The electron configuration of copper is 1s22s22p63s23p63d104s1.
The electron configuration of copper(II) is [Ar] 3d9 . Copper is [Ar] 3d10 4s1
The electron configuration of rutherfordium is: [Rn] 5f14 6d2 7s2.
The outer electron configuration of an alkali metal is one electron in the s subshell. This electron is easily lost to form a cation with a full valence shell, resulting in the high reactivity of alkali metals.
The electron configuration of Cu+1 is [Ar] 3d10 4s1. When copper loses one electron to become a +1 ion, it loses the 4s electron first, followed by one of the 3d electrons to attain a stable electron configuration.
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 electron configuration for copper is Ar 3d10 4s1.
The electron configuration of copper is Ar 3d10 4s1.
The condensed electron configuration for copper is Ar 3d10 4s1.
The electron configuration of copper (Cu) is Ar 3d10 4s1.
Because copper loose electron from its penultimate outer shell
The electron configuration of copper(II) is [Ar] 3d9 . Copper is [Ar] 3d10 4s1
The electron configuration of a Copper(II)ion is [Ar]4s0 3d9.
The electron configuration of copper is: [Ar]4s13d10. It isn't 4s23d9 because Cu is able to obtain a more stable electron configuration when it takes an electron from the 4s and adds it to 3d. A half filled 4s and a completely filled 3d is more stable.
halogens
The complete electron configuration for the copper atom is 1s2 2s2 2p6 3s2 3p6 4s1 3d10.
The outer electron configuration for oxygen is 2s^2 2p^4. This means that oxygen has 6 outer electrons in its valence shell.
The outer electron configuration for germanium is 4s^2 4p^2. Germanium has 4 valence electrons in the outermost shell.