Review - 1 (Basics)

AP chem Text: chapter 1 & 2 PROBLEMS 1. In most of its compounds, this element exists as a monoatomic cation. a. O b. Cl c. Na d. N e. I 2. 3. 4. 5. 6. 7. This element may form a compound with the formula CaXO4. a. Se b. Cl c. P d. Na e. He Which of the following elements may occur in the greatest number of different oxidation states? a. C b. F c. O d. Ca e. Na Choose the group that does not contain isotopes of the same element. a. atom I = 18 p, 18 n atom II = 18 p, 19 n b. atom I = 25 p, 30 n atom II = 25 p, 31 n c. atom I = 37 p, 42 n atom II = 37 p, 41 n d. atom I = 82 p, 126 n atom II = 82 p, 128 n e. atom I = 18 p, 18 n atom II = 17 p, 18 n Which of the following groups has the species correctly listed in order of increasing radius? 2+ 2+ 2+ a. Mg , Ca , Ba + + + b. K , Na , Li c. Br , Cl , F d. Na, Mg, Al 2+ 3+ e. Fe, Fe , Fe Which of the following elements has the lowest electronegativity? a. C b. K c. Al d. I e. F Which ion has the largest radius? a. F 3+ b. Al + c. K 2d. O e. I Review - 1 (Basics) 8. What is the name of the energy change when a gaseous atom, in the ground state, adds an electron? a. ionization energy b. sublimation energy c. atomization energy d. electron affinity e. lattice energy 9. The following ionization energies are reported for element X. (All the st nd values are in kJ/mol.) 1 = 500, 2 rd th th = 4560, 3 = 6910, 4 = 9540, 5 = 13400. Based on the above information, the most likely identity of X is a. Mg b. Cl c. Al d. Na e. Si 10. In general, as atomic number increases within a period, atomic radius a. first increases then decreases b. increases c. first decreases then increases d. does not change e. decreases 11. This element is a reactive gas a. Chlorine b. Gold c. Sodium d. Radon e. Radium 12. This element is an unreactive metal a. Chlorine b. Gold c. Sodium d. Radon e. Radium 13. Which of the following represents the correct formula for potassium trisoxalatoferrate(III)? a. P3[Fe(C2O4)3] b. K3[Fe(C2O4)3] c. KFe3(C2O4)3 d. K3FeO3 e. K3[Fe3(C2O4)3] 14. Which of the following substances will produce a colorless aqueous solution? a. Zn(NO3)2 b. CuSO4 c. K2Cr2O7 d. Co(NO3)2 e. NiSO4 Name: ____________________ 15. This element is a liquid at room temperature a. Hg b. Th c. Na d. Cl e. Co 16. This element is present in chlorophyll. a. K b. Ga c. Fe d. Mg e. Al 17. This element forms a protective oxide coating. a. K b. Ga c. Fe d. Mg e. Al 18. This element is used to improve the conductivity of germanium. a. K b. Ga c. Fe d. Mg e. Al 19. Which of the following aqueous solutions is blue? a. CuSO4 b. Cr2(SO4)3 c. NiSO4 d. ZnSO4 e. CoSO4 20. In order to separate two substances by fractional crystallization, the two substances must differ in which of the following? a. Solubility b. Specific gravity c. Vapor pressure d. Viscosity e. Freezing point 21. In a flame test, copper compounds impart which of the following colors to a flame? a. red b. orange c. blue to green d. violet e. yellow 22. What should you do if you spill sulfuric acid on the countertop? a. Neutralize the acid with vinegar. b. Sprinkle solid NaOH on the spill. c. Neutralize the acid with NaHCO3 solution. d. Neutralize the acid with Epsom salt (MgSO4) solution. e. Use paper towels to soak up the acid. 23. Which of the following can be achieved by using a visible-light spectrophotometer? i. Detecting the presence of isolated double bonds. ii. Finding the concentration of a KMnO4 solution. iii. Running a flame test to + + determine if Na or K is in a solution. a. iii only b. ii only c. i only d. ii and iii e. i and ii 24. You are given an aqueous solution of NaCl. The simplest method for the separation of NaCl from the solution is a. evaporation of the solution to dryness b. centrifuging the solution c. osmosis of the solution d. electrolysis of the solution e. filtration of the solution 25. The determination that atoms have small, dense nuclei is attributed to a. Rutherford b. Becquerel c. Einstein d. Dalton e. Bohr FREE-RESPONSE 26. Use the periodic table and other information concerning bonding and electronic structure to explain the following observations. 3+ 2+ a. The radii of the iron cations are less than that of an iron atom, and Fe is smaller than Fe . b. When moving across the periodic table from Li to Be to B, the first ionization energy increases from Li to Be, then drops for B. The first ionization energy of B is greater than that of Li. c. The electron affinity of F is higher than the electron affinity of O. d. The following observations have been made about the lattice energy and ionic radii of the compounds listed below. Compare NaF to CaO, and then compare CaO to BaO. All of the solids adopt the same crystal structure. compound cation radius (pm) anion radius (pm) lattice energy (kJ/mol) NaF 116 119 911 CaO 114 126 3566 BaO 149 126 3202 27. Name the following: a. Na2O b. MgCl2 c. CO d. SO3 e. P4O10 f. HCl(g) g. H2S(g) h. HCl(aq) 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. C A A E A B E D D E A B B A A D E B A A C C B A A i. j. k. l. m. n. o. p. H2S(aq) H2SO4(aq) H2SO3(aq) HNO3(aq) HNO2(aq) H3PO4(aq) Na2SO4 Na2SO3 q. r. s. t. u. v. w. x. KNO3 KNO2 (NH4)3PO4 Al2O3 (NH4)2SO4 MnO2 FeCl2 FeCl3 26. a. The observed trend of radii is: Fe > Fe2+ > Fe3+. There is an increase in the effective nuclear charge in this series. As electrons are removed, the repulsion between the electrons decreases. The larger the effective nuclear charge, the more the electrons are pulled towards the nucleus and the smaller the atom or ion becomes. b. When moving across a period on the periodic table, the value of the effective nuclear charge increases with atomic number. This causes a general increase from Li to Be to B. The even higher value of Be is due to the increases stability of the electron configuration of Be. Be has a filled s-subshell. Filled subshells have an increased stability and additional energy is required to pull an electron away. c. The effective nuclear charge in F is greater than the effective nuclear charge in O. This causes a greater attraction of the electrons. d. Because all the solids adopt the same structure, the structure is irrelevant. The sizes of the anions are smaller; thus, anion size arguments are not important. Two factors, other than structure, are important. The two compounds with the highest lattice energies contain divalent ions (+2 or -2) while NaF contains univalent ions (+1 or -1). The higher the charge is, the greater the attraction between the ions is. The lattice energy increases as the attraction increases. The difference between the CaO and BaO values is because the larger the ion is, the lower the attraction is (greater separation). The lower attraction leads to a lower lattice energy.