Question

question 6 of 10
not yet answered
points possible: 0.50
determine whether each of the molecules below is polar or nonpolar.
tetrahedral ccl4 choose...
linear cs2 choose...
trigonal pyramidal nh3 choose...

Explanation:

Step1: Analyze CCl₄

In CCl₄, the central carbon atom is bonded to four chlorine atoms in a tetrahedral geometry. The electronegativity difference between C and Cl creates bond - dipoles, but due to the symmetrical tetrahedral shape, these bond - dipoles cancel out. So, CCl₄ is non - polar.

Step2: Analyze CS₂

In CS₂, the central carbon atom is double - bonded to two sulfur atoms in a linear geometry. The electronegativity difference between C and S creates bond - dipoles, but the linear shape makes these bond - dipoles cancel each other. So, CS₂ is non - polar.

Step3: Analyze NH₃

In NH₃, the central nitrogen atom has a lone pair of electrons and is bonded to three hydrogen atoms in a trigonal pyramidal geometry. The N - H bonds are polar due to the electronegativity difference between N and H, and the presence of the lone pair distorts the symmetry, causing the bond - dipoles not to cancel. So, NH₃ is polar.

Answer:

Tetrahedral CCl₄: Non - polar
Linear CS₂: Non - polar
Trigonal pyramidal NH₃: Polar