Introduction of Chemical Bonding & Valence
The group 8's inert gas elements exist as monatomic gases and do not generally react with other elements. Differ from the other gaseous elements exist as diatomic molecules (H2, N2, O2, F2 & Cl2) and all but nitrogen are quite reactive. Some instances of this reactivity are expressed in the following equations.
Ionic Bonding
When in the chlorine atmosphere, sodium is burned then it produces compound sodium chloride. To give a conducting solution this has a high melting point (800 ºC) and dissolves in water. The Sodium chloride is an ionic compound and the structure of crystalline solid is shown on the right. Transfer of lone 3s electron of a sodium atom to the half-filled 3p orbital of a chlorine atom produces a chloride anion (argon valence shell) and a sodium cation (neon valence shell). The result of the Electrostatic attraction in these oppositely charged ions packed jointly in a lattice. The ions which are hold by the attractive forces in place can be referred to as ionic bonds.
Covalent Bonding
The three reactions other than this shown above give products that are very distinct from sodium chloride. Water is in the liquid form at room temperature; carbon tetra fluoride and carbon dioxide are gases. Not a single compound is composed of the ions. The other attractive interaction between the atoms known as covalent bonding is involved here. By a sharing of valence electrons the Covalent bonding occurs, rather than the outright electron transfer. Likenesses in physical properties (they are all gases) suggest that diatomic elements O2, H2, N2, and F2 & Cl2 also have covalent bonds.
Instances of a, covalent bonding shown below in the diagram which includes fluorine, hydrogen, carbon dioxide and carbon tetra fluoride. These cases use a simple Bohr notation, with the valence electrons denoted by colored dots. Note: in first example both hydrogen atoms achieve a helium-like pair of 1s-electrons by sharing. In other instances carbon, fluorine and oxygen achieve neon-like valence octets by the same sharing of electron pairs. The Carbon dioxide is important because it is an example in which two pairs of electrons (four in all) are shared by the same two atoms. This is a case of a double covalent bond.
To understand the covalent bonding these electron sharing diagrams (Lewis formulas) are a useful first step, but it's easier and quicker to draw formulas of Couper-Kekulé in which each shared electron pair is denoted by a line between the atom symbols. The dots shown in the diagram are the Non-bonding valence electrons. These formulas are determined from graphic notations suggested by A. The Couper and Kekulé are not the same to their original drawings. Some instances of this kind of structural formulas are given in the table.
Common Name
Molecular Formula
Lewis Formula
Kekulé Formula
Methane
CH4
Ammonia
NH3
Ethane
C2H6
Methyl Alcohol
CH4O
Ethylene
C2H4
Formaldehyde
CH2O
Acetylene
C2H2
Hydrogen Cyanide
CHN
The sharing of two or more electron pairs is known as Multiple bonding, is illustrated by the ethylene and formaldehyde (each has a double bond) and hydrogen cyanide and acetylene (each with a triple bond). Boron compounds like BH3 and BF3 are exceptional in that conventional covalent bonding does not expand the valence shell occupancy of boron to an octet. Consequently, these compounds have an affinity for electrons and they displays exceptional reactivity when compared with the compounds which are shown above.
Valence
The valence is the number of valence shell electrons an atom must gain or lose to achieve a valence octet. In the covalent compounds number of bonds which are characteristically formed by a given atom is equivalent to that atom's valence. From the formulas written in the following table, we reach at the following general valence assignments:
Atom
H
C
N
O
F
Cl
Br
I
1
4
3
2
The valences that are shown here represent the most common form these elements assume in organic compounds. Many elements, like chlorine, iodine and bromine are known to exist in several valence states in different inorganic compounds.
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