Honors Chemistry
Chemical Bonding
Name________________________________
Periodic Trends
1. Determine the common ion that each element would form and write its electron configuration:
a. Rb
b. N
c. Se
d. Br
e. Ga
f. K
2. Circle the smaller atom.
a. Mg
or
Be
e. S
or
P
b. Al
or
P
f. Au
or
Be
c. Br
or
Cs
g. Cl
or
I
d. Sb
or
Se
h. Sn
or
Sr
3. Explain why germanium has a larger radius than silicon.
4. Arrange each in order of increasing atomic volume.
a. O, Mg, Al, Si _____________________
b. O, S, Se, Te
_____________________
c. C, Sr, Ga, As _____________________
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5. Explain why germanium has a larger radius than arsenic.
6. Circle the larger particle.
a. Ca
b. F1−
or
or
Ca2+
e. Mg2+
Cl1−
f. Te2−
c. As3−
or
P3−
g. C
d. Pb4+
or
Pb
h. Ag
Be2+
or
or
or
or
Te
C4−
Ag1+
7. Explain why sulfide has a larger radius than sulfur.
8. Arrange in order of increasing ionic radius.
a. Ca2+, K1+, Al3+
________________________
b. Se2−, Br1−, Te2−
________________________
c. Al3+, Ca2+, Rb1+, K1+ ________________________
9. Which atom in each pair has the larger atomic radius?
a. ______ Li or
K
e. ______ Cl or Br
b. ______ Ca or Ni
f. ______ Be or Ba
c. ______ Ga or B
g. ______ Si or S
d. ______ O or C
h. ______ Fe or Sc
10. Which ion in each pair has the smaller radius?
a. ______ Na1+ or O2−
d. ______ K1+ or Cs1+
b. ______ Ba2+ or I1−
e. ______ Fe2+ or Fe3+
c. ______ Al3+ or P3−
f. ______ F1− or S2−
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11. Select three ions of your choosing that are isoelectronic. Arrange them in increasing order of ionic
radius and explain why that order is correct.
12. Which atom or ion in each pair has the larger (a) first ionization energy, (b) atomic radius,
(c) electron affinity, and (d) electronegativity?
Na or O
a. ______
b. ______
c. ______
d. ______
Be or Ba
a. ______
b. ______
c. ______
d. ______
Ar or Ne
a. ______
b. ______
c. ______
d. ______
Cu or Ra
a. ______
b. ______
c. ______
d. ______
I or Ne
a. ______
b. ______
c. ______
d. ______
K or V
a. ______
b. ______
c. ______
d. ______
Ca or Fr
a. ______
b. ______
c. ______
d. ______
W or Se
a. ______
b. ______
c. ______
d. ______
13. Chlorine, selenium, and bromine are located near each other on the periodic table. Which of these
elements is (a) the smallest atom? (b) the atom with the highest electron affinity?
14. Phosphorous, sulfur, and selenium are located near each other on the periodic table. Which of
these elements is (a) the largest atom? (b) the atom with the highest ionization energy?
15. Scandium, yttrium, and lanthanum are located near each other on the periodic table. Which of
these elements has a) a larger electronegativity value? (b) the atom with the smallest ionization
energy?
16. (a) Which of the following atoms is smallest: vanadium, chromium, or tungsten? (b) Which of
these has the highest electron affinity?
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17. Which of the following is the largest: a potassium atom, a potassium ion, or a rubidium atom?
