Draw the Lewis structure of NO2-
Assign formal charges to each atom in the O3 molecule shown below. Be sure to click the +/- button below (it will turn yellow when activated) before clicking on the molecule.
.. .. ..
:O--O==O
.. ..
Based on formal charges, what is the best Lewis structure for CLO^3-
*Include lone pairs of electrons and formal charges
PLEASE HELP WITH THESS 3Q PLEASE!!!!
the first oxygen has a -1 charge, the second oxygen has a +1 charge, and the last oxygen has a 0 charge.
Draw the Lewis structure of NO2-
Assign formal charges to each atom in the O3 molecule shown below. Be sure to click the +/- button below (it will turn yellow when activated) before clicking on the molecule.
.. .. ..
:O--O==O
.. ..
Based on formal charges, what is the best Lewis structure for CLO^3-
*Include lone pairs of electrons and formal charges
PLEASE HELP WITH THESS 3Q PLEASE!!!!
:N::O
 ..
 :O:
  ..
I'll see how this looks and do another one.
:N::O:
  ..
  :O:
  ..
If I can read what you intended to type for O3, the left O has a FC of -1, the middle one has a FC of -1 and the right O has a FC ;of +2.
ok so if the N is double bonded to the left O and single bonded to the right O , and N has a lone pair.. does that mean that the left O also has a lone pair and 3 lone pairs in the right side according to ur diagram.. also for the second Q .. (in my diagram i intended to draw .. 3 Os : the middle O is double bonded to right O and single bonded to the left O ..the left O has 3 lone pairs and the middle O has 1 lone paire and the right O has 2 lone pairs ... therfore the formal charges can't be -1,-1,+2 .. also i still don't get the third Q ...
Please help !!
study real hard
bkonoijohiughb
Sure, I'd be happy to help you with these questions!
1. Lewis structure of NO2-:
To draw the Lewis structure of NO2-, we first need to know the number of valence electrons in each atom. Nitrogen (N) is in Group 5A, so it has 5 valence electrons, and oxygen (O) is in Group 6A, so it has 6 valence electrons each.
Step 1: Count the total number of valence electrons. In NO2-, there is one nitrogen atom and two oxygen atoms, so we have:
1 nitrogen atom × 5 electrons = 5 electrons
2 oxygen atoms × 6 electrons = 12 electrons
Total = 5 + 12 = 17 electrons
Step 2: Determine the central atom. The central atom is the one with the lowest electronegativity, which in this case is nitrogen.
Step 3: Connect the atoms. Place the central atom (nitrogen) in the center and connect it with single bonds to the surrounding oxygen atoms. Remember to use a line to represent a single bond, and each line represents two electrons.
Step 4: Distribute the remaining electrons. Fill the octet of each atom by placing the remaining electrons around the atoms. If there are still extra electrons, place them on the central atom. If there are fewer than 8 electrons around the central atom (except hydrogen), try using multiple bonds (double or triple bonds) to satisfy the octet rule.
After following these steps, the Lewis structure of NO2- is:
..
:N=O:
..
2. Formal charges on O3 molecule:
Formal charge is a way to determine the distribution of electrons in a molecule. It is calculated by subtracting the number of valence electrons around an atom in its neutral form from the number of lone pair electrons plus half the number of shared electrons.
In the O3 molecule, we have three oxygen atoms.
Step 1: Count the total number of valence electrons. Each oxygen atom has 6 valence electrons, so for the O3 molecule, we have:
3 oxygen atoms × 6 electrons = 18 electrons
Step 2: Determine the formal charges. To assign the formal charges to each oxygen atom, we need to determine the number of valence electrons each oxygen atom "should have" (based on the octet rule) and compare that with the actual number of valence electrons.
In the Lewis structure of O3, each oxygen atom forms a single bond with the other two oxygen atoms. Therefore, the number of valence electrons each oxygen atom should have is: 6 valence electrons + 1 bond electron = 7 electrons.
By comparing this with the actual number of valence electrons, we can assign the formal charges to each oxygen atom.
For the Lewis structure given:
O:O=O with a double bond between O1 (left) and O2 (right) and a single bond between O2 and O3, we have:
..
:O--O==O:
..
Step 3: Calculate the formal charges. To do this, we use the formula: Formal charge = Valence electrons - Lone pair electrons - Shared electrons/2
For O1, the oxygen on the left side:
Valence electrons: 6
Lone pair electrons: 0
Shared electrons: 2 (one bond shared with O2)
Formal charge = 6 - 0 - 2/2 = 5/2 = +1/2
For O2, the oxygen in the center:
Valence electrons: 6
Lone pair electrons: 0
Shared electrons: 4 (two bonds shared with O1 and O3)
Formal charge = 6 - 0 - 4/2 = 6 - 2 = +2
For O3, the oxygen on the right side:
Valence electrons: 6
Lone pair electrons: 0
Shared electrons: 2 (one bond shared with O2)
Formal charge = 6 - 0 - 2/2 = 5/2 = +1/2
Therefore, the formal charges for the O3 molecule are:
O1: +1/2
O2: +2
O3: +1/2
3. Best Lewis structure for CLO3-:
To determine the best Lewis structure for CLO3-, we need to assign formal charges and consider the stability of the structure.
Step 1: Count the total number of valence electrons. Chlorine (Cl) is in Group 7A, so it has 7 valence electrons, oxygen (O) is in Group 6A, so it has 6 valence electrons each, and the negative charge (-1) adds 1 more electron.
For CLO3-, we have:
1 chlorine atom × 7 electrons = 7 electrons
3 oxygen atoms × 6 electrons = 18 electrons
1 extra electron from the negative charge = 1 electron
Total = 7 + 18 + 1 = 26 electrons
Step 2: Determine the central atom. The central atom is the one with the lowest electronegativity, which in this case is chlorine.
Step 3: Connect the atoms. Place the central atom (chlorine) in the center and connect it with single bonds to the surrounding oxygen atoms. Remember to use a line to represent a single bond, and each line represents two electrons.
Step 4: Distribute the remaining electrons. Fill the octet of each atom by placing the remaining electrons around the atoms. If there are still extra electrons, place them on the central atom. If there are fewer than 8 electrons around the central atom (except hydrogen), try using multiple bonds (double or triple bonds) to satisfy the octet rule.
After following these steps, we can determine that the best Lewis structure for CLO3- is:
..
.. :O--Cl--O:
.. ..
I hope this helps! Let me know if you have any further questions.
You can see the problem.
Add two electron to top of top O.
The other electrons are around the lower O with two of them shared with N. The entire ion has a -1 charge on it.