The four quantum numbers for the valence shell electron or last electron of Lithium (z=3) is:

Spin quantum number (s) Spin quantum number denotes the spin of the electron on its own axis. It is denoted by ‘s’. It can have only two values(+½ and -½).

Oxygen – eight electrons

• A. n=2, l=1, m=−1, s=−21​
• B. n=2, l=0, m=0, s=+21​
• C. n=3, l=2, m=−2, s=−21​
• D. n=2, l=2, m=−1, s=+21​

Oxygen has the electron configuration 1s22s22p4, with two unpaired electrons (one in each of the two 2p orbitals). Valence bond theory would predict that the two O–H bonds form from the overlap of these two 2p orbitals with the 1s orbitals of the hydrogen atoms.

Looking at the periodic table, you can see that Oxygen has 8 electrons. Based on the order of fill above, these 8 electrons would fill in the following order 1s, 2s and then 2p. So Oxygen’s electron configuration would be O 1s22s22p4.

Ernest Z. Truong-Son N. The biggest amount of oxygen is in 5,06×10-3 mol.

Hybrid orbitals are the atomic orbitals obtained when two or more nonequivalent orbitals form the same atom combine in preparation for bond formation. The four lobes of each of the sp 3 hybrid orbitals then overlap with the normal unhybridized 1s orbitals of each hydrogen atoms to form the tetrahedral methane molecule.

The term “sp3 hybridization” refers to the mixing character of one 2s-orbital and three 2p-orbitals to create four hybrid orbitals with similar characteristics. Each hybrid orbital consists of a large lobe and a small lobe, pointing in two opposite direction (figure 1).

What is d2sp3 Hybridization? d2sp3 hybridization is the mixing of s and p atomic orbitals of the same electron shell with d orbitals of another electron shell to form d2sp3 hybrid orbitals. This hybridization results in six hybrid orbitals. These hybrid orbitals are arranged in an octahedral geometry.

The sp2 hybridization is the mixing of one s and two p atomic orbitals, which involves the promotion of one electron in the s orbital to one of the 2p atomic orbitals. The combination of these atomic orbitals creates three new hybrid orbitals equal in energy-level.

If a carbon atom is sp3 hybridized it can only form sigma bonds. And in sp hybridization two unhybridized p orbitals will form pi bonds while the lone sp orbital will form the sigma bond.

two

three

All the carbon atoms in an alkane are sp3 hybridized with tetrahedral geometry. The carbons in alkenes and other atoms with a double bond are often sp2 hybridized and have trigonal planar geometry. The triple bond, on the other hand, is characteristic for alkynes where the carbon atoms are sp-hybridized.

For sp2 hybridized central atoms the only possible molecular geometry is trigonal planar. For sp3 hybridized central atoms the only possible molecular geometry is tetrahedral. If all the bonds are in place the shape is also tetrahedral.

NOTES: This molecule is made up of 4 equally spaced sp3 hybrid orbitals forming bond angles of approximately 109.5o. The shape of the orbitals is tetrahedral. Two of the orbitals contain lone pairs of electrons.

Tetrahedral is sp3 and Square planar dsp2. One example is Ni(CN)4 is square planar (evidence is from the fact that it is diamagnetic).