Chapter10: Potentiometry And Redox Titrations
Section: Chapter Questions
Problem 6P
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Question
Part B and C are two separate questions.
![Part B
Calculate the oxidation number of the atom S according to the Lewis structure in Part A.
Express your answer as a signed integer.
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Part C
Calculate the oxidation number of the atom O according to the Lewis structure in Part A.
Express your answer as a signed integer.
Submit
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Part D
oll the atoms. (There should b](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F49ea5ce9-c5c6-4d0f-a754-54c08e96facb%2Fdd7d0578-36a1-47bd-9b0a-65fb863b5fde%2Fxkj92tt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Part B
Calculate the oxidation number of the atom S according to the Lewis structure in Part A.
Express your answer as a signed integer.
Submit
Request Answer
Part C
Calculate the oxidation number of the atom O according to the Lewis structure in Part A.
Express your answer as a signed integer.
Submit
Request Answer
Part D
oll the atoms. (There should b
![Previous Answers
All attempts used; correct answer displayed
To draw the Lewis structure from a molecular formula, we need to find the sum of the valence electrons. Sulfur and oxygen are in group 6A (16) and contribute six electrons per atom. Therefore, the total number of electrons is
valence electrons in SO2 = (electrons contributed by S) + (electrons contributed by O) = (1 × 6) + (2 x 6) = 18 electrons
There are many ways to arrange atoms, but not all configurations will form a valid structure. We can begin drawing the structure by placing the first element in the middle and connecting the rest of the atoms to it through single bonds. This will
suffice for all binary compounds and for many others that do not begin with hydrogen (as hydrogen can only form one single bond and cannot be a central atom). This will give a structure with sulfur in the middle attached to two oxygens From
here we can complete the octet of each atom by forming a double bond between sulfur and one of the oxygens, and leaving the rest of the electrons as nonbonding This means that one oxygen will be attached through a single bond and have
three pairs of nonbonding electrons, whereas the other will be attached through a double bond and have only two pairs of nonbonding electrons. The sulfur, meanwhile, will have one pair of nonbonding electrons. This completes the octet for
each atom but leaves several with different formal charges. The formal charge can be calculated using the following formula:
Formal charge = valence electrons – (bonding electrons) – nonbonding electrons
Plugging in these values for the single-bonded oxygen, we get
Formal charge of Single – Bonded Oxygen = 6 – 5(2) – 6 = –1
Plugging in these values for the double-bonded oxygen, we get
Formal charge of Double – Bonded Oxygen = 6 – (4) – 4 = 0
And plugging in these values for the sulfur, we get
Formal charge of Sulfur
6 – (6) – 2 = +1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F49ea5ce9-c5c6-4d0f-a754-54c08e96facb%2Fdd7d0578-36a1-47bd-9b0a-65fb863b5fde%2F0kr9tpl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Previous Answers
All attempts used; correct answer displayed
To draw the Lewis structure from a molecular formula, we need to find the sum of the valence electrons. Sulfur and oxygen are in group 6A (16) and contribute six electrons per atom. Therefore, the total number of electrons is
valence electrons in SO2 = (electrons contributed by S) + (electrons contributed by O) = (1 × 6) + (2 x 6) = 18 electrons
There are many ways to arrange atoms, but not all configurations will form a valid structure. We can begin drawing the structure by placing the first element in the middle and connecting the rest of the atoms to it through single bonds. This will
suffice for all binary compounds and for many others that do not begin with hydrogen (as hydrogen can only form one single bond and cannot be a central atom). This will give a structure with sulfur in the middle attached to two oxygens From
here we can complete the octet of each atom by forming a double bond between sulfur and one of the oxygens, and leaving the rest of the electrons as nonbonding This means that one oxygen will be attached through a single bond and have
three pairs of nonbonding electrons, whereas the other will be attached through a double bond and have only two pairs of nonbonding electrons. The sulfur, meanwhile, will have one pair of nonbonding electrons. This completes the octet for
each atom but leaves several with different formal charges. The formal charge can be calculated using the following formula:
Formal charge = valence electrons – (bonding electrons) – nonbonding electrons
Plugging in these values for the single-bonded oxygen, we get
Formal charge of Single – Bonded Oxygen = 6 – 5(2) – 6 = –1
Plugging in these values for the double-bonded oxygen, we get
Formal charge of Double – Bonded Oxygen = 6 – (4) – 4 = 0
And plugging in these values for the sulfur, we get
Formal charge of Sulfur
6 – (6) – 2 = +1
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