Question

question 4 (1 point) listen draw the lewis structures and then identify which compound is non - polar. sf2 sf6 sf4 so2

Explanation:

Step1: Determine valence electrons

Sulfur (S) has 6 valence electrons, fluorine (F) has 7 valence electrons and oxygen (O) has 6 valence electrons.

Step2: Draw Lewis - structure of SF₂

S is the central atom. S forms single - bonds with two F atoms. S has 2 bonding pairs and 2 lone pairs. The molecule has a bent shape. The electronegativity difference between S and F makes the S - F bonds polar, and due to the bent shape, the bond dipoles do not cancel out, so SF₂ is polar.

Step3: Draw Lewis - structure of SF₆

S is the central atom. S forms 6 single - bonds with 6 F atoms. S has 6 bonding pairs and 0 lone pairs. The molecular geometry is octahedral. The bond dipoles in an octahedral geometry cancel out, so SF₆ is non - polar.

Step4: Draw Lewis - structure of SF₄

S is the central atom. S forms 4 single - bonds with 4 F atoms and has 1 lone pair. The molecular geometry is seesaw. The bond dipoles do not cancel out, so SF₄ is polar.

Step5: Draw Lewis - structure of SO₂

S is the central atom. S forms double - bonds with two O atoms and has 1 lone pair. The molecule has a bent shape. The S - O bonds are polar and due to the bent shape, the bond dipoles do not cancel out, so SO₂ is polar.

Answer:

B. SF₆