Honors Chemistry: Chapter 7 - Bonding
OBJECTIVES
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
Describe the nature of the chemical bond and its relationship to valence electrons.
Use electronegativities to predict the type of bond that will form between given atoms.
Define ionic bond, covalent bond and molecule.
Differentiate between the properties of ionic and covalent bonds.
Define the ionic radius, and use ionic radius to calculate the internuclear distance between ions in a crystal.
Distinguish between non polar, polar and covalent bond.
Use electronegativities to compare the polarities of bonds.
Describe the coordinate covalent bond.
Define polyatomic ions, and describe their bonding characteristics.
Explain metallic properties using the metallic bond concept.
Use Lewis dot structures to show molecular structures.
Illustrate, using examples, the concept of resonance.
13. Be able to write Lewis dot structures for cases that do not obey the octet rule.
Distinguish between shared and unshared electron pairs.
15. Explain how the shared and unshared pairs of electrons determine molecular structures.
Predict the shapes and bond angles of simple molecules based on the VSEPR theory.
Describe hybrid orbital.
Use hybridization theory to explain the bond angles in compound with multiple bonds.
Use hybridization theory to predict the shapes of molecules.
Differentiate between sigma and pi bonding.
Use the bonding theory to explain unsaturated bonds.
READING:
Textbook - Chapter 7
Section 7.1: Lewis Structures and the octet Rule, pages 180-187 (exclude Formal Charges), 188-191
Section 7.2: Molecular Geometry, pages 192-200
Section 7.3: Polarity of molecules, pages 200-201
Section 7.4: Atomic Orbitals; Hybridization, pages 203-209
WRITTEN ASSIGNMENTS:
Textbook, page 211:
Lewis Structures: Exercises 2- 20 even.
Resonance Structures: Exercises 22 - 26 even.
Molecular Geometry: Exercises 30 – 40 even.
Molecular Polarity: Exercises 42-46 even.
Hybridization: Exercises 48-60 even
Sigma and Pi bonds: Exercises 62, 64.
Unclassified: 68, 7.
Dittos in the packet as assigned.
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Honors Chemistry: Chapter 7 - Bonding
Introduction to Bonding: General Concepts (Chemical Bond)
DIRECTIONS: Write the letter preceding the word or expression that best completes the statement.
1.
In a chemical bond, the link between atoms results from the attraction between electrons and (a) Lewis structures; (b)
nuclei; (c) van der Waals forces; (d) isotopes
2.
A covalent bond consists of )a) shared electron; (b) a shared electron pair; (c) two electrovalent electrons; (d) an
octet of electrons
3.
If two covalently bonded atoms are identical, the bond is identified as (a) nonpolar covalent; (b) polar covalent; (c)
nonionic; (d) coordinate covalent
4.
A covalent bond in which there is unequal attraction for the shared electrons is (a) nonpolar; (b) polar; (c) ionic; (d)
dipolar
5.
Atoms with a strong attraction for electrons they share with another atom exhibit (a) zero electronegativity; (b) low
electronegativity; (c) high electronegativity; (d) Lewis electronegativity.
6.
Bonds with between 5% and 50% ionic character are considered to be (a) ionic; (b) pure covalent; (c) polar
covalent; (d) nonpolar covalent.
7.
A nonpolar covalent bond is likely to exist between (a) a metal and a nonmetal; (b) two ions; (c) two identical
atoms; (d) an atom and an ion.
8.
The greater the electronegativity difference between two bonded atoms, the greater the percentage of (a) ionic
character; (b) metallic character; (c) covalent character; (d) electron sharing.
9.
In which of these compounds is the bond between the atoms NOT a nonpolar bond? (a) Cl2; (b) H2; (c) HCl; (d)
O 2.
DIRECTIONS: Complete the following statements, forming accurate sentences.
10. The electrons involved in the formation of a chemical bond are called ____________________________________
11. A chemical bond resulting from electrostatic attraction between positive and negative ions is called a(n)
_____________________________________________________________________________________________
12. If the electrons involved in bonding spend most of the time close to one atom rather than the other, the bond is
_____________________________________________________________________________________________
DIRECTIONS: Consult your Periodic Table, specifically examine the graph of % ionic character, and answer the
following questions.
