2 Which electron configurations represent the first two elements in Group 17 (VIIA) of the Periodic Table?

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1 CHE-100 Review Questions 1 The total number of orbitals found in an f sublevel is A) 5 B) 3 C) 7 D) 1 2 Which electron configurations represent the first two elements in Group 17 (VIIA) of the Periodic Table? A) 1s 2 2s 2 2p 5 and [Ne] 3s 2 3p 5 B) 1s 2 2s 1 and 1s 2 2s 2 C) 1s 2 2s 2 2p 6 and [Ne] 3s 2 3p 5 D) 1s 2 2s 2 and 1s 2 2s 2 2p 1 3 Which type of bond is contained in a water molecule? A) electrovalent B) nonpolar covalent C) ionic D) polar covalent 4 Which orbital notation correctly represents the outermost principal energy level of a sulfur atom in the ground state? A) B) C) D) 5 The total number of sodium atoms in 46.0 grams of sodium is A) 12.0 x B) 3.01 x C) 24.0 x D) 6.02 x The maximum number of electrons that may be found in the third principal energy level is A) 32 B) 2 C) 8 D) Which Kelvin temperature is equal to -33 C? A) 33 K B) 306 K C) 240 K D) -33 K 8. Which 1-mole sample of atoms requires the least energy to form a mole of positive ions? A) K B) Ga C) Ca D) Ge 9. Two atoms of element A unite to form a molecule with the formula A 2. The bond between the atoms in the molecule is A) ionic B) nonpolar covalent C) polar covalent D) electrovalent

2 10. How many milliliters of 0.4 M HC1 are required to completely neutralize 200 milliliters of 0.16 M potassium hydroxide? A) 200 B) 500 C) 80 D) Which formula represents a polar molecule containing polar covalent bonds? A) H 2 O B) Cl 2 C) CO 2 D) NaCl 12. The arrangement of the elements in the present Periodic Table is based on atomic A) radius B) mass C) density D) number 13. A cube has a volume of 8.0 cm 3 and a mass of 21.6 grams. The density of the cube, in grams per cubic centimeter, is best expressed as A) B) 2.7 C) 0.37 D) Which element forms a diatomic molecule containing a triple covalent bond? A) oxygen B) chlorine C) nitrogen D) hydrogen 15. Which measurement contains a total of three significant figures? A) g B) 0.01 g C) g D) g 16. Which formula represents a polar molecule? A) N 2 B) CH 4 C) Cl 2 D) NH The most active metal in Group 2 (IIA) is A) Ca B) Ba C) Mg D) Sr 18. In the ground state, how many electrons are in the outermost s sublevel of each element in Group VIIA? A) 7 B) 5 C) 2 D) Which molecule is a dipole? A) CH 4 B) N 2 C) H 2 D) HC1 20. Which principal energy level has a maximum of three sublevels? A) 3 B) 4 C) 2 D) In the balanced equation: 2Na + 2H 2 O H 2 + 2X, the compound represented by X is A) NaH B) NaOH C) Na 2 O D) Na 2 O 2

3 22. What is the total number of valence electrons in an atom of phosphorus in the ground state? A) 7 B) 3 C) 5 D) What is the formula of nitrogen (I) oxide? A) NO B) NO 2 C) N 2 O 4 D) N 2 O 24. Proceeding from left to right in Period 2 of the Periodic Table, the covalent radius of the elements generally A) remains the same B) decreases C) increases 25. All atoms of Group IIA elements in the ground state have the same number of electrons in which principal energy level? A) 1 B) 3 C) 2 D) Which procedure represents the safest technique to use for diluting a concentrated acid? A) Add the acid to the water quickly B) Add the water to the acid quickly. C) Add the water slowly to the acid with steady stirring. D) Add the acid slowly to the water with steady stirring. 27. Which is the formula for magnesium sulfide? A) MgSO 3 B) MgS C) MnS D) MnSO Which element in Period 4 of the Periodic Table exhibits the most nonmetallic properties? A) Cr B) Ca C) Br D) Ga 29. Compounds with the greatest fluorine reacts with ionic character would form when A) metalloids (semimetals) B) noble gases C) Group 13 (IIIA) elements D) alkali metals 30. Which formula represents a mixture? A) H 2 O (l) B) NaCl(aq) C) H 2 O(s) D) NaCl (s) 31. The greatest absorption of energy occurs as an electron moves from A) 4s to 3p B) 4d to 4s C) 1s to 3s D) 3p to 3s 32. The total number of orbitals in the 4f sublevel is A) 1 B) 3 C) 5 D) 7

