Draw the Lewis structures of the acid HPO 2 F2 and its anion PO2 F2^- . What is the molecular ge

step 1 So starting with HPO2, F2, we're going to draw the Lewis structure. To do this, first I like to

Draw the Lewis structures of the acid HPO 2 F2 and its anion...

Draw the Lewis structures of the acid HPO $_{2} \mathrm{F}_{2}$ and its anion $\mathrm{PO}_{2} \mathrm{F}_{2}^{-} .$ What is the molecular geometry and hybridization for the phosphorus atom in each species? (H is bonded to the O atom in the acid.)

Key Concepts

Lewis Structures

Lewis structures are diagrams that depict the bonding between atoms of a molecule and the lone pairs of electrons that may exist. They are essential for determining the connectivity of atoms, evaluating formal charges, and identifying possible resonance structures, all of which are foundational for understanding the chemical behavior of a molecule.

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms in a molecule. It is determined by the number of bonding pairs and lone pairs around the central atom and is typically predicted using VSEPR theory. This concept is crucial for understanding molecular shapes, bond angles, and how these factors influence chemical reactivity and properties.

VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory helps predict the shape of a molecule by assuming that electron pairs (bonding and non-bonding) around a central atom will arrange themselves to minimize their mutual repulsion. This theory is instrumental in deducing molecular geometry from the Lewis structure.

Hybridization

Hybridization involves the mixing of atomic orbitals to form new, equivalent hybrid orbitals that can overlap to form chemical bonds in a specific geometry. The type of hybridization (such as sp3, sp3d, etc.) directly correlates with the observed molecular geometry and helps explain the bond angles and molecular structure.

Transcript

00:01 So starting with hpo2, f2, we're going to draw the lewis structure.

00:07 To do this, first i like to add up all the valance electrons of each atom that we have available to us to draw it.

00:13 So each hydrogen has one, each phosphorus has five, each oxygen has six, and each fluorine has seven valence electrons.

00:22 So in total we have 32 valence electrons.

00:25 The structure, the lewis structure, will have phosphorus as our central atom.

00:32 Bonded to two oxygens and one oxygen is bonded to a hydrogen and two fluorines.

00:44 So here we've already used up 10 electrons and we have 22 left.

00:49 So we're going to complete the octets of the remaining atoms.

00:55 So we have 22 left.

00:57 We have 20, 18, 16, 14, 12, 10, 8, 6, 10, 8, 6, 4 to 0.

01:11 Now, this is technically correct.

01:14 However, the formal charges are not minimized.

01:17 This is not the charge minimized structure.

01:20 So what we're going to do is we're going to remove two electrons from one of the oxygens or from this oxygen up here and make a double bond.

01:29 And this is okay because phosphorus can expand its octet and all of the other remaining atoms have a full octet, except for the hydrogen because it only needs two electrons to be happy...

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