1st Semester Review 2014-2015 Worth 10% of Exam Score Name: P: 1. Which of the following is the correct electron configuration for a neutral atom of oxygen in the ground state? A) 1s 2 2p 4 B) 1s 2 2s 4 C) 1s 2 2s 2 2p 2 D) 1s 2 2s 2 2p 4 E) 1s 2 2s 2 2p 6 3s 2 3p 4 2. The species having the same number of electrons as Mg 2+ is A) Na B) O 2 C) N D) Ar E) Ne 1+ 3. Which of the species is the most stable? A) He(g) B) He + (g) C) Ne(g) D) Ne + (g) E) Xe(g) 4. What is the Lewis electron dot diagram for the sulfide ion? E) 5. What is the number of electrons in an atom that has 3 protons and 4 neutrons? A) 1 B) 7 C) 3 D) 4 6. Which subatomic particles are located in the nucleus of an He-4 atom? A) electrons and neutrons B) electrons and protons C) neutrons and protons D) neutrons, protons, and electrons 7. Each diagram below represents the nucleus of a different atom. Which diagrams represent nuclei of the same element? A) D and E, only B) D, E, and Q C) Q and R, only D) Q, R, and E 8. When compared with the energy of an electron in the first shell of a carbon atom, the energy of an electron in the second shell of a carbon atom is A) less B) greater C) the same 9. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 10. Which list includes elements with the most similar chemical properties? A) Br, Ga, Hg B) Cr, Pb, Xe C) O, S, Se D) N, O, F 11. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have A) fewer valence electrons B) more valence electrons C) fewer D) more 12. Which two elements have the most similar chemical properties? A) Be and Mg B) Ca and Br C) Cl and Ar D) Na and P 13. Which Lewis electron-dot diagram represents calcium oxide? 14. Which element, represented by X, reacts with fluorine to produce the compound XF2? A) aluminum B) argon C) magnesium D) sodium 15. As the elements of Group 17 are considered in order of increasing atomic number, there is an increase in A) atomic radius B) electronegativity C) first ionization energy D) number of electrons in the first shell Page 1
16.Which two notations represent different isotopes of the same element? A) and B) and C) and D) and 17. Which element forms a compound with chlorine with the general formula MCl A) Rb B) Ra C) Re D) Rn 18. Which formula represents strontium phosphate? A) SrPO4 B) Sr3PO8 C) Sr2(PO4)3 D) Sr3(PO4)2 19. In which compound is the ratio of metal ions to nonmetal ions 1 to 2? A) calcium bromide B) calcium oxide C) calcium phosphide D) calcium sulfide 20. What is the total number of different elements present in? A) 7 B) 9 C) 3 D) 4 21. An unknown element X can form a compound with the formula XBr3. In which group on the Periodic Table would element X be found? A) 1 B) 2 C) 13 D) 14 22. What is the chemical formula of iron(iii) sulfide? A) FeS B) Fe2S3 C) FeSO3 D) Fe2(SO3)3 23. Which formula represents copper(i) oxide? A) CuO B) CuO2 C) Cu2O D) Cu2O2 24. Which formula represents lead(ii) chromate? A) PbCrO4 B) Pb(CrO4)2 C) Pb2CrO4 D) Pb2(CrO4)3 25. What is the IUPAC name for the compound FeS? A) iron(ii) sulfate B) iron(iii) sulfate C) iron(ii) sulfide D) Iron(III) sulfide 26. A correct name for N2O3 is A) nitrogen (I) oxide B) nitrogen (II) oxide C) nitrogen (III) oxide D) nitrogen (IV) oxide 27. The molecular formula of glucose is C6H12O6. What is the empirical formula of glucose? A) CHO B) CH2O C) C6H12O6 D) C12H24O12 28. What is the molecular formula of a compound that has a molecular mass of 54 and the empirical formula C2H3? A) C2H3 B) C4H6 C) C6H9 D) C8H12 29. What is the mass in grams of 2.0 moles of NO2? A) 92 B) 60. C) 46 D) 30. 30. The total number of moles represented by 20 grams of CaCO3 is A) 1 B) 2 C) 0.1 D) 0.2 31. What is the empirical formula of a compound that contains 28% iron, 24% sulfur, and 48% oxygen by mass? A) FeSO3 B) FeSO4 C) Fe2(SO3)3 D) Fe2(SO4)3 32. A compound consists of 25.9% nitrogen and 74.1% oxygen by mass. What is the empirical formula of the compound? A) NO B) NO2 C) N2O D) N2O5 33. What is the percent composition by mass of hydrogen in NH4HCO3 (gram-formula mass = 79 grams/mole)? A) 5.1% B) 6.3% C) 10.