Chapter 6 3 Which ionization process requires the most energy

15) Of the following, which element has the highest first ionization energy?

A) Ba

B) I

C) Rb

D) Po

16) Which ionization process requires the most energy?

A) Pt(g) → Pt+(g) + e–

B) Pt+(g) → Pt2+(g) + e–

C) Pt2+(g) → Pt3+(g) + e–

D) Pt3+(g) → Pt4+(g) + e–

17) Which of the following species will have the highest ionization energy?

A) Rb+

B) Kr

C) Br–

D) Se2-

18) Which ionization process requires the most energy?

A) Ar(g) → Ar+(g) + e–

B) Ar+(g) → Ar2+(g) + e–

C) Si(g) → Si+(g) + e–

D) Si+(g) → Si2+(g) + e–

19) Which of the following species will have the highest ionization energy?

A) Na+

B) Na2+

C) Na3+

D) Na4+

20) Which ionization process requires the most energy?

A) S(g) → S+(g) + e–

B) S+(g) → S2+(g) + e–

C) Cl(g) → Cl+(g) + e–

D) Cl+(g) → Cl2+(g) + e–

21) Which of the following represents the change in electronic configuration that is associated with the

first ionization energy of barium?

A) [Xe]6s16p1 → [Xe]6s1 + e–

B) [Xe]6s2 → [Xe]6s16p1

C) [Xe]6s2 → [Xe]6s1 + e–

D) [Xe]6s2 + e– → [Xe]6s26p1

22) Which element has the highest first electron affinity?

A) Fr

B) Ra

C) Po

D) Rn

23) Which element has the least favorable (least negative) electron affinity?

A) Cl

B) S

C) Mg

D) As

24) How many valence shell electrons does an atom of aluminum have?

A) 1

B) 2

C) 3

D) 13

25) How many valence shell electrons does an atom of Si have?

A) 1

B) 6

C) 4

D) 2

26) An element that has the valence electron configuration 2s22p2 belongs to which period and group?

A) period 2; group 2A

B) period 2; group 4A

C) period 3; group 2A

D) period 3; group 4A

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27) To reach a noble gas electron configuration how many electrons would tellerium have to adopt?

A) 1

B) 2

C) 7

D) 4

28) Which species does not have an octet of electrons for its outer core?

A) Si4-

B) As3-

C) Se2-

D) Mg+

29) An element M reacts with chlorine to form MCl2, with oxygen to form MO, and with nitrogen to form

M3N2. The most likely candidate for the element is

A) Na

B) Sr

C) B

D) Ge

30) How many electrons does barium lose and nitrogen need to form Ba3P2?

A) barium loses 2 and phosphorus gains 2

B) barium loses 2 and phosphorus gains 3

C) barium loses 3 and phosphorus gains 2

D) barium loses 3 and phosphorus gains 3

31) The octet rule is most likely to fail occasionally for which of the following elements?

A) C

B) Ca

C) Li

D) P

32) The electron configuration of an element, X, is [Ne]3s1. The formula of the most probable ionic

compound that this element will form with O is

A) X O

B) X2O3

C) X2O

D) X3O2

33) Which of the following ionic compounds would be expected to have the highest lattice energy?

A) RbF

B) RbCl

C) RbBr

D) RbI

34) Which of the following ionic compounds would be expected to have the highest lattice energy?

A) Li F

B) Na F

C) K F

D) Rb F

35) Which ionic compound would be expected to have the highest lattice energy?

A) Cs2O

B) BaO

C) Ga2 O3

D) CO2

36) Which of the following ionic compounds would be expected to have the highest lattice energy?

A) MgS

B) KBr

C) K2S

D) BeBr2

37) Which of the following ionic compounds would be expected to have the highest lattice energy?

A) CaBr2

B) NaBr

C) KBr

D) RbBr

38) Which ionic compound would be expected to have the highest lattice energy?

A) Li2Se

B) MgS

C) Al2O3

D) CO2

39) Which ionic compound would be expected to have the highest lattice energy?

A) AlH3

B) Al2S3

C) AlCl3

D) AlN

6.3 Short Answer Questions

1) Using shorthand notation, the ground-state electron configuration for Sr2 is predicted to be ________.

2) Using shorthand notation, the ground-state electron configuration for Co2+ is predicted to be ________.

3) Using shorthand notation, the ground-state electron configuration for Tl+ is predicted to be ________.

Answer: [Xe]6s24f145d10

Diff: 2 Var: 1

Topic: Section 6.1 Electron Configurations of Ions

Learning Obj: LO 6.1 Write ground-state electron configurations for main group and transition metal ions.

Global Obj: G4 Demonstrate the quantitative skills needed to succeed in chemistry.

4) Using shorthand notation, the ground-state electron configuration for F– is predicted to be ________.

5) Using shorthand notation, the ground-state electron configuration of the chromium ion in CrCl2 is

________.

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6) The tripositive ion with the electron configuration [Ar]3d6 is ________.

7) The neutral atom with the electron configuration [Ar}4s23d6 is ________.

8) The ion that has 28 protons and 26 electrons is ________.

9) The number of electrons in the ion Zn2+ is ________.

10) The number of electrons in the ion K+ is ________.

11) The ion Q2+ contains 36 electrons. The identity of element Q is ________.

12) Isoelectronic means having the same number of electrons. The dipositive ion that is isoelectronic with

Br– is ________.

13) The ionic radius of Cs+ is ________ than the atomic radius of Cs, and the ionic radius of I– is ________

than the atomic radius of I.

14) The element in period 4 with the smallest first ionization energy is ________.

15) The element in period 3 with the smallest seventh ionization energy is ________.

16) What is the third-row element having the successive ionization energies in kJ/mol: 738, 1451, 7733,

10,540, 13,630, 17,995, 21,703?

17) The element in group 7A with the least favorable (least negative) electron affinity is ________.

18) The third-row element having a less negative electron affinity than the elements on either side of it on

the periodic table is ________.

19) The group 4A element that always obeys the octet rule in its stable compounds is ________.

20) Lattice energy increases with ________ cation and anion charges and ________ cation and anion radii.