Review Pre-AP Chemistry Unit 1: Matter & Measurement
[KEY]
1.
Express 580,000 in scientific notation. ___5.8 x 105_______
2.
Express 2.03 x 106 in standard notation. ___2,030,000_________
3.
Express 0.000 000 320 in scientific notation. _____3.20 x 10–7___________
4.
Express 4.1 x 10–4 in standard notation. ___0.00041_____________
5.
Define accuracy: ___how close a measurement is to the true value________________.
6.
Define precision: ___how close measurements are to each other (consistency)____________.
7.
Six different people weigh a standard mass of 5.00 g on the same balance. Each person obtains a
reading of 2.50 g for the mass of the standard. Describe the accuracy and precision of the balance based
on these results.
Is the balance accurate? _N_
Is the balance precise? __Y__
Explain: __The measurements were consistently close to each other (precise), but not close to the true
value (not accurate).
8.
These values were recorded as the mass of products when the same chemical reaction was carried out
three separate times: 3.20 g; 2.87 g; 3.89 g.
The correct mass of products from that reaction was actually 3.45 g.
Are the measured masses accurate? _N__
Are the measured masses precise? _N__
Explain: _ The measurements were not consistently close to each other (not precise), and the average
(3.32) was not close to the true value (not accurate)_
9.
Record a valid measurement for the length of the metal strip with one digit of uncertainty: 4.40 cm
Which digit in a measurement is always the uncertain digit? _the last digit________________
What does the uncertain digit represent? __an estimate for one tenth of the smallest marks___
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10.
How many significant figures are in each of the following measurements?
0.0100 kg
__3__
11.
2000 m
__1__
30.50 g
__4__
0.0003 mL
__1__
How many zeroes are significant in 10.0020300? __6__
How many zeroes are significant in 0.0000400? __2__
12.
13.
Round each of the following measurements to the stated number of significant figures.
20.09 to three sig figs.
___20.1____
0.00045 to one sig fig.
__0.0005___
26.98 to three sig figs.
___27.0____
Complete the operation and round your answer to the correct number of significant figures.
a) 3.28 + 1.2 = __4.5___ (keep fewest decimal places)
b) 84.4 ÷ 4.0 = __21_____ (keep fewest sig figs)
c) 6000 ÷ 8.0 = __800___ (keep fewest sig figs)
d) 21 – 2.0 x 2.00 = ___17____
first… (2.0 x 2.00) = 4.0 (keep fewest sig figs)…
then… 21 – 4.0 = 17 (keep fewest decimal places)
14.
List the base unit and symbol for:
Length: _meter (m)_
15.
Mass: _gram (g)___
Volume: __liter (L)___
Rewrite the metric prefixes in order from largest to smallest.
deci- (d)
milli- (m)
kilo- (k)
largest
kilo- (k)
16.
centi- (c)
smallest
deci- (d)
centi- (c)
milli- (m)
Order the following masses from smallest to largest.
cg
mg
kg
smallest
__mg___
dg
largest
__cg___
__dg___
__kg___
2
17.
What is the quantity 65.5 m expressed in cm? ____6550 cm________
18.
Convert 2.3 mL into L. _____0.0023 L___________
19.
1 m is equal to __100___ cm.
20.
Which of the following steps in the scientific process did the scientist neglect to perform?
A.
B.
C.
D.
E.
21.
observation
question
hypothesis
experiment
conclusion
Which of the following questions is a scientific question that can be answered by observation and
experimentation?
A.
B.
C.
D.
Should scientists perform drug tests on animals?
Does the weight of an object change when measured at different heights?
Is water more useful as a liquid or as a gas?
Is the ozone layer the most important environmental issue today?
22.
Mass of solid (g)
Pressure (atm)
Volume of gas (mL)
50.0
1.00
83.0
20.0
1.00
34.7
10.0
1.00
18.3
5.0
1.00
8.9
50.0
76.50
23.8
23.
