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Assignment 1. Questions from chapters 1 and 2 of McMurry and Fay
Question numbers are from the fourth edition.
Chapter 1. Chemistry: Matter and Measurement
1.1
(a)
Cd (b)
Sb
(c)
Am
1.2
(a)
silver
(b)
rhodium
(c)
rhenium
(d)
cesium
(e)
argon
(f)
arsenic
1.3
(a)
Ti, metal
(b)
Te, semimetal
(c)
Se, nonmetal
(d)
Sc, metal
(e)
At, semimetal
(f)
Ar, nonmetal
1.4
The three
A
coinage metals
@
are copper (Cu), silver (Ag), and gold (Au).
1.5
(a)
The decimal point must be shifted ten places to the right so the exponent is
S
10.
The
result is 3.72 x 10
S
10
m.
(b)
The decimal point must be shifted eleven places to the left so the exponent is 11.
The
result is 1.5 x 10
11
m.
1.6
(a)
microgram
(b)
decimeter
(c)
picosecond
(d)
kiloampere
(e)
millimole
1.7
o
o
o
5
5
C =
x
F _ 32) =
x (98.6 _ 32) =
C
(
37.0
9
9
o
K =
C + 273.15 = 37.0 + 273.15 = 310.2 K
1.8
(a)
K =
o
C + 273.15 =
S
78 + 273.15 = 195.15 K = 195 K
(b)
o
o
o
o
9
9
F = ( x
C) + 32 = ( x 158) + 32 =
F =
F
316.4
316
5
5
(c)
o
C = K
S
273.15 = 375
S
273.15 = 101.85
o
C = 102
o
C
o
o
o
o
9
9
F = ( x
C) + 32 = ( x 101.85) + 32 =
F =
F
215.33
215
5
5
1.9
3
3
m
27.43
g
d =
=
= 2.212
g/
cm
V
12.40
cm
1.10
1
mL
volume = 9.37
g x
= 6.32
mL
1.483
g
1.11
The actual mass of the bottle and the acetone = 38.0015 g + 0.7791 g = 38.7806 g.
The
measured values are 38.7798 g, 38.7795 g, and 38.7801 g.
These values are both close to
each other and close to the actual mass.
Therefore the results are both precise and
accurate.
1.12
(a)
76.600 kg has 5 significant figures because zeros at the end of a number and after the
decimal point are always significant.
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4.502 00 x 10
3
g has 6 significant figures because zeros in the middle of a number
are significant and zeros at the end of a number and after the decimal point are always
significant.
(c)
3000 nm has 1, 2, 3, or 4 significant figures because zeros at the end of a number and
before the decimal point may or may not be significant.
(d)
0.003 00 mL has 3 significant figures because zeros at the beginning of a number are
not significant and zeros at the end of a number and after the decimal point are always
significant.
(e)
18 students has an infinite number of significant figures since this is an exact
number.
(f)
3 x 10
S
5
g has 1 significant figure.
(g)
47.60 mL has 4 significant figures because a zero at the end of a number and after
the decimal point is always significant.
(h)
2070 mi has 3 or 4 significant figures because a zero in the middle of a number is
significant and a zero at the end of a number and before the decimal point may or may
not be significant.
1.13
(a)
Since the digit to be dropped (the second 4) is less than 5, round down.
The result is
3.774 L.
(b)
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 Fall '07
 SCHMIDT
 Chemistry, Atom, Orders of magnitude, 15.9994 amu

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