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Basic Chemistry (Chapters 1-16)

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CHEMISTRY 2002 NAME PROBLEM SET #20: Ionic & Metallic Bonding DATE PERIOD READ  SECTIONS  14.4 – 14.6!  1. Define each of the following vocabulary terms (1 pt. per definition): ionic bond coordination number metallic bond 2. Which of the following pairs of elements are likely to form ionic compounds? Circle your choice(s): a. chlorine and bromine b. potassium and helium c. lithium and fluorine d. iodine and sodium 3. Write the correct chemical formula (the formula unit) for the following pairs of ions. a. K + , S −2 b. Ca +2 , O −2 c. Na + , SO 4 −2 d. Al +3 , PO 4 −3 4. Most ionic substances are brittle. Why? 5. Why does molten MgCl 2 conduct an electric current although crystalline MgCl 2 does not? 6. Why is it possible to bend metals but not ionic crystals?
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Unformatted text preview: Rules for drawing Lewis Structures: 1. Obtain the sum of the valence electrons from all of the atoms. Do not worry about keeping track of which electrons come from which atoms. It is the total number of electrons that is important. 2. Use one pair of electrons to form a bond between each pair of bound atoms. For convenience, a line (instead of a pair of dots) is generally used to indicate each pair of bonding electrons. 3. Arrange the remaining electrons to satisfy the duet rule for hydrogen and the octet rule for each second-row element. 7. Give the Lewis Structures of each of the following molecules: a. HF b. N 2 c. NH 3 d. CH 4 e. CF 4 f. NO 3 −...
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