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Chemistry | 12th Edition | ISBN: 9780078021510 | Authors: Raymond Chang; Kenneth Goldsby

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Author: Raymond Chang; Kenneth Goldsby
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Chapter 8 Problems

Chapter: 8 Problem: 8.1

Chemistry 12
Briefly describe the significance of Mendeleevs periodic table.

Chapter: 8 Problem: 8.2

Chemistry 12
What is Moseleys contribution to the modern periodic table?

Chapter: 8 Problem: 8.3

Chemistry 12
Describe the general layout of a modern periodic table

Chapter: 8 Problem: 8.4

Chemistry 12
What is the most important relationship among elements in the same group in the periodic table?

Chapter: 8 Problem: 8.5

Chemistry 12
Which of the following elements are metals, nonmetals, or metalloids? As, Xe, Fe, Li, B, Cl, Ba, P, I, Si.

Chapter: 8 Problem: 8.6

Chemistry 12
Compare the physical and chemical properties of metals and nonmetals.

Chapter: 8 Problem: 8.7

Chemistry 12
Draw a rough sketch of a periodic table (no details are required). Indicate regions where metals, nonmetals, and metalloids are located.

Chapter: 8 Problem: 8.8

Chemistry 12
What is a representative element? Give names and symbols of four representative elements.

Chapter: 8 Problem: 8.9

Chemistry 12
Without referring to a periodic table, write the name and give the symbol for an element in each of the following groups: 1A, 2A, 3A, 4A, 5A, 6A, 7A, 8A, transition metals.

Chapter: 8 Problem: 8.1b

Chemistry 12
Indicate whether the following elements exist as atomic species, molecular species, or extensive threedimensional structures in their most stable states at 25C and 1 atm and write the molecular or empirical formula for each one: phosphorus, iodine, magnesium, neon, carbon, sulfur, cesium, and oxygen.

Chapter: 8 Problem: 8.11

Chemistry 12
You are given a dark shiny solid and asked to determine whether it is iodine or a metallic element. Suggest a nondestructive test that would enable you to arrive at the correct answer

Chapter: 8 Problem: 8.12

Chemistry 12
What are valence electrons? For representative elements, the number of valence electrons of an element is equal to its group number. Show that this is true for the following elements: Al, Sr, K, Br, P, S, C.

Chapter: 8 Problem: 8.13

Chemistry 12
Write the outer electron configurations for the (a) alkali metals, (b) alkaline earth metals, (c) halogens, (d) noble gases.

Chapter: 8 Problem: 8.14

Chemistry 12
Use the first-row transition metals (Sc to Cu) as an example to illustrate the characteristics of the electron configurations of transition metals

Chapter: 8 Problem: 8.15

Chemistry 12
The electron configurations of ions derived from representative elements follow a common pattern. What is the pattern, and how does it relate to the stability of these ions?

Chapter: 8 Problem: 8.16

Chemistry 12
What do we mean when we say that two ions or an atom and an ion are isoelectronic?

Chapter: 8 Problem: 8.17

Chemistry 12
What is wrong with the statement The atoms of element X are isoelectronic with the atoms of element Y?

Chapter: 8 Problem: 8.18

Chemistry 12
Give three examples of first-row transition metal (Sc to Cu) ions whose electron configurations are represented by the argon core.

Chapter: 8 Problem: 8.19

Chemistry 12
In the periodic table, the element hydrogen is sometimes grouped with the alkali metals (as in this book) and sometimes with the halogens. Explain why hydrogen can resemble the Group 1A and the Group 7A elements

Chapter: 8 Problem: 8.2b

Chemistry 12
A neutral atom of a certain element has 17 electrons. Without consulting a periodic table, (a) write the ground-state electron configuration of the element, (b) classify the element, (c) determine whether this element is diamagnetic or paramagnetic.

Chapter: 8 Problem: 8.21

Chemistry 12
Group the following electron configurations in pairs that would represent similar chemical properties of their atoms: (a) 1s 2 2s 2 2p6 3s 2 (b) 1s 2 2s 2 2p3 (c) 1s 2 2s 2 2p6 3s 2 3p6 4s 2 3d104p6 (d) 1s 2 2s 2 (e) 1s 2 2s 2 2p6 (f) 1s 2 2s 2 2p6 3s 2 3p3

Chapter: 8 Problem: 8.22

Chemistry 12
Group the following electron configurations in pairs that would represent similar chemical properties of their atoms: (a) 1s 2 2s 2 2p5 (b) 1s 2 2s 1 (c) 1s 2 2s 2 2p6 (d) 1s 2 2s 2 2p6 3s 2 3p5 (e) 1s 2 2s 2 2p6 3s 2 3p6 4s 1 (f) 1s 2 2s 2 2p6 3s 2 3p6 4s 2 3d104p6

Chapter: 8 Problem: 8.23

Chemistry 12
Without referring to a periodic table, write the electron configuration of elements with the following atomic numbers: (a) 9, (b) 20, (c) 26, (d) 33. Classify the elements.

