Unit 3 Study Guide: Covalent & Ionic Bonding

Multiple Choice
Identify the choice that best completes the statement or answers the question.

____	1.	Figure 5-1 shows a portion of a blank periodic table. Identify the segments labeled A and B.
a.	A and B are both periods.	c.	A and B are both groups.	
b.	A is a period and B is a group.	d.	A is a group and B is a period.	

Figure 6-1

____	2.	Study the electron dot diagrams for lithium, carbon, fluorine, and neon in Figure 6-1. Choose the statement that correctly identifies the most stable of the elements.
a.	Lithium is the most stable element because it has to lose only one electron to achieve a stable configuration.	
b.	Carbon is the most stable element because it can form four bonds.	
c.	Fluorine is the most stable element because it has to gain only one electron to achieve a stable configuration.	
d.	Neon is the most stable element because its highest occupied energy level is filled.	

____	3.	The formation of an ionic bond involves the
a.	transfer of electrons.	c.	transfer of protons.	
b.	transfer of neutrons.	d.	sharing of electrons.	

____	4.	Which of the following statements correctly describes the substance with the formula KI?
a.	Molecules of potassium iodide contain one atom of potassium and one atom of iodine.	
b.	There is a one-to-one ratio of potassium ions to iodide ions.	
c.	Potassium iodide is a molecular compound.	
d.	Potassium iodide is a polyatomic ion.	

____	5.	In the compound MgCl2, the subscript 2 indicates that
a.	there are two magnesium ions for each ion of chlorine	
b.	the chloride ion is twice the size of the magnesium ion.	
c.	magnesium and chlorine form a double covalent bond.	
d.	there are two chloride ions for each magnesium ion.	

____	6.	Which of the following formulas represents a compound whose molecules contain a triple bond?
a.	NºN	c.	O3	
b.	O=O=O	d.	SO3	

Completion
Complete each statement.

	7.	In an electron dot diagram, each dot represents a(an) ____________________.

	8.	In an ionic compound, the attractions between cations and ____________________ hold the compound together.

	9.	In the binary ionic compound potassium bromide, KBr, the element that forms cations is ____________________.

	10.	The chemical formula for calcium chloride, CaCl2, shows that the compound contains two ____________________ ions for every ____________________ ion.

	11.	KBr is the formula for an ionic compound. The fact that neither symbol is followed by a subscript means that there is a(an) ____________________ ratio of ions in the compound.

	12.	If there are two long dashes between two atoms in a structural formula, molecules of the compound contain a(an) ____________________ bond.

	13.	When cesium and fluorine react, they form an ionic compound called cesium ____________________.

	14.	In ionic compounds, the sum of the charges of all the cations and anions must be ____________________.

Short Answer

	15.	Selenium has six valence electrons, while rubidium has one valence electron. Identify each element as a metal or a nonmetal.

	16.	What determines an element’s chemical properties?

	17.	Element X has five valence electrons, element Y has one valence electron, and element Z has five valence electrons. Which two of these elements are most likely to have similar properties? Explain your answer.

	18.	In a periodic table that included electron dot diagrams, in which column would the diagrams contain more dots—Group 2A (the alkaline metals) or Group 6A (the oxygen family)?

Figure 6-1

	19.	Study the electron dot diagrams in Figure 6-1. Which of the elements are most likely to react and form a compound? What type of compound are they likely to form?

	20.	In the binary ionic compound lithium iodide, LiI, which element forms anions?

	21.	Are covalent bonds more likely to be found in compounds containing both metals and nonmetals or compounds containing only nonmetals?

	22.	In potassium bromide, KBr, which element forms anions?

	23.	In sodium chloride, NaCl, are the cations sodium ions or chloride ions?

	24.	Why are metals good conductors of electric current?

	25.	Explain what it means to have a stable electron configeration.

	26.	For each pair of elements draw an atomic diagram showing electrons in different energy levels. Draw arrows to show where the outer electrons will go during a chemical reaction, then draw the resuting compound for Na + Cl= NaCl and Li + Cl = LiCl.

