Chapter 2 & 3

Question 1

Energy

Answer 1

the ability to do work

Question 2

Potential energy

Answer 2

energy stored for later use

Question 3

kinetic energy

Answer 3

the energy of motion

Question 4

what is heat

Answer 4

kinetic energy because it is associated with motion of particles

Question 5

Temperature

Answer 5

a measure of how hot or cold a substance is compared to another substance

Question 6

How does heat flow?

Answer 6

from a substance a higher temperature to a substance at lower temperature until the temperatures are the same

Question 7

3 types of thermometer scales

Answer 7

1. Fahrenheit
2. Celsius
3. Kelvin

Question 8

Fahrenheit 
•formula
•how many units is it based on
•freezing point
•boiling point

Answer 8

• (1.8 x C) + 32
• based on 180 units
• 32 F
• 212 F

Question 9

Celsius
•formula
•how many units is it based on
•freezing point
•boiling point

Answer 9

• (F-32) / 1.8
• based on 100 units
• 0 C
• 100 C

Question 10

Kelvin
•formula
•how many units is it based on
•freezing point
•boiling point

Answer 10

• C + 273.15
• based on 100 units
• 273 K
• 373 K

Question 11

hypothermia
•F
•C

Answer 11

• less than 96.8 F

* less than 36 C

Question 12

“Normal”
•F
•C

Answer 12

• 98.6 F

* 37 C

Question 13

Normal Range
•F
•C

Answer 13

• 96.8 - 100.4 F

* 36 - 38 C

Question 14

Hyperthermia
•F
•C

Answer 14

• greater than 100.4 F

* greater than 38 C

Question 15

Death
•F
•C

Answer 15

• greater than 105.8 F

* greater than 41 C

Question 16

How is heat measured?

Answer 16

in Joules or calories

Question 17

Calories

Answer 17

defined amount of energy

Question 18

Conversions of joules, calories, and kilocalories
•1 calorie (cal)  = \_\_ joules
•1 kJ = \_\_ joules
•1 kJ = \_\_ calories (cal)
•1 kJ = \_\_ Calories (Cal)

Answer 18

• 4,184 J
• 1,000 J
• 1,000 J
• 1,000 cal
• 1 Calorie

Question 19

1 calorie is the energy required to…

Answer 19

raise the temp of one gram of water by 1 C

Question 20

Specific heat
•definition
•allows comparison...
•example: Earth's moon (High 107 C, low -1576 C)
Mars (High 20 C, low -60 C)
Which one has a larger specific heat?

Answer 20

• the amount of heat that raises the temperature of 1g of a substance by 1 C
• of heat transfer between substances
• mars rock

Question 21

For the same amount of heat added, a substance with a large specific heat
•has a smaller increase in temperature
•has a greater increase in temperature

Answer 21

•has a smaller increase in temperature

Question 22

When water cools, the surrounding air
•cools
•warms

Answer 22

warms

Question 23

Sand in the desert is hot in the day and cool at night. Sand must have a
•high or low specific heat

Answer 23

low specific heat

Question 24

calorimeter
•what is it used for
•what does it contain
•what 2 things does it indicate

Answer 24

• used to measure heat transfer
• contains a reaction chamber and thermometer
• indicates heat lost by a sample
• indicates the heat gained by water

Question 25

Typical Energy (caloric) values for 3 food types 1. Carbohydrate (kJ/g ; kcal/g) 2. Fat (kJ/g ; kcal/g) 3. Protein (kJ/g ; kcal/g)

Answer 25

1. 17 kJ/g ; 4 kcal/g 2. 38 kJ/g ; 9 kcal/g 3. 17 kJ/g ; 4 kcal/g

Question 26

Matter •definition •how many physical states exist

Answer 26

* the material that makes up a substance | * 3

Question 27

Pure substance •definition •what is it when it is composed of one type of •what is it when composed of 2 or more elements combined in a definite ratio

Answer 27

* matter with a specific composition * element * compound

Question 28

2 types of pure substances

Answer 28

1. elements (copper) | 2. compounds (water)

Question 29

2 types of mixtures

Answer 29

1. Homogeneous (Brass - copper and zinc) | 2. Heterogeneous (water and copper)

Question 30

elements

Answer 30

pure substances that contain atoms of only one type

Question 31

compounds

Answer 31

contain 2 or more elements in a definite ratio

Question 32

Mixture is matter that consists of | •4 things

Answer 32

* 2 or more substances that are physically mixed, not chemically combined * substances that can be separated by physical methods * heterogeneous composition * homogeneous composition

Question 33

Heterogeneous compostion

Answer 33

* is uniform throughout | * can see separate parts (may be opaque)

Question 34

Homogeneous liquid

Answer 34

* composition is not uniform throughout * can't see separate parts, if liquid-will be clear * air

Question 35

Physical properties •what is it used for •how are they observed •change?

Answer 35

* used to describe a substance * observed or measured without changing the identity of a substance * do not change the amount of substance

Question 36

Physical change

Answer 36

* the identity and composition of the substance do not change * that state can change or the material can be torn into smaller pieces

Question 37

``` Sublimation •definition •example •where does it take place •what is it used for ```

Answer 37

* occurs when a solid changes directly to a gas * dry ice (sublimes at -78 C) * in a frost-free refrigerator * used to prepare freeze-dried foods for long term storage

Question 38

Evaporation

Answer 38

occurs when molecules on the surface gain sufficient energy to form a gas

Question 39

Condensation

Answer 39

Occurs when gas molecules lose energy and form a liquid

Question 40

Boiling

Answer 40

Occurs when molecules within the substance gain sufficient energy to become a gas, as indicated by formation of vapor bubbles

Question 41

Heating curve | •5 steps

Answer 41

1. Heating ice from -15 C to 0 C 2. Melt ice at 0 C 3. Heating water from 0 C to 100 C 4. Boiling water at 100 C 5. Heating steam from 100 C to 200 C

Question 42

Chemical properties

Answer 42

describe the ability of a substance to change into a new substance

Question 43

During a chemical change...

Answer 43

reacting substances form new substances with different compositions and properties

Question 44

Intermolecular forces •definition •what does it determine •3 main forces (called Van Der Waals forces)

Answer 44

•attractive forces that act between different molecules •determines physical properties of molecular compounds, liquid or solid or gas at a given temp 1. Dipole 2. London dispersion force 3. Hydrogen bonding