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Chemistry 6 > Exam Review > Flashcards

Exam Review Flashcards

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1
Q

Matter

A

• matter is anything that takes up space and has mass

- stuff

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2
Q

Mass
- mass is always
Mass is measured in

A

• mass is a measure of the amount of matter the object contains

  • mass is always constant
  • mass is measured in grams of kilograms
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3
Q

Volume

A

Volume

• the amount of space occupied by the object

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4
Q

What is a substance?

A

• matter that has a uniform and definite composition is called a substance

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5
Q

Properties of matter
• ask yourself can the properties of the objective observed or measured without changing the objects identity?
• If no -
• If yes -

A

If no - chemical property

If yes - physical property

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6
Q

Physical Properties of a Substance

A
  • a quality or condition of a substance that can be observed or measured without changing the substances composition
  • Describes a matters very existence: color, shape, smell, mass, density, conductivity, malleability
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7
Q

Physical property:

A

highly reflective, highly conductive, extremely high melting point, non magnetic

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8
Q

Physical property
• does the property depend on the amount of matter present?
• If no - intensive properties - color, density, luster, hardness, temperature, melting point
• If yes - extensive properties - volume, length, mass, weight

A
  • If no - intensive properties - color, density, luster, hardness, temperature, melting point
  • If yes - extensive properties - volume, length, mass, weight
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9
Q

Extensive properties -

A

property that depends on the amount of matter in a sample: volume, weight, mass, length

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10
Q

Intensive properties

A

a property that depends on type of matter in a sample not the amount: color, density, luster, hardness, temperature

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11
Q

Solid

A
  • a form of matte that has a definite shape and volume
  • It doesn’t depend on the shape of its container
  • The particles in a solid are packed tightly together
  • Particles move very slowly
  • Expand only slightly when heated
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12
Q

Liquid

A
  • arrangement of atoms is not rigid or orderly
  • Has a definite volume
  • Does not have a definite shape
  • Flows
  • Expand slightly when heated
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13
Q

Gas

A
  • takes the shape of it’s container
  • Can expand to fill any volume
  • Takes the shape and volume of its container
  • Molecules are far apart
  • Molecules move freely
  • Vapor is the gaseous state of a substance that is generally a liquid or solid at room temperature as water vapor.
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14
Q

During a physical change some properties of a material change, but the composition of the material does ____ change.
Physical changes can be described as ______ and _______

A

During a physical change some properties of a material change, but the composition of the material does not change. Boil, freeze, condense, break, split, cut, crush.
Physical changes can be described as reversible and irreversible

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15
Q

All physical changes that involve a change from one state to another are __________

A

Reversible

- solid to liquid

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16
Q

Chemistry (central science)

A

The study of composition and matter and the changes matter undergoes

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17
Q

Chemistry affects

A

All aspects of life and most natural events because all living and nonliving things are made of matter

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18
Q

Five traditional areas of Chemistry

A
  1. analytical chemistry
  2. Inorganic chemistry
  3. Organic chemistry
  4. Physical chemistry
  5. Biochemistry
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19
Q

Analytical chemistry

A

The area of chemistry that focuses on the composition of matter

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20
Q

Inorganic chemistry

A

The study of chemicals that normally do not contain carbon. Many inorganic chemicals are found in non living things, like construction materials

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21
Q

Organic chemistry

A

The study of all chemicals containing carbon

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22
Q

Physical chemistry

A

The area that deals with mechanism, rats and energy transfer that occurs when matter undergoes a change

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23
Q

Biochemistry

A

The study of processes that take place in living organisms like muscle contraction and digestion

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24
Q

Pure chemistry

A

The pursuit of chemical knowledge for its own sake

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25
Q

Applied chemistry

A

Research that is directed toward a practical goal or application

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26
Q

Chemistry as a central science:

A

Chemistry/overlaps with many other sciences like physicists, biologists, astronomers, and geologists

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27
Q

Elements are composed of tiny particles called

A

Atoms

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28
Q

Every atom contains a ______ and one or more _________

A

Nucleus, electrons

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29
Q

The type of products obtained in a chemical reaction is determined by

A

The electrons in the reacting chemicals

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30
Q

Chemical reactions involve processes in which

A

Reactants produce products

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31
Q

Kinetic theory -The particles in matter are in

A

Constant motion

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32
Q

The mole and quantifying matter -

A

When conducting a chemical reaction you need just the right amount of reacting material, so none is wasted. The measurement is possible using the mole.

