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115 Cards in this Set
- Front
- Back
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Which of the following is the lowest temperature? A. 42°C B. 57°C C. 318 K D. I ain't tellin' ya |
B. 57°C |
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A block of metal occupies a volume of 0.0950 L. What volume (L) would an equal mass of ethanol occupy? The density of the metal is 13.546 g/mL and the density of ethanol is 0.789 g/mL. A. 16.3 B. 12.9 C. 1.63 D. Never seen this question before! |
A. 16.3 |
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Which of the following are examples of extensive properties? A. Odor B. Temperature C. Density D. Mass E. Color |
D. Mass |
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How many argon atoms are contained in 7.66 x 10^5 mmol of argon? A. 1.84 x 10^28 Ar atoms B. 7.86 x 10^20 Ar atoms C. 1.15 x 10^28 Ar atoms D. 4.61 x 10^26 Ar atoms E. 3.24 x 10^26 Ar atoms |
D. 4.61 x 10^26 Ar atoms |
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(Interesting) When 0.1595 of a C,H,O containing compound are burned in a combustion apparatus, 0.449 g of CO2 and 0.184 g H2O are formed. Calculate the molecular formula of the original compound. GFM of original compound is 156 g/mol. A. C10H10O B. C10H20O C. C10H4O2 D. C8H20O2 E. OMH! |
B. C10H20O
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(Interesting) How many atoms of oxygen are contained in 47.6 g of aluminum carbonate? The molar mass of aluminum carbonate is 233.99 g/mol. A. 1.10 x 10^24 O atoms B. 3.68 x 10^23 O atoms C. 2.87 x 10^25 O atoms D. 2.96x 10^24 O atoms E. 1.23x 10^23 O atoms |
A. 1.10x 10^24 O atoms
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If an object has a density of 8.65 g/cm^3, what is its density in units of kg/m^3? A. 8.65 x 10^1 kg/m^3 B. 8.65 x 10^-7 kg/m^3 C.8.65 x 10^3 kg/m^3 D.8.65 x 10^-1 kg/m^3 E.8.65 x 10^-3 kg/m^3 F. Bruh |
C. 8.65 x 10^3 kg/m^3 |
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Give the formula for calcium hydrogen sulfate. A. CaHSO4 B. Ca2(HSO4)2 C. Ca2HSO4 D. Ca(HSO4)2 |
D. Ca(HSO4)2 |
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What mass (in mg) does 2.63 moles nickel have? A. 1.54 x 10^5 mg B. 44.8 mg C. 129 mg D. 2.23 x 10^4 mg E. 3.56 x 10^5 mg |
A. 1.54 x 10^5 mg |
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If the temperature is 128°F, what is the temperature in degrees Celsius? A. -145°C B. 262.4°C C. 328°C D. 401°C E. 53.3°C |
E. 53.3°C |
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Determine the volume of an object that has a mass of 455.6 g and a density of 19.3 g/cm^3. A. 87.9 mL B. 31.2 mL C. 42.4 mL D. 18.5 mL E. 23.6 mL |
E. 23.6 mL
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Systematic error is defined as
A. error that averages out the repeated trials B. error that is random C. error that tends to be too high or too low D. Not being a Chem/Biochem major!!! |
C. error that tends to be too high or too low
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Predict the charge that an ion formed from sulfur would have. A. 1- B. 2- C. 4+ D. 3- E. 6+ |
B. 2-
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How many molecules are in 2.50 moles of SO2? A. 7.53 x 10^23 atoms B. 4.52 x 10^24 atoms C. 3.01 x 10^24 atoms D. 1.51 x 10^24 atoms E. 5.02 x 10^23 atoms |
D. 1.51 x 10^24 atoms |
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Calculate the atomic mass of gallium if gallium has 2 naturally occurring isotopes with the follow masses and natural abundances: Ga-69 68.9256 amu 60.11% Ga-71 70.9247 amu 39.89% A. 69.93 amu B. 70.68 amu C. 69.80 amu D. 70.00 amu E. 69.72 amu |
E. 69.72 amu |
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Determine the empirical formula for a compound that is 36.86 % N and 63.14% O by mass. A. N2O B. N2O3 C. NO3 D. NO2 E. NO |
B. N2O3
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Give the name for SnO. A. tin (I) oxide B. tin (III) oxide C. tin (IV) oxide D. tin (II) oxide |
D. tin (II) oxide
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Round off 00907506 to four significant figures.
