Chlorine reacts with oxygen to form Cl2O7. (a) What is the name of this product (see Table 2.6)?

Chlorine reacts with oxygen to form Cl2O7. (b) Write a balanced equation for the formation of Cl2O71l2 from the elements.

Chlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH-1aq2?

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?

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?

Write balanced equations for the following reactions. a. barium oxide with water

Write balanced equations for the following reactions. c. sulfur trioxide with water

Write balanced equations for the following reactions. d. selenium dioxide with aqueous potassium hydroxide.

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.

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.

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water.

Write a balanced equation for the reaction that occurs in each of the following cases: (c) Sodium reacts with oxygen.

(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?

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)

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?

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.

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?

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.

Write a balanced equation for the reaction that occurs in each of the following cases: (d) Fluorine reacts with water.

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?

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?

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?

(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?

(b) Repeat these calculations using Slater’s rules.

(d) If you remove a single electron from a P atom, which orbital will it come from?