Describe the hybrid orbitals used by the central atom and the type(s) of bonds formed in (a) NO3

Describe the hybrid orbitals used by the central atom and...

Key Concepts

Hybrid Orbitals

Hybrid orbitals are formed when atomic orbitals of similar energies mix to form new orbitals that are oriented in specific directions. This concept explains how a central atom can maximize bonding with surrounding atoms by using appropriately directed orbitals, such as sp, sp2, or sp3, which directly influence the molecular geometry and bond formation.

Sigma Bonds

Sigma (?) bonds are the first bonds formed between two atoms, resulting from the head-on overlap of orbitals. They provide the primary bonding interaction and form along the internuclear axis, establishing a strong, localized bond that defines the basic molecular framework.

Pi Bonds

Pi (?) bonds occur through the side-to-side overlap of unhybridized p orbitals and are typically formed in addition to sigma bonds in double or triple bonds. These bonds contribute to the rigidity of the molecule and allow for additional electron density above and below the bonding axis, playing a key role in multiple bond formation.

Resonance and Electron Delocalization

Resonance is a concept where the actual electron distribution in a molecule is represented as a hybrid of several valid Lewis structures. This delocalization of electrons, often observed in molecules with conjugated bonds or equal bond distributions, contributes to extra stability and explains uniform bond characteristics in species that might otherwise exhibit localized double bonds.

Transcript

00:02 On this problem, we are going to find the hybrid orbitals used by the central atom.

00:09 Okay, and in addition, we're going to find the type of bonds on each one of these ions or molecules.

00:17 So the first thing, as always, is that we're going to find the valence electrons because we need to draw the lewis structures.

00:24 So we have five valence electrons for nitrogen, six valence electrons for oxygen, but we have three.

00:31 This is 18.

00:33 Since we have an ion, we need to add one or the charge that it says in here.

00:39 So we are looking at a total of 24 electrons.

00:45 Then what we're going to do is that we're going to draw the lewis dot structure.

00:50 So remember that since you're drawing an ion, you need to put it in brackets.

00:58 So you have o, o, and o.

01:02 You close your brackets, your charge goes at the end, and then you're going to start filling in electrons, okay, in the outer atoms.

01:12 So you already have six, eight, ten, twelve, fourteen, 16, 18, 18, 20, 22, 24.

01:23 Oh, but what happened? okay, nitrogen is not happy.

01:28 And remember that happy means eight electrons around.

01:31 So what we need to? do is that we need to relocate one of these pairs and make a double bond somewhere in here.

01:43 Okay, so what i'm going to do is that i'm going to use this one and i'm going to make a double bond in here.

01:52 And as you see, okay, now nitrogen is completely happy.

01:59 Now let's count.

02:00 We're going to count how many electron domains.

02:05 Nitrogen has around.

02:06 So it has one, two, and three electron domains.

02:11 So it has three electron domains.

02:20 If it has three electron domains, it means that it can make three orbitals.

02:25 So it has one, two, and three orbitals.

02:29 You know that the first orbital is s and the second one is p.

02:35 Right p has three but we're not using the third one that's the reason why i'm not writing it so the hybridization of this end is sp2 now let's count how many sigma and pi bonds this molecule has so if you see right here sigma bonds are single bonds so you have one two and always remember that a pi bond always have a sigma bond so this is three, and pie bonds are double bonds.

03:14 So this is one.

03:18 Now let's do exactly the same thing with cs2.

03:22 Okay, or carbon dioxide.

03:27 So you know that carbon has four valence electrons.

03:32 Surfer has six times two is 12, so we're looking at a total of 16 electrons.

03:38 So i have carbon, s, and s.

03:44 I already have four electrons, six, eight, ten, twelve, fourteen, fourteen, and sixteen.

03:58 Carbon is completely sad...