Chem 261 Chapter 6 Practice Quiz

Which electronic configuration(s) listed below is(are) correct for the elements provided? a) Nitrogen 1s22s22p3 b) Tin [Kr]5s24d105p2 c) Bromine 1s22s22p63s23p63d104s24p7 1. a only 2. a and b 3. a and c 4. b and c 5. All of the above

2. a and b

Which of the following is an acceptable orbital diagram for the valence shell of a carbon (Z = 6) atom in its ground state? 1. 2s 2p 2. 2s 2p 3. 2s 2p 4.2s 2p 5. none of these

3. 2s 2p

The valence shell orbital configuration of the Si atom in its ground state is: 1.3s 3p 2.3s 3p 3.3s 3p 4.3s 3p 5. none of these

3. 3s 3p

A chemical property of Magnesium metal, Mg (s) is that it reacts with oxygen, O2 (g) to produce Magnesium oxide, MgO as shown below. How does each element in the compound MgO attain an octet of electrons? 2 Mg (s) + O2 (g) 2 MgO (s) a. A Magnesium atom loses two electrons and the oxygen atom accepts the two electrons. b. An Oxygen atom loses two electrons and the Magnesium atom accepts the two electrons. c. A Magnesium atom loses two electrons and the oxygen atom loses six electrons. d. A Magnesium atom gains six electrons and the oxygen atom loses six electrons. e. A Magnesium atom and an oxygen atom share two electrons.

a. A Magnesium atom loses two electrons and the oxygen atom accepts the two electrons.

Which atom has the highest electron affinity (i.e., most favorable to add an electron)? a. S b. P c. Se d. As e. Sb

a. S

With respect to electron affinity, arrange the following elements in order from least favorable to most favorable in terms of acquiring an additional electron. Barium, Fluorine, Sulfur a. (Least favorable) Barium < Fluorine < Sulfur (Most favorable) b. (Least favorable) Barium < Sulfur < Fluorine (Most favorable) c. (Least favorable) Fluorine < Barium < Sulfur (Most favorable) d. (Least favorable) Fluorine < Sulfur < Barium (Most favorable) e. (Least favorable) Sulfur < Barium < Fluorine (Most favorable)

b. (Least favorable) Barium < Sulfur < Fluorine (Most favorable)

Arrange the following species in order of increasing radii. N3-, F-, Ne, Na+1, Mg2+ a. (smallest) N3- < F- < Ne < Na+1 < Mg2+ (largest) b. (smallest) Mg2+ < Na+1 < Ne < F- < N3- (largest) c. (smallest) Ne < Mg2+ < N3- < Na+1 < F- (largest) d. (smallest) F- < Na+1 < N3- < Mg2+ < Ne (largest) e. (smallest) Na+1 < F- < N3- < Ne < Mg2+ (largest)

b. (smallest) Mg2+ < Na+1 < Ne < F- < N3- (largest)

Which of the following species is not isoelectronic with Na+? a. Mg2+ b. Li+ c. Ne d. F1- e. O2-

b. Li+

How many valence electrons are present in an atom of Arsenic? a. 2 b. 3 c. 5 d. 13 e. 33

c. 5

Which species is not isoelectronic with the remaining atoms or ions listed? a. Kr b. Rb+1 c. Na+1 d. Br-1 e. Se-2

c. Na+1

Taking into account the size of ions and their respective charges, arrange the following three ionic compounds MgCl2, NaCl and MgO in order of increasing lattice energy. a. MgCl2 < NaCl < MgO b. MgCl2 < MgO < NaCl c. NaCl < MgCl2 < MgO d. NaCl < MgO < MgCl2 e. MgO < MgCl2 < NaCl

c. NaCl < MgCl2 < MgO

The ground state electron configuration 1s22s22p63s23p2 would be correct for which species listed below? a. Al b. P c. P+ d. S e. none of these

c. P+

Which element has the valence electrons 4s23d2? a. Ca b. Sc c. Ti d. V e. none of these

c. Ti

The ground state electron configuration of Se is: a. [Ar]3s23d103p4 b. [Ar]4s24d104p4 c. [Ar]4s23d104p4 d. [Ar]4s23d104p5 e. none of these

c. [Ar]4s23d104p4

Arrange the following elements in order of increasing first ionization energy. Br, Cl, Se a. (Lowest IE) Br < Cl < Se (Highest IE) b. (Lowest IE) Br < Se < Cl (Highest IE) c. (Lowest IE) Se < Cl < Br (Highest IE) d. (Lowest IE) Se < Br < Cl (Highest IE) e. (Lowest IE) Cl < Br < Se (Highest IE)

d. (Lowest IE) Se < Br < Cl (Highest IE)

What is the correct electronic configuration for Arsenic (Z = 33) taking into account the proper order for filling subshells? a. 1s22s22p63s23p6 b. 1s22s22p63s23p63d104s24p3 c.1s22s22p63s23p63d104s24p64d104f145s25p65d6 d. 1s22s22p63s23p64s23d104p3 e. [Kr]4p3

d. 1s22s22p63s23p64s23d104p3

The ground state of which species below has the most unpaired electrons? a. P b. O c. Se d. Fe e. N

d. Fe

From the restrictions on the three quantum numbers that define an orbital, which set of three quantum numbers listed below is forbidden? a. n = 4, = 3, m = -2 b. n = 4, = 2, m = -2 c. n = 4, = 3, m = 3 d. n = 4, = 4, m = -2 e. n = 4, = 1, m = 1

d. n = 4, = 4, m = -2

Three sets of quantum numbers are listed below. Pick the best answer. (1) n = 2, = 2, m, = 2, ms = ½ (2) n = 4, = 0, m, = 0, ms = ½ (3) n = 3, = 2, m, = 3, ms = ½ a. 1 and 2 are allowed sets, 3 is not b. 2 and 3are allowed sets, 1 is not c. all three are allowed sets d. only 2 is an allowed set e. all 3 are not allowed sets

d. only 2 is an allowed set

The quantum number l for an electron in an atom is 2. This electron is definitely located in: a. the first principal shell b. the second principal shell c. an s subshell d. a p subshell e. a d subshel

e. a d subshell

Of the three species, which would be isoelectronic with O? (i) N+ (ii) F- (iii) Ne2- a. (i) and (ii) are isoelectronic, c is not isoelectronic with O b. only (i) is isoelectronic with O c. only (ii) is isoelectronic with O d. all are isoelectronic with O e. none are isoelectronic with O

e. none are isoelectronic with O

Which of the following series of atoms is arranged in order of decreasing size? a. K > Ga > In b. Cl > Br > Kr c. Li > Mg > Ca d. H > He > Li e. none of these

e. none of these