Determine if each of the statements is True or False...

Determine if each of the statements is True or False regarding the best Lewis structure of SCN-. C is the central atom. 1) The C atom has two single bonds. [ Select ] 2) There are two lone pairs of (nonbonding pair) electrons around the nitrogen atom. [ Select ] 3) There are three lone pairs of (nonbonding pair) electrons around the sulfur atom. [ Select ] 4) The chemical bond between the carbon atom and the sulfur atom is a double bond. [ Select ]

Transcript

00:01 So for this question, they are given a bunch of statements about the lewis structure of the compound and then ask if those statements are true or false.

00:14 So first, let's figure out the lewis structure of the compound and then we'll be able to answer those questions pretty easily.

00:21 So we're told that carbon is the central atom.

00:25 So we'll put carbon in the middle and then we'll have it bonded it to nitrogen and sulfur.

00:31 Remember from the periodic table, sulfur is going to have six valence electrons, carbon has four valence electrons, and nitrogen has five.

00:41 And then this negative from the ion is going to give it an extra electron.

00:49 So this structure is going to have a total of 16 valence electrons that we have to include.

00:57 So we know that we have to have the octet rule fulfilled for e.

01:03 So if we have the carbon double bonded to each, the octet rule for carbon is fulfilled.

01:12 And then we have two lone pairs of electrons on the sulfur and two lone pairs of electrons on the nitrogen.

01:23 That's going to be 24, 6, 8, 10, 12, 14, 16.

01:27 So that's going to be all of our 16 valence electrons.

01:33 Now let's look at formal charges.

01:37 We have the octet rule fulfilled for each element.

01:39 And then if we look at formal charges, the formal charge on sulfur is going to be zero, right? because we have six valance electrons, and then we have four electrons in loan pairs and two electrons in bonding.

01:56 So it's going to have formal charges of zero...

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