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Study Resources (Chemistry)

4.1   Multiple Choice Questions 1) Of the species below, only __________ is not an electrolyte. A) HCl B) Rb2SO4 C) Ar D) KOH E) NaCl 2) The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is __________. A) 2H+ (aq)  +  2OH- (aq)  →  2 H2O (l) B) 2H+ (aq)  +  2KOH (aq)  → .
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101) A correct name for Fe(NO3)2 is __________. A) iron nitrite B) ferrous nitrite C) ferrous nitrate D) ferric nitrite E) ferric nitrate 102) The correct name for HNO2 is __________. A) nitrous acid B) nitric acid C) hydrogen nitrate D) hyponitrous acid E) pernitric acid 103) The proper formula for the hydronium ion is __________. A) H- B) OH- C) N-3 D) H3O+ E) NH4+ 104) The.
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1.3   Algorithmic Questions 1) The symbol for the element calcium is __________. A) Pt B) P C) Ca D) S E) K 2) The symbol for the element magnesium is __________. A) Rb B) Mn C) Ne D) Si E) Mg 3) The symbol for the element mercury is __________. A) Me B) Pb C) Sn D) Hg E) Na 4) The temperature of -25 °C is __________ in.
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41) There are __________ significant figures in the answer to the following computation: A) 1 B) 2 C) 3 D) 4 E) 5 42) There should be __________ significant figures in the answer to the following computation. A) 1 B) 2 C) 3 D) 4 E) 5 43) __________ significant figures should be retained in the result of the following calculation. A) 1 B).
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3.1   Multiple-Choice Questions 1) When the following equation is balanced, the coefficients are __________. C8H18  +  O2  →  CO2  +  H2O A) 2, 3, 4, 4 B) 1, 4, 8, 9 C) 2, 12, 8, 9 D) 4, 4, 32, 36 E) 2, 25, 16, 18 2) Of the reactions below, which one is not a combination reaction? A).
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61) The correct formula of iron(III) bromide is __________. A) FeBr2 B) FeBr3 C) FeBr D) Fe3Br3 E) Fe3Br 62) Magnesium and sulfur form an ionic compound with the formula __________. A) MgS B) Mg2S C) Mg S2 D) Mg2S2 E) Mg2S3 63) The formula of ammonium carbonate is __________. A) (NH4)2CO3 B) N H4CO2 C) (NH3)2CO4 D) (NH3)2CO3 E) N2(CO3)3 64) The formula of the chromate ion.
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41) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu. A) 219.7 B) 220.4 C) 220.42 D) 218.5 E) 221.0 42) Element X has three naturally occurring isotopes. The masses (amu) and.
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21) The molecular weight of glucose (C6H12O6), rounded to the nearest integer, is __________ amu. A) 24 B) 96 C) 136 D) 180 E) 224 22) What is the mass % of carbon in dimethylsulfoxide (C2H6SO) rounded to three significant figures? A) 60.0 B) 20.6 C) 30.7 D) 7.74 E) 79.8 23) The mass % of H in methane (CH4) is __________. A).
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91) The charge on the copper ion in the salt CuO is __________. A) +1 B) +2 C) +3 D) -1 E) -2 92) The charge on the iron ion in the salt Fe2O3 is __________. A) +1 B) +2 C) +3 D) -5 E) -6 93) Which formula/name pair is incorrect? A) Mn(NO2)4manganese(II) nitrite B) Mg(NO3)2 magnesium nitrate C) Mn(NO3)2manganese(II) nitrate D) Mg3N2magnesium nitrite E) Mg(MnO4)2magnesium.
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31) Calculate the percentage by mass of nitrogen in PtCl2(NH3)2. A) 4.67 B) 9.34 C) 9.90 D) 4.95 E) 12.67 32) Calculate the percentage by mass of lead in Pb(NO3)2. A) 38.6 B) 44.5 C) 62.6 D) 65.3 E) 71.2 33) Calculate the percentage by mass of nitrogen in Pb(NO3)2. A) 4.2 B) 5.2 C) 8.5 D) 10.4 E) 12.6 34) Calculate the percentage by mass of lead.