Chapter: 8 Problem: 8.24

Chemistry 12
Specify the group of the periodic table in which each of the following elements is found: (a) [Ne]3s 1 , (b) [Ne]3s 2 3p3 , (c) [Ne]3s 2 3p6 , (d) [Ar]4s 2 3d8

Chapter: 8 Problem: 8.25

Chemistry 12
A M21 ion derived from a metal in the first transition metal series has four electrons in the 3d subshell. What element might M be?

Chapter: 8 Problem: 8.26

Chemistry 12
A metal ion with a net 13 charge has five electrons in the 3d subshell. Identify the metal.

Chapter: 8 Problem: 8.27

Chemistry 12
Write the ground-state electron configurations of the following ions: (a) Li1, (b) H2, (c) N32, (d) F2, (e) S22, (f) Al31, (g) Se22, (h) Br2, (i) Rb1, (j) Sr21, (k) Sn21, (l) Te22, (m) Ba21, (n) Pb21, (o) In31, (p) Tl1, (q) Tl31.

Chapter: 8 Problem: 8.28

Chemistry 12
Write the ground-state electron configurations of the following ions, which play important roles in biochemical processes in our bodies: (a) Na1, (b) Mg21, (c) Cl2, (d) K1, (e) Ca21, (f) Fe21, (g) Cu21, (h) Zn21.

Chapter: 8 Problem: 8.29

Chemistry 12
Write the ground-state electron configurations of the following transition metal ions: (a) Sc31, (b) Ti41, (c) V51, (d) Cr31, (e) Mn21, (f) Fe21, (g) Fe31, (h) Co21, (i) Ni21, (j) Cu1, (k) Cu21, (l) Ag1, (m) Au1, (n) Au31, (o) Pt21.

Chapter: 8 Problem: 8.3b

Chemistry 12
Name the ions with 13 charges that have the following electron configurations: (a) [Ar]3d3 , (b) [Ar], (c) [Kr]4d6 , (d) [Xe]4f 145d6

Chapter: 8 Problem: 8.31

Chemistry 12
Which of the following species are isoelectronic with each other? C, Cl2, Mn21, B2, Ar, Zn, Fe31, Ge21.

Chapter: 8 Problem: 8.32

Chemistry 12
Group the species that are isoelectronic: Be21, F2, Fe21, N32, He, S22, Co31, Ar.

Chapter: 8 Problem: 8.33

Chemistry 12
Define atomic radius. Does the size of an atom have a precise meaning?

Chapter: 8 Problem: 8.34

Chemistry 12
How does atomic radius change (a) from left to right across a period and (b) from top to bottom in a group?

Chapter: 8 Problem: 8.35

Chemistry 12
Define ionic radius. How does the size of an atom change when it is converted to (a) an anion and (b) a cation?

Chapter: 8 Problem: 8.36

Chemistry 12
Explain why, for isoelectronic ions, the anions are larger than the cations.

Chapter: 8 Problem: 8.37

Chemistry 12
On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs: (a) Na, Cs; (b) Be, Ba; (c) N, Sb; (d) F, Br; (e) Ne, Xe

Chapter: 8 Problem: 8.38

Chemistry 12
Arrange the following atoms in order of decreasing atomic radius: Na, Al, P, Cl, Mg.

Chapter: 8 Problem: 8.39

Chemistry 12
Which is the largest atom in Group 4A?

Chapter: 8 Problem: 8.4b

Chemistry 12
Which is the smallest atom in Group 7A?

Chapter: 8 Problem: 8.41

Chemistry 12
Why is the radius of the lithium atom considerably larger than the radius of the hydrogen atom?

Chapter: 8 Problem: 8.42

Chemistry 12
Use the second period of the periodic table as an example to show that the size of atoms decreases as we move from left to right. Explain the trend.

Chapter: 8 Problem: 8.43

Chemistry 12
Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl2; (b) Na or Na1; (c) O22 or S22; (d) Mg21 or Al31; (e) Au1 or Au31.

