Ionization energy - energy required to remove an electron, Electronegetivity - Attraction of the nucleus of an atoms to another atoms electrons , Atomic radius - The distance of an atoms nucleus to its valance electrons, Shielding effect - The weakening of the attraction of valance electrons to the nucleus due to inner electrons , Which Element has the highest Ionization energy? - Helium, Which Element has the highest electronegetivity - Florine, Which Element has the largest atomic radius - Francium(Hint-Francium has the lowest electronegativity=low attraction), As Ionization Energy Increases - the attraction of the nucleus to valance electrons increases, As Ionization Energy decreases - the atom is more likely to give up its valance electrons, As electronegetivity increases - The attraction of the nucleus to electrons of other atoms increases, As electronegativity decreases - the atom is less strongly attracting electrons of other atoms, Ionic bonding - One atom gives up its electron-other gains an electron, Covalent bonding - Atoms share electrons, Do atoms with significantly different electronegativities gain/loose electrons or share them?  - gain/loose(ionic bonding), Do atoms with similar electronegativities gain/loose electrons or share them? - share them(covalent bonding, Hallogens - Very reactive, high ionization energy and high electronegetivity, Alkali metals - Very reactive, low ionization energy and low electronegetivity, Nobel gasses - energetically most stable, high ionization energy, When is an atom in its most energetically favorable form - When it has a full shell of valance elctrons(8), When is the atomic radius of an atom the smallest - When it has a high electronegativity with as close to a full shell of valance electrons as possible,

Periodic Trends

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