13. The percentage of ionic character and the type of bond for the Li-Cl bond in LiCl (electronegativity for Li = 1.0;
electronegativity for Cl = 3.0) is ______________________________________________________
14. The percentage of ionic character and the type of bond for the Br-Br bond in Br2 (electronegativity for Br = 2.8) is
______________________________________________________________________________________________
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Honors Chemistry: Chapter 7 - Bonding
Bonding – General Concepts (Ionic Bond)
DIRECTIONS: Write the letter preceding the word or expression that best completes the statement.
1.
In the formula unit of sodium chloride, NaCl stands for one (a) formula unit; (b) molecule; (c) crystal; (d) atom
2.
The chemical formula for an ionic compound represents the (a) number of atoms in each molecules; (b) the number
of ions in each molecule; (c) simplest ratio of the combined ions that gives neutrality; (d) total number of ions in
crystal structure.
3.
A formula that shows the types and numbers of atoms combined in a single molecule is called (a) molecular formula;
(b) ionic formula; (c) Lewis structure; (d) covalent formula.
4.
In a crystal of an ionic compound, each cation is surrounded by a number of (a) molecules; (b) positive ions; (c)
dipoles; (d) anions.
5.
In a crystal, the valence electrons of adjacent ions (a) repel each other; (b) attract each other; (c) neutralize each
other; (d) have no effect on each other.
6.
Compared the neutral atoms involved in its formation, the crystal lattice that results is (a) higher in potential energy;
(b) lower in potential energy; (c) equal in potential energy; (d) unstable.
7.
The lattice energy of a compound A is greater that that of a compound B. What can be deducted from this fact? (a)
Compound A is not an ionic compound. (b) It will be more difficult to break the bonds in compound A than in
compound B. (c) Compound B is probably a gas. (d) Compound A has larger crystals than compound B.
8.
Which of the following is NOT a property of an ionic compound? (a) vaporizes readily at room temperature; (b)
brittle; (c) hard; (d) electrical conductor in molten state.
9.
Compared to ionic compounds, molecular compounds (a) have higher boiling points; (b) are brittle; (c) have lower
melting points; (d) are harder.
10. The forces of attraction between molecules in a molecular compound are (a) stringer that the forces of ionic bonding;
(b) weaker that the forces of ionic bonding; (c) approximately equal to the forces of ionic bonding; (d) zero.
11. At room temperature, most ionic compounds will be (a) solids; (b) liquids; (c) gases; (d) molten.
DIRECTIONS: Complete each of the following statement with the best meaning word or expression.
12. A(n) _______________ is a shorthand representation of the composition of a substance using atomic symbols and
numerical subscripts.
13. In the NaCl crystal, the packing of Na+ ions and Cl- ions is such that each ion has clustered around it __________ of
the oppositely charged ions.
14. In an ionic compound, the orderly arrangement of ions in a crystal is the state of _____________ energy.
15. _________________energy is the type of energy released when one mole of an ionic crystalline compound is formed
from gaseous ions.
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Honors Chemistry: Chapter 7 - Bonding
Bonding: Ionic Bond
1.
Which of the following elements form positive ions when they react?
a. Li in Group 1
b. Ni, a transition element
c. S in Group 16
d. C in Group 14
2.
Explain, in terms of metallic character, why aluminum form a +3 ion much more readily than boron in the same group.
3.
Explain why nitrogen forms a -3 ion, N3- , while bismuth, Bi, in the same group, forms a +3 ion, Bi3+ .
4.
Why, in ionic crystal, are "+" ions surrounded by "-" ions rather than ions of the same charge?
5.
How do you explain the fact that solid ionic compounds do not conduct an electrical current, yet they become
conductors when melted?
6.
In general, which is larger:
a. a positive ion or the corresponding atom?
_____________________________
b. a negative ion or the corresponding atom?
_____________________________
c. a metal atom or a nonmetal atom in the same period of the Periodic table? _________________________
d. a metal ion or a nonmetal ion in the same period? _____________________________
7.
Give the electron configuration of:
a. Na1+
b. Ca2+
c. Al3+
8.
d. Cl1-
e. O2-
What charges would you expect for ions of the following metals?
a. K
b. Sc
c. Li
d. Al
e. Sr
9.
What charges would you expect for the ion of the following nonmetals?
a. S
b. F
c. N
d. I
e. O
10.
Which of the following ions have a noble-gas configurations?
a. Cs1+
b. Be2+
c. In3+
d. Mn2+
11.
12.
13.