Chapter: 8 Problem: 8.44

Chemistry 12
List the following ions in order of increasing ionic radius: N32, Na1, F2, Mg21, O22

Chapter: 8 Problem: 8.45

Chemistry 12
Explain which of the following cations is larger, and why: Cu1 or Cu21.

Chapter: 8 Problem: 8.46

Chemistry 12
Explain which of the following anions is larger, and why: Se22 or Te22.

Chapter: 8 Problem: 8.47

Chemistry 12
Give the physical states (gas, liquid, or solid) of the representative elements in the fourth period (K, Ca, Ga, Ge, As, Se, Br) at 1 atm and 25C

Chapter: 8 Problem: 8.48

Chemistry 12
Both H2 and He contain two 1s electrons. Which species is larger? Explain your choice.

Chapter: 8 Problem: 8.49

Chemistry 12
Define ionization energy. Ionization energy measurements are usually made when atoms are in the gaseous state. Why? Why is the second ionization energy always greater than the first ionization energy for any element?

Chapter: 8 Problem: 8.5b

Chemistry 12
Sketch the outline of the periodic table and show group and period trends in the first ionization energy of the elements. What types of elements have the highest ionization energies and what types the lowest ionization energies?

Chapter: 8 Problem: 8.51

Chemistry 12
Arrange the following in order of increasing first ionization energy: Na, Cl, Al, S, and Cs.

Chapter: 8 Problem: 8.52

Chemistry 12
Arrange the following in order of increasing first ionization energy: F, K, P, Ca, and Ne.

Chapter: 8 Problem: 8.53

Chemistry 12
Use the third period of the periodic table as an example to illustrate the change in first ionization energies of the elements as we move from left to right. Explain the trend.

Chapter: 8 Problem: 8.54

Chemistry 12
In general, ionization energy increases from left to right across a given period. Aluminum, however, has a lower ionization energy than magnesium. Explain.

Chapter: 8 Problem: 8.55

Chemistry 12
The first and second ionization energies of K are 419 kJ/mol and 3052 kJ/mol, and those of Ca are 590 kJ/mol and 1145 kJ/mol, respectively. Compare their values and comment on the differences.

Chapter: 8 Problem: 8.56

Chemistry 12
Two atoms have the electron configurations 1s 2 2s 2 2p6 and 1s 2 2s 2 2p6 3s 1 . The first ionization energy of one is 2080 kJ/mol, and that of the other is 496 kJ/mol. Match each ionization energy with one of the given electron configurations. Justify your choice.

Chapter: 8 Problem: 8.57

Chemistry 12
A hydrogenlike ion is an ion containing only one electron. The energies of the electron in a hydrogenlike ion are given by En 5 2(2.18 3 10218 J)Z2 a 1 n2 b where n is the principal quantum number and Z is the atomic number of the element. Calculate the ionization energy (in kJ/mol) of the He1 ion.

Chapter: 8 Problem: 8.58

Chemistry 12
Plasma is a state of matter consisting of positive gaseous ions and electrons. In the plasma state, a mercury atom could be stripped of its 80 electrons and therefore would exist as Hg801. Use the equation in Problem 8.57 to calculate the energy required for the last ionization step, that is, Hg

Chapter: 8 Problem: 8.59

Chemistry 12
(a) Define electron affinity. (b) Electron affinity measurements are made with gaseous atoms. Why? (c) Ionization energy is always a positive quantity, whereas electron affinity may be either positive or negative. Explain

Chapter: 8 Problem: 8.6b

Chemistry 12
Explain the trends in electron affinity from aluminum to chlorine (see Table 8.3).

Chapter: 8 Problem: 8.61

Chemistry 12
Arrange the elements in each of the following groups in increasing order of the most positive electron affinity: (a) Li, Na, K; (b) F, Cl, Br, I; (c) O, Si, P, Ca, Ba.

Chapter: 8 Problem: 8.62

Chemistry 12
Specify which of the following elements you would expect to have the greatest electron affinity and which would have the least: He, K, Co, S, Cl

Chapter: 8 Problem: 8.63

Chemistry 12
Considering their electron affinities, do you think it is possible for the alkali metals to form an anion like M2, where M represents an alkali metal?

Chapter: 8 Problem: 8.64

Chemistry 12
Explain why alkali metals have a greater affinity for electrons than alkaline earth metals.

Chapter: 8 Problem: 8.65

Chemistry 12
What is meant by the diagonal relationship? Name two pairs of elements that show this relationship

Chapter: 8 Problem: 8.66

Chemistry 12
Which elements are more likely to form acidic oxides? Basic oxides? Amphoteric oxides?

