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180 Cards in this Set
- Front
- Back
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The molecule H2O2 has (bonding and lone pairs) |
3 bonding pairs and 4 lone pairs |
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What is the formal charge on the nitrogen in NO2Cl
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+1
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Which of the following species has the strongest carbon-carbon bond?
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CHCH
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As the bond order of a bond increases, the bond energy ____ and the bond length _____.
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Increases, decreases |
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Based upon electronegativity differences, which of the following bonds are labeled correctly with respect to indication a bond dipole? I. C----N II. Cl-----C III. N-----O |
III only
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What is the shape (molecular geometry) of PCl3?
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Trigonal pyramidal
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Based on the Lewis structure for SiF5- given below, what is the formal charge on the central silicon atom?
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-1
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What is the shape (molecular geometry) of XeO3?
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trigonal pyramidal
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Use Lewis structures to predict the bond order for a nitrogen- oxygen bond in nitrite ion, NO2-.
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3/2
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The liquid 1, 2-ethanedithiol is insoluble in water. If a 75.5 g sample of 1,2 ethane dithiol has a volume of 61.2 mL, what is the density, and would it float or sink if poured into a beaker containing water?
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1.23 g/mL and it would sink in water. |
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Bacteria, sugar molecules, and water droplets are matter at the:
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microscale, nanoscale, macroscale
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how many significant figures are there in the number 0.0306960?
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6
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How would the measurement, 5125 m, be rounded off to three significant digits and expressed in scientific notation?
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5.13x10^3 m
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The element name and symbol is correctly matched for which of the following?
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Fe - iron
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A general chemistry student found a chuck of metal in the basement of a friend's house. She measured the mass of the metal to be 383.6 g. Then she dropped the metal into a graduated cylinder containing 20 mL of water, and the water level rose to 43 mL. Of the following metals, which is the most likely:
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Platinum, d=21.46 g/mL
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How many days are equivalent to 27360 minutes?
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19 days
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Which of the following is an example of a chemical change?
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skin burning in the sun
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Sugar, coffee, and bismuth are
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a pure substance, a homogenous mixture, and an element
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how many significant figures are there in the number 0.097
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2
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An empty Erlenmeyer flask weighs 241.3 g. When filled with water (density = 0.997 g/mL), the flask and its contents weigh 489.1 g. What volume of water does the flask hold?
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249 mL
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What is the symbol for an ion of an element which has 12 protons and 10 electrons?
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Mg2+
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The symbol and atomic number of the lightest semi-metal in Group 4A are:
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Si and 14
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The formal perbromic acid is?
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HBrO4
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What is the name of the compound with the formula PI3?
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phosphorus triodide
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Which group of three elements contains a nonmetal, a metal, and a metalloid?
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F, K, Sb
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What is the name for the compound with the formula HF?
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hydrofluoric acid
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Which combination of protons, neutrons, and electrons correctly represents a neutral 56^Fe atom?
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26 protons, 30 neutrons, 26 electrons
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The element indium has two stable isotopes, indium-113 with an atomic mass of 112.9 amu and indium-115 with an atomic mass of 114.9 amu. From the atomic weight found on the periodic table for indium, one can conclude that:
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Indium- 115 has the highest percent natural abundance
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Determine the atomic mass of the element
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35.37 amu
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What is the formula for the compound copper (I) carbonate?
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Cu2CO3
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Which of the following is a molecular compound?
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H2SO4
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What is the correct systematic name for ICl5?
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iodine pentachoride
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The gold-foil experiment performed by Rutherford's lab _______.
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led to the discovery of the atomic nucleus |
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Which of the following is not one of the postulates of Dalton's Atomic Theory?
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During a chemical reaction, atoms are changed into atoms of different types
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Which list below are elements that exist as diatomic elements in nature?
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F2, N2, I2
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All of the following are in aqueous solution. Which is incorrectly named?
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HCN, cyanic acid
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Which of the following is an example of a chemical change?
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silver tarnishing
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Which is higher: 144 degrees F, or 63 degrees C? (degF = 9/5 (degC) +32)
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63.6 degC
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What is the correct formula for iron (III) sulfide?
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Fe2S3
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A quarter has a mass of 5.52 g. What is the mass of a quarter in milligrams? |
5.52x10^3 mg
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The diameter of a US Quarter is approximately 2.35 cm. What is the diameter of a quarter expressed in km and scientific notation?
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2.35x10^-5
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How many protons, neutrons, and electrons are in 1 atom of ^69 V31 Ga ^2+
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31 p, 38n, 29 e-
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What is the compound which forms between the ammonium ion and bromine?
