Review for Bonding Basics
Bonding Basics
1. Put the following elements in order of increasing electronegativity, Cl, Ca and S. (2pt)
2. Explain how ionic bonding is different from covalent bonding. (2pt)
3. How many of these molecules are nonpolar molecules? (2pt)
BF3
SO2
CO2
SiH4
A. 1
B.2
C. 3
D. 4
H2S
E. 5
4. Using your knowledge of electronegativity, dipole moments and polar vs nonpolar
answer the following questions.
A) Explain the relationship between electronegativity and a dipole moment. (5pt)
B) Show the potential dipole moments in NH3. (5pt)
C) Explain why both CCl4 and CCl3F both have polar bonds but one molecule is
polar and one is nonpolar. (5pt)
Review Ionic Bonding
1. Explain the two principles of Coulomb’s Law that we use to determine the strength of
an ionic bond.
2. For each pair of compounds, circle the one that exhibits that strongest bond. Tell
whether you used size or charge to make the determination. (2pt each)
A. MgCl2 or KCl
B. SrCl2 or SrO
C. K2O or BaS
D. Fe(OH)2 or Fe(OH)3
3. Demonstrate how the following elements have ionic bonds. (5pts each)
a) Rb and Br
b) Fe+3 and O
c) K and P
Review H – You had better draw the structures!!!!
1. Estimate the H in kJ of one mole of acetylene, C2H2 (see reaction below) using the
following bond energies: (5 pt)
Bond
Bond Energy (kJ/mol)
C-C
347
C=C
614
O=O
495
C=O
799
O-H
467
C-H
413
C-O
358
C3H8(g) + 5 O2(g)  3CO2(g) + 4H2O(g)
2.
C2H6 + 7/2 O2  2CO2 + 3 H2O
Given the following table of bond energies, calculate the change in enthalpy. (5pt)
Bond
Bond Dissociation Energy (kJ/mol)
C-C
347
C-H
415
O-O
146
O=O
495
C=O
799
O-H
463
Review Everything Covalent
1. What is the structure of SF6? (2pt)
A. Tetrahedral
B. Pyramidal
C. Square Planar
D. tee-shape
E. Octahedral
2. Is the molecule in Question #1 polar or nonpolar? (2pt)
A.
Polar
B. Nonpolar
3. What is the structure of ICl3? (2pt)
A. Tetrahedral
B. Pyramidal
4.
C. Square Planar
D. tee-shape
E. Trigonal Planar
Is the molecule in Questions #3 Polar or Nonpolar? (2pt)
A.
Polar
B. Nonpolar
5. As the number of bonds between the two carbon atoms increases, which of the
following increases? (2pt)
A.
B.
C.
D.
E.
The number of electrons between the carbon atoms
The bond energy
The bond length
All of those
None of these
6. In the Lewis structure for elemental oxygen there is/are (2pt)
A.
B.
C.
D.
E.
A single bond between the oxygens
A double bond between the oxygens
A triple bond between the oxygens
Three unpaired electrons
None of these
7. The hybridization of the central atom carbon in CO2 is (2pt)
A. It is not hybridized.
B. sp
C. sp2
D. sp3
8. The hybridization of the central atom in C2H6 is (2pt)
A. d2sp3
B. sp
C. sp2
D. sp3
E. dsp3
9. Which of the following contains a pi bond? (2pt)
A. CH3OH
B. PF2
C. C2H6
D. NO2
E. CCl4
E. dsp3
For each of the following compounds you need to do the following: (Please make your
work neat) (6pt each)
1) Write the number of valence electrons
2) Draw the Lewis structure (show resonance if necessary)
3) Tell the shape of the structure
4) Tell the bond angle
5) Tell the polarity of the molecule
6) Give the hybridization of the central atom.
1) OF2
2) ICl3
3) AsH3
4) BrF5