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fewer or more than eight electrons. Compounds in which an atom has fewer than eight valence electrons ; 28. Compounds in which an atom has more than eight valence electrons ; Generally, if a nonmetal is in the third period or greater it can accommodate as many as twelve electrons, if it is the central atom. These elements have unfilled d ...

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Chapter10 Tro. 4. Based on the Lewis structure, the number of electron domains in the valence shell of the CO molecule is A) 1 B) 2 C) 3 D) 4 E) 5. Chapter10 Tro 1. All of the geometries listed below are examples of the five basic geometries for molecules with more than 3 atoms except A) planar triangular B) octahedral C) tetrahedral D) trihedral

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May 21, 2008 · Other atoms can expand their valence shells also; in fact, any element that contains d electrons can theoretically "expand" its valence shell. It all depends on the circumstances under which bonding occurs. I hope that helps. Good luck! *EDIT: Man, that's the second mistake I've made in two days. I originally said that sulfur has d orbitals in ...

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The third violation to the octet rule is found in those compounds with more than eight electrons assigned to their valence shell. These are called expanded valence shell molecules.Such compounds are formed only by central atoms in the third row of the periodic table or beyond that have empty d orbitals in their valence shells that can participate in covalent bonding.

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Group IVA elements: C, Si, Ge, having 4 electrons in the valence shell as shown in Figure below form compounds by sharing electrons with other elements without forming ions. This shared electron bonding is known as covalent bonding. Note that the center atom (and the others by extension) has completed its valence shell by sharing electrons.

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18 The construction of a Lewis structure with the octet rule (max. eight valence electrons near a nucleus) strictly applying to the elements C, N, O and F 19 Elements in periods 3-5 can accommodate more than eight valence electrons near the nucleus Second (level) period (quantum number n= 2) consist 16 elements, eight in shell ns = 3 (M - 2p,3s) and eight in shell ns = 4 (N - 3p,3s), elements from 5.Boron to element 20.Calcium. As we can see, until element with number 20.Calcium, there is no shell or sub shell with mark 3d .

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