{"id":911,"date":"2022-11-18T16:00:53","date_gmt":"2022-11-18T10:30:53","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=911"},"modified":"2022-11-19T16:25:44","modified_gmt":"2022-11-19T10:55:44","slug":"covalent-bond","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/covalent-bond\/","title":{"rendered":"What is Covalent Bond?"},"content":{"rendered":"
The\u00a0Covalent Bond<\/span><\/strong><\/p>\n People also ask<\/strong><\/p>\n 1. Single covalent bond:<\/strong><\/span> Bonding in metals:<\/span><\/strong> What is Covalent Bond? The\u00a0Covalent Bond Covalent bonds are formed when atoms of non-metals combine with each other to form a molecule. Non-metal + Non-metal \u2192\u00a0Covalent compound The non-metals involved can be (a) the elements from Groups 15, 16, and 17 of the Periodic Table. (b) carbon and silicon from Group 14 of the Periodic […]<\/p>\n","protected":false},"author":2,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[84],"tags":[99,98,97],"yoast_head":"\n\n
\nNon-metal + Non-metal \u2192\u00a0Covalent compound<\/li>\n
\n(a) the elements from Groups 15, 16,<\/strong> and 17<\/strong> of the Periodic Table.
\n(b) carbon and silicon from Group 14 of the Periodic Table.
\n(c) hydrogen, the smallest-sized atom. Hydrogen forms covalent bonds when it combines with more electronegative non-metal such as a fluorine, oxygen, nitrogen, chlorine, bromine, iodine or carbon.<\/li>\n
\nAs a result, covalent molecules<\/strong> are formed.<\/li>\nTypes of Covalent Bonds<\/strong><\/h2>\n
\n
\n<\/li>\n
\n<\/li>\n
\n<\/li>\n
\n(a) Single<\/strong> covalent bond
\n(b) Double<\/strong> covalent bond
\n(c) Triple<\/strong> covalent bond<\/li>\n\n
\n
\nA single covalent bond is formed when one pair of electrons is shared between two atoms.
\nExamples :<\/strong>
\n1. Formation of a hydrogen molecule (H2<\/sub>)<\/strong> :<\/span>
\nA molecule of hydrogen consists of two hydrogen atoms. Each hydrogen atom has one electron. When two atoms of hydrogen combine, one electron of each takes part in sharing. Thus, two electrons (one pair of electrons) are shared between the two atoms.
\nThe shared electron pair always exists between the two atoms. The two dots between the two H atoms represent the pair of shared electrons. One pair of shared electrons gives a single bond. Such a bond is represented by a short line between the two atoms. Thus, a hydrogen molecule may be represented as in figure.
\nOnce the bond is formed, the both atoms have a stable configuration of the noble gas helium.
\n2. Formation of a methane molecule (CH4<\/sub>) :<\/strong>
\nA carbon atom has four electrons in its outermost shell (valence shell). It shares its valence electrons with those of four H atoms. Thus, an atom of carbon forms four single covalent bonds with four H atoms.
\nPictorially, a methane molecule may be represented as in Figure.
\n2. Double covalent bond :<\/strong><\/span>
\nA double covalent bond is formed when two pairs of electrons are shared between the two combining atoms. A sharing of two pairs of electrons is shown by marking two short lines between the symbols of the two atoms.
\nExamples:<\/strong>
\n1. Formation of an oxygen molecule (O2<\/sub>) :<\/strong>
\nAn atom of oxygen contains six electrons in its valence shell. It requires two more electrons to attain a stable eight-electron configuration (octet). This is achieved when each of the two oxygen atoms shares its two electrons with the other, resulting in the formation of a stable oxygen molecule.
\nPictorially, the oxygen molecule may be represented as in figure.
\n2. Formation of an ethylene molecule (C2<\/sub>H4<\/sub>) :<\/strong>
\nIn the formation of an ethylene molecule (C2<\/sub>H4<\/sub>), each of the two C atoms combines with two H atoms to form two single covalent bonds. The remaining two electrons of each C atom form a double bond between the two C atoms.
\nPictorially, a molecule of ethylene (C2<\/sub>H4<\/sub>) may be represented a in figure.
\n3. Triple covalent bond:<\/strong><\/span>
\nA triple covalent bond is formed when three pairs of electrons (six electrons) are shared between the two combining atoms. A triple bond is shown by marking three short lines between the two symbols of the atoms.
\nExamples:<\/strong>
\n1. Formation of a nitrogen molecule (N2<\/sub>) :<\/strong>
\nAn atom of nitrogen has five electrons in its valence shell. It requires three more electrons to attain the stable octet. This is achieved when two nitrogen atoms combine together by sharing three electrons each to form a nitrogen molecule.
\nPictorially, a nitrogen molecule can be represented as in figure.
\n2.\u00a0<\/strong>Formation of an acetylene molecule (C2<\/sub>H2<\/sub>) :<\/strong>
\nIn an acetylene molecule, two C atoms combine with two H atoms. Each C atom shares three of its valence electrons with the other C atom. One electron of each C atom is shared with one electron of a H atom.
\nThus, in a molecule of acetylene, there is a triple covalent bond between the two C atoms and each C atom is joined to one H atom by a single covalent bond. Pictorially, a molecule of acetylene may be represented as in figure.
\nCharacteristics of covalent compounds:<\/strong><\/span><\/p>\n\n
\nAs you know, metals are hard solids and they are made up of atoms. It has been established that the atoms in a metal are very closely packed together.
\nThe force that holds the atoms closely together in a metal is known as the metallic bond.
\nMetal atoms lose one, two or three electrons to form positively charged ions, called cations.
\nThe electrons thus lost move freely in the metal, i.e., these electrons become mobile, but the cations do not leave their positions. So in a metal lattice it is assumed that the metal ions are immersed in a sea of electrons. Due to the presence of mobile electrons, metals are good conductors of heat and electricity.<\/p>\n","protected":false},"excerpt":{"rendered":"