This is because oxygen is more electronegative, nitrogen is less electronegative than oxygen, and the electronegative element with a negative charge is more stable. In the oxides of nitrogen, nitrogen always shows a positive charge, and oxygen possesses a negative charge. Nitrogen and oxygen readily combine to form various oxides as nitrogen shows variable oxidation states. To explain molecular geometry and bond angles, the most important theory we need to discuss is the VSEPR theory. Molecules forming a covalent bond with different atoms usually are arranged in various forms. Molecules forming a covalent bond with the same atoms with more than two atoms are polyatomic molecules for example, O3, P4, S8. Molecules forming a covalent bond with the same atoms, like homoatomic molecules, are usually arranged linearly for example, H2, I2, Br2, Cl2, F2 etc. A covalent bond is usually formed by sharing electrons, without ions, amorphous solids, and is directional. An ionic bond is formed by the transfer of electrons, forms ions and is crystalline and non-directional. Ionic and covalent molecules are very different from one another. They can have different bondings, like covalent and ionic. Molecules have atoms bonded around them and occupy space. Compounds have a fixed composition irrespective of the source from which they are prepared, and this follows the law of constant proportion. Molecules that are made of two atoms are binary compounds, while those made of three atoms are tertiary compounds. Molecules can be diatomic, triatomic, or polyatomic and can be made of the same type of atoms or different types of atoms. Elements that are naturally unstable combine with other elements to gain stability.
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