A. 9076 B. 9.075 x 10^5 C. 9100 D. 0091 |
B. 9.075 x 10^5 |
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Convert 10 cm^3 to m^3.
A. 1 x 10^7 m^3 B. 1 x 10^3 m^3 C. 1 x 10^-5 m^3 D. 1 x 10^-1 m^3 |
C. 1 x 10^-5 m^3
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Semiconductors are
A. metalloids B. metals C. noble gases D. nonmetals |
A. metalloids
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A substance composed of two or more elements in a fixed, definite proportion is
A. a compound B. a solution C. a homogeneous mixture D. a heterogeneous mixture E. SOMETHING |
A. a compound
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Convert 2μm to meters.
A. 2 x 10^-3 m B. 2 x 10^-6 m C. 2 x 10^-9 m D. 2 x 10^6 m |
B. 2 x 10^-6
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The recommended dosage for a prescription drug is 6.00 mg/kg of body mass. Calculate the dose in kilograms for a 115-lb human. 1 lb=453.59 g. A. 31.13 x 10^-4 B. 3.13 x 10^-4 C. 0.313 D. I don't like such questions! |
B. 3.13 x 10^-4
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Which of the following contains 39% carbon by mass? A. CH4 B. CH3NH2 C. CO2 D. C2H2 |
B. CH3NH2
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The diameter of an atom is approximately 1 x 10^-10 m. What is the diameter in millimeters? A. 1 x 10^-7 mm B. 1 x 10^-13 mm C. 1 x 10^-4 mm D. 1 x 10^-16 mm |
A. 1 x 10^-7 mm
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If a room needs 25.4 square yards of carpeting, what is the area of the floor in units of ft^2? A. 2.29 x 10^2 B. What's ft? C. 15.1 D. 229 |
A. 2.29 x 10^2
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Which of the following is the SMALLEST volume? A. 22 cm^3 B. 0.50 dL C. 2.8 10^3 mL D. 5.0 x 10^7 nL |
A. 22 cm^3
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A mass of mercury occupies 0.950 L. What volume would an equal mass of ethanol occupy? The density of mercury is 13.546 g/mL and the density of ethanol is 0.789 g/mL. A. 0.0553 L B. 16.3 L C. 18.1 L D. 0.0613 L |
B. 16.3 L
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How many electrons does the Al3+ ion possess? A. 10 B. 16 C. 13 D. 0 E. 6 |
A. 10
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Calculate the mass (in kg) of 4.87 x 10^25 atoms of Zn. A. 1.89 kg B. 1.09 kg C. 1.24 kg D. 5.29 kg E. 8.09 kg |
D. 5.29 kg
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Determine the number of protons, neutrons, and electrons in the following: 65 29 X A. p+ = 29 n° = 29 e- = 36 B.p+ = 36 n° = 29 e- = 36 C.p+ = 29 n° = 36 e- = 36 D.p+ = 29 n° = 36 e- = 29 E.p+ = 36 n° = 36 e- = 29 |
D. p+ = 29 n° = 36 e- = 29
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How many protons does the Br- ion possess? A. 36 B. 35 C. 34 D. 6 E. 8 |
B. 35 |
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How many electrons are in the ion, Cu2+? A. 64 B. 27 C. 29 D. 31 |
B. 27
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What element is defined by the following information? p+ = 11 n° = 12 e- = 11 A. Vanadium B. Titanium C. Magnesium D. Sodium |
D. Sodium
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(Interesting) Calculate the molar mass for magnesium perchlorate A. 123.76 g/mol B. 247.52 g/mol C. 119.52 g/mol D. 223.21 g/mol E. 75.76 g/mol |
D. 223.21 g/mol
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What is the mass (in kg) of 6.89 x 10^25 molecules for CO2? The molar mass of CO2 is 44.01 g/mol. A. 3.03 kg B. 3.85 kg C. 5.04 kg D. 2.60 kg E. 6.39 kg |
C. 5.04 kg
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(Interesting) Calculate the mass percent composition of sulfur in aluminum sulfate. A. 42.73% B. 9.372% C. 35.97% D. 28.12% E. 21.38% |
D. 28.12%
