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Chemistry Unit 1 - Chapters 1 to 3 > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

Significant Figures - Non-zero digits rule

A

All of them count - except digits after an underlined number.

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2
Q

Significant Figures - Scientific notation rule

A

All digits are significant AS LONG AS they are to the left of the “x”

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3
Q

Significant Figures - with a decimal point in the number rule (D or Drury) or {Pacific rule - decimal point is present}

A

start from the left and count from the first nonzero figure

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4
Q

Significant Figures - no decimal points in the number rule (ND or Notre Dame) or {Atlantic rule - decimal is absent}

A

start from the right and count from the first nonzero figure

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5
Q

significant figure multiplied, added or subtracted by a significant figure - how many significant figures will be in the final answer?

A

the final answer will have the same number of significant figures as the lowest significant figure

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6
Q

Accuracy

A

closest to the standard value or how close you came to it

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7
Q

Precision

A

closeness of 2 or more measured values and how they are RELATED to each other

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8
Q

Why are measurements always uncertain

A

depends on the device and the user

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9
Q

name four kinds of measurements in the laboratory

A

weight-grams; volume-litre; time-seconds; temperature-degree

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10
Q

Why is estimating important

A

helps you to focus on the range your answer will fall in

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11
Q

What is the accepted value (standard) in a game of darts

A

Height from floor to bullseye is 5’8”

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12
Q

“An instrument is only as good as its operator”

A

An instrument is fantastic, but if you don’t know how to use it, it is worthless

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13
Q

Factors that determine accuracy

A

The person and the object

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14
Q

Factors that determine precision

A

The instrument, how it is set up, how it is used

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15
Q

Qauntitative Measurements

A

Numbers and units

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16
Q

Qualitative Measurements

A

Descriptions

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17
Q

SI Unit of Measurement for Length and its symbol

A

Meter (m)

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18
Q

SI Unit of Measurement for Mass and its symbol

A

Kilogram (kg)

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19
Q

SI Unit of Measurement for Temperature and its symbol

A

Kelvin (K) or Degrees Celcius ( degree C)

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20
Q

SI Unit of Measurement for Time and its symbol

A

Second (s)

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21
Q

SI Unit of Measurement for Amount of Substance and its symbol

A

Mole (mol) 1 mol is 6.02 x 10 to the 23rd

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22
Q

SI Unit of Measurement for Luminosity and its symbol

A

Candela (cd)

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23
Q

SI Unit of Measurement for Electric Current and its symbol

A

Ampere (A)

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24
Q

SI Prefixes - Name all 7 of them

A

kilo, deci, centi, milli, micro, nano, pico

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25
Q

SI Prefixes for Length - Name all 4 of them

A

kilo, deci, centi, milli

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26
Q

SI Prefix for Pressure

A

micro

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27
Q

SI Prefix for Temperature

A

nano

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28
Q

SI Prefix for Energy

A

pico

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29
Q

Explain why milliliter and cubic centimeter have the same amount in ANY kind of container

A

milliliter = cubic centimeter

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30
Q

Difference between Mass and Weight

A

Mass is the anything that has mass and volume - it’s the stuff that things are made of; whereas, weight is the how heavy or what the force of gravity is on an object

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31
Q

How much does a brick with the mass of 5 pounds weigh?

A

5 pounds

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32
Q

How much does a brick with the mass of 5 pounds on a space shuttle weigh?

A

1 ounce (because of gravitational forces)

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33
Q

What is the specific gravity of water

34
Q

Why are things compared to water’s specific gravity

A

To explain whether it will sink or float

35
Q

What is the formula for percent error

A

Approximate minus exact divided by exact times 100

36
Q

What is the saying you need to memorize for labeling a graph and what does it stand for

A

DRYMIX - Dependent Resides on the Y, Making Independent the X

37
Q

Name the 6 things all graphs must contain

A

Title, dependent variables, independent variables, appropriate scale, labeled x- and y- axis, line connecting the variables

38
Q

Describe what the line looks like in a Direct relationship graph

A

Starts from the bottom left-hand corner and climbs diagonally to the top right-hand corner

39
Q

Describe what the line looks like in an Inverse or

A

Starts from the top left-hand corner and climbs diagonally down to the bottom right-hand corner

