Two orbitals.
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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.
That would be 1s2, 2s2, 2p6 are the 3 orbitals that are completely filled. The other one is not filled because it only has 1 configuration. Hopefully this help....if not I apologize. *PUMA #4*
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.
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
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Nitrogen (N) is atomic number 7, so has 7 electrons in the ground state. The configuration is1s2 2s2 2p3. From this, one can see that the 1s is full, as is the 2s. So, the number of completely filled orbitals is TWO.
Neon has completely filled orbitals, has stable electron configuration and hence neon atoms do not bind / join with each other.
because they have completely filled orbitals
In general, you use the Aufbau Principle which indicates the order in which the shells and orbitals are filled. You just have to learn it and then you can determine the electron configuration of the elements.
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.
That would be 1s2, 2s2, 2p6 are the 3 orbitals that are completely filled. The other one is not filled because it only has 1 configuration. Hopefully this help....if not I apologize. *PUMA #4*
Helium has completely filled orbitals and is hence chemically inert.
Argon has completely filled valence orbitals and hence is unreactive. Sodium has one valence electron. If sodium loses this electron it will attain the stable electron configuration of the nearest noble gas (argon) and hence is reactive.
Xenon has five electron shells.
Noble gases have completely filled orbitals / energy levels. They generally have 8 valence electrons (helium has only 2) and have stable electronic configuration.
Helium's atomic number is 2 because it has 2 protons in its nucleus.