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Chapter 7: Problem 73

Compare the elements bromine and chlorine with respect to the following properties: (a) electron configuration, (b) most common ionic charge, \((\mathbf{c})\) first ionization energy, (d) reactivity toward water, \((\mathbf{e})\) electron affinity, \((\mathbf{f})\) atomic radius. Account for the differences between the two elements.

Short Answer

Expert verified
In summary, Bromine (Br) and Chlorine (Cl) have similar electron configurations and both have a most common ionic charge of -1 due to their placement in Group 17 (halogens). However, Chlorine has a higher first ionization energy, greater reactivity towards water, and slightly higher electron affinity than Bromine due to its smaller atomic radius and fewer electron shells, resulting in stronger attractive forces for electrons. On the other hand, Bromine has a larger atomic radius as it is one period below Chlorine in the periodic table.

Step by step solution

01

1. Electron Configuration

Determine the electron configuration of both elements. Bromine (Br) has an atomic number of 35, and Chlorine (Cl) has an atomic number of 17. For Bromine, the electron configuration is: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^5\] For Chlorine, the electron configuration is: \[1s^2 2s^2 2p^6 3s^2 3p^5\]
02

2. Most Common Ionic Charge

Determine the most common ionic charge for both elements based on their electron configurations. Both Bromine and Chlorine are in Group 17, which are the halogens. They tend to gain one electron to achieve a full outer shell (noble gas configuration). Therefore, both Bromine and Chlorine most commonly form -1 ions.
03

3. First Ionization Energy

Compare the first ionization energy of Bromine and Chlorine. Ionization energy is the energy required to remove an electron from a neutral atom. Since Chlorine is closer to the nucleus (smaller atomic number) and has fewer electron shells than Bromine, it has a higher first ionization energy.
04

4. Reactivity towards Water

Compare the reactivity of Bromine and Chlorine towards water. Chlorine is more reactive towards water than Bromine because it has a higher electronegativity, which results in a stronger attraction for electrons. Chlorine readily reacts with water to form hydrochloric acid (HCl) and hypochlorous acid (HOCl), while Bromine reacts with water more slowly, forming hydrobromic acid (HBr) and hypobromous acid (HOBr).
05

5. Electron Affinity

Compare the electron affinity of Bromine and Chlorine. Electron affinity is the energy change when an electron is added to a neutral atom. Both elements have a high electron affinity since they only need one electron to have a complete outer shell. However, Chlorine has a slightly higher electron affinity than Bromine because it has a smaller atomic radius and fewer electron shells, which results in a stronger attraction for an incoming electron.
06

6. Atomic Radius

Compare the atomic radii of Bromine and Chlorine. Atomic radius generally increases as you go down a group due to additional electron shells being added. As Bromine is one period below Chlorine in the periodic table, it has a larger atomic radius. In conclusion, Bromine and Chlorine share similar properties due to their placement in Group 17 as halogens. However, there are differences in their properties such as ionization energy, reactivity towards water, electron affinity, and atomic radius due to Chlorine having fewer electron shells and a smaller atomic radius, resulting in stronger attractive forces for electrons.

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Most popular questions from this chapter

Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen, (b) the second ionization energy of ox ygen, and (c) the electron affinity of oxygen? (i) \(\mathrm{O}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{-}(g)\) (ii) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{+}(g)+\mathrm{e}^{-}\) (iii) \(\mathrm{O}(g)+2 \mathrm{e}^{-} \longrightarrow \mathrm{O}^{2-}(g)\) (iv) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{2+}(g)+2 \mathrm{e}^{-}\) $(\mathbf{v}) \mathrm{O}^{+}(g) \longrightarrow \mathrm{O}^{2+}(g)+\mathrm{e}^{-}$

Discussing this chapter, a classmate says, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." Do you agree or disagree?

Discussing this chapter, a classmate says, "An element that commonly forms a cation is a metal." Do you agree or disagree?

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7} .\) (a) What is the name of this product (see Table 2.6)? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q) ?(\mathbf{d})\) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the -2 oxidation state, what is the oxidation state of the \(\mathrm{Cl}\) ? What is the electron configuration of \(\mathrm{Cl}\) in this oxidation state?

The electron affinities, in \(\mathrm{kJ} / \mathrm{mol}\), for the group 11 and group 12 metals are as follows: (a) Why are the electron affinities of the group 12 elements greater than zero? (b) Why do the electron affinities of the group 11 elements become more negative as we move down the group? [Hint: Examine the trends in the electron affinities of other groups as we proceed down the periodic table.]
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