atomic orbitals and electron orbitals
The different orbitals are s orbitals, p orbitals, d orbitals, and f orbitals.
Argon has completely filled orbitals. It obeys octet rule (8 electrons in the valence orbitals / shells) and is stable and chemically inert
All p sublevels contain three orbitals, including the 4p sublevel.
The electron cloud is divided into s, p, d, and f orbitals. These orbitals also occur at different principle energy levels.
5 electrons in p orbitals in the outer shell. Cl has an electronic configuration of [Ne] 3s2, 3p5 In level 2 there a further 6 electrons in p orbitals making 11 electrons in total occupying p orbitals
The electronic configuration of silver is [Kr]4d105s1. If it loses 1 electron then it will have completely filled d orbitals as its valence orbitals and is stable. It will never attain the electronic configuration of noble gas.
hybridization is defined as the intermixing of different orbitals with different energies to form a new set of orbitals with equivalent energies and shapes
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Krypton is a noble gas and hence has stable electronic configuration. Its valence shell configuration is 4s2 4p6 . Therefore, it has 1-s and 3-p full orbitals in its valence shell.
Elements in the same vertical column or group have similar valence shell electronic configurations,the same number of electrons in the outer orbitals, and similar properties.
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Because the inner shell already has completely filled electronic configuration.