Noble gases have completely filled valence electrons. so removla of electrons will make them unstable
Silicon has 4 valence electrons. No noble gases will have 4 valence electrons.
Calcium loses two electrons to obtain a noble-gas electron configuration.
Fr is in the 1st period. It removes an electron to get noble gas configuration. Fr+ does not have valence electrons.Francium has 1 electron in its outermost energy level. It donates its outermost electron to stabilize its electron configuration. Francium(I) has no valence electrons.
The valence electron shell of noble gases id completely filled; as a consequence the affinity for electrons and the chemical reactivity are at an extremely low level.
They have one valence electron. If this electron is lost, the atoms form cations with the electronic configuration of the nearest noble gas.
Silicon has 4 valence electrons. No noble gases will have 4 valence electrons.
Valence electrons are the outer layer of electrons, the part that reacts. Argon is a noble gas, so it has a full valence electron level. It has eight valence electrons.
Noble gases have atoms with the valence electron shell filled.
Calcium loses two electrons to obtain a noble-gas electron configuration.
Because helium has completely filled valence orbitals similar to other noble gases.
Fr is in the 1st period. It removes an electron to get noble gas configuration. Fr+ does not have valence electrons.Francium has 1 electron in its outermost energy level. It donates its outermost electron to stabilize its electron configuration. Francium(I) has no valence electrons.
They all have a full set of valence electrons.
The valence electron shell of noble gases id completely filled; as a consequence the affinity for electrons and the chemical reactivity are at an extremely low level.
They have one valence electron. If this electron is lost, the atoms form cations with the electronic configuration of the nearest noble gas.
The ionization energy increases because the energy required to remove a valence electron will increase. The atoms want to keep their valence electrons because as you move more towards the right of the Periodic Table towards the noble gases. To write an abbreviation for electron configuration, it requires a noble gas and the valence electron configuration.
They have completely filled shells, with eight valence electrons.
S2- ion: [Ne]3s23p6