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∙ 12y agoH2O, with a bond angle of 104.5 degrees due to its three areas of electron density.
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∙ 12y agoClO3F would be tetrahedral.
In terms of struture, lone pairs contribute helping a molecule acquire a shape as dictated by VSEPR Theory (Valence Shell Electron Pair Repulsion Theory). Regarding chemical properties lone pair/s of electrons can make a molecule act as a Lewis base (like ammonia) in the reaction mixtures the extent of which depends on various other features in the structure of molecule.
Repulsion of the unshared electron pairs (2)and the bonded pairs (2) around the central oxygen atom. Repulsion of these 4 electron pairs attempts to form a tetrahedral shape. Describing the molecular shape, we ignore the unshared electrons and just describe the shape of the molecule based on the location of the atoms, thus bent.
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A. The geometry it will have
According to VSEPR theory, the carbon tetraiodide molecule (CI4) will have a square planar shape. This is because it has four bonding pairs of electrons around the central carbon atom, leading to a bond angle of 90 degrees and a symmetrical arrangement.
The VSEPR theory for an ammonia (NH3) molecule predicts that the molecule has a trigonal pyramidal shape. This is because the nitrogen atom has one lone pair of electrons, causing the bond angles to be slightly less than the ideal 109.5 degrees.
SiCl4 has a tetrahedral shape according to the VSEPR theory. Each Cl atom is located at the corner of the tetrahedron, with the silicon atom at the center.
The molecule HCl consists of only two atoms, hydrogen and chlorine, resulting in a linear molecular geometry. Due to its simplicity and lack of lone pairs on the central atom, hydrogen, VSEPR theory is not needed to predict the shape of HCl.
The VSEPR theory allows us to determine the molecular geometry of a molecule based on the number of electron pairs around the central atom. It helps predict the shape of molecules by minimizing electron pair repulsion. This theory is useful in understanding the spatial arrangement of atoms in molecules and their properties.
The VSEPR theory explains how the geometric arrangement of atoms around a central atom in a molecule affects the molecule's shape. It helps predict the shape of molecules based on the number of electron pairs (both bonding and non-bonding) around the central atom.
THC (tetrahydrocannabinol) does not have a defined VSEPR shape as it is a molecule with a complex structure containing multiple rings and functional groups. The molecule is quite flexible, leading to variations in its geometry.
Electrons influence the shape of a molecule through their distribution around the nucleus, which affects the bonding between atoms. The sharing or transfer of electrons between atoms makes chemical bonds that determine the geometry of the molecule. The arrangement of electron pairs (bonding and non-bonding) around the central atom determines the molecule's shape according to VSEPR theory.
VSEPR stands for Valence Shell Electron Pair Repulsion, and it describes how valence (bonding) electrons are arranged around an atom, and how they are used in creating a bond. This then can be used to help predict the GEOMETRIC SHAPE of the molecule being formed.
Valence electron pairs will move as far apart from each other as possible. (Apex)
Electron pairs repelling each other push atoms apart.