Name the following ions:
a. NH41+
b. CO32-
c. NO31-
e. Ca2+
d. ClO31-
Write the formula, include the charge, for the following polyatomic ions:
a. sulfate
b. phosphate
c, hydrogen carbonate
Give the simplest formula of a compound containing:
a. A+ and Xb. C3+ and X 1c. B2+ and Y2-
d. chromate
d. A1+ and Y2-
14.
Using the electronegativity table, arrange the following compounds in order of decreasing ionic character:
LiI, BaO, AlCl3, CsF, RbBr, K2S, CaO, ClF, P2S3, F2, NaI, Mg3N2 .
15.
What tests might you perform to determine whether a substance is ionic?
16.
Write a balanced equations for the reaction of oxygen with
a. Li
b. Zn
c. Sc
d. Bi(III)
17.
Give all the possible the charges of ions formed by the following transition elements:
Ag
b. Zn
c. Cu
d. Fe
18.
A certain ionic compound contains 60.7% O, 17.7% N, 15.2% C, 6.37% H. Find the simplest formula of the
compound and identify the ions present.
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Honors Chemistry: Chapter 7 - Bonding
Bond Classification
Classify the bonds between the following pairs of atoms as principally ionic or covalent.
1. Al -Si
4. C - H
7. Ca - Cl
2. Ba - O
5 . Li - S
8. F - S
3. Ca - P
6. B - N
9. Rb - Br
For each of the atom pair listed below, decide whether an ionic or a covalent bond would form
between the elements.
10. hydrogen - fluorine
11. astatine - beryllium
12. cobalt - fluorine
13. bromine - cerium
14. iron - fluorine
15. calcium - fluorine
Using any available information, estimate the percent of ionic character in the following bonds.
16. Pb - S
18. Na - Br
20. Cu - I
17. Ag - Cl
19. C - N
21. H - O
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Honors Chemistry: Chapter 7 - Bonding
Covalent Bond: Drawing Lewis Structures
Draw Lewis structures for the following molecules. The central atom is underlined. NOTE the number of
shared and unshared pairs of electrons.
1.
PCl3
23.
ClO31-
2.
SO42-
24.
GeF4
3.
PO43-
25.
HBr
4.
CH2Cl2
26.
PF3
5.
N2O
27.
NI3
6.
CO2
28.
SiH4
7.
HCN
29.
CH3Cl
8.
CO
30.
Br2
9.
H2S
31.
CHBr3
10.
H2Te
32.
CBr4
11.
H2CO3
33.
SO3
12.
H2S
13.
HBr
14.
NO31-
15.
PO2F21-
16.
CO
17.
CO2
18.
SCl2
19.
N31-
20.
ClF3
21.
CBr4
22.
XeF2
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Honors Chemistry: Chapter 7 - Bonding
Covalent Compounds: Geometry (1)
Determine the number of shared and unshared electron-pairs around the central atom for the following molecules.
1. H2Te
2. PF3
3. BeF2
4. CBr4
Determine the molecular geometry using the VSEPR theory.
5. AlCl3
13. PCl3
6. CBr4
14. H2O
7. BF3
15. H - Be - H
8. CO2
16.
OF2
F
9. HCN
17.
F
Xe
F
F
10. H2CO
18.
ClO31-
11. SO3
19.
NO31-
12. SF2
20. N = N = 0
Predict whether the bond angle of each of the following is greater than, less than, or equal to 109.5 o.
21.
F - N - F in NF3
23.
F - Te - F in TeF2
25.
F- As - F in AsF5
22.
F - Be - F in BeF2
24.
F - O - F in OF2
26.
O - Xe - O in XeO4
List all the bond angles in the following compounds:
27.
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CH4
28. H - C = C - H
29.
H H
H-C=C-H
7
Honors Chemistry: Chapter 7 - Bonding
Covalent Bond: Polar Bonds
1.
Arrange the following elements in order of increasing force of attraction for electrons in the bond.
Sb, F, In, O, N, Se, Cl
2.
Which of the following bonds is most polar? In each bond, indicate the atom that carries the partial
negative charge.
a. H - I
3.
b. P - I
c. As - Br
d. N - S
Predict whether the following molecules are polar or nonpolar.
a. SO2
b. AsCl3
c. H2Se
d. SO3
e. H2S
f. CO2
g. CO
i. I2
H
\
j. PH3
H
H
\
/
n. Cl - C - C – Cl
/
\
H
H
OH
/
q. H - O - S
\\
O
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k. SiCl4
l. SCl2
m.
