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Chemistry 110 > (Ch.3) Matter & Energy > Flashcards

(Ch.3) Matter & Energy Flashcards

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1
Q

Define Matter. What is it composed of?

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

Define Atoms.

A

Submicroscopic particles that are the building blocks of matter.

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3
Q

Define Molecules. What are molecule made of?

A

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

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4
Q

What are the three states of matter?

A

Solid, Liquid, Gas

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5
Q

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

A

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

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6
Q

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

A

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

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7
Q

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

A

S- Defined
L- Indefinite
G- Indefinite

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8
Q

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

A

S- Definite
L- Definite
G- Indefinite

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9
Q

Which state of matter is compressible? Why?

A
  1. Gas
  2. The particles in gaseous matter have space between them, thus they can be squeezed together-compressing the gas.
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10
Q

Matter has two sub-classifications, what are they?

A
  1. Pure Substances
  2. Mixtures
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11
Q

Define “Pure Substances.”
Define “Mixtures.”

A
  1. A form of matter with only one type of atom/molecule.
  2. A form of matter with 2+ types of atoms or molecules.
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12
Q

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

A
  1. Elements
  2. Compounds
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13
Q

Mixtures have two sub-classifications, what are they?

A
  1. Homogeneous
  2. Heterogeneous
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14
Q

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

A
  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.
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15
Q

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

A
  1. A mixture that is uniform throughout.
  2. A non-uniform mixture.
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16
Q

Define “Properties.”

A

Characteristics that distinguish one substance from another.

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17
Q

What are the two categories of properties?

A

Chemical & Physical

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18
Q

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

A

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

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19
Q

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

A

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

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20
Q

Define Physical Change in a substance.

A

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

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21
Q

Define Chemical Change in a substance.

A

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

22
Q

_______->chemical change->__________

A
  1. reactants
  2. products
23
Q

What are two ways to separate mixtures through physical changes?

A
  1. Distillation
  2. Filtration
24
Q

Explain the process of Distillation.

A

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.

25
Q

Explain the process of Filtration.

A

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

26
Q

Describe the Law of Conservation of Mass.

A

Matter is neither created or destroyed.

27
Q

Convert 215 cal to kilojoules? ♥️

A

I got 899560 instead of 899.56?

28
Q

Define Energy.

A

The capacity to do work.

29
Q

Define Kinetic Energy.

A

Energy associated with motion

30
Q

Define Potential Energy.

A

Energy associated with the position of matter.

31
Q

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

A

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)

32
Q

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

A
  1. Exothermic
  2. Endothermic
33
Q

Define Exothermic. Give an example.

A

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

34
Q

Define Endothermic. Give an example.

A

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

35
Q

Define Temperature. Give an example.

A

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

36
Q

What are the three units of temperature that we use?

A
  1. Farenheit
  2. Celsius
  3. Kelvin
37
Q

What is the conversion equation from Kelvin to Celsius?

A

K = C+273.15
or
C = K-273.15

38
Q

What is the conversion equation from Celsius to Fahrenheit?

A

C= F-32/1.8

39
Q

What temp does water freeze/boil in Fahrenheit?

A

Boil: 212 F
Freeze: 32 F

40
Q

What temp does water freeze/boil in Celsius?

A

Boil: 100 C
Freeze: 0 C

41
Q

What temp does water freeze/boil in Kelvin?

A

Boil: 373.15 K
Freeze: 273.15 K

42
Q

What is “Absolute Zero?”

A

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

43
Q

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

A

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

44
Q

Define Specific Heat Capacity.

A

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

45
Q

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

A

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

46
Q

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

A

q= (m) (C) (DeltaT)

47
Q

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

A

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

48
Q

Convert cal to J.

A

1 cal= 4.184 J

49
Q

Convert Cal to cal.

A

1 Cal= 1000 cal

50
Q

Convert kWh to J.

A

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

Chemistry 110 (13 decks)

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