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Chemistry 101 > Chapter 2 & 3 > Flashcards

Chapter 2 & 3 Flashcards

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1
Q

Energy

A

the ability to do work

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2
Q

Potential energy

A

energy stored for later use

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3
Q

kinetic energy

A

the energy of motion

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4
Q

what is heat

A

kinetic energy because it is associated with motion of particles

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5
Q

Temperature

A

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

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6
Q

How does heat flow?

A

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

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7
Q

3 types of thermometer scales

A
  1. Fahrenheit
  2. Celsius
  3. Kelvin
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8
Q 
Fahrenheit 
•formula
•how many units is it based on
•freezing point
•boiling point
A
  • (1.8 x C) + 32
  • based on 180 units
  • 32 F
  • 212 F
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9
Q 
Celsius
•formula
•how many units is it based on
•freezing point
•boiling point
A
  • (F-32) / 1.8
  • based on 100 units
  • 0 C
  • 100 C
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10
Q 
Kelvin
•formula
•how many units is it based on
•freezing point
•boiling point
A
  • C + 273.15
  • based on 100 units
  • 273 K
  • 373 K
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11
Q

hypothermia
•F
•C

A
  • less than 96.8 F

* less than 36 C

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12
Q

“Normal”
•F
•C

A
  • 98.6 F

* 37 C

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13
Q

Normal Range
•F
•C

A
  • 96.8 - 100.4 F

* 36 - 38 C

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14
Q

Hyperthermia
•F
•C

A
  • greater than 100.4 F

* greater than 38 C

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15
Q

Death
•F
•C

A
  • greater than 105.8 F

* greater than 41 C

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16
Q

How is heat measured?

A

in Joules or calories

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17
Q

Calories

A

defined amount of energy

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18
Q 
Conversions of joules, calories, and kilocalories
•1 calorie (cal)  = \_\_ joules
•1 kJ = \_\_ joules
•1 kJ = \_\_ calories (cal)
•1 kJ = \_\_ Calories (Cal)
A
  • 4,184 J
  • 1,000 J
  • 1,000 J
  • 1,000 cal
  • 1 Calorie
19
Q

1 calorie is the energy required to…

A

raise the temp of one gram of water by 1 C

20
Q 
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?
A
  • the amount of heat that raises the temperature of 1g of a substance by 1 C
  • of heat transfer between substances
  • mars rock
21
Q

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

A

•has a smaller increase in temperature

22
Q

When water cools, the surrounding air
•cools
•warms

A

warms

23
Q

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

A

low specific heat

24
Q

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

A
  • used to measure heat transfer
  • contains a reaction chamber and thermometer
  • indicates heat lost by a sample
  • indicates the heat gained by water
25
Q

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)
A
  1. 17 kJ/g ; 4 kcal/g
  2. 38 kJ/g ; 9 kcal/g
  3. 17 kJ/g ; 4 kcal/g
26
Q

Matter
•definition
•how many physical states exist

A
  • the material that makes up a substance

* 3

27
Q

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

A
  • matter with a specific composition
  • element
  • compound
28
Q

2 types of pure substances

A
  1. elements (copper)

2. compounds (water)

29
Q

2 types of mixtures

A
  1. Homogeneous (Brass - copper and zinc)

2. Heterogeneous (water and copper)

30
Q

elements

A

pure substances that contain atoms of only one type

31
Q

compounds

A

contain 2 or more elements in a definite ratio

32
Q

Mixture is matter that consists of

•4 things

A
  • 2 or more substances that are physically mixed, not chemically combined
  • substances that can be separated by physical methods
  • heterogeneous composition
  • homogeneous composition
33
Q

Heterogeneous compostion

A
  • is uniform throughout

* can see separate parts (may be opaque)

34
Q

Homogeneous liquid

A
  • composition is not uniform throughout
  • can’t see separate parts, if liquid-will be clear
  • air
35
Q

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

A
  • used to describe a substance
  • observed or measured without changing the identity of a substance
  • do not change the amount of substance
36
Q

Physical change

A
  • the identity and composition of the substance do not change
  • that state can change or the material can be torn into smaller pieces
37
Q 
Sublimation 
•definition
•example
•where does it take place
•what is it used for
A
  • 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
38
Q

Evaporation

A

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

39
Q

Condensation

A

Occurs when gas molecules lose energy and form a liquid

40
Q

Boiling

A

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

41
Q

Heating curve

•5 steps

A
  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
42
Q

Chemical properties

A

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

43
Q

During a chemical change…

A

reacting substances form new substances with different compositions and properties

44
Q

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

A

•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

Chemistry 101 (7 decks)

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