Draw the lewis structure for:
SiO3 -2
CNO-
TeO4 -2
F2PPCl2
thanks!
http://misterguch.brinkster.net/lewisstructures.html
To draw the Lewis structure for each molecule/ion, you need to follow some rules:
1. Count the total number of valence electrons in the molecule/ion. For atoms, you can find this number by referring to the periodic table. For ions, you need to consider their charges.
2. Arrange the atoms in the molecule/ion so that the more electronegative element is in the center. For polyatomic ions, the central atom is usually the one with the highest valence.
3. Connect the central atom(s) to the surrounding atoms using single bonds.
4. Distribute the remaining electrons as lone pairs to fulfill the octet rule (except for hydrogen, which can only have 2 electrons).
5. If there are still unaccounted electrons, place them as lone pairs on the central atom.
Now, let's draw the Lewis structures for the given compounds:
1. SiO3^2-
- Silicon (Si) is the central atom since it is less electronegative than oxygen (O).
- The total number of valence electrons is: 4 (Si) + 3(6) (O) + 2 (negative charge) = 32.
- Connect the Si with the O atoms using single bonds.
- Distribute the remaining electrons as lone pairs on the O atoms.
O-Si-O
|
O
2. CNO^-
- Carbon (C) is the central atom since it is less electronegative than nitrogen (N) and oxygen (O).
- The total number of valence electrons is: 4 (C) + 5 (N) + 6 (O) + 1 (negative charge) = 16.
- Connect the C with the N and O atoms using single bonds.
- Distribute the remaining electrons as lone pairs on the O atom.
O=C=N
3. TeO4^2-
- Tellurium (Te) is the central atom since it is less electronegative than oxygen (O).
- The total number of valence electrons is: 6 (Te) + 4 (6) (O) + 2 (negative charge) = 32.
- Connect the Te with the O atoms using single bonds.
- Distribute the remaining electrons as lone pairs on the O atoms.
O
|
O-Te-O
|
O
4. F2PPCl2
- Here, we can assume that P (phosphorus) is the central atom.
- The total number of valence electrons is: 2 (F) + 5 (P) + 2 (2 x P) (Cl) = 16.
- Connect P with the F and Cl atoms using single bonds.
- Distribute the remaining electrons as lone pairs on the P atom.
F-P-Cl
|
F
Remember that Lewis structures are a simple representation of molecules, showing only the valence electrons and connectivity between atoms. The actual bond angles and molecular geometry may vary.
To draw the Lewis structure for each compound, we need to know the number of valence electrons for each atom in the compound.
For SiO3^2-:
Silicon (Si) has 4 valence electrons, and each Oxygen (O) has 6 valence electrons. Since there are three Oxygens, the total number of valence electrons is 4 + (6 * 3) + 2 (charge) = 24.
Here's the step-by-step process for drawing its Lewis structure:
1. Place the least electronegative atom (Si in this case) in the center.
O
/
Si
\
O
/
O-
2. Connect the O atoms to the Si atom with a single bond (using 2 electrons for each bond):
O
/
Si
\
O--O
3. Place the remaining electrons around the atoms to satisfy the octet rule:
O
/
Si
\
O=O
For CNO^-:
Carbon (C) has 4 valence electrons, Nitrogen (N) has 5 valence electrons, and Oxygen (O) has 6 valence electrons. Since there is an extra electron due to the negative charge, the total number of valence electrons is 4 + 5 + 6 + 1 (charge) = 16.
Here's the step-by-step process for drawing its Lewis structure:
1. Place the least electronegative atom (C in this case) in the center.
N
/ \
C O
2. Connect the atoms with single bonds (using 2 electrons for each bond):
N
/ \
C---O
3. Place the remaining electrons around the atoms to satisfy the octet rule:
N
/ \
C=O
For TeO4^2-:
Tellurium (Te) has 6 valence electrons, and each Oxygen (O) has 6 valence electrons. Since there are four Oxygens, the total number of valence electrons is 6 + (6 * 4) + 2 (charge) = 32.
Here's the step-by-step process for drawing its Lewis structure:
1. Place the least electronegative atom (Te in this case) in the center.
O
/ \
O O
/ \
O Te
2. Connect the O atoms to the Te atom with a single bond (using 2 electrons for each bond):
O
/ \
O O
/ \
O---Te
3. Place the remaining electrons around the atoms to satisfy the octet rule:
O
/ \
O=Te=O
\ /
O
For F2PPCl2:
Fluorine (F) has 7 valence electrons, Phosphorus (P) has 5 valence electrons, and Chlorine (Cl) has 7 valence electrons. The number of valence electrons in this compound would be (7 * 2) + 5 + (7 * 2) = 33.
Here's the step-by-step process for drawing its Lewis structure:
1. Place the least electronegative atom (P in this case) in the center.
F F
| |
P Cl
|
F F
2. Connect the atoms with single bonds (using 2 electrons for each bond):
F F
| |
P---Cl
|
F F
3. Place the remaining electrons around the atoms to satisfy the octet rule:
F F
| |
F--P---Cl
|
F F
Note: Keep in mind that the Lewis structures only provide a two-dimensional representation of the molecule or ion, and the actual shape may differ in three dimensions.