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Form Code A NAME_________________________________________

 

Exam 3 Review (Sumner, Gower, Korolev, Angerhofer, Polanco)

 

Instructions: On your Scantron form, enter and bubble your name, UFID, and Form Code (see above). Turn in only your Scantron. You may keep your exam sheet and any other papers. Check bubbling carefully: bubbling errors are non-negotiable. As on all graded events, the loving of moles applies.

 

  1. Select the false statement below

 

      1. According to the Bohr Model, an atomic spectrum is not continuous because the atom’s energy is not continuous but rather exists in certain states.
      2. According to the Schrödinger equation, each of the equation’s solutions gives an energy state associated with a given atomic orbital. (3) The wavelength of a particle decreases as the particle’s energy increases.
      3. The Bohr Model is only effective for explaining hydrogen
      4. According to physicists, light exists in waves while matter exists in particles.

 

 

  1. Which element in each set would you expect to have the highest second ionization energy?

 

(I) Na, Mg, Al (II) Rb, K, Fe (III) Sc, Be, Mg

 

(1) Na, Rb, Be (2) Na, Fe, Mg (3) Al, Fe, Sc (4) Na, K, Be (5) Mg, K, Be

 

 

  1. Find the wavelength in nm of the photon absorbed when a hydrogen atom undergoes a transition from n = 1 to n = 3.

 

(1) 1.93*10-9 nm (2) 200 nm (3) 103 nm (4) 193 nm (5) 0.111 nm

 

 

  1. Arrange the following bond sets in order of increasing bond length.

 

H—Cl H—F H—Br H—I

 

      1. H—F< H—Cl < H—I < H—Br
      2. H—I < H—Br < H—Cl < H—F
      3. H—F < H—Cl < H—Br < H—I
      4. H—Cl < H—I < H—F < H—Br
      5. Since F, Cl, Br, and I are all in the same period and they are all connected to H, they have the same bond length

 

 

 

  1. Which of the Lewis Structures possess resonance?

 

I. NO3 II. SO42 − III. COCl2 IV. NH3

 

(1) I, II, and IV (2) I, II, and III

      1. I and II only
      2. III and IV only
      3. None of the Above

 

 

  1. Rank the following ions and atoms in increasing radii

 

Li, P3-, O, K+, Cl

 

(1) O < Li < K+ < Cl < P3- (2) O < Cl < P3- < Li < K+

      1. O < Li < Cl < P3- < K+
      2. Li < O < K+ < Cl < P3- (5) Li < K+ < O < Cl< P3-

 

 

  1. Why does Ca2+ naturally exist but Ca3+ does not?

 

      1. Ca is a Group II metal so its electronegativity is low
      2. Ca2+ has a higher electron affinity than the hypothetical Ca3+
      3. Ca3+ has too small of a radius so the core electrons would spin into the nucleus
      4. Ca is diamagnetic so it is unstable if it becomes paramagnetic
      5. The third ionization energy of Ca is too high

 

 

  1. How many valence and outer electrons do the following atoms have?

Cr, Na, Fe, and F

 

      1. Cr: 2 outer, 6 valence Na: 1 outer, 1 valence Fe: 2 outer, 8 valence F: 7 outer, 7 valence

 

      1. Cr: 6 outer, 24 valence Na: 1 outer, 11 valence Fe: 8 outer, 26 valence F: 7 outer, 9 valence

 

      1. Cr: 1 outer, 6 valence Na: 1 outer, 1 valence Fe: 2 outer, 8 valence F: 7 outer, 7 valence

 

      1. Cr: 2 outer, 6 valence Na: 1 outer, 1 valence Fe: 2 outer, 8 valence F: 2 outer, 7 valence

 

      1. Cr: 1 outer, 6 valence Na: 1 outer, 1 valence Fe: 2 outer, 8 valence F: 2 outer, 5 valence
  1. An analytical chemist reacts a metal and a nonmetal together. The metal has the valence configuration of ns2 and the nonmetal has a valence configuration of ns2np4. What is the potential format of the compound formula?

