1 of 8
Instructor: Nicole Stevens
Chemistry 100 Exam 1
Part 1: Multiple Choice
You may write on this test, but MARK YOUR FINAL ANSWERS on a separate bubble sheet.
1.
Which of the following is a chemical property?
a. density
b. color
c. reactivity with water
d. boiling point
e. odor
f. all of these are chemical properties
2.
Which measurement below is equivalent to 15.5 kilograms?
a. 155 g
d. 0.0155 g
7
b. 1.55 x 10 mg
e. 1,550 g
5
c. 1.55 x 10 g
f. 15,500 mg
3.
Which of the following is a chemical change?
a. burning a piece of paper
b. water boiling
c. ice melting
d. wadding up a piece of paper
e. melting gold
f. pouring water from a pitcher to a cup
4.
Refer to the Periodic Table. Which of the following elements is a metalloid?
a. calcium
d. magnesium
b. aluminum
e. oxygen
c. copper
f. silicon
5.
Which of the following is true of isotopes?
a. they have the same number of protons, but different number of electrons
b. they have different numbers of protons and neutrons, but similar physical properties
c. they have the same number of neutrons, but different number of protons
d. they have the same number of protons, but different number of neutrons
e. they have the same number of neutrons, but different number of electrons
6.
Which is the correct electron configuration of a non-metal?
1
2
3
4
a. 1s 2s 3s 4s
2
2
6
2
b. 1s 2s 2p 3s
2
2
6
2
5
c. 1s 2s 2p 3s 3p
2
2
6
2
6
2
4
d. 1s 2s 2p 3s 3p 4s 3d
2
2
6
2
6
1
e. 1s 2s 2p 3s 3p 4s
7.
Which can hold the fewest electrons?
a. energy level 3
b. a "p" energy sublevel
c. energy level 2
d. a "d" energy sublevel
e. a "d" orbital
f. energy level 4
8.
What is the molar mass of magnesium bromate?
a. 134.84 g/mol
d. 264.11 g/mol
b. 104.21 g/mol
e. 280.11 g/mol
c. 152.21 g/mol
f. 83.11 g/mol
9.
What is the formula mass of strontium chlorite?
a. 222.52 g/mol
d. 222.52 amu
b. 123.07 amu
e. 123.07 g/mol
c. 155.07 g/mol
f. 171.07 amu
Winter 2008
2 of 8
Instructor: Nicole Stevens
Winter 2008
Chemistry 100 Exam 1
Part 1: Multiple Choice
MARK YOUR FINAL ANSWERS on a separate bubble sheet.
Match each of the following scientists with the scientific research they did.
10. Rutherford
a.
b.
c.
d.
e.
f.
g.
h.
i.
11. Schrodinger
12. Thomson
Wrote The Sceptical Chymist in 1661
Discovered ions, realized atoms were electrical in nature
Organized elements into the Periodic Table
Coined term "electrons" based on work with cathode-ray tubes
Law of Conservation of Mass
"Electron cloud" surrounds nucleus, region of probability
Proposed an encompassing "atomic theory"
Gold-foil experiment suggested atomic structure
Oil drop experiment calculated mass of electrons
13. How many molecules of carbon dioxide are present in 1.5 moles of carbon dioxide?
23
a. 1.5 molecule
d. 6.022 x 10 molecules
23
b. 66 molecules
e. 9.03 x 10 molecules
c. 44.01 molecules
f. impossible to tell from given information
14. Which atom produces a cation when ionized?
a. Al
b. O
c. P
d. S
e. He
f. all of the above produce anions
Match the following to its correct name.
15.
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
PO23-
16. NO3
17. Na2SO3
phosphorus dioxide
hypophosphate ion
sodium sulfate
disodium sulfate
disodium sulfur trioxide
nitrate ion
phosphite ion
sodium sulfite
hypophosphite ion
nitrogen trioxide
Match the following to its correct formula.
18. Nickel (II) chloride
a. Mg3PO2
b. Ni2Cl
19. Magnesium phosphide
c.
20. Aluminum hyponitrite
d. Mg3P2
e. Al(NO)3
Al3(NO2)
21. What is the correct formula for ammonium carbonite?
a. (NH3)2CO2
d. Am2CO2
b.
(NH4)2CO2
c.
(NH3)2CO3
e. Al2CO2
f. Al2(CO2)3
f.
NiCl2
g. Ni2ClO2
h. Mg2P3
i.
AlN3
j.
AlNO3
g. NH4CO2
h. NH3CO2
i.
NH4CO4
3 of 8
Instructor: Nicole Stevens
Winter 2008
Chemistry 100 Exam 1
Part 1: Multiple Choice
You may write on this test, but MARK YOUR FINAL ANSWERS on a separate bubble sheet.
22. A linear VSEPR molecular shape is characteristic of which of the following?
SO22A.
H2O
B.