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If the walls in a room are 955 square feet in area, and a gallon of paint covers 15 square yards, how many gallons of paint are needed for the room? (3 ft = 1 yard) A. 24 gallons B. 47 gallons C. 7.1 gallons D. 2.3 gallons E. 21 gallons |
C. 7.1 gallons
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Identify the instrument that is used to determine the mass of a molecule. A. infrared spectrometer B. ultraviolet spectrophotometer C. gas chromatograph D. a golf club E. mass spectrometer |
E. mass spectrometer
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(Interesting) How many atoms of carbon are contained in 47.6 g of aluminum carbonate? The molar mass of aluminum carbonate is 233.99 g/mol? A. 2.96 x 10^24 C atoms B. 2.87 x 10^25 C atoms C. 3.68 x 10^23 C atoms D. 1.10 x 10^24 C atoms E. 1.23 x 10^23 C atoms |
C. 3.68 x 10^23 C atoms |
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The factor 10^-3 corresponds to which prefix? A. deka B. milli C. centi D. deci |
B. milli
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Determine the name for CoCl2 x 6H2O. Remember the Co forms several ions. A. cobalt (I) chloride heptahydrate B. cobalt (II) chloride C. cobalt (II) chloride hexahydrate D. cobalt (II) chloride heptahydrate E. cobalt chloride hydrate |
C. cobalt (II) chloride hexahydrate
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How many atoms of oxygen are in 2.50 moles of CO2? A. 7.53 x 10^23 atoms B. 1.51 c 10^24 atoms C. 3.01 x 10^24 atoms D. 5.02 x 10^23 atoms E. 4.52 x 10^24 atoms |
C. 3.01 x 10^24 atoms |
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How many atoms are in 2.50 moles of SO2? A. Never covered this in class B. 1.52 x 10^24 atoms C. 3.01 x 10^24 atoms D. 7.53 x 10^23 atoms E. 4.52 x 10^24 atoms |
E. 4.52 x 10^24 atoms
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Complete this phrase as used in this class; "Stay happy, ........................................................." |
A. You have incredible value
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Identify the common substance that has the lowest density. A. ethanol B. table salt C. titanium D. aluminum E. sugar |
A. ethanol
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Which of the following are examples of extensive properties? A. color B. solubility C. temperature D. density E. mass |
E. mass
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How many cm^3 are contained in 3.77 x 10^4 mm^3? A. 3.77 x 10^1 cm^3 B. 3.77 x 10^-10 cm^3 C. 3.77 x 10^6 cm^3 D. 3.77 x 10^20 cm^3 E. 3.77 x 10^4 cm^3 |
A. 3.77 x 10^1 cm^3
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How many liters of air are in a room that measures 10.0 ft x 11.0 ft and has an 8.00 ft ceiling? 1 in = 2.54 cm; 1 L = 10^3 cm^3 A. 2.49 x 10^4 B. 8.84 x 10^5 C. 2.68 x 10^7 D. 2.49 E. ant |
A. 2.49 x 10^4
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Calculate the amount of heat (of kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K to 385.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. A. 28.4 kJ B. 16.6 kJ C. 57.0 kJ D. 73.6 kJ E. 12.9 kJ |
B. 16.6 kJ
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(Interesting) Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide. _Ca(OH)2(aq)+_H3PO4(aq) -> _Ca3(PO4)2(aq) + _H2O(l) A. 33.8 mL B. 15.0 mL C. 22.5 mL D. OMH! |
B. 15.0 mL
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50.0 mL of a 0.500 M NaOH solution is placed in a coffee cup calorimeter at 25 degrees C and combined with 25.0 mL of 0.5M HCl at the same temperature. The final temperature attained by the solution is 27.21 degrees C. Assuming that the volumes are additive, the final density of the mixture is 1.00 g/mL, and the specific heat capacity is 4.184 J/g degree C, Calculate the ΔH of the reaction in kJ.