4 33. During a titration, a student used 50.0 milliliters of 0.1 M acid. How many moles of acid, expressed to proper significance, were used? A) B) C) D) Which electron configuration represents an atom in the excited state? A) 1s 2 2s 2 2p 6 3s 2 B) 1s 2 2s 2 3s 1 C) 1s 2 2s 1 D) 1s 2 2s 2 2p Which substance is made up of molecules that are dipoles? A) CO 2 B) CH 4 C) N 2 D) H 2 O 36. An electron in an atom will emit energy when it moves from energy level A) 2p to 1s B) 2s to 2p C) 2p to 3s D) 2s to 3p 37. An atom that has an electron configuration of is 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 is classified as A) an alkali metal B) a transition element C) a noble gas element D) an alkaline earth metal 38. How many moles of hydrogen atoms are there in one mole of C 6 H 12 O 6 molecules? A) 24 x (6.0 x ) B) 24 C) 12 D) 12 x (6.0 x ) 39. Which orbital notation represents the outermost principal energy level of a phosphorus atom in the ground state? A) B) C) D) 40. Which period contains three elements that commonly exist as diatomic molecules? A) Period 1 B) Period 2 C) Period 4 D) Period Using the rules for significant figures, the sum of gram and gram should be expressed as A) gram B) 0.03 gram C) gram D) gram 42. What is the electron configuration for Be 2+ ions? A) 1s 1 B) 1s 2 2s 2 C) 1s 2 D) 1s 2 2s 1

5 43. The maximum number of electrons that a single orbital of the 3d sublevel may contain is A) 5 B) 2 C) 3 D) In the laboratory, a student determined the percent by mass of water in a hydrated salt to be 17.3 percent. If the accepted value is 14.8 percent, the percent error is A) B) 5.92% C) 27.1% D) What is the mass number of a 1 3 H atom? A) 1 B) 4 C) 3 D) More than two-thirds of the elements of the Periodic Table are A) noble gases B) metals C) metalloids D) nonmetals 47. Which piece of laboratory apparatus would most likely be used to evaporate a 1-milliliter sample of a solution to dryness? A) buret B) pipette C) volumetric flask D) watch glass 48. Which atom in the ground state contains only one orbital that is partially occupied? A) Ne B) Si C) Na D) Ca 49. When a sodium atom becomes an anion, the size of the atom A) decreases by gaining an electron B) decreases by losing an electron C) increases by loosing an electron D) increases by gaining an electron 50. Given the reaction: 2H 2 (g) + O 2 (g) 2H 2 O (g) How many liters of H 2 (g) are required to produce a total of 10.0 liters of H 2 O(g)? A) 2.0 B) 1.0 C) 20.0 D) Which element in Period 2 is the most active metal? A) lithium B) beryllium C) neon D) fluorine 52. Given the reaction: (NH 4 ) 2 CO 3 2NH 3 + CO 2 + H 2 O what is the minimum amount of ammonium carbonate that reacts to produce 1.0 mole of ammonia? A) 0.25 moles B) 34 moles C) 0.50 moles D) 17 moles 53. The maximum number of electrons that may be found in the third principal energy level is A) 32 B) 8 C) 2 D) A fluoride ion (F 1- ) ion has the same electron configuration as A) Cl B) Na +1 C) Cl 1- D) Na

6 55. Given the reaction: 2Na + 2H 2 O 2NaOH + H 2 What is the-total number of moles of hydrogen produced when 4 moles of sodium react completely? A) 4 B) 1 C) 2 D) Given the following titration data: Volume of base (KOH) = 40.0 ml Molarity of base = 0.20 M Volume of acid (HC1) added 20.0 ml The concentration of HC1 required for the acid to neutralize the base is A) 0.10 M B) 1.0 M C) 0.20 M D) 0.40 M 57. Which represents the greatest mass of chlorine? A) 1 atom of chlorine B) 1 mole of chlorine C) 1 gram of chlorine D) 1 molecule of chlorine 58. Which is a formula of a binary compound? A) MgCl 2 B) BiPO 4 C) BaSO 4 D) Mg(ClO) Which of the following atoms will lose an electron most readily? A) potassium B) calcium C) strontium D) rubidium 60. If X is the represents symbol of an element, which pair correctly isotopes of X? A) X and X B) X and X C) X and X D) X and X 61. Which is the equivalent of calories? A) 75.0 kcal B) kcal C) 7.50 kcal D) kcal 62. When the equation C 2 H 4 + O 2 CO 2 + H 2 O is balanced using the smallest whole numbers, what is the coefficient of the O 2? A) 4 B) 1 C) 2 D) What type of bonding is found in the molecule HBr? A) nonpolar covalent B) ionic C) polar covalent D) metallic 64. What is the mass, in grams, of 1.0 mole of (NH 4 ) 2 S? A) 54 B) 68 C) 64 D) The volume of an acid required to neutralize exactly milliliters (ml) of a base could be measured most precisely if it were added to the base solution from a A) 100 ml graduated cylinder B) 50 ml beaker C) 125 ml Erlenmeyer flask D) 50.0 ml burete