% D) 50.% 34. The percentage by mass of Br in the compound AlBr3 is closest to A) 10.% B) 25% C) 75% D) 90.% 35. Which element forms an ionic compound when it reacts with lithium? A) K B) Fe C) Kr D) Br 36. An ionic compound is formed when there is a reaction between the elements A) strontium and chlorine B) hydrogen and chlorine C) nitrogen and oxygen D) sulfur and oxygen 37. Which substance contains bonds that involved the transfer of electrons from one atom to another? A) CO2 B) NH3 C) KBr D) Cl2 38. Which formula represents a nonpolar molecule containing polar covalent bonds? A) H2O B) CCl4 C) NH3 D) H2 Page 2
39. Based on bond type, which compound has the highest melting point? A) CH3OH B) C6H14 C) CaCl2 D) CCl4 40. A solid substance was tested in the laboratory. The test results are listed below. dissolves in water is an electrolyte melts at a high temperature Based on these results, the solid substance could be A) Cu B) CuBr2 C) C D) C6H12O6 41. Which molecule has a nonpolar covalent bond? 42. Two atoms of element A unite to form a molecule with the formula A2. The bond between the atoms in the molecule is A) electrovalent B) ionic C) nonpolar covalent D) polar covalent 43. Given the formula representing a molecule: The molecule is H C C H A) symmetrical and polar B) symmetrical and nonpolar C) asymmetrical and polar D) asymmetrical and nonpolar 44. Which formula represents a nonpolar molecule? A) HCl B) H2O C) NH3 D) CH4 45. Which formulas represent two polar molecules? A) CO2 and HCl B) CO2 and CH4 C) H2O and HCl D) H2O and CH4 46. Which particle has the least mass? C) 1 0n D) 0-1e 47. Which of the following sublevels has the highest energy? A) 2p B) 2s C) 3p D) 3s 48. Energy is absorbed when an electron moves from a 3d sublevel to a A) 1s sublevel B) 2s sublevel C) 3p sublevel D) 4p sublevel 49. Which electron configuration represents an atom of lithium in an excited state? A) 1s 1 2s 1 B) 1s 1 2s 2 C) 1s 2 2s 1 D) 1s 2 2s 2 50. The bright-line spectrum of sodium is produced when energy is A) absorbed as electrons move from higher to lower B) absorbed as electrons move from lower to higher C) released as electrons move from higher to lower D) released as electrons move from lower to higher 51. Which equation represents a single replacement reaction? A) B) C) D) 52. Given the balanced equations representing two chemical reactions: Cl2 + 2NaBr 2NaCl + Br2 2NaCl 2Na + Cl2 Which type of chemical reactions are represented by these equations? A) single replacement and decomposition B) single replacement and double replacement C) synthesis and decomposition D) synthesis and double replacement 53. Given the balanced equation representing a reaction: 4Al(s) + 3O2(g) 2Al2O3(s) Which type of chemical reaction is represented by this equation? A) double replacement B) single replacement C) substitution D) synthesis Page 3
54. Given the incomplete equation representing a reaction: 55. Given the unbalanced equation: 2C6H14 + O2 12CO2 + 14H2O What is the coefficient of O2 when the equation is completely balanced using the smallest whole-number coefficients? A) 13 B) 14 C) 19 D) 26 When the equation is correctly balanced using the smallest whole-number coefficients, what is the coefficient of CO? A) 1 B) 2 C) 3 D) 4 Page 4
Answer Key HC 1st Semester Final MC Review 2014-2015 1. D 2. B 3. A 4. B 5. C 6. C 7. B 8. B 9. B 10. C 11. A 12. A 13. D 14. C 15. A 16. A 17. A 18. D 19. A 20. C 21. C 22. B 23. C 24. A 25. C 26. C 27. B 28. B 29. A 30. D 31. D 32. D 33. B 34. D 35. D 36. A 37. C 38. B 39. C 40. B 41. A 42. C 43. B 44. D 45. C 46. D 47. C 48. D 49. B 50. C 51. C 52. A 53. D 54. C 55. C Page 5