General Chemistry I Test Bank Christopher King Department of Chemistry Troy State University Troy, AL 36082 cking@trojan.troyst This document contains 184 test questions and answers that I have used during the past three semesters. The text for the course was Jones and Atkins, Chemistry: Molecules, Matter, and Change, 4th ed., 1999. The questions pertain to chapters 1-4, and 7-9. The equations were created using MathType equation editor 5. This is an upgrade to the equation editor that comes with Word. I got it so that the equations could be displayed in a blue font (I show answers in blue on my web pages). To modify the equations, you will need to get the MathType free upgrade (dessci/en/). If you don’t purchase the upgrade, you can only change colors for the first 30 days. Categories Components of Atoms ........................................................................................................................ Symbols of Isotopes............................................................................................................................. Using the Periodic Table..................................................................................................................... Mixtures............................................................................................................................................... Solution Terminology.......................................................................................................................... Physical &amp;amp; Chemical Properties.......................................................................................................... Diatomic Elements............................................................................................................................... Anion and Cation Terms...................................................................................................................... Naming Compounds............................................................................................................................ Formulas of Compounds...................................................................................................................... Understanding Chemical Formulas................................................................................................... Significant Figures............................................................................................................................. Dimensional Analysis........................................................................................................................ Temperature....................................................................................................................................... Density............................................................................................................................................... Avogadro’s Number.......................................................................................................................... Molar Mass from % Abundance........................................................................................................ Molar Mass; grams  moles........................................................................................................ Understanding Molar Mass............................................................................................................... Percent Composition from Formula.................................................................................................. Formulas from Percent Composition Data........................................................................................ Product of Combination Reaction..................................................................................................... Balanced Reaction of Sodium or Potassium with Water.................................................................. Oxidation Numbers............................................................................................................................ Balance Simple Redox Equations..................................................................................................... Combustion Reactions....................................................................................................................... Apply Solubility Rules...................................................................................................................... Examples of Strong Acids &amp;amp; Bases.................................................................................................. Complete the Reaction; Net Ionic