The other members of group 8 have a characteristic valence shell electron octet (ns 2 + np x 2 + np y 2 + np z 2). This group of inert (or noble) gases also includes krypton (Kr: 4s 2, 4p 6), xenon (Xe: 5s 2, 5p 6) and radon (Rn: 6s 2, 6p 6). In the periodic table above these elements are colored beige.
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These atoms have only one electron in the valence shell, and on losing this electron arrive at the lower shell valence octet. As a consequence of this electron loss, these elements are commonly encountered as cations (positively charged atoms).
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I believe the ground state electron configuration of Na is: 1s2 2s2 2p6 3s1. Na+ means that the atom has lost an electron would the config then be:
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(x, y & z). As we progress from lithium (atomic number=3) to neon (atomic number=10) across the second row or period of the table, all these atoms start with a filled 1s-orbital, and the 2s-orbital is occupied with an electron pair before the 2p-orbitals are filled.
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Best Answer: Sodium 1s2 2s2 2p6 3s1 Iron 1s2 2s2 2p6 3s2 3p6 3d6 4s2 I can't give colbalt as it doesn't exist ..
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The highest occupied electron shell is called the valence shell, and the electrons occupying this shell are called valence electrons. The chemical properties of the elements reflect their electron configurations. For example, helium, neon and argon are exceptionally stable and unreactive monoatomic gases.
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Transfer of the lone 3s electron of a sodium atom to the half-filled 3p orbital of a chlorine atom generates a sodium cation (neon valence shell) and a chloride anion (argon valence shell). Electrostatic attraction results in these oppositely charged ions packing together in a lattice.
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what is the full electron configuration of sodium
The full electron configuration of sodium is 1s22s22p63s1.