Which of the following is an example of a heterogenous mixture? Hot sugar water Air An unopened can of soda Italian salad dressing Which combination of molecules would result in a homogenous mixture? Propanoic Acid (C3H6O2) in Water (H2O) Benzene (C6H6) in Methanol (CH3OH) Hydrobromic acid (HBr) in Toluene (C7H8) Sulfur tetrafluoride (SF4) in Ethanol (C2H5OH) Who formulated a nuclear model that portrays electrons orbiting the nucleus like a planet orbiting the sun? JJ Thomson Ernest Rutherford Gilbert Lewis Niels Bohr James Chadwick Dmitri Mendeleev John Dalton Michael Faraday True or False: As vapor pressure decreases, intermolecular force strength increases. True False Vapor pressure is useless. In the following list, which combination(s) would create a covalently-bonded compound? (CO3) + Sr Cl + Br K + (OH) (PO4) + (NH4) (MnO4) + Na I only II only III only IV only V only I, III, and V II and IV I, III, IV, and V Which nuclear reaction correctly depicts the beta decay of Uranium? 98240U 96236Th + 24He 98240U 98240U +e- 98240U 98240U + γ 98240U 98240U+ +e-
A magical wave has a wavelength of 0.63 mm. What is the frequency of this wave? 4.8 * 1011 Hz 1.9 * 105 Hz 3.0 * 108 Hz 2.1 * 10-12 Hz According to the ________ Principle, the position and velocity of a particle cannot be known at the exact same instant in time. Bohrian Momentum Lewis Cycle Heisenberg Uncertainty Schrodinger Compromise In to pass chemistry lab, 500. mL of C6H6 (MW = 78 g/mol)(ρ = 0.879 g/mL) must be formed by the following reaction: C6H6Br + NaOH C6H6 + NaBr + OH- How many grams of NaOH (MW = 40 g/mol) must be added to achieve the desired yield? 256 g 975 g 225 g 291 g Who is accredited with discovering the proton and nucleus in the early twentieth century? JJ Thomson Ernest Rutherford Gilbert Lewis Niels Bohr Chadwick Dmitri Mendeleev John Dalton Michael Faraday How many of the following ions are isoelectronic with Argon? S3-, Br-, Na+, P3+, Al3+ Zero One Two Three Four Five How many of the following molecules are H2, CHFBr, BI3, SCl2, SiH4, CH3CH2OCH2CH3 Zero One Two Three Four Five Six
The central atom in a strange compound is surrounded by three lone pairs and two single bonds. What is its molecular geometry? Bent Linear Tetrahedral Trigonal Bipyramidal Octahedral Square Pyramidal Trigonal Pyramidal Which ranking of electromagnetic waves is correct based on increasing frequency? X Ray > Gamma Ray > Visible Light > Infrared Visible Light > Infrared > Microwave > Ultraviolet Radio Wave > Microwave > Ultraviolet > Gamma Ray Gamma Ray > Visible Light > Infrared > Radio Wave True or False: Toluene (C7H8) is miscible with benzene (C6H6). True False “Miscible” is not a real word. Which set of quantum numbers corresponds to the electron with the most energy? n = 2, L = 1, mL = 0, ms = -1/2 n = 7, L = 0, mL = 0, ms = -1/2 n = 4, L = 3, mL = -3, ms = n = 5, L = 2, mL = 2, ms = +1/2 What is the hybridization at the starred carbon and oxygen in this molecule? C = sp O = sp C = sp O = sp2 C = sp O = sp3 C = sp2 O = sp C = sp2 O = sp2 C = sp2 O = sp3 C = sp3 O = sp C = sp3 O = sp2 C = sp3 O = sp3
