Lewis Dot Structures A How To
Step 1 Count the total valence electrons for the molecule To do this, find the number of valence electrons for each atom in the molecule, and add them up.
CO 2 Step 1: Valance electrons is 16 Carbon has four electrons, and each of the oxygens have six, for a total of 4 + 12 = 16 electrons Example
Step 2 Figure out how many octet electrons the molecule should have, using the octet rule The octet rule tells us that all atoms want eight valence electrons (except for hydrogen, which wants only two), so they can be like the nearest noble gas. Use the octet rule to figure out how many electrons each atom in the molecule should have, and add them up. Another weird element is boron - it wants six electrons.
CO 2 Step 1: Valance electrons is 16 Step 2: The number of octet electrons is equal to 24. Carbon wants eight electrons, and each of the oxygens want eight electrons, for a total of 8+16 = 24 electrons Example
Step 3 Subtract the valence electrons from octet electrons Or, in other words, subtract the number you found in Step 1 above from the number you found in Step 2 above. The answer you get will be equal to the number of bonding electrons in the molecule.
CO 2 Step 1: Valance electrons is 16 Step 2: The number of octet electrons is equal to 24. Step 3: 8. The number of bonding electrons is equal to the octet electrons minus the valence electrons, 24 16 = 8. Example
Step 4 Divide the number of bonding electrons by two Remember, because every bond has two electrons, the number of bonds in the molecule will be equal to the number of bonding electrons divided by two.
CO 2 Step 1: Valance electrons is 16 Step 2: The number of octet electrons is equal to 24. Step 3: 8. Step 4: The number of bonds is equal to 4. The number of bonds is equal to the number of bonding electrons divided by two, because there are two electrons per bond. 8/2 = 4 Example
Step 5 Draw an arrangement of the atoms for the molecule that contains the number of bonds you found in #4 above Hydrogen and the halogens bond once. The family oxygen is in bonds twice. The family nitrogen is in bonds three times. So does boron. The family carbon is in bonds four times. A good thing to do is to bond all the atoms together by single bonds, and then add the multiple bonds until the rules above are followed.
CO 2 Step 1: Valance electrons is 16 Step 2: The number of octet electrons is equal to 24. Step 3: 8. Step 4: The number of bonds is equal to 4. Step 5: O=C=O, where carbon is doublebonded to both oxygen atoms. If we arrange the molecule so that the atoms are held together by four bonds, we find that the only way to do it so that we get the following pattern: O=C=O Example
Step 6 Find the number of lone pair (nonbonding) electrons by subtracting the bonding electrons (#3 above) from the valence electrons (#1 above). Arrange these around the atoms until all of them satisfy the octet rule Remember, ALL elements EXCEPT hydrogen & boron want eight electrons around them, total. Hydrogen only wants two electrons while boron wants six.
CO 2 Step 1: Valance electrons is 16 Step 2: The number of octet electrons is equal to 24. Step 3: 8. Step 4: The number of bonds is equal to 4. Step 5: O=C=O, where carbon is double-bonded to both oxygen atoms. Step 6: The number of nonbonding electrons is equal to the number of valence electrons (from #1) minus the number of bonding electrons (from #3), which in our case equals 16-8, or 8. Looking at our structure, we see that carbon already has eight electrons around it. Each oxygen, though, only has four electrons around it. To complete the picture, each oxygen needs to have two sets of nonbonding electrons, as in this Lewis structure. Example
Overall Steps 1) Count the total valence electrons for the molecule 2) Figure out how many octet electrons the molecule should have, using the octet rule 3) Subtract the valence electrons from octet electrons 4) Divide the number of bonding electrons by two 5) Draw an arrangement of the atoms for the molecule that contains the number of bonds you found 6) Find the number of lone pair electrons by subtracting the bonding electrons from the valence electrons Arrange these around the atoms until all of them satisfy the octet rule
Hydrogen peroxide, H 2 O 2 More Examples!
Sulfuric acid, H 2 SO 4 More Examples!
Sulfur Trioxide, SO 3 More Examples!
Boron Trifluorine, BF 3 More Examples!
Ammonia, NH 3 More Examples!
Ammonium, NH 4 + More Examples!
Carbonate, CO 3 - More Examples!
Nitrate, NO 3 - More Examples!
Glycine, an amino acid, C 2 H 5 NO 2 Challenge Example!
Alanine, an amino acid, C 3 H 7 NO 2 Challenge Example!