Pushing Electrons
4th Edition
ISBN: 9781133951889
Author: Weeks, Daniel P.
Publisher: Cengage Learning
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Chapter 3, Problem 7EQ
Here are some exercises in sigma bond breaking. Supply the arrows and the products. Remember that charge must be conserved. That is, if a neutral molecule is dissociated, the algebraic sum of the charges on the products must equal zero. If a positively charged ion is dissociated, the algebraic sum of the charges on the products must equal +1.
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I need part C, please explain how to do the problem, it would help a lot!!
4) Hi, Can you solve the question 4 and make explanation please? and if you are gonna use handwrite please make sure that it is readable thank you.
Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-
radical combination reaction is the formation of a new electron-pair bond.
Consider the formation of hydrogen peroxide.
2 OH(g) → H₂O₂(g)
Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons.
OH(g)
Select Draw Rings More
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||| |||
Erase
Q2 Q
H₂O₂(g)
Select Draw Rings More
3
S
H
Erase
Q2 Q
Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry
Publisher: University Science B
Chapter 3 Solutions
Pushing Electrons
Ch. 3 - Prob. 1EQCh. 3 - Prob. 2EQCh. 3 - Prob. 3EQCh. 3 - Prob. 4EQCh. 3 - Prob. 5EQCh. 3 - Prob. 6EQCh. 3 - Here are some exercises in sigma bond breaking....Ch. 3 - Prob. 8EQCh. 3 - Prob. 9EQCh. 3 - Prob. 10EQ
Ch. 3 - Prob. 11EQCh. 3 - Prob. 12EQCh. 3 - Prob. 13EQCh. 3 - Prob. 14EQCh. 3 - Prob. 15EQCh. 3 - Prob. 16EQCh. 3 - Prob. 17EQCh. 3 - Prob. 18EQCh. 3 - Prob. 19EQCh. 3 - Prob. 20EQCh. 3 - Prob. 21EQCh. 3 - Prob. 22EQCh. 3 - Prob. 23EQCh. 3 - Prob. 24EQCh. 3 - Prob. 25EQCh. 3 - Prob. 26EQCh. 3 - Prob. 27EQCh. 3 - Prob. 28EQCh. 3 - Prob. 29EQCh. 3 - Prob. 30EQCh. 3 - The reaction just described is reversible....Ch. 3 - Prob. 32EQCh. 3 - Prob. 59EQ
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- You will not find “hydroxide” in the stockroom, but you will find sodium hydroxide (NaOH) andpotassium hydroxide (KOH). Lithium hydroxide (LiOH) is expensive and used in spacecraft airfilters since hydroxide reacts with carbon dioxide, and lithium is lighter than sodium or potassium.Cesium and francium hydroxides are very expensive and little used. Is this information consistentwith your answer to the previous question?arrow_forwardI had gotten this one incorrect, but i wanted to use it to study, so please give me the solution to all parts of this question.arrow_forwardMany free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-radical combination reaction is the formation of a new electron-pair bond. Consider the chemical equation. N(g)+NO(g) NNO(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons.arrow_forward
- Write a Lewis structure for formaldehyde, HC(=O)H, showing all valence electrons. • You do not have to consider stereochemistry. Explicitly draw all H atoms. • Include all valence lone pairs in your answer. ● TAYY Sn [Farrow_forwardThe formate ion is HCOO-. Carbon is the central atom. The other atoms are bonded only to the carbon atom. - Draw the best Lewis structure for the formate ion. Show all important resonance structures. Indicate all non-zero formal charges. - In the formate ion, are both carbon-oxygen bonds the same length? What is the oxidation state of carbon in the formate ion? -Which of the following molecules has the shortest carbon-oxygen bond length? HCOO- CO CO2arrow_forwardThe carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]arrow_forward
- Please don't provide handwriting solutionarrow_forwardA student claims “C = O bonds have a larger bond energy than the other types of bonds involved in this reaction, which means they require more energy input to make.” Do you agree or disagree with the students claim? Explain your response.arrow_forwardDraw Lewis structures and assign formal charges for the following compounds and ions. Note any resonance forms and explain which resonance form is the most important. Make a note of any other unusual features (such as "this one doesn't work" and why- what are the shortcomings of the model.) CO3²- CO NO₂ CNO (include isomers) Al₂Cl6 B₂H6 O2 (paramagnetic) H3O+ LiF IF7arrow_forward
- Please do it correctly.arrow_forwardCalculate the enthalpy of reaction for the equation using the bond energy values you previously calculated. H₂O →>> 3NO₂ 402 kJ NO + 2HNO3 6071472 k 926 kJ mol mol AH = [?] kJ rxn Hints: Bonds broken minus bonds formed and watch the coefficients! Include a + or - sign AND the magnitude in your answer. Enterarrow_forwardParts A-C only . not graded .arrow_forward
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