A certain molecule has ten single bonds, three double bonds, and four triple bonds. How many sigma (σ) and pi (π) bonds are in this molecule? 17 σ, 0 π 0 σ, 17 π 11 σ, 17 π 17 σ, 11 π 10 σ, 7 π 7 σ, 10 π 21 σ, 4 π 4 σ, 21 π Which molecule listed below will have the highest viscosity? H2O C2H2 SO2 HCl HI True or False: A pi (π) bond is formed from hybridized orbitals. True False Pi bonds should be eaten. What is the most correct electron configuration for Zr2+? 3d104p64d2 3d104p65s2 3d104p65s14d1 3d104p65s24d2 What is the most correct chemical reaction for the following situation? Liquid toluene (C7H8) is treated with bromine gas and carbon tetrachloride to form a gaseous mixture of benzyl bromide (C7H7Br), chlorine, and dibromo-dichloro methane (CBr2Cl2). C7H8 + Br2 + CCl4 C7H8Br + Cl2 + CCl2Br2 C7H8(L) + Br2(g) + CCl4(g) C7H8Br(g) + Cl2(g) + CCl2Br2(g) 2C7H8(L) + 2Br(g) + CCl4(g) 2C7H8Br(g) + 2Cl(g) + CCl2Br2(g) 2C7H8(L) + Br2(g) + CCl4(g) 2C7H8Br(g) + Cl2(g) + CCl2Br2(g) Reactions that are ________ show energy as a reactant in chemical equations. Single Displacement Isotropic Endothermic Combustion Addition Exothermic 2 2 2
Who discovered the first subatomic particle using the Cathode Ray Experiment? JJ Thomson Ernest Rutherford Gilbert Lewis Niels Bohr James Chadwick Dmitri Mendeleev John Dalton Michael Faraday Rank the following in terms of atomic size: Se, I, Rb, Fr, C, V, F Fr > Rb > C > V > I > Se > F Fr > C > I > Se > Rb > V > F Fr > Rb > V > I > Se > C > F Fr > I > Rb > V > C > Se > F A Bohr Model electron moves from n = to n = 7. How much energy was added or released to cause this transition? -5.01 * 10-19 J 5.01 * 10-19 J -7.79 * 10-19 J 7.79 * 10-19 J For the Angular Quantum Number, L = 0 corresponds to a(n) ______ orbital, and L = represents a(n) ______ orbital. s, f d, p p, s s, d This principle states that low-energy orbitals are filled before high-energy orbitals. Aufbau Principle Hund’s Rule Pauli Exclusion Principle Heisenberg Uncertainty Principle Photoelectric Effect ___GeF4 + ____Na2O ___GeO2 + ___NaF In the reaction, how many grams of Na2O is required to produce 25 g GeO2? 30. g 84 g 7.4 g 21 g The empirical formula for Catechol is C3H3O. If the molecular weight of this compound is 110.1 g/mol, what is the molecular formula? C12H12O4 C9H9O3 C6H6O2 C3H3O
Red light has a wavelength of 700 nm, lime-colored light is 560 nm, cyan light is 490 nm, and violet is 410 nm. Which colored light possesses the most energy? Cyan Lime Red Violet What two subgroups constitute pure substances? Elements and mixtures Suspensions and compounds Compounds and elements Mixtures and suspensions Matter and elements ________ refers to a solid changing to a gas in one step, and _______ refers to a liquid that changes into a gas. Vaporization, Melting Deposition, Vaporization Freezing, Condensation Sublimation, Vaporization Deposition, Sublimation Condensation, Freezing Which of the following pairs of compounds would combine to form a solution? CH2BrI and H2O C2H5OH and CF4 C6H6 and HCN H2O and C4H10 What is the overall charge on the following molecule? -2 -1 0 +1 +2 What is the proper name for Au(ClO4)3 Gold Chlorotetraoxide Gold (III) Perchlorate Gold (III) Chlorate Gold (III) Chlorite Gold (III) Hypochlorite Gold (I) Perchlorate Gold (I) Chlorate Gold (I) Chlorite Gold (I) Hypochlorite
The ________ and _______ are found in the nucleus, while the ________ are found in orbitals surrounding the nucleus. Neutrons, Electrons, Protons Protons, Electrons, Neutrons Protons, Neutrons, Electrons Electrons, Neutrons, Protons Electrons, Protons, Neutrons Which of the following molecules would have the highest boiling point? GaI3 KI CuTe CaBr2 AgF The electronegativity difference between two atoms is 0.80. Is this molecule nonpolar, polar, or ionic? Ionic Nonpolar Polar It doesn’t matter. Which of the following is nonpolar? Chlorine monoiodide Hexane C2H5COOH Rubidium Fluoride Who published a theory on the existence and properties of atoms in the beginning of the 19th century? JJ Thomson Ernest Rutherford Gilbert Lewis Niels Bohr James Chadwick Dmitri Mendeleev John Dalton Michael Faraday How many atoms of oxygen are in 33 g C6H5NO2? 33 * 1023 atoms 3.2 * 1023 atoms 4.9 * 1027 atoms 8.8 * 10-25 atoms 2041Ca, 2045Ca, and 2037Ca are all __________ of the element calcium. Ions Isotopes Reactions Metalloids Which of the following elements is the most electronegative? Os As Na Cl B I
