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A Case Study on Covalent Bonding

A Case Study on Covalent Bonding. By: Wong Wei Cong (31) 2A1. What is Covalent Bonding. What is Covalent Bonding . Sharing of electrons so as to achieve stable electronic configuration of noble gas Electrostatic attraction between nuclei of the atoms and the pair(s) of shared electrons

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A Case Study on Covalent Bonding

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  1. A Case Study on Covalent Bonding By: Wong Wei Cong (31) 2A1

  2. What is Covalent Bonding

  3. What is Covalent Bonding • Sharing of electrons so as to achieve stable electronic configuration of noble gas • Electrostatic attraction between nuclei of the atoms and the pair(s) of shared electrons • Molecules are formed • Generally, covalent bonds are formed between atoms of non-metals

  4. Exceptions to This Rule • Aluminium Chloride (AlCl3) • Beryllium Chloride (BeCl2)

  5. Electronegativity • Describes tendency of an atom to attract electrons towards itself and thus the tendency to form anions • Affected by both the number of protons and the distance that the valence electrons reside from the nucleus • As you go across a period, electronegativity increases • As you go down a group, electronegativity decreases

  6. Polar Bonds • If two atoms of equal electronegativity bond together… • Both have same tendency to attract bonding pair of electrons • Electron pair found on average half way between the atoms • Electron pair shared evenly between the atoms • “Pure” covalent bonds • If B is a lot more electronegative than A… • Electron pair dragged right over to B's end of the bond • A has lost control of its electron • B has complete control over both electrons • Ionic bonds

  7. Polar Bonds (II) • If B is slightly more electronegative than A… • B attracts electron pair more than A does • B’s end of the bond slightly negative • A’s end of the bond slightly positive • Polar bond Water is a polar covalent bond!

  8. Electronegativity of Elements

  9. Electronegativity & Bond Type

  10. So… yes! You guessed it… Electronegativity difference = 1.4 Aluminium Chloride is a polar covalent bond! Electronegativity difference = 1.4 Beryllium Chloride is a polar covalent bond!

  11. Formation of Aluminium Chloride Strongly heated aluminium foil burns in chlorine to form aluminium chloride

  12. Aluminium Chloride • Imagine that aluminum chloride is ionic instead • Contain Al3+ and Cl-ions • Aluminium ion: small & packed with 3 positive charges • High charge density – polarise chlorine ions • Electron pairs dragged back towards aluminium to such extent that the bonds become covalent • Chlorine more electronegative than aluminium – electron pairs will not be pulled half way between the atoms • Polar covalent bond formed

  13. Factors Affecting Polarising Ability • In aluminium chloride, aluminium ions polarise chloride ions • Positive ions can polarise nearby negative ions • The smaller the positive ion and the larger the number of charges, the greater the polarising ability • The bigger the negative ion, the easier it is to polarise it Aluminium iodide is covalent as electron pair is easily dragged away from iodide ion Aluminium fluoride is ionic as aluminium ion cannot polarise small fluoride ion sufficiently to form a covalent bond

  14. The Mystery of Aluminium Chloride • At room temperature, each aluminium surrounded by 6 chlorines • Ionic crystal structure with a lot of covalent character • At ordinary atmospheric pressure, it sublimes at about 180°C • If pressure raised to just over 2 atmospheres, it melts at 192°C • Comparatively weak attractions between molecules • Each aluminium now surrounded by 4 chlorines rather than 6 • Original lattice converted into Al2Cl6molecules • As temperature increases further, it increasingly breaks up into simple AlCl3molecules

  15. The Mystery of Aluminium Chloride (II)

  16. Beryllium Chloride • Imagine that beryllium chloride is ionic instead • Contain Be2+and Cl- ions • Beryllium ion: small & packed with 2 positive charges • High charge density – polarise chlorine ions • Electron pairs dragged back towards beryllium to such extent that the bonds become covalent • Chlorine more electronegative than beryllium – electron pairs will not be pulled half way between the atoms • Polar covalent bond formed

  17. The Mystery of beryllium Chloride • As a gas, Beryllium Chloride is a linear molecule with all three atoms in a straight line • As a solid, the molecules form long chains (polymers) • Coordinate bonds Arrows goes from the atom supplying the pair of electrons to the atom with the empty orbital Gas Solid

  18. Why is Beryllium Chloride not Ionic? • Beryllium has quite a high electronegativity compared with the rest of Group II • Attracts bonding pair of electrons towards itself more strongly • In order for an ionic bond to form, the beryllium has to let go of its electrons, but it is too electronegative to do that • Lewis acid – accepts lone pair of electrons • Boils at 520°C – low boiling point, so cannot contain ions • Reacts vigorously with water, forming acidic, steamy hydrogen chloride gas – typical of covalent chlorides

  19. Chemistry Music Video – Enjoy!  Two atoms met on one fine dayOne asked if he could bondWith the other atom thereOf whom he was really fondThe second atom shrugged and saidWhat’s your pleasure, son?Are you up for electron transferOr electron-sharing fun!Ionic or covalent?What kind of bonds are these?Involve valence electronsAnd form compounds with ease!Metal atoms lose electronsAnd become a charge of plusNon-metals gain them happily Look negative to all of us.The opposite charged ionsAttract to make ionic bondsThe E.N.D. one point seven plusThey dissolve real well in ponds!Ionic or covalent?What kind of bonds are these?Involve valence electronsAnd form compounds with ease! If the E.N.D. is point-five or moreAnd two non-metals hadYou have a polar covalent bondOne atoms happy, the others sad!The atom with less E.N. Gets a positive charge that’s slight

  20. Chemistry Music Video – Enjoy!  And the other, more greedy atom?Slightly negative to our sight!Ionic or covalent?What kind of bonds are these?Involve valence electronsAnd form compounds with ease!If the E.N.D. is point-four or lessTwo non-metal atoms bondWith equal pull on electronsEach atom is equal fondNo charges will developAnd, because of that, no polesThat’s why the bond is called non-polarOn and on and on we roll!Ionic or covalent?Now its easy for you to tellJust look up the E.N.D.And you will do real well! YouTube Link: http://www.youtube.com/watch?v=oNBzyM6TcK8

  21. Bibliography • http://www.chemguide.co.uk/atoms/bonding/electroneg.html • http://www.chemguide.co.uk/inorganic/period3/chlorides.html • http://www.chemguide.co.uk/inorganic/group2/beryllium.html • http://en.wikipedia.org/wiki/Electronegativity • http://en.wikipedia.org/wiki/Covalent_bond • http://en.wikipedia.org/wiki/Aluminium_chloride • http://en.wikipedia.org/wiki/Beryllium_chloride

  22. THANK YOU! The name’s Bond, Covalent Bond!

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