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Calculate the oxidation number of the atom O according to the Lewis structure in Part A.

Calculate the oxidation number of the atom O according to the Lewis structure in Part A.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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. 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
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
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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