Creatine is a dietary supplement used by some athletes to...

Name: Problem 46, Chapter 1: Organic Chemistry
Uploaded: 2019-03-11T02:10:04-08:00
Duration: 3 min 57 s
Channel: Chloe Schroeder
Description: Creatine is a dietary supplement used by some athletes to boost their athletic performance. (a) Draw in all lone pairs in creatine. (b) Draw two additional resonance structures showing all lone pairs and formal charges.

Creatine is a dietary supplement used by some athletes to boost their athletic performance. (a) Draw in all lone pairs in creatine. (b) Draw two additional resonance structures showing all lone pairs and formal charges.

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the arrangement of electrons in a molecule. They depict atoms, bonds, and lone pairs, providing a foundational visualization that aids in understanding molecular geometry and electron distribution.

Lone Pairs

Lone pairs are electrons that are not involved in bonding and reside on individual atoms. Their placement in molecular structures is crucial as they influence the shape, reactivity, and potential resonance forms of the molecule.

Resonance Structures

Resonance structures are different Lewis structures for the same molecule that illustrate the delocalization of electrons. They help demonstrate how electron density can be spread over multiple atoms, contributing to the overall stability of the molecule.

Formal Charges

Formal charges are a method for assigning the distribution of charge within a molecule by comparing the number of valence electrons in the isolated atom to the number assigned in the Lewis structure. They are key in evaluating the most stable electronic arrangement among resonance forms.

Transcript

00:01 To begin this problem, draw another loan pairs on creatine.

00:04 So i read your creatine here for you.

00:07 The atoms that can have lone pairs are nitrogen and oxygen.

00:11 Keep in mind that each atom needs to have a full octet.

00:14 So let's look at this nitrogen first.

00:17 It currently has two, four, six electrons, if you count all the bonds it currently has.

00:22 So it needs two more electrons.

00:25 It must have a single loan pair.

00:28 If we look at this top nitrogen, it has a full octet, two bonds to hydrogen, two more bonds to carbon, give it eight electrons.

00:35 It has a formal positive charge, however, because it came in with five valence electrons and currently only has four if you calculate the formal charge.

00:43 So no loan pairs here.

00:45 If we look at this nitrogen, it currently has two, four, six electrons around it.

00:50 It needs two more.

00:51 So it has a loan pair that was implied.

00:55 If we look at the carbonyl oxygen, it currently has two, four electrons.

01:01 But there's four more that are implied that would give it a full octet.

01:06 If we look at this final oxygen, it only has two electrons drawn in by bonds.

01:12 That means there must be six more around it, or three sets of loan pairs.

01:16 It has a formal negative charge.

01:20 Now we need to draw two additional resonance structures showing all the loan pairs and the formal charges.

01:26 I will say there are definitely more than two resonant structures you can draw.

01:29 The first one i chose to draw was to push this pie bond up onto nitrogen so that it satisfies its positive charge...

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