Here is my guide for drawing structural formulas:
After the guide, I will go thru the procedure for the carboxyl group.
You will need an Electronegativity Table to do step 2.
Structural Formulas
1. Write the formula of the compound.
2. Draw the possible picture with the least electronegative atom in the center.
3. Count the number of valence electrons for each atom. (This is the same as the column number.If you are drawing the structural formula for a polyatomic ion, add 1 e- for each -1 charge or subtract 1 e- for each +1 charge.
4. Multiply the total number of atoms by 8 since each atom needs an octet to be stable. (except for Hydrogen atoms which you multiply by 2)
5. Subtract #4 - #3 to determine the number of electrons to be shared as bonding pairs.
6. Divide this number by 2 (2 e-'s make a bond) to determine the number of
bonds needed.
7. Place these bonds between the atoms. One line represents a bond (2e-'s)
8. Place enough electron pairs around each atom to make an octet(except
hydrogen only needs 2e-'s) One line represents a pair of e-'s.
9. Check to make sure the number of electrons used equals the number of valance electrons available .(#3)
10. Check the shape. Electron pairs repel each other, so make the bonds as far away from each other as possible.
How many polar covalent bonds in carboxyl group?
The Carboxyl ion is CO3^-2
3) Determine the total number of valence electrons, which for elements in the 8 columns that make up the s2 p3 orbitals is the same as the column number.
C = 4
O = 6…3 O's = 18
-2 charge means 2 extra electrons
Total = 24 electrons
4) Multiply the total number of atoms by 8 since each atom needs an octet to be stable. (except for Hydrogen atoms which you multiply by 2)
4 atoms * 8 electrons per atom (octet) = 32
5) Subtract #4 - #3 to determine the number of electrons to be shared as bonding pairs
32 - 24 = 8 electrons to be shared as bonding pairs
6) Divide this number by 2 (2 e-'s make a bond) to determine the number of
bonds needed. 8 ÷ 2 = 4 bonds
7) Place these bonds between the atoms. One line represents a bond (2e-'s)
There are 3 O's bonded to 1 C. There are 4 bonds, 2 single bonds to 2 O's and a double bond to the other O. The molecule is Y shaped.
Yes...hydrogen fluoride (HF) has polar covalent bonds
Molecular substances can have both polar and nonpolar covalent bonds.
Hydrogen peroxide has both polar covalent bonds (-OH bonds) and non polar covalent bonds (O-O bond).
Sulfur dioxide is a polar molecules with polar covalent bonds.
Within the molecule, the bonds are covalent bonds. Between water molecules, they're hydrogen bonds.
H2O has polar covalent bonds, not non-polar covalent bonds.
Ionic bonds, Covalent bonds, Hydrogen bonds, Polar Covalent bonds, Non-Polar Covalent bonds, and Metallic bonds.
polar bonds are non metals bonded to non metals and non polar covalent bonds are bonds sharing electrons.....
Yes...hydrogen fluoride (HF) has polar covalent bonds
Molecular substances can have both polar and nonpolar covalent bonds.
Hydrogen peroxide has both polar covalent bonds (-OH bonds) and non polar covalent bonds (O-O bond).
Sulfur dioxide is a polar molecules with polar covalent bonds.
When electrons are shared, covalent bonds are formed. Covalent bonds are of two types, polar and non-polar. A complex type of covalent bonds are co-ordinate covalent bonds or dative bonds.
Within the molecule, the bonds are covalent bonds. Between water molecules, they're hydrogen bonds.
polar
polar
Covalent - Acids don't have metals in them, so they have covalent bonds.