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Chemistry Honors > Matter and Energy Unit > Flashcards

Matter and Energy Unit Flashcards

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1
Q

What is matter?

A

Anything which has mass and volume.

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2
Q

What is mass?

A

Mass is a measure of the amount of matter in a sample.

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3
Q

What is volume?

A

Volume is a measure of the amount of space occupied by a sample of matter.

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4
Q

What is the Law of Conservation of Energy?

A

Matter cannot be created or destroyed,but the particles of matter can be rearranged.

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5
Q

What is a substance?

A

A variety of matter that always has the same properties and composition.

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6
Q

What is energy?

A

Energy is the ability to move matter.

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7
Q

What is the Law of Conservation of Energy?

A

Energy cannot be created or destroyed, but it can change forms.

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8
Q

What are the two kinds of energy?

A

Potential: stored energy
Kinetic: energy of motion

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9
Q

How to determine significant figures?

A
  • non-zeros are significant
  • zeros between significant digits are significant
  • any zero to the right of a decimal place and to the right of a non-zero digit is significant
  • a zero to the right of a digit (if there is a decimal place) is significant
  • pure numbers have infinite significant digits.
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10
Q

What are the metric system units for mass?

A

Kilograms, grams, and miligrams

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11
Q

What are the metric system units for volume?

A

Liters and milliliters

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12
Q

What are the prefixes?

A

mili – thousandth (.001)
centi – hundredth (.01)
deci – tenth (.1)
kilo – thousand (1000)

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13
Q

What is kinetic theory?

A

All matter is made of atoms/molecules or particles that are in constant motion.

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14
Q

What is temperature?

A

Temperature is the average kinetic energy or movement of particles in a sample.

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15
Q

What is heat?

A

Heat is the total kinetic energy of all the particles in a substance. Heat can move from higher to lower temperature.

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16
Q

What is the difference between temperature and heat?

A

Heat cannot be measured, only calculated.

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17
Q

In Kelvin, what is the freezing and boiling point?

A

Freezing: 273 k
Boiling Point: 373 k

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18
Q

Why is 0 k a special temperature?

A

It is the lowest temperature possible. The particles stop moving completely. (-273 C)

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19
Q

What are exothermic reactions?

A

Reactions where heat goes out. It releases heat energy. Most reactions are like these.

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20
Q

What are endothermic reactions?

A

Reactions that absorb heat energy?

21
Q

What are the examples of exothermic reactions?

A

Freezing and condensation.

22
Q

What are examples of endothermic reactions?

A

Melting, evaporation, and sublimation.

23
Q

what do you need for calculating heat?

A

Temperature and mass.

24
Q

What is the specific heat capacity equation?

A

q = MCΔT

25
Q

What is sublimation?

A

A phase change for a solid to a gas.

26
Q

What is the heat of fusion?

A

It is the heat required to change the phase of 1 gram of substance from solid to liquid.

27
Q

What is the heat of fusion equation?

A

q=mHf

28
Q

Does temperature rise during phase changes?

A

It does not, it remains constant.

29
Q

What is the heat of vaporization?

A

It is the heat required to change the phase of 1 gram of substance from liquid to vapor.

30
Q

What is the heat of vaporization equation?

A

q=mHv

31
Q

When to use each equation?

A

q = MCΔT - change in temperature
q=mHf - susbtnace changes from solid to liquid
q=mHv - substance changes from liquid to gas

32
Q

What happens to kinetic and potential energy during phase change?

A

Kinetic energy is constant and potential energy increases. The opposite is true for other parts of the graph not in a phase change.

33
Q

What is the organization of solids like?

A

Particles are close together due to strong forces of attraction. Particles vibrate in place and are arranged in a regular geometric pattern. Solids have a definite shape and volume.

34
Q

What is the organization of liquids like?

A

Particles are tightly packed due to forces of attraction, but are far apart enough to move. They have an indefinite shape but a definite volume (they take the shape of their container).

35
Q

What is the organization of gasses like?

A

The particles have free movement under most conditions. The particles are far apart and move freely. Gas particles move in straight paths until they collide with another particle. Gasses have indefinite volume and shape.

36
Q

What are phase changes?

A

Phase changes are the rearrangement of particles into positions of greater or lesser potential energy. Heat energy is converted into potential energy or vice versa. Phase changes are physical changes.

37
Q

What are physical changes?

A

Division of a sample and phase changes.

38
Q

What are chemical changes?

A

Reactions, combustion, rusting, corrosion, and cooking.

39
Q

What are atoms?

A

Atoms are the simplest particles in nature. There are about 90 different naturally occurring types of atoms.

40
Q

What is an element?

A

A sample that has only one kind of atom. Elements cannot be made any simpler by ordinary chemical means.

41
Q

What is a compound?

A

Compounds are composed of 2 or more kinds of atoms that are chemically joined together by bonds in a specific ratio. A compound can be decomposed to its elements.

42
Q

Which forms of matter are substances?

A

Elements and compounds are substances. Mixtures are not.

43
Q

What is a mixture?

A

A mixture contains more than one substance not chemically joined together in no specific proportion.

44
Q

What is a homogeneous mixture?

A

A mixture that is uniform throughout (equally distributed).

45
Q

What is a heterogeneous mixture?

A

A mixture that is different in different parts (not uniform).

46
Q

What are the methods of separating mixtures?

A

Evaporation, distillation, and paper chromatography.

47
Q

What is the method of evaporation?

A

it is used to separate substances with different boiling points. A mixture is boiled and only one is evaporated.

48
Q

What is the method of distillation?

A

Used to separate dissolved substances. Combines evaporation and condensation.

49
Q

What is the method of paper chromatography?

A

Depends on differences in the mass of different particles and differences in their forces of attraction for the paper.

Chemistry Honors (11 decks)

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