Back
- What is the ground-state electron configuration for the Mg2+ ion? (LO 6.1) (a) 1s22s22p6 (b) 1s22s22p63s2 (c) 1s22s22p63s23p2 (d) 1s22s22p63s23p6
Problem 1
- Give the ground state electron configuration and number of unpaired electrons in a Ru2+ ion. (LO 6.1, 6.2) (a) 3Kr45s2 4d4 0 unpaired electrons (b) 3Kr45s2 4d6 0 unpaired electrons (c) 3Kr44d6 4 unpaired electrons (d) 3Kr45s24d4 4 unpaired electrons
Problem 2
- Identify the false statement about atomic and ionic radii. (LO 6.3) (a) I- has a larger radius than Br- (b) Ba2+ has a smaller radius than Ba (c) Te has a larger radius than Te2- (d) Sr2+ has a smaller radius than Se2-
Problem 3
- Arrange the ions Rb+, Br-, and Sr2+ from the smallest to the largest. (LO 6.4) (a) Br- < Rb+ < Sr2+ (b) Sr2+ < Br- < Rb+ (c) Rb+ < Sr2+ < Br- (d) Sr2+ < Rb+ < Br-
Problem 4
- Which of the following processes requires the largest input of energy? (LO 6.5) (a) (b) (c) (d)
Problem 5
- The successive ionization energies for a second-period element are given. What is the identity of the element? (LO 6.8) Ea1 = 1402 kJ/mol Ea2 = 2856 kJ/mol Ea3 = 4578 kJ/mol Ea4 = 7475 kJ/mol Ea5 = 9445 kJ/mol Ea6 = 53,266 kJ/mol Ea7 = 64,630 kJ/mol (a) Be (b) C (c) N (d) F
Problem 7
- Which of the following processes will release the most energy? (LO 6.9) (a) (b) (c) (d)
Problem 8
- Elements that have large negative electron affinities generally have (LO 6.10) (a) high values for Zeff and a vacancy in a valence orbital. (b) low values for Zeff and a vacancy in a valence orbital. (c) high values for Zeff and filled valence orbitals. (d) low values for Zeff and filled valence orbitals.
Problem 9
Problem 11
Which molecular scale image best represents the ionic com-pound that forms between cesium and chlorine? (Cesium is represented by red circles, and chlorine is represented by blue circles.) (LO 6.12) (a)
(b)
(c)
(d)
- For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because (LO 5.16) (a) a 3p orbital has more nodal surfaces than a 3s orbital. (b) an electron in a 3p orbital has a higher probability of being closer to the nucleus than an electron in a 3s orbital. (c) inner electrons shield electrons in a 3p orbital more effec-tively than electrons in a 3s orbital. (d) the energy of the electron can be spread between three 3p orbitals instead of only one 3s orbital.
Problem 12
Problem 12a
Given the following information, construct a Born–Haber cycle to calculate the lattice energy of CaCl2(s). (LO 6.13)
Net energy change for the formation of CaCl2(s) form Ca(s) and Cl2(g) = -795.4 kJ/mol
Heat of sublimation for Ca(s) = +178 kJ/mol
Ei1 for Ca(s) = +590 kJ/mol
Ei2 for Ca(g) = +1145 kJ/mol
Bond dissociation energy for Cl2(g) = +243 kJ/mol
Eea1 for Cl(g) = -348.6 kJ/mol
(a) 2603 kJ/mol (b) 2254 kJ/mol (c) 2481 kJ/mo (d) 1663 kJ/mol
- Which element has the largest atomic radius? (LO 5.20) (a) Rb (b) Co (c) Mg d) As
Problem 15
Problem 31
Three binary compounds are represented on the following drawing: red with red, blue with blue, and green with green. Give a likely formula for each compound.
Problem 33
Given the following values for steps in the formation of CaO(s) from its elements, draw a Born–Haber cycle similar to that shown in Figure 6.7. Eea1 for O1g2 = -141 kJ/mol Eea2 for O1g2 = 745.1 kJ/mol Heat of sublimation for Ca1s2 = 178 kJ/mol Ei1 for Ca1g2 = 590 kJ/mol Ei1 for Ca1g2 = 1145 kJ/mol Bond dissociation energy for O21g2 = 498 kJ/mol Lattice energy for CaO1s2 = 3401 kJ/mol
Problem 36
What is the difference between a molecule and an ion?
Problem 37a,b,d
Label the following species as molecules or ions. (a) NO3– (b) NH4+ (d) CH3CO2–
Problem 37c
Label the following species as molecules or ions. (c) NO2
Problem 38a
How many protons and electrons are in each of the following ions? (a) Be2+
Problem 38b
How many protons and electrons are in each of the following ions? (b) Rb+
Problem 38c
How many protons and electrons are in each of the following ions? (c) Se2-
Problem 38d
How many protons and electrons are in each of the following ions? (d) Au3+
- What are the likely ground-state electron configurations of the following anions? (a) Se2- (b) N3-
Problem 41
- Identify the element whose 2+ ion has the ground-state electron configuration [Ar] 3d10.
Problem 43
- Which doubly positive ion has the ground-state electron configuration 1s2 2s2 2p6?
Problem 44
- What tripositive ion has the electron configuration 3Kr4 4d3?
Problem 45
- Which element in the transition-metal series Sc through Zn has five unpaired electrons in its +3 ion?
Problem 47
- Which atom or ion in the following pairs would you expect to be larger? (c) Cr3+ or Cr6+
Problem 49
- Order the following ions from smallest to largest: Sr2+, Se2-, Br-, Rb+.
Problem 50
- Which ion has a larger atomic radius, Cu+ or Cu2+? Explain your reasoning.
Problem 52
- Which ion has a larger atomic radius, Fe2+ or Fe3+? Explain your reasoning.
Problem 53