I do not understand polar covalent bonds.?
Answer:
H-Cl is a polar covalent bond because of the difference in electronegativities of the two atoms. It is a covalent bond because the difference is not exceedingly great, however.
Neither is a metal, they are both nonmetals. I included a link to a table of electronegativity values for your reference.
H is not a metal.
Electronegativity of H = 2.1
Electronegativity of Cl = 3.0
3.0 - 2.1 < 2 so it is not an ionic bond
You can find on :
http://members.aol.com/profchm/covalent.
Actually electronegativity above 2 would be considered ionic. It’s polar-ionic
electronegativity of the two elements is what determines the covalence or ionization of bonding.
Cl = 3.16 H= 2.2
3.16-2.2 ~1
Non-polar covalent bond: 0.0-0.4
Slightly polar bond: 0.5-0.9
Moderately polar bond: 1-1.3
Highly polar bond: 1.4-1.7
Slightly ionic bond: 1.8-2.2
Ionic Bond: 2.3+
moderately polar!
H and Cl are both nonmetals, so there is no contradiction. You may be thinking of the rule that the left two thirds of the periodic table are metals, and H is in the upper left corner. However, H is an exception to this rule because it is the first element and could equally well be placed over the halogens.
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