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Chem 100 Class > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

Chemistry

A

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

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2
Q

Scientific Method

A

process of observation, inquiry, experimentation, and drawing conclusions

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3
Q

hypothesis

A

prediction of the expected outcome of the experiments designed to answer a given question

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4
Q

Scientific Method

A
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5
Q

Chemistry

A

study of composition, structure, properties, and reactions of matter

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6
Q

Matter

A

All substances that make up our world
Anything that has mass and occupies space
Can be pure substance or mixture

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7
Q

Natural chemical

A

Produced by nature

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8
Q

Synthetic chemical

A

Created in lab

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9
Q

Properties of Matter

A

characteristic useful for identifying a substance or object physical properties include:
– Size
– Color
– Temperature
Chemical properties include
-composition (what the natter is made of)
-reactivity (how the matter behaves)
-MP, BP

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10
Q

Scientific method

A
  1. Make observations about nature and ASK questions about what you OBSERVE
  2. Propose a hypothesis, which states a possible explanation of observations
  3. Several experiments may be done to test the hypothesis
  4. When the results of the experiments are analyzed, a conclusion is made as to whether the hypothesis may be true or false
  5. Observation
  6. Hypothesis
  7. Experiment
  8. Conclusion
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11
Q

Hypothesis is modified if

A

Modified if the results of the experiments do not support it

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12
Q

Physical quantity

A

Mass, volume, temperature, and density
Described by both a number and a unit
Physical quantity: a measurable physical quantity
Unit: a defined quantity used as a standard of measurement

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13
Q

Unit of Measurement and Abbreviations

A

1g = 1/1000 kg
1000 L = 1 m^3

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14
Q

Derived units

A

Represent the relationship between 2 measurable properties
Can’t be measured directly
Ex. Speed: meters per second (m/s) — length/ time
Density: grams per cubic centimeter (g/cm^3)—m/v

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15
Q

Mass

A

Measure of the amount of matter in object

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16
Q

Weight

A

Measure of the gravitational force that the earth or other large body exerts on an object

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17
Q

Mass units

A

1kg=1000g
1kg=2.20 lb
454g= 1lb
SI unit—kg used for larger masses
Metric unit—gram (g) used for smaller masses

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18
Q

Length units

A

1m = 100 cm
1m = 39.4 in
1m = 1.09 yd
2.54 cm = 1in
(Meter slightly longer than yard)

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19
Q

Volume units

A

SI unit: m^3
Metric unit: liter (slightly larger than a quart)
1 L =1000 mL
1 L =1.06 qt
946 mL = 1qt

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20
Q

Cubic centimeter

A

Volume of a cube whose dimensions are 1cm on each side
Cubic cm same volume as a milliliter, often used interchangeably
1cm^3 = 1cc = 1mL
1000 cm^3 = 1000 mL = 1 L

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21
Q

Prefixes and equalities

A

Can replace prefix with numerical value
Ex. Kilo = 1000 = 10^3
So
kilometer = 1000 meters (10^3 m)
Kiloliter = 1000 liters (10^3 L)
Kilogram = 1000 grams (10^3 g)

22
Q

Physical quantities

A

Unit sizes can be modified using prefixes to refer to smaller or larger quantities

23
Q

Prefixes for writing very large or very small numbers using scientific notation or units with appropriate numerical prefixes

A
24
Q

Significant figures

A

-all nonzero digits and zeros between digits
-zeros at the end of a decimal number
-zeros that act as placeholders before digits

25
Q

When one or more zeros in a large number are significant, place a decimal point after a significant zero at the end of a number.

A

300 m is = 3.0 × 102 m. (2 sig figs.)
300 m = 300. m or 3.00 × 102 m (3 sig figs)

26
Q

Zeros at the end of large standard numbers without a decimal point are not significant.

A

400,000 g = 4 × 105 g (1 sig fig)
850,000 m = 8.5 × 105 m (2 sig figs)

27
Q

Zeros at the beginning of a decimal number are used as placeholders and are not significant.

A

0.0004 s = 4 × 10−4 s. (1 sig fig)
0.0000046 g = 4.6 × 10−6 g. (2 sig figs)

28
Q

Significant figures

A
29
Q

Rounding off

A
30
Q

Rounding off: addition and subtraction

A

calcuations cannot have more digits after the decimal point than the original measured values.

31
Q

Density

A

m/v
Solids, liquids = g/cm^3 or g/mL
Gas = g/L
Note: 1mL =1 cm^3

32
Q

Density

A

For most pure substances, the solid phase is the most dense because most substances contract when cooled and expand when heated.
– Water behaves differently; it contracts when cooled from 100 °C to 3.98 °C, but below this temperature it begins to expand again.
– Ice is less dense than liquid water
-Less dense substances will float on top of a more dense fluid
-Any substance with a density > water will sink in water.

33
Q

Specific gravity

A

density of a substance divided by the density of water at the same temperature.
– At normal T, the density of water is very close to 1 g/mL.
– At normal T, the specific gravity of a substance is numerically equal to its density.
-can be measured using a hydrometer

34
Q

Common equalities

A
35
Q

Results

A

Results are experimental data that includes detailing all observations and measurable evidence.

36
Q

All pure substances have

A

Density

37
Q

Length

A

Metric and SI
meter (m)

38
Q

Volume

A

Metric: liter (L)
SI: cubic meter (m^3)

39
Q

Mass

A

Metric: gram (g)
SI: kilogram (kg)

40
Q

Temperature

A

Metric: Celsius
SI: Kelvin (K)

41
Q

Time

A

Metric and SI
Seconds

42
Q

Giga

A

G
10^9

43
Q

Mega

A

M
10^6

44
Q

Kilo

A

k
10^3

45
Q

Deci

A

d
10^-1

46
Q

Centi

A

c
10^-2

47
Q

Milli

A

m
10^-3

48
Q

Micro

A

Mew
10^-6

49
Q

Nano

A

n
10^-9

50
Q

Pico

A

p
10^-12

51
Q

Femto

A

f
10^-15

52
Q

Unit conversions

A

1mL = 1cm^3
If it’s water 1mL = 1 gram

Chem 100 Class (9 decks)

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