A. -55.4 B. -693 C. 693 D. WTH |
A. -55.4
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What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution? 2AgC2H3O2 + MgCl2 -> 2AgCl + Mg(C2H3O2)2 A. 2.56 g B. 0.859 g C. 0.838 g D. 1.70 g E. 1.72 g |
C. 0.838 g
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Consider the following balance reaction. How many grams of water are required to form 75.9 g of HNO3? Assume there is no excess NO2 present. The molar masses are as follows: H2O=18.02 g/mol, HNO3=63.02 g/mol. 3NO2 + H2O -> 2HNO3 + NO A. 10.9 g H2O B. 26.5 g H2O C. 43.4 g of H2O D. 38.0 g of H2O E. I don't like this question |
A. 10.9 g H2O
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A mixture of 0.220 moles CO, 0.350 moles N2 and 0.640 moles Ne has a total pressure of 2.95 atm. What is the pressure of CO? A. 0.536 atm B. 0.649 atm C. 1.86 atm D. 1.54 atm E. 0.955 atm |
A. 0.536 atm
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Which of the following samples has the greatest density at STP?
A. Xe B. NO2 C. SF6 D. SO2 E. What does STP mean? |
C. SF6
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How many milliliters of a 0.266 M NaNO3 solution are required to make 150.0 mL of 0.075 M NaNO3 solution? A. 53.2 mL B. 42.3 mL C. 18.8 mL D. 23.6 mL E. 35.1 mL |
B. 42.3 mL
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Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed. A. 2Li+ + S2- + Cu2+ + 2NO3- -> CuS + 2Li+ + 2NO3- B. Li+ + S- + Cu+ NO3- -> CuS + LiNO3 C. 2Li+ + S2- + Cu 2+ + 2NO3- -> Cu2+ +S2- +2LiNO3 D. Li+ + SO4 2- + Cu+ + NO3- -> CuS + Li+ +NO3- E. NOPE |
A. 2Li+ + S2- + Cu2+ + 2NO3- -> CuS + 2Li+ + 2NO3-
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In the following reaction (balanced) identify the species that is reduced HBr + KOH -> H2O + KBr A. K B. Br C. O D. H |
D. H
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(Interesting) A 10.0 mL solution of 1.00 M AgNO3 is added to 10.0 mL NaCl solution is a calorimeter at 25°C to form AgCl solid/ppt. The temperature of the aqueous mixture increases to 32.6°C. The specific heat of the aqueous mixture is 4.18 J/g°C and the density of the mixture is 1.00 g/mL. Assuming the calorimeter absorbs no heat; calculate the ΔH per mole of AgCl for the reaction in kJ. Assume volume of solution is additive. A. 6.53 B. 65.3 C. 63.5 D. 53.6 |
C. 63.5
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What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385K? A. 53.1 g B. 69.2 g C. 86.7 g D. 18.8 g E. 24.4 g |
C. 86.7 g
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How many grams of CaCl2 are formed when 15.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas?
2 Ca(OH)2 + 2 Cl2 ->Ca(OCl)2 + CaCl2 + 2H2O A. 0.0507 g B. 0.00789 g C. 0.00197 g D. 0.00394 g |
C. 0.00197 g |
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Lithium and nitrogen react in a combination reaction to produce lithium nitride:
6Li + N2 -> 2Li3N How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen? A. 0.40 B. 3.6 C. 0.30 D. 0.20 E. 1.8 |
E. 1.8 |
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A student prepared a stock solution by dissolving 10.0g of KOH in enough water to make 150 mL of solution. She then took 15 mL of the stock solution and diluted it with enough water to make 65 mL of a final solution. What is the concentration of KOH for the final solution? A. 3.56 M B. 2.81 M C. 0.274 M D. 0.356 M |
C. 0.274 M |
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A fixed amount of gas at 25°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.