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NH4Br
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How many protons and electrons does the most stable ion for calcium have?
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20 p, 18 e-
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A wavelength of red light is measured at 655 nm. What is the measurement in centimeters?
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6.55x10^-5
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When 51.8 and 67.5 are multiplied, the product has ___ significant figures, and when 51.8 and 67.5 are added, the sum has ___ significant figures.
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3, 4
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The main difference between a proton and a neutron is:
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a proton is charged, a neutron is not.
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Which of the following is not a physical property of water?
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Water can be broken down into hydrogen gas and oxygen gas
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What is the chemical formula for the compound magnesium phosphate?
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Mg3(PO4)2
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How many protons, neutrons and electrons are there in a neutral atom of the isotope of silver named silver-109
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47p, 62n, 47e-
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What is the name of the halogen that is in period 4?
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Bromine
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How many significant figures are there in the number 0.097
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2
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What is the mass of 25.0 mL of an oil if its density is 0.843 g/mL?
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21.1
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An empty Erlenmeyer flask weighs 230.5999999999 g. When filled with ethyl alcohol (density = 0.789 g/mL), the flask and it contents weigh 585.2 g. What volume of ethyl alcohol does the flask hold?
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449.4296577 mL
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What is the name of the compound with the formula Cr2S3?
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Chromium (III) sulfide
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A specially prepared sample of nitrogen contains 30% 14N (mass = 14.00 amu) and 70% 15 N (mass = 15.00 amu). What is the atomic mass of the nitrogen in this sample?
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14.7 amu
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What is the identity of alkaline earth element in the 6th period?
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Ba
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According to the following reaction, how many grams of hydrogen will be formed upon the complete reaction of 23.8 g of sodium with excess water? 2 Na+2H20-->2NaOH+H2 |
1.05 g
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How many grams of aluminum are present in 4.04 g of aluminum iodide, AlI3?
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0.267 g Al
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What is the mass in grams of 0.698999 mol of glucose, C6H12O6?
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126 g
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What mass of Al2S3 is formed when 5 g of Al is heated with 10 g of S? There are no other products.
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13.9 g
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How many tin atoms are there in 88.5 g sample of tin?
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4.49x10^23 atoms
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A mass of 6.849999 g N2H4 reacts with excess oxygen. If 14.6 g NO2 is collected, what is the percent yield of the reaction? N2H4+3O2-->2NO2+2H2O |
74.1%
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How many molecules of O2 would react with 56 C2H6 molecules according to the following balanced equation? 2C2H6+7O2-->4CO2+6H2O |
196
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If 49.6 g of O2 is mixed with 49.6 g of H2 and the mixture is ignited, what is the maximum mass of water that may be produced?
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55.79 g
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How many grams of silver will be formed when 27.9 g of copper reacts +with excess silver nitrate, according to the balanced equation below? 2AgNO3+Cu-->Cu(NO3)2+2Ag |
94.7 g
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How many moles of ammonia can be made by reacting 12 mol of N2 with 17 mol of H2?
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11
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What is the molar mass of ammonium sulfate, (NH4)2SO4?
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132 g/mol
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A compound is found to contain 46.59% phosphorus, 10.54% nitrogen, and 42.87% fluorine by weight. What is the empirical formula for this compound?
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P2NF3
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Butyric acid, found in rancid butter, has a molar mass of 88 g/mol. If butyric acid is 54.5% C, 9.09% H and 36.4% O, what is the molecular formula?
