Problem 64
Question
Which of the following is the strongest oxidizing agent? (a) \(\mathrm{F}_{2}\) (b) \(\mathrm{Cl}_{2}\) (c) \(\mathrm{Br}_{2}\) (d) \(\mathrm{I}_{2}\)
Step-by-Step Solution
Verified Answer
F_2
is the strongest oxidizing agent.
1Step 1: Understand Oxidizing Agent
An oxidizing agent is a substance that gains electrons in a reaction, causing another substance to be oxidized. The stronger the oxidizing agent, the more easily it gains electrons.
2Step 2: Review Halogen Oxidizing Strength
Halogens from the periodic table include fluorine (
F_2
), chlorine (
Cl_2
), bromine (
Br_2
), and iodine (
I_2
). Their oxidizing strength decreases as we move down the group. Therefore, the order from strongest to weakest oxidizing agent is:
F_2
>
Cl_2
>
Br_2
>
I_2
.
3Step 3: Determine the Strongest Oxidizing Agent
Since
F_2
is at the top of the list, it is the strongest oxidizing agent among the halogens provided in the options.
Key Concepts
Halogen Oxidizing StrengthElectron GainHalogens in the Periodic Table
Halogen Oxidizing Strength
Halogens are elements found in Group 17 of the periodic table and are known for their strong oxidizing properties. These elements include fluorine, chlorine, bromine, and iodine.
Oxidizing strength refers to the ability of an element or compound to accept electrons during a chemical reaction. For halogens, this strength decreases as you move down the group in the periodic table. In simpler terms, halogens higher up in the group, like fluorine, are better at attracting and gaining electrons compared to those lower down like iodine.
Therefore, the halogen oxidizing strength follows this order:
Oxidizing strength refers to the ability of an element or compound to accept electrons during a chemical reaction. For halogens, this strength decreases as you move down the group in the periodic table. In simpler terms, halogens higher up in the group, like fluorine, are better at attracting and gaining electrons compared to those lower down like iodine.
Therefore, the halogen oxidizing strength follows this order:
- Fluorine ( F_2 ) - strongest
- Chlorine ( Cl_2 )
- Bromine ( Br_2 )
- Iodine ( I_2 ) - weakest
Electron Gain
Electron gain refers to the process of an atom or molecule acquiring extra electrons. This process is central to how oxidizing agents function. In a chemical reaction, oxidizing agents gain electrons and become reduced, while causing the other substance to lose electrons, or be oxidized.
For halogens, their ability to gain electrons is closely tied to their position in the periodic table. This ability directly impacts their oxidizing strength. Because fluorine is at the top of the halogen group, it has the greatest tendency to gain electrons due to its high electronegativity. This makes it the strongest oxidizing agent among the halogens and allows it to facilitate oxidation of other substances more effectively.
In contrast, iodine, found at the bottom of the group, has a much weaker tendency to gain electrons, making it the weakest oxidizing agent in this context.
For halogens, their ability to gain electrons is closely tied to their position in the periodic table. This ability directly impacts their oxidizing strength. Because fluorine is at the top of the halogen group, it has the greatest tendency to gain electrons due to its high electronegativity. This makes it the strongest oxidizing agent among the halogens and allows it to facilitate oxidation of other substances more effectively.
In contrast, iodine, found at the bottom of the group, has a much weaker tendency to gain electrons, making it the weakest oxidizing agent in this context.
Halogens in the Periodic Table
Halogens are located in Group 17 of the periodic table. This family includes elements like fluorine, chlorine, bromine, and iodine, each known for its distinct reactivity and oxidation properties.
Halogens have seven electrons in their outermost electron shell, making them highly reactive as they seek to gain one additional electron to achieve a stable noble gas configuration. This desire to gain one more electron makes them potent oxidizing agents.
Their reactivity and willingness to gain electrons decrease as you move from top to bottom in the group. This trend is due to the increasing atomic size and decreasing electronegativity. The further down you go, the more distant the valence electrons are from the nucleus, weakening the attraction for additional electrons.
This positioning and reactivity play a vital role in their functions within chemical reactions and their relative oxidizing strength as a family.
Halogens have seven electrons in their outermost electron shell, making them highly reactive as they seek to gain one additional electron to achieve a stable noble gas configuration. This desire to gain one more electron makes them potent oxidizing agents.
Their reactivity and willingness to gain electrons decrease as you move from top to bottom in the group. This trend is due to the increasing atomic size and decreasing electronegativity. The further down you go, the more distant the valence electrons are from the nucleus, weakening the attraction for additional electrons.
This positioning and reactivity play a vital role in their functions within chemical reactions and their relative oxidizing strength as a family.
Other exercises in this chapter
Problem 62
Which of the following has the least bond energy? (a) \(\mathrm{H}_{2}\) (b) \(\mathrm{F}_{2}\) (c) \(\mathrm{O}_{2}^{2}\) (d) \(\mathrm{N}_{2}\)
View solution Problem 63
Which of the following has the highest electronegativity? (a) \(\mathrm{K}\) (b) B (c) \(\mathrm{Cl}\) (d) \(\mathrm{Na}\)
View solution Problem 65
Which of the following is the correct relation with regard to the electron afinity of halogen? (a) \(\mathrm{F}>\mathrm{Cl}\) (b) \(\mathrm{F}>\mathrm{I}\) (c)
View solution Problem 66
The configuration of inert gas with smallest size and highest IE is (a) \(1 \mathrm{~s}^{2}\) (b) \(1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6}\) (c) \
View solution