Question

Procedure: For Part 1, write the Lewis Dot (or Electron Dot) structure for each atom, followed by the ions that each element would form, the compound that would be formed from the combination of the two elements and finally the Lewis Dot structure for the compound.

For Part 2, show the Lewis Dot structure for each molecules, its AXE designation and finally its Electron Pair/ Geometric Shape geometries. Also indicate any partial charges that may exist on that molecule.

PART 1: IONS AND IONIC BONDING

Lewis Dot for atoms Ions formed Formula for compound Lewis Dot for compound

Li F

K O

Na N

Mg Cl

Ca S

Al Br

Mg P

PART 2: LEWIS STRUCTURES AND GEOMETRY FOR MOLECULES

Lewis structure/ AXE / Electron Pair Geo./Geometric Shape

CH4

H2O

H3O+

HCl

NH3

H2CO

Cl2O

BrO3-

SO4 ^-2

CO2

HCN

CO

CCl4

C2H6

CO3 ^-2

NO2 ^-

SO2

C2H4

C2H2

N2H4

CF3Cl

ClO3 ^-

CH3OH

CF4

Question #1 :

Which of the molecules in this exercise have polar bonds, but the molecule itself is non-polar? What makes that molecule(s) non-polar?

**You should find nine (9) structures!. Remember that a difference of electronegativities greater than 0.1 determines a polar covalent bond, but a symmetrical structure will cancel bond polarity and be a non-polar molecule.**

Answer 1

Part-1:

Lewis dot for atoms: The number of valence electrons in an atom is equal to the number of electrons present in the outer most shell. e.g K, Na etc. have 1 (group-1 element), O, S etc. have 6 (group 16 element), F, Cl, Br etc. have 7 (group-17)

Ions formed: When a metallic atom loss electrons, cation is formed. The number of electrons lost by a cation is equal to the valence electrons. The charge of a cation is equal to the number of atoms lost.

When a non-metallic atom loss electrons, anion is formed. A non-metal gains electrons till it completes octet. The charge of a anion is equal to the number of atoms gained.

Formula of compound: Exchange the magnitude of charge and write them as subscript to get the formula of the compound.

Part-2: