Hybridization

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Questions and Answers

What is the primary reason for the bent shape of the water molecule (H₂O)?

  • The equal distribution of bonding electrons around the oxygen atom.
  • The repulsion between the lone pairs of electrons on the oxygen atom. (correct)
  • The lack of hybridization of oxygen's 2s and 2p orbitals.
  • The presence of exactly two sigma bonds between oxygen and hydrogen atoms.

In the formation of water (H₂O), oxygen's 1s² electrons directly participate in the hybridization process.

False (B)

Describe the type of hybridization that occurs in the oxygen atom of a water molecule (H₂O) and explain how it affects the molecule's shape.

sp³ hybridization causes a bent molecular shape due to repulsion from two lone pairs.

In water (H₂O), the oxygen atom undergoes ______ hybridization, resulting in four hybrid orbitals.

<p>sp³</p> Signup and view all the answers

Match the following descriptions to the correct components regarding the formation of a water molecule:

<p>Oxygen's ground state electron configuration = 1s² 2s² 2p⁴ Hybridization type in water = sp³ Number of sigma bonds formed by oxygen = Two Effect of lone pairs on molecular shape = Bent shape</p> Signup and view all the answers

Considering the electron configuration of oxygen in a water molecule, which orbitals are involved in the sp³ hybridization process?

<p>The 2s and three 2p orbitals. (C)</p> Signup and view all the answers

The bond angle in a water molecule is exactly 109.5° due to perfect tetrahedral geometry.

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

Explain how the electron configuration of the oxygen atom changes during the formation of a water molecule, focusing on the role of its valence electrons.

<p>The 2s and 2p valence electrons rearrange into four sp³ hybridized orbitals, forming sigma bonds with hydrogen atoms.</p> Signup and view all the answers

Which of the following statements accurately describes the relationship between sigma ($\sigma$) and pi ($\pi$) bonds?

<p>Sigma bonds are stronger and form before pi bonds. (D)</p> Signup and view all the answers

In a molecule with sp² hybridization, you would expect to find two pi ($\pi$) bonds and two sigma ($\sigma$) bonds.

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

What type of hybridization is present in a molecule with a linear geometry and a bond angle of 180°?

<p>sp</p> Signup and view all the answers

A triple bond consists of one sigma ($\sigma$) bond and ______ pi ($\pi$) bonds.

<p>two</p> Signup and view all the answers

Match the following hybridizations with their corresponding geometries:

<p>sp³ = Tetrahedral sp² = Trigonal Planar sp = Linear</p> Signup and view all the answers

Which molecule is an example of sp³ hybridization?

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

Sp hybridization results in three hybrid orbitals and one unhybridized p orbital.

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

In ethene (C₂H₄ ), how many sigma and pi bonds are present between the two carbon atoms?

<p>One sigma bond and one pi bond</p> Signup and view all the answers

An atom with four sigma bonds and no pi bonds or lone pairs is hybridized as ______.

<p>sp³</p> Signup and view all the answers

What characteristic is associated with sigma ($\sigma$) bonds?

<p>Direct overlap of orbitals between two atoms. (C)</p> Signup and view all the answers

What is the primary reason why the bond angle in water (H₂O) is approximately 104.5° instead of the ideal tetrahedral angle of 109.5°?

<p>The repulsive forces between the two lone pairs of electrons on the oxygen atom. (C)</p> Signup and view all the answers

In sp² hybridization, one s orbital and two p orbitals combine to form three sp² hybrid orbitals, resulting in a tetrahedral geometry.

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

How many unhybridized p orbitals remain when a carbon atom undergoes sp hybridization?

<p>two</p> Signup and view all the answers

In ethene (C₂H₄), each carbon atom undergoes sp² hybridization, forming a ______ bond between the two carbon atoms.

<p>pi</p> Signup and view all the answers

Match each type of hybridization with its corresponding molecular geometry:

<p>sp = Linear sp² = Trigonal Planar sp³ = Tetrahedral</p> Signup and view all the answers

Which type of hybridization is associated with molecules containing triple bonds?

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

Hybridization fundamentally changes the electron configuration of an atom by altering the number of core electrons.

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

What is the bond angle in a molecule with linear geometry resulting from sp hybridization?

<p>180</p> Signup and view all the answers

Oxygen has ______ unpaired electrons, each occupying a different 2p orbital.

<p>two</p> Signup and view all the answers

In H₂O, how many of the sp³ hybrid orbitals on oxygen are used to form sigma (σ) bonds with hydrogen atoms?

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

The concept of hybridization is used because unhybridized atomic orbitals always accurately predict molecular shapes and bonding.

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

What is the spatial arrangement of the three sp² hybrid orbitals?

