273 TC. Mass Length Volume 1 lb = g * 1 in = 2.54 cm 1 L = qt* 1 kg = lb * 1 m = yd * 1 ft 3 = L * 1 mi = 1.

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1 Chem 106 Midterm Study Questions Name: Chapters 1-5,11-12 Review Mon 10/10/2016 Due 10/13/2016 (Midterm exam) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach the work to these. Useful information to be provided on exam: T F 1.8T 32 C T C TF 32 TK TC 273 TC TK Mass Length Volume 1 lb = g * 1 in = 2.54 cm 1 L = qt* 1 kg = lb * 1 m = yd * 1 ft 3 = L * 1 mi = km * 1. Define the following terms: a. science b. chemistry 2. Write 8,353 in standard scientific notation. A) 8353 B) C) D) E) The number expressed in scientific notation is A) B) C) D) E) Page 1

2 kilograms contain this many grams. A) B) C) D) E) Convert: 1.0 mm = km. A) km B) km C) km D) km E) km 6. Convert m to decimeters. A) dm B) dm C) dm D) dm milliseconds is equal to how many seconds? A) s B) s C) s D) s E) 0.69 s 8. Using the rules of significant figures, calculate the following: = A) 76 B) 80 C) D) 77 E) Page 2

3 9. The number rounded to four significant figures is A) B) C) D) How many significant figures are in the number ? A) 1 B) 2 C) 3 D) 4 E) A student finds that the weight of an empty beaker is g. She places a solid in the beaker to give a combined mass of g. To how many significant figures is the mass of the solid known? A) 1 B) 2 C) 3 D) 4 E) The product of will have how many significant figures? A) 2 B) 3 C) 23 D) E) Convert: K = o C. A) o C B) 49.3 o C C) o C D) o C E) o C Page 3

4 14. Convert: 37.5 o F = o C. A) 38.6 o C B) 3.1 o C C) o C D) 9.9 o C E) o C 15. An object is inches in height. Express this height in centimeters. A) cm B) cm C) 8.76 cm D) cm E) cm o F is equivalent to A) o C B) o C C) o C D) o C E) o C 17. What is the mass in pounds of a human who weighs kg? A) lb B) lb C) lb D) lb 18. The density of gold is 19.3 g/ml. What is the volume of a gold nugget that weighs 73.8 g? A) ml B) 3.82 ml C) ml D) 54.5 ml Page 4

5 19. A graduated cylinder contains 20.0 ml of water. An irregularly shaped object is placed in the cylinder, and the water level rises to the 31.2-mL mark. If the object has a mass of 96.3 g, what is its density? A) 8.60 g/ml B) g/ml C) 3.09 g/ml D) 4.81 g/ml 20. Which of the following is a chemical change? A) Water condenses on a mirror. B) A damp towel dries. C) Peanuts are crushed. D) A tin can rusts. E) At least two of the above (a-d) exhibit a chemical change. 21. If iodine melts at 114 C and boils at 184 C, what is its physical state at 120 C? 22. Which of the following is an element? A) air B) water C) salt D) helium E) sugar 23. Which is an example of a homogeneous mixture? A) vodka B) oily water C) soil (dust) D) sodium chloride E) aluminum 24. True or False? The normal boiling point of water is 100 o C, which is a physical property of the substance water. A) True B) False Page 5

6 25. True or False? Metal rusting is an example of a chemical change. A) True B) False 26. Which statement below is incorrect? A) Dalton's statement "All atoms of a given element are identical" is no longer accepted because of the existence of isotopes and ions. B) O3 (ozone) is considered a molecule but is not considered an element. C) The number in the measurement "12 apples" has an infinite number of significant figures. D) Rutherford's discovery revealed the atom is mostly made up of empty space. E) At least two of the above statements (a-d) are incorrect. 27. The total number of atoms indicated by the formula Ca3(PO4)2 is A) 4 B) 8 C) 12 D) 13 E) Which atomic particle determines the chemical behavior of an atom? A) proton B) electron C) neutron D) nucleus 29. Which particle has the smallest mass? A) neutron B) proton C) electron D) helium nucleus 30. An atom with 15 protons and 16 neutrons is an atom of A) P B) Ga C) S D) Pd E) Rh Page 6

7 31. A certain isotope X + contains 54 electrons and 78 neutrons. What is the mass number for this element? A) 133 B) 132 C) 131 D) 55 E) The number of protons in the nucleus of an atom is called its A) mass number B) valence C) isotope number D) atomic number 33. Which pair have approximately the same mass? A) a hydrogen, 1 H, and a deuterium, 2 1 1H, atom B) a neutron and an electron C) a proton and a neutron D) an electron and a proton 34. Which of the following elements is an alkaline earth metal? A) Ca B) Cu C) Fe D) Na E) Sc 35. Which of the following elements is most similar to chlorine? A) H B) He C) Na D) Hg E) Br 36. How many protons, electrons, and neutrons does the isotope Fe have? Page 7

