1.	Convert 2374.0 g to mg.	
A)	23.740 mg	
B)	237.40 mg	
C)	2.3740 ´ 103 mg	
D)	2.3740 ´ 106 mg	

2.	Perform the following conversion:        6.47 m/s = __________ km/h	
A)	23.3 km/h	
B)	0.388 km/h	
C)	1.80 km/h	
D)	556. km/h	

3.	The number 2.00162 rounded to four significant figures is	
A)	2.002	
B)	2.001	
C)	2.000	
D)	2.162	

4.	Using the rules of significant figures, calculate the following:
6.167 + 70 =	
A)	76	
B)	80	
C)	76.167	
D)	77	

5.	Which of the following involves a chemical change?	
A)	boiling water	
B)	melting ice	
C)	chopping wood	
D)	cooking an egg	

6.	An example of a mixture is	
A)	hydrogen fluoride	
B)	purified water	
C)	gold	
D)	the air in this room	

7.	An atom that has 54 protons, 54 electrons, and 78 neutrons is	
A)		
B)		
C)		
D)		

8.	The numbers of protons, neutrons, and electrons in K+ are:	
A)	20 p, 19 n, 19 e	
B)	20 p, 19 n, 20 e	
C)	19 p, 20 n, 20 e	
D)	19 p, 20 n, 18 e	

9.	Which among the following represent a set of isotopes? Atomic nuclei containing:

 I.	
20 protons and 20 neutrons.	

II.	
21 protons and 19 neutrons.	

III.	
22 neutrons and 18 protons.	

IV.	
20 protons and 22 neutrons.	

V.	
	
21 protons and 20 neutrons.	

A)	I, II, III	
B)	III, IV	
C)	I, V	
D)	I, IV and II, V	

10.	Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.21% abundance), X-29 (28.976 amu, 4.70% abundance), and X-30 (29.974 amu, 3.09% abundance). Calculate the atomic weight of X.	
A)	28.1 amu	
B)	35.3 amu	
C)	29.1 amu	
D)	86.9 amu	

11.	How many unpaired electrons are there in an atom of sulfur in its ground state?	
A)	0	
B)	1	
C)	2	
D)	3	

12.	1s22s22p63s23p64s23d7 is the electron configuration for which of the following atoms?	
A)	Fe	
B)	Cr	
C)	Ar	
D)	Co	

13.	Choose the correct ground-state electron configuration for oxygen.	
A)	[He]2s22p4	
B)	[He]2s22p6	
C)	[Ne]2s22p4	
D)	[He]3s23p4	

14.	The electron configuration for Cr2+ is	
A)	[Ar]4s23d4	
B)	[Ar]4s13d5	
C)	[Ar]3d4	
D)	[Ar]4s23d2	

15.	Which of the following elements is most similar to chlorine?	
A)	He	
B)	Na	
C)	Hg	
D)	Br	

16.	Which of the following atoms has the largest ionization energy?	
A)	Li	
B)	Ne	
C)	Be	
D)	K	

17.	Order the elements S, Cl, and F in terms of increasing atomic radii.	
A)	Cl, F, S	
B)	F, S, Cl	
C)	F, Cl, S	
D)	S, F, Cl	

18.	Identify the trend in reactivity for metals and non metals as you go down the periodic table	
A)	metals increase, nonmetals increase	
B)	metals increase, nonmetals decrease	
C)	metals decrease, nonmetals decrease	
D)	metals decrease, nonmetals increase	

19.	What is the formula for calcium hydroxide?	
A)	CaOH	
B)	Ca(OH)2	
C)	Ca(OH)3	
D)	Ca2(OH)3	

20.	What is the formula for sulfur trioxide?	
A)	SO	
B)	SO2	
C)	SO3	
D)	S3O	

21.	The correct name for FeO is	
A)	iron oxide	
B)	iron(II) oxide	
C)	iron(III) oxide	
D)	iron monoxide	

22.	The correct name for P2O5 is	
A)	phosphorus(II) oxide	
B)	phosphorus(V) oxide	
C)	diphosphorus oxide	
D)	diphosphorus pentoxide	

