The document provides examples of different types of measurement scales including triple beam balances, graduated cylinders, thermometers, and scales for scientific notation, significant figures, and temperature conversion. It asks the reader to determine measurements or values indicated by each example and to perform conversions between units like Celsius, Kelvin, and Fahrenheit.

1. Name _
THE TRIPLE AND FOUR
BEAM BALANCES
What masses are shown on each of the following balances?
Triple Beam Balance
0 10 Q() 30 40 50 60 70 aD gO 100
~
600 800 qoo
Answer:
,j I . ,(
0 2. :3 5 6 7 8 '1 10
0 10 20 30 40 50 60 70 ao qO 100
100 2.00 300 "l00 500 600 700 800 qoo 1000
Answer: °
0 2. 3 4 5 7 B q (0
y--y---y----y--
0 10 2.0 ~o ""0 50 60 70 BO qo 100
0 100 2.00 2100 400 500 600 700 800 1000
Answer:
0 "3 4 5 6 7 8 10
Four Beam Balance 0 100 200
0 0 20 30 40 50 60 70 80 gO 100
Answer: 0 2 3 4 5 6 7 8 'I 10
0 0.1 0,2 0,3 0,4- 0,5 0,6 0,7 0.8 0.'1 1.0
,~
;;
<
,:;:;
0 10 20 30 40 60 70 BO roo
0 2. 3 4 5 6 7 8J q 10
Answer:
I I !IIII mill 111111 1111 I I I1l!llIlllllllllm9m 1llllHllll,lll II III
1111 rI1lTfTll11iTITl11
0 0.1 0.2 0.3 0.4 0,5 0.6 0.7 o.e 0.<1 LO
~.
100 200
0
0 10 2.0 30 40 50 60 70 80 qO 100
.,
Answer: 0 2- 3 4 5 6 7 8 q 10
,-;!
'i':
-~::,
~
0 O. 0.2. 0.3 0.4- 0.5 0.7 o.B o.q 1.0 -~f_
!]
Chemistry IF8766 3 ©Instructional Fair, Inc.

2. Name _
MEASURING LIQUID VOLUME
What volume is indicated on each of the graduated cylinders below? The unit of vole
is mL.
60
4 I
50 2S
'3
I
a) b) c)
I
251
I 80
:-;
2.0
is/
75
70
r
I ---
4
3
10 65
1
ct) e) f)
I
I I
I
40 1
30 3
20 2.
I
fa f 40
J ---
g) h) f)
Chemistry IF8766 4 ©Instructionc
_ .. _ ._. ___ ••. __ ,_ •. ___ .,_ •• _._"" ____ ~,. ___ • __ , __ '._ .• ____ •. _._ .• _ •• w. ___ , _____ ·___ ~ _____ ~·_· ___ •· __ ~·_·

3. Name _
READING THERMOMETERS
What temperature isindicated on each of the thermometers below?
10 2.0
5
o - .•...
-10
-10 - ..•..
-0

4. Name _
SCIENTIFIC NOTATION
Scientists very often deal with very small and very large numbers, which can lead to a lot 0
confusion when counting zeros! We have learned to express these numbers as powers of 10
Scientific notation takes the form of M x lon where 1 -::;M < 10 and "n" represents the number
of decimal piaces to be moved. Positive n indicates the standard form is a large number.
Negative nindicates a number between zero and one.
Example 1: Convert 1,500,000 to scientific notation.
We move the decimal point so that there is only
one digit to its left, a total of 6 places.
1,500,000 = 1.5 x 106
Example 2: Convert 0.000025 to scientific notation.
For this, we move the decimal point 5 places to the
right.
0.000025 =
2.5 x 10-5
(Note that when a number starts out less than one,
the exponent is always negative.)
Convert the following to scientific notation.
1 . 0.005 = 6. 0.25 ::
2. 5,050 = 7. 0.025 =
3. 0.0008 = 8. 0.0025 =
4. 1,000 = 9. 500 =
t;
v. 1,000,000 == 10. 5,000 =
Convert the following to standard notation.
1. 1.5 x 103= _ 6. 3.35 X 10-1 ;:
2. 1.5 X 10-3 ;: _ 7. 1.2 X 10-4 ;:
3. 3.75 X 10-2 ;: _ 8. 1x lQ4 ::
4. 3.75 X 102 =: ~_ 9. 1 X 10-1 ==
5. 2.2x lOS = __ ~ _ 10. 4x 10° .-
Chemistry' IF8766 8 ©Instructionai Fair, i"e
- - ~ i'

5. Name _
SIGNIFICANT FIGURES
)f
A measurement can only be as accurate and precise as the instrument that produced it.
A scientist must be able to express the accuracy of a number, not just its numerical value.
10.
We can determine the accuracy of a number by the number of significant figures it
er contains.
1) All digits 1-9inclusive are significant.
Example: 129has 3 significant figures.
2) Zeros between significant digits are always significant.
Example: 5,007 has 4 significant figures.
3) Trailing zeros in a number are significant only if the
number contains a decimal point.
Example: 100.0has 4 significant figures.
I 100has 1 significant figure.
I 4) Zeros in the beginning of a number whose only function
ls to place the decimal point are not significant.
Example: 0.0025 has 2 significant figures.
5) Zeros following a decimal significant figure are
significant.
Example: 0.000470 has 3 significant figures.
0.47000 has 5 significant figures.
Determine the number of significant figures in the foilowing numbers.
i. 0.02 6. 5,000.
2. 0.020 7. 6,051.00
3, 501 B. 0.0005
4. 501.0 9. 0.1020
5. 5,000 10. 10,001
Determine the location of the last significant place value by placing a bar over the digit.
(Example: 1.700)
1, 8040 6. 90,100
2, 0,0300 7. 4.7 x 10-8
3, 699.5 8. 10,800,000.
4, 2,000 x 102 9, 3.01 x 1021
5. 0.90100 10. 0.000410
Chemistry IF8766 9 ©Instructional Fair, Inc.

6. l TEMPERATURE AND Name _
ITS MEASUREMENT
Temperature (which measures average kinetic energy of the molecules) can be
measured using three common scales: Celsius,Kelvin and Fahrenheit We use the
following formulas to convert from one scale to another. Celsius isthe scale most
desirable for laboratory work. Kelvin represents the absolute scale. Fahrenheit isthe old
Englishscale which isnever used in lab.
°C ::: K - 273 K :::°C + 273
of::: 9/50C + 32°C::: 5/geF - 32)
Complete the following chart. All measurements are good to 1° C or better.
--------------~-----~4-5-0-K-----~--------------1
_______
. 4- -+ 9_8_,6_0_F lll
-273° C .
294K
225 K
Chemistry IF8766 12 ©Instructionol