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class4_GRPHW - − 1 0 b 0 − 1 c 1 − 1 d 1 0 e 3 − 1...

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Name _________________________Chem 108 Section # ________ Class 4 Page 7 Group Work Homework: Electronegativity and Bond Polarity 1. Put these atoms in order of increasing electronegativity. B Cl Li Br Cs O a) B < Li < Cs < Cl < Br < O b) O < Cl < Br < B < Li < Cs c) Cs < Li < B < Cl < Br < O d) Cs < B < Li < Br < Cl < O e) Cs < Li < B < Br < Cl < O 2. Which one of the following bonds is polar? You should be able to do this using only the periodic table. (a) C H (b) H F (c) H H (d) C C (e) O O 3. Which one of the following bonds is least polar? a) C H b) H F c) H Br d) O H e) Cl H
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Name _________________________Chem 108 Section # ________ Class 4 Page 8 Group Work Homework: Lewis structures See page 8 and 9 of Study Guide 1. How many valence electrons are there on the following atoms? a) P b) Ar c) Te d) Br 2. What is the formal charge on N and Br in NO 2 Br (nitrogen is the central atom)? N Br a) 1 0 b) 0
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Unformatted text preview: − 1 0 b) 0 − 1 c) +1 − 1 d) +1 0 e) +3 − 1 3. Draw the Lewis structure of NO 2 − . Which statement about NO 2 − is correct? a) There is one short N O bond and one long N O in the ion b) The formal charge of N in NO 2 − is − 1. c) There are two resonance structures that represent the structure of NO 2 − . d) There are 2 bonded pairs and 6 lone pairs in the structure of NO 2 − . 4. Draw the Lewis structures for each of the following ions. Be sure to show the structure below. Identify the structures that do not obey the octet rule and explain why they do not A BH 3 B. I 3 − C O 2 − a) The structure obeys the octet rule. b) The structure does not obey the octet rule: there are an odd number of electrons. c) The structure does not obey the octet rule: there are too few electrons on the central atom. d) The structure does not obey the octet rule: there is an expanded octet on the central atom....
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