H
/
C=C
/
\
Cl
Cl
o. H2O
H H
| |
p. H - C - C = O
H
r.
Cl
\
/
C=C
/
\
Cl
H
8
Honors Chemistry: Chapter 7 - Bonding
Covalent Bond: Hybridization
1.
Mixing of atomic orbitals in an atom (usually the central atom) to generate a set of new atomic orbitals is
called _________________________________.
2.
The ________ orbitals will result in four equal-energy bonds.
3.
When two equal-energy orbitals are formed as a result of mixing ______ and _____ orbitals you obtain sp
hybridization.
4.
sp3d2 hybrid orbitals will form only in elements of which periods?
5.
The most common hybridization for an atom in group 13 is the _____ hybridization; and in group 14 is the
_________ hybridization.
6.
What is the usual hybridization in group 2? ____________________
7.
Determine the hybridization for the following underlined atoms:
a.
Te
/ \
H H
d.
Cl
|
Al
/ \
Cl Cl
P
/ | \
HH H
c.
Br Br
\ /
C
/ \
Br Br
e. O = C = O
f
H-C=N
b.
H
\
g.
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S
/ \
H H
h
H
/
C=C
/
\
H
H
I.
H H H
\ | /
S
/ | \
H H H
9
Honors Chemistry: Chapter 7 - Bonding
Bonding: Review - Vocabulary
In the spaces to the left, write the term that correctly completes each statement.
bond angle
delocalized
molecule
conjugated system
geometric isomers
pi bond
unshared pairs
covalent radius
metallic bond
covalent bond
delocalization
hybrid orbitals
shared pairs
potential energy
ionic bond
bond length
internuclear distance
double bond
isomers
sigma bond
bond energy
bond axis
electronegativity
van der Waals radius
functional isomers
Lewis electron dot diagram
triple bond
_____________________1.
The average distance along an imaginary line joining the nuclei of two atoms in a molecule is
known as the __________________________ .
_____________________ 2. Named for a physicist, the ____ is the minimum distance between nuclei for atoms on adjacent
molecules.
_____________________ 3. A _______ results when two or more atoms form a covalent bond.
_____________________ 4. The electrostatic force known as the ____ holds two ions together due to their differing charges.
_____________________ 5.
The imaginary line joining the nuclei of two bonded atoms in a molecule is called the
_______.
_____________________ 6. An atom's relative tendency to attract electrons to itself when bound with a another atom is
called its _______.
_____________________ 7. The )_____ is the average number of degrees between two bond axes extending from the same
atom.
_____________________ 8. Adding the radii of two ions in a compound results in their _____.
_____________________ 9. When atoms with the same or nearly the same electronegativities share electrons, the resulting
shared pair or pairs of electrons constitute a _________.
_____________________ 10. When electrons in metals are ___, they are free to travel among positive ions.
_____________________ 11. The sum of one ____ with another is the internuclear distance between two atoms.
_____________________ 12. Delocalized electrons holding metallic atoms together constitute a ____.
_____________________ 13. In substances with the same molecular formula but different structures, those structures are
called ___.
_____________________ 14.
A(n) ___ is formed when two p orbitals overlap sideways with their axes parallel.
_____________________ 15. Outer electron pairs bonding two nuclei are called _____.
_____________________ 16.
When three orbitals from a single bonding electron cloud, a(n) ___ occurs.
_____________________ 17. A simplified means of depicting the electrons in an atom's outer level is shown in a(n)
_________.
_____________________ 18. A(n) ___ is formed by the direct overlap of two orbitals.
_____________________ 19. A single electron cloud
made of two orbitals is considered a(n) ____.
_____________________ 20. When carbon s and p orbitals merge, they theoretically, form four equivalent ____.
_____________________ 21. _____ refers to the existence of two or more substances with the same molecular formula, but
different structures.
_____________________ 22. The two non-bonding outer electron pairs are called ______.
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Honors Chemistry: Chapter 7 - Bonding
_____________________ 23. A stabilized molecule containing multiple p overlaps is called a(n) ___.
_____________________ 24. ___are composed of the same atoms bonded in the same order, but with a different arrangement
of atoms around a double bond.
_____________________ 25. Equal sharing of the pi electrons among all the carbon atoms, without confinement to one atom
or bond, is known as ____.