<p>trigonal planar</p> Signup and view all the answers

Which of the following describes the 'effective' configuration of oxygen after sp³ hybridization in H₂O?

<p>1s² (sp³)^4 (A)</p> Signup and view all the answers

In sp hybridization, two ______ orbitals remain unhybridized and can participate in forming pi bonds.

<p>2p</p> Signup and view all the answers

How many sigma (σ) bonds does each carbon atom form with hydrogen atoms in ethene (C₂H₄)?

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

Flashcards

What is Hybridization?

The mixing of atomic orbitals to form new hybrid orbitals suitable for chemical bonding.

What are sp³ hybrid orbitals?

Hybrid orbitals formed by mixing one 2s and three 2p orbitals.

What is Oxygen (O)?

Atomic number 8; its electron configuration is 1s² 2s² 2p⁴.

What are valence orbitals?

The outermost electron shell; the 2s² and 2p⁴ orbitals are these for oxygen.

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What is sp³ hybridization in water?

In H₂O, the oxygen atom undergoes this; the 2s and three 2p orbitals mix to form four sp³ hybrid orbitals.

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What are the functions of the four sp³ orbitals in H₂O?

Two of these contain lone pairs; the other two form bonds with hydrogen atoms in H₂O.

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Why does H₂O have a bent shape?

The shape of the water molecule due to repulsion between lone pairs of electrons, leading to a bond angle of about 104.5°.

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How does H₂O form sigma bonds?

Each hydrogen atom contributes one 1s electron that overlaps with oxygen’s sp³ hybrid orbitals to form two sigma bonds.

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sp³ Hybridization

Mixing one s and three p orbitals to form four hybrid orbitals.

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sp³ Geometry

Tetrahedral shape with 109.5° bond angles.

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sp² Hybridization

Mixing one s and two p orbitals to form three hybrid orbitals.

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sp² Geometry

Trigonal planar shape with 120° bond angles.

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sp Hybridization

Mixing one s and one p orbital to form two hybrid orbitals.

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sp Geometry

Linear shape with 180° bond angles.

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Sigma (σ) Bond

Formed by direct overlap of orbitals; single bonds.

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Pi (π) Bond

Formed by side-by-side overlap of unhybridized p orbitals; double/triple bonds.

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sp³ Hybridization Rule

Atom with four sigma bonds/lone pairs.

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sp² Hybridization Rule

Atom with three sigma bonds and one pi bond.

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Valence Orbitals

Orbitals important for bonding; for oxygen, these are 2s² 2p⁴.

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Hybridization

Mixing atomic orbitals (like 2s and 2p) to form new hybrid orbitals.

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sp³ Orbitals in Water (H₂O)

Two sp³ orbitals form bonds, two hold lone pairs.

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Bond Angle of Water (H₂O)

The angle is ~104.5° due to lone pair repulsion.

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Shape of Water (H₂O)

Bent or V-shaped.

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Oxygen's Configuration After sp³ Hybridization in H₂O

1s² (sp³)⁴, where sp³ orbitals account for both bonding and lone pairs.

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Geometry of sp² Orbitals

Trigonal planar, 120° apart.

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Unhybridized p Orbital in sp²

Forms pi (π) bonds, like in double compounds.

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sp² Hybridization in Ethene (C₂H₄)

Each carbon utilizes sp² hybridization.

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Two sigma (σ) bonds with two hydrogen atoms with sp² in Ethene (C₂H₄)

One sigma (σ) bond between the two carbon atoms.

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Geometry of sp Orbitals

Linear, 180° bond angle.

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Unhybridized p Orbitals in sp

Forms two pi (π) bonds, found in triple compounds.

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Study Notes

  • In hybridization, 2s and 2p orbitals combine to form sp, sp², or sp³ hybrid orbitals depending on the bonding environment.

sp³ Hybridization and H₂O

  • Oxygen (O) has an atomic number of 8, with an electron configuration of 1s² 2s² 2p⁴.
  • Valence orbitals (2s² and 2p⁴) participate in bonding.
  • Oxygen atom in H₂O undergoes sp³ hybridization, where the 2s orbital and three 2p orbitals mix to form four sp³ hybrid orbitals.
  • Two sp³ orbitals contain lone pairs, and two form sigma bonds with hydrogen atoms.
  • H₂O has a bent shape with a bond angle of about 104.5° due to repulsion between lone pairs.
  • Oxygen starts with 1s² 2s² 2p⁴, then hybridizes to four sp³ orbitals for bonding.
  • Two sp³ orbitals bond with hydrogen atoms.
  • Two sp³ orbitals remain as lone pairs.

