How to draw a Lewis dot structure....
the combustion reaction of ethylene produces 11.7 grams of water. how many of ethylene were is the reaction
Lewis dot structure in this find out number of electron not bonded lets take so4 charge of O= -2x4= -8 s can attain maximum charge 6 so 2 will be free in oxygen so make 8 dots around hydrogen and 6 around sulphur then join one electron of oxygen with sulphur at last you will have 2 unpaired electron so there you go that is your lewis dot structure
I D K S O R R Y M A N ;(
Drawing a Lewis dot structure is a way of representing the valence electrons of an atom or molecule. Here's a step-by-step guide on how to draw a Lewis dot structure:
1. Determine the total number of valence electrons: Look at the periodic table to find the group number (also known as the family number) of the element you are drawing the structure for. The group number represents the number of valence electrons. For example, oxygen is in group 16, so it has 6 valence electrons.
2. Identify the central atom: In most cases, one atom will serve as the central atom, and the others will be bonded to it. The central atom is usually the least electronegative element, except hydrogen. However, not all molecules have a central atom. Some molecules are symmetrical and do not possess a central atom. It's important to identify the central atom before proceeding.
3. Distribute electrons around the central atom: Start by placing one electron around each atom connected to the central atom. Once all atoms are given one electron, subtract the number of electrons used from the total number of valence electrons. Distribute the remaining electrons around the atoms, usually starting with the outer atoms. Aim to satisfy the octet rule (except for elements like hydrogen and helium), where each atom (except for hydrogen) wants 8 electrons in its valence shell to achieve stability.
4. Create double or triple bonds (if needed): If the central atom does not have an octet after distributing all the valence electrons, you can form double or triple bonds. Convert one or more lone pairs of electrons on the surrounding atoms into bonds to satisfy the octet rule. Remember that double bonds consist of two pairs of shared electrons, and triple bonds consist of three pairs of shared electrons.
5. Check the formal charges: Calculate the formal charges of each atom in the structure. The formal charge is the difference between the number of valence electrons an atom should have and the number it actually has in the Lewis structure. An optimal Lewis structure should have minimal formal charges or the most stable arrangement of charges.
6. Review the Lewis structure: Examine the Lewis dot structure for any errors or inconsistencies. Make sure each atom has the correct number of electrons and formal charges are as close to zero as possible.
Remember, Lewis dot structures are a simplified representation of the valence electron distribution and are useful for understanding bonding in molecules. They do not provide a complete picture of molecular geometry or represent the 3D structure accurately.