Chapter 8 Mastering Chemistry

11. How many unpaired electrons are present in the ground state As atom? A. 2 B. 4 C. 0 D. 1 E. 3

3

5. How many valence electrons does an atom of sulfur have? Hints A. 10 B. 16 C. 4 D. 6

6

22. How many valence electrons do the halogens possess? A. 7 B. 1 C. 6 D. 5 E. 2

7

1. In the periodic table we use today, the ordering of the elements is based on _____. Hints A. octaves (groups of eight) of elements, which resulted in every eighth element having similar properties B. atomic mass C. triads (groups of three) of elements with similar properties D. atomic number

atomic number

23. How many valence electrons do the alkali metals possess? A. 6 B. 7 C. 8 D. 1 E. 2

1

17. Give the number of core electrons for Cl-. A. 12 B. 17 C. 30 D. 10 E. 22

10

21. Give the electron configuration for O. A. 1s2 2s2 2p4 B. 1s2 2s1 2p1 C. 1s2 2s2 2p3 D. 1s2 2s2 2p5 E. 1s2 2p4

1s2 2s2 2p4

10. The complete electron configuration of gallium, element 31, is ________. A. 1s4 2s4 2p10 3s4 3p9 B. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p1 C. 1s2 2s2 2p10 3s2 3p10 4s2 3d3 D. 1s4 2s4 2p6 3s4 3p6 4s4 3d3 E. 1s4 2s4 2p8 3s4 3p8 4s3

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p1

15. Place the following in order of decreasing radius. Te2- F- O2- A. Te^2- > O^2- > F- B. F- > O^2- > Te^2- C. O2- > F- > Te^2- D. F- > Te^2- > O^2- E. Te^2- > F- > O^2-

A. Te^2- > O^2- > F-

16. Identify the species that has the smallest radius. A. cation B. anion C. neutral D. they are all the same size

Cation

19. Which of the following species will have the highest ionization energy? A. Cl- B. Ar C. K+ D. S^2-

K+

26. Arrange the following elements in order of decreasing first ionization energy: Po, Ar, Te, and Se. Rank elements from largest to smallest. To rank items as equivalent, overlap them.

Largest First Ionization Energy: Ar Next largest: Se Next: Te Smallest First Ionization Energy: Po

27. Arrange the following elements in order of decreasing metallic character: Rb, N, Si, P, Ga, and Al. Rank elements from most to least metallic character.

Most Metallic Character: Rb Next most metallic: Ga Next: Al Next: Si Then: P Least Metallic Character: N

14. Place the following in order of increasing radius. Br- Na+ Rb+ A. Br- < Na+ < Rb+ B. Rb+ < Br- < Na+ C. Na+ < Rb+ < Br- D. Br- < Rb+ < Na+ E. Rb+ < Na+ < Br-

Na+ < Rb+ < Br-

20. Which element has the highest first electron affinity? O Na Mg Ne

O

13. Part A Arrange the elements in decreasing order of first ionization energy. Rank from highest to lowest first ionization energy. To rank items as equivalent, overlap them. Arrange the elements in order of decreasing first ionization energy. Element Radius (pm) X 109 Y 184 Z 261 Rank from highest to lowest first ionization energy. To rank items as equivalent, overlap them.

Part A: Highest first ionization energy: Se Next highest: Ge Next: In Lowest first ionization energy: Cs Part B: Highest first ionization energy: element X Next Highest: element Y Lowest first ionization energy: element Z

18. Part A Rank the following elements in order of decreasing atomic radius. Rank from largest to smallest radius. To rank items as equivalent, overlap them. Part B Rank the following elements in order of decreasing atomic radius. Rank from largest to smallest radius. To rank items as equivalent, overlap them. Part C The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively? Hints A. +5 and +8 B. +3 and +6 C. +5 and +6 D. +3 and +8 E. +1 and +4

Part A: Largest Radius: Sn Next largest: Ge Next: Si Smallest Radius: C Part B: Largest Radius: Na Next largest: Mg Next: Al Smallest Radius: Si Part C: +3 and +6

