Silicon has an atomic number of 14 and it is in period 3 and in group XIV and is a p-block element. Thus, it has 4 valence electrons in the 3p orbital. Its electron configuration is
1s2 2s2 2p6 3s2 3p2
4 electrons in the outer shell 2-8-4 electron configuration :D
The electron configuration of silicon is 1s2 2s2 2p6 3s2 3p2. You can represent this in shorthand notation by writing [Ne] 3s2 3p2, which indicates that silicon's configuration is the same as neon's configuration followed by the outermost electron sublevels of 3s2 3p2.
Phosphorus has more outer electrons than silicon. Phosphorus has 5 outer electrons (in group 15), while silicon has 4 outer electrons (in group 14) in its electronic configuration.
Silicon gains electrons to achieve a stable electron configuration, as it has four valence electrons and tends to form covalent bonds by sharing electrons with other atoms.
The element with the electron configuration of 1s2 2s2 2p6 3s2 3p2 is Silicon (Si).
Krypton (Kr) has the same electron configuration as silicon, which is [Ne]3s^23p^2.
Silicon has 14 electrons. The electron configuration for silicon is 1s^2 2s^2 2p^6 3s^2 3p^2.
Silicon has 14 electrons in the following orbital configuration 1s2 2s2 2p6 3s2 3p2, when neutral in charge.
The element with the electron configuration Ne3s^23p^4 is sulfur.
4 electrons in the outer shell 2-8-4 electron configuration :D
The electron configuration of silicon is 1s2 2s2 2p6 3s2 3p2. You can represent this in shorthand notation by writing [Ne] 3s2 3p2, which indicates that silicon's configuration is the same as neon's configuration followed by the outermost electron sublevels of 3s2 3p2.
Phosphorus has more outer electrons than silicon. Phosphorus has 5 outer electrons (in group 15), while silicon has 4 outer electrons (in group 14) in its electronic configuration.
Silicon gains electrons to achieve a stable electron configuration, as it has four valence electrons and tends to form covalent bonds by sharing electrons with other atoms.
Silicon will tend to gain electrons in order to achieve a stable outer electron configuration, as it has 4 valence electrons and typically forms covalent bonds with other elements by sharing electrons.
The noble gas configuration of silicon is [Ne] 3s^2 3p^2, where [Ne] represents the electron configuration of the noble gas neon. Silicon has 14 electrons, with two in the 3s orbital and two in the 3p orbital.
In silicon, an atom can either gain 4 electrons to achieve a stable electron configuration with 8 valence electrons (like the noble gas argon) or lose 4 electrons to achieve a stable configuration with 4 valence electrons (like the noble gas neon). Silicon typically forms covalent bonds by sharing electrons rather than losing or gaining them.
The element with the electron configuration of 1s2 2s2 2p6 3s2 3p2 is Silicon (Si).