Attention: Please study problem set 1, 2, 5 and 6 as well. This review does not contain these chapters.

Transcription

1 Chemistry 101 Review for Final Attention: Please study problem set 1, 2, 5 and 6 as well. This review does not contain these chapters. 1. Use the following ions to write the chemical formula for each ionic compound: a) Ca 2+ NO 3 - b) Mg 2+ SO 4 2- c) Fe 2+ PO 3 3- d) Ga 3+ N 3-2. Find the charge of each element/polyatomic ion in these ionic compounds: a) Fe(ClO 3 ) 2 d) PbI 2 b) HgHPO 4 e) (NH 4 ) 2 CO 3 c) AlPO 3 f) CuNO 3 3. Find the name of the following compounds: a) Ca(HSO 4 ) 2 e) SnO 2 b) HF f) LiClO c) FeCO 3 g) H 2 PO 3 d) Al(OH) 3 h) HClO 2 4. Write the formula for the following compounds: a) Boron trifluoride d) Sodium dihydrogen phosphate b) Hydrochloric acid e) Barium permanganate c) Ammonium carbonate f) Carbon tetrachloride

2 5. Predict whether a precipitate will form when aqueous solutions of the following compounds are mixed. If a precipitate will form, write its formula, and write a net ionic equation. Identify the spectator ions. a) K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) b) NaOH(aq) + H 2 SO 4 (aq) c) AgNO 3 (aq) + CuCl 2 (aq) d) AlCl 3 (aq) + Li 2 CO 3 (aq) 6. Balance the following equations: a) Na + (aq) + CO 3 2- (aq) + Sr 2+ (aq) + Cl - (aq) SrCO 3 (s) + Na + (aq) + Cl - (aq) b) Cu + Zn 2+ Cu + + Zn c) Al 3+ + Fe Al + Fe 3+ d) Fe 2+ + Cu 2+ Fe 3+ + Cu 7. In the following equations, which species are oxidized and which species are reduced? Which ones are the oxidizing agents and which ones are the reducing agents? a) 2Fe Ni 2Fe + 3Ni 2+ b) C 2 H 4 O(l)+ H 2 O 2 (l) C 2 H 4 O 2 (l) + H 2 O(l) 8. Identify each of the following unbalanced reaction equations as belonging to one or more the following categories: precipitation, acid-base, oxidation-reduction, synthesis, decomposition, single replacement, double replacement, or combustion. a) I 4 O 9 (s) I 2 O 6 (s) + I 2 (s) + O 2 (g)

3 b) HCl(aq) + AgC 2 H 3 O 2 (aq) AgCl(s) + HC 2 H 3 O 2 (aq) c) SiCl 4 (l) + Mg(s) MgCl 2 (s) + Si(s) d) Ca(OH) 2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + H 2 O(l) 9. Considering the following reaction: NaClO 2 (aq) + Cl 2 (g) ClO 2 (g) + NaCl(aq) If 78.3g of NaClO 2 is used, how many grams of NaCl will be formed? 10. Lead(II) nitrate and aluminum chloride react according to the following equation: 3Pb(NO 3 ) 2 + 2AlCl 3 3PbCl 2 + 2Al(NO 3 ) 3 In an experiment, 8.00 g of lead nitrate reacted with 2.67g of alumium chloride to give 5.15 g of lead chloride. a) Which reactant was the limiting reagent? b) What was the percent yield? 11. Using the equation: Fe 2 O 3 (s) + 3CO(g) 2Fe(s) + 3CO 2 (g) If 105g of Fe 2 O 3 reacts with 21g CO, what volume of CO 2 gas will be formed at STP condition? 12. Write the complete orbital box diagram, electron configuration, and noble gas notation for each of the following elements/ions: a) Iodine, Z = 53

4 b) Krypton, Z = 36 c) Se 2-, Z = 34 d) Ba 2+, Z = Find the valence level and valence electrons for each of the elements/ions in problem Arrange the elements in each set in order of decreasing the size of the atom (by using only the periodic table). a) Ge, C, Si, Sn b) Be, B, Li c) K, Rb, Na, Li d) Sr, I, Sb, Te 15. Arrange the elements in each set in order of increasing ionization energy (by using only the periodic table). a) As, Br, Se, Ga b) P, As, N, Sb c) Ba, Cs, Pb d) Sr, Be, Ca, Mg 16. Find the location and the name of the following elements by using their electron configurations. a) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 b) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1

5 c) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 2 d) [Ar]4s 2 3d 10 4p What is the same and what is the difference in the electron configuration of: a) Ca and Sr b) P and As 18. Arrange the elements in each set in order of increasing electronegativity (by using the periodic table). a) As, N, P, Sb b) O, C, N, F c) Be, Sr, Ca, Mg d) As, Se, Ga, Br 19. Draw the Lewis structure for each covalent compound. a) CH 3 OCH 3 b) CH 3 CH 2 OH c) HCN d) COCl Predict the shape of each molecule and bond angles by using VSEPR. a) SCl 2 b) CH 3 COOH c) C 2 H 2

6 d) P 2 H In problem 20, which of the molecules are polar? Why? 22. In K 2 O, use the electron configuration of potassium and oxygen and then K + and O 2- to show how an ionic bond is produced between them. The electron configuration of potassium ion and oxide ion are similar to which noble gases? 23. A balloon contains 4 moles of an ideal gas with a volume of 5.0 L. If an additional 8 moles of the gas is added at constant pressure and temperature, what will be the final volume of the balloon? 24. If 2.6 moles of nitrogen gas are confined to a 6.0 L vessel at 177 C and 12.0 atm. If the vessel is allowed to expand isothermically (constant temperature) to 36.0 L, what would be the final pressure? 25. How many grams of nitrogen will occupy a 7.5 liter container at STP?

7 26. Suppose you have 56g of ammonia gas (NH 3 ) at 264 F, occupying a container which is 500. ml in size. What is the pressure of this gas in atmospheres? 27. When sodium bicarbonate, NaHCO 3 (s), is heated. Sodium carbonate (Na 2 CO 3 ) is produced, with the evaluation of water vapor and carbon dioxide gas. 2NaHCO 3 (s) Na 2 CO 3 (s) + H 2 O(l) + CO 2 (g) What total volume of gas, measured at 29 C and 769 torr, is produced when 1.50g of NaHCO 3 (s) is completely converted to Na 2 CO 3 (s)? 28. Suppose that 4.18g of oxygen gas and 3.68g of nitrogen gas are confined in a 11.3-L container at 36 C. What would be the pressure of container? Calculate the partial pressure of each gas in this mixture.