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Study Resources (Chemistry)

2.1   Multiple-Choice Questions 1) An example of kinetic energy is  A) a coiled spring. B) running water. C) a tree. D) natural gas. E) chemical energy. 2) The energy associated with the motion of particles in a substance is called  A) temperature. B) electrical energy. C) heat. D) chemical energy. E) potential energy. 3) Which of the following is an example.
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2.4   Matching Questions Identify the physical state(s) corresponding to the regions on the cooling curve below. A) solid and gas B) liquid and gas C) gas D) liquid and solid E) solid 1) A 2) B 3) C 4) D 5) E Match the state of matter with each of the following descriptions of a substance. A) solid B) liquid C) solid + liquid D) liquid.
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21) Gold in a wedding ring is a(n) A) compound. B) heterogeneous mixture. C) element. D) homogeneous mixture. E) None of the above. 22) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 23) Which of the following is a property of a solid?  A) It takes the.
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31) The name of Al2(SO4)3 is A) aluminum(III) sulfate. B) dialuminum trisulfate. C) dialuminum sulfate. D) dialuminum trisulfide. E) aluminum sulfate. 32) A group of covalently bonded atoms that has an overall electrical charge is called a(n) A) ionic compound. B) anion. C) polyatomic ion. D) cation. E) molecule. 33) Which of the following polyatomic ions has a positive charge? A) hydroxide B) sulfate C).
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6.1   Multiple-Choice Questions 1) A chemical equation is balanced when A) the total number of molecules is the same in reactants and products. B) the total number of ions is the same in reactants and products. C) the sum of the coefficients of the reactants is equal to the sum of the coefficients of.
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51) What is the electron configuration for aluminum? A) 1 s22s22 p63s23p1 B) 1 s22s22p63s23p3 C) 1 s22s22p63s23p5 D) 1 s22s22p63s23p6 E) 1 s22 22p63s23p8 52) Which of the following electron configurations is impossible? A) 1s22s22p63s23p1 B) 1s22 s42p63s23p3 C) 1s22s22p63s23 p5 D) 1s22s22p63s23p6 E) 1s22s22p63s23p3 53) What is the electron configuration for potassium (atomic number 19)? A) 1s22s22p63s23p7 B) 1s22s22p63s23p53d2 C) 1s22s22p83s23p5 D) 1s22s22p63s23p64s1 E) 1s22s22p63s23p54s1 54).
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  Give the correct charge for ions of the following elements. A) 1- B) 0 C) 2- D) 3+ E) 2+ 10) Ca 11) Cl 12) O 13) Al 14) K Indicate the type of bonding you would expect between the following elements. A) nonpolar covalent B) ionic C) none D) polar covalent 15) Na and F 16) N and F 17) F and F 18) He and F 19).
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21) Nitrogen-17 is a beta emitter.  What is the isotope produced in the radioactive decay? A) C B) B C) N D) F E) O 22) The nuclear reaction Sn  →  Sb  +  ? A) fusion. B) fission. C) translation. D) alpha emission. E) beta emission. 23) What is the radioactive particle released in the following nuclear equation? Sr  →  Y  +  ?.
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11) The process in which a nucleus spontaneously breaks down by emitting radiation is known as A) transmutation. B) transformation. C) fusion. D) a chain reaction. E) radioactive decay. 12) The nuclear reaction shown below is an example of what type of process? A) fusion B) fission C) translation D) alpha emission E) beta emission 13) Gamma rays require the heaviest shielding.
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3.4   Matching Questions Do the following represent elements in a group, a period, or neither? A) period B) neither C) group 1) Li, C, F 2) F, S, P 3) O, S, Se 4) He, H, I Match the correct symbols with the names of elements.   A) C B) Co C) Cu D) Cl E) Ca 5) calcium 6) copper 7) carbon 8) chlorine 9) cobalt   .
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5.3   Matching Questions Match the correct name of the polyatomic ions with the formulas given. A) sulfate B) nitrate C) hydrogen carbonate D) hydroxide E) nitrite F) oxide G) phosphate H) carbonate I) hydrogen sulfite J) carbonite K) sulfite L) hydrogen sulfate M) phosphate 1) NO3- 2) CO32- 3) SO42- 4) SO32- 5) PO43- 6) NO2- 7) HCO3- 8) HSO4- 9) OH-   .
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11) Isotopes have the same atomic number but different mass numbers. 12) Potassium has one valence electron. 13) The electron configuration of potassium is 1s22s22 p63s1. 14) A lithium atom is larger than a potassium atom. 15) A sodium atom is larger than a silicon atom. 16) Chlorine has a higher ionization energy than aluminum. 17).
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5.1   Multiple-Choice Questions 1) The number of valence electrons found in an atom of a Group A element is equal to A) its atomic number. B) its mass number. C) its group number. D) eight. E) eight minus the group number. 2) Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the.
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51) The types of compounds that use prefixes in their names are A) ionic compounds. B) ionic compounds involving transition metals. C) polyatomic ions. D) covalent compounds. E) compounds that contain polyatomic ions. 52) The correct name for the compound N2O3 is A) nitrogen oxide. B) nitrogen trioxide. C) dinitride trioxide. D) dinitrogen oxide. E) dinitrogen trioxide. 53) What is the formula.
