Draw the Lewis structures for TeCl4, ICl5, PCl5, KrCl4, and XeCl2 . Which of the compounds exhib

Draw the Lewis structures for TeCl4, ICl5, PCl5, KrCl4, and...

Key Concepts

Lewis Structures

Lewis structures are diagrams that show the distribution of valence electrons among atoms in a molecule. They provide a way to visualize bonds, lone pairs, and the occurrence of multiple bonds, which helps in predicting the geometry and reactivity of the molecule.

Valence Electron Counting

Valence electron counting is the process of determining the total number of electrons available for bonding in a molecule. This is a fundamental step in drawing Lewis structures as it ensures that all bonding and non-bonding electron pairs are accurately represented, which in turn influences the molecule’s structure and properties.

VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of molecules based on the repulsions between electron pairs in the valence shell of the central atom. It explains how bond angles adjust to minimize repulsion, leading to different molecular geometries such as linear, trigonal planar, tetrahedral, and square planar.

Expanded Octet

The expanded octet concept applies to elements in the third period and beyond, which have access to d orbitals and can accommodate more than eight electrons. This allows such elements to form compounds with more than four electron pairs around the central atom, leading to a variety of molecular geometries that are not possible for second period elements.

Hybridization

Hybridization is the mixing of atomic orbitals to form new, equivalent hybrid orbitals that dictate the bonding structure and geometry in a molecule. It explains how atoms with different types of orbitals combine to form bonds that result in specific molecular shapes such as tetrahedral, trigonal planar, or square planar.

Square Planar Geometry

Square planar geometry is a molecular shape where a central atom is surrounded by four atoms located at the corners of a square plane. This geometry is often associated with dsp² or d²sp³ hybridization and is characteristic of certain coordination compounds and main group compounds with the appropriate electronic configuration.

Molecular Polarity

Molecular polarity refers to the uneven distribution of electron density within a molecule, resulting in a net dipole moment. It is determined by both the differences in electronegativity between atoms (bond polarity) and the overall molecular geometry. A molecule is polar if the geometry does not cancel out the individual bond dipoles.

Transcript

00:05 So t e, cl4, number of balance electrons on this is 6 plus 7 into 4 .34.

00:16 And this is what we subtract from when we do the lewis structure.

00:21 So, cl on all four sides.

00:24 It's obviously going to have electrons, two electrons shared with each cl.

00:30 So 4 into 2, we subtract that out with 26 electrons.

00:36 And then we have to complete the electron octet configuration on all of these co atoms.

00:47 So you have 4 into 6, that's 24.

00:51 So you have two electrons left, which will reside on the tullum.

00:57 So the actual structure would look something like this according to vscpr theory and one electron.

01:07 This is definitely polar because while the dipole moments on these two sides get cancelled out.

01:18 There is a dipole moment from the telurium and chlorides that are not quite balanced.

01:27 So this molecule will be polar.

01:31 Now moving on to the second molecule we have, it's ico5.

01:38 Number of balanced electrons is 7 plus 5 into 7.

01:44 That's 35.

01:45 25 so 42 is what we subtract from.

01:50 Let's write down the 5 cls around iodine.

01:55 It shares two electrons with each molecule.

02:02 So we can subtract that out, so it's 32.

02:06 Then we complete the acted configuration for each of these cl atoms.

02:16 We subtract that out 2, so it's 6 into 5, that's 30, so we have 2 electrons left that will reside on this iodine.

02:22 So if you write it out, then according to the vacpr theory, it will look something like this.

02:28 Cl, cl, cl, cl.

02:33 And then you have the double bond over there.

02:36 So the dipole moments in these four cases will obviously cancel out, but the dipole moment of this chlorine here will not.

02:48 So this will definitely be a polar molecule.

02:57 Moving on to the next atom, sorry molecule that we have.

03:01 It's pcl 5...

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