Valence Bond Theory and Hybridization
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Questions and Answers

What type of hybridization occurs in a molecule with 3 bonded atoms and 0 lone pairs?

  • sp3d
  • sp
  • sp3
  • sp2 (correct)

Which of the following molecules has sp3 hybridization?

  • PCl5
  • BeCl2
  • BF3
  • NH3 (correct)

How many total hybrid orbitals are used in the hybridization of SF6?

  • 4
  • 6 (correct)
  • 5
  • 7

Which statement correctly describes the bond formation in a sigma bond?

<p>It has electron density concentrated along the internuclear axis. (A)</p> Signup and view all the answers

What is the total number of lone pairs and bonded atoms in the molecule that exhibits sp hybridization?

<p>2 (C)</p> Signup and view all the answers

How many hybrid orbitals are formed when two atomic orbitals are mixed?

<p>Two (A)</p> Signup and view all the answers

Which type of hybridization results in the formation of four hybrid orbitals?

<p>sp3 (B)</p> Signup and view all the answers

What is the primary purpose of hybridization in the context of valence bond theory?

<p>To form covalent bonds through orbital overlap (D)</p> Signup and view all the answers

When mixing orbitals for sp² hybridization, which atomic orbitals are primarily involved?

<p>One s and two p orbitals (B)</p> Signup and view all the answers

Which hybridization involves mixing one s orbital with all three p orbitals?

<p>sp3 (D)</p> Signup and view all the answers

What type of hybrid orbitals are formed in BeCl2?

<p>sp (A)</p> Signup and view all the answers

Which hybridization occurs in BF3?

<p>sp2 (C)</p> Signup and view all the answers

In which molecule do sp3 hybrid orbitals occur?

<p>CH4 (D)</p> Signup and view all the answers

What type of bond is a sigma bond?

<p>A bond formed through hybrid orbitals (C)</p> Signup and view all the answers

Which hybridization type is involved in SF6?

<p>sp3d2 (B)</p> Signup and view all the answers

What type of bond has electron density concentrated around the internuclear axis?

<p>Sigma bond (B)</p> Signup and view all the answers

In a double bond, how many pi bonds are present?

<p>One pi bond (D)</p> Signup and view all the answers

How many total bonds (sigma and pi) are present in a triple bond?

<p>One sigma and two pi bonds (B)</p> Signup and view all the answers

What is the total number of sigma bonds in acetic acid (CH3COOH)?

<p>7 (B)</p> Signup and view all the answers

What is the electron density characteristic of a pi bond?

<p>Above and below the plane of nuclei (A)</p> Signup and view all the answers

What type of bond is formed when two adjacent nuclei share a pair of electrons and have a side-to-side overlap of orbitals?

<p>Pi bond (B)</p> Signup and view all the answers

Which type of molecule is formed with both sigma and pi bonds?

<p>Covalent compounds (C)</p> Signup and view all the answers

In the acetic acid molecule, how many pi bonds are there?

<p>One (D)</p> Signup and view all the answers

How many s bonds are present in the hybridized structure?

<p>8 (D)</p> Signup and view all the answers

What type of hybridization is observed in the central carbon atoms in the given structure?

<p>sp3 (C)</p> Signup and view all the answers

Which atom is likely to form a p bond in the given hybridized molecule?

<p>Oxygen (A)</p> Signup and view all the answers

In compounds with sp2 hybridization, what is the angle between the bonds?

<p>120 degrees (A)</p> Signup and view all the answers

How many p bonds can be present around a single sp3 hybridized carbon atom?

<p>0 (D)</p> Signup and view all the answers

Which hybridization is involved in the formation of double bonds?

<p>sp2 (A)</p> Signup and view all the answers

Which of the following molecule components is characterized by sp hybridization?

<p>Acetylenes (C)</p> Signup and view all the answers

What is the geometric shape around a carbon atom that is sp2 hybridized?

<p>Trigonal planar (C)</p> Signup and view all the answers

Flashcards

Hybridization

Mixing atomic orbitals to form new hybrid orbitals.

Number of Hybrid Orbitals

Same as the number of atomic orbitals mixed.

Hybrid Orbitals

New orbitals formed by combining atomic orbitals.

Types of Hybrid Orbitals

sp, sp2, sp3, sp3d, sp3d2, etc.

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Predicting Hybridization

A process to determine the type of hybrid orbitals on a central atom, depending on the number of electron pairs and lone pairs.

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Sigma (σ) bond formation

A sigma bond forms when atomic orbitals overlap head-on along the internuclear axis.

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sp2 hybridization

Three hybrid orbitals are created from one s and two p orbitals.

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sp3 hybridization

Four hybrid orbitals are created from the combination of one s and three p orbitals

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Pi bond

A type of covalent bond where electron density is concentrated above and below the plane of the nuclei of the bonding atoms.

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Sigma bond

A type of covalent bond where electron density is concentrated along the internuclear axis, the line connecting the two nuclei.

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Single Bond

A bond formed by the sharing of one electron pair between two atoms, consisting of one sigma bond.

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Double Bond

A bond formed by the sharing of two electron pairs between two atoms, consisting of one sigma bond and one pi bond.

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Triple Bond

A bond formed by the sharing of three electron pairs between two atoms, consisting of one sigma bond and two pi bonds.

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How many sigma and pi bonds in a molecule?

To determine this, first draw the Lewis structure of the molecule. The number of single bonds corresponds to the number of sigma bonds. Then, the number of double or triple bonds indicates the number of pi bonds.

