past one another.

A

Liquid

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7
Q

Usually refers to pure compounds or simple mixtures of pure compounds

A

Liquid

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8
Q

A complex liquid

A

Blood

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9
Q

Has no definite shape or volume, expands to fill the volume and assumes the shape of whatever container it is put in, and has particles that are very far apart and move around randomly.

A

Gas

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10
Q

Minimal Attractive Forces between atoms of molecules

A

Gas

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11
Q

Can be observed or measured without changing the composition of the material

A

Physical Properties

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12
Q

boiling point (bp), melting point (mp), solubility, color, odor

A

Physical properties

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13
Q

Alters the material without changing its composition

A

Physical change

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14
Q

Melting ice (solid water) to form liquid water or boiling liquid water to form steam (gaseous water).

A

Physical change example

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15
Q

Determine how a substance can be converted into another substance.

A

Chemical properties

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16
Q

Or chemical reaction, converts one substance into another.

A

Chemical change

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17
Q

A piece of paper burning, metabolizing an apple for energy, or oxygen and hydrogen combining to form water.

A

Chemical change examples

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18
Q

Is composed of a single component, has a constant composition, regardless of sample size and origin of sample, and cannot be broken down to other pure substances by a physical change. Table sugar (C12H22O11) and water (H2O) are both pure substances.

A

Pure substance

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19
Q

Is composed of more than one substance, can have varying composition (any combination of solid, liquid, and gas), depending on the sample, can be separated into its components by a physical change, sugar dissolved in water = mixture

A

Mixture

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20
Q

are complex

A

Mixtures

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21
Q

A pure substance that cannot be broken down by a chemical change.

A

Element

22
Q

A pure substance formed by chemically joining two or more elements.

A

Compound

23
Q

is composed of a number and a unit

A

Every measurement

24
Q

Proper aspirin dosage = 325 (what? milligrams or pounds?). A fast time for the 100-meter dash = 10.00 (seconds or days?).Numbers need units to acquire tangible meaning

A

Numbers need units to acquire tangible meaning

25
Q

Other units are related to the base unit by a power of 10. The prefix of the unit name indicates if the unit is larger or smaller than the base unit.The Metric System of Units – Decimal based

A

The Metric System of Units – Decimal based

26
Q

1,000 meters (m) = 1 kilometer (km)

A

1 m = 0.001 km

27
Q

1 meter (m) = 100 centimeters (cm)

A

0.01 m = 1 cm

28
Q

1 meter (m) = 1000 millimeters (mm)

A

0.001 m = 1 mm

29
Q

A measure of the amount of matter in an object.

A

Mass

30
Q

The force exerted on the object in a gravitational field. Depends on gravitational field.

A

Weight

31
Q

1,000 liters (L) = 1 kiloliter (kL)

A

1 L = 0.001 kL

32
Q

1 liters (L) = 1,000 milliliter (mL)

A

0.001 L = 1 L

33
Q

Volume = Length x Width x Height

A

= cm x cm x cm
= cm3

mL = 1 cm3 = 1 cc

34
Q

Results from counting objects or is part of a definition. 10 fingers, 10 toes
1 meter = 100 centimeters

A

Exact number

35
Q

Results from a measurement or observation and contains some uncertainty. 15.3 cm, 1000.8 g, 0.0034 mL

A

Inexact number

36
Q

All the digits in a measured number including one estimated digit.

A

Significant figures

37
Q

Are always significant

A

Nonzero digits

38
Q

A zero counts as a significant figure when it occurs

A

Rules to Determine When a Zero is a Significant Figure

39
Q

A zero counts as a significant figure when it occurs

A

between two nonzero digits, as in or at the end of a number with a decimal place.

40
Q

A zero does not count as a significant figure when it occurs

A

Rules to Determine When a Zerois a Significant Figure

41
Q

A zero does not count as a significant figure when it occurs

A

at the beginning of a number, at the end of a number that does not have a decimal.

42
Q

Changing the position of a decimal does not change the number of significant figures.

A

Significant figures

43
Q

The answer has the same number of significant figures

as the original number with the fewest significant figures.

A

Significant Figures Rules for Multiplication and Division

44
Q

If the first digit to be dropped is between 0 and 4, between 5 and 9.

A

Then, drop it and all remaining digits, round up the last digit to be retained by adding 1.

45
Q

Significant Figures Rules for Addition and Subtraction

A

The answer has the same number of decimal places as the original number with the fewest decimal places.

46
Q

A term that converts a quantity in one unit to a quantity in another unit. They are usually written as equalities, but to use them they must be written as fractions

A

Conversion factor

47
Q

Uses conversion factors to convert a quantity in one unit to a quantity in another unit. The units are treated like numbers and cancel any unwanted numbers.

A

Factor-label method

48
Q

Using Conversion Factors Solving a Problem Using Two or MoreConversion Factors

A

Always arrange the factors so that the denominator in

one term cancels the numerator in the preceding term.

49
Q

measure of how hot or cold an object is

A

Temperature

50
Q

degrees Fahrenheit (°F), degrees Celsius (°C), Kelvin (K)

A

Three temperature scales are used

51
Q

a physical property that relates the mass of a substance to its volume.

A

Density

CHEM121 (1 decks)

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