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POLAR BONDING results when two different non-metals unequally share electrons between them.<br />
One well known exception to the identical atom rule is the combination of carbon and hydrogen in all<br />
organic compounds.<br />
The non-metal closer to fluorine in the Periodic Table has a greater tendency to keep its own electron<br />
and also draw away the other atom's electron. It is NOT completely successful. As a result, only<br />
partial charges are established. One atom becomes partially positive since it has lost control of its<br />
electron some of the time. The other atom becomes partially negative since it gains electron some of<br />
the time.<br />
Hydrogen Chloride<br />
Hydrogen Chloride forms a polar covalent molecule. The graphic<br />
on the left shows that chlorine has 7 electrons in the outer shell.<br />
Hydrogen has one electron in its outer energy shell. Since 8<br />
electrons are needed for an octet, they share the electrons.<br />
However, chlorine gets an unequal share of the two electrons,<br />
although the electrons are still shared (not transferred as in ionic<br />
bonding), the sharing is unequal. The electrons spends more of the<br />
time closer to chlorine. As a result, the chlorine acquires a "partial"<br />
negative charge. At the same time, since hydrogen loses the<br />
electron most - but not all of the time, it acquires a "partial" charge.<br />
The partial charge is denoted with a small Greek symbol for delta.<br />
Water<br />
Water, the most universal compound on all of the earth, has the property of<br />
being a polar molecule. As a result of this property, the physical and<br />
chemical properties of the compound are fairly unique.<br />
Dihydrogen Oxide or water forms a polar covalent molecule. The graphic on<br />
the left shows that oxygen has 6 electrons in the outer shell. Hydrogen has<br />
one electron in its outer energy shell. Since 8 electrons are needed for an<br />
octet, they share the electrons.<br />
Notes Section:<br />
Formula charges 3 steps:<br />
1- Count Valence electrons<br />
2- Find central atom, Subtract electrons in bonds from the total, Add Lone pairs to the compound,<br />
Add LP & Double/Triple Bonds (Steps 2-8)<br />
3- Find formal charges. Get the charges as close to zero as possible by moving electrons and bonds<br />
A central atom in period two can be an exception to the octic rule<br />
Covalent bonding- non-metals with a bond of 2 electrons being shared between 2 atoms, neither atom fully gaining/losing a<br />
2 types of covalent bonding: Polar and Non-polar<br />
Non-polar: Two atoms of the same non-metal equally sharing electrons.<br />
Polar: Two different non-metals unequally sharing electrons, with the more electronegative being partially negative, the less<br />
partially positive.<br />
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