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C4H8O2
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When 50 mL of 1.2 M of HCl is combined with 50 mL of 1.3 M of NaOH in a coffee-cup calorimeter, the temperature of the solution increases by 8.01 degrees C. What is the change in enthalpy for this balanced reaction? HCl+NaOH-->NaCl+H2O Assume that the solution density is 1.00 g/mL, the specific heat capacity of the solution is 4.18 J/g x degrees C, and the volumes are additive. |
-55.79 kJ
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Exactly 105.2 J will raise the temperature of 10 g of a metal from 25 degrees C to 60 degrees C. What is the specific heat capacity of metal? |
0.30057 J/g x degrees C |
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A 42.89 g sample of cobalt (c=0.4209) initially at 157.19 degrees C, is placed in an insulated vessel containing 120.9 g of water (c=4.180), initially at 19.19 degrees C. Once equilibrium is reached, what is the final temperature of the metal-water mixture? Neglect the heat capacity of the vessel. |
24 degrees C |
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The first law of thermodynamics states that |
energy is neither created nor destroyed during a physical or chemical process, but is changed transformed from one form to another |
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Calculate the kinetic energy, in joules, of a 1200 kg automobile moving at 18 m/s. |
1.944x10^5 J |
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How many joules are there in 9.52 kcal? (1 calorie = 4.184 J) |
3.98 x 10^4J |
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Given the thermochemical equation 4AlCl3+3O2-->2Al2O3+6Cl2; H change=-529 kJ find H change for the following reaction (1/3) Al2O3+Cl2-->(2/3) AlCl3+(1/2) O2 |
88.2Kj |
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Given the following reactions N2+O2-->2H change H=180.7 kJ 2N2O-->O2+2N2 change H=-162.3 kJ the enthalpy for the reaction for 2NO2 --> 2NO+N2 is _____ kJ. |
17.5 kJ |
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How much heat is gained by copper when 51.79 g of copper is warmed from 15.5 degrees C to 76.40 degrees C? The specific heat of copper is 0.385 J/g x degrees C. |
1.21 x 10^3 J |
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Which one of the following statements is false? |
The actual numerical value of E can be measured. |
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A chemical reaction that absorbs heat from the surrounding is said to be _____ and has a _____ H change at constant pressure. |
endothermic, positive |
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The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.2 J/mol K. The conversion of 50 of ice at 0.00 degrees C to liquid water at 22 degrees C requires ____ kJ of heat. |
21.3 kJ |
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What is the change in internal energy of the system if 10 kJ of heat energy is absorbed by the system and 70 kJ of work is done by the system for a certain process? |
-60 kJ |
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For the reaction: 3H2+N2-->2NH3 determine how the work is being with the correct sign. |
work is being done on the system and w will be positive |
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What quantum numbers provide information with respect to the spatial orientation of an atomic orbital? |
Magnetic quantum number, "ml" |
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A photon of light has a frequency of 3.26 x 10^15 hertz. What is the wavelength? The speed of light is 2.998 x 10^8 m/s. |
92 nm |
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n is known as the |
principal quantum number, and it specifies the size and energy of the shell in which the orbital resides |
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How many values are there for the magnetic quantum number when the value of the angular momentum quantum number is 4? |
9 |
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A local FM radio station broadcasts at a frequency of 99 MHz. Calculate the wavelength at which it is broadcasting. (1 MHz=10^6 Hz). |
3.03 m |
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How many electrons can be described by the quantum numbers n=4, =1? |
6 |
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How many orbitals are there in n=2 in an atom? |
4 |
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What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from level n=9 to level n=5? (c=2.998 x10^8 m/s, h=6.626x10^-34 Jxs, constant in the Bohr Equation = 2.179x10^-18 J) |
3.3x10^-6 m |
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Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. |
n=4, l=3, ml=-2 |
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When n=4, how many d orbitals are present? |
5 |
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What is the ground state electron configuration of the Al3+ ion? |
1s2 2s2 2p6 |
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How many orbitals are possible when l=0? |
1 |
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How many sublevels are contained in the second energy level (n=2) of a given atom? |
2 |
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Which of the following is the correct noble gas electron configuration for an ion of barium? |
[Kr] 5s2 4d10 5p6 |
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the electron configuration of antimony is |
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3 |
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Which of the following electron configurations is possible, according to Pauli exclusion principle? |
1s2 2s5 |
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A (pi) bond is the result of the |
sidewise overlap of two parallel p orbials |
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What is the hybridization of the sulfur atom in sulfur tetra fluoride, SF4? |
sp3d |
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What type of hybridization below would be most polar? |
sp3 |
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How many sigma and pi bonds does C have in HCN? |
2 sigma and 2 pi |
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Use VSEPR theory to predict the molecular geometry of IF5. |
