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Arrange \(0, S\) and Se in the increasing order of their electron affinity. (1) \(\mathrm{Se}<\mathrm{S}<\mathrm{O}\) (2) \(\mathrm{O}<\mathrm{Se}<\mathrm{S}\) (3) \(\mathrm{S}<\mathrm{O}<\mathrm{Se}\) (4) \(\mathrm{S}<\mathrm{Se}<\mathrm{O}\)

Short Answer

Expert verified
Option (1) \ \( \text{Se} < \text{S} < \text{O} \)

Step by step solution

01

Understand electron affinity

Electron affinity is the amount of energy released when an atom in the gaseous state accepts an electron to form an anion.
02

Identify periodic trends

Electron affinity generally increases across a period and decreases down a group in the periodic table.
03

Locate the elements in the periodic table

Oxygen (O), Sulfur (S), and Selenium (Se) are in Group 16, with Oxygen at the top, followed by Sulfur, and then Selenium.
04

Compare electron affinities

Oxygen has higher electron affinity than Sulfur, and Sulfur has higher electron affinity than Selenium. Thus, the order is \ \( \text{Se} < \text{S} < \text{O} \).
05

Verify with options

Option (1) \ \( \text{Se} < \text{S} < \text{O} \) matches the order derived from periodic trends.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

periodic trends
Periodic trends refer to patterns in the properties of elements across different periods and groups in the periodic table. One important periodic trend is electron affinity, which typically increases across a period and decreases down a group. This occurs because atoms get smaller and nuclear charge increases as you move across a period, making it more energetically favorable to add an electron. Conversely, as you move down a group, atoms get larger and the added electron feels less attraction to the nucleus, resulting in lower electron affinity.
group 16 elements
Group 16 elements, also known as the chalcogens, include Oxygen (O), Sulfur (S), Selenium (Se), Tellurium (Te), and Polonium (Po). These elements share common properties due to their similar electron configurations.
  • Oxygen is the most electronegative and has the highest electron affinity in the group.
  • Moving down the group, the size of the atoms increases and electron affinity generally decreases.
  • For the elements in question, Oxygen has the highest electron affinity, followed by Sulfur, and then Selenium.
This trend informs us about their reactivity and ability to form anions.
chemical periodicity
Chemical periodicity is the recurring pattern in the properties of elements revealed in the periodic table. It helps us predict how elements will behave based on their position in the table. Elements in the same group often exhibit similar chemical behaviors due to having the same number of valence electrons. For instance, in Group 16:
  • All elements tend to form -2 anions.
  • They show a decrease in electron affinity as you move down the group.
  • Electron affinity is a key factor in determining how elements interact with others, affecting their chemical reactivity and the types of bonds they form.
Understanding these patterns allows us to predict properties and behaviors of elements not only in isolation but also in compound formation.

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Most popular questions from this chapter

The valency shell of an clement \(\Lambda\) contains 3 electrons while the valence shell of another clement \(B\) contains 6 electrons. If \(\Lambda\) combines with \(\mathrm{B}\), the probable formula of the compound formed will be (1) \(\Lambda \mathrm{B}_{2}\) (2) \(\Lambda_{2} B\) (3) \(\mathrm{A}_{2} \mathrm{~B}_{3}\) (4) \(\Lambda_{3} B_{2}\)

The statement that is not correct for the periodic classification of elements is (1) The properties of elements are the periodic functions of their outer electronic configurations. (2) Non-metallic elements arc lesser in number than metallic elements. (3) For transition elements the d-subshells are filled with electrons monotonically with increase in atomic number. (4) In the periodic table metallic elements appear in the right-hand columns.

Among the following pairs of atomic numbers, the pair which belongs to \(p\) -block is (1) 8,16 (2) 4,8 (3) 6,12 (4) 12,24

\(\mathrm{IP}_{2}\) for an clement is invariably higher than \(\mathrm{IP}_{\mathrm{L}}\) because (1) The size of cation is smaller than its atom. (2) It is difficult to remove electron from cation. (3) Effective nuclear charge is more for cation. (4) All

Among the following elements the configuration having highest ionisation energy is (1) \(|\mathrm{Ne}| 3 \mathrm{~s}^{2} 3 \mathrm{p}^{\prime}\) (2) \(|\mathrm{Ne}| 3 \mathrm{~s}^{2} 3 \mathrm{p}^{3}\) (3) \(|\mathrm{Ne}| 3 \mathrm{~s}^{2} 3 \mathrm{p}^{2}\) (4) \(|\mathrm{Ar}| 3 \mathrm{~d}^{10} 4 \mathrm{~s}^{2} 4 \mathrm{p}^{3}\)

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