Chemistry Ch 1

Front 1

What provides information that is used to discard, revise or accept a hypothesis?

Back 1

Experiments in the scientific method

Front 2

The branch of science involved with the study of matter and change?

Back 2

Chemistry

Front 3

What are laws?

Back 3

Statements used to describe things that are consistently observed

Front 4

What are laws used for?

Back 4

They preduct what may occur in the future?

Front 5

What do laws not do?

Back 5

Give explanations to why

Front 6

What are the steps of the scientific method?

Back 6

Observe, form a hypothesis, experiments, either accept, revise, or discard the hypothesis and if accepted then form a theory

Front 7

What is a hypothesis?

Back 7

Tenative explanation aka an educated guess

Front 8

What do experiments do?

Back 8

Tests hypothesis'

Front 9

What is a theory?

Back 9

Experimentally tested explanations of an observed behavior, it must be consistent and predict accurate results/ predict future observations

Front 10

Matter is defined as?

Back 10

Anything occupying space

Front 11

Physical properties are what in terms of matter?

Back 11

Charecteristics described without changing the chemical composition, they convert matter between physical states

Front 12

Examples of physical properties are?

Back 12

color, taste, electric charge, durability?

Front 13

Physical properties are measured by?

Back 13

The melting point

Front 14

Matter is found in what physical states?

Back 14

Solids, gas, and liquid

Front 15

Mass vs Weight

Back 15

Mass is the amount of matter in an object while weight refers to the force that gravity attracts the object with. weight differs, mass does not

Front 16

Length

Back 16

Metric and SI units use the meter, defined as the light traveling in a vacuum, 1/299,792,458

Front 17

Volume

Back 17

Amount of space occupied by an object, in SI units it is measured by the cubic meter, the metric unit uses liters

Front 18

Temperature

Back 18

Metric uses celsius, US uses Fahrenheit and Scientists use the Kelvin Scale

Front 19

Melting and boiling point of Celsius?

Back 19

Freezes at 0 and boils at 100

Front 20

Melting and boiling point of Fahrenheit?

Back 20

Freezes at 32 and boils at 212

Front 21

Melting and boiling of Kelvin?

Back 21

Freezing point is 273.15 K and boiling is 373.15 K

Front 22

What is the absolute zero?

Back 22

Used in Kelvin SI units, it is the temperature of 0 K, which is all heat energy removed

Front 23

Energy is measured by what?

Back 23

the calorie (cal) in metric and common systems and the Joule (J) in the SI system

Front 24

Define calorie

Back 24

the amount of energy required to raise the temperature of 1 g of water by 1 degree C

Front 25

How many calories are in one food calorie (Cal)? potential energy...

Back 25

1000 cal

Front 26

How many Joule's are in 1 cal?

Back 26

4.184, which is the amount of energy a human heart uses to expend each beat

Front 27

An exponent with positive values is _____ while an exponent with negative values tell you to _____ by 10

Back 27

multiply and divide

Front 28

prefixes are used for what?

Back 28

to indicate how the new unit relates to the original

Front 29

Giga has the exponent of ____ while mega has an exponent of ____?

Back 29

9 and 6

Front 30

Micro has an exponent of ____ while nano has an exponent of _____

Back 30

-6 and -9

Front 31

Accuracy measure what

Back 31

how close a value is to the true value

Front 32

Precision measures?

Back 32

reproducibility and how close measurements are to each other

Front 33

The definition of significant figures

Back 33

digits in a measurement that are reproducible when the measurement is repeated AND with the first doubtful digit

Front 34

Why do significant figures only apply to measurement?

Back 34

Measurements always contain some degree of error except if they are exact

Front 35

Rules in scientific notation for significant figures

Back 35

All digits, even zeros are significant

Front 36

Are nonzero digits significant?

Back 36

Yes

Front 37

Are zeros places between nonzero digits significant?

Back 37

Yes

Front 38

Zeros at the end of a number when there is a decimal point, ex: 4.0

Back 38

Yes

Front 39

Are zeros at the end of a number with no decimal point significant? ex: 40

Back 39

No

Front 40

Zeros placed at the ____ of a number are not significant even if there is a decimal?

Back 40

beginning, ex: 0.0006 has 1 sign. fig

Front 41

SIgnificant figures with multiplication, the answer should have?

Back 41

the same number of significant figures as the quantity with the fewest

Front 42

With addition and subtraction, significant figure answers need to be?

Back 42

the same number of decimal places as the quantity with the fewest decimals

Front 43

What is the factor label method?

Back 43

the systematic approach using conversion factors to transform units into others

Front 44

What does density relate to?

Back 44

Both mass and volume, it is the amount of mass ontained in a given volume

Front 45

_____ is determined when density of a substance is known because it makes it increase

Back 45

Temperature

Front 46

So density and temperatures do what?

Back 46

Allow thermometers to be used because together they are the basis for mercury which rises when volume amounts rise

Front 47

What does specific gravity relate to?

Back 47

the density of something compared to water

Front 48

To measure density you must measure ____ and ____ of a substance space at a given temperature

Back 48

mass and volume

Front 49

Specific heat is defined as?

Back 49

the amount of heat energy needed to raise temperature of 1 gram of substance by 1 degree C

Front 50

Specific heat uses energy in ____ and mass in ____ and temperature in ____

Back 50

calores, mass, celsius

Front 51

Waters specific heat is what per gram Celcius and what does that mean?

Back 51

1.000 cal/ g C, meaning 1.000 cal of heat will raise the temperature of 1 g of water by 1 degree C