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Acetone (CH3)2CO: Bonds and Orbitals

Acetone has three carbon atoms connected in a chain. Two carbon atoms each have three hydrogen atoms attached, and the central carbon atom has a double bond to an oxygen atom. The bonds are sigma bonds between C-H and C-C, and a sigma bond between C-O. The double bond between C-O contains one sigma bond and one pi bond.

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Lewis Structure: What does it tell us?

The Lewis structure of a molecule helps us understand the arrangement of atoms and the distribution of bonding and nonbonding electrons. This helps us determine the number of sigma and pi bonds in the molecule.

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What type of hybridization is involved in the C=O bond?

The carbon atom in a C=O double bond undergoes sp2 hybridization. It forms three sp2 hybrid orbitals that are involved in sigma bonding with the oxygen atom, another carbon atom, and a hydrogen atom. The remaining unhybridized p orbital forms a pi bond with the oxygen atom's unhybridized p orbital.

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What type of hybridization occurs in a molecule with a triple bond?

Atoms involved in triple bonds undergo sp hybridization. One s and one p atomic orbital combine to form two sp hybridized orbitals. The remaining two p orbitals are unhybridized and form two pi bonds.

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How many sigma bonds are in the molecule?

Sigma bonds are formed by the overlap of orbitals along the internuclear axis. To count sigma bonds, count each single bond, as well as one bond from each double or triple bond.

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How many pi bonds are in the molecule?

Pi bonds are formed by the side-on overlap of unhybridized p orbitals. To count pi bonds, count the remaining bonds from double or triple bonds.

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What type of hybridization is present in a molecule with only single bonds?

Atoms forming only single bonds undergo sp3 hybridization. One s orbital and three p orbitals combine to form four sp3 hybrid orbitals, each of which forms a sigma bond.

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What is the shape of a molecule with sp3 hybridization?

sp3 hybridized atoms have a tetrahedral geometry with bond angles of approximately 109.5 degrees. This is because of the repulsion between the four electron pairs around the atom.

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What is the shape of a molecule with sp2 hybridization?

sp2 hybridized atoms have a trigonal planar geometry with bond angles of approximately 120 degrees.

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What is the shape of a molecule with sp hybridization?

sp hybridized atoms have a linear geometry with bond angles of 180 degrees.

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Hybridization in BeCl2

In gaseous BeCl2, the beryllium atom undergoes sp hybridization. This involves mixing one s and one p atomic orbital to form two sp hybrid orbitals, which then overlap with the p orbitals of the two chlorine atoms to form two sigma bonds.

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Orbital Overlap in BeCl2

In BeCl2, the two sp hybrid orbitals on the beryllium atom overlap head-on with the p orbitals of the chlorine atoms to form two sigma bonds. This overlap is responsible for the linear shape of the molecule.

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Study Notes

Valence Bond (VB) Theory and Orbital Hybridization

  • Valence Bond (VB) Theory explains covalent bonding by assuming overlap of atomic orbitals.
  • Orbital hybridization involves mixing of atomic orbitals to form new hybrid orbitals.
  • The number of hybrid orbitals equals the number of atomic orbitals mixed.
  • Hybridization type depends on the atomic orbitals involved.

Types of Hybrid Orbitals

  • sp: Linear shape
  • sp²: Trigonal planar shape (120°)
  • sp³: Tetrahedral shape (109.5°)
  • sp³d: Trigonal bipyramidal shape
  • sp³d²: Octahedral shape

Molecular Orbital (MO) Theory and Electron Delocalization

  • Molecular Orbital (MO) Theory describes bonding by combining atomic orbitals to form molecular orbitals.
  • Electrons fill molecular orbitals following the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
  • Delocalization of electrons in molecular orbitals leads to increased stability.

Sigma (σ) and Pi (π) Bonds

  • Sigma (σ) bonds: Formed by head-on overlap of atomic orbitals, concentrated along the internuclear axis.
  • Pi (Ï€) bonds: Formed by side-by-side overlap of p orbitals, concentrated above and below the internuclear axis.
  • Multiple bonds contain both sigma and pi bonds.
  • Single bonds are sigma bonds.

Determining Hybridization

  • Count the number of lone pairs and bonded atoms around the central atom.
  • Add the number of lone pairs and bonded atoms.
  • The resulting number corresponds to a specific hybridization type.

Hybrid Orbital Examples by central atom and molecule

  • BeClâ‚‚ (sp): Linear shape, 2 bonding pairs, 0 lone pairs
  • BF₃ (sp²): Trigonal planar shape, 3 bonding pairs, 0 lone pairs
  • CHâ‚„ (sp³): Tetrahedral shape, 4 bonding pairs, 0 lone pairs
  • NH₃ (sp³): Tetrahedral shape, 3 bonding pairs, 1 lone pair
  • Hâ‚‚O (sp³): Bent shape (non-linear), 2 bonding pairs, 2 lone pairs
  • PClâ‚… (sp³d): Trigonal bipyramidal shape, 5 bonding pairs, 0 lone pairs
  • SF₆ (sp³d²): Octahedral shape, 6 bonding pairs, 0 lone pairs

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Hybridization PDF

Description

This quiz explores Valence Bond (VB) Theory and the concept of orbital hybridization. It covers the types of hybrid orbitals, the hybridization process, and introduces Molecular Orbital (MO) Theory. Engage with the fundamental concepts that govern covalent bonding and electron delocalization.

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