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What has more outer electrons phosphorus or silicon?
Phosphorus has more outer electrons than silicon. Phosphorus has 5 outer electrons (in group 15), while silicon has 4 outer electrons (in group 14) in its electronic configuration.
How many more electrons does silicon need in order to have a stable octet?
Silicon, like carbon, has four valance electrons, and needs another four to have a stable octet.
Why is there a large increase in ionic radius from silicon to phosphorus?
The increase in ionic radius from silicon to phosphorus is due to the addition of an extra electron in the outermost shell of the atom. This added electron increases the electron-electron repulsion forces, causing the electron cloud to expand and the ionic radius to increase.
Would an atom of phosphorus gain or lose electrons when ionized?
If phosphorus forms a monatomic ion, it gains electrons and form a phosphide ion. More commonly, however, phosphorus forms a polyatomic anion including one or more oxygen atoms. The bonds within these polyatomic anions are covalent, but phosphorus is considered to have a positive oxidation number in such anions, and positive oxidation number corresponds to losing electrons.
How many electrons must be gained for phosphorus to have a stable electron configuration?
Its outer shell needs 3 more electrons (because 2+3=5) you need 8 in order for the outer shell to become stable being that there is 5 on the outer shell already what plus 5 gives you 8 3 of course so that why you add 3.
What has more outer electrons phosphorus or silicon?
Phosphorus has more outer electrons than silicon. Phosphorus has 5 outer electrons (in group 15), while silicon has 4 outer electrons (in group 14) in its electronic configuration.
How many more electrons does phosphorus have than boron?
Phosphorus has 10 more electrons. A neutral atom of phosphorus has 15 electrons, 3 in the outer 3p shell There are 5 electrons in a neutral atom of boron, 1 in the outer 2p shell.
What is smaller chlorine sulfur silicon or phosphorus?
Chlorine is the smallest of those elements, followed by sulfur, silicon, and phosphorus. The size of an atom is determined by the number of protons and electrons it has, with more protons making the atom smaller.
Which elements most readily accepts electrons silicon or sulfur or chlorine or phosphorus?
Chlorine most readily accepts electrons among silicon, sulfur, chlorine, and phosphorus. Chlorine is a halogen and has a high electron affinity due to its high electronegativity, making it more likely to accept electrons to achieve a stable electron configuration. Silicon, sulfur, and phosphorus are nonmetals with varying electron affinities but are generally less likely to accept electrons compared to chlorine.
How many more electrons does silicon need to fill its outer shell?
silicon's atomic number is 14 so, its electron configuration is 2.8.4, the third shell needs 4 more electrons to make it 8 and to become stable. ---> so the answer is 4.
When silicon is doped with phosphorous what type of semiconductor results?
it would be a n-type semiconductor because phosphorus has more valence electrons than silicon does.
How many more electrons does silicon need in order to have a stable octet?
Silicon, like carbon, has four valance electrons, and needs another four to have a stable octet.
If silicon has four electrons in its outer energy level what type of bond will silicon form with?
A Covalent bond, because it takes too much energy to gain/lose more than two electrons, thus leaving the option of sharing electrons forming a covalent bond.
Can phosphorus expand its octet in chemical bonding?
Yes, phosphorus can expand its octet in chemical bonding by forming more than 8 valence electrons in its outer shell.
Is Chlorine more reactive than Silicon?
No. Chlorine is more reactive than silicon. This is because Chlorine has 7 valence electrons; nearly a full outer shell, while silicon has only 4 valence electrons. An element needs 8 valence electrons to react, and Chlorine only needs one more valence electron before it can react, unlike Silicon, which needs 4.
Why is there a large increase in ionic radius from silicon to phosphorus?
The increase in ionic radius from silicon to phosphorus is due to the addition of an extra electron in the outermost shell of the atom. This added electron increases the electron-electron repulsion forces, causing the electron cloud to expand and the ionic radius to increase.
How doping change structure of semiconductor?
This is copied from a similar question to yours fyi. Using boron, phosphorus, and silicon as examples. P-type doping is a process where a silicon atom in the lattice is replaced by a boron atom. A Boron atom has 3 electrons in the outer shell, compared with an electron occupancy of 4 for a silicon atom. So a Boron atom provides a vacancy for any free electrons to occupy with a little effort, when an electron chances to be nearby (the four boron-silicon covalent bonds needs 8 electrons to be stable, but only 7 are provided). The net charge of the material is still zero. More about from where the free electron is coming. N-type doping is using a phosphorus atom to replace a silicon atom. A phosphorus atom has 5 electrons in the outer shell. So a phosphorus atom provides an electron that can be freed with a little effort (the four phosphorus-silicon covalent bonds only need 8 electrons to be stable, each atom needing only to contribute four electrons; the 9th electron will be loosely bound). The net charge of the material is still zero. Where can the electron go? Magic happens when p-type silicon is brought in contact with n-type silicon to form a pn junction. The excess electron vacancies (holes) in p-Si now can exchange with the excess electrons in n-Si, but the net charge of the p-n silicon entity is still zero. However, microscopically, a depletion region is formed at the pn junction, where excess carriers can cross over to the other side. In the p-Si, excess electrons from the n-Si start filling up the holes (the lack of the 8th outer-shell electron to form the four stable boron-silicon covalent bonds) and negatively-charged boron atoms are formed. In the n-Si, excess holes from the p-Si start swallowing up the loosely-bound electrons (the 9th electron in the outer shell) of phosphorus atoms and positively-charged phosphorus atoms are formed. Once formed, and in the absence of an electric field, the depletion region now presents an energy barrier to any further carrier movement and a steady state results -- no net current in the pn junction.