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3.4   Short Answer Questions 1) Complete and balance the following reaction, given that elemental rubidium reacts with elemental sulfur to form Rb2S (s).  Na (s)  +  S (s)   →  __________ 2) A compound was found to contain 90.6% lead (Pb) and 9.4% oxygen. The empirical formula for this compound is __________. 3) The.
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51) How many significant figures are in the number 0.0034050? A) 3 B) 4 C) 5 D) 6 E) 7 52) How many significant figures should be retained in the result of the following calculation? A) 2 B) 3 C) 4 D) 5 E) 6 53) In which one of the following numbers are all of the zeros significant? A) 100.090090 B) 0.143290 C) 0.05843 D).
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81) What is the molecular formula for butane? A) C2H8 B) C3H6 C) C3H8 D) C4H8 E) C4H10 82) What is the molecular formula for octane? A) C4H10 B) C5H10 C) C6H14 D) C14H28 E) C8H18 83) What is the molecular formula for pentane? A) C2H8 B) C3H6 C) C4H8 D) C5H12 E) C5H10 84) What is the molecular formula for nonane? A) C9H18 B) C9H20 C) C10H20 D) C10H22 E) C10H24 85) What.
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3.2   Bimodal Questions 1) When the following equation is balanced, the coefficients are __________. NH3 (g)  +  O2 (g) →  NO2 (g)  +  H2O  (g) A) 1, 1, 1, 1 B) 4, 7, 4, 6 C) 2, 3, 2, 3 D) 1, 3, 1, 2 E) 4, 3, 4, 3 2) When the following equation is balanced,.
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21) The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is __________. A) C12H14O6 B) CHO C) CH2O D) C6 H7O3 E) C2H4O 22) __________ typically form ions with a 2+ charge. A) Alkaline earth metals B) Halogens C) Chalcogens D) Alkali metals E) Transition metals 23) What is the formula of.
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41) The correct name for Al2O3 is __________. A) aluminum oxide B) dialuminum oxide C) dialuminum trioxide D) aluminum hydroxide E) aluminum trioxide 42) The correct name for Ca H2 is __________. A) hydrocalcium B) calcium dihydride C) calcium hydroxide D) calcium dihydroxide E) calcium hydride 43) The correct name for SO is __________. A) sulfur oxide B) sulfur monoxide C) sulfoxide D) sulfate E) sulfite 44) The.
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2.1   Multiple-Choice Questions 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of __________. A) the law of multiple proportions B) the law of constant composition C) the law of conservation of mass D) the law of conservation of energy E) none of the above 2) Which.
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21) Which atom has the largest number of neutrons? A) phosphorus-30 B) chlorine-37 C) potassium-39 D) argon-40 E) calcium-40 22) There are __________ electrons, __________ protons, and __________ neutrons in an atom of . A) 132, 132, 54 B) 54, 54, 132 C) 78, 78, 54 D) 54, 54, 78 E) 78, 78, 132 23) An atom of the most common isotope.
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71) Which species has 54 electrons? A) Xe+ B) Te2- C) Sn2+ D) Cd E) Xe2+ 72) Which species has 16 protons? A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O 73) Which species has 18 electrons? A) 39K B) 32S-2 C) 35Cl D) 27Al+3 E) 64Cu+2 74) The species __________ contains 16 neutrons. A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O 75) Which species is an isotope of 39Cl? A) 40Ar+ B).
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1.2   Bimodal Questions 1) Solids have a __________ shape and are not appreciably __________. A) definite, compressible B) definite, incompressible C) indefinite, compressible D) indefinite, incompressible E) sharp, convertible 2) __________ is the chemical symbol for elemental sodium. A) S B) W C) So D) Na E) Sn 3) If matter is uniform throughout and cannot be separated into other substances by physical.
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11) Elements in Group 2A are known as the __________. A) alkaline earth metals B) alkali metals C) chalcogens D) halogens E) noble gases 12) Elements in Group 6A are known as the __________. A) alkali metals B) chalcogens C) alkaline earth metals D) halogens E) noble gases 13) Elements in Group 7A are known as the __________. A) chalcogens B) alkali metals C) alkaline.
