. What is the energy of one mole of light that has a wavelength of 400 nm?(a) 4.97 x 10-28 J(b) 4.97 x 10-19 J(c) 2.99 x 10-4 J(d) 2.99 x 105 J

2. Helium can be singly ionized by losing one electron to become the He+ cation. Which of the following statements is true concerning this helium cation?

(a)The line spectrum of this helium cation will resemble the line spectrum of a hydrogen atom.

(b)The line spectrum of this helium cation will resemble the line spectrum of a lithium cation.

(c) The line spectrum of this helium cation will remain the same as for unionized helium.

(d)The line spectrum of this helium cation will resemble the line spectrum of a lithium atom.

3. Which of the following atoms has the largest diameter?(a) F(b) Cl(c) Br(d) I

4. Which of the following ions has the smallest diameter?(a) O2-

(b) Na+

(c) F-

(d) Al3+

5. Which of the following elements has the greatest electronegativity?(a) Si(b) P(c) N(d) O

6. Which element would have the greater difference between the first ionization energy and the second ionization energy?

(a) potassium(b) calcium

(c)Both should have the same differences because they are in the same period of the periodic table.

7. Which element would have the higher electron affinity?(a) chlorine(b) bromine

(c)Both should have the same electron affinity because they are in the same group of the periodic table and both will gain only 1 electron.

1. What is the hybridization of the oxygen atom in water?

(a) sp(b) sp2

(c) sp3

(d) It is not hybridized.2. When a double bond is formed between two atoms, one of the bonds is a sigma bond and the other is a pi bond. The pi bond is created by the overlap of...

(a) sp2 hybrid orbitals(b) sp3 hybrid orbitals(c) p orbitals(d) s orbitals

3. The central atom in BrF5 has _?_ bonding pairs of electrons and _?_ non-bonding pairs of electrons.

(a) 1...5(b) 0...5(c) 5...1(d) 5...0

4. Which of the following molecules does not have a net dipole moment?(a) H2O(b) NH3

(c) BF3

(d) BrF5

5. What is the bond order in NO2+?

(a) 1.5(b) 2(c) 3(d) 4

6. What is the electron-pair geometry of the central oxygen atom of ozone (O3)?(a) linear(b) trigonal planar(c) tetrahedral(d) trigonal bipyramidal

7. What is the molecular geometry for ammonia (NH3)?(a) saw horse(b) trigonal planar(c) tetrahedral(d) pyramidal

8. The molecular orbital diagram for the carbide ion (C22-) would show which of the

following molecular orbitals?

(a) s2

s2s

2s

2p4

(b) s2

s2s

2s

2p4    p

2

(c) s2

s2s

2s

2p4    p

2    p

2

(d) s2

s2s

2s

2p4    p

2    p

4

9. Which of the following best represents the 3-dimensional view of H2N-?

10. Which of the following represents the best resonance structure for N2O?

11. What is the hybridization of the sulfur atom is SF4?(a) sp2

(b) sp3

(c) sp3d(d) sp3d2

12. What is the hybridization of the xenon atom in XeF4?(a) sp2

(b) sp3

(c) sp3d(d) sp3d2

1. Which of the following is the correct electron-dot formula for water?

2. Which of the following is the correct electron-dot formula for carbon dioxide?

3. Which of the following represents the correct formula for aluminum oxide?(a) AlO(b) Al2O3

(c) AlO2

(d) Al2O4. Which of the bonds, shown by the dash, has the greatest polarity?

(a) H-Cl(b) H-NH2

(c) H-OH(d) H-SH

5. What is the major attraction between water molecules in the solid physical state?(a) dipole-dipole interactions(b) electrostatic interactions between charged atoms(c) hydrogen-bonds(d) physical entanglement of the molecules

6. Which of the following is the correct name for NaHCO3?(a) sodium hydrogen carbonate(b) sodium acetate(c) nitrogen hydrogen carbonate(d) sodium hydrogen carbon trioxide

7. What is the formal charge of the oxygen atom of the following compound?

(a) +3(b) +1(c) -2(d) -3

8. The molecule N2 is isoelectronic with...(a) O2

(b) F2

(c) NO(d) CN-

9. In which of the following compounds does ionic bonding predominate?(a) NH4Cl(b) CO2

(c) CH4

(d) LiBr10. Which of the following molecules contains only one non-bonding pair of valence electrons?

(a) NH4+

(b) HCN(c) C2H4

(d) N2

11. The following electron-dot formulas for carbon dioxide both satisfy the octet rule for all of the atoms. Which of these structures is the better structure and why is this the case?

(a) "A" is the better structure because there is no formal charge on any of the atoms.

(b)"A" is the better structure because all the bonds and non-bonding electron pairs are arranged in a symmetrical pattern.

(c)"B" is the better structure because there are opposite formal charges on the two oxygen atoms which attract each other and give the molecule a lower energy.

(d)"B" is the better structure because the bond energies of a single bond and a triple bond are higher than the bond energies of two double bonds.