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1.3   Matching Questions Are the numbers in each of the following statements measured or exact? A) exact B) measured 1) In the U.S. system there are 5280 feet in one mile. 2) The patient's blood sugar level is 350 mg/dL. 3) There are 452 pages in a book. 4) The rabbit weighs 2.5 pounds. 5) There are.
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71) The carbon tetrachloride molecule, CCl4, is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds. 72) The ammonia molecule ( NH3 ) is A) a polar molecule with polar bonds. B).
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5.2   Short Answer Questions Identify each of the following molecules as polar or nonpolar. 1) carbon tetrachloride 2) water 3) carbon dioxide 4) hydrogen sulfide 5) hydrogen fluoride 6) carbon monoxide 7) nitrogen trichloride 8) carbon tetrachloride 9) potassium oxide 10) carbon dioxide 11) sodium fluoride 12) dihydrogen sulfide 13) The weakest type of force between particles of a substance is termed __________. 14) Are.
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  Identify each of the following transformations as a chemical or physical change A) physical B) chemical 11) water evaporating 12) a button falling off of a shirt 13) silver tarnishing 14) cutting the grass 15) a nail rusting 16) baking a cake 17) placing photographs in a scrapbook 18) formation of green leaves on a plant 19) burning leaves 20) melting.
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11) Which of the following properties is NOT a characteristic of the Group 1A(1) elements (alkali metals)? A) They are shiny. B) They are good conductors of heat. C) They react vigorously with water. D) Most of them are liquids at room temperature. E) They are good conductors of electricity. 12) The Group 8A(18) elements A) are.
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4.4   Matching Questions Indicate whether each of the following is characteristic of the fission or fusion process. A) both fission and fusion B) fusion C) fission 1) A large nucleus is split into smaller nuclei. 2) Very high temperatures must be achieved to initiate the reaction. 3) This nuclear process provides the energy of the Sun. 4) This.
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4.2   Short Answer Questions 1) One symbol for the β particle is β. Another symbol for the same particle is __________. 2) Tc  →  Tc  +  __________ 3) U  +  n  →  __________  +  Kr  +  3n  +  energy 4) Sr  →  __________  +  e  +  energy 5) The radiation dose required to produce death.
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4.3   True/False Questions 1) The production of nitrogen-13 and a neutron from boron-10 by bombardment with a helium-4 nucleus is an example of radioactive decay. 2) The correct symbol for hydrogen-3 is He. 3) An alpha particle is emitted when Am-241 decays to Np-237. 4) A beta particle is emmited when Co-60 decays to.
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3.3   True/False Questions 1) The symbol for potassium is P. 2) The symbol for gold is Au. 3) Sulfur is a nonmetal. 4) Chromium is a metal. 5) Radon is a metal. 6) Mercury is a metal. 7) Iodine is a metal. 8) An electron has a positive charge. 9) Protons and neutrons are located in the nucleus of.
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4.1   Multiple-Choice Questions 1) What is the nuclear symbol for a radioactive isotope of copper with a mass number of 60? A) Cu B) Cu C) 29Cu D) Cu E) Cu 2) The nuclear symbol of helium, He, is also the symbol for designating a(n) A) proton. B) neutron. C) gamma ray. D) beta particle. E) alpha particle. 3) The symbol e is.
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31) Iodine-131 decays by beta emission to A) iodine-132. B) tellurium-131. C) iodine-130 D) bromine-131 E) xenon-131. 32) A sample of cerium-141 for a diagnostic test was dissolved in saline solution to an activity of 4.5 millicuries/mL. If the patient undergoing the test needs a dose of 10. millicuries, how much of the solution should be.
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  Give the correct number of electrons. A) one B) seven C) two D) eight E) five 10) in the second energy level of magnesium 11) in the highest occupied energy level of chlorine 12) in the outer energy level of nitrogen 13) in the first energy level of chlorine 14) in the third energy level of sodium Classify the following elements. A).
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2.2   Short Answer Questions 1) The energy of motion is called __________ energy. 2) The lowest temperature on the Kelvin scale is __________ kelvin. 3) The simplest type of pure substance is an  __________. 4) A mixture which has uniform properties is a    __________ mixture. 5) The change of state from.
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3.1   Multiple-Choice Questions 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Au is the symbol for A) gold. B) silver. C) argon. D) aluminum. E) sodium. 3) aluminum A) Al B) Am C) Au D) Sn E) Ag 4) iron A) Ir B) Fs C) Fe D) In E) FE 5) sodium A) So B) Na C) No D) Sm E) Au 6) potassium A) P B) Po C).
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21) Identify the metalloid in the following list. A) sulfur B) fluorine C) silver D) copper E) germanium 22) Semiconductors are located in the periodic table on (or in) the A) left side of the table. B) right side of the table. C) line dividing metals from nonmetals in the table. D) first period of the table. E) last period of.
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