HOMO stands for highest occupied molecular orbital, representing the highest energy level at which an electron can be found in a molecule. LUMO stands for lowest unoccupied molecular orbital, representing the lowest energy level at which an electron can be promoted to in a molecule. These orbitals are important in understanding chemical reactivity and properties.
The Highest Occupied Molecular Orbital (HOMO) of butadiene is a pi orbital located above and below the plane of the molecule, created from the overlap of the p orbitals on each carbon atom in the conjugated system. This orbital is responsible for the involvement of butadiene in various chemical reactions and its unique reactivity.
Homopolypropylene is made up of only propylene monomer units, while copolypropylene contains a mixture of propylene and other comonomer monomer units. This difference in composition results in variations in properties such as melting point, density, and chemical resistance between homo and copolypropylene materials. Copolypropylene is often used to improve impact resistance and flexibility compared to homopolypropylene.
It is a hydrocarbon with the formula, C4H10
4
Butane is not an element, but a complex hydrocarbon molecule, C4H10.
The bond anhles are 109.5 degrees so it is tetrahedral.
C4H10, also known as butane, is a nonpolar molecule. This is because it is symmetrical with carbon atoms attached to hydrogen atoms, resulting in an equal distribution of charge and no overall dipole moment.
The prefix "but-" indicates a molecule with 4 carbon atoms. Examples include butane (C4H10) and butene (C4H8).
To draw two isomers of butane, start with the straight-chain butane molecule (C4H10) and then draw the branched isomer, known as 2-methylpropane (C4H10). The second isomer can be drawn by rearranging the carbon atoms to create a different branched isomer, such as 2,2-dimethylpropane (C4H10).
No, C4H10 (butane) and H2O (water) are not miscible because they have different polarities. Butane is a nonpolar hydrocarbon while water is a polar molecule. As a result, they do not mix together and will form separate layers.
The intermolecular forces present in C4H10 (butane) are primarily London dispersion forces. As a nonpolar molecule, butane does not have dipole-dipole interactions or hydrogen bonding. The London dispersion forces result from temporary dipoles that occur due to fluctuations in electron distribution within the molecule.
C4H10 is the molecular formula for butane, as it represents the actual number of atoms of each element in a single molecule of the compound. The empirical formula for butane would be CH5, as it shows the simplest whole number ratio of atoms present in the compound.
The standard enthalpy of formation for liquid butane (C4H10) is -126 kJ/mol.
1 mole C4H10 = 58.1222g = 6.022 x 1023 molecules 11.7g C4H10 x 6.022 x 1023 molecules/58.1222g = 1.21 x 1023 molecules C4H10