Chapter: 8 Problem: 8.67

Chemistry 12
Use the alkali metals and alkaline earth metals as examples to show how we can predict the chemical properties of elements simply from their electron configurations.

Chapter: 8 Problem: 8.68

Chemistry 12
Based on your knowledge of the chemistry of the alkali metals, predict some of the chemical properties of francium, the last member of the group.

Chapter: 8 Problem: 8.69

Chemistry 12
As a group, the noble gases are very stable chemically (only Kr and Xe are known to form compounds). Use the concepts of shielding and the effective nuclear charge to explain why the noble gases tend to neither give up electrons nor accept additional electrons.

Chapter: 8 Problem: 8.7b

Chemistry 12
Why are Group 1B elements more stable than Group 1A elements even though they seem to have the same outer electron configuration, ns1 , where n is the principal quantum number of the outermost shell?

Chapter: 8 Problem: 8.71

Chemistry 12
How do the chemical properties of oxides change from left to right across a period? From top to bottom within a particular group?

Chapter: 8 Problem: 8.72

Chemistry 12
Write balanced equations for the reactions between each of the following oxides and water: (a) Li2O, (b) CaO, (c) SO3.

Chapter: 8 Problem: 8.73

Chemistry 12
Write formulas for and name the binary hydrogen compounds of the second-period elements (Li to F). Describe how the physical and chemical properties of these compounds change from left to right across the period

Chapter: 8 Problem: 8.74

Chemistry 12
Which oxide is more basic, MgO or BaO? Why?

Chapter: 8 Problem: 8.75

Chemistry 12
State whether each of the following properties of the representative elements generally increases or decreases (a) from left to right across a period and (b) from top to bottom within a group: metallic character, atomic size, ionization energy, acidity of oxides

Chapter: 8 Problem: 8.76

Chemistry 12
With reference to the periodic table, name (a) a halogen element in the fourth period, (b) an element similar to phosphorus in chemical properties, (c) the most reactive metal in the fifth period, (d) an element that has an atomic number smaller than 20 and is similar to strontium.

Chapter: 8 Problem: 8.77

Chemistry 12
Write equations representing the following processes: (a) The electron affinity of S2. (b) The third ionization energy of titanium. (c) The electron affinity of Mg21. (d) The ionization energy of O22.

Chapter: 8 Problem: 8.78

Chemistry 12
List all the common ions of representative elements and transition metals that are isoelectronic with Ar

Chapter: 8 Problem: 8.79

Chemistry 12
Write the empirical (or molecular) formulas of compounds that the elements in the third period (sodium to chlorine) should form with (a) molecular oxygen and (b) molecular chlorine. In each case indicate whether you would expect the compound to be ionic or molecular in character

Chapter: 8 Problem: 8.8b

Chemistry 12
Element M is a shiny and highly reactive metal (melting point 63C), and element X is a highly reactive nonmetal (melting point 27.2C). They react to form a compound with the empirical formula MX, a colorless, brittle white solid that melts at 734C. When dissolved in water or when in the molten state,

Chapter: 8 Problem: 8.81

Chemistry 12
Match each of the elements on the right with its description on the left: (a) A dark-red liquid (b) A colorless gas that burns in oxygen gas (c) A reactive metal that attacks water (d) A shiny metal that is used in jewelry (e) An inert gas

Chapter: 8 Problem: 8.82

Chemistry 12
Arrange the following species in isoelectronic pairs: O1, Ar, S22, Ne, Zn, Cs1, N32, As31, N, Xe.

Chapter: 8 Problem: 8.83

Chemistry 12
In which of the following are the species written in decreasing order by size of radius? (a) Be, Mg, Ba, (b) N32, O22, F2, (c) Tl31, Tl21, Tl1.

Chapter: 8 Problem: 8.84

Chemistry 12
Which of the following properties show a clear periodic variation? (a) first ionization energy, (b) molar mass of the elements, (c) number of isotopes of an element, (d) atomic radius.

Chapter: 8 Problem: 8.85

Chemistry 12
When carbon dioxide is bubbled through a clear calcium hydroxide solution, the solution appears milky. Write an equation for the reaction and explain how this reaction illustrates that CO2 is an acidic oxide.

Chapter: 8 Problem: 8.86

Chemistry 12
You are given four substances: a fuming red liquid, a dark metallic-looking solid, a pale-yellow gas, and a yellow-green gas that attacks glass. You are told that these substances are the first four members of Group 7A, the halogens. Name each one.