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33
Q

Every chemical process uses or produces _______, often in the form of _____

A

Energy, heat

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34
Q

Changes in quantity called _______ _________ allow you to predict whether a reaction will …..

A

Free energy, whether a reaction will actually occur under the given conditions

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35
Q

Carbon chemistry

A

Carbon compounds are the basis of life in all living organisms

36
Q

Alchemy

Alchemy didn’t provide a logical explanation for the changes in ______ they observed

A

-Field prior to chemistry that searched for methods to change metals, such as lead into gold

did not provide a logical set of explanatis for the changes in matter they observed

37
Q

Alchemy spurred the development of ____

  • it developed ____ and _____ for working with chemistry
  • it developed processes for _______ _____ and _______ _______
A
  • chemistry
  • tools and techniques
  • separating mixtures and purifying chemicals
38
Q
  • In the late 1700s ________ helped to transform chemistry from a science of _________ to a science of _______ that it is today
  • Designed a balance that could measure ______ to the nearest 0.0005 gram
  • Demonstrated that _______ is required for a material to burn.
A

• Lavoisier, observation, measurement
- mass
• Oxygen

39
Q

Scientific methodology

A

Involves making observations, proposing and testing hypotheses, and developing theories

40
Q

Hypothesis

A

Is a proposed explanation for an observation

41
Q

In an experiment when one variable changes and all the other remain constant it is called a

A

Controlled experiment

42
Q

Independent variable

A

The variable that is manipulated or purposefully changed

43
Q

Dependent variable

A

The variable that is observed and that changes in response to the independent variable

44
Q

A model

A

Is a representation of an object or event

45
Q

Law of conservation of mass

A

States that there is no detectable change in the quantity of matter during an ordinary chemical reaction

46
Q

Reasons to collaborate

A
  1. Scientists of different disciplines can be brought together to share expertise
  2. Industry may collaborate with scientists each benefitting
47
Q

Conflict with collaboration among scientist

A

Who gets the credit

48
Q

Ways of communication for scientists

A
  1. Journal - scientists establish their records in scientific journals
    - most reliable source of information about new discoveries
  2. The internet - major source of information
49
Q

Extensive properties

A

The property that depends on the amount of matter in a sample

50
Q

Intensive properties

A

Is a property that depends on the type of matter not the amount

51
Q

Physical changes can be described as

A

Reversible or irreversible

52
Q

Mixture

A

Refers to the physical combination of two or more substances in which the identities are retained

53
Q

Heterogenous mixture

A

A mixture in which the composition is not uniform

Ex: skittles

54
Q

Homogenous mixture

A

When the composition is uniform throughout

Ex: jello

55
Q

What is a phase?
How many phases does a heterogeneous mixture have?
How many phases does a homogeneous mixture have ?

A
  • any part of a sample with uniform composition and properties
  • heterogeneous has two or more phases
  • homogenous has one
56
Q

Separating mixtures

A

Mixtures can be separated by recognizing and using the differences in physical properties

  • filtration
  • distillation
  • magnetism
57
Q

Filtration

A

Process that separates a solid from a liquid

58
Q

Distillation

A

A liquid is boiled to produce a vapor that is then condensed into a liquid

59
Q

Element

A

Simplest form of matter that has unique properties

- there are over 100 known elements

60
Q

Compounds

A

A substance that contains 2 or more calmly combined is a fixed proportion

61
Q

Elements cannot be _____ ____

A

Broken down

62
Q

_______ can be broken down into simpler substances by chemical means

A

Chemicals

63
Q

Breaking down compounds:

