Bonding, Structure and Properties When atoms join together, neither with similar atom or an alternate atom, the method it joins, has considerable effect on its structure and then consequently on its properties. The joining of an atom to another atom is called Bonding. Bonding involves each atom neither donating or accepting electron from another atom. It shall also be done through sharing electrons. There exists 3 variations of bonding that shall be discussed here.
Ionic Bonding The bonding involves ions as the name suggests. When an atom becomes a positive ion by losing an electron, this positive ion shall look for a negative ion to attract. A negative ion shall be the atom that has gained an electron. When these positive and negative ions meet, through attraction of opposites a bonding shall be formed, that is known as ionic bonding. The substances that should have this kind of bondings are compounds of metals with non-metals.
For example Sodium Chloride, which involves metal for example Sodium and non-metal for example Chlorine, most grow to ions. Sodium has one electron in its outer shell, which it shall lose to grow to a positive ion. Chlorine has seven electrons in its outer shell that is why shall gain one electron to shape a stable outer shell and grow to a negative ion. The structure, that is present in ionic bonded compounds, is Giant Lattice. Ionic bonding shows properties of high melting and boiling point.
They can be very hard but brittle and conduct electricity when dissolved in water, or molten. They can be often soluble in h2o and generally insoluble in non-polar solvents. This kind of bonding involves sharing of electrons between the 3 atoms. It is present in non-metals for example Carbon, Chlorine, and Oxygen. For example, in Oxygen, there exists seven electrons within the outer shell.
It should bond with another Oxygen by sharing its 3 electron with other Oxygen's 3 electron that is why sharing a total of 4 electrons. This is a double bond. In a lone bond only one pair of electrons are shared for example between Chlorine and Chlorine. Covalent bonds are tough and hold a very high melting and boiling point. It does not conduct electricity and is insoluble in h2o and non-polar solvents.
Metallic Bonding This bonding joins metal atoms together for example Magnesium atoms. Many MgAtoms bond together to shape a solid metal. Magnesium atoms are positive ions surrounded by delocalised electrons. Due to these delocalised electrons, they conduct electricity. The melting and boiling points are generally high in Metallic bonding.
No comments:
Post a Comment