Aluminum chloride, AlCl³, is used in a variety of organic reactions as a Lewis acid. Although it adopts a more complex geometry in the solid state, consider it as a single molecule (i.e., in the gas phase). AICI3 has 24 total valence electrons. Draw the Lewis structure for AlCl3 that minimizes the formal charges on all atoms.

Draw one valid Lewis structure (including all lone pair electrons and any formal charges) for the anion (CH2CN)−. HCCN   H

Consider the following ion: BrO3−. a)  Show the full electron configuration for Br.  b)  Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c)  If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why.  d)  What is the electronic geometry of BrO3−? What is its molecular shape?  e)  Does BrO3− have a dipole moment? Briefly justify your answer. f)  On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer.  g)  Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. (IMAGE WITH POSSIBILITIES) h)  What is the molecular formula for Compound C? What is the empirical formula for Compound C?

The value of Ka1 of hypophosphorous acid, H3PO2, is nearly the same as the Ka1 of phosphoric acid, H3PO4. Draw a Lewis structure for phosphoric acid that is consistent with this behavior. Draw the Lewis structure with the formal charges minimized. Do not include formal charges in your structure. Include hydrogen atoms and nonbonding electrons in the structure.

For a molecule of XeCl3H a) Draw the Lewis structure then predict the shape of the compound and draw the shape of the compound b) Determine if the molecule is polar or nonpolar and explain how you made that determination. If there is a dipole moment, draw it.

An incompicie Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of -1. N-C-C-H Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges. H N=c=c-H

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. We can draw three inequivalent Lewis structures for the sulfite ion, SO3²-. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge S 01 Use the References to access important values if needed for this question. 02 03 S KNENEN :0: B A I 2- 2. The best Lewis structure for SO3²- is A :0: C Previous Next

Draw regular Lewis structures (no need to use dashed lines and wedges) for each of the following molecules and indicate which exception, if any, to the octet rule is found in each of them: SCI6, CH3, XeF4, BBR3.

The compound below (Cl2O2) plays a role in ozone depletion in the stratosphere, where it serves as a reservoir of Cl atoms that catalyze the destruction of O3. Draw a Lewis structure for Cl2O2 based on the arrangement of atoms shown above.

When drawing the Lewis structure of the HCC13 molecule, the structure should represent a total of 26 valence electrons. What is the best description of the complete Lewis structure of the molecule? Select one: AH atom should be in the center with single bonds to each Cl atom and a double bond to the C atom. A Cl atom should be in the center with a single bond to the C atom and a single bond to the H atom. AC atom should be in the center with a double bond to the H atom and double bonds to each Cl atom. AC atom should be in the center with single bonds to each Cl atom and a single bond to the H atom.