Funsheet 9.1 [VSEPR] Gu 2015

Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF

Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NHF 2 PF 5 CO 2 SiF 4 SCl 6

Funsheet 9.11 [CONDUCTIVITY] Gu 2015 1. From the samples below, circle the ones that will exhibit good to excellent conductivity. a) CH 3 OH (l) b) Al (s) c) C 2 H 2(l) d) liquid sugar e) ethanol (aq) f) MgCl 2(aq) g) Na 2 SO 4(aq) h) CH 3 COOH (aq) i) LiCl (s) j) distilled H 2 O k) Fe (s) l) CO 2(aq) m) MgSO 4(l) n) HCl (aq) o) NaCl (s) p) C 6 H 12 O 6(s) q) table salt r) BaSO 4(aq) s) LiCl (l) t) Cu (s) 2. Circle the compound that will exhibit higher conductivity from each of the following pairs. a) Fe (s) NaCl (aq) b) 0.1 M KF 0.2 M KF c) 0.1 M LiCl (aq) 0.1 M BaCl 2(aq) d) 1 M Mg(ClO) 2 1 M Cr(OH) 3

Funsheet 9.2 [INTERMOLECULAR FORCES] Gu 2015 1. For each of the following molecules a) Draw the 3D Lewis structure (VSEPR) b) Indicate any bond dipoles c) Indicate whether or not the molecule is polar, and if it is, indicate the molecular dipole d) State whether the molecule will have dipole dipole forces NF 3 O 3 HCN PCl 5 CBr 4 H 3 O + 2. Which of the following molecules would you expect to be able to H bond? a) HBr b) H 2 SO 4 c) C 2 H 6

Funsheet 9.2 [INTERMOLECULAR FORCES] Gu 2015 3. Circle the H atoms that are capable of hydrogen bonding in the following molecules and put a box around the atoms that H can H bond to. 4. For each set of molecules, indicate which you would expect to have the greatest London forces. a) CH 4 C 6 H 12 b) O 2 H 2 Br 2 5. Rank the following molecules in order of increasing boiling point and justify your answer. a) H 2 SO 4 O 2 C 10 H 22 b) Provide an explanation for the observation in increasing boiling point: I 2 > HNO 3 > CH 2 Cl 2

Funsheet 9.3 [LIKE DISSOLVES LIKE] Gu 2015 1. Classify each solute and solvent as polar or non polar, and then predict which solvents will dissolve which solutes. Solvent Polar /Non Polar Solvent Polar/Non Polar a) Water H 2 O g) Acetic Acid CH 3 COOH b) Methanol CH 3 OH h) Chloroform CHCl 3 c) Ethanol CH 3 CH 2 OH i) Carbon tetrachloride CCl 4 d) Benzene C 6 H 6 j) Heptane C 7 H 16 e) (C 2 H 5 ) 2 O k) Ammonia NH 3 f) Acetone CH 3 COCH 3 Solute Polar/Non polar /Ionic a) H 2 O polar b, c, e, f, g, h, k b) CH 3 NH 2 c) CH 3 CH 2 CH 3 d) CH 3 CH 2 OONa + e) BaCl 2 f) CH 3 CH 2 CH 2 OH Will dissolve in these solvents (from above): 2. Which of the following is the best solvent for dissolving Br 2? H 2 O CO CH 4 CH 3 OH 3. Which of the following is the best solvent for dissolving HCN? C 2 H 2 HF CF 4 HI 4. Which of the following is the best solvent for dissolving CCl 4? H 2 SO 4 CH 3 Cl NaOH CH 3 CH 2 F 5. Which of the following is the best solvent for dissolving NH 3? C 2 H 4 CH 3 Br CH 3 F C 3 H 8

Funsheet 9.3 [LIKE DISSOLVES LIKE] Gu 2015 6. From the following compounds, circle the ones that will dissociate in water to form ionic solutions. a) NaCl b) CH 3 OH c) C 3 H 5 (OH) 3 d) Li 2 Cr 2 O 7 e) C 6 H 12 O 6 f) Mg 3 P 2 g) BeF 2 h) Co 2 (C 2 O 4 ) 3 i) K 2 SO 4 j) C 2 H 2 7. Write the dissociation equation for each circled compound from question 6.

Funsheet 9.4 [MOLARITY] Gu 2015 1. What is the concentration of NaCl when 4.99 g is dissolved in 250.0 ml? 2. What is the concentration of Li 2 SO 4 when 3.0 g is dissolved in 2.0 L? 3. What mass of Ca(OH) 2 was dissolved in 500.0 ml to make a 0.20 M solution? 4. What is the molarity of a solution in which 10.0 g of AgNO 3 is dissolved in 500.0 ml of solution? 5. How many grams of KNO 3 should be used to prepare 2.00 L of a 0.500 M solution? 6. How much water do you need to add to 5.0 g of KCl in order to prepare a 0.25 M solution? 7. What is the concentration of each ion in a 1.24 M Na 3 PO 4 solution? 8. What is the concentration of each ion when 36.4 g of aluminum sulfate is dissolved in 960.0 ml of water?

