Write Lewis structures for the following: (a) \(\mathrm{H}_{2} \mathrm{CO}\) (both \(\mathrm{H}\) atoms are bonded to $\mathrm{C} \mathrm{)},(\mathbf{b}) \mathrm{H}_{2} \mathrm{O}_{2},(\mathbf{c}) \mathrm{C}_{2} \mathrm{~F}_{6}($ contains a \(\mathrm{C}-\mathrm{C}\) bond $),(\mathbf{d}) \mathrm{AsO}_{3}^{3-},(\mathbf{e}) \mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{H}$ is bonded to \(\mathrm{O})\) (f) \(\mathrm{NH}_{2} \mathrm{Cl}\).

#tag_title#Lewis Structure for C2F6 (Hexafluoroethene)#tag_content#Total valence electrons: 2 * 4 (from C) + 6 * 7 (from F) = 44 valence electrons Central atoms: Carbon (C) and Carbon (C) 1. Connect the C atoms with a single bond: C-C 2. Connect the F atoms to the central C atoms: F-C-F and F-C-F 3. Assign the remaining electrons: add three lone pairs to each F atom. The octet rule is satisfied for all atoms. 4. Formal charges: all atoms have a formal charge of zero. Final Lewis structure: F-C-F / F-C-F #tag_title#Lewis Structure for AsO3^{3-} (Arsenite Ion)#tag_content#Total valence electrons: 5 (from As) + 3 * 6 (from O) + 3 (from negative charge) = 24 valence electrons Central atom: Arsenic (As) 1. Connect 2 O atoms to the central As atom 2. Add one O with a double bond: O=As-O 3. Assign the remaining electrons: add lone pairs on 2 O atoms and 1 lone pair on As. The octet rule is satisfied for all atoms. 4. Formal charges: -1 on each O with a single bond, 0 on O with a double bond, and 1 on As. Final Lewis structure: (O^{-})-As(=O)-O^{-} Multiple resonance structures are possible #tag_title#Lewis Structure for H2SO3 (Sulfurous Acid)#tag_content#Total valence electrons: 6 (from S) + 2 * 1 (from H) + 3 * 6 (from O) = 24 valence electrons Central atom: Sulfur (S) 1. Connect the two H atoms to one of the O atoms: S-O 2. Connect the other two O atoms with single bonds: HO-S-O 3. Assign the remaining electrons: add two lone pairs to each oxygen. The octet rule is satisfied for S and O. 4. Formal charges: 0 on S, -1 on O with a single bond, and 1 on O with H. Final Lewis structure: HO-S(=O)-O-H #tag_title#Lewis Structure for NH2Cl (Chloramine)#tag_content#Total valence electrons: 5 (from N) + 2 * 1 (from H) + 7 (from Cl) = 14 valence electrons Central atom: Nitrogen (N) 1. Connect the H atoms to the central N atom 2. Connect the Cl atom to the central N atom with a single bond 3. Assign the remaining electrons: add two lone pairs to Cl and one lone pair on N. The octet rule is satisfied for all atoms. 4. Formal charges: all atoms have a formal charge of zero. Final Lewis structure: H-N-Cl-H