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Hey there! Some molecules can accommodate more than 8 valence electrons because they have expanded valence shells. These molecules are from periods 3 or higher because starting from n=3, atoms have d-orbitals that can accommodate for more that 9 valence electrons.

The electron configuration can be visualized as the core electrons, equivalent to the noble gas of the preceding period, and the valence electrons: each element in a period differs only by the last few subshells. Phosphorus, for instance, is in the third period.
A radioactive actinide metal, neptunium is the first transuranic element. Its position in the periodic table just after uranium, named after the planet Uranus, led to it being named after Neptune, the next planet beyond Uranus. A neptunium atom has 93 protons and 93 electrons, of which seven are valence electrons.
The next orbital we will examine is more complicated than the s orbital, it is known as the p orbital. p orbitals can have three possible orientations each of which is perpendicular to the two others in three-dimensional space (Figure 2), and each of the p orbitals can contain a maximum of two electrons, for a total of six electrons.
Atoms with more than ten electrons require more than two shells. These elements occupy the third and subsequent rows of the periodic table. The factor that most strongly governs the tendency of an atom to participate in chemical reactions is the number of electrons in its valence shell. A valence shell is an atom's outermost electron shell ...
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2. Beryllium = 2 Valence Electrons 3. Elements in period 3 can occupy more than 8 valence electrons (e.g. Phosphorus and Sulfur) f. So if carbon has four electrons it may accommodate four more electrons i. How can it do so? It may gain four more bonds 1. One bond = 2 electrons 2. Carbon “takes on” one of those electrons from a given bond ...
• Lewis (electron dot) structures show all the valence electrons of the atoms in the molecule or polyatomic ion. • The octet rule refers to the fact that most atoms form a stable arrangement with eight electrons in their outer shell. • Exceptions to the octet rule include: less than an octet – BeCl2, BF3 (central atom very small)
Jul 19, 2017 · The original and often quoted definition of the term relates to a molecule that contains one or more main group elements formally bearing more than eight electrons in their valence shell. One well-known example dating from 1992 of a molecule to which the term hypervalent was applied is CLi 6 [3] , where the description carbon can expand its ...
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  • Draw a Lewis structure for ClO4- and determine the formal charge on chlorine, which obeys the octet rule. a. +1 b. +2 c. +3 d. 0 e. +4
  • A second shell is necessary to hold the electrons in all elements larger than hydrogen and helium. Lithium (Li), whose atomic number is 3, has three electrons. Two of these fill the first electron shell, and the third spills over into a second shell. The second electron shell can accommodate as many as eight electrons.
  • Q. Why do the other elements form trications? A. Because they have the valence electronic configuration ns2np1 and when three electrons are lost they have a full valence shell. The metals however can also form covalent compounds with non-metals depending on the difference in electronegativity.
  • Question: Which Element Can Accommodate More Than Eight Electrons In Its Valence Shell? Which Element Can Accommodate More Than Eight Electrons In Its Valence Shell? He O C P
  • An atom like phosphorus or sulfur which has more than an octet is said to have expanded its valence shell. This can only occur when the valence shell has enough orbitals to accommodate the extra electrons. For example, in the case of phosphorus, the valence shell has a principal

A revised MRCI-algorithm coupled to an effective valence-shell Hamiltonian. II. Application to the valence excitations of butadiene. NASA Astrophysics Data System (ADS) Strodel, Paul; Tavan, Paul. 2002-09-01. In Paper I of this work we have sketched an improved MRCI algorithm and its coupling to the effective valence-shell Hamiltonian OM2.

SiO32⁻ > CO32⁻ > CO2 6) Which element can expand its valence shell to accommodate more than eight electrons? a. N b. O c. Br d. He 7) How many lone pairs of electrons are on the S atom in SF 4? a. 0 b. 1 c. 2 d. 3 8) Use the bond energies provided to estimate ΔH° rxn for the reaction below. C2H4(g) + H2(g) → C2H6(g) ΔH° rxn =? Dative covalent (coordinate) bond can be formed. 3. Molecules / Ions where the central atom has more than an octet (8) of valence e-s Elements in 3rd and higher periods have ns and np and unfilled nd orbitals that can be used for bonding. e.g. PCl 5 have to expand valence shell to place 10 e-s around central phosphorus atom.
The second energy level can accommodate a maximum of eight electrons. Although the third and outer shells can each contain more than eight electrons, they are most stable when only eight are present. We may consider the first shell complete when it contains two electrons and every other shell complete when it contains eight electrons. Dec 31, 2012 · It is true that maximum number of electrons is given by the formula 2n^2 ,but it is a fact that maximum number of electrons in the last (valence) shell of an element is always 8. The atom with 8 electrons in its outermost shell is said to be the most stable one.

octet rule: A rule stating that atoms lose, gain, or share electrons in order to have a full valence shell of 8 electrons. (Hydrogen is excluded because it can hold a maximum of 2 electrons in its valence shell.

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Jun 22, 2011 · to break it down, so you can understand why, look at the periodic table, in the fourth period you're gonna have s,p,d, and f orbitals. the max amount of electrons that can occupy each subshell is: s=2 e p=6 e d=10 e f=14 e EDIT: wow. 3 people just posted the same thing at the same time lol