Hybridization Relationship With Bond Angle and Bond length

Hybridization relationship with bond angle and bond length, such us:

1. Carbon Atoms

a. Sp3 hybridization

Larbon atom has two orbitals (2s and 2p) to form a bond, meaning that if it reacts with hydrogen will be formed two CH bonds. In fact, the carbon atoms form four CH bonds and produce a methane molecule to form a tetrahedron geometry. Linus Pauling (1931) describes mathematically how the orbital s and three p orbitals combine or hybridized form four equivalent atomic orbitals with tetrahedral shape. Orbital called tetrahedral shaped sp3 hybridization.

In the excited position, carbon has four unpaired electrons and can form four bonds with hydrogen. Although it requires an energy of 96 kcal / mol to excite an electron in advance, the bond formed by H (at CH4) is much more stable than the CH bond

CH2 molecules. Pd CH methane bonds have a bond strength of 104 kcal / mol with the bond length 1:10 A. HCH bond angle of 109.5 degrees.

b. Sp2 hybridization; Orbital and Structure of Ethylene

When we form the orbital hybridization of sp3 to explain the bonding in methane, which is done first is to promote an electron from the 2s orbital excited state to produce four unpaired electrons. Sp2 hybridization terjadijika one electron is excited to orbital p. As a result, the sp 2 hybridized carbon atom can only form three sigma bond and one pi bond. Pi bond occurs as a result of the overlap of electrons in 2p-2p orbitals. Two sp2 carbon atom can form a strong bond with each other, they form a sigma bond through sp2-sp2 orbital overlap. A combination of sigma sp2-sp2 bonds and pi bonds 2p-2p produce form carbon-carbon double bond. Shape geometry of

bond sp2 hybridized carbon atom is trigonal planar.

c. Hybridization sp

The carbon atom has the ability to form three types of bonds, namely single bonds, double and triple. Acetylene, C2H2, the simplest example of a carbon-carbon bond triplicate. In addition can be combined with two or three p orbitals, hybrid orbitals 2s also can combine with the p orbitals. Sp orbitals have a linear geometry with HC-C bond angle of 180 degrees which have been verified from experimental results. Hydrogen-carbon bond length and bond length of 1.06A

Carbon-carbon is 1:20 A.

2. Nitrogen Atom

Covalent bonds are formed not only in carbon compounds, but can also be formed by atoms of other atrom. All covalent bonds formed by the elements in the periodic table can be explained by orbital hybrid. In principle, the same hybrid formation with the carbon atoms. Bond angle formed is 107.3 degrees, approaching the tetrahedral angle (109.5 degrees). Nitrogen has five electrons in its outer shell.

3. Oxygen Atom

Electrons in the ground-state atomic oxygen has a configuration:

1s2 2s2 2px2 2py1 2pz1, and oxygen is a divalent atom. By looking at the electron configuration, it can be predicted that oxygen is able to form two sigma bonds because the outer shell has two unpaired electrons (2py and 2pz). Water is an example of a compound containing oxygen sp3.

bond angle of 104.5 degrees formed is estimated that the lone pair orbital by pressing the HOH bond angle, so that the angle formed smaller than the ideal angle (109.5derajat), as well as the free electron pairs in ammonia pressing HNH bond angles.

4. Association Alkena

the language of valence bond, sp2 hybridized carbon atom and has three hybrid orbitals are equivalent. Bond angle formed is 120 degrees to one another. Secondly, the language of molecular orbitals, the interaction between the p orbitals trigger the formation of a bonding orbital and an anti-bonding orbital pi.

5. Association of alkyne

Triple bond resulting from the interaction of carbon-carbon sp hybridized. When two sp hybridized carbon atoms interacting it will form a σ bond and two π bonds. It is known that the bond angles at the sp hybridized carbon is 180 degrees, thus, acetylene C2H2, is a linear molecule with HCC bond angle of 180 degrees.