A. 7.56 L B. 2.07 L C. 10.9 L D. 48.4 L E. 13.2 L |
E. 13.2 L
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A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne?
A. 0.54 atm B.1.3 atm C. 1.1 atm D.0.40 atm E. 0.80 atm |
C. 1.1 atm
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A gas occupies 22.4 L at STP and 19.0L at 100°C and 1.50 atm pressure. How many moles of gas did the system gain or lose?
A. 0.08 moles gained B. 0.01 moles lost C. 0.01 moles gained D. 0.07 moles lost |
D. 0.07 moles lost
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Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4.
Some possibly useful molor masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol N2O4 (l) + 2 N2H4 (l) ---> 3 N2(g) + 4 H2O(g) A. LR=N2O4, 45.7 g N2 formed B. LR=N2H4, 59.0 g N2 formed C. LR=N2O4, 105 g N2 formed D. No LR, 45.0 g N2 formed E. LR=N2H4, 13.3 g N2 formed |
A. LR=N2O4, 45.7 g N2 formed
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How many molecules of sucrose are contained in 14.3 ml of 0.140 M sucrose solution?
(C12H22O11, molar mass=342.30 g/mol) A. 1.21 x 10^21 molecules B. 5.90 x 10^24 molecules C. 1.63 x 10^23 molecules D. 8.29 x 10^22 molecules E. 6.15 x 10^22 molecules |
A. 1.21 x 10^21 molecules
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Determine the density of CO2 gas at STP.
A. 1.96 g/L B. 1.80 g/L C. 2.24 g/L D. 4.46 g/L E. 5.10 g/L |
A. 1.96 g/L
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A gas occupies 4.23 L at 2.25 atm. What is the volume at 3.46 atm?
A. 1.84 L B. 32.9 L C. 2.75 L D. 6.50 L E. 0.364 L |
C. 2.75 L
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When 1.22 g of HC7H5O2 (MM 122.12) is burned in a bomb calorimeter; the temperature rises from 20.27°C to 22.67°C. If ΔE for the reaction is -3.23 x 10^3 kJ/mol, what is the heat capacity of the calorimeter in kJ/°C?
A. 32.3 B. 14.3 C. 32.27 D. 13.4 |
D. 13.4
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Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.
A. 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) B. 2 H+(aq) + CO32-(aq) → H2CO3(s) C. 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) D. 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) E. No reaction occurs. |
A. 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)
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When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed?
A. 1.07 g B. 2.24 g C. 6.44 g D. 3.31 g |
A. 1.07 g |
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(Interesting) How many pounds of CO2 are produced from the complete combustion of 1.00 gal of gasoline?Assume that gasoline has the formula C8H18 and has a density of 0.703 g/mol?
(1 gallon = 3785 mL) A. 2660 B. 1.81 C. 18.1 D. 81.9 |
C. 18.1
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(Interesting) The titration of 80ml of an unknown concentration of H3PO4 solution requires 126ml of 0.218M KOH solution. What is the concentration of the H3PO4 solution (in M)?
A. 0.114 M B. 0.343 M C. 1.03 M D. 0.138 M E. 0.0461 M |
A. 0.114 M
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Which of the following substance would show the greatest temperature change upon absorbing 100 J of heat?
A. 10.0 g H2O, CH2O = 4.18 J/g°C B. 10.0 g ethanol, Cethanol = 2.42 J/g°C C. 10.0 g Cu, CCu= 0.385 J/g°C D. 10.0 g Pb, CPb= 0.128 J/g°C E. 10.0 g Al, CAl = 0.903 J/g°C |
D. 10.0 g Pb, CPb= 0.128 J/g°C
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A balloon is inflated from L to 0.400 L against an external pressure of 10.00 atm. How much work is done in joules? 101.3 J = 1 L x atm
A. -0.395 J B. -39.5 J C. 0.395 J D. -395 J E. 39.5 J |
B. -39.5 J |
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Complete this phrase as used in this class, "Stay happy..........................................."
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A. You have incredible value.