8 37. The form of EMR that has a longer wavelength than infrared rays but a shorter wavelength than radio waves is A) microwaves B) untraviolet C) gamma rays D) X rays 38. Which color of visible light has the lowest frequency? A) violet B) blue C) green D) yellow E) red 39. According to the Bohr model of the atom, the energy levels of the hydrogen atom (and all atoms) are, meaning that only certain discrete energy levels are allowed. A) varied B) quantized C) ramp-like D) continuous E) two of these 40. Which of the following is a reasonable criticism of the Bohr model of the atom? A) It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. B) It does not adequately predict the line spectrum of hydrogen. C) It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. D) It does not adequately predict the ionization energy of the first-energy-level electrons for one-electron species for elements other than hydrogen. E) It shows the electrons to exist outside the nucleus. 41. The f sublevel allows a maximum of orbital(s). A) 1 B) 3 C) 5 D) 7 E) 9 Page 8

9 42. The maximum number of electrons allowed in the p sublevel of the third principal level is A) 1 B) 2 C) 3 D) 6 E) The maximum number of electrons allowed in the fourth energy level is A) 2 B) 4 C) 8 D) 18 E) The number of unpaired electrons in a nitrogen atom is A) 1 B) 2 C) 3 D) 4 E) Which below is the correct ground-state electron configuration for oxygen. A) [He]2s 2 2p 4 B) [He]2s 2 2p 6 C) [Ne]2s 2 2p 4 D) [He]3s 2 3p 4 E) [He]1s 2 2p The alkaline earth metals have how many valence electrons? A) 8 B) 7 C) 3 D) 2 E) 1 Page 9

10 47. How many electrons are in the third principal energy level (n = 3) of one atom of Fe? A) 2 B) 8 C) 14 D) When moving down a group (family) in the periodic table, the number of valence electrons A) remains constant B) increases by 2 then 8 then 18 then 32 C) doubles with each move D) decreases regularly E) changes in an unpredictable manner 49. The electron configuration for manganese is A) [Ar] 3d 7 B) 1s 2 2s 2 2p 6 3s 1 3d 6 C) [Ar] 4s 2 3d 5 D) 1s 2 2s 2 2p 6 3s 2 3d 4 E) [Ar] 4s 2 4p Which of the following atoms has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1? A) Sc B) Ca C) Sr D) Ar 51. What element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5? A) Cl B) Se C) I D) Kr E) Br Page 10

11 52. What element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2? A) Ba B) Sn C) Pb D) Po 53. Write the electron configuration for Cd. 54. Write the electron configuration for Cl. 55. Write the electron configuration for Rb. 56. Which of the following is ranked in order of largest to smallest atomic radius? A) Rb > Mn > S > Ge > F B) F > S > Ge > Mn > Rb C) Mn > Rb > F > S > Ge D) Rb > Ge > Mn > F > S E) Rb > Mn > Ge > S > F 57. Which of the following atoms has the highest ionization energy? A) Al B) Si C) P D) As E) Sb 58. Order the elements S, Cl, and F in terms of increasing ionization energy. A) S, Cl, F B) Cl, F, S C) F, S, Cl D) F, Cl, S E) S, F, Cl 59. Which has the higher ionization energy, K or Br? Page 11

12 60. True or false: Covalent bonding occurs when electrons are shared by nuclei. A) True B) False 61. True or false? The greater the difference in electronegativity between two bonded atoms, the more polar the bond. A) True B) False 62. True or false? N2 is an example of a covalent bond. A) True B) False 63. Draw the Lewis structures for the following compounds and use VSEPR theory to answer the question. CBr2H2 BH3 SO2 CS2 HCl Which compound has bond angles of around the central atom? A) CBr2H2 B) BH3 C) SO2 D) CS2 E) HCl 64. Which of the following compounds contains an ionic bond? A) HCl(g) B) NaCl C) CCl4 D) SO2 E) O2 65. The most electronegative element of those listed is A) Rb B) Cs C) Fr D) K E) Li Page 12

13 66. In ionic bonding A) the electrons are shared between the atoms. B) the atoms are repelled by each other. C) the bonding that occurs is usually between two nonmetal atoms. D) a noble gas configuration is formed for each element or ion. E) At least two of the above statements are correct. 67. Which of the following atoms has the greatest electronegativity? A) Na B) Rb C) Cl D) Se 68. Which of the following has nonpolar bonds? A) H2S B) HCl C) Br2 D) OF2 E) All are nonpolar. 69. Which of the following bonds is non-polar? A) N-H B) O-H C) F-H D) H-H E) S-H 70. True or false? The F - and O 2- ions have the same electron configuration. A) True B) False 71. The electron configuration for the bromide ion is identical to that of A) Br B) Kr C) K D) I - Page 13

