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Answers_worksheet_4 - CH1020 Exercises (Worksheet 4)...

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CH1020 Exercises (Worksheet 4) (Electronegativity, polarity of molecules, bond length, bond strength and bond order) 1. Using only the periodic table, predict the order of increasing electronegativity in each of the following groups of elements: a. Na, K, Rb b. B, O, Ga Rb<K<Na Ga<B<O c. F, Cl, Br d. S, O, F Br<Cl<F S<O<F e. Br, Cl, P f. I, F, O 2. Rank the following bonds in order of increasing ionic character (Check electronegativity values, Figure 9.19, page 352; Silberberg 4 th edition): N-O, Ca-O, C-F, Br-Br, K-F Br-Br < N-O < C-F < Ca-O < K-F 3. Explain the difference between pure covalent bond and polar covalent bond. Pure covalent: equal sharing of electron pair(s); polar covalent: unequal sharing of electron pair (s) 4. Explain the difference between polar covalent bond and ionic bond. Polar covalent: unequal sharing of electron pair (s); ionic bond: complete transfer of electrons from one atom to another to form ions 5. Atoms X and Y have different electronegativities. Will the diatomic molecule X- Y necessarily be polar? Explain. What factors affect the size of the dipole moment of a diatomic molecule? Yes. If X and Y have different electronegativities, they have different attractions for the electrons in the molecule. The electron density around the more electronegative atom will be greater, producing a charge separation or dipole in the molecule. Magnitude of the charges and the distance between them affect the size of the dipole moment in a diatomic molecule. 6.
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This note was uploaded on 04/17/2008 for the course CHE 1020 taught by Professor Kumar during the Summer '08 term at WPI.

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Answers_worksheet_4 - CH1020 Exercises (Worksheet 4)...

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