3.1.3.6 Bond Polarity
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What is electronegativity?
The ability of an atom to attract the pair of electrons in a covalent bond
What does electronegativity depend on?
Nuclear charge Inner shielding Distance factor
Why are smaller atoms more likely to attract electrons?
Because the nucleus is closer to the outer shell and so the larger the attractive force and the bigger the electronegativity
How does electronegativity change on the periodic table?
Left to right: electronegativity increases Up to down: electronegativity decreases
What is the most electronegative element?
Fluorine
What group of the periodic table doesn’t have an electronegativity?
Group 0: the noble gases
What is the continuum?
Which one atom is more electronegative, the electrons are drawn closer within the bond to the one with the higher electronegativity
What are the electronegativity ranges for the type of covalent bond?
Non-covalent (ionic): 2 + Nonpolar covalent: 0.0 - 0.3 Polar covalent: 0.4 - 2.0
What is bond polarity?
How electrons are shared between two atoms in a covalent bond due to the difference in electronegativities
What factors increase polarisation?
For positive ions: small size, high charge For negative ions: large size, high charge