Question

which molecule is likely to be polar based on its lewis dot structure?
a. ch4
b. n2
c. h2o
d. co2

Explanation:

Step1: Analyze CH₄

CH₄ has a tetrahedral shape with symmetric charge - distribution around the central carbon atom. The bond dipoles cancel out, making it non - polar.

Step2: Analyze N₂

N₂ is a diatomic molecule with a triple bond between two nitrogen atoms. The two atoms have the same electronegativity, so there is no electronegativity difference and the molecule is non - polar.

Step3: Analyze H₂O

H₂O has a bent shape. Oxygen is more electronegative than hydrogen. The bond dipoles do not cancel out due to the bent geometry, resulting in a net dipole moment and making the molecule polar.

Step4: Analyze CO₂

CO₂ has a linear shape. The bond dipoles are symmetrically arranged and cancel each other out, making the molecule non - polar.

Answer:

C. H₂O