How do you draw the Lewis Structure for SO4,SF6,NH3 and H2S
Maybe chemistry??
Assistance needed.
Please type your subject in the School Subject box. Any other words are likely to delay responses from a teacher who knows that subject well.
Since this is not my area of expertise, I searched Google under the key words "Lewis structure" to get these possible sources:
http://en.wikipedia.org/wiki/Lewis_structure
http://www.ausetute.com.au/lewisstr.html
http://www.stolaf.edu/depts/chemistry/courses/toolkits/123/js/lewis/
http://www.chem.lsu.edu/htdocs/people/sfwatkins/MERLOT/drawlewis/dls.html
http://antoine.frostburg.edu/chem/senese/101/bonds/faq/simple-lewis-structures.shtml
In the future, you can find the information you desire more quickly, if you use appropriate key words to do your own search. Also see http://hanlib.sou.edu/searchtools/.
I hope this helps.
To draw the Lewis Structure for molecules like SO4, SF6, NH3, and H2S, you need to follow a few steps:
1. Determine the total number of valence electrons:
- For SO4, sulfur (S) is in Group 6A (16 valence electrons) and there are four oxygen (O) atoms (6 valence electrons each). So, the total is 16 + (4 × 6) = 40 electrons.
- For SF6, sulfur (S) is in Group 6A (16 valence electrons) and there are six fluorine (F) atoms (7 valence electrons each). So, the total is 16 + (6 × 7) = 58 electrons.
- For NH3, nitrogen (N) is in Group 5A (5 valence electrons) and there are three hydrogen (H) atoms (1 valence electron each). So, the total is 5 + (3 × 1) = 8 electrons.
- For H2S, sulfur (S) is in Group 6A (6 valence electrons) and there are two hydrogen (H) atoms (1 valence electron each). So, the total is 6 + (2 × 1) = 8 electrons.
2. Choose a central atom:
- In SO4, sulfur (S) is the central atom since it is the least electronegative and can make multiple bonds.
- In SF6, sulfur (S) is also the central atom.
- In NH3, nitrogen (N) is the central atom since it is the least electronegative and can make multiple bonds.
- In H2S, sulfur (S) is the central atom since it is the least electronegative and can make multiple bonds.
3. Arrange the atoms around the central atom:
- For SO4, place the four oxygen (O) atoms around sulfur (S) using single bonds.
- For SF6, arrange six fluorine (F) atoms around sulfur (S) using single bonds.
- For NH3, place the three hydrogen (H) atoms around nitrogen (N) using single bonds.
- For H2S, place the two hydrogen (H) atoms around sulfur (S) using single bonds.
4. Distribute the remaining electrons:
- For SO4, distribute the remaining electrons so that each oxygen atom has a full octet by forming double bonds with sulfur (S).
- For SF6, sulfur (S) can expand its octet since it is in the third period. Distribute the remaining electrons so that sulfur (S) has a full octet, with all six fluorine (F) atoms using single bonds.
- For NH3, distribute the remaining electrons so that nitrogen (N) has a full octet, and each hydrogen (H) atom has a full duet.
- For H2S, distribute the remaining electrons so that sulfur (S) has a full octet, and each hydrogen (H) atom has a full duet.
5. Check the formal charges:
- Make sure the formal charges on each atom are minimized by redistributing the electrons as needed.
Completing these steps will yield the Lewis Structures for SO4, SF6, NH3, and H2S.