	27.	Draw Lewis Dot Structures for each of the following: NH3, CH4, NH3, CO2, and N2

Unit 3 Study Guide: Covalent & Ionic Bonding
Answer Section

MULTIPLE CHOICE

	1.	ANS:	B	PTS:	1	DIF:	L1	
OBJ:	5.2.1  Describe the arrangement of elements in the modern periodic table.
STA:	SPS4. | SPS4.a		

	2.	ANS:	D	PTS:	1	DIF:	L1	
OBJ:	6.1.2  Predict an element’s chemical properties using the number of valence electrons and electron dot diagrams.	STA:	SPS4.a.1

	3.	ANS:	A	PTS:	1	DIF:	L2	
OBJ:	6.1.3  Describe how an ionic bond forms and how ionization energy affects the process.
STA:	SPS1.b

	4.	ANS:	B	PTS:	1	DIF:	L2	
OBJ:	6.1.4  Predict the composition of an ionic compound from its chemical formula.

	5.	ANS:	D	PTS:	1	DIF:	L1	
OBJ:	6.1.4  Predict the composition of an ionic compound from its chemical formula.

	6.	ANS:	A	PTS:	1	DIF:	L2	
OBJ:	6.2.1  Describe how covalent bonds form and the attractions that keep atoms together in molecules.
STA:	SPS1.b

COMPLETION

	7.	ANS:	valence electron

PTS:	1	DIF:	L1	OBJ:	6.1.1  Recognize stable electron configurations.

	8.	ANS:	anions

PTS:	1	DIF:	L1	
OBJ:	6.1.3  Describe how an ionic bond forms and how ionization energy affects the process.
STA:	SPS1.b

	9.	ANS:	potassium

PTS:	1	DIF:	L2	
OBJ:	6.1.3  Describe how an ionic bond forms and how ionization energy affects the process.
STA:	SPS1.b

	10.	ANS:	chloride, calcium

PTS:	1	DIF:	L1	
OBJ:	6.1.4  Predict the composition of an ionic compound from its chemical formula.

	11.	ANS:	one-to-one

PTS:	1	DIF:	L2	
OBJ:	6.1.4  Predict the composition of an ionic compound from its chemical formula.

	12.	ANS:	double

PTS:	1	DIF:	L2	
OBJ:	6.2.1  Describe how covalent bonds form and the attractions that keep atoms together in molecules.
STA:	SPS1.b

	13.	ANS:	cesium floride

PTS:	1	DIF:	L2	
OBJ:	6.3.1  Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions.	STA:	SPS2.c.1 | SPS2.b

	14.	ANS:	zero

PTS:	1	DIF:	L1	
OBJ:	6.3.2  Name and determine chemical formulas for ionic and molecular compounds.
STA:	SPS2.c.1 | SPS2.c.2	

SHORT ANSWER

	15.	ANS:	
Selenium is a nonmetal. Rubidium is a metal.

PTS:	1	DIF:	L2	
OBJ:	5.3.1  Relate the number of valence electrons to groups in the periodic table and to properties of elements in those groups.		STA:	SPS4.b | SPS4.a	

	16.	ANS:	
the number of valence electrons

PTS:	1	DIF:	L1	
OBJ:	5.2.1  Describe the arrangement of elements in the modern periodic table.
STA:	SPS4. | SPS4.a		

	17.	ANS:	
Elements X and Z will have similar properties because they have the same number of valence electrons.

PTS:	1	DIF:	L1	
OBJ:	5.3.1  Relate the number of valence electrons to groups in the periodic table and to properties of elements in those groups.		STA:	SPS4.b | SPS4.a	

	18.	ANS:	
Group 6A, the oxygen family

PTS:	1	DIF:	L1	
OBJ:	6.1.2  Predict an element’s chemical properties using the number of valence electrons and electron dot diagrams.	STA:	SPS4.a.1

	19.	ANS:	
lithium, Li, and fluorine, F; an ionic compound

PTS:	1	DIF:	L2	OBJ:	6.1.1  Recognize stable electron configurations.

	20.	ANS:	
iodine, I

PTS:	1	DIF:	L2	
OBJ:	6.1.4  Predict the composition of an ionic compound from its chemical formula.

	21.	ANS:	
in compounds containing only nonmetals

PTS:	1	DIF:	L1	
OBJ:	6.2.1  Describe how covalent bonds form and the attractions that keep atoms together in molecules.
STA:	SPS1.b

	22.	ANS:	
bromine, Br

PTS:	1	DIF:	L2	
OBJ:	6.3.1  Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions.	STA:	SPS2.c.1 | SPS2.b

	23.	ANS:	
sodium ions

PTS:	1	DIF:	L1	
OBJ:	6.3.1  Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions.	STA:	SPS2.c.1 | SPS2.b

	24.	ANS:	
Metals contain a shared pool of electrons that are free to move.

PTS:	1	DIF:	L2	OBJ:	6.4.2  Relate the properties of metals to their structure.
STA:	SPS2.

	25.	ANS:	
in a stable electron cigeration, the highest occupied energy level is filled with electrons

PTS:	1

	26.	ANS:	
n

PTS:	1

	27.	ANS:	
n

PTS:	1