CHAPTER 3 & 4 PREP-TEST

Transcription

1 Name: Class: Date: CHAPTER 3 & 4 PREP-TEST Multiple Choice Identify the choice that best completes the statement or answers the question. 1. According to Dalton's atomic theory, atoms a. of different elements combine in simple whole-number ratios to form compounds. b. can be divided into protons, neutrons, and electrons. c. of all elements are identical in size and mass. d. can be destroyed in chemical reactions. 2. Rutherford fired positively charged particles at metal foil and concluded that most of the mass of an atom was a. in the electrons. c. evenly spread throughout the atom. b. concentrated in the nucleus. d. in rings around the atom. 3. The nucleus of most atoms is composed of a. tightly packed protons. c. tightly packed protons and neutrons. b. tightly packed neutrons. d. loosely connected protons and electrons. 4. Most of the volume of an atom is occupied by the a. nucleus. c. electron cloud. b. nuclides. d. protons. 5. The charge on the electron cloud a. prevents compounds from forming. b. balances the charge on the nucleus. c. attracts electron clouds in other atoms to form compounds. d. does not exist. 6. The smallest unit of an element that can exist either alone or in combination with other such particles of the same or different elements is the a. electron. c. neutron. b. proton. d. atom. 7. Isotopes of an element contain different numbers of a. electrons. c. neutrons. b. protons. d. nuclides. 8. The total number of protons and neutrons in the nucleus of an atom is its a. atomic number. c. mass number. b. Avogadro constant. d. number of neutrons. 9. As the mass number of the isotopes of an element increases, the number of protons a. decreases. b. increases. c. remains the same. d. doubles each time the mass number increases. 10. The average atomic mass of an element depends on both the masses of its isotopes and each isotope's a. atomic number. c. relative abundance. b. radioactivity. d. mass number. 1

2 Name: 11. What is the atomic number for aluminum a. 13 c b. 14 d A neutral atom of silicon contains. a. 14 electrons. c. 16 electrons. b electrons. d. 38 electrons. 13. An atom of potassium has 19 protons and 20 neutrons. What is its mass number a. 19 c. 39 b. 20 d Ag-109 has 62 neutrons. The neutral atom has a. 40 electrons. c. 53 electrons. b. 47 electrons. d. 62 electrons. 15. Silicon-30 contains 14 protons. It also contains a. 16 electrons. c. 30 neutrons. b. 16 neutrons. d. 44 neutrons. 16. Neon-22 contains 12 neutrons. It also contains a. 12 protons. c. 22 electrons. b. 22 protons. d. 10 protons. 17. Mendeleev's table was called periodic because the properties of the elements a. showed no pattern. b. occurred at repeated intervals called periods. c. occurred at regular time intervals called periods. d. were identical. 18. Argon, krypton, and xenon are a. alkaline earth metals. c. actinides. b. noble gases. d. lanthanides. 19. In the modern periodic table, elements are ordered according to a. decreasing atomic mass. c. increasing atomic number. b. Mendeleev's original design. d. the date of their discovery. 20. To which group do lithium and potassium belong Refer to your periodic table. a. alkali metals c. halogens b. transition metals d. noble gases 21. Refer to your periodic table. To which group do fluorine and chlorine belong a. alkaline-earth metals c. halogens b. transition elements d. actinides 22. What is the charge on the strontium ion a. 2 c. 1 b. 1 d Which of the following elements does NOT form an ion with a charge of 1 a. fluorine c. potassium b. hydrogen d. sodium 2

3 Name: 24. An ion of Cl has _ protons and _ electrons. a. 17, 22 c. 35, 17 b. 17, 35 d. 17, How many neutrons are found in this isotope of Carbon a. 6 c. 14 b. 12 d The following data was collected from a student s Isotopes of Pennium Lab. Number of Pre- 82 Pennies (relative abundance) 12 (60%) Number of Post- 82 Pennies (relative abundance) 8 (40%) Ave. Atomic Mass of Pre- 82 Pennies 3.00 Ave. Atomic Mass of Post- 82 Pennies 2.50 Calculate the Ave. Atomic Mass of this sample of Pennium using the following equation: Ave. Atomic Mass of Pe = (relative abundance of pre- 82 pennies x Ave. At. Mass Pre- 82 Pennies) + (relative abundance of post- 82 pennies x Ave. At. Mass of post- 82 pennies) a c b d Two isotopes of a new element (Ma) recovered from Mars have mass numbers of 130 and 132. Ma-130 has a relative abundance of 20% while Ma-132 has a relative abundance of 80%. What is the Average Atomic Mass of Ma a c b d Of the acids containing oxygen, which is true regarding those ending in -ous compared to those ending in -ic a. contains more hydrogen. c. contains less oxygen. b. contains more oxygen. d. contains the same amount of oxygen. 3

