Module 3 DBA & Exam Review 
This review is neither a replica of the exam nor does it contain every concept in the module.  It is always best practice to review all lessons and assessments and ensure you have your comprehensive notes. Resubmitting is a great way to review/learn and improve your grade.   In this review, questions 1 – 32 are the general topics for the multiple choice type questions on the module exam; questions 33-35 are covered as an essay on the exam. Questions 36-40 are the honors extension questions. The number in parenthesis is the corresponding lesson. Please contact your instructor with any questions (Answer key)
Segment 1 Formula Sheet - Google Copy
Segment 1 Formula Sheet - RTF download

Needed for next module: 
Module 4 Overview "Cheat Sheet" (Google Doc)
Module 4 Overview "Cheat Sheet" (RTF download)

●	Module 3 Regular Exam: There are 18 questions on the actual exam
○	16 multiple choice and 2 essay/free responses.
●	Module 3 Honors Exam: There are 21 questions on the actual exam
○	19 multiple choice and 2 essay/free responses.

Multiple Choice format questions:

1.	Which of the following atoms has 3 valence electrons?  (3.01)
a.	Aluminum   		c. 	Carbon
b.	Nitrogen		d. 	Xenon

2.	There are two atoms: A and B.  Atom A has 7 electrons and atom B has 13 electrons. Which of the following is true? (3.01)
a.	Atom A is more reactive than atom B
b.	Atom B will give up electrons to form bonds
c.	Both atoms will gain electrons to become stable
d.	Neither atom is reactive

3.	An atom has an electron configuration of: 1s22s22p63s23p64s2.  Which of the following is not true?  (3.01)
a.	The element is located in group 4
b.	The element is reactive
c.	The element has 2 valence electrons
d.	This element is a metal

4.	What is the correct formula for potassium chlorate?  (3.02)
a.	PClO3				c.	KClO3	
b.	PCl				d.	K(ClO3)2

5.	What is the correct formula when aluminum bonds with hydroxide? (3.02)
a.	AlOH33			c.  OH3Al
b.	Al(OH)3			d.  Al(OH)2

6.	What is the correct name for Pb3(PO4)2? (3.02)
a.	Lead phosphide		c.	Lead phosphate	
b.	Lead (II) phosphate		d.	Lead (III) phosphate

7.	Which of the following is a correct pair of formula and name? (3.02)
a.	CO:  monocarbon monoxide		c. SO2:  sulfur oxide
b.	N2O: dinitrogen oxide			d. BF3: boron trifluoride

8.	What is the charge of an atom that loses three electrons? (3.03)
a.	0	 			c.  +3 
b.	Not possible			d. - 3

9.	Which of the following best describes what happens when an ionic bond forms? (3.03)
a.	A metal accepts electrons from a nonmetal
b.	A nonmetal accepts electrons from a metal
c.	A metal donates electrons to a metal
d.	A nonmetal donates electrons to a nonmetal

10.	What happens when the compound CaCl2 forms? (3.03)
a.	Calcium donates one electron
b.	Chlorine accepts two electrons
c.	Calcium accepts one electron
d.	Calcium donates two electrons

11.	When one atom of lithium (Li) combines with one atom of chlorine (Cl), their bonding results in a molecule of LiCl. Which of the following describes the arrangement of valence electrons in a bond between Li and Cl? (3.03)
a.	The valence electrons spend more time around Li
b.	The valence electrons are given up by the Li and gained by the Cl	
c.	The valence electrons are shared equally between Li and Cl
d.	These two atoms will not form a bond.

12.	Which of the following best describes the formula unit for a compound made from Li and S? (3.03)
a.	It is LiS because the total negative charge on S is one.
b.	It is Li2S because the total negative charge on S is two.
c.	It is Li2S because the total positive charge on Li is two.
d.	It is LiS because the total positive charge on S is one.

13.	Which of the following best describes what  is represented by the following Lewis Dot Structure? (3.03)

a.	Oxygen is accepting an electron to form a -1 charge
b.	Sodium  is donating two electrons to form a +2 charge
c.	Each sodium atom is donating one electron to oxygen, which will then have a  +2 charge
d.	Each sodium atom is donating one electron to oxygen, which will then have a -2 charge

14.	Which of the following pairs of elements could possibly be in the same group? (3.03)
a.	X has a +3 ion; Y has a -3 ion.
b.	X tends to form a +1 ion; Y has one valence electron.
c.	X will tend to gain two electrons; Y has two valence electrons.
d.	X has an atomic number 49; Y forms a +2 ion.

15.	Which of the following best compares ionic and covalent bonding? (3.04)
a.	Covalent bonding transfers electrons whereas ionic bonding shares electrons
b.	Ionic bonding transfers electrons whereas covalent bonding shares electrons
c.	Both ionic and covalent share electrons, but we draw their Lewis Dot Structures differently
d.	Both ionic and covalent transfer electrons, but we draw their Lewis Dot Structures differently

16.	Which of the following best describes the bonding in a molecule of H2S? (3.04)
a.	The sulfur atom shares an electron pair with each H atom.	
b.	Each hydrogen atom receives an electron pair from the sulfur atom.
c.	One hydrogen atom shares one electron with the other  H atom, which shares an electron with sulfur
d.	Each hydrogen atom shares an electron with the sulfur atom.

