Electron configuration for silver ion

Answer 1

Ag 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

or simply,

[Kr] 5s1 4d10
The atomic number of silver is 47, which it means it has 47 protons. A neutral silver atom will also have 47 electrons. Its electron configuration is [Kr]4d105s1.

Answer 2

Ag 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

or simply,

[Kr] 5s1 4d10
The atomic number of silver is 47, which it means it has 47 protons. A neutral silver atom will also have 47 electrons. Its electron configuration is [Kr]4d105s1.

Answer 3

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10 that's for silver

simplified to [Kr] 5s1 4d10

The down electron from the 5s moves to fill the d orbitals because it is more stable there.

a+1 ion (silver's only oxidation state) would be [Kr] 4d10

Outer orbitals are always removed first, so you cannot start to remove the 4d electrons until all of the 5s are gone.

Answer 4

The chemical element, silver, is in group 11, period 5. Thus, its electron configuration is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s1 4d10. This can be written shorter as [Kr] 4d10 5s1 since krypton's electron configuration is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6.

Answer 5

The atomic number of silver is 47, which it means it has 47 protons. A neutral silver atom will also have 47 electrons. Its electron configuration is [Kr]4d105s1.

Answer 6

Ag(long): 1s22s22p63s23p64s23d104p65s14d10 Ag(short): [Kr]5s14d10 notice that one electron from 5s is promoted to 4d because full and half-full subshells offer extra stability.