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8th Grade Science Chapter 2 and 3 Matter Test Review

front 1

Substance

back 1

a single kind of matter that is pure, meaning it always has a specific make-up - or composition - and a specific set of properties.

front 2

element

back 2

a pure substance that cannot be broken down into any other substance by physical or chemical means. Elements are the simplest substances.

front 3

What are the simplest substances?

back 3

Elements

front 4

Atom

back 4

The basic particle from which all elements are made. Different elements have different properties because they have different atoms.

front 5

Compound

back 5

pure substance made of two or more elements chemically combined in a set ratio.

front 6

How do you represent a compound?

back 6

using a chemical formula which shows the elements and their ratio of atoms.

front 7

Chemical Bond

back 7

when atoms combine they use the force of attraction between two atoms.

front 8

Mixture

back 8

made of two or more substances, elements or compounds or both, that are together in the same place but are not chemically combined.

front 9

How do mixtures differ from compounds?

back 9

Two ways:
1. Each substance keeps its individual properties.
2. Parts of a mixture are not combined in a set ratio.

front 10

Mass

back 10

measurement of the amount of matter in an object.

front 11

Weight

back 11

measure of the force of gravity on an object.

front 12

Does mass or weight change with the location of the object?

back 12

Mass does not, weight does.

front 13

Volume

back 13

The amount of space that matter occupies.

front 14

Density

back 14

relates the mass of a material in a given volume.

front 15

Endothermic Change

back 15

a change that occurs when energy is absorbed by a substance.

front 16

Formula for Volume

back 16

V= Length x Width x Height

front 17

SI unit for Volume

back 17

centimeters cubed

front 18

Formula for Density

back 18

D = Mass/Volume

front 19

exothermic change

back 19

a change that occurs when energy is released by a substance.

front 20

Energy

back 20

the ability to do work or cause change

front 21

fluid

back 21

a substance that flows

front 22

viscosity

back 22

a property of liquid to resist flowing

front 23

pressure

back 23

the force of a gas's outward push divided by the area of the walls of the container

front 24

What is the formula for pressure?

back 24

PRESSURE = FORCE/AREA

front 25

surface tension

back 25

the result of the inward pull among the molecules of a liquid that brings the molecules on the surface closer together. It is a property of liquids. As a result of this property, some liquids can act as a sort of skin.

front 26

What is a physical property of matter? Give two examples.

back 26

A characteristic of a pure substance that can be observed without changing it into another substance. Examples: freezing, melting, evaporation points, harness, texture, color, state, dissolvable, luster, malleability, flexibility,

front 27

What is a chemical property? give two examples.

back 27

characteristic of a pure substance that describes its ability to change into different substances. To observe these properties you must try to turn it into another substance. Examples: flammability, rust, oxidation, reactivity,

front 28

What are two types of mixtures?

back 28

Heterogeneous
Homogenous

front 29

Define Heterogeneous Mixture

back 29

You can see the different parts of the mixture.

front 30

Homogenous mixture

back 30

so evenly mixed that you can not see the different parts. A SOLUTION is an example.

front 31

What is the best example of a HOMOGENOUS MIXTURE?

back 31

A solution; Air, Salt Water, Brass

front 32

What is an example of a HETEROGENOUS MIXTURE?

back 32

Soil, salad, legos

front 33

Define Molecule.

back 33

Groups of two or more atoms held together by chemical bonds.

front 34

3 Examples of Molecules

back 34

Water, Oxygen, Carbon Dioxide, Salt

front 35

What is Chemistry?

back 35

Study of the properties of matter and how matter changes.

front 36

List and describe the 5 disciplines of chemistry.

back 36

Organic Chemistry - the study of carbon and its compounds; the study of the chemistry of life.

Inorganic Chemistry - the study of compounds not-covered by organic chemistry; the study of inorganic compounds or compounds which do not contain a C-H bond. Many inorganic compounds are those which contain metals.

Analytical Chemistry - the study of the chemistry of matter and the development of tools used to measure properties of matter.

Physical Chemistry - the branch of chemistry that applies physics to the study of chemistry. Commonly this includes the applications of thermodynamics and quantum mechanics to chemistry.

