Lewis structure

Question 1

what are the rules to the lewis structures?

Answer 1

1. you want the formal charge of the compound to be very small or equal to zero.
2. like charges should not be close to each other (repel)
3. the more electronegative atom has the lowest formal charge.

Question 2

What are valence electrons?

Answer 2

1. These are charges located on the farthest shell of the element that usually for chemistry
   
   1. You can tell from the periodic table the charge of a compound by by looking at the group.

Question 3

What is the octect rule? and what are the exceptions?

Answer 3

1. This is a rule that allows atoms to be stable by allowing their last shell to have only 8 electrons. All atoms want in one way or another to resemble the noble gases. So they would do anythin necessary
2. Exception to the octect rule
   
   1. Helium Noble gases: this is a noble gas that only have 2 electron in it’s most outershell to be comfortable.
      
      1. Group 1: Hydrogen and Lithium want to resemble Helium so they only need 2 electron to be comfortable
      2. Groups 2: all elements in the group 2 want to also resemble Helium therefore they give off 2 electrons to do so
   2. Group 3: they need 6 valence electron to be stable they have 3 valence electrons in their outer shells. Whenever they have 6 their formal charge is zero.
   3. Explanded octect rules: elements in the 3 period and pass Si ( Silicon and below can expand)
      
      1. can have either 10 electrons or 12 electrons
      2. common expanded octects:
         
         1. PCL5
         2. SF6
         3. Br Fl3
         4. Xe F4

Question 4

How to calculate formal charges?

Answer 4

1. Formal charges: valence (oxidation number)- (non-binding electron (lone pair))- Bonding e (the elctron bonded and the electron of the other atom)/ 2