square pyramidal |
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Which response includes all of the molecules listed that have the same molecular geometry as electronic geometry, and only those molecules? |
BCl3, AsF5 |
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When a carbon atom has sp3 hybridization, it has |
one pi bond, and three sigma bonds |
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If an atom has sp2 hybridization in a molecule, what is the maximum number of sigma and pi bond that the atom can form? |
3 sigma and 1 pi |
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How many valence electrons does an atom of tin (Sn) have? |
4 |
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Which nonmetal exists as a diatomic solid? |
Iodine |
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Place the following ions in order from smallest to largest ionic radii: Se2-, Sr2+, Y3+, and Br-. |
Y3+ |
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Place the following atoms in order of increasing atomic radii: K, Na, Be, and Li? |
Be |
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What is the ground state electron configuration of the sulfide ion? |
1s2 2s2 2p6 3s2 3p6 |
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Arrange the following atoms in order of increasing atomic radius: arsenic oxygen bromine |
oxygen |
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Of the following elements, which has been shown to form compounds? helium, neon, argon, kyrpton, xenon |
xenon, krypton, and argon |
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Name the elements described in each of the following: Smallest atomic radius in Group 6A |
O |
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Choose the species below which would be paramagnetic |
Cl |
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Element M reacts with oxygen to form an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. Element M could be _____. |
Ba |
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Alkali metals tend to be more reactive than alkaline earth metals because |
alkali metals have lower ionization energies |
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The electron affinity value expected for Br+e--->Br- the process would be |
a large negative number |
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What is the mass in grams of 0.6989 mol of glucose, C6H12)6? |
126 g |
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You need to make an aqueous solution of 0.125 M barium iodide for an experiment in lab, using a 300 mL volumetric flask. How much solid barium iodide should you add? |
14.7 g |
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Which of the following is correct net ionic equation for the reaction that occurs when aqueous barium hydroxide and hydrochloric acid are combined? |
H+ + OH- = H2O |
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Which response includes all of the following that are single displacement reactions, and no other reactions? I. P4O10+6Na2O=4Na3PO4 II. 2AgNO2 + Zn = 2Ag + Zn(NO3)2 III. Ca + 2HCl = CaCl2 + H2 IV.Fe (OH)2 +2HCl = FeCl2 + 2H2O |
II and III |
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Which of the following is the correct net ionic equation for the reaction that occurs when excess nitric acid and manganese (II) carbonate are combined? |
2H+ + MnCO3 = H2O + CO2 + Mn2+ |
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What volume of 0.378 M hydroiodic acid (HI) is required to neutralize 21.6 mL of 0.520 M barium hydroxide, Ba(OH)2? |
59.4 mL |
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How many sulfur atoms are present in 10 g of sulfur? |
1.88x10^23 |
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Which of the following would you predict to be insoluble in water? |
ZnS |
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A compound is found to contain 55.39% boron, 8.280% hydrogen, and 36.33% chlorine. What is the empirical formula for this compound? |
B5H8Cl |
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What mass of oxalic acid dihydrate, H2C2O4 x 2H2O, is required to prepare 250 mL of a 1.32 M solution of oxalic acid? |
41.6 g |
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Which list contains only strong acids? |
HCl, H0ClO3, HClO4, HI |
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How many grams of selenium are in 4.79 moles of selenium? |
378 g |
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Which one of the following substances is insoluble in water? |
FeS |
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The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.19 g of CCl4, carbon tetrachloride: 2CHCl3 + 2Cl2 = 2CCl4 + 2HCl What is the percent yield? |
66.5%
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You need to make a aqueous solution of 0.139 M aluminum nitrate, Al(NO3)3 for an experiment in the lab, suing a 300 mL volumetric flask. how much solid aluminum nitrate (Molar mass = 213.012 g/mol) should you add? |
8.88 g |
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The compound ammonium iodide is a strong electrolyte. Which of the following equations represents the transformation that occurs when ammonium iodide dissolves in water? |
NH4I(s) + NH4(aq) +I-(aq)
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What is the oxidation state of sulfur in sulfur dioxide, So2? |
+4 |
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The precipitate that form when aqueous solutions of barium chloride and potassium sulfate are mixed is: |
BaSO4 |
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Which of the following is an incorrect designation for an atomic orbital? |
1p |
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Choose the statement that is true: |
Core electrons effectively shield outer electrons from nuclear charge |
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What is the order filling the following atomic subshells? (lowest energy to highest energy) 4f, 5p, 5d, 6s |
5p<6s<4f<5d |
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the ground state valence shell configuration of a particular atom is 4s2 3d10 4p2. The element to which this atom belongs is a |
p-block main-group element |
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How many electrons can be described by the quantum number n=4, l=3? |
