Match each of the Lewis structures (a to c) with the correct diag...

Question

Match each of the Lewis structures (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or nonpolar. Assume X and Y are nonmetals and all bonds are polar covalent. (6.6, 6.8, 6.9)1.
2.
3.
c.

2.

3.

c.

Accepted Answer

Welcome back. Everyone shown below is the les structure of a compound identify its molecular shape representation from the diagrams one through four and give the name of the shape determine whether the molecule is polar or nonpolar if all the bonds are polar covalent. Now, let's begin by defining the given molecular shapes in diagrams. One through four. Beginning with diagram one, we need to consider any electron groups, any bonding groups and then any lone pairs of electrons. And just so this is visible, I'm going to move this over. So in diagram one, we can observe that we have four bonded atoms to our central atom, Which would account for a total of four electron groups. As far as bonding groups as we stated, we have four atoms bonded to our central atom via polar covalent bonds, meaning that each of our atoms are nonmetals where one of our atoms have a higher electron negativity, which is most likely going to be our terminal atoms. So again, we would have four bonding groups based on these four bonded atoms to our central atom. And as far as lone pairs, because we observe that in diagram one, we have a tetrahedral molecular geometry shape. We would have zero lone pairs in order to attain this molecular shape. Now, we're going to compare diagram two to which as far as electron groups, we would observe that we have a lone pair that we need to draw in on our central atom, which influences our molecular shape where we see the three atoms towards the bond bonded towards the bottom of our central atom, which will account for a total of four electron groups total. So that includes the lone pair and our three bonded atoms to our central atom. And as far as bonding groups, only three are bonded to our central atom out of our four electron groups. So we have three bonding groups. As far as lone pairs, we had to draw in one loan pair. And due to the presence of this loan pair, this influences how our three atoms are bonded to our central atom. And thus, we would have the results of a trigonal pure middle molecular shape. Now, we move on to diagram three to which we observe three atoms bonded to our central atom resulting in three electron groups, three of our bonded atoms would correspond to three bonding groups and we would not observe any lone pairs based on our shape of our molecule in diagram three being trigonal planar. Now we have diagram four to which we're going to need to draw in two sets of lone pairs on our central atom and we observe two bonded atoms to our central atom. So the two lone pairs and the two bonded atoms account for a total of four electron groups where two of these four electron groups are bonding groups. So we have two bonding groups because of those two bonded atoms to our central atom. And then as far as lone pairs, we had to draw in two sets of lone pairs. So we have two lone pairs and due to the presence of these two sets of lone pairs, this affects our molecule so that we have a bent molecular geometry or shape. Now with our shapes in diagrams, one through four outlined, we're going to focus on our given lower structure of our compound. We would observe that we have as far as bonding groups, bonding groups, we would have a total of two of our y atoms bonded. So we have two bonding groups. And as far as loan pairs on our central atom, which appears to be X, since we just have one X, we would have a set of two loan pairs that we can count in our given leer structure. So adding up our loan pairs and our bonding groups, we would have a total of four electron groups being again two of our bonded Y atoms to our central atom X and then the two lone pairs on our central atom X resulting in four electron groups total. Now, based on what we outlined below in diagrams one through four, when we have four electron groups, where two are bonding groups and two are lone pairs. This will result in the bent molecular geometry. So the name of our shape for our given le structure is going to be bent, which can also be interpreted as V shaped and can also be interpreted as angular. So any of these names are acceptable. And then we need to determine whether our bonds are polar or nonpolar. Now, based on the fact that we have two lone pairs, this will influence our shape of our molecule to be asymmetrical. So we will not have a perfect bent shape. And because we have this asymmetrical shape, we therefore have a net dipole present. And therefore we have a polar molecule Since we will not be able to have our di pulse cancel. And so our final answers are going to be that we've determined that Diagram four is the best molecular representation of our Lewi structure given of our compound, which is a bent shape as our name of our shape. And then we have a polar molecule overall due to the presence of our two lone pairs on our central atom X. So bent polar and diagram four are our final answers. I hope this made sense. And let us know if you have any questions.

Struggling with GOB Chemistry?

Match each of the Lewis structures (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or nonpolar. Assume X and Y are nonmetals and all bonds are polar covalent. (6.6, 6.8, 6.9)1.
2.
3.
c.

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Molecular Polarity (Simplified) practice set

Struggling with GOB Chemistry?

Match each of the Lewis structures (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or nonpolar. Assume X and Y are nonmetals and all bonds are polar covalent. (6.6, 6.8, 6.9)1. 2. 3. c.

Watch next

Molecular Polarity (Simplified) practice set

Match each of the Lewis structures (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or nonpolar. Assume X and Y are nonmetals and all bonds are polar covalent. (6.6, 6.8, 6.9)1.
2.
3.
c.