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Chemistry I Test I Review

Total questions: 44

Worksheet time: 54mins

Name
Class
Date
1.

Complete the following sentence. A theory is

a)

a statement describing a relationship between phenomena that is always the same under the same conditions.

b)

a tentative explanation for a set of observations that can be tested by further experimentation.

c)

a unifying principle that explains a body of facts and relations.

d)

a model used to visualize the invisible.

2.

Which of the following is an example of a physical property?

a)

corrosiveness of sulfuric acid

b)

toxicity of cyanide

c)

flammability of gasoline

d)

neutralization of stomach acid with an antacid

e)

lead becomes a liquid when heated to 601oC

3.

A microliter corresponds to:

a)

10–2 liters.

b)

10–3 liters.

c)

10–6 liters.

d)

10–9 liters.

e)

10–12 liters.

4.

2.4 km is how many millimeters?

a)

2,400 mm

b)

2.4 x 104 mm

c)

2.4 x 105 mm

d)

2.4 x 106 mm

e)

2.4 x 10–5 mm

5.

The element gallium melts at 29.8°C. What temperature is this in °F?

a)

–54.1°F

b)

–7.8°F

c)

+85.6°F

d)

+51.3°F

e)

+13.5°F

6.

Liquid nitrogen boils at –195.8°C. Express the boiling point of liquid nitrogen in kelvin.

a)

–469.0 K

b)

–77.4 K

c)

all temperatures are 0 K on the Kelvin scale

d)

77.4 K

e)

469.0 K

7.

The number 1.050 x 109 has how many significant figures?

a)

2

b)

3

c)

4

d)

9

e)

13

8.

After carrying out the following operations, how many significant figures are appropriate to show in the result?
            (13.7+0.027)÷8.221\left(13.7+0.027\right)\div8.221  

a)

1

b)

2

c)

3

d)

4

e)

5

9.

A piece of metal with a mass of 611 g is placed into a graduated cylinder that contains 25.1 mL of water, raising the water level to 56.7 mL. What is the density of the metal?

a)

19.3 g/cm3

b)

10.5 g/cm3

c)

8.96 g/cm3

d)

7.13 g/cm3

e)

2.70 g/cm3

10.

The density of lead is 11.4 g/cm3 at 25°C. Calculate the volume occupied by 25.0 g of lead.

a)

6.05 cm3

b)

2.19 cm3

c)

0.456 cm3

d)

285 cm3

e)

1.24 cm3

11.

Radio waves travel at the speed of light, which is 3.00 x 108 m/s. How many minutes does it take for a radio message to reach Earth from Saturn if Saturn is 7.9 x 108 km from Earth?

a)

4.4 x 10-2 min

b)

1.6 x 105 min

c)

4.0 x 1015 min

d)

44 min

e)

2.6 min

12.

Which of the following elements is most likely to be a good conductor of electricity?

a)

N

b)

S

c)

He

d)

Cl

e)

Fe

13.

Which of the following scientists developed the nuclear model of the atom?

a)

John Dalton

b)

Robert Millikan

c)

J. J. Thomson

d)

Henry Moseley

e)

Ernest Rutherformd

14.

How many neutrons are there in an atom of uranium whose mass number is 235?

a)

92

b)

143

c)

235

d)

238

e)

327

15.

An atom of the isotope chlorine-37 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)

a)

17 p, 18.45 n, 17 e

b)

17 p, 20 n, 7 e

c)

17 p, 20 n, 17 e

d)

17 p, 37 n, 17 e

e)

20 p, 17 n, 20 e

16.

Which one of the following elements is most likely to form a 2– ion?

a)

scandium

b)

selenium

c)

silicon

d)

strontium

e)

iodide

17.

Two isotopes of an element differ in their

a)

symbol

b)

atomic number

c)

atomic mass

d)

number of protons

e)

number of electrons

18.

Name the binary compound formed between barium and phosphorus.

a)

barium phosphorus

b)

barium phosphide

c)

barium phosphate

d)

barium diphosphate

e)

barium triphosphide

19.

Which is the correct formula for copper(II) phosphate?

a)

Cu2PO4

b)

Cu2PO3

c)

Cu(PO4)2

d)

Cu3(PO4)2

e)

Cu(PO3)2

20.

The correct name for NH4NO3 is

a)

ammonium nitrate

b)

ammonium nitrogen trioxide

c)

ammonia nitrogen oxide

d)

hydrogen nitrogen oxide

e)

hydrogen nitrate

21.