Equations.................................................................................... Molarity.............................................................................................................................................. Dilution.............................................................................................................................................. Titration.............................................................................................................................................. Limiting Reactant, Theoretical Yield, % Yield................................................................................. Energy  Wavelength  Frequency....................................................................................... Quantum Numbers............................................................................................................................. Orbitals............................................................................................................................................... Electron Configurations of Elements................................................................................................ Electron Configurations of Ions........................................................................................................ Hund’s Rule....................................................................................................................................... Periodic Trends.................................................................................................................................. Valence Electrons.............................................................................................................................. Ionic or Covalent from Electronegativity.......................................................................................... Formal Charges.................................................................................................................................. Resonance Structures......................................................................................................................... Deviations from Idea Geometry (and some mixed questions).......................................................... Lewis Acids, Bases, and Adducts...................................................................................................... Lewis Structures, Shapes, and Polarities........................................................................................... Hybridization; sigma and pi bonds.................................................................................................... Molecular Orbitals............................................................................................................................. You must show your work to get credit (or partial credit). Watch significant figures and show units. Some constants: c = 3 × 108 m/s h = 6 × 10-34 J s RH = 3 × 1015 Hz NA = 6 × 1023 Components of Atoms 1 (2 pts) Atoms of the same element, regardless of charge, all have the same number of ___protons______. 2 (2 pts) Comparing the mass of an electron to the mass of a proton, one could say that the electron is _____much less________ massive than the proton. 3 (2 pts) Comparing the mass of a neutron to the mass of a proton, one could say that the neutron a) is much less massive than the proton. b) is less massive than the proton. c) has nearly the same mass as the proton. d) is more massive than the proton. e) is much more massive than the proton. 4 (2 pts) How large is the nucleus compared to the size of an atom? Very small. 5 (4 pts) What two kinds of atomic particles are found in the nucleus of an atom? ____protons__________ and _____neutrons_________ 14 (6 pts) Give the symbol that identifies the following isotope. Include the charge if the isotope is not neutral (for example, 1H+) 53 protons, 76 neutrons, 54 electrons: 129 – I 15 (12 pts) Give the symbol that identifies the following species. Include the charge if the species is not neutral (for example, 1H+) 9 protons, 10 neutrons, 10 electrons: 19 – 94 protons, 150 neutrons, 91 electrons: F 244 Pu3+ 16 (6 pts) Give the symbol that identifies the following isotope. (For example, 1H+) 8 protons, 9 neutrons, 10 electrons: _______ 17O217 (6 pts) Give the symbol that identifies the following species. (For example, 1H+) 16 protons, 16 neutrons, 16 electrons: _______ 32S 92 protons, 146 neutrons, 88 electrons: _______ 238U4+ 13 18 (6 pts) Give the number of subatomic particles in 6 C . protons _____ 6 neutrons _____ 7 electrons _____ 6 19 (2 pts) An atom containing which one of the following is an isotope of carbon? a) 6 neutrons and 7 protons b) 7 neutrons and 6 protons c) 12 neutrons and 12 protons d) 13 neutrons and 13 protons e) 14 neutrons and 14 protons 20 (2 pts) The current scientific theory is that the elements heavier than hydrogen (this includes the elements from which we are made) are formed from/in _____stars or supernova___. Using the Periodic Table 21 (6 pts) Classify the following as metal, nonmetal, or metalloid: chlorine _ nonmetal___; sodium ___metal____; boron __metalloid__ 22 (2 pts) The formula of the ion of sulfur that would be expected to form based on sulfur’s position in the periodic table is _________. S2- Element symbol must have correct charge. 23 (10 pts) Fill in the boxes to identify the five parts of the periodic table that are circled. transition metals (or elements) noble gases halogens alkali metals actinides Mixtures 24 (8 pts) Classify each of the following as a pure substance, a heterogeneous mixture, or a homogeneous mixture. (a) chocolate-chip cookie ______________________ heterogeneous mixture (b) distilled water ______________________ pure substance (c) vodka ______________________ homogeneous mixture (d) a pure gold coin ______________________ pure substance 25 (6 pts) Classify each of the following as a pure substance, a heterogeneous mixture, or a homogeneous mixture. an ear of corn ______________________ heterogeneous mixture sodium chloride ______________________ pure substance sugar water ______________________ homogeneous mixture 26 (8 pts) Classify each of the following as an element, compound, or mixture. (a) the air we breath ______________________ mixture (b) the gas in a tank of chlorine used to disinfect water ______________________ element (c) table salt ______________________ compound (d) a mosquito ______________________ mixture 27 (8 pts) Classify each of the following as an element, compound, or mixture. (a) aluminum metal ______________________ element 33 (1 pts) Paper chromatography separations are based on the fact that A) the components to be separated are volatile. B) The components to be separated have different tendencies to stick to the paper. C) liquids are adsorbed on calcium carbonate. D) a carrier gas is unreactive. E) the components can be distilled. Diatomic Elements 34 (5 pts) Name five elements that are diatomic. hydrogen 5 pts for correct elements oxygen (Wanted to charge 5 pts for spelling, but too many people nitrogen just gave symbols instead of names) fluorine chlorine bromine iodine 35 (2 pts) “So,” your great-uncle asks you, “is chlorine an element or a molecule?” What would be the best answer? It is both. Recognize that it is both an element and a molecule. –1 for just element. 36 (5 pt) Give the formulas of 4 diatomic elements: N2, O2, H2, F2, Cl2, Br2, I2 1 pt for the subscripts Anion and Cation Terms 37 (2 pt) When an atom loses an electron, it becomes an ion. What is an ion with a positive charge called? A cation 38 (2 pt) When an atom loses an electron, it becomes an ion. What is an ion with a negative charge called? An anion Naming Compounds 39 (29 pts) Name the following compounds. CuNO3·6H2O copper(I)nitrate hexahydrate 5 pts KCN potassium cyanide 2 pts SiC (commonly called carborundum) silicon carbide 3 pts N2O5 dinitrogen pentaoxide 4 pts The common name used for NH3 ammonia 2 pts HCl(g) hydrogen chloride 3 pts HCl(aq) hydrochloric acid 4 pts H2SO4(aq) sulfuric acid 3 pts HClO3(aq) chloric acid 3 pts 40 (30 pts) Name the following compounds. (Co is cobalt, Z = 27) Na2CO3·10H2O sodium carbonate decahydrate 4 pts Co(CN)2·3H2O cobalt(II)cyanide trihydrate 4 pts SiC (commonly called carborundum) silicon carbide 3 pts P4O10 tetraphosphorus decaoxide 4 pts The common name used for NH3 ammonia 2 pts HCl(g) hydrogen chloride 3 pts HCl(aq) hydrochloric acid 4 pts HNO3(aq) nitric acid 3 pts HIO3(aq) iodic acid 3 pts 41 (25 pts) Name the following compounds (Fe is iron). FeSO4·7H2O iron(II)sulfate heptahydrate 5 pts NH4CN ammonium cyanide 4 pts ClO2 chlorine dioxide 3 pts IF5 iodine pentafluoride 3 pts HI(g) hydrogen iodide 3 pts HI(aq) hydroiodic acid 4 pts LiNO2 lithium nitrite 3 pts 42 (20 pts) Name the following compounds (Ni, nickel, is element number 28). NiCl4·8H2O nickel (IV)chloride octahydrate 5 pts Ca(CN)2 calcium cyanide 3 pts CS2 carbon disulfide 3 pts P2S5 diphosphorus pentasulfide 4 pts NaClO4 sodium perchlorate 4 pts 43 (14 pts) Name the following compounds. NiSO4·6H2O nickel(II) sulfate hexahydrate 5 pts SF6 sulfur hexafluoride 3 pts HBr(g) hydrogen bromide 3 pts HNO3(aq) nitric acid 3 pts 44 (17 pts) Name the following compounds. Al(ClO3)3 aluminum chlorate 4 pts sulfuric acid H2SO4 4 pts phosphoric acid H3PO4 4 pts 51 (21 pts) Give formulas for the following compounds. (manganese, Mn, is element number 25) manganese(IV) oxide MnO2 3 pts sodium carbonate hexahydrate Na2CO3·6H2O 9 pts phosphoric acid H3PO4 5 pts perbromic acid HBrO4 4 pts 52 (20 pts) Give formulas for the following compounds. iron(III) oxide Fe2O3 4 pts potassium sulfite dihydrate K2SO3·2H2O 8 pts diphosphorus trisulfide P2S3 4 pts periodic acid HIO4 4 pts 53 (4 pts) The formula of dinitrogen tetraoxide is _______________. N2O4 54 (4 pts) The formula for aqueous perchloric acid is _______________. HClO4(aq) The (aq) is optional 55 (9 pts) Give the formula of the compound that is apt to be formed from the following: a) calcium ions and nitrate ions __________ Ca(NO3)2 -2 for Ca3N2 b) aluminum and sulfur __________ Al2S3 56 (8 pts) Give the formula of the compound that is apt to be formed from the following: a) beryllium and chlorine __________ BeCl2 b) boron and oxygen __________ B2O3 Understanding Chemical Formulas 57 (2 pts) How many atoms are in one molecule of (NH4)3PO4? ____ 20 58 (2 pts) How many atoms are in one “formula unit” of Al2(SO4)3? ____ 17 Significant Figures 59 (2 pts) How many significant figures should be given in the result of ? (Note: no calculation is necessary.) 