4 Name: 29. Changing a subscript in a correctly written chemical formula a. changes the number of protons represented by the formula. b. changes the charges on the other ions in the compound. c. changes the formula so that it no longer represents that compound. d. has no effect on the formula. 30. What is the formula for the compound formed by lead(ii) ions and chromate ions a. PbCrO 4 c. Pb 2 (CrO 4 ) 3 b. Pb 2 CrO 4 d. Pb(CrO What is the formula for tin(iv) chromate a. Sn(CrO 4 ) 4 c. Sn 2 (CrO 4 ) 4 b. Sn 2 (CrO 4 d. Sn(CrO Name the compound CuCO 3. a. copper(i) carbonate c. copper(iv) carbonate b. copper(iii) carbonate d. copper(ii) carbonate 33. What type of ions have names ending in -ide a. only cations c. only metal ions b. only anions d. only gaseous ions 34. When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a. a. prefix c. Roman numeral following the name b. suffix d. superscript after the name 35. An -ate or -ite at the end of a compound name usually indicates that the compound contains. a. fewer electrons than protons c. only 1 element b. neutral molecules d. a polyatomic anion 36. Which of the following compounds contains the Mn 3 ion a. MnS c. Mn 2 O 3 b. MnBr 2 d. MnO 37. Which of the following formulas represents an ionic compound a. CS 2 c. N 2 O 4 b. BaI 2 d. PCl Which of the following compounds contains the lead(ii) ion a. PbO c. Pb 2 O b. PbCl 4 d. Pb 2 S 39. What is the correct formula for potassium sulfite a. KHSO 3 c. K 2 SO 3 b. KHSO 4 d. K 2 SO 4 4

5 Name: 40. What is the ending for the names of all binary compounds, both ionic and Type III a. -ide c. -ade b. -ite d. -ate 41. Which of the following correctly shows a prefix used in naming binary molecular compounds with its corresponding number a. deca-, 10 c. hexa-, 8 b. nona-, 5 d. octa-, Which of the following formulas represents a Type 3 compound a. ZnO c. SO 2 b. Xe d. BeF What is the name of H 2 SO 3 a. hyposulfuric acid c. sulfuric acid b. hydrosulfuric acid d. sulfurous acid 44. What is the formula for hydrosulfuric acid a. H 2 S 2 c. HSO 2 b. H 2 SO 2 d. H 2 S 45. Select the correct formula for sulfur hexafluoride. a. S 2 F 6 c. FS 6 b. F 6 SO 3 d. SF What is the correct name for the compound CoCl 2 a. cobalt(i) chlorate c. cobalt(ii) chlorate b. cobalt(ii) chloride d. cobalt(i) chloride 47. What is the correct formula for barium chlorate a. Ba(ClO 3 c. Ba(ClO b. Ba(ClO 2 d. BaCl What is the correct formula for calcium dihydrogen phosphate a. CaH 2 PO 4 c. Ca(H 2 PO 4 b. Ca 2 H 2 PO 4 d. Ca(H 2 HPO Which of the following is the correct name for N 2 O 5 a. nitrous oxide c. nitrogen dioxide b. dinitrogen pentoxide d. nitrate oxide 50. What is the correct name for Sn 3 (PO 4 a. tritin diphosphate c. tin(iii) phosphate b. tin(ii) phosphate d. tin(iv) phosphate 5

6 Name: The word Nomenclature comes from Nomenclator, who is a person who calls out names. "Nomen" means names and "clator" is a person who calls out. When students get their diploma, the nomenclator is the person who calls out the students' names. In chemistry, "nomenclature" is learning to call out chemical names. Understanding chemistry nomenclature is like learning any language. It takes practice and study, but the reward is that it gives you the ability to talk to people you couldn't talk to before. 51. What does the term nomenclature mean a. learning to call out chemical names c. to mold from clay b. writing formulas d. to practice and study 52. What is the stock system name for the ionic compound stannous fluoride a. can t be names using the stock system c. tin (II) fluoride b. tin (IV) fluoride d. stannic fluoride Use the following information (and the table above) for the next two questions. Cuprous oxide is commonly used as a pigment, a fungicide, and an antifouling agent for marine paints. Rectifier diodes based on this material have been used industrially as early as 1924, long before silicon became the standard. 53. What is the charge of the copper in cuprous oxide a. 1+ c. 1- b. 2+ d What is the correct stock system name for cuprous oxide. a. Can t be determined c. copper (II) oxide b. copper (I) oxide d. copper oxide Matching Match each item with the correct statement below. a. proton d. electron b. nucleus e. neutron c. atom 55. the smallest particle of an element that retains the properties of that element 6

7 Name: 56. a positively charged subatomic particle 57. a negatively charged subatomic particle 58. a subatomic particle with no charge 59. the central part of an atom, containing protons and neutrons Match each item with the correct statement below. a. mass number d. atomic mass b. atomic mass unit e. isotope c. atomic number 60. atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom 61. the total number of protons and neutrons in the nucleus of an atom 62. the number of protons in the nucleus of an element 63. the weighted average of the masses of the isotopes of an element 64. one-twelfth the mass of a carbon atom having six protons and six neutrons 7