  • _____ ______ that are used to separate mixtures CANNOT be used to separate a compound into simpler substances
  • a ______ change that produces matter with a different composition than the original matter
A
  • physical methods

- chemical

64
Q

Distinguishing substances and mixtures

  • If the composition of a material is _____ the material is a ________
  • If the composition of a material may _____ the material is a _____
A
  • fixed, substance

- vary, mixture

65
Q

Symbols and formulas:

Chemists use _______ symbols to represent _________ and ________ _________ to represent _______

A

Chemical

Elements

Chemical formulas

Compounds

66
Q

Each _____ is represented by a one- or two- chemical symbol

A

Element

67
Q

First letter is _____ and the second is ______

This represents its

A

Capitalized, lowercased

Latin name

68
Q

The periodic table:
The arrangement of elements in Which elements the elements are separated into groups based on?
This allows the comparison of what?

A
  • on a set of repeating properties

- this allows the comparison of one element to another

69
Q

Periodic table:
There are horizontal rows called what?
The elements are arranged according to what?
There are vertical rows called what?
The elements within a group have similar what

A
  • periods
  • atomic numbers
  • group
  • Similar chemical and physical properties
70
Q
  • During a chemical change what always changes?
  • usually one or more _____ is produced during s chemical change
  • are they reversible or irreversible
A
  • the composition of matter
  • substances
  • Irreversible
71
Q

Recognizing a chemical change:
There are usually four clues that indicate a chemical change

  • every chemical changes involves a
A
  1. Transfer of energy
  2. Change in color
  3. The production of a gas
  4. The formation of a precipitate
  • transfer of energy
72
Q

Law of conservation of mass

A

During any chemical reaction, the mass of the product is always equal to the mass of the reactants

73
Q

During physical changes mass also holds

A

Constant

74
Q

How do you write numbers in scientific notation

A
  • Measurement is a quantity that has both a number and a unit
  • Measurements are fundamental to the experimental sciences
75
Q

In scientific notation of a given number is written as the product of two numbers

A
  1. Coefficient

2. 10 raised to a power

76
Q

What does a positive exponent indicate

A

• A positive exponent indicates how many times the coefficient must be multiplied by 10

77
Q

Numbers bigger than 10 have what?

A

• Numbers bigger than 10 have a positive exponent and equals the number of places the decimal has been moved to the left.

78
Q

A negative exponent indicates

A

• A negative exponent indicates how many times the coefficient must be divided by 10

79
Q

Numbers smaller than one have what?

A

• Numbers smaller than one have a negative exponent and equals the number of places the decimal has been moved to the right.

80
Q

Accuracy

To evaluate accuracy what must be compare?

A

is a measure of how close a measurement comes to the actual or true value of whatever is measured
• to evaluate accuracy of a measurement, the measured value must be compared to the correct value

81
Q

Precision

To evaluate precision what must be compared?

A

Precision - is a measure of how close a series of measurements are to one another irrespective of the actual value
• To evaluate precision of a measurement you must compare the values of two or more repeated measurements

82
Q

Accepted value

A

the correct value for the measurement based on a reliable reference

83
Q

Experimental value -

A

The value measured in a lab

84
Q

Significant figures:

- the significant figures in a measurement include what

A

Significant figures
• include all of the digits that are known plus a last digit that is estimated
• Significant figures are calculated answers often depend on the number of significant figures in the values used in the calculation

85
Q

Significant figures:
- Zeros appearing between nonzero digits are:
• leftmost zeros appearing in front of the nonzero digits are: , They act as placeholders
• Leading zeros are
• Zeros at the end of a number and to the right of a decimal point are always
• Trailing zeros count as ________ if there is a decimal
• Zeros at the rightmost end of a measurement that lie to the left of an understood decimal point are __________ if they serve as place holders to show the magnitude of the number

A
  • significant
  • not significant
  • not significant
  • significant
  • significant
  • not significant
86
Q

Unlimited significant figures occur in two situations:

A
  1. Counting. A munger that is counted is exact

2. Exactly defined quantities such as chosen found in a system of measurement

Chemistry 6 (8 decks)

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