Back
Problem 63a
Chlorine reacts with oxygen to form Cl2O7. (a) What is the name of this product (see Table 2.6)?
Problem 63b
Chlorine reacts with oxygen to form Cl2O7. (b) Write a balanced equation for the formation of Cl2O71l2 from the elements.
Problem 63c
Chlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH-1aq2?
Problem 64a
An element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58 °C. (a) XCl4 reacts with water to form XO2 and another product. What is the likely identity of the other product?
Problem 64b
An element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58 °C. (b) Do you think that element X is a metal, nonmetal, or metalloid?
Problem 65a
Write balanced equations for the following reactions. a. barium oxide with water
Problem 65c
Write balanced equations for the following reactions. c. sulfur trioxide with water
Problem 66d
Write balanced equations for the following reactions. d. selenium dioxide with aqueous potassium hydroxide.
Problem 69a
Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas.
Problem 69a,b,c
Write a balanced equation for the reaction that occurs in each of the following cases: (b) Strontium oxide is added to water. (c) A fresh surface of lithium metal is exposed to oxygen gas. (d) Sodium metal reacts with molten sulfur.
Problem 70a
Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water.
Problem 70c
Write a balanced equation for the reaction that occurs in each of the following cases: (c) Sodium reacts with oxygen.
Problem 71
(a) As described in Section 7.7, the alkali metals react with hydrogen to form hydrides and react with halogens to form halides. Compare the roles of hydrogen and halogens in these reactions. Write balanced equations for the reaction of fluorine with calcium and for the reaction of hydrogen with calcium. (b) What is the oxidation number and electron configuration of calcium in each product?
Problem 72b
Potassium and hydrogen react to form the ionic compound potassium hydride. (b) Use data in Figures 7.10 and 7.12 to determine the energy change in kJ/mol for the following two reactions:
K(g) + H(g) → K+(g) + H-(g)
K(g) + H(g) → K-(g) + H+(g)
- Compare the elements bromine and chlorine with respect to the following properties: (a) electron configuration (b) most common ionic charge (c) first ionization energy (d) reactivity toward water (e) electron affinity (f) atomic radius
Problem 73
Problem 74a
Little is known about the properties of astatine, At, because of its rarity and high radioactivity. Nevertheless, it is possible for us to make many predictions about its properties. (a) Do you expect the element to be a gas, liquid, or solid at room temperature?
Problem 74b
Little is known about the properties of astatine, At, because of its rarity and high radioactivity. Nevertheless, it is possible for us to make many predictions about its properties. (b) Would you expect At to be a metal, nonmetal, or metalloid? Explain.
Problem 74c
Little is known about the properties of astatine, At, because of its rarity and high radioactivity. Nevertheless, it is possible for us to make many predictions about its properties. (c) What is the chemical formula of the compound it forms with Na?
- (a) Why was the term inert gases dropped? (b) What discovery triggered this change in name? (c) What name is applied to the group 18 elements now?
Problem 75
- (b) Using appropriate reference sources, look up the bond lengths of Xe—F bonds in several molecules. How do these numbers compare to the bond lengths calculated from the atomic radii of the elements?
Problem 76
Problem 77a,b,c
Write a balanced equation for the reaction that occurs in each of the following cases: (a) White phorphrous, P4(s), reacts with chlorine gas. (b) Sodium metal reacts with water. (c) Sulfur reacts with hydrogen gas.
Problem 77d
Write a balanced equation for the reaction that occurs in each of the following cases: (d) Fluorine reacts with water.
- Write a balanced equation for the reaction that occurs in each of the following cases: (a) Calcium metal is heated in an atmosphere of oxygen gas. (b) Copper oxide is heated in an atmosphere of hydrogen gas. (c) Chlorine reacts with nitrogen gas. (d) Boron tribromide reacts with water.
Problem 78
Problem 79
Consider the stable elements through lead (Z = 82). In how many instances are the atomic weights of the elements out of order relative to the atomic numbers of the elements?
Problem 80a
Figure 7.4 shows the radial probability distribution functions for the 2s orbitals and 2p orbitals. (a) Which orbital, 2s or 2p, has more electron density close to the nucleus?
Problem 80b
Figure 7.4 shows the radial probability distribution functions for the 2s orbitals and 2p orbitals. (b) How would you modify Slater's rules to adjust for the difference in electronic penetration of the nucleus for the 2s and 2p orbitals?
Problem 81a
(a) If the core electrons were totally effective at screening the valence electrons and the valence electrons provided no screening for each other, what would be the effective nuclear charge acting on the 3s and 3p valence electrons in P?
Problem 81b
(b) Repeat these calculations using Slater’s rules.
Problem 81d
(d) If you remove a single electron from a P atom, which orbital will it come from?
Problem 83
In Table 7.8, the bonding atomic radius of neon is listed as 0.58 Å, whereas that for xenon is listed as 1.40 Å. A classmate of yours states that the value for Xe is more realistic than the one for Ne. Is she correct? If so, what is the basis for her statement?