Draw the Lewis structures of HSO 3 F and SO3 F^-. What is the molecular geometry and hybridizati

step 1 So we're going to start by drawing the Lewis structure of H .S .O .3F. First, I like to add up a

Draw the Lewis structures of HSO 3 F and SO3 F^-. What is...

Key Concepts

Hybridization

Hybridization describes the process by which atomic orbitals mix to create new, equivalent orbitals suitable for bonding. The type of hybridization, such as sp, sp2, or sp3, is determined by the number of electron groups (bonds and lone pairs) around the atom, and it correlates with specific molecular geometries.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

VSEPR theory predicts the three?dimensional arrangement of atoms around a central atom based on the repulsions among electron pairs—both bonding and lone pairs. By counting the regions of electron density, one can infer the electron geometry (and thus the molecular geometry) associated with a molecule.

Expanded Octet

Elements in the third period or beyond, such as sulfur, are capable of accommodating more than eight electrons in their valence shell because of the availability of low?lying d orbitals. This expanded octet allows these atoms to form more than four bonds, leading to a wider variety of bonding arrangements and molecular structures.

Lewis Structures

Lewis structures are diagrams that depict how valence electrons are distributed among atoms in a molecule, showing bonds and lone pairs. They serve as a fundamental tool in understanding molecular architecture, allowing one to assign connectivity, identify possible resonance contributors, and calculate formal charges.

Formal Charge

Formal charge is a bookkeeping tool used to determine the most plausible Lewis structure of a molecule. It is calculated by comparing the valence electrons of a free atom with the electrons assigned to it in the molecule. Structures with minimized formal charges and charge separation are generally more stable.

Transcript

00:01 So we're going to start by drawing the lewis structure of h .s .o .3f.

00:07 First, i like to add up all of the valance electrons that we have available to us.

00:12 So that is one valance electron on hydrogen, six on sulfur, six on each oxygen, and seven on fluorine.

00:20 And that gives us a total of 32 valence electrons.

00:24 So sulfur is our central atom, and that is bonded to 1, 2, 2 ,000.

00:31 Three oxygens and this oxygen is bonded to a hydrogen and the sulfur is also bonded to a fluorine so now we've used up 246, 8, 10 of our electrons and we have 22 left so we can use those up by completing the octet of the remaining atoms so i'm going to complete the octet of the fluorine and of the oxygens and now each atom has its completed octet.

01:06 However, this structure is not charge minimized, or the formal charges are not minimized.

01:12 So each of these oxygens here and here have a formal charge of negative one, and the sulfur will have a formal charge of positive 2.

01:20 And we can fix this by making a double bond to each of the oxygens.

01:28 So the lewis structure will look like this.

01:32 The octets are complete for all of the, for the oxygens and the fluorine.

01:42 Sulfur can expand its octet, so it's allowed to make six bonds and its charge is minimized.

01:48 So those are the correct lewis structure for this molecule.

01:55 Now, the molecular geometry is tetrahedral, since there are four things bonded to the central atom.

02:09 And the hybridization of the sulfur is sp3 hybridized...

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