40
Q

What is the formula for Kelvin

A

C degrees + 273

41
Q

What is the formula for Celsius

42
Q

Compare Kelvin scale size to Celsius Scale size

A

Kelvin has a larger size RANGE compared to Celsius

43
Q

Definition of Chemistry

A

The study of the composition of matter, their properties and how they interact, combine or the study of matter and the changes matter undergoes

44
Q

Definition of Matter

A

The STUFF things are made of

45
Q

Difference between pure chemistry and applied chemistry

A

Pure chemistry is the study of chemistry in a scientific and laboratory environment; applied chemistry is how products are used in everyday life

46
Q

Give 2 examples of applied chemistry

A

hairspray, clothing

47
Q

Physical Chemistry studies what

A

Behavior of matter

48
Q

Organic Chemistry studies what

A

Carbon compounds of matter

49
Q

Analytical Chemistry studies what

A

Composition of matter

50
Q

Inorganic Chemistry studies what

A

Compounds without carbon

51
Q

Biochemistry studies what

A

Life and chemistry of the body

52
Q

Purpose of Experiments according to the Scientific Method

A

To test a hypothesis and the reason for the observation

53
Q

Experiment yields unexpected results. According to the Scientific Method you should

A

Repeat it several times and if same results occur - then change your hypothesis

54
Q

Name 2 things that will make learning chemistry a success

A

Study every day, make great notes

55
Q

Chemical change results from

A

A chemical reaction

56
Q

Physical change results from

A

Matter stays the same - just takes on a different form

57
Q

Examples of Chemical Change

A

burning, cooking, rusting, rotting

58
Q

Examples of Physical Change

A

boiling, melting, freezing

59
Q

Can Physical Changes be Undone

A

Yes - just by adding energy

60
Q

Can Chemical Changes be Undone

A

Sometimes-but only by another chemical reaction

61
Q

What are the 3 phases of H2O

A

ice, water, steam

62
Q

Name the 5 steps of the Scientific Method

A

State the Problem, Make Observations, Form a Hypothesis, Perform Experiments, State your theory or re-word your hypothesis

63
Q

SI Unit of Measure for Volume and its symbol

A 
Cubic meter (m to the power of 3) or Liter (L) 
[remember... 1 ml = 1 cm cubed]
64
Q

SI Unit of Measure for Density and its symbol

A

Grams per cubic meter (g/m3)

65
Q

SI Unit of Measure for Pressure and its symbol

A

Pascal (Pa) or Atmosphere (atm)
{convert psi to mmHg (Torr)}
[1 psi (pound per square inch) = 51.7149 millimeters of mercury]

66
Q

SI Unit of Measure for Energy and its symbol

A

Joule (J) or Calorie (cal)

67
Q

Kilo symbol and exponent and meaning

A

K or 10 to the 3rd power or 1000 times larger

68
Q

Deci symbol and exponent

A

d and 10 to the negative 1 power

69
Q

Centi symbol and exponent and meaning

A

c and 10 to the negative 2 power or 100 times larger

70
Q

Milli symbol and exponent

A

m and 10 to the negative 3 power

71
Q

Micro symbol and exponent and meaning

A

“u”-looking type of thing and 10 to the negative 6 power or 1 million times larger

72
Q

Nano symbol and exponent

A

n and 10 to the negative 9 power

73
Q

Pico symbol and exponent and meaning

A

p and 10 to the negative 12 power or 1 trillion times larger

74
Q

Scientific Notation Formula

A

a times 10 to the b

where a is the coefficient and b is the exponent

75
Q

Scientific Notation Rules when Adding/Subtracting

A

Exponents must be the same and then add/subtract the numbers AND the exponent stays the same

76
Q

Scientific Notation Rules when Multiplying

A

Multiple the numbers but ADD the coefficients

77
Q

Scientific Notation Rules when Dividing

A

Divide the numbers but SUBTRACT the coefficients

78
Q

How many SI Base Units are there - name them

A

7 base units: Length-meter (m); Time-seconds (s); Amouitn of Substance-mole (mol); Electric Current-Ampule (A); Temperature-kelvin (K); Luminostiy-candela (cd); Mass-kilogram (kg)

79
Q

What is the formula for Density

A

Density = mass divided by volume

80
Q

What is the formula for Mass

A

Mass = Density times Volume

81
Q

What is the formula for Volume

A

Volume = mass divided by density

Chemistry Unit 1 - Chapters 1 to 3 (1 decks)

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