Why Carbon can form Chain 1,2,and 3

Uniqueness of Carbon Atoms
1. Carbon atom has four valence electrons
Based on the configuration of electrons held six carbon atoms found that its valence electrons is 4. To achieve stability, the atoms still needs 4 more electrons by covalent bonds. No element of other groups that can form covalent bonds with as many as 4 pieces of the octet rule.
2. Small Relative Elemental Carbon Atoms
Judging from the electron configuration, it is known that atoms
carbon lies in period 2, which means the atom has a second skin
atom, so the atomic radius is relatively small. This causes the bond
formed relatively strong covalent and can form a covalent bond
duplicate.
3. Carbon Atom Can Establish Carbon Chain
The state of the carbon atom to carbon atom thus cause
forming a very long carbon chains with covalent bonding, covalent bonding either single, dual 2, or 3 copies. Moreover, it can also form a chain ring (cyclic).
Uniqueness of Carbon Atoms: Has Ability Form Chain - One of the perks of carbon that is not owned by the other elements is their ability to form chains of carbon atoms, which we hereafter refer to as the carbon chain.

Carbon chains may be either a single bond, double bond, or a triple bond. Forms of carbon chains themselves are very varied, there is a straight (unbranched), there is a branching, there are open, and there is a closed (circular).
Compounds with an open chain compounds called aliphatic compounds while closed or circular chain called cyclic compounds. The compounds are all carbon bond is a single bond, - C - C - called unsaturated carbon compounds, while having a carbon-carbon double bond, - C - C -, or triple - C = C -, called unsaturated carbon compounds.
Cyclic compounds having conjugated bonds, the carbon-carbon bond alternating single and dual, are called aromatic compounds. All cyclic compounds that are not included aromatic compounds are called alicyclic compounds, (the word comes from the word ali alicyclic and cyclic). These compounds are called alicyclic compound because it has a circular shape, but its properties resemble aliphatic compounds.
Why carbon can form so many compounds, with very varied types? Why is this not happening in the adjacent element or elements are classified with the carbon in the periodic table? BC has the electron configuration of atoms 2 4. The four valence electrons distributed on the four C atoms in a symmetrical position.

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ability to bind carbon atoms and follow the octet rule is different from other atoms, even within a single class. For example, boron and nitrogen atoms. Electron configuration of two atoms is J3: 2 3 and _n: 2 5. Boron atom has three valence electrons so that when the covalent bonds, resulting compounds do not follow the octet Kaidan.

The compound BH, has the form of a symmetrical molecule and has three covalent bonds. In contrast to compound BH3, NH3 compounds follow the octet rule, but the shape of the molecule is not symmetrical because there is a lone pair.

Thus, compounds BH, and NH3 only has three covalent bonds. What about silicon? The silicon atom has an electron configuration 2 8 4. The silicon atom has four valence electrons with the carbon atom. The four electrons in the silicon atom is distributed on four sides symmetrically.

 Carbon has four valence electrons with the atomic radii price the smallest of the atomic radius of other elements in the group IVA. It facilitates the C atom to form covalent bonds with other atoms, especially with atomic H, O, N, and halogen atoms (F, Cl, Br, and I). Covalent bonds are formed to meet the octet rule. The carbon atom can form up to four covalent bonds. Covalent bond formed by atoms C is more powerful than other covalent bonds, so that the carbon compounds are stable.

The position of carbon atoms in the periodic table in the middle so it has a moderate electronegativity value (2.5). This trait causes the carbon atoms can bind atoms having electronegativity greater or even smaller. The carbon atom can have a positive oxidation state (+2, +4), negative (-2, -4), or even zero.



 

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