Funsheet 9.6 [DILUTIONS] Gu 2015 1. How much concentrated 18 M sulfuric acid is needed to prepare 250.0 ml of a 6.0 M solution? 2. What is the final concentration of NaOH when 50.0 ml of water is added to a 250 ml of a 1.2 M solution? 3. How much concentrated 12 M hydrochloric acid is needed to prepare 100 ml of a 2.0 M solution? 4. To what volume should 25 ml of 15 M nitric acid be diluted to prepare a 3.0 M solution? 5. To how much water should 50. ml of 12 M hydrochloric acid be added to produce a 4.0 M solution? 6. How much water should be added to change the concentration of a NaCl solution from 2.0 M to 1.5 M? The initial volume is 15 ml.

Funsheet 9.7 [MIXING SOLUTIONS] Gu 2015 1. A 5.34 g sample of calcium chloride and 9.85 g of aluminum chloride are dissolved in 4.50 L of solution. Assuming that no reaction occurs, calculate the concentration of each ion in the solution. 2. Calculate the final concentration of KOH when 50.0 ml of a 0.750 M solution is mixed with a 25.0 ml of 0.500 M solution. 3. Find the concentration of all ions when 1.55 ml of a 2.0 M CaBr 2 solution is mixed with 3.50 ml of a 1.5 M Ca(NO 3 ) 2 solution, assuming no reaction occurs.

Funsheet 9.8 [CONCENTRATION & STOICHIOMETRY] Gu 2015 1. What volume of a 0.250 M LiOH solution is needed to completely neutralize 80.0 ml of a 0.10 M HCl solution? 2. Determine the concentration of a hydrochloric acid solution if it is found that 16.00 ml of HCl reacts exactly with 50.00 ml of a 0.2000 M calcium hydroxide solution. 3. What mass of AgCl is formed when 24.8 ml of a 2.40 M MgCl 2 solution is added to a solution with excess moles of silver nitrate? 4. The following data was obtained with 0.1098 M NaOH was titrated against a 25.00 ml sample of HCl. Determine the concentration of the acid. Trial 1 Trial 2 Trial 3 Final Volume of NaOH 15.98 ml 32.56 ml 49.18 ml Initial Volume of NaoH 0.02 ml 15.98 ml 32.56 ml Volume of NaOH Used

Funsheet 9.8 [CONCENTRATION & STOICHIOMETRY] Gu 2015 5. 30.0 ml of 1.25 M hydrochloric acid is reacted with 25.0 ml of 1.50 M sodium hydroxide. a) Find the limiting reagent. b) Calculate the number of moles of sodium chloride produced. c) How much excess reactant is left over in moles? 6. 500.0 ml of a 0.150 M lead (ll) nitrate solution is mixed with 500.0 ml of a 0.250 M solution of sodium chloride. A double replacement reaction occurs in which a precipitate of lead (ll) chloride is formed. a) Find the limiting reagent. b) Find the mass of lead (ll) chloride c) Find the mass of the other product.

Funsheet 9.9 [SOLUBILITY] Gu 2015 Write equations for the following. If a precipitate forms, remember to write "(s)" 1. Na 3 PO 4(aq) + CaCl 2(aq) Complete formula Complete ionic equation Net ionic equation 2. CuSO 4(aq) + CaS (aq) Complete formula Complete ionic equation Net ionic equation 3. FeBr 3(aq) + SrI 2(aq) Complete formula Complete ionic equation Net ionic equation 4. Ba(NO 3 ) 2(aq) + Li 2 SO 4(aq) Complete formula Complete ionic equation Net ionic equation

Funsheet 9.10 [CALCULATIONS WITH SOLUBILITY] Gu 2015 1. Find the concentrations of all of the ions when the following solutions are mixed. a) 400. ml of 0.45 M potassium chloride is mixed with 200. ml of 0.75 M silver nitrate. b) 25 ml of 0.15 M calcium nitrate is mixed with 15 ml of 0.76 M sodium sulphate. c) 1.30 L of 0.75 M sodium iodide is mixed with 0.750 L of 2.40 M lead (II) nitrate.

Funsheet 9.10 [CALCULATIONS WITH SOLUBILITY] Gu 2015 d) 1.65 L of 1.0 M aluminum chloride is mixed with 1.00 L of 0.750 M sodium chromate, Na 2 CrO 4. The precipitate is Al 2 CrO 4. 2. In an experiment, 200.0 ml of 0.632 M calcium nitrate is mixed with 300.0 ml of 0.367 M lithium phosphate in a flask. The contents of the flask are then filtered. What is the expected mass of the solid product?