phosphorus
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.
Silicon, like carbon, has four valance electrons, and needs another four to have a stable octet.
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.
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.
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.
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.
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.
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.
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.
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.
it would be a n-type semiconductor because phosphorus has more valence electrons than silicon does.
Silicon, like carbon, has four valance electrons, and needs another four to have a stable octet.
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.
Yes, phosphorus can expand its octet in chemical bonding by forming more than 8 valence electrons in its outer shell.
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.
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.
Donor impurities in silicon are atoms of elements that have one more electron than silicon, such as phosphorus or arsenic. These impurities are used to make silicon into an n-type semiconductor, which means they increase the number of free electrons in the material, making it conductive.