CHM 2041 Exam 2

Which of the following elements has the most positive electron affinity? A) C B) Ar C) Cr D) Zn E) Cl

B) Ar

The ion with the configuration 1s2 2s2 2p6 and charge -1 is A) Ne B) F- C) O2- D) Cl- E) Ne-

B) F-

Which of the following lists the atoms in order of increasing ionization energy (smallest to largest)? A) N < P < Si < Al B) Si < P < N < F C) Be < Li < Mg < Na D) I < Te < Sb < Sn

B) Si < P < N < F

Arrange these elements based on their increasing ionization energy: Cl, Br, Ca, Sr A) Ca < Cl < Br < Sr B) Sr < Ca < Br < Cl C) Cl < Br < Ca < Sr D) Ca < Cl < Sr < Br E) Br < Cl < Sr < Ca

B) Sr < Ca < Br < Cl

Give the number of core electrons for Cl A) 12 B) 16 C) 2 D) 10 E) 8

D) 10

Which of the following statements is/are true? A) The periodic table is divisible into four blocks corresponding to the fillings of the four quantum sublevels (s, p, d, and f). B) The group number of a main-group element is equal to the number of valence electrons for that element. C) The row number of a main-group element is equal to the highest principal quantum number of that element. D) All of the above are true. E) None of the above is true.

D) All of the above are true.

Give the ground state electron configuration for Pb. A) [Xe] 6s2 6p6 B) [Xe] 6s2 5d10 6p2 C) [Xe] 6s2 5f14 6d10 6p2 D) [Xe] 6s2 4f14 5d10 6p2 E) [Xe] 6s2 4f14 5d10 6s2 6p2

D) [Xe] 6s2 4f14 5d10 6p2

Which of the following orbitals can hold two electrons? A) 2pz B) 3s C) 4dxy D) all of the above E) none of the above

D) all of the above

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to complete the electron configuration of the Ne atom. A) n = 3, l = 1, ml = 1, ms = + ½ B) n = 2, l = 0, ml = 1, ms = - ½ C) n = 2, l = 2, ml = 1, ms = + ½ D) n = 2, l = 1, ml = 1, ms = - ½ E) n = 3, l = 2, ml = 1, ms = - ½

D) n = 2, l = 1, ml = 1, ms = - ½

Which of the following statements is false? A) The sublevels of each principal level are not degenerate for multielectron atoms. B) In a hydrogen atom, the sublevels of each principal level are degenerate. C) Due to shielding, the 3d orbitals lie lower in energy than the 4s orbital. D)Some atoms have anomalies in their electron configurations due to the fact that energy separations of the orbitals become smaller as the principal quantum number increases.

Due to shielding, the 3d orbitals lie lower in energy than the 4s orbital.

Which of the following is true? A) Be is smaller than Mg due mainly to differences in Zeff. B) Na is larger than Mg due mainly to differences in the principal quantum number. C) C is smaller than F due to an increase in the outermost energy levels of electrons. D) P is larger than N due primarily to stronger attractions between electrons in the outermost orbitals. E) Ca is larger than Mg due to larger orbitals.

E) Ca is larger than Mg due to larger orbitals.

Which of the following has the largest second ionization energy? A) P B) Si C) Al D) Mg E) Na

E) Na

Which one of the following atoms or ions is diamagnetic? A) O- B) Cl C) Mo2+ D) Cu E) Sn2+

E) Sn2+

Which of the following is false? A) No two electrons in an atom can have the same four quantum numbers. B) Electron spin is a fundamental property of electrons. C) All electrons have the same amount of spin. D) The orientation of an electron's spin is quantized. E) The possible values of spin are +1 and -1.

E) The possible values of spin are +1 and -1.

Consider the following electron configurations to answer the question. (i) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 (ii) 1s2 2s2 2p6 3s2 3p5 (iii) 1s2 2s2 2p6 3s2 3p6 4s2 3d8 (iv) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 (v) 1s2 2s2 2p4 3s1 Which ground state electron configuration has the smallest number of valence electrons?

(i)

Consider the following electron configurations to answer the question. (i) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 (ii) 1s2 2s2 2p6 3s2 3p5 (iii) 1s2 2s2 2p6 3s2 3p6 4s2 3d8 (iv) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 (v) 1s2 2s2 2p4 3s1 Which represents the ground state electron configuration for a halogen?

(ii)

Consider the following electron configurations to answer the question. (i) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 (ii) 1s2 2s2 2p6 3s2 3p5 (iii) 1s2 2s2 2p6 3s2 3p6 4s2 3d8 (iv) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 (v) 1s2 2s2 2p4 3s1 An example of a configuration of a transition metal is ________.

(iii)

Consider the following electron configurations to answer the question. (i) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 (ii) 1s2 2s2 2p6 3s2 3p5 (iii) 1s2 2s2 2p6 3s2 3p6 4s2 3d8 (iv) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 (v) 1s2 2s2 2p4 3s1 An example of an excited state is ________.

(v)

Arrange these elements based on their increasing atomic radii: Br, Ca, Ge, F A) F < Br < Ge < Ca B) Ca < Ge < Br < F C) Ge < Ca < F < Br D) Br < F < Ca < Ge E) F < Br < Ca < Ge

A) F < Br < Ge < Ca

Which of the following are false? I) K+ < K II) K < K+ III) Cl < Cl- IV) Cl- < Cl V) S2- < S A) II, IV, V B) I, II C) III, IV D) I, III E) I, III, V

A) II, IV, V

Which reaction below represents the electron affinity of Li? A) Li(g) + e- -> Li-(g) B) Li(g) -> Li+(g) + e- C) Li(g) + e- -> Li+(g) D) Li+(g) -> Li(g) + e- E) Li+(g) + e- -> Li(g)

A) Li(g) + e- -> Li-(g)

Which of the following atoms or ions is the largest? A) O2- B) F- C) Ne D) Na+ E) Mg2+

A) O2-

The number of valence electrons for Ga is A) 18 B) 1 C) 3 D) 5 E) 31

C) 3

Which atoms are listed in order of increasing size (smallest to largest)? A) C < N < O < F B) N < O < P < Si C) Mg < Ca < K < Rb D) Cl < S < O < F

C) Mg < Ca < K < Rb