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I. Periodic Trends Electron Negativity Metallic Property II. Periodic Table Non-Metallic Property Atomic Size/ Atomic Radius Ionic Size Cations<atom<anion Ionization energy Electron Affinity III. Periodic Law Mendeleev: “the properties of the elements are a periodic function of their atomic masses” 1914- Henry Moseley arranged the elements according to their increasing atomic numbers Moseley: “the properties of the elements are a periodic function of their atomic numbers” IV. Ionic Bonds - Bond between metal and non-metal LEDS: Lewis electron dot structure - - Transfer of electrons Very high melting and boiling points Compounds in the solid state are nonconductors of electricity while those in liquid or molten state are conductors of electricity Basis: static electrical attraction Groups: 1A 2A 3A 4A 5A V. Covalent Bonds - bond existing between two nonmetals - resulting compounds have low melting and boiling points and are nonconductors of electricity -sharing of electrons - the number of atoms that combine to form a covalent molecular compound is such that each atom would attain an octet -lone pair- non bonded pair of electrons -bond length- distance between the number of two boned atoms -single bond>double bond>triple bond -groups : 4A 5A 6A 7A -polar bond: 0.5- 1.8 - non polar bond: 0-0.4 -polar compound: shared unequally -non polar compound: shared equally VI. Molecular Geometry