Respuesta :
Option :
A will give up electrons to form bonds.
B will give up electrons to form bonds.
C. Both A and B will be chemically unreactive.
D. Both A and B will gain electrons to become stable.
Further explanation
In an atom there are levels of energy in the shell and sub shell
This energy level is expressed in the form of electron configurations.
The electron configurations for atoms A :
1s²2s²2p⁶
The electron configurations for atoms B :
1s²2s²2p⁶3s²3p⁶
If we look at the configuration of these two atoms, they both show the same number of valence atoms, which is 8, and the last orbital (p orbital) is fully filled, so that both atoms are stable (don't want to achieve stability by binding or removing electrons)
Because these two atoms are stable, it becomes difficult for them to react to form bonds
So C. Both A and B will be chemically unreactive.
The atoms are stable and the octet is complete, thus both the elements are chemically unreactive. Thus statement 3 is correct.
The complete question has options as:
- A will give up electrons to form bonds.
- B will give up electrons to form bonds.
- Both A and B will be chemically unreactive.
- Both A and B will gain electrons to become stable.
The number of electrons in an A atom is 10. The electronic configuration will be:
2, 8
The number of electrons in the B atom is 18. The electronic configuration will be:
2, 8, 8
Both the atoms have completely filled orbitals. They will neither take electrons nor give electrons. Thus options 1, 2, and 4 are incorrect.
The atoms are stable and the octet is complete, thus both the elements are chemically unreactive. Thus statement 3 is correct.
For more information about the electrons in an atom, refer to the link:
https://brainly.com/question/19042048