Fr How many of the following molecules demonstrate ionic character? HF, GaI3, NH4F, O2, CH3OH, BaS, Al(PO4) Zero One Two Three Four Five Six Seven Which of the following is the smallest atom? Rb+, Sr+, Br-, Ba, As3-, Br- Ba Rb+ As3- Sr+ set of quantum numbers corresponds to the last electron added to Gold? n = 6, L = 2, mL = 1, ms = -1/2 n = 5, L = 1, mL = -1, ms = n = 6, L = 3, mL = 2, ms = +1/2 n = 5, L = 3, mL = 1, ms = -1/2 n = 6, L = 2, mL = -1, ms = +1/2 n = 5, L = 2, mL = 1, ms = -1/2 n = 6, L = 2, mL = -1, ms = n = 5, L = 3, mL = -2, ms = +1/2 How many micromoles of molybdenum(VI) chloride are produced in the following reaction if 11 L of molten MgCl2 (ρ = 2.32 kg/L) is added? ____Mo(SiO3)3 + ___MgCl2(l) ____Mg(SiO3) + ____MoCl6 8.94 * 107 μmol 8.51 * 109 μmol 1.68 * 107 μmol 7.22 * 101 μmol 7.66 * 10-2 μmol 24.112 mg of glucose is to be added to 6.20 mg of water. What is the total mass of the solution (in mg) to the correct number of sig figs? 24.17 mg 24.2 mg 644.11 mg 644 mg 30.3 mg 30.31 mg 86.11 mg 86 mg Which of the following elements would have properties most like Phosphorus?
F Li C N S Al Who first created a basic version of the periodic table in the mid-late 19th century? JJ Thomson Ernest Rutherford Gilbert Lewis Niels Bohr Chadwick Dmitri Mendeleev John Dalton Michael Faraday 130Te has _______ protons, _______ neutrons, and ________ electrons. 52, 130, 52 130, 52, 52 52, 52, 130 52, 78, 52 78, 52, 52 52, 52, 78 26, 78, 26 78, 26, 26 26, 26, 78 How much energy per photon is contained in a wave whose wavelength is 104 nm? 2.07 * 10-32 J 1.91 * 10-18 J 2.30 * 10-49 J 31.2 J Ionization energy increases as you move ______ and ______ across the periodic table. Left and Up Right and Up Left and Down Right and Down What is the molecular geometry of Iodine Tetrafluoride? (Hint: free radicals count as an electron domain (“port”)) Tetrahedral Square Pyramidal Square Planar Octahedral Linear For n = 5, what are the possible values for the angular quantum number, L? 0,1,2, 0,1,2,3 0,1,2,3,4 0,1,2,3,4,5 0 1 3 4 5 True or False: Hund’s Rule states that you pair electrons before filling other orbitals at the exact same energy level. True False
Which of the following are diatomic atoms? Carbon Nitrogen Helium Hydrogen Sulfur Lithium Iodine I only II only III only IV only V only VI only VII only VIII only More than one is correct What is the most proper name of PbSO4? Probium Sulfur Tetraoxide Probium Sulfite Probium Sulfate Lead (II) Sulfur Tetraoxide Lead (II) Sulfite Lead (II) Sulfate Lead (I) Sulfur Tetraoxide Lead (I) Sulfite Lead (I) Sulfate How many of the following are resonance structures for the compound above? None One Two Three Four How many of the following are strong electrolytes? NaBr, CH3COOH, C6H5F, NH4Cl, HNO3, H2CO3 Zero One Two Four Five Six Which of the following is not a strong acid? HBr H3PO4