23.	This molecule shows the smallest number of lone pairs in its Lewis structure.	
A)	CH3CHO	
B)	CO2	
C)	CH3Cl	
D)	C2H6	

24.	Which of the following species has a trigonal bipyramid structure?	
A)	NH3	
B)	IF5	
C)	I3–	
D)	PCl5	

25.	Which of the following molecules is polar?	
A)	BCl3	
B)	SiCl4	
C)	PCl3	
D)	Cl2	

26.	Which of the species below does not exhibit hydrogen bonding?	
A)	NH3	
B)	H2O	
C)	HF	
D)	CH4	

27.	Order the intermolecular forces (dipole-dipole, London Dispersion, ionic, and hydrogen-bonding) from weakest to strongest .	
A)	dipole-dipole, London Dispersion, ionic, and hydrogen-bonding	
B)	London Dispersion, dipole-dipole, hydrogen-bonding, ionic	
C)	hydrogen-bonding, dipole-dipole, London Dispersion, and ionic	
D)	London Dispersion, ionic, dipole-dipole, and hydrogen-bonding	

28.	When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type?

Sn + NaOH  Na2SnO2 + H2	
A)	1	
B)	2	
C)	3	
D)	4	

29.	When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type?

Al + Fe3O4  Al2O3 + Fe	
A)	1	
B)	3	
C)	6	
D)	9	

30.	CH4(g) + 2O2(g) ® CO2(g) + 2H2O(g)	
A)	single replacement	
B)	synthesis	
C)	decomposition	
D)	combustion	

31.	Zr(s) + O2(g) ® ZrO2(s)	
A)	synthesis	
B)	decomposition 	
C)	single replacement	
D)	double replacement	

32.	The equation 2Ag2O(s) ® 4Ag(s) + O2(g) is a(n) ______________ reaction.	
A)	replacement reaction	
B)	synthesis	
C)	decomposition	
D)	combustion	

33.	Zn(s) + 2HCl(aq) ® H2(g) + ZnCl2(aq)	
A)	decomposition 	
B)	single replacement	
C)	double replacement	
D)	sythesis	

34.	KBr(aq) + AgNO3(aq) ® AgBr(s) + KNO3(aq)	
A)	Combustion	
B)	Single replacement	
C)	Double replacement	
D)	Sythesis	

35.	Which of the following compounds is a product of the reaction C6H14 + O2 	
A)	H2O 	
B)	O2	
C)	H2	
D)	CO	

36.	What is the product of the following reaction? K + Cl2	
A)	KCl2	
B)	K2Cl	
C)	KCl	
D)	K2Cl2	

37.	What are the products when Magnesium Oxide decomposes? 	
A)	Mg + O	
B)	Mg + 2O	
C)	Mg + O2	
D)	2Mg + O2	

38.	Predict the products for when Iodine is combined with sodium chloride (dont worry about balancing the reaction)	
A)	NaI2 + Cl	
B)	INaCl	
C)	NaI + Cl	
D)	NaI + Cl2	

39.	Predict the products: Calcium Sulfate added to Iron (III) Phosphate yields ________	
A)	Fe2(SO4)3 + Ca3(PO4)2	
B)	Fe2SO4 + Fe2PO4	
C)	FePO4 + Ca3(PO4)2	
D)	Ca3SO4 + Ca3PO4	

Answer Key

1.	D	
2.	A	
3.	A	
4.	B	
5.	D	
6.	D	
7.	A	
8.	D	
9.	D	
10.	A	
11.	C	
12.	D	
13.	A	
14.	C	
15.	D	
16.	B	
17.	C	
18.	B	
19.	B	
20.	C	
21.	B	
22.	D	
23.	D	
24.	D	
25.	C	
26.	D	
27.	B	
28.	A	
29.	D	
30.	D	
31.	A	
32.	C	
33.	B	
34.	C	
35.	A	
36.	C	
37.	C	
38.	D	
39.	A