First, you have to look at the noble gas on the row above potassium, [Ar] then you have to write the shorthand electron configuration which would be simply 1s1. Your final answer would be [Ar]1s1
1s2, 2s2, 2p6, 3s2, 3p6, 4s1, or [Ar] 4s1.
Potassium, K, atom number 19, has an electron configuration in 4 shells
(K,L,M,N) = 2, 8, 8, 1
1s2 2s2 2p6 3s2 3p6 4s1
K+ is 18 electrons 1s2 2s2 2p6 3s2 3p6
[Ar] 4s1
or
2, 8, 8, 1
[Ar]4s1
Potassium must lose one electron (to have the same configuration as the noble gas argon), and fluorine must gain one electron (to have the same configuration as neon)
The electron configuration for a ground-state potassium atom is 1s22s22p63s23p64s1. The noble gas shorthand configuration is [Ar]4s1.
There is only one valance electron in potassium.
Selenium: [Ar] 3d10 4s2 4p4 or 2, 8, 18, 6 Phosphorus: [Ar] 3d10 4s2 4p3 or 2, 8, 18, 5
1 electron in the s orbital
The shell configuration of potassium is 2,8,8,1.
No - but the potassium ion does
19K+=1s2,2s2,2p6,3s2,3p6,3d1
Ar is Argon and Ar 4s1 is the short form of the electron configuration 1s2 2s2 2s6 3s2 3s6 4s1. It means add 4s1 to the electron configuration of Argon to get the electron configuration of potassium.
Potassium must lose one electron (to have the same configuration as the noble gas argon), and fluorine must gain one electron (to have the same configuration as neon)
The electron configuration for a ground-state potassium atom is 1s22s22p63s23p64s1. The noble gas shorthand configuration is [Ar]4s1.
Sulfur (S) has the electron configuration 1s22s22p63s23p4.
The electron configuration of 1s22s22p3s1 is not the ground state electron configuration of any element. This configuration contains 8 electrons, which in the ground state would be oxygen. The ground state configuration of oxygen is 1s22s22p4.
There is only one valance electron in potassium.
Potassium.
argon atom
The element with that electron configuration is Iron.