_____________________ 26. ________ is a measure of the strength of a chemical bond.
_____________________ 27. Generally, a chemical change will tend to occur if it leads to a lower state of _______.
28.
What factor is most important in determining the type of bond formed between two atoms?
a. the size of atoms
b. the physical state of the elements
c. the charge on the nuclei of the atoms
d. the energy changes that accompany bond formation
e. the Lewis structure of the atoms
29.
Write the electron dot structure of the nitrogen atom.
30.
Write the electron dot structure of the chlorine ion.
31.
Which of the following ions has the noble-gas configuration?
a. Fe+2
b. Pb+2
c. Tl+1
d. Sn+2
e. Ca+2
32.
Write the Lewis structure for Br2.
33.
How many lone pairs are present in hydrazine, N2H4?
34.
How many electrons are there in a double bond?
35.
What is the correct arrangement of atoms in the Lewis structure of phosphorus trichloride, PCl 3?
36.
What is the correct arrangement of atoms in the Lewis structure of NO2Cl?
37.
How many valence electrons are there in the Lewis structure of difluoromethane, CH2F2?
38.
How many valence electrons are there in the Lewis structure of the perchlorate ion, ClO 4-1?
39.
Write the Lewis structure for the sulfite atom, SO3-2.
40.
Each of the elements shown except one is capable of achieving an expanded octet. Which one is not?
a. I
b. S
c. O
d. Xe
e. P
41.
Which of the following compounds has an atom with an expanded octet?
a. SF5
b. H2O
c. PCl3
d. HBr
42.
43.
44.
45.
H
H
N-N
H
H
Which element can have more than one oxidation number?
a. C
b. O
c. S
d. F
e. Al
Which element often has an incomplete octet in its compounds?
a. F
b. O
c. B
d. Xe
e. P
Which of the following is an odd-electron molecule?
a. N2O
b. N2O4
c. NH3
d. NO3
e. N2O5
e. NH3
All but one of the following species exhibit the phenomenon of resonance. Which one does not?
a. NO3-1
b. SO2
c. CO2
d. SO4-2
e. C6H6
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Honors Chemistry: Chapter 7 - Bonding
46.
All but one of the statements regarding resonance is correct. Which one is incorrect?
a. A species that undergoes resonance changes rapidly from one form to another.
b. Resonance lowers the energy of the species.
c. One Lewis structure will not properly describe a molecule that undergoes resonance.
d. Resonance involves changing the positions of double bonds in Lewis structures.
e. Resonance averages out certain bond lengths in a Lewis structure.
47.
Which of the following structures represent resonance structures of a single species?
:X=A-X:
I
a. I and III
48.
49.
X-A=X:
II
:X-X=A:
III
b. I and II
c. II and III
d. I, II, and III
Which molecule has a central atom with an expanded octet?
a. CO2
b. XeF4
c. CF4
d. SO3
e. NCl3
Which molecule has a central atom with an incomplete octet?
a. CH4
b. BeF2
c. N2
d. SO2
e. PBr3
e. none of the above
For the questions 50 through 55 answer the following:
1.
How many electron pairs surround the central atom ?
2.
What is the shape of the molecule?
# of electron pairs
Shape
50.
CBr4
_____________________________________________________________________
51.
SF4
_____________________________________________________________________
52.
CO3-2
_____________________________________________________________________
53.
SO2
_____________________________________________________________________
54.
GaCL3
_____________________________________________________________________
55.
TeCl4
_____________________________________________________________________
56.
What is the effect of lone pairs of electrons on bond angles?
57.
Which bond is predominantly ionic?
a. Ge-F
b. Sn-Cl
c. As-Br
58.
Which of the following is polar?
a. CO2
b. NH3
c. CF4
d. N-O
d. BF3
e. So-O
e. SeO2
59.
A molecule consists of a central atom surrounded by some number of atoms of the same element. What shape
molecule of this type is likely to be polar?
a. linear b. octahedral
c. square planar d. T-shaped
e. trigonal planar
60.
Which of the following is nonpolar?
a. SeO2
b. CH3F
c. H2O
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d. ClF3
e. XeF4
12
Honors Chemistry: Chapter 7 - Bonding
61.
One of the following does not apply to a covalent bond. Which one?
a. electron pairs
b. electrons are shared
c. orbitals overlap
e. electrons localized on one atom
d. may be polar
62.
What hybridization is associated with a trigonal planar arrangement of electron pairs?
a. sp3d
b. sp2
c. sp3d2
d. sp
e. sp3
63.
What hybridization is associated with an octahedral arrangement of electron pairs?
a. sp3d
b. sp2
c. sp3d2
d. sp
e. sp3
64.
What arrangement of electron pairs occurs with sp3 hybridization?
a. trigonal planar
b. T-shaped
c. octahedral
d. tetrahedral
e. trigonal bipyramidal
65.
An octahedral arrangement of electron pairs can lead to all of the molecular shapes given except one. Which
molecular shape cannot arise from an octahedral arrangement of electron pairs?
a. trigonal planar
b. octahedral
c. square planar
d. square pyramidal
e. linear
66.
An AB4 molecule has two lone pairs. What is the hybridization of the central atom?
a. sp3d
b. sp2
c. sp3d2
d. sp
e. sp3
67.
Head-to-head overlap of an sp3 hybrid orbital with an sp2 hybrid orbital creates a
a. double bond
b. sigma bond
c. pi bond
d. triple bond
68.
A triple bond consists of
a. three sigma bonds
c. two sigma bonds and one pi bond
69.
70.
b. one sigma bond and two pi bonds
d. three pi bonds e.
Side-by-side overlap of a p-orbital with another p-orbital creates a
a. single bond
b. sigma bond
c. pi bond
d. triple bond
An atom with the valence electron configuration shown is expected to form four sigma bonds. What hybridization is
expected?
   
s
p p p
a. sp
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b. sp3
c. sp3d
d. sp2
e. sp2d3
13
Honors Chemistry: Chapter 7 - Bonding
SELF-TEST: CHAPTER 7
1.
The total number of electron pairs around phosphorus for PCl5 is: a. 2
b. 3
2.
An atom X is surrounded by 3 sigma bonds and 1 pi bond. The bond angle around the central atom is
a. 90º
b. 109º
c. 120º
d. 180º
3.
An atom X is surrounded by an unshared pair of electrons, 2 sigma bonds and one pi bond. The hybridization for the molecule
with X as central atom is a. sp
b. sp2
c. sp3
d. sp3d
e. sp3d2
4.
Which of the following bonds would be most polar?
a. C-C
b. C-O
c. C-F
d. C-N
5.
All of the following molecules have double bonds except: a. BeF 2
b. CO2
c. SO3
d. NO
6.
Arsenic pentafluoride forms an expanded octet. Which of the following statements are true?
a. There are five bonds to the central atom.
b. There is pair of unshared electrons around the central atom.
c. Its geometry is that of trigonal bipyramid.
d. Its geometry is tetrahedral.
7.
Which of the following form expanded octet?
a. (1), (2)
b. (3),(4) c. (1), (4)
8.
For which of the following species can one write reasonable resonance structures?
(1) ClO2(2) CO3-2 (3) SO2
(4) NO2(5) ClO4-
9.
Which of the following lists the molecular geometries of SiF4, SO3, and SF5 correctly and in order?
a. tetrahedral, triangular planar, triangular bipyramid
b. octahedral, bent, triangular bipyramid
c. octahedral, triangularplanar, triangular bipyramid
d. triangular bipyramid, linear, tetrahedral
10.
Which of the following molecules is/are nonpolar?
a. ClF3
b. CH2F2
c. SO2
(1). NF 3
(2). CO3-2
d. (2), (3)
d. OF2
c. 4
(3). XeF4
e. a, b, c, d are polar
d. 5
e. 6
(4). ClF3
f. a, b, c, d, are nonpolar
Problems:
Give the Lewis structures and all resonance forms, if any, of the following:
1. PO3-1
3. ClO3-1
2. CS2
Consider the following molecules. Determine:
a. their Lewis structures
b. their geometry
c. their bond angles
d. the hybridization on the central atom
f. the number of sigma and pi bonds
If the molecule is an expanded octet, determine only its Lewis structure, geometry, and hybridization.
