The Lewis structure and geometry of Al 2 Cl 6 is to be shown, the hybridization state of aluminum in AlCl 3 and Al 2 Cl 6 is to be described, and whether the molecules AlCl 3 and Al 2 Cl 6 possess dipole moment or not is to be determined. Concept introduction: Hybrid orbital theory is based upon the formation of hybrid orbitals by the mixing of atomic orbitals. To explain bonding by hybrid orbitals, the number of electrons around the central atom is determined by drawing the Lewis structure of the molecule. The ground state orbital diagram for the central atom is drawn. Excitation of electrons to higher orbitals occurs to get the highest number of unpaired electrons. The required number of hybrid orbitals are combined to obtain the hybridization of the central atom. Electron domain is the bond pair and lone pair of electrons around the central atom.
The Lewis structure and geometry of Al 2 Cl 6 is to be shown, the hybridization state of aluminum in AlCl 3 and Al 2 Cl 6 is to be described, and whether the molecules AlCl 3 and Al 2 Cl 6 possess dipole moment or not is to be determined. Concept introduction: Hybrid orbital theory is based upon the formation of hybrid orbitals by the mixing of atomic orbitals. To explain bonding by hybrid orbitals, the number of electrons around the central atom is determined by drawing the Lewis structure of the molecule. The ground state orbital diagram for the central atom is drawn. Excitation of electrons to higher orbitals occurs to get the highest number of unpaired electrons. The required number of hybrid orbitals are combined to obtain the hybridization of the central atom. Electron domain is the bond pair and lone pair of electrons around the central atom.
Solution Summary: The author explains the Lewis structure and geometry of Al_Text2 TextCl
The Lewis structure and geometry of Al2Cl6 is to be shown, the hybridization state of aluminum in AlCl3 and Al2Cl6 is to be described, and whether the molecules AlCl3 and Al2Cl6 possess dipole moment or not is to be determined.
Concept introduction:
Hybrid orbital theory is based upon the formation of hybrid orbitals by the mixing of atomic orbitals.
To explain bonding by hybrid orbitals, the number of electrons around the central atom is determined by drawing the Lewis structure of the molecule.
The ground state orbital diagram for the central atom is drawn.
Excitation of electrons to higher orbitals occurs to get the highest number of unpaired electrons.
The required number of hybrid orbitals are combined to obtain the hybridization of the central atom.
Electron domain is the bond pair and lone pair of electrons around the central atom.
For each of the following molecule: (i) draw the correct Lewis structure; (ii) determine the molecular geometry and the type of hybridization on the central atom, and (iii) predict whether the molecule is polar or nonpolar.
(a) BrCl5
Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths:
(a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.
A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.
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Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY