Math Snap

STEP 1

1. The molecule in question is $\text{SI}_2$, which consists of two iodine atoms bonded to a central sulfur atom.
2. Electronegativity values are known: Sulfur (S) has an electronegativity of 2.5, and Iodine (I) has an electronegativity of 2.5.
3. The bond type is determined based on the electronegativity difference.
4. The molecular shape is determined by the VSEPR theory.
5. Symmetry and polarity are determined by the molecular shape and electronegativity differences.
6. The dominant intermolecular force is determined by the molecular polarity and the presence of hydrogen atoms.

STEP 2

1. Calculate the electronegativity difference.
2. Determine the bond type.
3. Determine the molecular shape.
4. Determine the symmetry of the shape.
5. Determine the polarity of the molecule.
6. Determine the dominant intermolecular force.

STEP 3

Calculate the electronegativity difference between sulfur and iodine:
$$\text{Electronegativity difference} = |2.5 - 2.5| = 0.0$$

STEP 4

Since the electronegativity difference is 0.0, the bond is classified as:
Covalent

STEP 5

Determine the molecular shape using VSEPR theory. $\text{SI}_2$ has a central sulfur atom with two iodine atoms and no lone pairs, resulting in a:
Linear shape

STEP 6

The linear shape is:
Symmetrical

STEP 7

Since the molecule is symmetrical and the electronegativity difference is zero, the molecule is:
Nonpolar

For nonpolar molecules, the dominant intermolecular force is:
London dispersion
The answers to the questions are:
1. 0.0
2. Covalent
3. Linear
4. Symmetrical
5. Nonpolar
6. London dispersion