4. OCS
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5. NO3-1
6. H3C-O-CCl3
7. SO2
8. PCl3F2
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Honors Chemistry: Chapter 7 - Bonding
ANSWERS TO QUESTIONS IN CHAPTER 7 PACKET
Page 2:
1- b
2-b
3-a
9-c
10 – valence electron
14- 0, nonpolar covalent
4-b
5-c
11-ionic bond
6-c
12-ionic
7-c
8-a
13-63%, ionic
4-d
5-a
12-chemical formula
6-b
13. six
7-b
Page 3:
1-a
2-c
9-c
10-b
14- minimum potential
3-a
11-a
15-lattice
8-a
Page 4:
1- a, b
2- Larger atom, lower ionization energy
3. N has high electronegativity, Bi has very low
electronegativity, low ionization energy, easily forms + ion
4. opposite charges attract
5-when melted the crystalline structure breaks and the ions are mobile, thus conducting electric current
6. a-atom, b- negative ion; c- metal atom; d- nonmetal ion
7. a-[Ne] ; b- [Ar]; c- [Ne]; d- [Ar]; e- [Ne]
8. a) +1; b) +3; c) +1; d) +3; e) +2
9. a) –2; b)-1; c) –3; d) –1; e) –2
10. a; b; e
11. a) ammonium, b) carbonate; c) nitrate; d) chlorate
12. a) SO4-2 b) PO4-3 c) HCO3-1 d) CrO4-2
13. a)AX; b) CX3 c) BY d) A2Y
14. CsF, BaO, CaO, RbBr, Mg3N2, K2S, NaI, AlCl3=LiI, ClF, P2S3, F2
15. dissolve the compound in water and check for electric conductivity
16. 2Li + O2  Li2O; 2Zn + O2  2ZnO ; 4Sc + 3O2  2Sc2O3; Bi + O2  Bi2O3
17. a) +1; b) +2; c) +2, +1; d) +2, +3
18. CH5NO3; NH4HCO3
Page 5:
1. covalent
6. covalent
11. covalent
16. 12%
21. 39%
Page 6:
2. ionic
7. ionic
12. ionic
17. 28%
3. covalent
8. covalent
13. ionic
18. 60%
4. covalent
9. ionic
14. ionic
19. 4-9%
5. ionic
10. ionic
15. ionic
20. 9%
See attached handwritten page
Page 7:
1. 2 shared (S), 2 Unshared (U)
2. 3S, 1U
3. 2S, 0 Unshared
5. triangular planar
6. tetrahedral
7. triangular planar
9. linear
10. triangular planar 11. triangular planar
13. triangular pyramid
14. bent
15. linear
17. square pyramid
18. triangular planar 19. triangular planar
21-less than
22- greater than
23- less
24- less
26- less
27- 109.5
28- 180
29- 120 each
4. 4S
8. linear
12. bent
16. bent
20. linear
25- 120, 90
Page 8:
1. In, Sb, Se, Cl=N, O, F
2. most polar As-Br
3. a) polar; b) polar; c) v. slightly polar
d) nonpolar; e) polar; f) nonpolar; g) polar; i) nonpolar; j) polar; k) nonpolar; l) polar; m) polar;
n) nonpolar o) polar q) polar
p) polar
r) nonpolar
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Honors Chemistry: Chapter 7 - Bonding
Page 9:
5. sp2, sp3;
1. hybridization
2. hybrid
3. s & p;
4. transition elements
6. sp 7. a) sp3; b) sp3 ; c) sp3; d) sp2; e) sp; f) sp; g) sp3; h) sp2; I) sp3d2
Page 10 through 13
1. bond length
5. bond axis
9. covalent bond
13. isomers
17. Lewis electron dot
20. hybrid orbitals
24. geometric isomers
2. van der Waals radius
6. electronegativity
10. delocalized
14. sigma
27. potential energy
28. d
3. molecule
7. bond angle
11. covalent radius
15. shared pairs
18. sigma
22. unshared pairs
25. pi bond
21. functional isomers
4. ionic bond
8. intermolecular distance
12. metallic bond
16. triple bond
19. double bond
23. conjugated
26. bond energy
..
29.
N 

30.  Cl :

.
31. e
32. Br-Br
33. 2
34. 4
35. trigonal pyramid
36. trigonal planar
37. 20 e
38. 32 e
39. trigonal planar
40. c
41. a
42. c
43. c
44. d
45. d
46. a
47. b
48. b
49. b
50. 4, tetrahedral
51.
52. trigonal planar
55. see-saw
56. lower the bond
59. d
65. a
60. e
66. e
53. bent
54. trigonal planar
57. a,b
61. e
67. b
58. b
62. b
68. b
63. d
69. c
64. tetrahedral
70. b
Page 14:
1. d
8. c
2. c
9. a
3. b
10. d
4. c
5. a
6. d
7. b
Problems:
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