Chapter: 8 Problem: 8.87

Chemistry 12
Calculate the change in energy for the following processes: (a) Na(g) 1 Cl(g) Na1(g) 1 Cl2(g) (b) Ca(g) 1 2Br(g) Ca21(g) 1 2Br2(g)

Chapter: 8 Problem: 8.88

Chemistry 12
Calculate the change in energy for the following processes: (a) Mg(g) 1 2F(g) Mg21(g) 1 2F2(g) (b) 2Al(g) 1 3O(g) 2Al31(g) 1 3O22(g) The electron affinity of O2 is 2844 kJ/mol.

Chapter: 8 Problem: 8.89

Chemistry 12
For each pair of elements listed, give three properties that show their chemical similarity: (a) so dium and potassium and (b) chlorine and bromine.

Chapter: 8 Problem: 8.9b

Chemistry 12
Name the element that forms compounds, under appropriate conditions, with every other element in the periodic table except He, Ne, and Ar.

Chapter: 8 Problem: 8.91

Chemistry 12
Explain why the first electron affinity of sulfur is 200 kJ/mol but the second electron affinity is 2649 kJ/mol.

Chapter: 8 Problem: 8.92

Chemistry 12
The H2 ion and the He atom have two 1s electrons each. Which of the two species is larger? Explain.

Chapter: 8 Problem: 8.93

Chemistry 12
Predict the products of the following oxides with water: Na2O, BaO, CO2, N2O5, P4O10, SO3. Write an Calcium (Ca) Gold (Au) Hydrogen (H2) Argon (Ar) Bromine (Br2) equation for each of the reactions. Specify whether the oxides are acidic, basic, or amphoteric.

Chapter: 8 Problem: 8.94

Chemistry 12
Write the formulas and names of the oxides of the second-period elements (Li to N). Identify the oxides as acidic, basic, or amphoteric.

Chapter: 8 Problem: 8.95

Chemistry 12
State whether each of the following elements is a gas, a liquid, or a solid under atmospheric conditions. Also state whether it exists in the elemental form as atoms, as molecules, or as a three-dimensional network: Mg, Cl, Si, Kr, O, I, Hg, Br

Chapter: 8 Problem: 8.96

Chemistry 12
What factors account for the unique nature of hydrogen?

Chapter: 8 Problem: 8.97

Chemistry 12
The air in a manned spacecraft or submarine needs to be purified of exhaled carbon dioxide. Write equations for the reactions between carbon dioxide and (a) lithium oxide (Li2O), (b) sodium peroxide (Na2O2), and (c) potassium superoxide (KO2).

Chapter: 8 Problem: 8.98

Chemistry 12
The formula for calculating the energies of an electron in a hydrogenlike ion is given in Problem 8.57. This equation cannot be applied to many-electron atoms. One way to modify it for the more complex atoms is to replace Z with (Z 2 ), where Z is the atomic number and is a positive dimensionless qu

Chapter: 8 Problem: 8.99

Chemistry 12
Why do noble gases have negative electron affinity values?

Chapter: 8 Problem: 8.1c

Chemistry 12
The atomic radius of K is 227 pm and that of K1 is 133 pm. Calculate the percent decrease in volume that occurs when K(g) is converted to K1(g). [The volume of a sphere is 1 4 32r 3 , where r is the radius of the sphere.]

Chapter: 8 Problem: 8.101

Chemistry 12
The atomic radius of F is 72 pm and that of F2 is 133 pm. Calculate the percent increase in volume that occurs when F(g) is converted to F2(g). (See Problem 8.100 for the volume of a sphere.)

Chapter: 8 Problem: 8.102

Chemistry 12
A technique called photoelectron spectroscopy is used to measure the ionization energy of atoms. A sample is irradiated with UV light, and electrons are ejected from the valence shell. The kinetic energies of the ejected electrons are measured. Because the energy of the UV photon and the kinetic ener

Chapter: 8 Problem: 8.103

Chemistry 12
Referring to the Chemistry in Action essay on p. 358, answer the following questions. (a) Why did it take so long to discover the first noble gas (argon) on Earth? (b) Once argon had been discovered, why did it take relatively little time to discover the rest of the noble gases? (c) Why was helium no

Chapter: 8 Problem: 8.104

Chemistry 12
The energy needed for the following process is 1.96 3 104 kJ/mol: Li(g) Li31(g) 1 3e2 If the first ionization energy of lithium is 520 kJ/mol, calculate the second ionization energy of lithium, that is, the energy required for the process Li1(g) Li21(g) 1 e2 (Hint: You need the equation in Problem