14 |
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1s2 2s2 2p6 3s2 3p6 4s2 3d3 is the correct electron configuration for which of the following atoms? |
V |
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How many unpaired electrons are present in the ground state of phosphorus atom? |
3 |
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Which of the following statements is true about the ionization energy of Mg+? |
It will be equal to and opposite in sign to the electron affinity of Mg2+. |
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Which atom listed below has the highest electron affinity? |
S |
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What 2- ion has the following ground state electron configuration? |
sulfide ion |
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Arrange the element Ba, Be, and Ca in order of increasing first ionization energy based upon their position on the periodic table. |
Ba |
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Which of the following corresponds to the noble gas electron configuration for iodine? |
[Kr] 5s2 4d10 5p5 |
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Which species has this ground state electron configuration: 1s2 2s2 2p6 3s2 3p6 3d10 |
Zn2+ |
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Which of the following chemical equation refers to the second ionization of Al? |
Al+(g) = Al2+(g) + e- |
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When 50 mL of 1.18 M of HCl is combined with 50 mL of 1.64 mL of 1.64 M of NaOH in a coffe-cup calorimeter, the temperature of the solution increases by 6.67 degrees C. What is the change in enthalpy for this balanced reaction? HCl + NaOH = NaCl + H2O |
-55.8 kJ |
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Exactly 132.6 J will raise the temperature of 10 g of a metal from 25 degrees C to 60 degrees C. What is the specific heat capacity of the metal? |
0.379 J/g degrees C |
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The change in internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is ____. |
-10,155 J |
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Which of the following elements would have the highest first ionization energy? |
Carbon |
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ml is known as the |
magnetic quantum number, and it specifies the orbital orientation |
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Given the following reactions: 2NO=N2+O2 H change=-180 kJ 2NO+O2=2NO2 H change_-112 kJ the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide N2+2O2=2NO2 is ______. |
68kJ |
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Which of the following is an exothermic process? |
condensation of water vapor |
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What is the wavelength of a photon that has an energy of J? ( c=2.998x10^8 m/s, h=6.626x10^-34 Jxs) |
788 nm |
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For the species in the reaction below, Hf change o is zero for _____. 2Co(s) + H2(g) + 8PF3(g) = 2HCo(PF3)4(l) |
both Co(s) and H2(g) |
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The value of Ho change for the reaction below is -482 kJ. Calculate the heat (kJ) releasedto the surroundings when 12 go of CO reacts completely. |
103 kJ |
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What is the molarity of NaI solution that contains 7.29 g of NaI in 28 mL of solution? |
1.7 M |
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On oxide of iron has the formula Fe3O4. What mass percent of iron does it contain? |
72% |
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Analysis of a compound containing only C and Br revealed that it contains 33.33% C atoms by number and has a molar mass of 515.46 g/mol. what is the molecular formula of this compound? |
C3Br6 |
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Assign oxidation number to each atom in calcium 0bromite, Ca(BrO2)2. |
Ca=+2; Br=+3; O=-2 |
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What is the net ionic equation for the reaction of NH3 with HClO4? |
NH3(aq) + H+(aq) = NH4(aq) |
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What is the reducing agent in the reaction below? Zn(s) + CuSO4(aq) = ZnSO(aq) + Cu(s) |
Zn |
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Which of the following compounds in soluble in water? |
Na3P |
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What mass of H3PO4 (98 g/mol) is present in 36.2 L of a 0.08269 M solution of H3PO4? |
2.93x10^2 |
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the balanced net ionic equation for the reaction of magnesium sulfite with nitric acid is |
MgSO3(s) + 2H+(aq) = Mg2+(aq) + SO2(g) + H2O(l) |
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Which of the following would you predict to be insoluble in water? |
ZnS |
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What mass of KOH is needed to prepare .5 L of .1 molar slution? |
2.8 g |
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What volume of 0.378 M hydroiodic acid (HI) is required to neutralize 21.6 mL of 0.520 M barium hydroxide, Ba(OH)2? |
59.4 mL |
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A 50 mL sample of .108 M H2SO4 is diluted to 250 mL. What is its new molarity? |
0.0216 M |
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A dilute solution is prepared by transferring 45 mL of a 0.56159 M stock solution to a 400 mL volumetric flask and diluting to mark. What is the molarity of this dilute solution? |
0.06318 M |
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What is the net ionic equation for the following formula unit equation? 2HClO3(aq) + Sr(OH)2(aq) = Sr(ClO3)2(aq) + 2H2O(l) |
2H+(aq) + 2OH-(aq) = 2H2O(l) |
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The oxidation number of nitrogen is highest in which of the following? |
NaNO3 |
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Identify the oxidizing and reducing agents in the redox reaction below 3Fe(s) + 8H+(aq) + 2NO3-(aq) = 3Fe2+(aq) + 2NO(g) + 4H2O |
reducing agent: Fe; oxidizing agent: NO3- |
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A 29 g sample of NaOH is dissolved in water, and the solution is diluted to give a final volume of 1.6 L. The molarity of the final solution is |
0.453 M |