14 72. Calcium reacts with fluorine to form a compound with which formula below? A) CaF B) CaF2 C) Ca2F D) Ca2F3 73. Which element or ion listed below has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6? A) S B) Ne C) Cl D) S Draw the Lewis electron structure for the sulfur atom. 75. The Lewis structure for which of the following contains the greatest number of nonbonding electrons? A) CH4 B) HF C) F2 D) H2O E) H2 Page 14

15 76. Choose the correct Lewis structure for the NH4 + ion. A) H +.. H. N.. H H B) C) D) H.. H. N. H.. H.. H. N. H.. H H. H. N. H. H Draw the Lewis electron structure for the HI molecule. 78. Draw the Lewis structure for SiH Draw the Lewis structure for Na2O. hint: there are no covalent bonds; this structure is ionic 80. Which of the following has a double bond? A) H2O B) NH3 C) O2 D) CO E) H2S Page 15

16 81. Which of the following molecules have tetrahedral geometry? (Check all that apply.) A) HBr B) NO3 C) H2O D) SiF4 E) BrO4 82. Which of the following molecules has a 120 o bond angle? (Check all that apply.) A) HBr B) NO3 C) H2O D) BF3 E) NH3 83. Draw the Lewis Structure and predict the 3-dimensional geometry of each molecule below, including bond angles. NO2 C2H4 (note: there are two central atoms) PF3 84. The charge on a barium ion in its ionic compound is A) +1 B) +2 C) +3 D) -1 E) Various charges are possible. 85. The name for the NO3 - ion is A) nitrate ion B) nitrite ion C) nitrogen ion D) nitric ion E) nitrous ion Page 16

17 86. The formula for the compound formed from the polyatomic ions NH4 + and PO4 3- is A) NH4(PO4)3 B) NH4PO4 C) (NH4)3PO4 D) (NH4)2(PO4)2 87. Potassium chlorate has the formula A) KCl B) KClO C) KClO2 D) KClO3 E) KClO4 88. The name for the compound Fe2O3 is. 89. The name for PbS2 is. 90. Give the formula for magnesium phosphate. 91. Give the formula for sodium chromate. 92. Give the formula for titanium(iv) chloride. 93. Give the name for Al(OH)3. Page 17

18 Answer Key 1. a. Acquisition of knowledge of the natural universe through the use of the Scientific Method. b. The science that deals with matter and the changes it undergoes. Chapter: 1.2, E Chapter: D Chapter: A Chapter: A Chapter: D Chapter: C Chapter: B Chapter: A Chapter: E Chapter: B Chapter: B Chapter: B Chapter: A Chapter: D Chapter: B Chapter: A Chapter: B Chapter: A Chapter: D Chapter: liquid Page 18

19 Chapter: D Chapter: A Chapter: A Chapter: A Chapter: B Chapter: 4.3,4.9,2.4, D Chapter: B Chapter: C Chapter: A Chapter: A Chapter: D Chapter: C Chapter: A Chapter: E Chapter: The isotope contains 26 protons, 23 electrons, and 31 neutrons. Chapter: 4.7, A Chapter: E Chapter: B Chapter: C Chapter: D Chapter: D Chapter: E Chapter: 11.8 Page 19

20 44. C Chapter: A Chapter: D Chapter: C Chapter: A Chapter: C Chapter: A Chapter: E Chapter: A Chapter: [Kr] 5s 2 4d 10 Chapter: [Ne] 3s 2 3p 5 Chapter: [Kr] 5s 1 Chapter: E Chapter: C Chapter: A Chapter: Br Chapter: A Chapter: A Chapter: A Chapter: A Chapter: 12.6, B Chapter: 12.1, E Chapter: D Page 20

21 Chapter: 12.1,12.4, C Chapter: C Chapter: D Chapter: A Chapter: B Chapter: B Chapter: 4.x,12.5, D Chapter: Chapter: C Chapter: B Chapter: S.... H I... Chapter: 12.6 H H Si H H Chapter: 12.6 [Na] O. [Na] +.. Chapter: C Chapter: D, E Chapter: B, D Chapter: 12.9 Page 21

22 83. Chapter: 12.6,7,8,9 84. B Chapter: A Chapter: C Chapter: D Chapter: iron(iii) oxide Chapter: 5.2 Page 22

23 89. lead(iv) sulfide Chapter: Mg3(PO4)2 Chapter: Na2CrO4 Chapter: TiCl4 Chapter: aluminum hydroxide Chapter: 5.5 Page 23

Chem 106 Midterm Study Questions Chapters 1-5,11-12

Chem 106 Midterm Study Questions Chapters 1-5,11-12 Name: Review Mon 10/12/15 Due 10/13/15 (Midterm exam) This is a homework assignment. Please show your work for full credit. If you do work on separate