Chemical Bonding There are numerous types of chemical bonds and forces acting jointly to combine molecules together. The two most fundamental types of bonds are ionic and covalent bond. In ionic bonding, atoms transfer electrons to each other. Ionic bonds need at least one electron donor and one electron acceptor. On the contrary, atoms that have similar electro negativity share electrons through covalent bonds as for such atoms, donating or receiving electrons are not favorable. Chemical bonding is a means through which atoms unite to form molecules. Chemical bond exists between two atoms or groups of atoms when the forces acting between them are physically powerful enough to result to the formation of an aggregate with adequate stability to be termed an autonomous species. The no of bonds an atom forms matches up to the number of electron at its outer shell. Bond energy is the quantity of energy necessary to break a bond and create neutral atoms. In line with Coulomb’s law every bond as a result of attraction that exist between unlike charges. On the other hand, the manner this force is manifested varies depending on the atoms concerned. The main types of chemical bond are the ionic, covalent, metallic, and hydrogen bonds. The ionic and covalent bonds are ideal forms but the majority of the bond types are of an intermediary type. Bonding energy between two atoms The interaction energy between two atoms at equilibrium is referred to as the bonding energy between the two atoms. To break the bond, this energy must be supplied from outside. Breaking the bond means that the two atoms become infinitely separated. In real substances that are made up of varieties of atoms, bonding is calculated by stating the bonding energy of the entire substances in terms of the disjointing distances among all atoms. There are different types of bonding: • Primary bonding: Ionic (involves transfer of outermost electrons) • Covalent (involves sharing of outermost electrons, directional) • Metallic (involves delocalization of valence electrons) • Secondary or van der Waals Bonding:(widespread, but less strong than primary bonding) • Dipole-dipole • H-bonds • Polar molecule-induced dipole • Variable dipole (the most weak bond) The Ionic Bonding Ionic bonding is the total transfer of outermost electron(s) between atoms. It is the type of chemical bond that produces two oppositely charged ions. In ionic bonds, the metal loses electrons to turn into a positively charged cation, while the non-metal receives those electrons to turn into a negatively charged anion. For ionic bond to occur there must be an electron donor, metal, and an electron acceptor, non metal. Ionic Bonding is occurs because metals have a small number of electrons in their outmost orbital. Through the loss of those electrons, these metals can attain noble-gas configuration and meet the octet rule. Likewise, non metals that have nearly 8 electrons in their outermost shell have the tendency of readily accepting electrons to attain their noble gas configuration. In ionic bonding, over 1 electron can be donated or received to fulfill the octet rule. The charge on the anion and cation matches up with the number of electrons contributed or received. In ionic bonds, the net charge of the compound must be zero. The ionic bond is a chemical bond formed as a result of attraction between two opposite charged ions. The atoms of metallic elements like sodium easily lose their valence electrons, whereas the atoms of non-metals like chlorine have the tendency to gain electrons. The reaction between them results to a highly stable ions which maintain their individual structures while approaching one another to form a stable molecule or crystal. In an ionic crystals such as sodium chloride, no separate diatomic molecules are present; instead, the crystal is made up of composed of independent Na+ and Cl− ions, with each being attracted to adjoining ions of the opposite charge giving rise to one single gigantic molecule. chemistry
Posted on: Fri, 17 Oct 2014 18:02:24 +0000