7 66. Atoms of which of the following elements have the strongest attraction for electrons? A) chlorine B) aluminum C) sodium D) silicon 67. Which sequence of atomic numbers represents elements which have similar chemical properties? A) 19, 23, 30, 36 B) 3, 12, 21, 40 C) 4, 20, 38, 88 D) 9, 16, 33, Which is the correct formula for iron (III) sulfate? A) Fe 3 SO 4 B) Fe(SO 4 ) 3 C) Fe 2 SO 4 D) Fe 2 (SO 4 ) Which gas sample contains a total of 3.0 x molecules? A) 14 g of N 2 B) 38 g of F 2 C) 71 g of Cl 2 D) 2.0 g of H The nucleus of an atom consists of 8 protons and 6 neutrons. The total number of electrons present in a neutral atom of this element is A) 6 B) 2 C) 8 D) Which of the following particles has the smallest radius? A) Na 0 B) Na 1+ C) K 0 D) K Which electron notation represents the valence electrons of a phosphorus atom in the ground state? A) B) C) D) 73. In an experiment the gram atomic mass of magnesium was determined to be Compared to the accepted value 24.3, the percent error for this determination was A) B) 24.7 C) 1.65 D) Which bond has the greatest degree of ionic character? A) Li Br B) S O C) H C1 D) F F 75. What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons?

8 A) 21 B) 45 C) 42 D) A compound has an empirical formula of CH 2 and a molecular mass of 56. What is its molecular formula? A) C 2 H4 B) CH 2 C) C 3 H 6 D) C 4 H How many grams of ammonium chloride (molecular formula mass = 53.5 g) are contained in L of a 2.00 M solution? A) 53.5 g B) 10.0 g C) 107 g D) 26.5 g 78. The number of calories needed to raise the temperature of 10 grams of water from 20 C to 30 C is A) 20 B) 40 C) 100 D) An ionic bond forms between atoms of A) P and C1 B) I and Cl C) H and C1 D) K and Cl 80. Which of the following best describes exothermic chemical reactions? A) They always release heat. B) They never release heat. C) They never occur spontaneously. D) They always occur spontaneously. 81. Which sample of O 2 contains a total of 3.01 x molecules at STP? A) 2.00 moles B) 16.0 grams C) 1.00 mole D) 32.0 grams 82. What is the ratio by mass of carbon to hydrogen in the compound C 2 H 6? A) 1:4 B) 6:2 C) 4:1 D) 2:6 83. Which is the electron configuration of a transition element? A) B) C) D) Which is an empirical formula? A) Al 2 Cl 6 B) C 2 H 2 C) C 2 H 4 D) K 2 O 85. Given the unbalanced equation: Al 2 (SO 4 ) 3 + Ca (OH) 2 A1(OH) 3 + CaSO 4 When the equation is completely balanced using the smallest whole-number coefficients, the sum of the coefficients is A) 3 B) 5 C) 9 D) Why is NH 3 classified as a polar molecule? A) Nitrogen and hydrogen are both nonmetals. B) NH 3 molecules have asymmetrical charge distributions. C) N H bonds are nonpolar. D) NH 3 is a gas at STP.

9 87. Which of the following atoms has the greatest nuclear charge? A) 14 7N B) 12 6C C) 4 2He D) 2 1 H 88. Which formula represents an ionic compound? A) NH 3 (g) B) H 2 O(l) C) NaCl (s) D) CCl 4 CHE-100 Review Questions Answer Key 1. C 2. A 3. D 4. B 5. A 6. D 7. C 8. A 9. B 10. C 11. A 12. D 13. B 14. C 15. A 16. D 17. B 18. C 19. D 20. A 21. B 22. C 23. D 24. B 25. A 26. D 27. B 28. C 29. D 30. B 31. C 32. D 33. A 34. B 35. D 36. A 37. B 38. C 39. A 40. B 41. D 42. C 43. B 44. A 45. C 46. B 47. D 48. C 49. B 50. D 51. A 52. C 53. D 54. B 55. C 56. D 57. B 58. A 59. D 60. C 61. B 62. D 63. C 64. B 65. D 66. A 67. C 68. D 69. A 70. C 71. B 72. D 73. C 74. A 75. B 76. D 77. A 78. C 79. D 80. A 81. B 82. C 83. A 84. D 85. C 86. B 87. A 88. C

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