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Review Ch. 1 sec. 1-8
Consider the substance ethanol, CH
3
CH
2
OH.
1. a. Draw the Lewis structure for ethanol.
2. Fill in the chart for each central atom in ethanol. Refer to your Lewis structure in #1. b. Draw bond polarity arrows for any polar bonds shown your Lewis structure in part a.
(The C-H bond is nonpolar.)
Central Atom VSEPR Molecular
Shape
Ideal bond angle
Observed bond angle
C (terminal)
C (middle)
O
3. a. Is the ethanol molecule polar or nonpolar? Explain.
b. How would you expect a thin stream of ethanol to behave next to a charged wand?
Explain.
4. Can ethanol form hydrogen bonds?_______ If so, draw 2 ethanol molecules and indicate where hydrogen bonding takes place.
5. List all types of intermolecular forces found in ethanol.
6. Would you classify ethanol as an element, compound, or mixture?
7. Would you expect ethanol to be a solid, liquid, or gas at room conditions? Explain.

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8. How would ethanol interact with methanol, CH
3
OH? Explain. Use drawings to support your answer.
9. Which has a higher boiling point, ethanol or methanol? Explain.
10. a. How could you separate a mixture of ethanol and methanol?
b. Is this separation process a chemical or physical change? Explain.
11. a. Rank in order from smallest to largest atomic radius: C, H, O.
______< _______<______
b. Explain the rationale for your order. Use drawings to support your answer.
Include core charge and valence electrons in your drawings.
12. Draw a Lewis structure for a a. K atom b. P atom
13. a. Draw Lewis structures for the ionic compound potassium phosphide.
b. Write the empirical formula for potassium phosphide.