12. Which of the following gases would be most soluble in water?(a) N2

(b) NH3

(c) CH4

(d) CO2

13. Which of the following compounds should have the highest boiling point?(a) NH3

(b) CH4

(c) H2O(d) HF

1. The probability area that best represents the shape of one of the atomic 3d orbitals is...

2. The common isotopes of carbon are 12C and 13C. The average mass of carbon is 12.01115 amu. What is the abundance of the 13C isotope?

(a) 1.115%(b) 98.885%(c) 0.480%(d) 99.52%

3. If the abundance of 6Li (6.015121 amu) is 7.500% and the abundance of 7Li (7.016003 amu) is 92.500%, what is the average atomic mass?

(a) 6.0750 amu(b) 6.0902 amu(c) 6.9250 amu(d) 6.9409 amu

4. What do the following have in common?

20Ne     19F-     24Mg2+

(a) They are isotopes of each other.(b) They are isomers of each other.(c) They are isoelectronic with each other.(d) They are different elements so they have nothing in common.

5. How many valence electrons does an oxygen atom have?(a) 2(b) 6(c) 8(d) 16

6. Fluorine atoms tend to...?...when they form chemical compounds with metals.(a) lose electrons(b) gain electrons(c) neither lose nor gain electrons...they usually share electrons equally with metals.(d) Fluorine atoms do not form compounds with other atoms...fluorine is an inert gas.

7. The identity of an element is determined by...(a) the number of its protons.(b) the number of its neutrons.(c) the number of its electrons.(d) its atomic mass.

8. The probability area that best represents the shape of an atomic 3p orbital is...

9. Which of the following electron configurations represents the electron configuration for a magnesium cation...Mg2+?

(a) 1s22s22p63s2

(b) 1s22s22p63s23p2

(c) 1s22s22p6

(d) 1s22s22p4

10. Which of the following orbital box diagrams represents silicon, which has 14 electrons?

11. The half-life of francium-212 is 19 minutes. How many minutes will it take for 1 gram of this isotope to decay to 0.125 grams?

(a) 4.75 minutes(b) 9.5 minutes(c) 38 minutes(d) 57 minutes

12. The atom formed by the beta decay of carbon-14 is...(a) oxygen-18(b) beryllium-10(c) boron-14(d) nitrogen-14

1. The pressure of a gas will     ?        when the volume is decreased and will     ?        when the absolute temperature is decreased.

(a) increase...increase(b) increase...decrease(c) decrease...increase(d) decrease...decrease

2. If the absolute temperature of a gas is doubled and the pressure of the gas is halved, how will the volume change?

(a) It will increase by two times its original value.(b) It will decrease to one fourth of its original value.(c) It will stay the same as its original value.(d) It will increase by four times its original value.

3. If both the volume and the pressure of a gas are doubled, how will the absolute temperature change?

(a) It will increase by two times its original value.(b) It will decrease to one fourth of its original value.(c) It will stay the same as its original value.(d) It will increase by four times its original value.

4. If 88.0 grams of solid carbon dioxide evaporates, how many liters of CO2 gas will be formed at a temperature of 300 K and 2.00 atmospheres of pressure? The ideal gas law

constant "R" is...

(a) 98.5 liters(b) 2170 liters(c) 24.6 liters(d) 1080 liters

5. The solubility of a gas will _?_ when a solution containing the gas is heated and the solubility of a gas in a solution will _?_ when the pressure over the solution is decreased.

(a) decrease...decrease(b) decrease...increase(c) increase...decrease(d) increase...increase

6. What is the total pressure, in atmospheres, of a 10.0 L container that contains 10 moles of nitrogen gas and 10 moles of oxygen gas at 300 K?

(a) 24.6 L(b) 49.3 L(c) 2,460 L(d) 4,930 L

1. How many moles of CO2 are present in 220 mg?(a) 5 moles(b) 0.005 mole(c) 5000 moles(d) 10 moles

2. What is the percent water in hydrated calcium chloride...CaCl2·2H2O?(a) 66.67%(b) 32.47%(c) 24.51%(d) 12.26%

3. What is the empirical formula for a compound that contains 17.34% hydrogen and 82.66% carbon?

(a) C5H(b) C2H5

(c) CH3

(d) CH2

4. What is the molecular formula for a compound that is 46.16% carbon, 5.16% hydrogen and 48.68% fluorine if the molar mass of this compound is 156.12 g?

(a) C3H4F2

(b) C5H10F5

(c) C6H8F4

(d) C6H6F3

5. If 2.68 g of hydrated sodium sulfate, Na2SO4·nH2O, on heating produces 1.26 g of water,

what is the empirical formula of this compound?(a) Na2SO4·H2O(b) 2Na2SO4·H2O(c) Na2SO4·7H2O(d) 9Na2SO4·8H2O

6. One mole of (NH4)2HPO4 contains _?_ moles of hydrogen atoms.(a) 1(b) 5(c) 6(d) 9