select the correct electron configurations from the list below. you can refer to the periodic table for atomic numbers. check all that apply. check all that apply.
the electron configuration of s2− is [ne]3s23p6.
the electron configuration of ag+ is [kr]5s14d9.
the electron configuration of ni is [ar]4s23d8.
the electron configuration of rb is [kr]5s04d1.
the electron configuration of si is [ne]3s23p2.

Ni = [Ar] 4s² 3d⁸

S²⁻ = [Ne] 3s² 3p⁶

Si = [Ne] 3s² 3p²

Explanation:

Correct options.

Ni = [Ar] 4s² 3d⁸

The atomic number of nickel is 28. Orbitals are correctly filled with 28 electrons. That's why it is correct electronic configuration.

S²⁻ = [Ne] 3s² 3p⁶

it is correct because atomic number of sulphur is 16 and two electrons are present because of 2- charge so that's why 6 electrons are present in 3p⁶.

Si = [Ne] 3s² 3p²

it is correct electronic configuration.

Other options:

Ag⁺ = [Kr] 5s¹ 4d⁹

It is incorrect electronic configuration because electron cannot remove from the 4d¹⁰ because it is stable. The one electron must be removed from 5s¹.

Rb = [Kr] 5s⁰ 4d¹

The correct electronic configuration is [Kr] 5s¹.

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally