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intro to Chem > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

convert 1 meter into nano

A

1m = 10^9 nm

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2
Q

convert 1 meter into milli

A

1m = 10^3 mm

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3
Q

convert 1 meter into centi

A

1m = 100 cm

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4
Q

dimensional analysis: rearrange the question 5 meters/seconds X (times) 10 seconds

A

5 x 10 x m/s x s. Then cross out the two s’. You then get 50 m

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5
Q

why is it important to make measurements in science?

A

science is very quantitative and collects data

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6
Q

Is metric used most in science true or false?

A

True

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7
Q

all quantitative data requires a __ and a __ unit

A

number; unit

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8
Q

what is the purpose of using scientific notation?

A

used to simply very large or very small numbers

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9
Q

what are the two things required for scientific notation?

A

a number between 1 and 10, and a power of 10

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10
Q

how would you write 0.000012 in scientific notation

A

1.2 x 10 ^-5

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11
Q

ignore

A

ignore

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12
Q

Scientific notation: if you have a very large number, it is represented as?

A

10^n

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13
Q

Scientific notation: if you have a very small number, it is represented as

A

10^-n

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14
Q

when you have a really big number, like 120000, what is the scientific notation? What would the process look like?

A

count/move the decimal place through each zero till you place the decimal spot in between 1 and 2. Then count the number of moves as the 10^n

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15
Q

using a calculator: you replace 10 with what?

A

E on calculator

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16
Q

Calculator: After you’ve used E for your equation, and want to see the number in scientific notation, what do you do?

A

press 2nd then SCI.

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17
Q

Which SI unit and symbol is represented for Mass?

A

kilogram; kg

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18
Q

Which SI unit and symbol is represented for length

A

Meter; M

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19
Q

Which SI unit and symbol are represented for Time?

A

Second; S

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20
Q

Which SI unit and symbol is represented for temperature

A

Kelvin; K

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21
Q

Which SI unit and symbol are represented for amount?

A

Mole; mol

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22
Q

Convert 1 meter into kilo

A

1m = 10^-3 km

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23
Q

ignore

A

ignore

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24
Q

when something says scaling factors, what does it mean?

A

the symbols used for measurements (kg, cm, m etc)

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25
Q

Definition of mass

A

quantity of matter inside an object

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26
Q

The process of determining mass is called?

A

weighing

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27
Q

do not confuse mass with ___

A

weight

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28
Q

what is the key difference between mass and weight?

A

mass is the quanity of matter in an object; weight is the gravitation force acting on an object’s mass

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29
Q

why is the kelvin scale important?

A

because it is based on molecular motion

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30
Q

at 0 K, what is the kinetic energy?

A

zero kinetic energy

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31
Q

when kelvin is at zero, celsius is at?

A

-273.15

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32
Q

what are 2 examples of the derived units of area and volume?

A

cm^2; cm^3

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33
Q

Density is the

A

ratio of mass to volume

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34
Q

what is volume

A

the amount of space a substance has in a container

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35
Q

solids = g/__

A

cm^3

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36
Q

liquids = g/__

A

ml

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37
Q

gases/g/__

A

L

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38
Q

ignore

A

ignore

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39
Q

why do you use g/L when measuring gas?

A

because gas takes up a lot more space

40
Q

how do you determine volume?

A

by water displacement

41
Q

who discovered volume?

A

archimedes

42
Q

how would you approach the question: you find that a n in ml of a liquid weights n in g, what is the density?

A

n in g/n in ml

43
Q

what is the formula for density?

A

mass divided by the volume

44
Q

when you heat up an object, what happens to the density

A

it changes

45
Q

when a question uses the wording “ it displaces by x amount” what are they really asking?

A

the volume

46
Q

density = what / divided by what

A

mass divided by volume

47
Q

what unit measurement is volume always displayed as ___

A

cm^3

48
Q

if you make measurements persistently but not accurately there is no scientific value

A

true

49
Q

what are the two types of errors?

A

random errors and systematic errors

50
Q

what are the most common type of errors

A

random errors

51
Q

meaning of random errors

A

-results from the limitations of the experimenters skills

52
Q

meaning of systematic errors

A

inherent errors in instruments and cause consistent errors

53
Q

how do you reduce random errors?