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2.4   Short Answer Questions 1) What group in the periodic table would the fictitious element  ::  be found? 2) Which element in Group IA is the most electropositive? 3) The formula for potassium sulfide is __________. 4) What is the name of an alcohol derived from hexane? 2.5   True/False Questions 1) The possible oxidation numbers.
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71) Copper and chlorine form an ionic compound whose formula is CuCl2.  The name of this compound is __________. A) copper chlorine B) copper (III) dichloride C) monocopper dichloride D) copper (II) dichloride E) cupric chloride 72) The name of the binary compound N2O4 is __________. A) nitrogen oxide B) nitrous oxide C) nitrogen(IV) oxide D) dinitrogen tetroxide E) oxygen nitride 73).
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51) The correct name for HClO is __________. A) hydrochloric acid B) perchloric acid C) chloric acid D) chlorous acid E) hypochlorous acid 52) The correct name for HBrO4 is __________. A) hydrobromic acid B) perbromic acid C) bromic acid D) bromous acid E) hydrobromous acid 53) The correct name for HBrO is __________. A) hydrobromic acid B) perbromic acid C) bromic acid D) bromous acid E).
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31) Different isotopes of a particular element contain the same number of __________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) subatomic particles 32) Different isotopes of a particular element contain different numbers of __________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) None of the above is correct. 33).
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3.3   Algorithmic Questions 1) The molecular weight of acetic acid ( HC2H3O2), the acid in vinegar, is __________ amu (rounded to one decimal place). A) 59.0 B) 29.0 C) 60.1 D) 8.0 E) 32.0 2) Determine the mass percent (to the hundredths place) of Na in sodium bicarbonate (NaHCO3). 3) There are __________ mol of carbon atoms in.
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81) Which of the following compounds would you expect to be ionic? A) H2O B) CO2 C) SrCI2 D) SO2 E) H2S 82) Which pair of elements is most apt to form an ionic compound with each other? A) barium, bromine B) calcium, sodium C) oxygen, fluorine D) sulfur, fluorine E) nitrogen, hydrogen 83) Which pair of elements is most apt to.
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11) Cathode rays are __________. A) neutrons B) x-rays C) electrons D) protons E) atoms 12) Cathode rays are deflected away from a negatively charged plate because __________. A) they are not particles B) they are positively charged particles C) they are neutral particles D) they are negatively charged particles E) they are emitted by all matter 13) In the absence of.
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61) Which one of the following molecular formulas is also an empirical formula? A) C6H6O2 B) C2H6SO C) H2O2 D) H2P4O6 E) C6H6 62) Which compounds do not have the same empirical formula? A) C2H2, C6H6 B) CO, CO2 C) C2H4, C3H6 D) C2H4O2, C6H12O6 E) C2H5COOOCH3, CH3CHO 63) Of the choices below, which one is not an ionic compound? A) PCl5 B) MoCl6 C).
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2.3   Algorithmic Questions 1) A certain mass of carbon reacts with 23.3 g of oxygen to form carbon monoxide. __________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions? A) 25.6 B) 11.7 C) 23.3 D) 233 E) 46.6 2) An atom of 14C.
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21) 1 kilogram = __________ milligrams A) 1 × 10-6 B) 1,000 C) 10,000 D) 1,000,000 E) none of the above 22) "Absolute zero" refers to __________. A) 0 Kelvin B) 0° Fahrenheit C) 0° Celsius D) °C + 9/5(°F - 32) E) 273.15 °C 23) The density (in g/cm3) of a gold nugget that has a volume of 1.68 cm3 and.
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51) Elements __________ exhibit similar physical and chemical properties. A) with similar chemical symbols B) with similar atomic masses C) in the same period of the periodic table D) on opposite sides of the periodic table E) in the same group of the periodic table 52) Which pair of elements would you expect to exhibit the.
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21) When the following equation is balanced, the coefficient of nitric acid is __________. N2O5 (g)  +  H2O (l)  →  HNO3 (aq) A) 5 B) 2 C) 3 D) 4 E) 1 22) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air.  What is the coefficient of methanol in.
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