Draw the Lewis structure of H2O. Include any nonbonding electron
pairs.
Draw the molecule by placing atoms on the grid and connecting
them with bonds. Include all lone pairs of electrons.
Part B
What is the electronic geometry of H2O?
Enter the electronic geometry of the molecule.
Part C
What is the electronic geometry of ClF3?
Enter the electronic geometry of the molecule.
Part D
What is the electronic geometry of BBr3?
Draw the Lewis structure for AsF3
Draw the Lewis dot structure. To change the symbol of an atom,
double-click on the atom and enter the letter of the new atom.
Draw the Lewis structure for CH3+. Be sure to show the formal
charge on any atom that has a non-zero formal charge.
Draw the Lewis dot structure.
Draw the Lewis structure for BrF3
Draw the Lewis dot structure.
Draw a Lewis structure for each of the following compounds:(a) C_22H_66 \hspace{.2cm} (b) C_22H_44 \hspace{.2cm} (c) C_22H_22 \hspace{.2cm} (d) C_33H_88 \hspace{.2cm} (e) C_33H_66 \hspace{.2cm} (f) CH_33OH
Draw a Lewis structure for each of the following compounds:(a) C_22H_66 \hspace{.2cm} (b) C_22H_44 \hspace{.2cm} (c) C_22H_22 \hspace{.2cm} (d) C_33H_88 \hspace{.2cm} (e) C_33H_66 \hspace{.2cm} (f) CH_33OH
Compare and contrast the lewis dot structure for N3- and I3-.
Based on your assessment of structure and formal charge(s), what
would you suggest about the relative stabilities of the two
ions?