Draw and explain any three example of covalent and coordinate covalent bond
Answers
Answer:
1. Ammonium (NH4+) ion
The ammonium ion is formed from the reaction of ammonia (NH3) gas with hydrogen chloride (HCl) gas. In NH4+, the fourth hydrogen is attached by a coordinate covalent bond because only the hydrogen’s nucleus is transferred from the chlorine to the nitrogen. The hydrogen’s electron is left behind on the chlorine to form a negative chloride (Cl–) ion.
2. Ammonia Boron Trifluoride (NH3.BF3)
Boron trifluoride (BF3) is a compound that does not have a noble gas structure around the boron (B) atom. The boron only has three pairs of electrons in its valance shell and requires a pair to complete the orbital. Hence, BF3 is electron deficient. The lone pair on the nitrogen (N) of the ammonia (NH3) molecule is used to overcome that deficiency, and a complex compound forms through a coordinate covalent bond.
3. Hydronium ion (H3O+)
When hydrogen chloride (HCl) gas dissolves in water to make hydrochloric acid (HCl aq.), a coordinate covalent bond is formed in the hydronium ion. The hydrogen (H) nucleus is transferred to the water (H2O) molecule, which has a lone pair of electrons to form hydronium. So, H does not contribute any electrons to the bond.
4. Aluminum Chloride (Al2Cl6)
The bonding in aluminum chloride (AlCl3) is essentially covalent. Each aluminum (Al) atom has a deficit of two electrons in its valance shell, and chlorine (Cl) has a lone pair. Al forms a coordinate covalent bond with the Cl atom on an adjacent AlCl3 group. As each of two Al atoms does this, then aluminum chloride is a covalent dimer molecule with the formula Al2Cl6.
5. Carbon monoxide (CO)
Carbon (C) has four electrons in its valence shell, and oxygen (O) has six. Both carbon and oxygen share their two electrons. While the octet rule is satisfied with oxygen, there is still a deficit of two electrons on the carbon. So, oxygen shares its two electrons with carbon to form a coordinate covalent bond, in addition to the two regular (double) covalent bonds.
Explanation:
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ÌÑŚŤÂĞŘÂM Srinivas_Rao_2008
