Question

In what way(s) is(are) the structure of water similar to that of CHCl3? In what way is the structure of water different from that of CHCl3?

Answer 1

The structure of water (H₂O) and CHCl₃ are similar in their polarity and polar covalent bonds; both have a central atom in a tetrahedral arrangement with water having a bent shape. They differ in the types of atoms they are bonded to, water's lone pairs affecting its bond angle, and the resultant physical and chemical properties.

Step-by-step explanation:

The structure of water (H₂O) is similar to that of CHCl₃ in that both molecules are polar and have polar covalent bonds. The primary similarity is the presence of a central atom (oxygen in water and carbon in CHCl₃) bonded to other atoms in a tetrahedral geometry, although water has a bent shape due to its two lone pairs. Water's hydrogen atoms are positively charged due to oxygen's higher electronegativity, similarly, in CHCl₃ the chlorine atoms are more electronegative than the carbon.

The differences lie in the bonded atoms and the result of the molecule's electron distribution. Water is a molecule with two hydrogen atoms attached to an oxygen atom, while CHCl₃ contains three chlorine atoms and one hydrogen atom attached to a carbon atom. This results in different physical and chemical properties such as boiling points and solubility in water. Water's bent structure is due to the two lone pairs of electrons on the oxygen, making the bond angle approximately 105°. In contrast, CHCl₃ has a tetrahedral structure with a bond angle closer to 109.5°, without the presence of lone pairs affecting the bond angle significantly.

Answer 2

See explanation below

Step-by-step explanation:

In both cases the central atoms, C in CHCl₃ and O in H₂O, are sp³ hybridized .

Since they are sp³ hybridized we predict an angle between the H-C-Cl and H-O-H of 109.5 º ( tetrahedral ), but two of the sp³ orbitals in water are occupied by lone pairs.

These lone pairs do excercise more repulsion ( need more room ) than the bonds oxygen is making with hydrogen.

As a consequence of this repulsion the angles H-O-H are less than the predicted 109.5º in tetrahedra. ( Actually is 104.5 º)