Answer:
Because of their spaceeeee isss different
They have small differences in electronegativity
i think thats right
Answer :
(A) Br₂ (s) : molecular solids
(B) AgCl (s) : ionic solids
(C) S (s) : atomic solids
(D) CH₄ (s) : molecular solids
Explanation :
Molecular solids : It is defined as the solids in which they are held together by covalent forces, dipole interactions as attractive forces etc.
Ionic solids : It is defined as the solids in which the atoms composed with oppositely charged ions.
Atomic solids : It is defined as the solids in which the molecules are held together by covalent forces and also includes pure substance.
(A) Br₂ (s)
It is molecular solids because they are held together by covalent forces.
(B) AgCl (s)
It is ionic solids because in this atoms composed with oppositely charged ions.
(C) S (s)
It is atomic solids because it is a pure substance.
(D) CH₄ (s)
It is molecular solids because they are held together by covalent forces.
Answer:- There are 
moles.
Solution:- It is a unit conversion problem where we are asked to convert mg of aspartame to moles. Aspartame is 
and it's molar mass is 294.31 grams per mole.
mg are converted to grams and then the grams are converted to moles as:
= moles of aspartame
So, there would be moles of aspartame in 1.00 mg of it.
C.Ions with greater charge are more soluble in water.
Explanation:
Compounds with small ions tend to be less soluble than those with large ions.
The solubility of a compound is the result of a competition. The ions in the compound attract each other, and the water molecules attract the ions.
If the water molecules have a greater attraction to the ions than ions have for each other, then the compound will be soluble in water.
Compounds with small ions are less soluble than compounds with large ions. Small ions are closer to each other, so they have strong attractive forces. It is more difficult for the water to break them apart, so they are less soluble.