2 534× 321 × 0 7 ×10−3 (0 only has 2 significant figures) 60 (2 pts) How many significant figures should be given in the result of 534× 321 × 0 ? 7 ×10−3 (Note: no calculation is necessary.) 3 (0 only has 3 significant figures) 61 (1 pts) Do the following measurement calculation. 11 -4 7 (Just counting number of significant figures.) 62 (2 pts) How many significant figures are there in the measured number 0? 5 63 (2 pts) How many significant figures are in the measured number 0? 7 Dimensional Analysis 64 (2 pts) A bottle of cola purchased in Europe gave the volume as 50 cL. What is this volume in mL? a) 0 L b) 5000 mL c) 500 mL d) 50 mL e) 0 L 65 (8 pts) If a little old lady is doing 98 kilometers/hour, will she get a speeding ticket if the speed limit is 55 miles / hour? [USE: 5280 feet = 1 mile and 2 cm = 1 inch] (Show how to convert to miles / hour, even if your calculator does it for you.) ? mile 98  1000m  1cm  1in.  1 ft   1mile  =       h h  1km  10−2 m  2  12in.   5280 ft  = 61 / hour Would get a speeding ticket. 66 (5 pts) A supersonic transport (SST) airplane consumes about 18,000 L of kerosene per hour of flight. Kerosene has a density of 0 kg/L. What mass of kerosene is consumed on a flight lasting 3 hours? 18, 000L 0 × 3hr × = 52,110 kg hr L 1 1 1 1 1 for sig. figs. 67 (8 pts) Santa visits about 95,000 chimneys a minute on a certain night of the year (ask Einstein how he does it). How many sleigh loads per hour is this? [USE: 12 presents = 1 chimney, and 27,000 presents = 1 sleigh load] 72 (5 pts) The average Christmas present has a density of 2 kg/L. What would you expect the mass to be of a present having a volume of 3 L? m d = ,so m = dv v  2  ? g = 3 L    L  = 7 = 7 73 (7 pts) One of Santa’s elves determined that the average Christmas present has a density of 2 kg/L. What would you expect the mass to be of a present having a volume of 364 mL? m d = ,so m = dv v  2 kg  1 L  ? g = 364mL     L  1000 mL  = 0 kg = 0 kg, or 783 g 1 pt, sig. figs.; 1 pt m = dv; 2 pts for (1L / 1000 mL) -2 pts for 783 kg (NOTE: This density is unrealistically high, and should be changed.) 74 (2 pts) 8 grams of granite has a density of 2 g/mL. What is the density of 16 g of granite? 2 g/mL Avogadro’s Number 75 (6 pts) How many moles of hydrogen atoms are in 5 × 1022 hydrogen molecules?  1mol   1 H 2 molecule  ? moles H 2 molecules = 5 ×1022 H atoms   23    6 × 10   2 H atoms  = 0 H 2 molecules -2 pts for 0 moles 76 (6 pts) A glass of water contains 4 mol of water molecules. How many hydrogen atoms are in the water?  6 × 1023   2 H atoms  ? H atoms = 4 H 2 O     1mol  1 H 2 O molecule  = 5 ×1024 H atoms 77 (6 pts) How many moles of chlorine atoms are in 4 × 1021 chlorine molecules?  1mol   2 Cl atoms  ? moles Cl 2 atoms = 4 ×1021 Cl molecules   23    6 × 10   1 Cl 2 molecule  = 0 Cl 2 atoms = 0 Cl2 atoms -2 pts for 0 moles; -1 for 0 moles 78 (6 pts) How many moles of bromine atoms are in 8 × 1020 bromine molecules, Br2?  1mol   2 Br atoms  ? moles Br atoms = 8 × 1020 Br2 molecules   23    6 ×10   1 Br2 molecule  = 0 Br atoms = 0 Br atoms -2 pts for 0 moles; -1 for 0 moles Molar Mass from % Abundance 79 (5 pts) A certain element consists of two stable isotopes with the masses and percent abundances given below. Determine the molar mass AND identify this element. (NA = 6 × 1023/mol) Mass of an atom % abundance 1×10-23 1×10-23 ( 1 ×10−23 ) × 0 = 3 ×10−24 + ( 1 × 10−23 ) × 0 = 1 × 10−23 1 ×10−23 × ( 6 ×1023 ) 10 g / mol Identity of element: ___B Molar Mass; grams  moles 80 (4 pts) Determine the molar mass of Ca3(PO4)2. 3Ca 3 × 40 g/mol 2P 2 × 30 g/mol 8O 8 × 16,00 g/mol 310 g/mol 81 (6 pts) How many moles are in 8 g of Ca3(PO4)2?  mol  ? mol = 8 g    310 g  = 0 = 0 82 (5 pts) How many moles are in 2 g of Ca3(PO4)2? 19 80 molar mass Ag ×100 molar mass AgCl 3 for setup, 1 for right answer 107 = × 100 35 + 107 = 75% % Ag = 92 (5 pts) What is the mass percent of nitrogen in N2O (laughing gas)? mass N 2 ×14 / mole %N = ×100 = = 63%Cl mass N 2 O 2 ×14 / mole + 16 g / mole -2 pts for 31% (from not using 2 nitrogens) Formulas from Percent Composition Data 93 (4 pts) 4 g of sulfur combined with 11 g fluorine to produce a gas. What is the empirical formula of the gas? (Must show work to get credit.) S + F → an SF compound 4 g 11 g 0 mol 0 mol Divide by smallest, get 1 S to 4 F, so formula is SF4. 