Unit 1

Question 1

Chemistry

Answer 1

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

Question 2

Scientific Method

Answer 2

process of observation, inquiry, experimentation, and drawing conclusions

Question 3

hypothesis

Answer 3

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

Question 4

Scientific Method

Answer 4

Question 5

Chemistry

Answer 5

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

Question 6

Matter

Answer 6

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

Question 7

Natural chemical

Answer 7

Produced by nature

Question 8

Synthetic chemical

Answer 8

Created in lab

Question 9

Properties of Matter

Answer 9

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

Question 10

Scientific method

Answer 10

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

Question 11

Hypothesis is modified if

Answer 11

Modified if the results of the experiments do not support it

Question 12

Physical quantity

Answer 12

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

Question 13

Unit of Measurement and Abbreviations

Answer 13

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

Question 14

Derived units

Answer 14

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

Question 15

Mass

Answer 15

Measure of the amount of matter in object

Question 16

Weight

Answer 16

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

Question 17

Mass units

Answer 17

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

Question 18

Length units

Answer 18

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

Question 19

Volume units

Answer 19

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

Question 20

Cubic centimeter

Answer 20

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

Question 21

Prefixes and equalities

Answer 21

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)

Question 22

Physical quantities

Answer 22

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

Question 23

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

Answer 23

Question 24

Significant figures

Answer 24

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

Question 25

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.

Answer 25

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

Question 26

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

Answer 26

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

Question 27

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

Answer 27

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

Question 28

Significant figures

Answer 28

Question 29

Rounding off

Answer 29

Question 30

Rounding off: addition and subtraction

Answer 30

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

Question 31

Density

Answer 31

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

Question 32

Density

Answer 32

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.

Question 33

Specific gravity

Answer 33

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

Question 34

Common equalities

Answer 34

Question 35

Results

Answer 35

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

Question 36

All pure substances have

Answer 36

Density

Question 37

Length

Answer 37

Metric and SI meter (m)

Question 38

Volume

Answer 38

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

Question 39

Mass

Answer 39

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

Question 40

Temperature

Answer 40

Metric: Celsius SI: Kelvin (K)

Question 41

Time

Answer 41

Metric and SI Seconds

Question 42

Giga

Answer 42

G 10^9

Question 43

Mega

Answer 43

M 10^6

Question 44

Kilo

Answer 44

k 10^3

Question 45

Deci

Answer 45

d 10^-1

Question 46

Centi

Answer 46

c 10^-2

Question 47

Milli

Answer 47

m 10^-3

Question 48

Micro

Answer 48

Mew 10^-6

Question 49

Nano

Answer 49

n 10^-9

Question 50

Pico

Answer 50

p 10^-12

Question 51

Femto

Answer 51

f 10^-15

Question 52

Unit conversions

Answer 52

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