18. Which of the following is the largest: a chlorine atom, a chlorine ion, or an argon atom?
19. Which of the following is the smallest: a lithium atom, a lithium ion, or a sodium atom?
20. Which is more metallic, zinc or cadmium?
21. Which is more non-metallic, oxygen or sulfur?
22. Which is more reactive, calcium or barium?
23. Which is more reactive, chlorine or bromine?
Na
Mg
Al
Si
P
S
Cl
Ar
IE1
496
738
578
786
1012
1000
1251
1521
IE2
IE3
IE4
IE5
IE6
4560
1450
7730
1820
2750
11600
1580
3230
4360
16100
1900
2910
4960
6270
22200
2250
3360
4560
7010
8500
2300
3820
5160
6540
9460
2670
3930
5770
7240
8780
Ionization Energy values are measured in kJ/mol
IE7
27100
11000
12000
24. The thermochemical equation for the removal of one electron from sodium is:
Na + 496 kJ → Na+ + 1e−
Write the thermochemical equation for:
a. The removal of a second electron from sodium
b. The removal of the first electron from phosphorus
c. The removal of the third electron from aluminum.
5
25. Refer to the table above and explain the following:
a. Chlorine’s first ionization energy is larger than sulfur’s.
b. Magnesium’s first ionization energy is larger than sodium’s, but its second ionization
energy is significantly lower.
c. Aluminum’s first ionization energy is lower than that of magnesium despite the trend.
d. Sulfur’s first ionization energy is lower than that of phosphorus despite the trend.
26. Calculate the total amount of energy required to remove 1 electron from every atom in a 2.36 g
sample of magnesium.
27. Sodium metal has a first ionization energy of 496 kJ/mol.
a. What wavelength of light, in nanometers, is sufficient to provide a photon with the
necessary energy to remove 1 electron from an atom of sodium?
b. How many photons of this light are needed to remove the first electron from each sodium
atom that is present in a piece of sodium that has dimensions of 4.36 cm x 36.2 mm x 2.46
in? (DNa = 0.97 g/cm3)
c. What would be the mass and charge of these removed electrons?
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Chemical Bonds
28. Based on electronegativity trends, complete the chart below.
Degree of Polarity (check one)
Bond Type
a
H–O
b
As – Cl
c
Cs – N
d
O–O
e
O–F
f
Na – Br
g
S8
h
S – Cl
i
P–F
j
I2
slightly moderately extremely
Nonpolar
polar
polar
polar
29. For each of the following properties, indicate if the compound’s bond type is ionic (I),
covalent (C), or unable to be determined (X).
a. _____melts at 150 oC
e. _____liquid at room temp
b. _____conducts a current in solution
f. _____solid does not conduct a current
c. _____solid at 100 oC
g. _____linear molecule
d. _____boils at 15 oC
h. _____cubic crystal
The "more
negative"
atom if
polar
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30. Draw the Lewis dot diagram and chemical formula for the compounds formed when the following
elements ionically bond.
a. barium and chlorine
b. potassium and sulfur
c. strontium and arsenic
d. aluminum and nitrogen
31. Draw the Lewis dot diagram for the following ionic compounds:
a. calcium phosphide
b. lead(IV) sulfide
32. How many covalent bonds will each of the following nonmetals likely make?
a. N ______
b. O ______ c. H ______ d. Ne ______ e. Cl ______
f. As ______
g. C ______
h. B ______
l. F ______
i. Si ______ j. P ______
k. Br ______
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33. Complete the table below for the indicated covalently bonded compounds.
Total
Number
of
Valence
Electrons
PH3
SiCl4
O2
Cl2
Continued on next page
Lewis Dot Diagram
Number
of
Bonding
Pairs
Number
of Lone
pairs
Total
Number of
electrons in
Dot
Diagram
9
Total
Number
of
Valence
Electrons
N2
CS2
HF
SO2
Lewis Dot Diagram
Number
of
Bonding
Pairs
Number
of Lone
pairs
Total
Number of
electrons in
Dot
Diagram
10
34. Draw Lewis structures for the following compounds using lines for bonds. Remember to count
valence electrons and confirm that all are present in the completed structure.
