T Use this condensed chemical structure to complete the table below. The condensed chemical structure of para-difluorobenzene. Some facts about the para-difluorobenzene molecule: molecular formula: number of major resonance structures: number of carbon-hydrogen single (C-H) bonds: number of lone pairs: I Don't Know Submit DELL F1 F2 F3 F4 F5 F7 ( 23 2$ V 3. 4. 8.

T Use this condensed chemical structure to complete the table below. The condensed chemical structure of para-difluorobenzene. Some facts about the para-difluorobenzene molecule: molecular formula: number of major resonance structures: number of carbon-hydrogen single (C-H) bonds: number of lone pairs: I Don't Know Submit DELL F1 F2 F3 F4 F5 F7 ( 23 2$ V 3. 4. 8.

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 15CTQ

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Similar questions

Some of the figures below represent invalid sets of resonance structures for this molecule.
Calculate the bond energy of C-F given that the heat of atominzation of CHFClBr is 1502 kj/mol, and that the bond energies of C--H, C--Br, and C-Cl are 413, 276 and 328 kj/mol, respectively. show the calculations
Below each structure in the previous question is a “condensed structure” that tells you somethingabout how the atoms are arranged. Draw complete Lewis structures for each of the followingcondensed structures. (The net charge, if any, on each molecule is given at the end.) a. CH3CH2 b. CH2CH2 c. CH2CCH2 d. C( CH3)3+ e. BF4 f. NCO g. CH2OH+ (two different acceptable answers) h. CH2CHCHCHCH2+ which may alsobe written as CH2(CH)3CH2+ (more than one acceptable answer)
A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.
NOx and SOx are industrial air pollutants of grave concern. Draw the correct Lewis diagrams including formal charges on the atoms and resonance structures as appropriate for the following examples of these species: (Hint: don't use any Lewis structures with formal changes exceeding +1 or -1) [Please answer part 4 and include the nitrogen trioxide radical NO3 for 2-4] Nitrous oxide, N2O, and disulfur monoxide, S2O The nitrogen trioxide radical, NO3- and sulfur trioxide, SO3; Use VSERP to assign the shape to these 4 molecules. Describe the polarity of each molecule. Which one is more polar? Justify your answer in terms of dipole moments and geometry.
There is persuasive evidence for the brief existence of the unstable molecule OPCl. (a) Draw a Lewis diagram for this molecule in which the octet rule is satisfied on all atoms and the formal charges on all atoms are zero. (b) The compound OPCl reacts with oxygen to give O2PCl. Draw a Lewis diagram of O2PCl for which all formal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.
A resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part3: Draw the least important resonance contributor for fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized and should include all nonzero formal charges and all nonbonding electrons.
A resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons.
Draw the shapes of the following molecules and ions in 3-dimension. Show clearly any lone pairs of electrons on the central atom, state the number of bond pairs and lone pairs of electrons on the central atom and name the shape of the molecule or ion. (a) CH3+, methyl carbocation (b) HOBr, bromic (I) acid (c) NCl3, nitrogen trichloride Provide everything stated in the instructions for each compound.
Draw Lewis Structures for the following compounds. (Be sure to minimize formal charges and draw resonance structures where appropriate.): XeF2O, ClO4-, HNO2, CH3CH(NH2)COOH (amino acid alanine). Identify the molecules with the following labels (1 is more than one label): Oxyacid, has a resonance structure, expanded octet, has a carbon backbone For the molecule with resonance structures—what is the bond order for the atoms that share e-?
NOx and SOx are industrial air pollutants of grave concern. Draw the correct Lewis diagrams including formal charges on the atoms and resonance structures as appropriate for the following examples of these species: (Hint: don't use any Lewis structures with formal changes exceeding +1 or -1) Nitrous oxide, N2O, and disulfur monoxide, S2O The nitrogen trioxide radical, NO3- and sulfur trioxide, SO3; Use VSERP to assign the shape to these 4 molecules. Describe the polarity of each molecule. Which one is more polar? Justify your answer in terms of dipole moments and geometry.
Q1 The balanced equation for the fomplete combustion of acetone(C3H6O) is: C3H6O + 4O2 --> 3CO2 + 3H2O ΔrH-1790kJmol^-1 If a bottle of nail polish remover contains 177mL of avetone(density 0.788gmL^-1) how much heat is released by its complete combustion? Q2. Draw the lewis structures for O-N-Cl and N-O-Cl. calculate the formal charges of the atoms and use these to determine which of these isomers is more stable. Q3. The work function of aluminum is 412kJmol^-1. If light corresponding to 471kJ mol^-1 is shone on the metal what is the velocity of the electrons that are emitted from the metal?