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Lithium and nitrogen react to produce lithium nitride:
6Li+N2---2Li3N How many moels of N2 are needed to react with 0.500 mol of lithium? A. 0.500 B. 3000 C. 1.50 D. 0.167 E. 0.0833 |
E. 0.0833
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Determine the theoretical yield of H2S (in moles) if 64.0 mol Al2S3 and 4.0 mol H2O are reacted according to the balanced reaction. (Al2S3, MM= 150.17 g/mol) AL2S3(S)+6H2O(L)-2AL(OH)3(S)+3H2S(G) A. 128 mol H2S B. 64 mol H2S C. 32 mol H2S D. 192 mol H2S E. 96 mol H2S |
C. 32 mol H2S
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Based on the balanced chemical equation shown below, detemine the molarity of a solution containing Fe^2+aq if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0.250 M potassium bromate, KBrO3(aq), solution.
The chemical equation for the reaction is 6Fe^(2+)aq + BrO3^(-)aq + 6H^(+) -->6Fe^(3+)aq + Br6(-)aq + 3H2O A. 1.12 M B. 0.188 M C. 0.0312 M D. 2.00 M |
A. 1.12 M
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How many of the following species are diamagnetic?
Fr Zr2+ Al3+ Hg2 A. 4 B. 1 C. 0 D. 2 E. 3 |
D. 2
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(Interesting) The de Broglie wavelength of an electron with a velocity of 6.00 x 10^6 m/s is ____ m. The mass of the electron is 9.11 x 10^-22 micrograms.
A. 8.25 x 10^12 B. 8.25 x 10^9 C. 1.21 x 10^-13 D. 1.21 x 10^-10 E. 1.21 x 10^-16 |
D. 1.21 x 10^-10
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When a wave encounters an obstacle or slit that is comparable in size to its wavelength, it bends around it. This characteristic is called____.
A. Destructive interference B. Diffraction C. Distraction D. Constructive Interference E. Something |
B. Diffraction
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How many unpaired electrons are present in the ground state As atom?
A. 1 B. 4 C. 2 D. 0 E. 3 |
E. 3
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Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 x 10^8 MHz.
A. 436 nm B. 485 nm C. 206 nm D. 675 nm E. 229 nm |
A. 436 nm
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Give the ground state electron configuration for the ion of Ba.
A. [Kr] 5s24d105p6 B. [Kr] 5s24d105p66s26p2 C.[Kr] 5s25p6 D. [Kr] 5s24d105p66s1 E.[Kr] 5s24d105p66s2 |
A. [Kr] 5s24d105p6 |
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An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz. The wavelength of this radiation is ____m.
A. 3.018 x 10^16 B. 3.018 x 10^10 C. 0.3353 D. 2.982 E. 2.982 x 10^6 |
D. 2.982
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Give the ground state electron configuration for Br-.
A. [Ar]4s23d104p6 B.[Ar]4s24d104p6 C. [Ar]4s23d104p4 D.[Ar]4s24p6 E. [Ar]4s23d104p5 |
A. [Ar]4s23d104p6
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Identify the color flame test for lithium.
A. violet B. blue C. yellow D. red E. white |
D. red
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Place the following elements in order of decreasing atomic radius.
Xe Rb Ar A. Rb>Xe>Ar B. Ar>Rb>Xe C. Xe>Rb>Ar D. Rb>Ar>Xe E. Ar>Xe>Rb |
A. Rb>Xe>Ar
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Which of the following types of electromagnetic radiation has the lowest frequency?
A. orange B. purple C. blue D. yellow E. green |
A. orange
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Give the ground state electron configuration for Se.
A. [Ar]4s23d104p4 B.[Ar]3d104p4 C.[Ar]4s23d10 D.[Ar]4s23d104p6 E. [Ar]4s23d104p4 |
A. [Ar]4s23d104p4
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Choose the paramagnetic species from below.
A. Nb3+ B. O2- C. Zn2+ D. Cd E. Ca |
E. Ca
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(Interesting) Calculate the total energy (in kJ) contained in 1.0 mol photons, all with a frequency of 2.75 x 10^8 MHz?
