the number of electrons in the m shell of silicon is 4.
the number of electrons in the m shell of silicon is 4.
number of electrons in the m shell of silicon?
4
tetrahedral coordination is a major structural motif in silicon chemistry just as it is for carbon chemistry. however, the 3p subshell is rather more diffuse than the 2p subshell and does not hybridise so well with the 3s subshell. as a result, the chemistry of silicon and its heavier congeners shows significant differences from that of carbon, and thus octahedral coordination is also significant. for example, the [[electronegativity]] of silicon (1.90) is much less than that of carbon (2.55), because the valence electrons of silicon are further from the nucleus than those of carbon and hence experience smaller electrostatic forces of attraction from the nucleus. the poor overlap of 3p orbitals also results in a much lower tendency toward [[catenation]] (formation of si–si bonds) for silicon than for carbon, due to the concomitant weakening of the si–si bond compared to the c–c bond: the average si–si bond energy is approximately 226 kj/mol, compared to a value of 356 kj/mol for the c–c bond. this results in multiply bonded silicon compounds generally being much less stable than their carbon counterparts, an example of the [[double bond rule]]. on the other hand, the presence of 3d orbitals in the valence shell of silicon suggests the possibility of [[hypervalence]], as seen in five and six-coordinate derivatives of silicon such as and . lastly, because of the increasing energy gap between the valence s and p orbitals as the group is descended, the divalent state grows in importance from carbon to lead, so that a few unstable divalent compounds are known for silicon; this lowering of the main oxidation state, in tandem with increasing atomic radii, results in an increase of metallic character down the group. silicon already shows some incipient metallic behavior, particularly in the behavior of its oxide compounds and its reaction with acids as well as bases (though this takes some effort), and is hence often referred to as a [[metalloid]] rather than a nonmetal. however, metallicity does not become clear in group 14 until germanium and dominant until tin, with the growing importance of the lower +2 oxidation state.
silicon
each shell can contain only a fixed number of electrons: the first shell can hold up to two electrons, the second shell can hold up to eight (2 + 6) electrons, the third shell can hold up to 18 (2 + 6 + 10) and so on. the general formula is that the "n"th shell can in principle hold up to 2("n") electrons. since electrons are electrically attracted to the nucleus, an atom's electrons will generally occupy outer shells only if the more inner shells have already been completely filled by other electrons. however, this is not a strict requirement: atoms may have two or even three incomplete outer shells. (see madelung rule for more details.) for an explanation of why electrons exist in these shells see electron configuration.
electron shell