Chapter: 8 Problem: 8.105

Chemistry 12
An element X reacts with hydrogen gas at 200C to form compound Y. When Y is heated to a higher temperature, it decomposes to the element X and hydrogen gas in the ratio of 559 mL of H2 (measured at STP) for 1.00 g of X reacted. X also combines with chlorine to form a compound Z, which contains 63.89

Chapter: 8 Problem: 8.106

Chemistry 12
A student is given samples of three elements, X, Y, and Z, which could be an alkali metal, a member of Group 4A, and a member of Group 5A. She makes the following observations: Element X has a metallic luster and conducts electricity. It reacts slowly with hydrochloric acid to produce hydrogen gas. E

Chapter: 8 Problem: 8.107

Chemistry 12
Identify the ions whose orbital diagrams for the valence electrons are shown below. The charges of the ions are: (a) 11, (b) 31, (c) 41, (d) 21. (a) 4s 3d hg hg hg hg hg (b) 4s 3d h h h h h h h h h h h (c) 4s 3d (d) 5s 4d

Chapter: 8 Problem: 8.108

Chemistry 12
What is the electron affinity of the Na1 ion?

Chapter: 8 Problem: 8.109

Chemistry 12
The ionization energies of sodium (in kJ/mol), starting with the first and ending with the eleventh, are 495.9, 4560, 6900, 9540, 13,400, 16,600, 20,120, 25,490, 28,930, 141,360, 170,000. Plot the log of ionization energy (y axis) versus the number of ionization (x axis); for example, log 495.9 is pl

Chapter: 8 Problem: 8.11c

Chemistry 12
Experimentally, the electron affinity of an element can be determined by using a laser light to ionize the anion of the element in the gas phase: X2(g) 1 hn X(g) 1 e2 Referring to Table 8.3, calculate the photon wavelength (in nanometers) corresponding to the electron affinity for chlorine. In what

Chapter: 8 Problem: 8.111

Chemistry 12
Explain, in terms of their electron configurations, why Fe21 is more easily oxidized to Fe31 than Mn21 to Mn31.

Chapter: 8 Problem: 8.112

Chemistry 12
The standard enthalpy of atomization of an element is the energy required to convert one mole of an element in its most stable form at 25C to one mole of monatomic gas. Given that the standard enthalpy of atomization for sodium is 108.4 kJ/mol, calculate the energy in kilojoules required to convert o

Chapter: 8 Problem: 8.113

Chemistry 12
Write the formulas and names of the hydrides of the following second-period elements: Li, C, N, O, F. Predict their reactions with water

Chapter: 8 Problem: 8.114

Chemistry 12
Based on knowledge of the electronic configuration of titanium, state which of the following compounds of titanium is unlikely to exist: K3TiF6, K2Ti2O5, TiCl3, K2TiO4, K2TiF6.

Chapter: 8 Problem: 8.115

Chemistry 12
Name an element in Group 1A or Group 2A that is an important constituent of each of the following substances: (a) remedy for acid indigestion, (b) coolant in nuclear reactors, (c) Epsom salt, (d) baking powder, (e) gunpowder, (f) a light alloy, (g) fertilizer that also neutralizes acid rain, (h) ceme

Chapter: 8 Problem: 8.116

Chemistry 12
In halogen displacement reactions a halogen element can be generated by oxidizing its anions with a halogen element that lies above it in the periodic table. This means that there is no way to prepare elemental fluorine, because it is the first member of Group 7A. Indeed, for years the only way to pr

Chapter: 8 Problem: 8.117

Chemistry 12
Write a balanced equation for the preparation of (a) molecular oxygen, (b) ammonia, (c) carbon dioxide, (d) molecular hydrogen, (e) calcium oxide. Indicate the physical state of the reactants and products in each equation

Chapter: 8 Problem: 8.118

Chemistry 12
Write chemical formulas for oxides of nitrogen with the following oxidation numbers: 11, 12, 13, 14, 15. (Hint: There are two oxides of nitrogen with 14 oxidation number.)

Chapter: 8 Problem: 8.119

Chemistry 12
Most transition metal ions are colored. For example, a solution of CuSO4 is blue. How would you show that the blue color is due to the hydrated Cu21 ions and not the SO4 22 ions?

Chapter: 8 Problem: 8.12c

Chemistry 12
In general, atomic radius and ionization energy have opposite periodic trends. Why?

Chapter: 8 Problem: 8.121

Chemistry 12
Explain why the electron affinity of nitrogen is approximately zero, while the elements on either side, carbon and oxygen, have substantial positive electron affinities.

