CHM 101Review for the Final Section of Exam 4

  1. Which element would be expected to have chemical and physical properties closest to fluorine?
  2. S b. Fec. Ned. Cl
  1. The 1s orbital is smallest in which atom?
  2. F b. Clc. Brd. I
  1. The atomic radius generally increases down a group because
  2. Effective nuclear charge increases down a group
  3. Effective nuclear charge decreases down a group
  4. The principal quantum number of the valence orbital increases
  5. Both the effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases.
  1. Which of the following gives the correct order for atomic radius?
  2. Mg > Na > P > Si > Ar
  3. Ar > Si > P > Na > Mg
  4. Si > P > Ar > Na > Mg
  5. Na > Mg > Si > P > Ar
  1. Of the following elements, which has the largest first ionization energy?
  2. Se b. Asc. Sd. Sb
  1. Which of the following correctly represents the second ionization energy of calcium?
  2. Ca(g)  Ca+(g) + e-
  3. Ca+(g)  Ca2+(g) + e-
  4. Ca(g)  Ca2+(g) + 2e-
  5. Ca+(g) + e- Ca(g)
  1. Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more reactive than magnesium and has a smaller radius than barium. Element M is
  2. Sr b. Kc. Nad. Be
  1. Oxides of metals combine with water to form
  2. Metal hydroxidesb. Metal hydrides

c. Hydrogen gasd. Water and a salt

  1. Which one of the following compounds produces an acidic solution when dissolved in water?
  2. CH4b. Na2Oc. CO2d. CCl4
  1. Based on the octet rule, iodine most likely forms an ion of what charge?
  2. -1 b. -2c. -3d. +1
  1. For which of the following atoms does the Lewis symbol have no unpaired electrons?

OFSeNNeC

  1. Ne b. C and Nec. C, O, and Ned. O, F, C, and Se
  1. Which of the following species has the electron configuration [Ar]3d4?
  2. Mn2+b. Cr2+c. V3+d. Fe3+
  1. In which series are the ionic compounds arranged in order of increasing ionic bond strength?
  2. MgO < CaO < SrO
  3. LiCl < NaCl < NaF
  4. RbCl < SrCl2 < MgCl2
  5. CaO < SrO < ScN
  1. In which of the following is the carbon-carbon bond length the shortest?
  2. H2C=CH2b. H-CC-Hc. H2C=C=CH2d. H3C-CH2-CH3
  1. How many pairs of electrons are shared in a double bond?
  2. 1 b. 2c. 3d. 4
  1. Which of the following covalent bonds is most polar?
  2. C-Hb. N-Hc. O-Hd. O-C
  1. Which of the following molecules has the most polar bond?
  2. HBrb. HIc. HCld. HF
  1. Using the table of bond dissociation energies, calculate H for the following reaction:

H-CC-H + H-I  H2C=CHI

Bond: / CC / C=C / H-I / C-I / C-H
BDE (kJ/mol) / 839 / 614 / 299 / 240 / 413
  1. +506b. -931c. -506d. –129

For questions 19 - 22 consider the Lewis structures of the following:

H2OBF3CH4CO2NO3-

iiiiiiivv

  1. Which have lone pairs?
  2. i, iv, and vb. ii, iv, and vc. iiid. i, ii, iv, and v
  3. Which have multiple bonds?
  4. ii, ivb. iii, iv, and vc. iv and vd. iii
  5. Which have atoms (other than H) that do not obey the octet rule?
  6. ii b. ii and vc. iv and vd. ii, iv, and v
  7. Which exhibit resonance?
  8. v b. iic. iv and vd. ii, iv, and v
  1. What is the electron domain geometry of SO3?
  2. Triganol planarb. tetrahedralc. triganol bipyramidal d. octahedral

24. What is the molecular geometry of XeF2?

  1. Triganol planarb. tetrahedralc. linear d. octahedral

25.What is the molecular geometry of selenium tetrafluoride?

a. seesawb. tetrahedralc. triganol bipyramidal d. octahedral