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Questions and Answers
What is the bond order for B2?
What is the bond order for B2?
For C2, how many electrons occupy the antibonding orbitals?
For C2, how many electrons occupy the antibonding orbitals?
What type of interference results in the σ 2pz bonding molecular orbital?
What type of interference results in the σ 2pz bonding molecular orbital?
In which case is the energy ordering of (π2px) and (π2py) lower than (σ2pz)?
In which case is the energy ordering of (π2px) and (π2py) lower than (σ2pz)?
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Why is O2 considered highly reactive?
Why is O2 considered highly reactive?
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What type of bond is formed between the carbon and hydrogen atoms in methane?
What type of bond is formed between the carbon and hydrogen atoms in methane?
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What is the geometry of ammonia (NH3) resulting from its hybridization?
What is the geometry of ammonia (NH3) resulting from its hybridization?
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In ethylene (C2H4), which type of bond is formed in addition to the sigma bond between the carbon atoms?
In ethylene (C2H4), which type of bond is formed in addition to the sigma bond between the carbon atoms?
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What causes the bond angles in water (H2O) to be smaller than the ideal angle for tetrahedral geometry?
What causes the bond angles in water (H2O) to be smaller than the ideal angle for tetrahedral geometry?
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What hybridization occurs in acetylene (C2H2)?
What hybridization occurs in acetylene (C2H2)?
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What is the main reason for nitrogen not promoting an electron to a higher energy orbital during hybridization?
What is the main reason for nitrogen not promoting an electron to a higher energy orbital during hybridization?
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Which hybridization results from the combination of one s orbital and two p orbitals?
Which hybridization results from the combination of one s orbital and two p orbitals?
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What type of molecular orbitals are formed in homonuclear diatomic molecules originating from s and p orbitals?
What type of molecular orbitals are formed in homonuclear diatomic molecules originating from s and p orbitals?
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What type of bond is formed when two atomic orbitals pair unpaired electrons?
What type of bond is formed when two atomic orbitals pair unpaired electrons?
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Which of the following describes a pi bond?
Which of the following describes a pi bond?
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How many total bonds can carbon form through sp3 hybridization?
How many total bonds can carbon form through sp3 hybridization?
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What is the hybridization state of carbon in methane (CH4)?
What is the hybridization state of carbon in methane (CH4)?
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In which scenario would carbon exhibit sp hybridization?
In which scenario would carbon exhibit sp hybridization?
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Which characteristic is true for sp3 hybrid orbitals?
Which characteristic is true for sp3 hybrid orbitals?
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What feature distinguishes a single bond from a double bond?
What feature distinguishes a single bond from a double bond?
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Which of the following best defines hybridization in atomic orbitals?
Which of the following best defines hybridization in atomic orbitals?
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What is the bond order for Helium (He2)?
What is the bond order for Helium (He2)?
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Which of the following correctly describes the relationship between bonding and antibonding orbitals?
Which of the following correctly describes the relationship between bonding and antibonding orbitals?
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How many molecular orbitals are formed from two atomic orbitals?
How many molecular orbitals are formed from two atomic orbitals?
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What is the bond order for H2 according to the molecular orbital theory?
What is the bond order for H2 according to the molecular orbital theory?
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Which type of orbital results from destructive interference of two atomic orbitals?
Which type of orbital results from destructive interference of two atomic orbitals?
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For which of the following molecules does the molecule theoretically exist based on the bond order calculation?
For which of the following molecules does the molecule theoretically exist based on the bond order calculation?
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What is true about π*-orbitals when two p orbitals interfere?
What is true about π*-orbitals when two p orbitals interfere?
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What happens to the energy of bonding orbitals when two atomic orbitals combine?
What happens to the energy of bonding orbitals when two atomic orbitals combine?
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What is the primary characteristic of molecular orbitals in MO theory?
What is the primary characteristic of molecular orbitals in MO theory?
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What does a bonding molecular orbital signify in terms of energy?
What does a bonding molecular orbital signify in terms of energy?
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Which statement correctly describes antibonding molecular orbitals?
Which statement correctly describes antibonding molecular orbitals?
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What is the function of the linear combination of atomic orbitals (LCAO) in forming molecular orbitals?
What is the function of the linear combination of atomic orbitals (LCAO) in forming molecular orbitals?
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In terms of electron probability density, what occurs in the region between the nuclei of two atoms in a bonding molecular orbital?
In terms of electron probability density, what occurs in the region between the nuclei of two atoms in a bonding molecular orbital?
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Which of the following statements about the energy levels of molecular orbitals is true?
Which of the following statements about the energy levels of molecular orbitals is true?
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What happens to the probability density of electrons in an antibonding molecular orbital?
What happens to the probability density of electrons in an antibonding molecular orbital?
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In the molecular orbital theory, which molecular orbital designation indicates a bonding orbital derived from s orbitals?
In the molecular orbital theory, which molecular orbital designation indicates a bonding orbital derived from s orbitals?
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Study Notes
Chemical Bonding II: Orbital Hybridisation
- Orbital hybridisation is a concept in valence bond theory
- It describes the mixing of atomic orbitals to form new hybrid orbitals
- This allows atoms to form different types of bonds (sigma and pi)
Valence Bond Theory
- Considers atomic orbital interactions on separate atoms forming molecules
- Bonds form from pairing unpaired electrons in atomic orbitals
- Wavefunctions of electron pairs are combined (superimposed) from fragments of molecules
Sigma (σ) and Pi (π) Bonds
-
Sigma (σ) bonds: Cylindrically symmetrical around the bond axis; no nodal plane.
- For example, a σ bond can form between two 's' orbitals, 's' and 'p', or two 'p' orbitals
-
Pi (π) bonds: Electron density in two lobes with a single nodal plane along the bond axis
- A π bond is formed in addition to a sigma bond to form double or triple bonds
sp³ Hybridisation
- Formed from one 's' orbital and three 'p' orbitals
- Example: Methane (CH₄)
- Results in tetrahedral geometry (109.5° bond angles)
sp² Hybridisation
- Formed from one 's' orbital and two 'p' orbitals
- Example: Ethylene (C₂H₄)
- Results in trigonal planar geometry (120° bond angles)
sp Hybridisation
- Formed from one 's' orbital and one 'p' orbital
- Example: Acetylene (C₂H₂)
- Results in linear geometry (180° bond angle)
Molecular Orbital (MO) Theory
- Valence electrons are delocalized across the entire molecule
- Molecular orbitals (MOs) are formed by combining atomic orbitals
- Linear combination of atomic orbitals (LCAO) forms bonding and antibonding MOs
Homonuclear Diatomic Molecules
- Molecules of the same atom
- Example: H₂, He₂, Li₂
- MO diagrams show how atomic orbitals combine to form MOs
- Bond order is calculated to determine the stability of a molecule
Heteronuclear Diatomic Molecules
- Molecules of different atoms
- Example: HCl, CO, NO
- Energy level ordering of MOs can be different from that of homonuclear molecules
- Depends on the electronegativity difference between the atoms
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Description
Explore the intricacies of orbital hybridisation within valence bond theory. Understand the formation of sigma and pi bonds as well as the significance of sp³ hybridisation in molecules like methane. This quiz will test your comprehension of how atomic orbitals interact to create different bonding scenarios.