A

reduce by making repeat measurements

54
Q

what do you do if you run into systematic errors

A

you need to find the source of the error

55
Q

what is an example of a systematic error?

A

a faulty balance

56
Q

measuring meniscus in a container (its just a substance) the measurement looks concave. Which part do you measure?

A

the bottom of the concave meniscus

57
Q

always estimate __ the lines

A

between

58
Q

what are significant figures used for

A

used to express the uncertainty in a measurement

59
Q

6.003 - how many significant numbers

A

4

60
Q

0.00035 how many significant numbers

A

2

61
Q

0.00035000 how many significant numbers

A

5

62
Q

“trailing zeros” reffer to what

A

zeros that come after a significant number after a decimal point. IE: 0.035000 (the last three zeros are significant)

63
Q

10,000 has how many significant figures?

A

1

64
Q

do the zeros in 0.0025 count as significant numbers?

A

no

65
Q

101 - does the zero count as a significant number?

A

yes

66
Q

all non zero digits do/do not count as significant figures?

A

they do count

67
Q

zeros in-between number do or do not count as sig figs

A

they do count

68
Q

1.00, how many sig figs?

A

3

69
Q

differentiate the sig figs of 10,000. & 10,000

A

10,000. = 5 10,000 = 1

70
Q

how many sig figures have in 1.050

A

4

71
Q

150.0 has how many sig figs

A

4

72
Q

if 150 has 2 sig figs, how would you write it in scientific notation?

A

1.5 x 10^2

73
Q

if 150 has 3 sig figs, how would you write it in scientific notation?

A

1.50 x 10^2

74
Q

round these two significant figures to 2 sf: 3.15 & 1.36

A

3.2 1.4

75
Q

0.04450 has how any sig figs?

A

4

76
Q

when something has a definitive answer. How many sig figs are there?

A

infinite number

77
Q

how many sig figs in 1.000 x 10^5

A

4 - the digit 1 and the trailing 0’s (just ignore the 10^5)

78
Q

how many sig figs in 0.00002

A

1 (do not count the leading zeros)

79
Q

determine the amount of significant figures and the range of precision: 0.00120 **even if you get these right, put it that you got them wrong so you can practice more

A

3 sig figs - 0.00119 to 0.00121

80
Q

determine the amount of significant figures and the range of precision: 120. **even if you get these right, put it that you got them wrong so you can practice more

A

3 sig figs, 119 to 121

81
Q

determine the amount of significant figures and the range of precision: 12.00 **even if you get these right, put it that you got them wrong so you can practice more

A

4 sig - 11.99 to 12.01

82
Q

determine the amount of significant figures and the range of precision: 1.20 x 10^3 **even if you get these right, put it that you got them wrong so you can practice more

A

3 sig figs 1190 to 1210

83
Q

what is the rule about multiplying/dividing significant figures

A

of sig figs in the answer should be the same as the measurement with the least number of sig figs

84
Q

sig fig addition/subtraction rule

A

the number of sig. figs. in the answer is limited by the least number of decimal place

85
Q

when multiplying 5.02 x 89.665 x 0.10, how many significant figures would the answer have?

A

2 sig figs (lowest sig figs in question was 0.10 (2 sig figs)

86
Q

1 ml = ___ g?

A

0.768

87
Q

1 ml= __ L?

A

10^-3

88
Q

1 kg = ___ g?

A

1000

89
Q

There are three rules on determining how many significant figures are in a number:

A

Non-zero digits are always significant. Any zeros between two significant digits are significant. A final zero or trailing zeros in the decimal portion ONLY are significant.

90
Q

a change in color, the formation of bubbles, the spontaneous increase or decrease in temperature are signs of a

A

chemical change

91
Q

a change in color, the formation of bubbles, the spontaneous increase or decrease in temperature are signs of a

A

chemical change

92
Q

reversed

chemical change

A

a change in color, the formation of bubbles, the spontaneous increase or decrease in temperature are signs of a

93
Q

phase changes are a

A

physical change

94
Q

*reversed card - physical change

A

phase changes are a

95
Q

what are the qualitative observation to make for solids:

A

colour or colourless

96
Q

what are the qualitative observation to make on liquids and gas

A

liquids : colour or colourless, clear or cloudy

gas - colour or colourless

intro to Chem (11 decks)

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