Home
Class 11
CHEMISTRY
Which of the following electronic config...

Which of the following electronic configurations has the lowest value of ionisation energy? Explain.
a. `1s^(2) 2s^(2)2p^(6)`
b. `1s^(2) 2s^(2)2p^(5)`
c. `1s^(2) 2s^(2)2p^(6) 3s^(1)`

Text Solution

AI Generated Solution

To determine which electronic configuration has the lowest value of ionization energy, we need to analyze each option provided. ### Step 1: Analyze the configurations 1. **Option a: `1s^(2) 2s^(2) 2p^(6)`** - This configuration represents a noble gas (Neon). Noble gases have completely filled outer shells, which makes them very stable. The ionization energy for noble gases is typically very high because it requires a significant amount of energy to remove an electron from a stable configuration. 2. **Option b: `1s^(2) 2s^(2) 2p^(5)`** ...
Promotional Banner

Topper's Solved these Questions

  • PERIODIC CLASSIFICATION OF ELEMENTS AND GENERAL INORGANIC CHEMISTRY

    CENGAGE CHEMISTRY|Exercise Solved Examples|34 Videos

  • PERIODIC CLASSIFICATION OF ELEMENTS AND GENERAL INORGANIC CHEMISTRY

    CENGAGE CHEMISTRY|Exercise Ex 1.1|14 Videos

  • P-BLOCK GROUP 14 - CARBON FAMILY

    CENGAGE CHEMISTRY|Exercise Exercises Archives (Subjective)|9 Videos

  • PURIFICATION OF ORGANIC COMPOUNDS AND QUALITATIVE AND QUANTITATIVE ANALYSIS

    CENGAGE CHEMISTRY|Exercise Assertion Reasoning Type|5 Videos

Similar Questions

Explore conceptually related problems

Q .Which of the following electron configurations is correct for nickel (atomic number "28" )? a) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(1)3d^(9) (b) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(8) (c) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(0)3d^(10)

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) Which of the electronic configurations given above would you expect to have the lowest ionization enthalpy?

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) Which of the electronic configuration given above would you expect for the noble gas?

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) List the above configurations in order of increasing ionization enthalpy.

Elements with their electronic configurations are given below: Answer the following questions: (I) 1s^(2) 2s^2 (II) 1s^(2) 2s^(2) 2p^(6) (III) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (IV) 1s^(2) 2s^(2) 2p^(3) (V) 1s^(2) 2s^(2) 2p^(5) The element with lowest value of electron affinity is:

Elements with their electronic configurations are given below: Answer the following questions: (I) 1s^(2) 2s^2 (II) 1s^(2) 2s^(2) 2p^(6) (III) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (IV) 1s^(2) 2s^(2) 2p^(3) (V) 1s^(2) 2s^(2) 2p^(5) The element with highest I.E. is: