Section 9.5 Electronegativity = ? –Ability to attract electrons When atoms react, the electronegativity between atoms will determine which type of bond.

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Presentation transcript:

Section 9.5 Electronegativity = ? –Ability to attract electrons When atoms react, the electronegativity between atoms will determine which type of bond is formed

Predicting Bond Type Calculate the difference between electronegativities of the elements 1.7 to 4.0 = ionic bond Large differences indicate a transfer of electrons

To calculate difference between electronegativity 1.7 to 4.0 = ionic bond NaCl – 0.9 = 2.1

If difference is between 0.3 and 1.7  polar covalent Electronegativity difference is not strong enough for a transfer of electrons

Electrons are shared Unequal sharing of electrons because one atom is more electronegative Electrons spend more time around the more electronegative element and molecules becomes polar Polar Covalent

For example… H2OH2O – 2.1 = 1.4

If electronegativity difference is between 0 and 0.3  nonpolar covalent Atoms are approximately equal in electronegativies Most common in diatomic molecules and hydrocarbons

N2N – 3.0 = 0 N

Difference in all of the bonds… IonicPolar CovalentNon-Polar Covalent 1.7   1.70  0.3 High melting point Low melting point SolidsSolids and liquids Liquids and gases No dipolesDipolesNo dipoles Dissolves in polar covalent Dissolve in nonpolar covalent

ChargeElectro- negativity Elements+_Formula+_DifferenceBond Li + Br H + Br C + O K + O C + Cl Na + Cl

ChargeElectro- negativity Elements+_Formula+_DifferenceBond Ca + P Si + F C + N K + O C + I H + P