Why does Sodium Fluoride (NaF) have a higher melting point than Rubidium Fluoride (RbF)?
Answers
Answer:
Sodium fluoride is in the structure of an ionic lattice. It has a high melting point because the force of attraction between the two oppositely charged ions (Na+ and F-) is really strong, and requires a lot of heat energy to break them.
Answer:
Sodium fluoride has a high melting point due to hydrogen bonding in it's aqueous solution and in it's free state the fluoride ions being smaller are closely packed so NaF has a higher inter ionic attraction between Na+ and F-
Explanation:
Ionic radius decreases in the order I- > Br- > Cl- > F-. Individual Na-halide bonds become shorter and stronger in the same order. The effect is multiplied because in an octahedral environment each sodium is in contact with six halides, resulting in a much greater lattice energy for NaF compared with its congeners. Greater lattice energy means that more energy is required to melt the lattice.