Question

2. Predict the formula of the ionic compounds formed from the following pairs of elements using Lewis symbols. Name the compounds. a. Al and I b. Rb andS 3. Rank the following in order of increasing bond length and bond strength. a. Si-F Si-C; Si-o 4. Calculate the amount of energy necessary to break all the bonds in formaldehyde CH20. What type of process is this? -O 5. Predict which pairs give ionic, polar covalent, or nonpolar covalent compounds by looking at the periodic table. Mg and S Cu and oO N and O Cand S 6. Use electronegativity values to determine the types of bonds formed for the pairs in problem 5 and evaluate your predictions

Answer 1

PART 2 PART 5 a. Al and I Mg and S: Polar covalent Cu and O: Ionic N and O: Polar covalent .Al +3.i: -> A+3 Aluminium Iodide b. Rb and S 2Rb + .S > 2Rb+s2 Rubidium Sulfide and S: apolar covalent PART 3 PART 6 a. Bond lenght: Si-F, Si-O, Si-C Mg and S: Polar covalent Bond strenght: Si-C, Si-O, Si-F △EN-Xs.xMg= 2.5-1-3 = 1.2 b. Bond lenght: N N, N-N, N-N Bond strenght: N-N, N-N, N N Cu and O: Polar covalent △ENzX -X = 3.5-1.9-1.6 N and O: Polar covalent AEN XoXN 3.5 -3.0 0.5 and S: apolar covalent AEN- Xs-X 2.5-2.5- 0