Chapter 3 Prentice Hall

Front 1

measurement

Back 1

a number and a unit
(what you know plus an estimated digit)

Front 2

Accuracy

Back 2

measure of how close a measurement comes to the actual or true value of whatever is measured

Front 3

Precision

Back 3

measure of how close a series of measurements are to one another

Front 4

Error

Back 4

what you get minus what you should have got

Front 5

Measurements and Their Uncertainty

Back 5

1) All nonzero numbers are significant
2) Zeroes found between significant figures are significant
3) Terminal zero is significant (zero in the last position to the right of the decimal point.

Front 6

87.073 meters
(round)

Back 6

87.1 meters = 8.71 x 10 (3rd)

Front 7

8792 meters
(round)

Back 7

8800m

Front 8

1.2349
(round)

Back 8

1.23

Front 9

How many sig fig does
1.2 x 10(3) have?

Back 9

2
(look at the coefficient and that tells you)

Front 10

scientific notation

Back 10

a given number written as th product of two numbers: a coefficient and 10 raised to a power

Front 11

scientific notation
(when multiplying/dividing)

Back 11

add exponents(multiply)
subtract exponents (divide)

Front 12

accuracy (to evaluate)

Back 12

to evaluate the accuracy the measurement must be compared to the correct value & to evaluate the precision of a measurement you must compare the values of 2 or more repeated measurements

Front 13

accepted value

Back 13

correct value based on reliable references

Front 14

experimental value

Back 14

value measured in a lab

erro= experimental value - accepted value

Front 15

percent error

Back 15

absolute value of error divided by the accepted value and multipied by 100

Front 16

Why must measurements be reported to the correct number of significant figures?

Back 16

Significant figures in measurements are
the certain values and the estimated value.

Front 17

significant figures

Back 17

include all of the digits that are known, plus a last digit that is estimated

Front 18

How does the precision of a calculated answer compare to the precision of the measurements used to obtain it?

Back 18

In general, a calculated answer cannot be more precise than the least precise measurement from which it was calculated.
The calculated value must be rounded to make it consistent with the measurements from which it was calculated.

Front 19

Energy

Back 19

capacity to do work or generate heat

Front 20

Water freezes at...

Back 20

32degress Fahrenheit
0degrees Celsius
273 Kelvin

Front 21

Water boils at..

Back 21

212degrees Fahrenheit
100degrees Celsius
373Kelvin
(0degrees Kelvin= absolute zero- when all motion in a particle stops)

Front 22

Which five SI base units do chemists commonly use?
(SI revised version of the metric system)

Back 22

meter, the kilogram, the kelvin, the second, and the mole

Front 23

What metric units are commonly used to measure length?

Back 23

Common metric units of length include the centimeter, meter, and kilometer

Front 24

What metric units are commonly used to measure volume?

Back 24

Common metric units of volume include the liter(non SI cubicmeter), milliliter, cubic centimeter, and microliter.

Front 25

What metric units are commonly used to measure mass?

Back 25

Common metric units of mass include kilogram, gram, milligram, and microgram.

Front 26

Weight

Back 26

a force that measures the pull on a given mass by gravity

Front 27

Temperature

Back 27

a measure of how hot or cold an object is

Front 28

How do you convert from celsius to kelvin?

Back 28

add or subtract 273
k= c + 273
c= k - 273

Front 29

common units of energy

Back 29

joule- the SI unit of energy and
calorie- the quantity of heat that raises the temperature of 1 g of pure water by 1°C.

Front 30

mole
(mole day celebrated oct 23)

Back 30

A mole is the quantity of anything that has the same number of particles found in 12.000 grams of carbon-12

Front 31

What happens when a measurement is multiplied by a conversion factor?

Back 31

When a measurement is multiplied by a conversion factor, the numerical value is generally changed, but the actual size of the quantity measured remains the same.

Front 32

Why is dimensional analysis useful?

Back 32

Dimensional analysis is a way to analyze and solve problems using the units, or dimensions, of the measurements.
(alternative approach to problem solving)

Front 33

What types of problems are easily solved by using dimensional analysis?

Back 33

Problems in which a measurement with one unit is converted to an equivalent measurement with another unit are easily solved using dimensional analysis.

Front 34

What determines the density of a substance?
(density = m/v)

Back 34

Density is an intensive property that depends only on the composition of a substance, not on the size of the sample.

Front 35

How does a change in temperature affect density?

Back 35

The density of a substance generally decreases as its temperature increases.