17.	How many single bonds are in a molecule of nitrogen gas in its natural state? (3.04)
a.	0			c. 1
b.	2			d. 3

18.	As a covalent bond lengthens, what happens to its strength? (3.04)
a.	The strength increases. 				
b.	The strength decreases.
c.	The strength of a bond is not measurable.	
d.	There is no change to the strength of a bond.

19.	Select the best explanation for the formula that is formed when nitrogen bonds with hydrogen. (3.04)
a.	N3H because each hydrogen contributes three electrons to the triple bonds.
b.	NH3 because nitrogen contributes one electron to each of the single bonds.
c.	N3H because each hydrogen contributes three electrons to each of the single bonds.
d.	NH3 because each hydrogen contributes three electron pairs to the double bonds.

20.	Identify the molecular shape and number of domains for a molecule of silicon dioxide (SiO2). (3.05)
a.	Linear with two domains				
b.	Trigonal planar with two domains
c.	Linear with three domains			
d.	Trigonal planar with three domains

21.	Which of the following is correct for a molecule of HCN? (3.05)

	VSEPR molecular shape	Total Domains (bonded/lone pairs) around central atom	
a	Trigonal Planar	1 total domain; 1 bonded pairs and two lone pairs 	
b	Bent	4 total domains; 3 bonded pairs and 0 lone pair	
c	Tetrahedral	4 total domains; 2 bonded pairs and two lone pairs	
d	Linear	2 total domains; 2 bonded pairs and no lone pairs	

22.	Which of the following is NOT true about hydrogen bonding?  (3.06)
a.	It is an intermolecular force				
b.	It exists between any element and hydrogen.
c.	It is the 2nd strongest of all the intermolecular forces.	
d.	Water experiences hydrogen bonding.

23.	Electrostatic attraction of permanent dipoles in polar molecules is a definition of which type of intermolecular force?   (3.06)
a.	London Dispersion		c.  Dipole-dipole
b.	Ion-Dipole			d.  Hydrogen Bonding

24.	Which of the following is true of London Dispersion forces?   (3.06)
a.	The get weaker as the number of electrons increases
b.	They are a permanent attractive force between two adjacent molecules forming permanent dipoles.
c.	They occur between all particles and molecules.
d.	They are stronger than hydrogen bonding.

25.	Dipole-dipole interactions form between which types of molecules?  (3.06)
a.	Non-polar molecules		c.  Polar molecules
b.	Ionic compounds		d.  All of the above

26.	On the basis of strength of intermolecular forces, which of the following elements would be expected to have the highest melting point?  (3.06)
a.	Br2 				c.  Cl2  
b.	F2  				d.  Kr
27.	For the previous question #27, why does that compound have the highest melting point?  (3.06)
a.	Because it has dipole-dipole forces while the others have london dispersion
b.	Because they all have london dispersion forces, but this compound has more electrons
c.	Because they all have dipole-dipole forces, but this compound has more electrons

28.	Which of the following substances has the highest boiling point?  
a.	H2O			c.  Kr
b.	CO2			d.  NH3

29.	Which of the following molecules would be most polar? (3.06)
a.	H2			c.  HF
b.	HBr			d.  HCl

Essay format questions:
30.	The electron configuration of an element is: 1s2 2s2 2p6 3s2 3p6 4s2 (3.01)
a.	Identify the group name this element belongs to in the periodic table and explain your answer.
b.	Based on the electron configuration, write one chemical property of this element.

31.	 What is the correct name for PdO2? Explain how you determined the charges of each element and how you named it.  (3.03)

Honors Extension (all MC on the exam):

32.	(3.07H) What does the picture to the right represent? 
a.	Amine 			c.  Alcohol
b.	Polymer		d.  Carbohydrate

33.	(3.07H) Which group has an oxygen atom bonded between two carbon atoms in the carbon chain and are not very soluble in water.
a.	Amine			c. Ether
b.	Carbohydrate		d. Alcohol

34.	(3.07H) In an experiment, two unknown compounds (one an amine and the other an alcohol) of equal molecular mass were dissolved in water. The result of the experiment is shown in the table. 
Solubility Comparison
Unknown Compound	Solubility 
(g/100mL water)	
A	5.9	
B	4.6	

Which of the following correctly explains the identity of Compound A and its solubility?
a.	It is an alcohol because the lack of hydrogen bonding between the OH− groups make it less soluble.
b.	It is an amine; because the lower electronegativity of N than H makes it more soluble.
c.	It is an amine; it contains a nitrogen atom that will allow nitrogen-hydrogen bonds to form while in water and they are stronger than the oxygen-hydrogen bonds.
d.	It is an alcohol because the hydrogen bonding is more polar than the N - C bonds and makes it more soluble.

35.	(3.07H) All of the following are properties of carbon, except: 
a.	Has 3 valence electrons		c. Can form double bonds
b.	Can form bonds with 4 atoms		d. Can form rings