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Chemistry > Chapter 2- Scientific Method And Measurements > Flashcards

Chapter 2- Scientific Method And Measurements Flashcards

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1
Q

Define observation/asking a question

A

Gather existing information knowledge. Ask an informed question

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2
Q

Define hypothesis

A

Make a prediciton based off observations

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3
Q

Define experiment

A

Design implement experiments to test hypothesis. Should produce results that can be interpreted ambiguously with regards to the validity of the hypothesis. Carefully designed controls identify positive and negative results.

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4
Q

Define data and results

A

Record the results of the experiments.

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5
Q

Define conclusion

A

Summarize and interpret results to determine if hypothesis has been proven true or false. Future hypothesis and experiments can be discussed

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6
Q

Why do scientists need to use standard units of measure?

A

So everyone has the same measurements and uses the same numbers.

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7
Q

What is SI?

A

International System of Units

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8
Q

What is a base unit?

A

A unit based on something in the real world. Is independent of others.

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9
Q

How many SI base units are there

A

7

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10
Q

What is the SI base unit for length?

A

Meters

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11
Q

What is the SI base unit for mass?

A

Kilograms

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12
Q

What is the SI base unit for time?

A

Seconds

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13
Q

What is the SI base unit for temperature?

A

Kelvin

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14
Q

What is the second based on?

A

The frequency of radiation given off an atom.

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15
Q

What is the meter based on?

A

The distance that light travels in a vacuum.

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16
Q

What is the kilogram based on?

A

Planck’s constant

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17
Q

What is volume?

A

The space occupied by an object.

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18
Q

What is the SI unit for volume?

What do chemists often use?

A

Cubic meters (m³)

Liter (L)

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19
Q

One liter is equal to ____ cubic meters (cm³)?

A

1000

20
Q

What is density

A

Amount of mass per unit volume

21
Q

What is the formula for density

A

Mass divided by the volume (m/v)

22
Q

The best unit for density for solids is _____

The best unit for density for liquids is _____

A

g/cm³

g/mL

23
Q

What is Tera?

A

T
1×10¹²

24
Q

What is giga?

A

G
1×10⁹

25
Q

What is mega?

A

M
1×10⁶

26
Q

What is kilo?

A

k
1×10³

27
Q

What is hecto?

A

h
1×10²

28
Q

What is deka?

A

da
1×10¹

29
Q

What is deci

A

d
1×10-¹

30
Q

What is centi

A

c
1×10-²

31
Q

What is milli

A

m
1×10-³

32
Q

What is micro?

A

µ
1×10-⁶

33
Q

What is nano?

A

n
1×10-⁹

34
Q

What is pico?

A

p
1×10-¹²

35
Q

Define accuracy

A

How close measurements are to a target (accepted value)

36
Q

Define precision

A

How close measurements are to one another.

37
Q

What is the equation for percent error?

A

|experimental value - accepted value|
___________________________________ ×100
accepted value

38
Q

What do significant figures indicate?

A

The precision of a measurement

39
Q

List the three rules for which digits are significant.

A
  1. Any non zero numbers
  2. Zeros between non zero numbers.
  3. Any final zeros to the right of a decimal.
40
Q

Do a place holder zeros count as significant figures?

A

NO

41
Q

If the digit to the right of the last significant figure is greater than 5 round ____

A

Up

42
Q

If the digit to the right of the last significant figure is less than 5 round _____

A

Down

43
Q

If the digit to the right of the last significant figure is equal to 5 and the next digit is nonzero round ____

A

Up

44
Q

Round ____ if the last significant figure is odd

A

Up

45
Q

Round _____ if the last significant figure is even

A

Down

46
Q

When adding or subtracting significant figures, count the number of spaces after the ______ for each value. Should match the lowest one

A

Decimal

47
Q

When multiplying or dividing significant figures, count the number of __________ for each value. Should match the lowest one.

A

Significant figures

Chemistry (10 decks)

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