SF2 Molecular Geometry and Polarity

The video tutorial explains the polarity of the SF2 molecule. It begins by examining the Lewis structure, showing two fluorine atoms and lone pairs around sulfur. Using VSEPR theory, the video describes how electron pairs and fluorine atoms spread out, resulting in a bent molecular geometry. This asymmetry leads to SF2 being a polar molecule due to differences in electronegativity. The tutorial concludes by confirming SF2's polarity.

What is the first step in determining whether SF2 is polar or non-polar?

• Examining the molecular weight

• Looking at the Lewis structure

• Checking the boiling point

• Analyzing the color of the compound

According to VSEPR theory, what causes the molecular geometry of SF2 to be bent?

• The presence of hydrogen bonds

• The repulsion between lone pairs and bond pairs

• The symmetrical distribution of electrons

• The attraction between sulfur and fluorine

What is the shape of the SF2 molecule as described in the video?

• Tetrahedral

• Trigonal planar

• Linear

• Bent

What role do the lone pairs of electrons play in the geometry of SF2?

• They attract the fluorine atoms closer

• They cause the molecule to be linear

• They do not affect the geometry

• They push the fluorine atoms down, creating a bent shape

What is incorrect about the model shown in the video regarding fluorine?

• The number of fluorine atoms

• The position of fluorine atoms

• The color representation of fluorine

• The charge on fluorine atoms

Why is SF2 considered a polar molecule?

• Due to the presence of ionic bonds

• Because it has a symmetrical shape

• Due to the equal distribution of electrons

• Because of the differences in electronegativity and unequal sides

What is the significance of the unequal sides in the SF2 molecule?

• They have no effect on the molecule's properties

• They make the molecule non-polar

• They result in a symmetrical shape

• They contribute to the molecule's polarity