Chapter: 8 Problem: 8.122

Chemistry 12
Consider the halogens chlorine, bromine, and iodine. The melting point and boiling point of chlorine are 2101.0C and 234.6C while those of iodine are 113.5C and 184.4C, respectively. Thus, chlorine is a gas and iodine is a solid under room conditions. Estimate the melting point and boiling point of b

Chapter: 8 Problem: 8.123

Chemistry 12
Write a balanced equation that predicts the reaction of rubidium (Rb) with (a) H2O(l), (b) Cl2(g), (c) H2(g).

Chapter: 8 Problem: 8.124

Chemistry 12
The successive IE of the first four electrons of a representative element are 738.1 kJ/mol, 1450 kJ/mol, 7730 kJ/mol, and 10,500 kJ/mol. Characterize the element according to the periodic group.

Chapter: 8 Problem: 8.125

Chemistry 12
Little is known of the chemistry of astatine, the last member of Group 7A. Describe the physical characteristics that you would expect this halogen to have. Predict the products of the reaction between sodium astatide (NaAt) and sulfuric acid. (Hint: Sulfuric acid is an oxidizing agent.)

Chapter: 8 Problem: 8.126

Chemistry 12
As discussed in the chapter, the atomic mass of argon is greater than that of potassium. This observation created a problem in the early development of the periodic table because it meant that argon should be placed after potassium. (a) How was this difficulty resolved? (b) From the following data, c

Chapter: 8 Problem: 8.127

Chemistry 12
Calculate the maximum wavelength of light (in nanometers) required to ionize a single sodium atom.

Chapter: 8 Problem: 8.128

Chemistry 12
Predict the atomic number and ground-state electron configuration of the next member of the alkali metals after francium.

Chapter: 8 Problem: 8.129

Chemistry 12
Why do elements that have high ionization energies also have more positive electron affinities? Which group of elements would be an exception to this generalization?

Chapter: 8 Problem: 8.13c

Chemistry 12
The first four ionization energies of an element are approximately 579 kJ/mol, 1980 kJ/mol, 2963 kJ/mol, and 6180 kJ/mol. To which periodic group does this element belong?

Chapter: 8 Problem: 8.131

Chemistry 12
Some chemists think that helium should properly be called helon. Why? What does the ending in helium (-ium) suggest?

Chapter: 8 Problem: 8.132

Chemistry 12
(a) The formula of the simplest hydrocarbon is CH4 (methane). Predict the formulas of the simplest compounds formed between hydrogen and the following elements: silicon, germanium, tin, and lead. (b) Sodium hydride (NaH) is an ionic compound. Would you expect rubidium hydride (RbH) to be more or less

Chapter: 8 Problem: 8.133

Chemistry 12
Give equations to show that molecular hydrogen can act both as a reducing agent and an oxidizing agent.

Chapter: 8 Problem: 8.134

Chemistry 12
Both Mg21 and Ca21 are important biological ions. One of their functions is to bind to the phosphate groups of ATP molecules or amino acids of proteins. For Group 2A metals in general, the tendency for binding to the anions increases in the order Ba21 , Sr21 , Ca21 , Mg21. Explain the trend.

Chapter: 8 Problem: 8.135

Chemistry 12
Match each of the elements on the right with its description on the left: (a) A pale yellow gas that reacts with water. (b) A soft metal that reacts with water to produce hydrogen. (c) A metalloid that is hard and has a high melting point. (d) A colorless, odorless gas. (e) A metal that is more react

Chapter: 8 Problem: 8.136

Chemistry 12
Write an account on the importance of the periodic table. Pay particular attention to the significance of the position of an element in the table and how the position relates to the chemical and physical properties of the element.

Chapter: 8 Problem: 8.137

Chemistry 12
On the same graph, plot the effective nuclear charge (see p. 334) and atomic radius (see Figure 8.5) versus atomic number for the second period elements Li to Ne. Comment on the trends.

Chapter: 8 Problem: 8.138

Chemistry 12
One allotropic form of an element X is a colorless crystalline solid. The reaction of X with an excess amount of oxygen produces a colorless gas. This gas dissolves in water to yield an acidic solution. Choose one of the following elements that matches X: (a) sulfur, (b) phosphorus, (c) carbon, (d) b

Chapter: 8 Problem: 8.139

Chemistry 12
When magnesium metal is burned in air, it forms two products A and B. A reacts with water to form a basic solution. B reacts with water to form a similar solution as that of A plus a gas with a pungent odor. Identify A and B and write equations for the reactions. (Hint: See Chemistry in Action on p.