SO2
C.
a. A
b. B
c. C
d. D
-
NO2
D.
CO2
E.
e.
f.
g.
h.
E
A and C
A and D
A, B and D
i.
j.
C and E
all of the above
23. What is the term that means an an average of all an element's isotopes?
a. polarity
d. molecular shape
b. mass number
e. electronegativity
c. atomic number
f. atomic mass
24. A chlorine atom has gained one electron. Which of the following is NOT true about the atom now?
a. it is an anion
d. it has the same electron configuration as argon
b. its mass number increases
e. it would be attracted to positive ions and form ionic bonds
c. it carries a -1 charge
f. all of the above are true
25. Sodium reacts with chlorine gas to form table salt (sodium chloride). In the balanced equation, what are the
coefficients in front of sodium and chlorine gas, respectively?
a. 3 and 3
d. 3 and 2
b. 2 and 3
e. 3 and 1
c. 2 and 1
f. 1 and 1
Indicate whether the following statements are true or false.
a.
b.
TRUE
FALSE
26. The subscripts in a molecular formula represent proportions or ratios of moles.
27. One mole of water contains the same number of molecules as one mole of carbon dioxide.
28. An s-orbital in energy level 1 has both the same shape and the same volume as an s-orbital in energy level 3.
29. Alkaline earth metals react more vigorously with water than alkali metals.
30. p-orbitals are dumbell shaped, while s-orbitals are spherical.
4 of 8
Instructor: Nicole Stevens
Winter 2008
Name
Chemistry 100 Exam 1
Part 2 : Write-on
Please write your answers clearly in the space provided. SHOW ALL WORK!
I.
Write the full electron configuration for each of the following elements in order of how the orbitals fill.
a.
Copper
b.
Krypton
II.
If a piece of aluminum has a density of 1.73g/mL and a volume of 8.75mL, what is its mass?
(Answer to 2 decimal places)
III.
Convert each of the following measurements into kilometers:
a.
b.
IV.
1.75 x 109 mm
1.45 m
Write each of the following in scientific notation:
a.
564,000
b.
0.000523
The chemical symbol of the following elements is represented by "X". Refer to the following figures
for questions V - VII.
46
23
X
a.
46
22
X
b.
47
22
X
c.
V.
Which of the above figures are isotopes of each other?
VI.
Which of the above figures have the same number of neutrons?
VII. Figure (b) represents which element from the Periodic Table?
46
21
X
d.
48
24
X
e.
Instructor: Nicole Stevens
5 of 8
Winter 2008
Name
Chemistry 100 Exam 1
Part 2 : Write-on
Please write your answers clearly in the space provided. SHOW ALL WORK!
VIII. Consider a molecule of nitrogen trihydride (ammonia).
a. Draw the complete electron-dot configuration of nitrogen trihydride.
IX.
b.
What is the VSEPR molecular shape of this molecule?
c.
What is the intramolecular force for this molecule?
d.
What is the intermolecular force for this molecule?
e.
What state of matter is this compound most likely to be?
Perform the following "Roadmap" calculations: (Answers to 2 decimal places)
a.
How many grams of chromium are present in a sample that contains 3.25 x 1021 Cr atoms?
b.
How many atoms of oxygen are present in 96.4g of aluminum sulfate?
c.
How many grams of phosphorus are present in 49.7g of magnesium phosphite?
6 of 8
Instructor: Nicole Stevens
Winter 2008
Name
Chemistry 100 Exam 1
Part 2 : Write-on
Please write your answers clearly in the space provided. SHOW ALL WORK!
X.
Dihydrogen sulfide reacts with iron (III) perchlorate to form iron (III) sulfide and hydrogen perchlorate.
BONUS!!
a.
Write the balanced equation.
b.
If I begin with 32.0g of iron (III) perchlorate, how many grams of hydrogen perchlorate will form?
(Answer to 2 decimal places)
c.
If I want to form 60.0g of iron (III) sulfide, how many grams of dihydrogen sulfide to I need to react?
(Answer to 2 decimal places)
d.
What state of matter is the dihydrogen sulfide most likely to be?
How can you tell?
e.
What state of matter is the iron (III) sulfide most likely to be?
How can you tell?
Instructor: Nicole Stevens
7 of 8
Winter 2008
Chemistry 100 Exam 1
Roadmap to Chemistry Mass
Calculations
Grams of
element
Grams of
compound A
Grams of
compound B
Molar mass
of element
(g/mol)
Molar mass of
compound A
Molar mass of
compound B
Moles of
element
Subscripts
in formula
Moles of
compound
A
Avogadro’s
number of
atoms or ions
Avogadro’s
number of
molecules
Atoms or
Ions
Molecules
Atomic mass
(amu / atom)
Formula
mass (amu /
molecule)
Amu of
element
Amu of
compound
Coefficients in
balanced
equation
Moles of
compound
B