In the molecule HOCN (skeleton as written). Draw a Lewis structure that puts zero formal charge on all atoms. What orbitals overlap to make the C N sigma bond? O Csp? and Nsp² O Csp and Nsp O Csp°d and Nsp O Csp and Nsp3 O Csp? and Nsp O Cp and Np O Csp and Nsp O Csp and Nsp?

Write the Lewis structures for CH2N2, including all resonance forms, and show formal charges.

The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Use the References to access important values if needed for this question. We can draw three inequivalent Lewis structures for dinitrogen monoxide, N₂O . The concepts of formal charge and electronegativity can help us choose the structure that is the most significant representation. 1. Assign formal charges to the elements in each of the structures below. Formal Charge N₁ N₂ :N,=N,-O: || A N=N,=Ô N-N,=O: C 2. The structure that contributes most significantly to the overall electronic structure of N₂O is ↑ Formal Charge

What are the formal charges present in in the ion CH3NH3*? Assume all atoms other an hydrogen hau an octet and that there are two central atoms. O N is 0 and C is +1 O N is +1 and C is -1 O N is +1 and C is 0 O N is 0 and C is 0 O N is +2 and C is -1

Consider the SO 3 molecule. How many valence electrons does the molecule have?   How many lone pairs of electrons are on the central atom?   How many lone pairs of electrons in total are on the substituent atoms?   How many resonance structures can be drawn for the molecule?  If the ion doesn't exhibit resonance, indicate "1" as only one structure can be drawn for the molecule.

Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. a. SeO2 b. CO32- c. ClO- d. NO2-

Explain formation of covalent bonds in the following chemical compounds (using three theories). C2? · NO , NO2 , NaF , H2S

2. Use the data provided below to calculate the lattice energy of calcium chloride. Electron affinity of Cl = -348.7 kJ/mol 1st ionization energy of Ca = 590.0 kJ/mol 2nd ionization energy of Ca = 1145.0 kJ/mol Bond energy of Cl2 = 242.6 kJ/mol Sublimation energy of Ca = 178.0 kJ/mol AH¡ [CaCl. (s)] =-795.0 kJ/mol

Draw the Lewis structure for sulfate (SO4) with minimized formal charges. Provide an incorrect lewis structure for sulfate and explain why it is incorrect.

Write the Lewis structure for each ion. Include resonance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge. SO32-