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
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.
Potassium can lose one electron from its outer shell to achieve a stable electron configuration similar to argon. Fluorine can gain one electron to fill its outer shell and attain a stable electron configuration like neon. In both cases, the atoms are trying to achieve a full valence shell and become stable like the nearest noble gas.
The atomic number of potassium is 19. This means that potassium atoms have 19 protons in their nuclei. Neutral potassium atoms will also have 19 electrons. So then you follow the rules for the orbital filling pattern for the atoms of the elements, until you get to 19 electrons, and you get the following: 1s22s22p63s23p64s1.
Potassium loses one electron. All Alkali metals lose one electron.
No, potassium does not have a noble gas electron configuration. The noble gas configuration for potassium would be [Ar] 4s¹, but instead, potassium has the electron configuration 1s² 2s² 2p^6 3s² 3p^6 4s¹.
The electron configuration for a potassium ion (K+) is [Ar] 4s1. Potassium loses one electron to form the +1 ion, resulting in a noble gas configuration like argon.
Argon has the same electron configuration as a potassium ion, as both species have 18 electrons with the electron configuration of [Ne]3s²3p⁶.
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.
Potassium is an electron donor. It donates one electron to achieve a more stable electron configuration.
The shell configuration of potassium is 2,8,8,1.
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.
The electron configuration for a neutral potassium atom is 1s2 2s2 2p6 3s2 3p6 4s1. This configuration represents the arrangement of electrons in the energy levels around the nucleus of the potassium atom.
[Ar]4s1 Or 4n Or s-orbital (I don't know exactly what you're asking)
The electron configuration for a ground-state potassium atom is 1s22s22p63s23p64s1. The noble gas shorthand configuration is [Ar]4s1.
The noble gas configuration for potassium is [Ar] 4s^1. To form a cation, potassium would lose its one valence electron, resulting in a 1+ ion. Therefore, the ion formed when potassium achieves a noble gas electron configuration is K^+.
1s2, 2s2, 2p6, 3s2, 3p6, 4s1, or [Ar] 4s1.