SO3
SO3-2
CO2
CO
CO3-2
H2CO3
PO4-3
NO3-
NO+
HNO2
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37. Complete the following table:
Lewis Structure
NBr3
CH3Cl
ClO2-
TeO3
Continued on next page
Structural Formula
Electron
Geometry
Bond
angle
Molecular
Geometry
Lewis Structure
SO4-2
SCl2
HCN
BF3
Continued on next page
Structural Formula
Electron
Geometry
Bond
angle
12
Molecular
Geometry
Lewis Structure
CS2
O3
N2
NO2-
Structural Formula
Electron
Geometry
Bond
angle
13
Molecular
Geometry
14
39. The Lewis structures for the following molecules have all been drawn in previous questions. For
each of these molecules, draw the structural formula to the proper shape and indicate if it is polar
or nonpolar. If polar, draw the arrow indicating the direction of the dipole.
NBr3
O3
CO2
SCl2
SO3
CO
BF3
CH3Cl
N2
TeO3
15
40. Complete the following table:
Lewis Structure
ICl
CBr4
AsF3
CHF3
BH3
Structural Formula
(drawn to shape)
(indicate polarity)
electron
geometry
bond
angle
molecular
geometry
16
Review
41. Circle the element in each pair that has a smaller radius
a.
Fe
or
Os
b. As
or
Ge
c. O
or
O−2
d. Ca
or
Ca+2
d. Na+
or
S−2
e.
or
Se−2
Br−
42. Arrange the following in order from smallest radius to largest:
P−3, K+, Ar, Cl−
43. Circle the element with the larger ionization energy.
a. Mn
or
Co
b. Bi
or
N
44. Which has a larger second ionization energy, potassium or calcium? Why?
45. Why does nitrogen have a larger first ionization energy than oxygen?
46. Why does Kr have a larger atomic radius than Ne?
47. Why does aluminum have a lower electronegativity than silicon?
48. Circle the element with the higher electronegativity.
a. C
or F
b.
Ra
or
Ba
49. Predict the bond type between:
a. P – O
b. F – F
c. K – Br
50. Draw Lewis dot diagrams for the following ionic compounds.
a. AlP
b. CaCl2
c. The compound containing Sr and N
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51. Complete the following table:
Lewis Structure
CTe2
POCl
SeO3
AsBr3
OF2
Structural Formula
(indicate polarity)
electron
geometry
bond
angle
molecular
geometry
18
52. Draw the structural formulas for the following oxyacids:
a. HClO2
b. H3PO3
c. H2SO3
53. How many single bonds are in 427 mL of sulfur trioxide at STP?
54. Draw the structure of a carbonate ion.
Cumulative Questions
55. Write balanced equations for the following.
a. Solid sodium carbonate is heated.
b. A piece of aluminum metal is placed into a solution of magnesium nitrate.
c. Solutions of acetic acid and calcium hydroxide are mixed.
d. The fusion of californium-252 with boron-10 to produce 5 neutrons and a nuclide
56. Write the complete electron configuration for chromium.
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57. Sodium hypochlorite, the main ingredient in household bleach, is produced according the
following reaction.
Sodium hydroxide + chlorine → sodium chloride + sodium hypochlorite + water
What is the percent yield of the reaction if 1.25 kg of chlorine reacts to form 0.90 kg of sodium
hypochlorite?
58. Xylitol is a sweetener that has anticavity properties because it does not stick to teeth. Elemental
analysis of a sample resulted in 0.5921 g carbon, 0.1184 g hydrogen and 0.7895 g oxygen. The
molar mass was determined by an effusion rate comparison with oxygen gas. Oxygen was found
to effuse 2.18 times faster than xylitol when vaporized. Determine xylitol’s molecular formula.
59. Calculate the mass of the solid product formed by reacting 20.00 mL of 0.150 molar solution of
sodium sulfide with 35.00 mL of 0.100 molar solution of cadmium nitrate.
60. What mass of lead(II) nitrate would contain 8.36 x 1023 oxygen atoms?
61. A 1.952 gram sample of hydrated calcium sulfate was heated intensely. At the end of the heating
process, 1.398 grams of material remained. What is the chemical formula of the hydrate?