Chapter: 8 Problem: 8.14c

Chemistry 12
The ionization energy of a certain element is 412 kJ/mol. When the atoms of this element are in the first excited state, however, the ionization energy is only 126 kJ/mol. Based on this information, calculate the wavelength of light emitted in a transition from the first excited state to the ground s

Chapter: 8 Problem: 8.141

Chemistry 12
Use your knowledge of thermochemistry to calculate the DH for the following processes: (a) Cl2(g) S Cl1(g) 1 2e 2 and (b) K1(g) 1 2e 2 S K2(g).

Chapter: 8 Problem: 8.142

Chemistry 12
Referring to Table 8.2, explain why the first ionization energy of helium is less than twice the ionization energy of hydrogen, but the second ionization energy of helium is greater than twice the ionization energy of hydrogen. [Hint: According to Coulombs law, the energy between two charges Q1 and Q

Chapter: 8 Problem: 8.143

Chemistry 12
As mentioned in Chapter 3 (p. 105), ammonium nitrate (NH4NO3) is the most important nitrogencontaining fertilizer in the world. Describe how you would prepare this compound, given only air and water as the starting materials. You may have any device at your disposal for this task.

Chapter: 8 Problem: 8.144

Chemistry 12
One way to estimate the effective charge (Zeff) of a many-electron atom is to use the equation IE1 5 (1312 kJ/mol)(Z2 eff/n2 ), where IE1 is the first ionization energy and n is the principal quantum number of the shell in which the electron resides. Use this equation to calculate the effective charg

Chapter: 8 Problem: 8.145

Chemistry 12
To prevent the formation of oxides, peroxides, and superoxides, alkali metals are sometimes stored in an inert atmosphere. Which of the following gases should not be used for lithium: Ne, Ar, N2, Kr? Explain. (Hint: As mentioned in the chapter, Li and Mg exhibit a diagonal relationship. Compare the c

Chapter: 8 Problem: 8.146

Chemistry 12
Describe the biological role of the elements in the human body shown in the following periodic table. (You may need to do research at websites such as www.webelements.com.) H Na K Ca Cr Mn Fe Co Cu Zn Br I P S Cl CNO Mg

Chapter: 8 Problem: 8.147

Chemistry 12
Recent theoretical calculations suggest that astatine may be a monoatomic metal rather than a diatomic molecule like the other halogens. (a) Rationalize this prediction based on astatines position in the periodic table. (b) The energy required to remove an electron from one At atom was determined by

Chapter: 8 Problem: 8.148

Chemistry 12
Consider the first 18 elements from hydrogen to argon. Would you expect the atoms of half of them to be diamagnetic and half of them to be paramagnetic? Explain.

Chapter: 8 Problem: 8.149

Chemistry 12
Compare the work function for cesium (206 kJ/mol) with its first ionization energy (376 kJ/mol). Explain the difference.

Chapter: 8 Problem: 8.15c

Chemistry 12
The only confirmed compound of radon is radon difluoride, RnF2. One reason that it is difficult to study the chemistry of radon is that all isotopes of radon are radioactive so it is dangerous to handle the substance. Can you suggest another reason why there are so few known radon compounds? (Hint: R

Chapter: 8 Problem: 8.151

Chemistry 12
Arsenic (As) is not an essential element for the human body. (a) Based on its position in the periodic table, suggest a reason for its toxicity. (b) When arsenic enters a persons body, it quickly shows up in the follicle of the growing hair. This action has enabled detectives to solve many murder mys

Chapter: 8 Problem: 8.152

Chemistry 12
The boiling points of neon and krypton are 2245.9C and 2152.9C, respectively. Using these data, estimate the boiling point of argon.

Chapter: 8 Problem: 8.153

Chemistry 12
Using the following boiling-point data, estimate the boiling point of francium: Metal Li Na K Rb Cs Fr B.pt.(C) 1347 882.9 774 688 678.4 ?

Chapter: 8 Problem: 8.154

Chemistry 12
The energy gap between the 6s and 5d levels in gold is 4.32 3 10219 J. Based on this information, predict the perceived color of gold vapor. (Hint: You need to be familiar with the notion of complementary color; see Figure 23.18.)

Chapter: 8 Problem: 8.155

Chemistry 12
Calculate the volume of 1 mole of K atoms (see Figure 8.5) and compare the result by using the density of K (0.856 g/cm3 ). Account for the difference.

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