AP Chemistry: Chemical Bonding I & II
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1 AP Chemistry: Chemical Bonding I & II WarmUps (Show your work for credit) Name Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8.
2 AP Chemistry Chapter 10: Chemical Bonding II 2 WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8.
3 AP Chemistry Chapter 10: Chemical Bonding II 3 Warmups and problems will be collected before you take the test. Read Chapter 10: Chemical Bonding II: Molecular Geometry and the Hybridization of Atomic Orbitals Answer the following problems in the space provided. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units. 3. Show the final answer with units. There is no credit without showing work. Molecular Geometry 1. Predict geometries of the following species, and state bond angles: (a) AlC1 3 (b) ZnCl 2 (c) ZnCl 4 2. Predict geometries of the following ions: (a) NH 4 + (b) NH 2 (c) CO 3 (d) ICl 2 (e) ICl 4 (f) AlH 4 (g) H 3O + (h) BeF 4 3. Which of the following species are tetrahedral? (a) SiCl 4 (b) SeF 4 (c) XeF 4 (d)ci 4 (e) CdCl 4 4. Predict the bond angles for the following molecules: (a) BeCl 2 (b) BC1 3 (c) CC Place these compounds in order of increasing bond angle: SH 2, SO 2, PCl 3, SO 3, and CCl 4.
4 AP Chemistry Chapter 10: Chemical Bonding II 4 Polarity 6. What is the difference between bond polarity and molecular polarity? 7. Explain how can a molecule have polar bonds but be a nonpolar molecule? Give an example. 8. Draw Lewis structures for the following molecules, state whether each is symmetrical or nonsymmetrical, and predict whether each is polar or nonpolar. (a) SeO 2 (b) SO 3 (c) CH 3Br (d) ClF 3 (e) BrCl 5 (f) PCl 3 Hybridization 9. Draw Lewis structures and state the hybridization of each carbon atom in the following molecules: (a) Propene (b) 1butyne (c) butane 10. What is the hybridization of Si in: (a) SiH 4 (b) H 3Si SiH For the following reaction, describe the changes in hybridization (if any) of the B and N atoms as a result of this reaction. BF 3 + NH 3 F 3B NH Draw a Lewis structure and determine the hybridization of the each N atom in the azide ion, N 3? (Arrangement of atoms: NNN.)
5 AP Chemistry Chapter 10: Chemical Bonding II State the hybridization of the central atom in the following molecules: (a) AlCl 3 (b) BrF 5 (c) XeF How many pi bonds and sigma bonds are there in 1,3pentadiene? CH 3 CH=CH CH=CH For each of the following molecules, draw a single resonance Lewis structure, and state the number of pi and sigma bonds in the molecule: (a) nitrogen dioxide (b) hydrogen cyanide (c) thiocynate ion 16. Although both carbon and silicon are in Group 4A, silicon does not often form Si=Si bonds. Account for the instability of silicontosilicon double bonds in general. (Hint: Compare the atomic radii of C and Si. What effect would the larger size have on pi bond formation?) 17. The formation of H 2 from two H atoms is an energetically favorable process. Yet statistically there is less than a 100 percent chance that any two H atoms will undergo the reaction. Apart from energy considerations, account for this observation based on the electron spins in the two H atoms. 18. Polyatomic ions are more stable than expected due to delocalized molecular orbitals. Draw the Lewis structure of the nitrate ion showing it can exhibit delocalized MO s. Which bonds are localized and which are delocalized? 19. Nitryl fluoride (FNO 2) is a very reactive molecule. Draw the Lewis structure, state the hybridization of each atom, state the number of pi and sigma bonds, and state whether you expect FNO 2 to have delocalized MO s.
Instant download Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten CLICK HERE
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