- Relative attraction of an atom for electrons, its own and those of other atoms.. - Electronegativities of the Elements Electronegativities of the Elements. - Non-polar bonds: diff. - Polar bonds: diff. - Ionic bonds: diff. - Ionic Compounds. - Ionic Compounds Ionic Compounds. - nickel(II) chloride hexahydrate (NiCl2•6H2O, green). - and cobalt(II) chloride hexahydrate (CoCl2•6H2O). - Covalent Bonding. - Sharing of electrons Sharing of electrons. - A covalent bond is formed when two atoms share one or more pairs of electrons.. - Covalent bonding occurs when the lectronegativity difference between elements (atoms) is zero or relatively small.. - Is O=O expected to be. - valence shell electrons = Group A. - Shell Model of the Atom Shell Model of the Atom. - Lewis Structures Lewis Structures. - In compound formation an atom gains or loses electrons, or shares pairs of electrons, until its valence shell has eight electrons.. - Lewis Structures. - Multiple Covalent Bonds Multiple Covalent Bonds. - Double bond: 2 pairs shared. - Triple bond: 3 pairs shared. - a C atom and a N, O or S atom a N atom and a O or S atom. - a S atom and an O atom. - 3 bond pairs. - 1 lone pair =>. - Shape: IF Shape: IF5 5. - 1 lone pair =>. - Shape: IF. - 4 bond pairs. - 2 lone pairs =>. - AB4E2 square planar shape. - 0 lone pairs =>. - trigonal planar shape. - What would be expected to be the shape of chloroform, CHCl3?. - square planar tetrahedral. - Sigma Bond Sigma Bond σ σ. - Bond with the greatest electron density on a line connecting the atomic nuclei. - s-s type p-p type s-p type. - s-sp3 type s-sp2 type s-sp type. - p-sp3 type p-sp2 type p-sp type. - sp3 - sp3 type sp2-sp2 type sp-sp type. - Pi Bond Pi Bond π π. - Bond with the greatest electron density above and below a line connecting the atomic nuclei. - Bonding in Ethylene Bonding in Ethylene. - Bonding in Acetylene Bonding in Acetylene. - Dipole-Dipole Forces Dipole-Dipole Forces. - Hydrogen Bonds Hydrogen Bonds. - masses yet the boiling point for water is approximately 200oC higher than that for methane. - The higher boiling point is due to:. - hydrogen bonding in water polarity of water molecules. - both of the above none of the above
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