Draw the Lewis dot structures for the following molecules. None
of the atoms have a formal charge.
CH3OH (methanol) CH3COOH (acetic acid)
Draw the Lewis dot structure for the polyatomic ion acetate (CH3COO-). Next to your diagram, draw a resonance structure
Draw the Lewis dot structures for the following molecules. None of the atoms have a formal...
Draw the Lewis dot structures for the following molecules. Note that none of the atoms have a formal charge. HCN (hydrogen cyanide) CO2 (carbon dioxide)
Draw complete Lewis (electron-dot) structures and calculate the formal charges for all the atoms in the species listed below. If more than one reasonable resonance structure is possible, draw them all, with the corresponding formal charges, and indicate which structure represents the best or would contribute the most to the hybrid resonance structure of the given molecule/ion. a) AlCle b) N20 c) Dithionite anion, S202 d) Methyl azide, CH3-N3
Draw the Lewis structure (including resonance structures) for diazomethane (CH2N2). For each resonance structure, assign formal charges to all atoms that have formal charge. Draw the molecules by placing atoms on the canvas and connecting them with bonds. Include all lone pairs of electrons. Show the formal charges of all atoms in the correct structures.
PART II a) Draw all of the Lewis structures possible for the molecules below (resonance structures) and b) Indicate the formal charge on all of the atoms in your structures. Based on the formal charges, are the structures equivalent or not equivalent. If not determine the "best" resonance structure. (a) CO, (b) NO, (c) NO, (d) N,
2.) Draw correct Lewis dot structures for each of the following molecules. Draw all reasonable resonance structures. Expand the octet of the central atom (if possible) in order to minimize formal charges. Calculate formal charges on each atom. 12 pt.) a. CIO, b. NO, C. SO,
Draw Lewis Structures for the following molecules. Include any resonance structures and formal charges. Indicate the most probable structure. ClF3 CN(-)
1. Using molecular models, construct the following molecules/polyatomic ions, and write their Lewis formulas. Record the following information for each in your laboratory notebook. a) Molecule or ion b) # of valence electrons c) Lewis structure d) Draw any resonance structures if applicable e) Calculate all formal charges for molecules that have resonance structures f) For molecules that have resonance structures identify, which resonance structure contributes the most to the hybrid? 10. XeOF 11. AsF3 12. 1F4* 13. SO, 14....
Lewis Dot structures- VSEPR-CHEM 1412 for each of the following molecules, draw: 1. the Lewis structure 2. indicate the molecular shapes 3. bond angles 4. hybridization on the central atom, 5. For the 4 problems with an "calculate the formal charge of the eleent in bold. Lewis structure Molecular Shape bond hybridization or formal charge for angles on central atom element in Bold 1. carbon tetraflouride 'N 2.)* NHA 3.) carbon monoxide 14.) -2 CO3 5.) COCI "O Lewis structure...
2. (10 pts, 2.5 pts each) Draw the Lewis dot structure for the following and CIRCLE the structures that display resonance. Also indicate the formal charge of any positively or negatively charged atoms in a structure (so you do not have to indicate formal charge for neutral atoms or those with a formal charge of zero) C₂H₂O₂ C4H g F2 PO4 CO2 3. (6pts) What are the possible magnetic quantum number values if the angular quantum number is 2?
1. Using molecular models, construct the following molecules/polyatomic ions, and write their Lewis formulas. Record the following information for each in your laboratory notebook. a) Molecule or ion b) # of valence electrons c) Lewis structure d) Draw any resonance structures if applicable e) Calculate all formal charges for molecules that have resonance structures f) For molecules that have resonance structures identify, which resonance structure contributes the most to the hybrid? 5. HCN 6. PO, 7. Galz 8. BrF3 9....