Problem 58
Question
Which of the following sets has the strongest tendency to form anions? (a) \(\mathrm{V}, \mathrm{Cr}, \mathrm{Mn}\) (b) \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) (c) Ga, In, Tl (d) \(\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}\)
Step-by-Step Solution
Verified Answer
Set (b) \\(N, O, F\\) is most likely to form anions.
1Step 1: Understanding Anions
Anions are negatively charged ions formed when an atom gains electrons. Elements that typically form anions are non-metals with high electronegativity and high electron affinity.
2Step 2: Analyze Each Set
- Set (a): \(V, Cr, Mn\) are all transition metals, known for forming cations, not anions.- Set (b): \(N, O, F\) are non-metals and part of the p-block; they have high electronegativity and commonly form anions.- Set (c): \({\text{Ga, In, Tl}}\) are metals in group 13 which typically form cations.- Set (d): \(Na, Mg, Al\) are metals from the s-block also known to form cations.
3Step 3: Determine the Best Candidate
Given the analysis of each set, Set (b) \(N, O, F\) contains non-metals which are highly electronegative and form anions easily, unlike the other sets.
Key Concepts
ElectronegativityElectron AffinityNon-metalsTransition Metals
Electronegativity
Electronegativity refers to the tendency of an atom to attract electrons towards itself when it is in a chemical bond.
As a key concept in chemistry, it helps us understand why certain atoms are more likely to form negative ions or anions.
- **High Electronegativity**: Atoms with high electronegativity tend to pull electrons closer, making them more likely to gain an electron and become negatively charged, or anions. - **Trends in the Periodic Table**: Electronegativity typically increases as you move across a period from left to right, and decreases as you move down a group. Thus, non-metals like nitrogen (N), oxygen (O), and fluorine (F) are highly electronegative.
This is why these atoms, found in Set (b) of the original exercise, are more likely to form anions compared to metals or other less electronegative elements.
As a key concept in chemistry, it helps us understand why certain atoms are more likely to form negative ions or anions.
- **High Electronegativity**: Atoms with high electronegativity tend to pull electrons closer, making them more likely to gain an electron and become negatively charged, or anions. - **Trends in the Periodic Table**: Electronegativity typically increases as you move across a period from left to right, and decreases as you move down a group. Thus, non-metals like nitrogen (N), oxygen (O), and fluorine (F) are highly electronegative.
This is why these atoms, found in Set (b) of the original exercise, are more likely to form anions compared to metals or other less electronegative elements.
Electron Affinity
Electron affinity is another important concept in understanding anion formation. It measures the amount of energy released when an atom gains an electron.
A higher electron affinity means the atom strongly attracts an additional electron, often resulting in anion formation.
- **Relation to Anion Formation**: Atoms with high electron affinity release more energy when they gain an electron, which makes anion formation energetically favorable. - **Comparison among Elements**: Non-metals, particularly halogens like fluorine, exhibit high electron affinities, making them eager to form anions.
In contrast, metals generally have lower electron affinities and are not as inclined to form anions. This difference in electron affinity helps to differentiate sets like (b) from (a), (c), and (d) in the exercise.
A higher electron affinity means the atom strongly attracts an additional electron, often resulting in anion formation.
- **Relation to Anion Formation**: Atoms with high electron affinity release more energy when they gain an electron, which makes anion formation energetically favorable. - **Comparison among Elements**: Non-metals, particularly halogens like fluorine, exhibit high electron affinities, making them eager to form anions.
In contrast, metals generally have lower electron affinities and are not as inclined to form anions. This difference in electron affinity helps to differentiate sets like (b) from (a), (c), and (d) in the exercise.
Non-metals
Non-metals are a group of elements that are typically found on the right side of the periodic table. They have a distinct set of properties that influence their chemical behavior and their tendency to form anions.
- **Characteristics**: Non-metals often have higher electronegativity and electron affinity compared to metals. These properties lead them to attract and gain electrons more readily. - **Common Examples**: Typical non-metals include nitrogen, oxygen, and fluorine, all of which are part of Set (b) in the exercise. These elements are not just known for forming anions but are essential in various chemical processes because of their ability to do so. - **Role in Chemistry**: Non-metals often play crucial roles in forming compounds such as acids and bases, and are integral in biological molecules like proteins and nucleic acids.
Understanding non-metals and their properties helps clarify why they are more likely to form anions, unlike transition metals or alkali metals.
- **Characteristics**: Non-metals often have higher electronegativity and electron affinity compared to metals. These properties lead them to attract and gain electrons more readily. - **Common Examples**: Typical non-metals include nitrogen, oxygen, and fluorine, all of which are part of Set (b) in the exercise. These elements are not just known for forming anions but are essential in various chemical processes because of their ability to do so. - **Role in Chemistry**: Non-metals often play crucial roles in forming compounds such as acids and bases, and are integral in biological molecules like proteins and nucleic acids.
Understanding non-metals and their properties helps clarify why they are more likely to form anions, unlike transition metals or alkali metals.
Transition Metals
Transition metals are a group of metals located in the middle of the periodic table. These elements are known for their range of oxidation states and ability to form complex ions. However, they rarely form anions.
- **Electronegativity and Electron Affinity**: Transition metals typically have moderate electronegativity and low electron affinity. This means they do not easily attract or gain electrons, making anion formation uncommon. - **Typical Behavior**: Unlike non-metals, transition metals often lose electrons to form positive ions or cations due to their d-orbital electrons. - **Uses in Everyday Life**: Transition metals, such as vanadium (V), chromium (Cr), and manganese (Mn) from Set (a), are widely used in industries for their magnetic, catalytic, and conductive properties, rather than for forming anions.
In the context of the exercise, recognizing these properties explains why transition metals are less likely to form anions compared to non-metals.
- **Electronegativity and Electron Affinity**: Transition metals typically have moderate electronegativity and low electron affinity. This means they do not easily attract or gain electrons, making anion formation uncommon. - **Typical Behavior**: Unlike non-metals, transition metals often lose electrons to form positive ions or cations due to their d-orbital electrons. - **Uses in Everyday Life**: Transition metals, such as vanadium (V), chromium (Cr), and manganese (Mn) from Set (a), are widely used in industries for their magnetic, catalytic, and conductive properties, rather than for forming anions.
In the context of the exercise, recognizing these properties explains why transition metals are less likely to form anions compared to non-metals.
Other exercises in this chapter
Problem 55
Which of the following has the lowest bond angle? (a) \(\mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{CH}_{4}\) (c) \(\mathrm{H}_{2} \mathrm{~S}\) (d) \(\mathrm{NH}
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Which one of the following elements does not form the compound, \(\mathrm{M}_{4} \mathrm{O}_{10}(\mathrm{M}=\) element \() ?\) (a) As (b) Bi (c) \(\mathrm{Sb}\)
View solution Problem 59
Which one of the following statements is correct with respect to the basic character? (a) \(\mathrm{PH}_{3}=\mathrm{NH}_{3}\) (b) \(\mathrm{PH}_{3}>\mathrm{P}\l
View solution Problem 60
The correct order for decreasing ionic nature of lead dihalides is (a) \(\mathrm{PbF}_{2}>\mathrm{PbBr}_{2}>\mathrm{PbCl}_{2}>\mathrm{PbI}_{2}\) (b) \(\mathrm{P
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