Biohemistry - the study of chemical processes that occur inside of living organisms.

front 37

What is the difference between mass and weight?

back 37

Mass does not change and is the amount of matter in an object. Weight changes with position in a gravity field and the gravity field and is just the measure of gravity affecting an object.

front 38

What is the formula for density?

back 38

DENSITY = MASS/VOLUME

front 39

What is the SI unit for Density?

back 39

g/cm3 (grams per centimeters cubed)

front 40

What is a physical change in matter? Give two examples.

back 40

Any change that alters the form or appearance of matter but does not make any substance in the matter into a different substance. EXAMPLE:
1. Change in state (solid, liquid, gas)
2. Change in shape

front 41

What is a chemical change in matter? Give two examples.

back 41

a change in matter that produces one or more new substances. EXAMPLES:
1. Combustion
2. Electrolysis
3. Oxidation
4. Tarnishing

front 42

What is the difference between ENDOTHERMIC and EXOGTHERMIC?

back 42

ENDOTHERMIC: Absorbs energy to support a reaction.
EXOTHERMIC: radiates energy as a product of a reaction.

front 43

What are the three states of matter?

back 43

Solid
Liquid
Gas

front 44

Create a table describing the shape and volume for each state of matter.

back 44

STATE SHAPE VOLUME EXAMPLE
Solid Definite Definite Diamond
Liquid Not Definite Definite Water
Gas Not Definite Not Definite Air

front 45

Sketch Picture of the particles of gas, liquid, and solid.

back 45

DRAW THEM.

front 46

List and define the six phase changes. tell whether they are endothermic or exothermic.

back 46

1. Melting: Change from a solid to a liquid. ENDOTHERMIC.
2. Freezing: Change from a liquid to a solid. EXOTHERMIC.
3. Evaporation: When a liquid turns into a gas only at the surface. ENDOTHERMIC.
4. Boiling: Liquid changes to a gas below its surface as well as at the surface. ENDOTHERMIC
5. Condensation: occurs when particles in gas loses enough energy to form a liquid. EXOTHERMIC
6. Sublimation: Particles of a solid go strait to gas. ENDOTHERMIC

front 47

Exothermic or Endothermic - Melting?

back 47

ENDOTHERMIC

front 48

Exothermic or Endothermic - Freezing?

back 48

EXOTHERMIC

front 49

Exothermic or Endothermic - Evaporation?

back 49

ENDOTHERMIC

front 50

Exothermic or Endothermic - Boiling?

back 50

ENDOTHERMIC

front 51

Exothermic or Endothermic - Condensation?

back 51

EXOTHERMIC

front 52

Exothermic or Endothermic - Sublimation?

back 52

ENDOTHERMIC

front 53

What are two types of vaporization?

back 53

Evaporation
Boiling

front 54

Define Evaporation:

back 54

Changing from a liquid to a gas at the surface.

front 55

Define Boiling:

back 55

Changing from a liquid to a gas at the surface and below the surface at the same time.

front 56

How are evaporation and boiling different?

back 56

Water does not change to gas below the surface during evaporation. Substances have a boiling point. they don't have evaporation points.

front 57

Sketch a heating curve of matter.

back 57

DRAW

front 58

Sketch the cooling curve of matter

back 58

DRAW

front 59

What is Boyles Law?

back 59

At a constant temperature:

1.To increase pressure you must reduce the volume.
2. To decrease pressure you must increase the volume.

front 60

Is Boyles law direct or an inverse relationship?

back 60

Inverse

front 61

What stays constant in BOYLES LAW?

back 61

Temperature.

front 62

What are the two variables in BOYLES LAW?

back 62

Pressure and Volume

front 63

What is Charles Law?

back 63

At constant pressure:
1. To increase temperature you must decrease volume.
2. To decrease temperature you must increase volume.

front 64

What stays constant in Charles law?

back 64

Pressure

front 65

What are the two variables in Charles Law?

back 65

Temperature and Volume

front 66

Draw a graph of Boyles Law. Label the X and Y Axis.

back 66

DRAW.

front 67

Draw a graph of Charles Law. Label the X and Y Axis.

back 67

DRAW