(Ch.3) Matter & Energy

Question 1

Define Matter. What is it composed of?

Answer 1

1. Anything that occupies space and has mass.
2. Atoms

Question 2

Define Atoms.

Answer 2

Submicroscopic particles that are the building blocks of matter.

Question 3

Define Molecules. What are molecule made of?

Answer 3

1.Two or more atoms joined together in a specific geometric arrangement.
2. Bonded atoms.

Question 4

What are the three states of matter?

Answer 4

Solid, Liquid, Gas

Question 5

What “Motion” do the three states of matter have?

Answer 5

S- Vibrating/Oscillating about a fixed point
L- Free to move relative to one another
G- Free to move relative to one another

Question 6

What “Spacing” do the three states of matter have?

Answer 6

S- Close together
L- Close together
G- Far apart

Question 7

What “Shape” do the three states of matter have?

Answer 7

S- Defined
L- Indefinite
G- Indefinite

Question 8

What “Volume” do the three states of matter have?

Answer 8

S- Definite
L- Definite
G- Indefinite

Question 9

Which state of matter is compressible? Why?

Answer 9

1. Gas
2. The particles in gaseous matter have space between them, thus they can be squeezed together-compressing the gas.

Question 10

Matter has two sub-classifications, what are they?

Answer 10

1. Pure Substances
2. Mixtures

Question 11

Define “Pure Substances.”
Define “Mixtures.”

Answer 11

1. A form of matter with only one type of atom/molecule.
2. A form of matter with 2+ types of atoms or molecules.

Question 12

Pure Substances have two sub-classifications, what are they?

Answer 12

1. Elements
2. Compounds

Question 13

Mixtures have two sub-classifications, what are they?

Answer 13

1. Homogeneous
2. Heterogeneous

Question 14

Define an Element.
Define a Compound.
What are their defining differences?

Answer 14

1. A substances that can’t be broken down into a smaller substance.
2. The CHEMICAL combination of 2+ elements.
3. Elements can’t be broken down into simpler substances by chemical processes, while compounds can decompose.

Question 15

Define homogeneous mixtures.
Define heterogeneous mixtures.
What are their defining differences?

Answer 15

1. A mixture that is uniform throughout.
2. A non-uniform mixture.

Question 16

Define “Properties.”

Answer 16

Characteristics that distinguish one substance from another.

Question 17

What are the two categories of properties?

Answer 17

Chemical & Physical

Question 18

What does it mean that a substance is displaying physical properties? Give an example.

Answer 18

Physical Properties a properties/characteristics substance displays without changing it’s composition.
(ex. smell, color, shape, boiling point, density)

Question 19

What does it mean that a substance is displaying chemical properties? Give an example.

Answer 19

Chemical properties are properties/characteristics a substance can display only by changing it’s composition.
(ex. flammability, iron rusting, corrosion)

Question 20

Define Physical Change in a substance.

Answer 20

Physical change is change that affects only the appearance of a substance- not it’s chemical composition.

Question 21

Define Chemical Change in a substance.

Answer 21

Chemical change is change in which matter changes composition (to a new substance.)

Question 22

_______->chemical change->__________

Answer 22

1. reactants
2. products

Question 23

What are two ways to separate mixtures through physical changes?

Answer 23

1. Distillation
2. Filtration

Question 24

Explain the process of Distillation.

Answer 24

The mixture is heated and the liquid with the lower boiling point evaporates first and is collected. The collected vapor is allowed to cool and return to it’s liquid state.

Question 25

Explain the process of Filtration.

Answer 25

A mixture of liquid and solid is funnelled against a filter paper, separating the two.

Question 26

Describe the Law of Conservation of Mass.

Answer 26

Matter is neither created or destroyed.

Question 27

Convert 215 cal to kilojoules? ♥️

Answer 27

I got 899560 instead of 899.56?

Question 28

Define Energy.

Answer 28

The capacity to do work.

Question 29

Define Kinetic Energy.

Answer 29

Energy associated with motion

Question 30

Define Potential Energy.

Answer 30

Energy associated with the position of matter.

Question 31

What does it mean that kinetic and potential energy are interconvertible?

Answer 31

They are capable of being exchanged for one other. (ex. a ball on a hill exhanges it's potential energy for kinetic once it stops rolling)

Question 32

Physical and chemical changes are associated with Energy Change. What are the two classifications of energy change?

Answer 32

1. Exothermic 2. Endothermic

Question 33

Define Exothermic. Give an example.

Answer 33

A chemical reaction that releases energy. (ex. TNT, wax in a candle burning) (vapor->water->ice)

Question 34

Define Endothermic. Give an example.

Answer 34

A chemical reaction that absorbs energy. (ice->water->vapor) Absorbs heat from the surroundings in order to melt/evaporate.

Question 35

Define Temperature. Give an example.

Answer 35

A measure of thermal energy. (ex. The colder the temperature the less thermal motion/energy)

Question 36

What are the three units of temperature that we use?

Answer 36

1. Farenheit 2. Celsius 3. Kelvin

Question 37

What is the conversion equation from Kelvin to Celsius?

Answer 37

K = C+273.15 or C = K-273.15

Question 38

What is the conversion equation from Celsius to Fahrenheit?

Answer 38

C= F-32/1.8

Question 39

What temp does water freeze/boil in Fahrenheit?

Answer 39

Boil: 212 F Freeze: 32 F

Question 40

What temp does water freeze/boil in Celsius?

Answer 40

Boil: 100 C Freeze: 0 C

Question 41

What temp does water freeze/boil in Kelvin?

Answer 41

Boil: 373.15 K Freeze: 273.15 K

Question 42

What is "Absolute Zero?"

Answer 42

This is the coldest temperature possible, and the lowest degree in terms of the Kelvin Scale.

Question 43

What happens to molecules when they are in Absolute Zero Kelvin?

Answer 43

All motion stops (or at least slows down as much as it can.)

Question 44

Define Specific Heat Capacity.

Answer 44

The quantity of heat required to change the temp. of 1 gram of the substance by 1 degree C.

Question 45

What is the common substance with an abnormally high specific heat capacity?

Answer 45

Water! It takes a ton of heat energy to raise or lower the temp of water.

Question 46

What is the equation to find the relationship between temp and energy change?

Answer 46

q= (m) (C) (DeltaT)

Question 47

In the Equation q= (m)(C)(DeltaT) what do each of the letters represent?

Answer 47

q= amount of heat in J m= amount of mass in grams c= specific heat capacity DeltaT= Change in temp (Tf-Ti)

Question 48

Convert cal to J.

Answer 48

1 cal= 4.184 J

Question 49

Convert Cal to cal.

Answer 49

1 Cal= 1000 cal

Question 50

Convert kWh to J.

Answer 50

1 kWh=3.60 * 10^6 (3,600,000)