Basics of Chemical Bonding - 2

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Chemical Bonding Part 2

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There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 - 200 kcal/mol). Whether two atoms can form a covalent bond depends upon their electronegativity i.e. the power of an atom in a molecule to attract electrons to itself. If two atoms differ considerably in their electronegativity - as sodium and chloride do - then one of the atoms will lose its electron to the other atom. This results in a positively charged ion (cation) and negatively charged ion (anion). The bond between these two ions is called an ionic bond. Covalent BondsIonic Bonds Polarity:LowHigh Formation:A covalent bond is formed between two non-metals that have similar electronegativities. Neither atom is \"strong\" enough to attract electrons from the other. For stabilization, they share their electrons from outer molecular orbit with othersAn ionic bond is formed between a metal and a non-metal. Non-metals(-ve ion) are \"stronger\" than the metal(+ve ion) and can get electrons very easily from the metal. These two opposite ions attract each other and form the ionic bond. Shape:Definite shapeNo definite shape What is it?:Covalent bonding is a form of chemical bonding between two non metallic atoms which is characterized by the sharing of pairs of electrons between atoms and other covalent bonds.Ionic bond, also known as electrovalent bond is a type of bond formed from the electrostatic attraction between oppositely charged ions in a chemical compound. These kinds of bonds occur mainly between a metallic and a non metallic atom. Melting point:lowHigh Examples:Methane (CH4), Hydro Chloric acid (HCl)Sodium chloride (NaCl), Sulphuric Acid (H2SO4 ) Occurs between:Two non-metalsOne metal and one non-metal Boiling point:LowHigh State at room temperature:Liquid or gaseousSolid Ability to conduct electricity in molten/aqueous state: Yes Ability to conduct electricity in solid state: Solution There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 - 200 kcal/mol). Whether two atoms can form a covalent bond depends upon their electronegativity i.e. the power of an atom in a molecule to attract electrons to itself. If two atoms differ considerably in their electronegativity - as sodium and chloride do - then one of the atoms will lose its electron to the other atom. This results in a positively charged ion (cation) and negatively charged ion (anion). The bond between these two ions is called an ionic bond. Covalent BondsIonic Bonds Polarity:LowHigh Formation:A covalent bond is formed between two non-metals that have similar electronegativities. .

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Explain covalent bond? Explain Metallic bond and what important property derives from it in metals? Solution Covalent bonding occurs when pairs of electrons are shared by atoms. Atoms will covalently bond with other atoms in order to gain more stability, which is gained by forming a full electron shell. By sharing their outer most (valence) electrons, atoms can fill up their outer electron shell and gain stability. Nonmetals will readily form covalent bonds with other nonmetals in order to obtain stability, and can form anywhere between one to three covalent bonds with other nonmetals depending on how many valence electrons they posses. Although it is said that atoms share electrons when they form covalent bonds, they do not usually share the electrons equally. Link : http://chemwiki.ucdavis.edu/Theoretical_Chemistry/Chemical_Bonding/General_Principles/Covalent_Bonds Metallic bond is the reaction between molecules within metals called alkali reactive force. It was first discovered by K. Manishekar. It is the sharing of a sea of delocalised electrons amongst a lattice of positive ions, where the electrons act as a \"glue\" giving the substance a definite structure. The electrons and the positive ions in the metal have a strong attractive force between them. Therefore metals often have high melting or boiling points. The principle is similar to that of ionic bonds. The metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, luster, conduction of heat and electricity. Because the electrons move independently of the positive ions in a sea of negative charge, the metal gains some electrical conductivity. It allows the energy to pass quickly through the electrons generating a current. Heat conduction works on the same principle - the free electrons can transfer the energy at a faster rate than other substances such as those which are covalently bonded, as these have their electrons fixed into position. There also are few non-metals which conduct electricity: graphite (because, like metals, they have free electrons), and molten and aqueous ionic compounds which have free moving ions Link : https://simple.wikipedia.org/wiki/Metallic_bond .

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For Ionic Bond 1.It is generally formed of the metals and non-metals. The metal atom loses one or more electrons present in its valence shell and these electrons accept by the non-metallic atom. 2.One of the species is cation and the other is an anion.By losing electrons, the metal atom changes to (positive ion) cation.Similarly, the non-metal atom gaining the electrons, get change to (negative Ion) anion. The oppositely charged ions attract each other. Therefore, come closer resulting the formation of the ionic bond (Electrovalent Bond).

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