1 each for moles, 1 for 4, 1 for formula 94 (13 pts) The percentage composition of fructose, a sugar, is 40% carbon, 6% hydrogen, and 53% oxygen. The molar mass of fructose is 180 g/mol. What is the molecular formula of fructose? 40% C 40 g C 6% H → 6 g H 53% O 53 g O  mol  ? mol = 40 g C   = 3 C  12   mol  ? mol = 6 g H   = 6 H  1 g   mol  ? mol = 53 g O   = 3 O  16 g  C 3 H 6 O 3 = C1 H2 O1 3 3 3 = CH 2 O, which has a molar mass of 30g/mol. 180/mol = 6, so the molecular formula is C6 H12 O6 . 30g/mol 1 pt, convert to g; 6 pts, convert to mol; 2 pts, divide by smallest; 1 pt, empirical formula; 3 pts, molecular formula. 95 (13 pts) Cacodyl, which has an intolerable garlicky odor and is used in the manufacture of cacodylic acid, a cotton herbicide, has a molar mass of 209 g/mol. Its mass composition is 22% C, 5% H, and 71% As. (Yes, it contains arsenic). What is the molecular formula of cacodyl? 22% C 22 g C 5% H → 5 g H 71% As 71 g As  mol  ? mol = 22 g C   = 1 C  12   mol  ? mol = 5 g H   = 5 H  1 g   mol  ? mol = 71 g As   = 0 As  74 g  C 1 H 5 As 0 = C2 H5 As1 0 0 0 = C2 H 6 As, which has a molar mass of 105g/mol. 209/mol = 2, so the molecular formula is C4 H12 As2 . 105g/mol 1 pt, convert to g; 6 pts, convert to mol; 2 pts, divide by smallest; 1 pt, empirical formula; 3 pts, molecular formula. -7 pts for C4Has better 96 (13 pts) One of the components of frankincense is boswellic acid, which is 78% carbon, 10% hydrogen, and 10% oxygen. The molar mass of boswellic acid is 456 g/mol. What is the molecular formula of boswellic acid? 78% C 78 g C 10% H → 10 g H 10% O 10 g O  mol  ? mol = 78 g C   = 6 C  12   mol  ? mol = 10 g H   = 10 H  1 g   mol  ? mol = 10 O   = 0 O  16 g  99 (10 pts) A white compound that is used to absorb water contains 43% P and 56% oxygen. What is the empirical formula of the compound? 43% P 43 g P →→ 56% O 56 g O  mol  ? mol = 43 g P   = 1 P  30 g   mol  ? mol = 56 g O   = 3 O  16 g  P1 O 3 = P1O2 = P2 / 2 O5 / 2 1 1 = P2 O5 1 pt, convert to g; 4 pts, convert to mol; 2 pts, divide by smallest; 3 pts, convert to P2O5. 100(4 pts) The molar mass of pyrazine is 80 g/mol and its empirical formula is C2H2N. What is its molecular formula? The molar mass of C2H2N is 40 g/mol. The molar mass of pyrazine is twice that, so its molecular formula is C4H4N2. 101(4 pts) A certain edible compound has a molar mass of 180 g/mol. Its empirical formula is CH2O. What is its molecular formula? The molar mass of CH2O is 30 g/mol. Dividing 180 by 30 gives 6, indicating the molecule consists of 6 empirical formula “units”, so its molecular formula is C6H12O6. Product of Combination Reaction 102(4 pts) Bromine and aluminum react to form a white solid. Give the formula of the solid. AlBr3 103(4 pts) Magnesium and nitrogen react to form a gray solid. Give the formula of the solid. Mg3N2 (-1 for Mg2N3) Balanced Reaction of Sodium or Potassium with Water 104(8 pts) Write a balanced equation describing the reaction of sodium metal with water to produce hydrogen gas and sodium hydroxide. 2Na(s) + 2H2O(l) → H2(g) + 2NaOH(aq) 1 pt for states -1 for H instead of H2 105(7 pts) Write a balanced equation describing the reaction of potassium metal with water to produce hydrogen gas and potassium hydroxide. 2K(s) + 2H2O(l) → H2(g) + 2KOH(aq) 1 pt for states, 2 for balancing Oxidation Numbers 106(17 pts) a) Give the oxidation number of each element in the following chemical reaction: 3HNO3(aq) + Al(s)  Al3+ + 3NO2(g) + 3OH-

Was this document helpful?

Premium

This is a Premium Document. Some documents on Studocu are Premium. Upgrade to Premium to unlock it.

Chemistry Test Bank

Course: Honors: General Chemistry I (CHEM 128 )

University: The University of Tennessee

Was this document helpful?

This is a preview

Do you want full access? Go Premium and unlock all 52 pages

Access to all documents
Get Unlimited Downloads
Improve your grades

Upload

Share your documents to unlock

Already Premium?

General Chemistry I Test Bank

Christopher King

Department of Chemistry

Troy State University

Troy, AL 36082

cking@trojan.troyst.edu

This document contains 184 test questions and answers that I have used during the past three

semesters. The text for the course was Jones and Atkins, Chemistry: Molecules, Matter, and

Change, 4th ed., 1999. The questions pertain to chapters 1-4, and 7-9. The equations were created

using MathType equation editor 5.1. This is an upgrade to the equation editor that comes with

Word. I got it so that the equations could be displayed in a blue font (I show answers in blue on

my web pages). To modify the equations, you will need to get the MathType free upgrade

(http://www.dessci.com/en/). If you don’t purchase the upgrade, you can only change colors for

the first 30 days.