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8.3. Molecular Orbitals. Molecular Orbitals How are atomic and molecular orbitals related?. 8.3. Molecular Orbitals. When two atoms combine, the molecular orbital model assumes that their atomic orbitals overlap to produce molecular orbitals , or orbitals that apply to the entire molecule.
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8.3 Molecular Orbitals • Molecular Orbitals • How are atomic and molecular orbitals related?
8.3 Molecular Orbitals • When two atoms combine, the molecular orbital model assumes that their atomic orbitals overlap to produce molecular orbitals, or orbitals that apply to the entire molecule.
8.3 Molecular Orbitals • Just as an atomic orbital belongs to a particular atom, a molecular orbital belongs to a molecule as a whole. • A molecular orbital that can be occupied by two electrons of a covalent bond is called a bonding orbital.
8.3 Molecular Orbitals • Sigma Bonds • When two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting two atomic nuclei, a sigma bond is formed.
8.3 Molecular Orbitals • A Sigma Bond
8.3 Molecular Orbitals • When two fluorine atoms combine, the p orbitals overlap to produce a bonding molecular orbital. The F—F bond is a sigma bond.
8.3 Molecular Orbitals • Pi Bonds • In a pi bond (symbolized by the Greek letter ), the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms.
8.3 Molecular Orbitals • Pi-bonding Molecular Orbital
8.3 VSEPR Theory • VSEPR Theory • How does VSEPR theory help predict the shapes of molecules?
8.3 VSEPR Theory • The valence-shell electron-pair repulsion theory, or VSEPR theory, explains the three-dimensional shape of methane.
8.3 VSEPR Theory • According to VSEPR theory, the repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far apart as possible.
8.3 VSEPR Theory • The hydrogens in a methane molecule are at the four corners of a geometric solid. All of the H—C—H angles are 109.5°, the tetrahedral angle.
8.3 VSEPR Theory • An ammonia molecule is pyramidal. The unshared pair of electrons repels the bonding pairs. The measured H—N—H bond angle is only 107°.
8.3 VSEPR Theory • The measured bond angle in water is about 104.5°
8.3 VSEPR Theory • The carbon dioxide molecule is linear.
8.3 VSEPR Theory • Nine Possible Molecular Shapes
8.3 Hybrid Orbitals • Hybrid Orbitals • In what ways is orbital hybridization useful in describing molecules?
8.3 Hybrid Orbitals • Orbital hybridization provides information about both molecular bonding and molecular shape. • In hybridization, several atomic orbitals mix to form the same total number of equivalent hybrid orbitals.
8.3 Hybrid Orbitals • Hybridization Involving Single Bonds
8.3 Hybrid Orbitals • Hybridization Involving Double Bonds
8.3 Hybrid Orbitals • Hybridization Involving Triple Bonds
8.3 Section Quiz. • 1. A molecular orbital belongs to a • specific atom. • molecule as a whole. • specific pair of atoms. • central atom.
8.3 Section Quiz. • 2. VSEPR theory enables prediction of 3-dimensional molecular shape because the valence electron pairs • are attracted to each other. • form molecules with only four possible shapes. • stay as far apart as possible. • always form tetrahedral shapes.
8.3 Section Quiz. • 3. Orbital hybridization provides information about • both molecular bonding and molecular shape. • both molecular bonding and bond energy. • neither molecular bonding nor molecular shape. • neither molecular bonding nor bond energy.