A. 110 B. 1.82 x 10^-19 C. 109.7 D. 1.10 x 10^2 |
D. 1.10 x 10^2
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How many of the following species are paramagnetic?
Sc3+ Cl- Ba2+ Se A. 3 B. 4 C. 2 D. 0 E. 1 |
E. 1
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Identify the number of valence electrons in Cl-1.
A. 6 B. 8 C. 5 D. 4 E. 7 |
B. 8
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Identify the species that has the smallest radius. A. N0 B. N3+ C. N1+ D. N2- E. N5- |
B. N3+
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Choose the diamagnetic species from below.
A. I B. N C. Sn2+ D. Cr E. None of the above are diamagnetic |
C. Sn2+
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How many orbitals are there in the fourth shell?
A. 4 B. 16 C. 6 D. 3 |
B. 16
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Choose the ground state electron configuration for Ti2+. A. [Ar]4s2 B. [Ar]3d4 C. [Ar]4s23d2 D. [Ar]3d2 E. [Ar]4s23d4 |
A. [Ar]4s2
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(Interesting) Determine the mass of a particle with a wavelength of 3.45 x 10^-34 m and a velocity of 655 cm/s.
A. 293 g B. 12.6 g C. 346 g D. 3.41 g E. 0.293 g |
A. 293 g
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(Interesting) Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of 5.49 x 10^5 GHz. Avogadros number is 6.022 x 10^23.
A. 4.68 x 10^19 J B. 2.75 x 10^-19 J C. 3.64 x 10^-19 J D. 1.83 x 10^-19 J E. 5.46 x 10^-19J |
C. 3.64 x 10^-19 J
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Give the number of core electrons for Cd. A. 46 B. 47 C. 44 D. 48 E. 45 |
A. 46
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(Interesting) Calculate the wavelength of a baseball (m= 155 g) moving at 1950 meters per minute.
A. 2.15 x 10^-32 m B. 3.57 x 10^-32 m C. HAHAHA!!! Funny!! Baseballs don't have wavelengths!! Nice try. D. 2.68 x 10^-34 m E. 1.32 x 10^-34 m |
E. 1.32 x 10^-34 m
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Place the following in order of increasing radius. Br- Na+ Rb+ A. Rb+ < Na+ < Br- B. Na+ < Rb+ < Br- C. Br- < Na+ < Rb+ D. Rb+ < Br- < Na+ E. Br- < Rb+ < Na+ |
Na+ < Rb+ < Br- |
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How many of the following elements have 2 unpaired electrons in the ground state?
C Te Hf Si A. 2 B. 1 C. 3 D. 4 |
D. 4
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Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The energy of one photo of this light is _____J. Avogadro's number is 6.022 x 10^23.
A. 3.79 x 10^-19 B. 2.64 x 10^18 C. 3.79 x 10^-28 D. 1.04 x 10^-22 E. 1.04 x 10^-31 |
A. 3.79 x 10^-19
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How many electrons are in the outermost shell of the Ga 3+ ion in its ground state?
A. 18 B. 6 C. 3 D. 2 |
A. 18
OR D. 2 |
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Complete this phrase as used in this class; "Stay happy............................................................"
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You have incredible value.
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Which of the following quantum numbers describes the orientation of an orbital?
A. principal quantum number B. magnetic quantum number C. Schrodinger quantum number D. angular quantum number E. spin quantum number |
B. magnetic quantum number
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Place the following types of electromagnetic radiation in order of increasing frequency.
x-ray microwaves gamma rays A. microwaves < gamma rays < x-rays B. gamma rays < microwaves < x-rays C. x-rays < gamma rays < microwaves D. gamma rays < x-rays < microwaves E. microwaves < x-rays < gamma rays |
E. microwaves < x-rays < gamma rays
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Identify the color that was a wavelength of 540 nm.
A. green B. red C. yellow D. blue |
A. green
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Choose the ground state electron configuration for Hf2+. A. [Xe] B. [Xe] 6s25d4 C. [Xe]6s2 D. [Xe]5d2 E. [Xe] 6s25d2 |
E. [Xe] 6s25d2 |
