Question

Which one of the following is a correct electronic configuration of Ne atom ?

• A. 2,8
• B. 2,7
• C. 2,6
• D. 2,5

Hint:

Remember the maximum number of electrons each shell can hold (2 for K, 8 for L, 18 for M, etc.). For noble gases like Neon, their outermost shell is completely filled, which is why they are stable and unreactive.

Answer 1

The Correct Option is A

Step 1: Identify the element and its atomic number.
The element is Ne, which stands for Neon.
Neon (Ne) is an element in Group 18 of the periodic table, which are the noble gases.
The atomic number of Neon (Ne) is 10. The atomic number represents the total number of electrons in a neutral atom. Step 2: Determine the electronic configuration based on the atomic number.
The electrons in an atom fill electron shells in a specific order:
The first shell (K shell) can hold a maximum of 2 electrons.
The second shell (L shell) can hold a maximum of 8 electrons.
The third shell (M shell) can hold a maximum of 18 electrons, and so on. For a neutral Neon atom with 10 electrons:
The first shell will be completely filled with 2 electrons.
The remaining electrons ($10 - 2 = 8$) will go into the second shell.
The second shell will be completely filled with 8 electrons. Therefore, the electronic configuration of Neon is 2, 8. Step 3: Compare the derived configuration with the given options.
(1) 2,8: This matches the derived electronic configuration.
(2) 2,7: This configuration has a total of 9 electrons, corresponding to Fluorine (F).
(3) 2,6: This configuration has a total of 8 electrons, corresponding to Oxygen (O).
(4) 2,5: This configuration has a total of 7 electrons, corresponding to Nitrogen (N). Step 4: Conclude the correct electronic configuration.
The correct electronic configuration for a Neon (Ne) atom is 2,8. $$(1) 2,8$$