 

(1) MX3 (2) MX (3) MX2 (4) MX4 (5) M3X2

 

 

  1. Calculate the lattice enthalpy for lithium fluoride, given the following information:

 

Enthalpy of sublimation for solid lithium = 161 kJ/mol

 

First ionization energy for lithium = 520 kJ/mol

 

F-F bond dissocation energy = 154 kJ/mol

 

Enthalpy of formation for F(g) = 77 kJ/mol

 

Electron affinity for fluorine = -328 kJ/mol

 

Enthalpy of formation for solid lithium fluoride = -617 kJ/mol

 

(1) -1047 kJ/mol (2) 1047 kJ/mol (3) -823.5 kJ/mol (4) -523.5 kJ/mol

 

(5) 1980 kJ/mol

 

 

  1. Which of the following compounds is the most basic and acidic?

 

N2O5, MgO, SiO2, P4O10, Al2O3

 

        1. Basic: N2O5 Acidic: MgO
        2. Basic MgO Acidic: N2O5
        3. Basic: P4O10 Acidic: Al2O3
        4. Basic: MgO Acidic: N2O5
        5. Basic: SiO2 Acidic: P4O10

 

 

  1. Which of the molecules is not necessarily polar

 

        1. CO2
        2. XeBr2F2
        3. CH2Cl2
        4. H2O
        5. All molecules are either polar or nonpolar. They cannot be both.

 

  1. Which choice contains a possible set of quantum numbers (n, l, ml, ms) for the first electron removed from a ground state vanadium atom?

 

      1. 4, 0, 0, +½
      2. 4, 1, 0, –½
      3. 3, 2, 0, +½
      4. 3, 1, 1, +½
      5. 4, 2, 2, –½

 

 

  1. Which of the following is not isoelectronic with the others ?

 

(1) Ca2+ (2) Sc3+ (3) S2− (4) Ar (5) Zn2+

 

 

  1. Predict which of the following covalent bonds is the most polar.

 

(1) P—O (2) S—Cl (3) C—H (4) N—S (5) O—F

 

 

  1. In which of the following is it necessary to use an expanded octet to represent a Lewis structure which has a zero formal charge of the central atom?

I. SO42− II. SeO2 III. CO32− IV. PO43− V. SO3

 

      1. I and II only
      2. III, IV, and V only
      3. I, II, IV, and V only
      4. IV and V only
      5. V only

 

 

  1. Name the Period 3 element with the following successive ionization energies (in kJ/mol):

IE1 IE2 IE3 IE4 IE5 IE6

1012 1903 2910 4956 6278 22,230

 

(1) Si (2) P (3) S (4) Cl (5) As

 

  1. Estimate the standard molar enthalpy of formation (ΔH°f) of ClNO, expressed as kJ per mol of ClNO formed, using any of the following average bond enthalpy data that may apply : Cl—Cl, 243 kJ/mol ; N—N, 160 kJ/mol ; N=N, 418 kJ/mol ; N≡N, 945 kJ/mol ; O—O, 204 kJ/mol ; O=O, 498 kJ/mol ; Cl—N, 200 kJ/mol ; N=O, 607 kJ/mol ; N—O, 201 kJ/mol.

 

      1. 879 kJ/mol
      2. 72 kJ/mol
      3. 36 kJ/mol
      4. −504 kJ/mol
      5. −252 kJ/mol

 

  1. Which of the following is true ?

 

      1. atomic size increases across a period because Zeff increases
      2. atomic size increases down a group because Zeff decreases
      3. atomic size decreases across a period because Zeff decreases
      4. atomic size decreases down a group because Zeff increases
      5. atomic size decreases across a period because Zeff increases

 

 

  1. Consider the following species with tetrahedral electron-pair geometries and select the species with the smallest predicted bond angle(s).

 

(1) PF3 (2) CH4 (3) SO42− (4) SiCl4 (5) OF2

 

 

  1. Which of the following is not properly listed in order of decreasing energy required to break the bond ?

 

      1. RbI > NaCl
      2. MgS > NaCl

word image 948

(5) N−F > N−O

 

 

  1. Which of the compounds have the highest lattice energy is the highest?

 

(1) MgO (2) CaCl2 (3) Na2O (4) CH3Cl (5) BeO

 

 

word image 2815

GOOD LUCK, SMILE ON THE EXAM, and remember to

love your moles: all 6.022*1023 of them!

-Teaching Center

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