H2SO4 HClO4 HF There are two correct answers. Three are three correct answers. None of the above. How would you prepare a 4.2 M solution of MgO (MW = 40.3 g/mol)? 170 g MgO 9.6 g MgO 81 g MgO 430 g MgO How many of the following are soluble in water? AgNO3, Ba(OH)2, HgCH3COO, HClO3, Li3(PO4) One Two Three Four Five As temperature _________, liquid solubility decreases, and as pressure _________ gas solubility increases. Increases, Increases Increases, Decreases Decreases, Increases Decreases, Decreases Which of the following is a strong base? NH4+ Ag(OH) Sr(OH)2 C5H10N Mg(OH)2 What is the molarity of a 23.15 g sample of NH4CH3COO that is dissolved in water to give 800. mL of solution? 28.9 M 0.240 M 0.375 M 2.66 M Barium hydroxide is added to water to form a 1 L solution. How many moles of hydroxide ions are in the solution if 42 g Ba(OH)2 was added? 21 mol OH- 0.25 mol OH- 0.49 mol OH- 2.47 mol OH- 4.9 mol OH- What do the following reactions represent? I)2CuNO3(aq) + K2CO3(aq) 2KNO3(aq) + Cu2(CO3)(s) II)NH4+(l) + NH3(l) + CH3COOH(l) II)HI(aq) + Rb(OH)(aq) RbI(aq) + H2O(l) I) Precipitation II/III) Acid-Base I) Redox II/III) Precipitation I) Precipitation
II) Combustion III) Acid-Base I/II) Redox III) Acid-Base How many of the following would you expect to see dissolve in ethanol (C2H5OH)? Iron (III) Nitrate Cesium Fluoride Molybdenum (VI) Acetate Calcium Chlorate Strontium Hydroxide Lithium Sulfide One Two Three Four Five Six PdI2(aq) + 2HgNO3(aq) Pd(NO3)2(aq) + 2HgI(s) In the reaction above, who is(are) the spectator ion(s)? Pb2+ I- Hg+ NO3+ Pb2+ and I- Pd2+ and NO3- Hg+ and NO3- I- and Hg2+ How do you prepare a 21% by volume solution of aqueous hydroiodic acid? 79 mL HI per 100 mL 79 L HI per 100 mL 21 mL HI per 100 mL 21 L HI per 100 mL 12 mL HI per 100 mL 12 L HI per 100 mL 3250 cm3 of a 3.40 M potassium hydroxide solution is to be diluted to 1.10 M. What will be the final volume (in liters) of the solution? 1.15 L 10.1 L 1.05 L 6.05 L A(n) ____________ _____ is a proton donor in solution. Brønsted–Lowry Acid Arrhenius Base Arrhenius Acid Brønsted–Lowry Base What is the oxidation state of carbon in CO32-? -2 +2 –4 +4 -6
39% 2C6H7Br + Sr(OH)2 + SrBr2 + 2H2O Using the above reaction, what is the maximum amount of benzene (C6H6) that is produced when 42.1 g C6H7Br (MW = 159 g/mol) and 49.5 g Sr(OH)2 (MW = 121 g/mol) are added? 6690 mol C6H6 0.265 mol C6H6 5990 mol C6H6 0.818 mol C6H6 0.133 mol C6H6 0.409 mol C6H6 142 mol C6H6 How many of the following are strong electrolytes? HF, Sr(OH)2, HNO3, HNO2, AgBr One Two Three Four Five Six __CaCO3 3CaO + __CO2 In the above reaction, 10.3 kg of CaCO3 (MW = 100.09 g/mol) is used to produce calcium oxide and carbon dioxide. If the actual yield of CaO (MW = 56.08 g/mol) is 4.32 kg, what is the percent yield? 63% 75% 52% 83% 31% Oxidation can be described in three ways: the gain of ______, loss of ______, or the _______ of electrons. Hydrogen, Oxygen, Gain Hydrogen, Oxygen, Loss Oxygen, Hydrogen, Gain Oxygen, Hydrogen, Loss What is the molarity of a nitrobenzene (C6H5NO2) solution if there are 6.2 moles in 720 mL of liquid? 0.0086 M 120 M 0.12 M 8.6 M Reduction is the _______ of electrons, and a(n) _______ in the oxidation number. Gain, Decrease Gain, Increase
Loss, Decrease Loss, Increase How many of the following are strong Be(OH)2, NO2-, NaOH, HClO, Ba(OH)2, OH- One Two Four Five Six IF + CH4 HF + CH3I In the above reaction, carbon was ______ because its oxidation number _______. Reduced, Increased Reduced, Decreased Oxidized, Increased Oxidized, Decreased An unknown compound consists of 36% carbon, 54% beryllium, and 9% hydrogen by mass. What is the empirical formula for this unknown compound? CBeH C2Be4H2 C3Be2H C2Be3H CBe2H3 C3BeH2 What is the oxidation number of manganese in RbMnO4? +8 +7 +6 +5 +4 0 -4 -5 -6 -7 -8 + Sr(NO3)2 Be(NO3)2 + SrSO4 In the above reaction, is a precipitate formed? Yes No It’s impossible to tell. If 5.000 mol Ba2TiO4 (MW = 386.5 g/mol) is combined in sulfuric acid, how many grams of barium sulfate (MW = 233.4 g/mol) is produced? ___Ba2TiO4 + ___H2SO4 ___H4TiO4 + ___BaSO4 1167 g BaSO4 1933 g BaSO4 3865 g BaSO4 2334 g BaSO4 6.039 g BaSO4