The element oxygen consists of three naturally occuring isotopes: 16O, 17O, and 18O. The atomic mass of oxygen is 16.0 amu. What can be implied about the relative abundances of these isotopes?

a)

More than 50% of all O atoms are 17O.

b)

Almost all O atoms are 18O.

c)

Almost all O atoms are 17O.

d)

The isotopes all have the same abundance, i.e. 33.3%.

e)

The abundances of 17O and 18O are very small.

22.

If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of g/mol?

a)

228 g/mol

b)

17.1 g/mol

c)

4.38 g/mol

d)

217 g/mol

23.

Which one of the following does not represent 1.00 mol of the indicated substance?

a)

6.02 x 1023 C atoms

b)

26.0 g Fe

c)

12.01 g C

d)

65.4 g Zn

e)

6.02 x 1023 Fe atoms

24.

Determine the number of moles of aluminum in 96.7 g of Al.

a)

0.279 mol

b)

3.58 mol

c)

7.43 mol

d)

4.21 mol

e)

6.02 x 1023 mol

25.

Which of the following samples contains the greatest number of atoms?

a)

100 g of Pb

b)

2.0 mole of Ar

c)

0.1 mole of Fe

d)

5 g of He

e)

20 million O2 molecules

26.

What is the molar mass of acetaminophen, C8H9NO2?

a)

43 g/mol

b)

76 g/mol

c)

151 g/mol

d)

162 g/mol

e)

125 g/mol

27.

The molecular formula of aspirin is C9H8O4. How many aspirin molecules are present in one 500-milligram tablet?

a)

2.77 molecules

b)

2.77 x 10-3 molecules

c)

1.67 x 1024 molecules

d)

1.67 x 1021 molecules

28.

As the frequency of an electromagnetic wave increases

a)

its speed must increase.

b)

its wavelength must increase.

c)

its amplitude must increase.

d)

its energy must increase.

29.

Complete this sentence: Atoms emit visible and ultraviolet light

a)

as electrons jump from lower energy levels to higher levels.

b)

as the atoms condense from a gas to a liquid.

c)

as electrons jump from higher energy levels to lower levels.

d)

as they are heated and the solid melts to form a liquid.

e)

as the electrons move about the atom within an orbit.

30.

Which one of the these sets of quantum numbers is not possible?

a)

A

b)

B

c)

C

d)

D

e)

E

31.

Electrons in an orbital with l = 3 are in a/an

a)

d orbital

b)

f orbital

c)

g orbital

d)

p orbital

e)

s orbital

32.

Which ground-state atom has an electron configuration described by this orbital diagram?

a)

phosphorus

b)

nitrogen

c)

arsenic

d)

vanadium

e)

none of these

33.

Which element has the following ground-state electron configuration?

[Ar]4s23d104p5

a)

arsenic

b)

bromine

c)

iodine

d)

selenium

34.

Which one of the following elements is a transition element?

a)

antimony

b)

barium

c)

chromium

d)

potassium

e)

selenium

35.

How many valence electrons does an oxygen atom have?

a)

2

b)

4

c)

6

d)

7

e)

8

36.

What is the charge on the monatomic ion that calcium forms in its compounds?

a)

+2

b)

+1

c)

-1

d)

-2

e)

-3

37.

How many 3d electrons does an Fe3+ ion have?

a)

9

b)

6

c)

5

d)

4

e)

3

38.

Which of the atoms listed below has the largest radius?

a)

Cl

b)

I

c)

P

d)

Sb

e)

Se

39.

Which of the elements listed below has the highest first ionization energy?

a)

C

b)

Ge

c)

P

d)

O

e)

Se

40.

What type of chemical bond holds the atoms together within a water molecule?

a)

ionic bond

b)

polar covalent bond

c)

nonpolar covalent bond

d)

coordinate covalent bond

41.

The Lewis structure for AsCl3 shows

a)

a total of 84 electrons

b)

three single bonds and 10 lone pairs

c)

two single bonds, one double bond and 9 lone pairs

d)

one single bond, two double bonds, and 8 lone pairs

e)

three single bonds and one lone pair

42.

Which of the following Lewis structures is incorrect?

a)
b)
c)
d)
e)
43.

What is the formal charge on the sulfur in the best Lewis structure for the SCN- (thiocyanate) ion?

a)

+2

b)

-2

c)

+1

d)

-1

e)

0

44.

Which one of the following compounds does not follow the octet rule?

a)

NF3

b)

CF4

c)

PF5

d)

ASH3

e)

HCl

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