Valence Shell Electron Pair Repulsion Theory

Now under valence shell electron pair repulsion theory, also known as vesper theory, we say that the geometry of the molecule is based on minimizing the repulsion between electron groups on the central element. Now, when we say the term electron group, an electron group equals a lone pair or lone pairs on the central element plus bonding groups. Now, when we say bonding groups referring to the surrounding elements that are directly attached to our central element. Now, in addition to this, we can say that our lone pair electrons, they exhibit an electron cloud that further adds to repulsion. So we're going to start looking at different types of molecular shapes and we're gonna see the number of electrons groups associated with each one of these unique molecular shapes.

How many electron groups on the nitrogen atom? Based on the following lewis dot structure? So here we have a picture of ammonia. Ammonia has one lone pair and three surrounding elements. Remember your electron groups equal the number of lone pairs on the central element, as well as the number of bonding groups, which are just the number of surrounding elements. So if we take a look here, we're gonna say we have one, 234 electron groups on the nitrogen atom. Also realized here when we talk about a lone pair, it's just a pair of electrons not forming a bond. Remember they exhibit an electron cloud. So we see this electron cloud as this LaPierre. This just helps push bonds further away from itself, causing even more propulsion within our molecule. So again, in this particular question, we have one lone pair and three bonding groups on the nitrogen atom, giving us a total of four electron groups.

using desperate theory, the locations of surrounding elements and lone pairs around the central element are determined. Now it's important to realize that remember lone pairs cause further propulsion in terms of a molecular shape and the molecular shapes are going to see are drawn that way on purpose. These are the actual arrangements of the atoms based on the number of electron groups around the central element. So if we take a look here, we have electron groups that go from 2-6. And based on your number of electron groups, we can produce different types of molecular shapes. If we take a look at the first electron group pairing, we have two electron groups. There's only one possible molecular shape associated with it. It's a central element connected to two bonding groups or surrounding elements. When we have three electron groups around the central element to possible shapes can happen. One where we have three surrounding elements and one we have to surrounding elements and one lone pair. Remember lone pairs. Again they have an electron cloud Aranda, which we show with this slope if we have four electron groups and three shapes are possible. One where all four electron groups are surrounding elements, one where it's three surrounding elements, one lump hair And one where it's to surrounding elements and two lone pairs. If you have five electron groups, this is the most complex of all of them because it gives us four different shapes here, we have our first option words, five surrounding elements. one where it's four surrounding elements in one lone pair, one where it's three surrounding elements in two lone pairs, and finally one where it's to surrounding elements and three lone pairs. Finally, when we have six electron groups around the central element, we have three possible shapes, one where it's three surrounding elements, I'm six surrounding elements around the central element, then one where it's only one long pair and five surrounding elements, and then one where it's too long pairs and four surrounding elements. Now, as you go deeper and deeper in terms of shapes will learn the names associated with each one of these molecular shapes shown. But again, remember the number of electron groups kind of limits the different types of molecular shapes that are possible for any given molecule.

How many electron groups lone pairs and bonding groups does the compound have, respectively? So here we have s. four. Now, if we look at the total number of electron groups, remember electron groups kicks into account the lone pair as well as the bonding groups on the central element. So we have total electron groups, lone pairs, lone pairs on the central element. Remember they have an electron cloud. So we have one lone pair on our central element, and then bonding groups are just the surrounding elements attached to the central element. So that is one, 2, 3, 4 bonding groups. So this is how we break down the different types of groups found within SEF four.