Honors Chemistry Name________________________________Chemical Bonding
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 _____________________
25. Explain why germanium has a larger radius than arsenic.
6. Circle the larger particle.
a. Ca or Ca2+ e. Mg2+ or Be2+
b. F1− or Cl1− f. Te2− or Te
c. As3− or P3− g. C or C4−
d. Pb4+ or Pb h. Ag or 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
b. ______ Ca or Ni
c. ______ Ga or B
d. ______ O or C
e. ______ Cl or Br
f. ______ Be or Ba
g. ______ Si or S
h. ______ Fe or Sc
10. Which ion in each pair has the smaller radius?
a. ______ Na1+ or O2−
b. ______ Ba2+ or I1−
c. ______ Al3+ or P3−
d. ______ K1+ or Cs1+
e. ______ Fe2+ or Fe3+
f. ______ F1− or S2−
311. 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?
417. 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?
IE1 IE2 IE3 IE4 IE5 IE6 IE7
Na 496 4560Mg 738 1450 7730Al 578 1820 2750 11600Si 786 1580 3230 4360 16100P 1012 1900 2910 4960 6270 22200S 1000 2250 3360 4560 7010 8500 27100Cl 1251 2300 3820 5160 6540 9460 11000Ar 1521 2670 3930 5770 7240 8780 12000
Ionization Energy values are measured in kJ/mol
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
625. 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?
7Chemical Bonds
28. Based on electronegativity trends, complete the chart below.
Degree of Polarity (check one)
Bond Type Nonpolar
slightly polar
moderately polar
extremely polar
The "more negative" atom if polar
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
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
b. _____conducts a current in solution
c. _____solid at 100 oC
d. _____boils at 15 oC
e. _____liquid at room temp
f. _____solid does not conduct a current
g. _____linear molecule
h. _____cubic crystal
830. 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 ______ i. Si ______ j. P ______ k. Br ______ l. F ______
933. Complete the table below for the indicated covalently bonded compounds.
Total Number
of Valence
Electrons
Lewis Dot Diagram
Number of
Bonding Pairs
Number of Lone
pairs
Total Number of electrons in
Dot Diagram
PH3
SiCl4
O2
Cl2
Continued on next page
10Total
Number of
Valence Electrons
Lewis Dot Diagram
Number of
Bonding Pairs
Number of Lone
pairs
Total Number of electrons in
Dot Diagram
N2
CS2
HF
SO2
1134. 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
35. For each structure drawn above indicate which bonds are coordinate covalent bonds.
1236. Draw all of the possible resonance structures for the following compounds.
NO2-
O3
SeO2
N2O4
(each nitrogen atom is bonded to two oxygen atoms and to the other nitrogen)
1337. Complete the following table: Indicate coordinate covalent bonds in structural formulas.
Lewis Structure Structural Formula Electron Geometry
Bond angle
Molecular Geometry
NBr3
CH3Cl
ClO2-
TeO3
Continued on next page
14
Lewis Structure Structural Formula Electron Geometry
Bond angle
Molecular Geometry
SO4-2
SCl2
HCN
BF3
Continued on next page
38.
15
Lewis Structure Structural Formula Electron Geometry
Bond angle
Molecular Geometry
CS2
O3
N2
NO2-
1639. 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
1740. Complete the following table:
Lewis StructureStructural Formula (drawn to shape) (indicate polarity)
electron geometry
bond angle
molecular geometry
ICl
CBr4
AsF3
CHF3
BH3
18Review
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. Br− or Se−2
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
1951. Complete the following table:
Lewis Structure Structural Formula (indicate polarity)
electron geometry
bond angle
molecular geometry
CTe2
POCl
SeO3
AsBr3
OF2
2052. Draw the structural formulas for the following oxyacids and identify all coordinate covalent
bonds:
a. HClO2 b. H3PO3 c. H2SO3
53. How many coordinate covalent bonds are in 427 mL of sulfur trioxide at STP?
54. Draw all of the possible resonance structures for the 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.
2157. 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?
