it gave me two answer and that is it
All atoms have quantized energy levels that are systematically labeled as different orbitals all having different rules of how they can be populated. While this system isn't 100% correct, it's good enough to be extended to the molecular level. Molecular orbitals are called hybridization orbitals and they are modeled as combinations of the constituent atoms that are bonded together to make them.
it gave me two answer and that is it
Looking at the electron configuration of carbon (at. no. 6) you have 1s2 2s2 2p2. In the 2 p subshell, you have 1 electron in the 2px orbital, and 1 electron in the 2py orbital and no electrons in the 2pz orbital. So, the answer is that there are TWO half filled orbitals in the carbon atom. This is the case BEFORE hybridization. After hybridization, there are FOUR half filled orbitals which are called sp3 hybrids.
This breeding method is called hybridization. It is possible only in those cases where sexual barrier of crossing does not exist.
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
the bonding between the carban and the nitrogen in hydrogen cyanide or hydrocyanic acid is a triple bond, hence the hybrid orbital is sp, due to the linear geometry of the molecule
sp3 is the hybridization of the nitrogen atom in NCl3.
If inner d orbital is involved in hybridization, it is called inner d orbital complex. and if outer d orbital is involved in hybridization then it is called 'outer d orbital complex'.
sp3d2
Orbital hybridization provides information about both molecular bonding and molecular shape.
The hybridization of Titanium in TiCl4 is Sd3 covalant Liqiid with boilling point 136 degree centigrade. The 4S2 electron is promoted to 3d orbital to make it d3 followed by Sd3 tetrahedral hybridization.
methane is the simplist example of hybridization. hybridization is basically exciting electrons so that it can bond with other elements. methane is CH4. tetrahederal shape, sp3 hybridization because it's all single bonds. when you excite the 2s orbital, you leave one electron in that orbital and bring it up to the 2p orbital, namely the 2pz, and then have the four hydrogens share electrons with the unfilled orbitals.
Hi, The nitrogen is glycine is sp3 hybrid. The shape is tetrahedral.
sp3d2 Br hybridizes 4s, 4p and 4d If I'm not mistaken. Seems kind of strange for a hybridization since it involves two 4d orbital when you'd expect it to hybridize with only one 4d orbital, but that's what I found on a few websites.
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Molecular orbital theory(MOT) provides information about both molecular shape and molecular bonding.
Sp2 orbitals are used in the expansion of the molecules shape. The difference in distance between the Sp2 orbital in an SP hybridization is 120 degrees.
Yes it does. three of the sp3 orbitals are used to bond to the three Hydrogens. the fourth sp3 orbital is used to hold the lone pair of electrons (of the nitrogen)
The hybridization of the bonding orbitals of carbon in carbon tetrachloride are sp3 hybridized. The hybridization occurs between the s orbital of the hydrogen atom and the px, py, pz orbitals of the carbon atom, hence it is sp3 hybridized.