Question

Показать гибридизацию электронных облаков центрального атома в молекуле PH3 и геометрическую форму этой молекулы, когда угол между химическими связями составляет 93 ° 18`. Сравните полярность химической связи с этой молекулой и всей молекулой.

Answer 1

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Answer 2

Hybridization of Electronic Orbitals in PH3 Molecule

In the molecule PH3 (phosphine), the central atom is phosphorus (P). To determine the hybridization of the electronic orbitals around the central atom, we need to consider the number of electron groups (bonded atoms and lone pairs) around the central atom.

Phosphorus has 5 valence electrons. In PH3, there are 3 hydrogen atoms bonded to the central phosphorus atom, and there is one lone pair of electrons on phosphorus. Therefore, there are a total of 4 electron groups around the central atom.

The hybridization of the electronic orbitals in PH3 can be determined using the following guidelines:

- If there are 2 electron groups, the hybridization is sp. - If there are 3 electron groups, the hybridization is sp2. - If there are 4 electron groups, the hybridization is sp3. - If there are 5 electron groups, the hybridization is sp3d. - If there are 6 electron groups, the hybridization is sp3d2.

Since there are 4 electron groups around the central phosphorus atom in PH3, the hybridization of the electronic orbitals is sp3.

Geometric Shape of PH3 Molecule

The geometric shape of a molecule is determined by the arrangement of the bonded atoms and lone pairs around the central atom. In PH3, the central phosphorus atom is surrounded by 3 hydrogen atoms and 1 lone pair of electrons.

The arrangement of these electron groups in PH3 is tetrahedral. The bond angles in a tetrahedral arrangement are approximately 109.5 degrees. However, in this case, the given angle between the chemical bonds is 93 degrees and 18 minutes.

The actual bond angle in PH3 is slightly less than the ideal tetrahedral angle of 109.5 degrees due to the repulsion between the lone pair of electrons and the bonded atoms. The presence of the lone pair causes a slight compression of the bond angles.

Therefore, the geometric shape of the PH3 molecule, with an angle of 93 degrees and 18 minutes between the chemical bonds, is trigonal pyramidal.

Polarity of the Chemical Bond and the Molecule

To determine the polarity of a chemical bond or molecule, we need to consider the electronegativity difference between the atoms involved in the bond.

In the case of PH3, phosphorus (P) is less electronegative than hydrogen (H). Therefore, the P-H bonds are polar, with the hydrogen atom being slightly more electronegative and having a partial negative charge, while the phosphorus atom has a partial positive charge.

However, the overall polarity of the PH3 molecule depends on the molecular geometry and the vector sum of the individual bond polarities.

In a trigonal pyramidal molecule like PH3, the lone pair of electrons on the central atom creates an uneven distribution of electron density. This results in an overall molecular polarity.

Therefore, the PH3 molecule is polar due to the presence of the lone pair and the asymmetric arrangement of the polar P-H bonds.

Note: The polarity of a molecule can also be influenced by other factors such as molecular symmetry and molecular interactions.