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Question 1: 2nd electron affinity for halogens is zero – explain.
Solution: After addition of one electron in halogen atom formation of halide ion takes place which has fully filled configuration (ns2np6) and thus possesses no tendency to gain one more electron.
Question 2: NaOH behaves as a base while Zn(OH)2 is amphoteric why?
Solution: In NaOH the bond electronegativity difference between Na and oxygen is greater than between H and O and therefore it is the Na–O bond that breaks releasing OH–. But in case of Zn—O—H bond the difference of electronegativity of Zn—O and O—H are almost same. So there is equal probability that the bond breaks in both ways leading to an amphoteric behavior.
Question 3: Why does xenon react with fluorine whereas neon does not?
Solution: Xe has lower ionisation energy than Ne. The valence electrons in Xe (n = 5) are much farther from the nucleus than those of Ne (n=2) and much less tightly held by the nucleus; they are more willing to be shared that those in neon. Also xenon has empty 5d orbital which can help to accommodate the bonding pairs of electrons, while neon has all the valence orbitals filled.
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FAQs on Solved Examples: Classification of Elements & Periodicity in Properties - Mock Tests for JEE Main and Advanced 2025
| 1. What are the main groups or categories of elements in the periodic table? |  |
Ans. The main groups or categories of elements in the periodic table are metals, nonmetals, and metalloids. Metals are generally shiny, conductive, and malleable, while nonmetals are typically dull, non-conductive, and brittle. Metalloids have properties that are intermediate between metals and nonmetals.
| 2. How are elements classified based on their electronic configurations? | |
Ans. Elements are classified into periods and groups based on their electronic configurations. Periods are horizontal rows in the periodic table, and they represent the number of electron shells an element's atoms have. Groups are vertical columns, and they represent elements with similar valence electron configurations.
| 3. What is the significance of the periodic law in classifying elements? | |
Ans. The periodic law states that the properties of elements are periodic functions of their atomic numbers. This law provides a basis for classifying elements in the periodic table. Elements with similar properties are grouped together, and their properties change in a repetitive manner as you move across periods and down groups.
| 4. How does periodicity in properties of elements occur? | |
Ans. Periodicity in properties of elements occurs because of the recurring patterns in the arrangement of electrons in the atom. The number of electron shells and the distribution of electrons within those shells determine an element's properties. As you move across periods, the number of valence electrons increases, leading to similar chemical behavior. Moving down groups, the number of electron shells increases, resulting in similar chemical behavior within a group.
| 5. Why do elements in the same group have similar chemical properties? | |
Ans. Elements in the same group have similar chemical properties because they have the same number of valence electrons. Valence electrons are responsible for an element's chemical reactivity and bonding behavior. Elements in the same group have the same valence electron configuration, which leads to similar chemical behavior and the ability to form similar types of compounds.
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