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Jul 8
Methane (CH4) is a simple hydrocarbon molecule composed of one carbon atom bonded to four hydrogen atoms. The structure of methane is a tetrahedral shape, with the carbon atom at the center and the four hydrogen atoms positioned at the four corners of the tetrahedron. Each hydrogen atom is bonded to the carbon atom through a single covalent bond, resulting in a stable and symmetrical molecule.
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Google Gemini AI
Jul 8
Tetrahedral Structure
Methane (CH₄) has a tetrahedral molecular geometry, which is the simplest three-dimensional shape with four equivalent bonds.
Carbon Atom at the Center
The carbon atom is located at the center of the tetrahedron.
Hydrogen Atoms at the Corners
The four hydrogen atoms are located at the four corners of the tetrahedron.
Bond Angles
The carbon-hydrogen bond angles are all approximately 109.5 degrees. This is known as the tetrahedral angle and is due to the repulsion between the electron pairs around the carbon atom.
Bond Lengths
The carbon-hydrogen bond lengths are all approximately 1.09 angstroms.
Key Features of the Tetrahedral Structure:
- All the bonds are equivalent.
- The molecule is nonpolar.
- It has no permanent dipole moment.
- The electron density is evenly distributed around the molecule.
- The carbon atom is sp³ hybridized.
Additional Notes:
- The tetrahedral structure of methane is due to the hybridization of the carbon atom's atomic orbitals.
- The four valence electrons of carbon are hybridized to form four equivalent sp³ hybrid orbitals.
- Each sp³ orbital overlaps with an s orbital of a hydrogen atom to form a carbon-hydrogen bond.
- The tetrahedral geometry minimizes the electron-electron repulsion between the electron pairs around the carbon atom.
Methane (CH₄) has a tetrahedral molecular geometry, which is the simplest three-dimensional shape with four equivalent bonds.
Carbon Atom at the Center
The carbon atom is located at the center of the tetrahedron.
Hydrogen Atoms at the Corners
The four hydrogen atoms are located at the four corners of the tetrahedron.
Bond Angles
The carbon-hydrogen bond angles are all approximately 109.5 degrees. This is known as the tetrahedral angle and is due to the repulsion between the electron pairs around the carbon atom.
Bond Lengths
The carbon-hydrogen bond lengths are all approximately 1.09 angstroms.
Key Features of the Tetrahedral Structure:
- All the bonds are equivalent.
- The molecule is nonpolar.
- It has no permanent dipole moment.
- The electron density is evenly distributed around the molecule.
- The carbon atom is sp³ hybridized.
Additional Notes:
- The tetrahedral structure of methane is due to the hybridization of the carbon atom's atomic orbitals.
- The four valence electrons of carbon are hybridized to form four equivalent sp³ hybrid orbitals.
- Each sp³ orbital overlaps with an s orbital of a hydrogen atom to form a carbon-hydrogen bond.
- The tetrahedral geometry minimizes the electron-electron repulsion between the electron pairs around the carbon atom.
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