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Questions and Answers
A molecular orbital can accommodate a maximum of ________ electron(s).
A molecular orbital can accommodate a maximum of ________ electron(s).
2
A typical double bond ________.
A typical double bond ________.
- Consists of one σ bond and one π bond (correct)
- Is stronger than a single bond (correct)
- Allows for rotation around the bond
- All of the above (correct)
A typical triple bond ________.
A typical triple bond ________.
consists of one σ bond and two π bonds
According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will be arranged in a(n) ________ geometry.
According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will be arranged in a(n) ________ geometry.
According to valence bond theory, which orbitals overlap in the formation of the bond in HCl?
According to valence bond theory, which orbitals overlap in the formation of the bond in HCl?
An electron domain consists of ________.
An electron domain consists of ________.
For which of the molecules is the molecular geometry the same as the VSEPR electron domain arrangement?
For which of the molecules is the molecular geometry the same as the VSEPR electron domain arrangement?
For a molecule with the formula AB3, the molecular shape is ________.
For a molecule with the formula AB3, the molecular shape is ________.
For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?
For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?
How many hybrid orbitals are formed upon the mixing of three atomic orbitals?
How many hybrid orbitals are formed upon the mixing of three atomic orbitals?
Of the following species, ________ will have bond angles of 120°.
Of the following species, ________ will have bond angles of 120°.
The π bond in ethylene, H2C=CH2, results from the overlap of ________.
The π bond in ethylene, H2C=CH2, results from the overlap of ________.
The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately ________.
The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately ________.
The bond angle marked a in the following molecule is about ________.
The bond angle marked a in the following molecule is about ________.
The central atom in a certain molecule has 1 nonbonded electron pair and 2 bonded electron pairs in its valence shell. The molecular geometry of this molecule is ________.
The central atom in a certain molecule has 1 nonbonded electron pair and 2 bonded electron pairs in its valence shell. The molecular geometry of this molecule is ________.
The electron domain and molecular geometry of SO3 are ________.
The electron domain and molecular geometry of SO3 are ________.
The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn will always be the same if ________.
The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn will always be the same if ________.
The electron-domain geometry of a boron-centered compound BH3 is trigonal planar. The hybridization of the central boron atom is ________.
The electron-domain geometry of a boron-centered compound BH3 is trigonal planar. The hybridization of the central boron atom is ________.
The hybridization and molecular shape of the carbon atom in carbon dioxide is ________.
The hybridization and molecular shape of the carbon atom in carbon dioxide is ________.
The hybridization of nitrogen in the H—C≡N: molecule is ________.
The hybridization of nitrogen in the H—C≡N: molecule is ________.
The molecular geometry of the BCl3 molecule is ________, and this molecule is ________.
The molecular geometry of the BCl3 molecule is ________, and this molecule is ________.
The molecular geometry of the BeCl2 molecule is ________, and this molecule is ________.
The molecular geometry of the BeCl2 molecule is ________, and this molecule is ________.
The molecular geometry of the BrO3- ion is ________.
The molecular geometry of the BrO3- ion is ________.
The molecular geometry of the CHCl3 molecule is ________.
The molecular geometry of the CHCl3 molecule is ________.
The molecular geometry of the CHF3 molecule is ________, and the molecule is ________.
The molecular geometry of the CHF3 molecule is ________, and the molecule is ________.
The molecular geometry of the H3O+ ion is ________.
The molecular geometry of the H3O+ ion is ________.
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
The molecular geometry of the left-most carbon atom in the molecule below is ________.
The molecular geometry of the left-most carbon atom in the molecule below is ________.
The molecular geometry of the right-most carbon in the molecule below is ________.
The molecular geometry of the right-most carbon in the molecule below is ________.
The sp2 atomic hybrid orbital set accommodates ________ electron domains.
The sp2 atomic hybrid orbital set accommodates ________ electron domains.
There are ________ σ and ________ π bond(s) in the H2C=CH2 molecule.
There are ________ σ and ________ π bond(s) in the H2C=CH2 molecule.
There is/are ________ π bond(s) in the molecule below.
There is/are ________ π bond(s) in the molecule below.
Using the VSEPR model, the electron-domain geometry of the central atom in O3 is ________.
Using the VSEPR model, the electron-domain geometry of the central atom in O3 is ________.
Using the VSEPR model, the molecular geometry of the central atom in CH4 is ________.
Using the VSEPR model, the molecular geometry of the central atom in CH4 is ________.
Using the VSEPR model, the molecular geometry of the central atom in SO3 is ________.
Using the VSEPR model, the molecular geometry of the central atom in SO3 is ________.
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Study Notes
Molecular Orbitals and Bonding
- A molecular orbital accommodates a maximum of 2 electrons.
- A typical double bond consists of one σ bond and one π bond.
- A typical triple bond consists of one σ bond and two π bonds.
VSEPR Theory
- According to VSEPR theory, three electron domains in an atom lead to a trigonal planar geometry.
- The molecular geometry matches the electron domain geometry for CCl4 and SF6.
Hybridization
- Two types of hybridization with distinct shapes:
- sp2 hybridization leads to a trigonal planar arrangement.
- sp hybridization results in a linear arrangement.
- The mixing of three atomic orbitals produces three hybrid orbitals.
- The hybridization of nitrogen in H—C≡N molecule is sp.
Molecular Shapes and Angles
- For AB3 molecules, shapes can vary: trigonal planar, trigonal pyramidal, or T-shaped depending on lone pairs.
- Geometrical configurations vary based on the numbers of bonded and lone pairs.
- Bond angles vary: BCl3 has bond angles of approximately 120°, while SiCl2F2 has bond angles of around 109.5°.
- Molecules with one central atom only need one lone pair for molecular polarity.
Specific Molecular Geometries
- Molecular geometries include:
- BCl3: trigonal planar, nonpolar.
- BeCl2: linear, nonpolar.
- BrO3-: trigonal pyramidal.
- CHCl3: tetrahedral.
- CHF3: tetrahedral and polar.
- H3O+: trigonal pyramidal.
- PF3: trigonal pyramidal and polar.
Electron Domains
- An electron domain can be defined as a region where electrons are likely to be found, including bonded atoms and lone pairs.
- The electron-domain geometry and molecular geometry align in the absence of lone pairs on the central atom.
σ and π Bonds
- In the H2C=CH2 molecule, there are 5 σ bonds and 1 π bond.
- The presence of π bonds typically involves overlap of p atomic orbitals.
General Molecular Models
- The molecular geometry of molecules can be identified through the VSEPR model, determining shapes like tetrahedral for CH4 and trigonal planar for SO3.
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