What is the independent variable in the above experiment? mass of solid
(manipulated, tested, etc.)
24.
What is the dependent variable in above experiment? volume of gas
(measured amount depended on amount of solid used)
25.
What is the controlled variable in above experiment? __pressure____
Explain: __The pressure was held constant and did not change (controlled)_______
26.
Describe a procedure for how the student can find the mass of the powder.
1) Mass the empty plastic weighing dish with the triple-beam balance.
2) Place the sulfur powder in the dish with the scoopula and mass the dish again.
3) Subtract the two masses to determine the mass of just the sulfur without the dish.
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27.
A student completed an experiment measuring the mass and volume of a solid.
The student plotted four data points on a graph of Mass vs. Volume shown below:
M
V
What property does the slope of the best fit line represent about the solid: _density__
(slope = rise/run = M/V)
28.
Write the equation for calculating density in this box:
29.
The mass of a soft lump of metal is 214 g, and the volume is 11.3 cm3.
What is the density of the metal in g/cm3 ? (SHOW WORK)
Table 1
Density of various metals
d = (214) = 18.9 g/cm3
Metal
Density
(11.3)
3
Using Table 1, identify of the metal: __gold_
Aluminum
Iron
Gold
Platinum
(in g/cm )
2.7
7.9
19.3
21.4
The soft metal lump is then smushed together with another lump of the exact same soft metal.
The density of the new larger lump is greater than / equal to / less than the original lump.
30.
What is the volume of 36.0 g of air if the density of air is 0.0012 g/mL? (SHOW WORK)
d = m
V
31.
V = 36.0
0.0012
.
V = 30,000 mL (or 30 L)
or 3.0 x 104 mL (with 2 sig figs)
A sample of lead has a density of 11.4 g/cm3 and a volume of 8.00 cm3.
What is its mass? (SHOW WORK)
d = m
V
32.
0.0012 = (36.0)
V
11.4 = m
8.00
m = 11.4 x 8.00
m = 91.2 g (with 3 sig figs)
The density of a plastic is 0.95 g/mL. Place a check next to each liquid in which it will sink.
Water (d = 1.0 g/mL)
___ (will float)
10W30 Motor Oil (d = 0.89 g/mL)
_X_ (will sink)
Corn Syrup (d = 1.35 g/mL)
___ (will float)
Gasoline (d = 0.66 g/mL)
_X_ (will sink)
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33.
Describe what happens when 2 g of aluminum (density = 2.70 g/cm3) is placed in 100 g of water.
It will _sink___ because it is __more dense____ than water.
34.
Which of these statements about density is FALSE?
A.
B.
C.
D.
Different size samples of the same substance have the same density.
Lighter objects are less dense.
Density depends only on the substance, not the amount of it.
The density of an object depends on mass and volume, not weight and volume.
35. mass and volume
36. a, b, d, e, g, h, i
37. solids: definite volume, definite shape, particles vibrate in place (moving a little), not compressible
liquids: definite volume, indefinite shape, particles are close together but can move past each other,
(moving a little), not easily compressible
gases: indefinite volume, indefinite shape, takes the shape of its container, particles are very far apart,
(moving a lot), easily compressible
plasma: indefinite volume, indefinite shape, occurs only at extremely high temperatures. Most electrons have
been stripped away creating ionized matter. (moving a whole lot!)
38.
a. element
b. mixture
c. compound
d. element
39. diagrams 1,3,4 …because each particle is identical.
40. a. heterogeneous mixture
g. heterogeneous mixture
b. homogeneous mixture
h. compound
c. homogeneous mixture
i. compound
d. element
j. compound
e. element
k. compound
f. homogeneous mixture
41. d, e, h, i, j, k
42. density
43. chemical properties: b, c
44.
D. heterogeneous
physical properties: a, d, e
B. compound
A. element
C. homogeneous
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