Electron Configuration Post-Hybridization

  • For oxygen in H₂O the original electron configuration before bonding is 1s² 2s² 2p⁴.
  • Post-hybridization, the 2s and 2p orbitals combine to form four sp³ hybrid orbitals.
  • Two sp³ hybrid orbitals contain lone pairs.
  • Two sp³ hybrid orbitals form O-H sigma bonds by overlapping with hydrogen 1s electrons.
  • Effective configuration after hybridization is: 1s² (sp³)⁴.

sp² Hybridization

  • One 2s orbital and two 2p orbitals combine to form three sp² hybrid orbitals.
  • Shape of the three sp² hybrid orbitals is trigonal planar geometry, 120° apart.
  • One 2p orbital remains unhybridized and can form pi (π) bonds (usually in double bonds).
  • Each carbon in ethene undergoes sp² hybridization.
  • Three sp² hybrid orbitals on each carbon:
  • Two sigma (σ) bonds with two hydrogen atoms
  • One sigma (σ) bond between the two carbon atoms
  • One unhybridized 2p orbital on each carbon creates a pi (π) bond between the two carbons, forming a C=C double bond.

sp Hybridization

  • One 2s orbital and one 2p orbital combine to form two sp hybrid orbitals.
  • Two sp hybrid orbitals arrange in are arranged in a linear geometry at 180°.
  • Two 2p orbitals remain unhybridized and create two pi (π) bonds (usually in triple bonds).
  • Each carbon atom in ethyne undergoes sp hybridization.
  • Two sp hybrid orbitals on each carbon:
  • One sigma (σ) bond with hydrogen
  • One sigma (σ) bond between the two carbon atoms
  • Two unhybridized 2p orbitals on each carbon form two pi (π) bonds, creating the C≡C triple bond.

Hybridization Summary

  • sp³ Hybridization
  • Orbitals is one s + three p = four sp³ hybrid orbitals.
  • Geometry: tetrahedral, 109.5° bond angles.
  • Example: methane (CH₄), H₂O.
  • No unhybridized p orbitals.
  • sp² Hybridization
  • Orbitals is one s + two p = three sp² hybrid orbitals.
  • Geometry: trigonal planar, 120° bond angles.
  • Example: ethene (C₂H₄).
  • One unhybridized p orbital, forms π bonds.
  • sp Hybridization
  • Orbitals is one s + one p = two sp hybrid orbitals.
  • Geometry: linear, 180° bond angles.
  • Example: ethyne (C₂H₂).
  • Two unhybridized p orbitals, forms π bonds.

Hybridization, Geometry, and Bonding Summary

  • sp³: 4 hybrid orbitals, tetrahedral geometry, 109.5° bond angles.
  • Example: methane (CH₄), H₂O.
  • Four sigma bonds (CH₄); two sigma bonds + two lone pairs (H₂O).
  • No unhybridized p orbitals; only sigma bonds.
  • sp²: 3 hybrid orbitals, trigonal planar geometry, 120° bond angles.
  • Example: ethene (C₂H₄).
  • Three sigma bonds; one pi bond in double bonds.
  • One unhybridized p orbital; forms one pi bond and three sigma bonds.
  • sp: 2 hybrid orbitals, linear geometry, 180° bond angles.Ethyne (C₂H₂).
  • Example: ethyne (C₂H₂).
  • Two sigma bonds; two pi bonds in triple bonds.
  • Two unhybridized p orbitals; forms two pi bonds and two sigma bonds.

Sigma (σ) and Pi (π) Bonds

  • Sigma (σ) Bonds is the strongest covalent bond.
  • Formed by direct overlap of orbitals between atoms.
  • Can form from overlap of hybrid orbitals (sp, sp², sp³) or hybrid and non-hybridized orbitals (s).
  • All single bonds consist of one sigma bond.
  • Pi (π) Bonds form when two unhybridized p orbitals overlap side-by-side.
  • Forms only after a sigma bond.
  • Occur in double or triple bonds.
  • Double bond is one sigma bond and one pi bond.
  • Triple bond is one sigma bond and two pi bonds.
  • Sigma bonds allow free rotation, pi bonds restrict rotation.

Determining Hybridization and Bond Type

  • sp³ - Atom with four sigma bonds or lone pairs with no pi bonds is sp³ hybridized.
    • Examples: methane (CH₄), water (H₂O).
    • Tetrahedral geometry, no pi bonds (only sigma bonds).
  • sp² - Atom with three sigma bonds and one pi bond is sp² hybridized.
    • Example: ethene (C₂H₄).
    • Trigonal planar geometry; pi bonds occur in double bonds.
    • Double bonds consist of one sigma bond and one pi bond.
  • sp - Atom with two sigma bonds and two pi bonds is sp hybridized.
    • Example: ethyne (C₂H₂).
    • Linear geometry; pi bonds occur in triple bonds.
    • Triple bonds consist of one sigma bond and two pi bonds.

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