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Name: _____________________ Date: _______________ AP Chemistry-Chapter 6 MC Questions Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 1. Which periodic group or series of elements is not correctly matched with its common family name? IIA a. alkaline earth metals IIIA b. alkali metals lanthanides 58Ce - 71Lu c. halogens VIIA d. VIIIA e. noble gases ____ 2. Of the following, which element does not match its designation? representative metal a. 38Sr In representative nonmetal b. 49 metalloid c. 14Si d-transition metal d. 74W f-transition metal e. 90Th ____ 3. Of the following, which periodic group(s) do not match their designation? a. d-transition metals IIIB IIB IA, IIA b. representative metals VIIIB c. noble gases IIA d. alkaline earth metals halogens VIIA e. ____ 4. __________ is a noble gas. a. 22Ti b. 42Mo c. 81Tl d. 36Kr e. 92U ____ 5. __________ is an actinide. a. 22Ti b. 42Mo c. 81Tl d. 36Kr e. 92U ____ 6. Which one of the following is an inner transition (f-transition) element? a. Rb b. Ho c. Co d. Ru e. Bi ____ 7. What would be the outer electron configuration of group IIIB (Sc, Y, La . . .)? a. ns2nd2np0 b. nd1ns2 c. ns2(n-1)d1 d. ns1np3 e. (n-1)d1ns2 ____ 8. What would be the outer electron configuration of alkaline earth metals? a. ns2np2 b. np2 c. ns0np2 d. nd2 e. ns2 ____ 9. Choose the term that best describes all members of this series of elements: K, Ca, Ba, Cl, N a. b. c. d. e. metalloids d-transition elements alkaline earth metals alkali metals representative elements ____ 10. Which of the following statements is false? a. The effective nuclear charge experienced by an electron in an outer shell is less than the actual nuclear charge. b. Within a family (vertical group in the periodic table) of representative elements atomic radii increase from top to bottom. c. Electrons in inner shells screen, or shield, electrons in outer shells from the full effect of the nuclear charge. d. The atomic radii of representative elements decrease from left to right across a period (horizontal row in the periodic table). e. Transition elements have larger atomic radii than the preceding IA and IIA elements in the same period because transition elements have electrons in their d orbitals. ____ 11. Which element has the largest atomic radius? a. Al b. Si c. P d. S e. Cl ____ 12. Which element has the largest atomic radius? a. F b. Cl c. Sn d. Kr e. Se ____ 13. Which element has the smallest radius? a. Na b. Mg c. Al d. Si e. P ____ 14. Arrange the following elements in order of increasing atomic radii. Sr, Rb, Sb, I, In a. b. c. d. e. Rb < Sr < In < Sb < I I < Sb < In < Rb < Sr In < Sb < I < Sr < Rb Sb < I < In < Sr < Rb I < Sb < In < Sr < Rb ____ 15. The first ionization energy of sulfur is less than that of phosphorus. A reasonable explanation for this fact involves a. the stability of the half-filled subshell in atomic sulfur. b. pairing of two electrons in one 3p orbital in sulfur atoms. c. the smaller size of sulfur atoms relative to phosphorus atoms. d. the ease with which phosphorus attains a noble gas electronic configuration. e. the higher electronegativity of sulfur relative to phosphorus. ____ 16. Which element has the highest first ionization energy? a. Be b. B c. C d. N e. O ____ 17. The amount of energy absorbed in the process in which an electron is added to a neutral gaseous atom is defined as __________. a. shielding effect b. electronegativity c. electron affinity d. first ionization energy e. standard reduction potential ____ 18. Which one of the following species is not isoelectronic with neon? a. Mg2+ b. Na+ c. O2d. Cle. Al3+ ____ 19. Which ion has the largest radius? a. O2b. S2c. Se2d. Te2e. Po2- ____ 20. Consider the group of ions that are isoelectronic with krypton. Which response contains all the true statements and no others? I. II. III. IV. V. a. b. c. d. e. The ion with the highest positive charge is the largest ion. The ion with the highest atomic number bears the highest positive charge. The ion with the lowest atomic number bears the least negative charge. The ion with a 1- charge is obtained by adding one electron to a Group VIIA element. All the ions have a noble gas electronic configuration. II and III I, II, and V II, IV, and V I and IV II, III, IV, and V ____ 21. Which ion has the smallest radius? a. As3b. Se2c. Brd. Rb+ e. Sr2+ ____ 22. A property that measures the ability of an atom to attract electrons in a chemical bond is a. binding energy. b. mass defect. c. electron affinity. d. ionization energy. e. electronegativity. ____ 23. Which element has the highest electronegativity? a. N b. Si c. As d. P e. C ____ 24. Which pair of elements below would be least likely to form an ionic bond between them? a. Na and S b. C and N c. Al and F d. Mg and Br e. Cs and O ____ 25. In general, ionization energies a. increase down a group and increase across a period. b. increase down a group and decrease across a period. c. decrease down a group and increase across a period. d. decrease down a group and decrease across a period. e. increase with atomic mass and increase with atomic radii. ____ 26. In general, atomic radii a. increase down a group and decrease across a period. b. increase down a group and increase across a period. c. decrease down a group and decrease across a period. d. are proportional to atomic mass. e. decrease down a group and increase across a period. ____ 27. Which of the following chemical expressions refers to the first ionization energy of calcium? a. Ca(s) Ca+(s) + eb. Ca(g) + e- Ca+(g) c. Ca(s) + e- Ca+(s) d. Ca(g) Ca+(g) + ee. Ca(g) Ca2+(g) + e____ 28. Which statement is false? a. Cations are smaller than their corresponding neutral atom. b. Anions are smaller than their corresponding neutral atom. c. Mg2+ is larger than Be2+. d. O2- is larger than F-. e. Br- is smaller than I-. ____ 29. Which element has the largest first ionization energy? a. Be b. Ca c. Mg d. Sr e. Ba ____ 30. The change in energy for the following reaction is referred to as the ____ for fluorine. F(g) + ea. b. c. d. e. F-(g) oxidation energy electron affinity electronegativity energy first ionization energy second ionization energy