7. Part A Complete an orbital diagram for boron. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Part B Complete an orbital diagram for scandium (Sc). Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Part C Electron configurations are a shorthand form of an orbital diagram, describing which orbitals are occupied for a given element. For example, 1s2 2s2 2p1 is the electron configuration of boron. Use this tool to generate the electron configuration of arsenic (As). https://drive.google.com/file/d/0B4_51_spvHBTV2piWjRoZDhwUk0/view?usp=sharing&resourcekey=0-MfjevlrJkVn0VVF4OmeDGw https://drive.google.com/file/d/0B4_51_spvHBTbFprT1hiYXd2QkE/view?usp=sharing&resourcekey=0-c7QvqkuOB3STg5plomji7w https://drive.google.com/file/d/0B4_51_spvHBTYVNDYjFpOWZKYWs/view?usp=sharing&resourcekey=0-QtXavdFQI_obNMFO5K0fCw

Part A: 1s2 2s2 2p1 Part B: 1s2 2s2 2p6 3s2 3p6 4s2 3d1 Part C: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3 (use links for answers)

24. Use the periodic table to determine each of the following: Part A The number of 3s electrons in Mg. Express your answer as an integer. Part B The number of 3d electrons in Cr. Express your answer as an integer. Part C The number of 4d electrons in Y. Express your answer as an integer. Part D The number of 6p electrons in Po. Express your answer as an integer.

Part A: 2 Part B: 5 Part C: 1 Part D: 4

4. 1s2 2s2 2p6 3s2 3p3 is the ground state electron configuration for what element? Hints A. Phosphorus, P B. Argon, Ar C. Nitrogen, N D. Arsenic, As

Phosphorus, P

12. Place the following elements in order of decreasing atomic radius. Xe Rb Ar A. Rb > Ar > Xe B. Ar > Xe > Rb C. Rb > Xe > Ar D. Xe > Rb > Ar E. Ar > Rb > Xe

Rb > Xe > Ar

25. Arrange the following isoelectronic series in order of increasing radius: Cl−, Sc^3+, S^2−, Ca^2+, and K+. Rank ions from smallest to largest. To rank items as equivalent, overlap them.

Smallest Radius: Sc^3+ Next smallest: Ca^2+ Next: K+ Next: Cl− Largest Radius: S^2−

6. Gold, Au, is found in which block of the periodic table? Hints A. The p-block B. The s-block C. The f-block D. The d-block

The d-block

8. Give the ground state electron configuration for Sr. A. [Kr]5s2 4d2 B. [Kr]5s2 4d10 5p2 C. [Kr]5s2 5d10 5p2 D. [Kr]5s2 4d10 E. [Kr]5s2

[Kr]5s2

9. Give the ground state electron configuration for I. A. [Kr]5s2 5p6 B. [Kr]5s2 4d10 5p6 C. [Kr]5s2 4d10 5p5 D. [Kr]4d10 5p6 E. [Kr]5s2 5d10 5p6

[Kr]5s2 4d10 5p5

3. An implication of Hund's rule is that _____. Hints A. if two electrons occupy the same orbital they must have opposite spin quantum numbers (m s). B. electrons will fill the lowest energy orbitals first before occupying higher energy orbitals C. electrons fill degenerate orbitals singly first, with parallel spins, before the electrons will pair up D. in multielectron atoms the 4s orbital is lower in energy than the 3d orbital.

electrons fill degenerate orbitals singly first, with parallel spins, before the electrons will pair up

2. An implication of the Pauli exclusion principle is that _____. Hints A. electrons will fill the lowest energy orbitals first before occupying higher energy orbitals B. electrons fill degenerate orbitals singly first, with parallel spins, before the electrons pair up C. if two electrons occupy the same orbital, they must have opposite spin quantum numbers (m s) D. in multielectron atoms, the 4s orbital is lower in energy than the 3d orbital

if two electrons occupy the same orbital, they must have opposite spin quantum numbers (m s)