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Along the period (rarr) atomic//ionic ra...

Along the period `(rarr)` atomic`//`ionic radii and metallic character decreases while `IE`, `EN` , non-metallic character and oxidising
power increases. Down the group `(darr)`, atomic`//`ionic radii, metallic character and reducing character increase while `IE` and `EN`
decrease. However, `Delta_(eg)H^(ɵ)` becomes less negative down a group
but more negative along a period.
Which of the following isoelectronic species has lowest `IE_(1)` ?

A

`K^(o+)`

B

`Ca^(2+)`

C

`S^(2-)`

D

`Cl^(ɵ)`

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding which isoelectronic species has the lowest first ionization energy (IE₁), we will follow these steps: ### Step-by-Step Solution: 1. **Identify the Isoelectronic Species**: The given isoelectronic species are K⁺, Ca²⁺, S²⁻, and Cl⁻. Isoelectronic species have the same number of electrons. 2. **Determine the Number of Electrons**: - K⁺ (Potassium ion): Atomic number = 19, loses 1 electron → 18 electrons. - Ca²⁺ (Calcium ion): Atomic number = 20, loses 2 electrons → 18 electrons. - S²⁻ (Sulfide ion): Atomic number = 16, gains 2 electrons → 18 electrons. - Cl⁻ (Chloride ion): Atomic number = 17, gains 1 electron → 18 electrons. All species have 18 electrons. 3. **Count the Number of Protons**: - K⁺: 19 protons - Ca²⁺: 20 protons - S²⁻: 16 protons - Cl⁻: 17 protons 4. **Analyze the Relationship Between Protons and Ionization Energy**: Ionization energy is influenced by the effective nuclear charge, which is the net positive charge experienced by an electron in a multi-electron atom. The more protons present, the higher the effective nuclear charge, and thus, the higher the ionization energy. 5. **Determine Which Species Has the Lowest Ionization Energy**: Since S²⁻ has the least number of protons (16), it will have the lowest effective nuclear charge. This means that the electrons in S²⁻ will be held less tightly compared to the other species, making it easier to remove an electron. 6. **Conclusion**: Therefore, the isoelectronic species with the lowest first ionization energy (IE₁) is S²⁻. ### Final Answer: **S²⁻ has the lowest ionization energy (IE₁).** ---
To solve the question regarding which isoelectronic species has the lowest first ionization energy (IE₁), we will follow these steps: ### Step-by-Step Solution: 1. **Identify the Isoelectronic Species**: The given isoelectronic species are K⁺, Ca²⁺, S²⁻, and Cl⁻. Isoelectronic species have the same number of electrons. 2. **Determine the Number of Electrons**: ...
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