1. Most ionic compounds have a crystal structure. You must break the chemical bond and tear away the crystal structure. Basically it takes less energy to break the covalent bonds than an ionic bond.
2. Dissolve the compound in water and test the conductivity. Strong electrolytes have high conductivity, weak electrolytes have medium to low conductivity and non-electrolytes have no conductivity. This is not a good test for those ionic compounds that are not soluble in water. For those one can melt the crystal and test the conductivity of the molten solution.
3.
a. atom
b. ion
c. molecule
4.a.) strontium--atoms
B.) CaCl2--ions
C.) CCl4--molecule
D.) SO2--molecule
E.) helium--atom
F.) bromine--moleulce
G.) MgO--ions
You supply the reasoning.
1. Explain why the melting points of ionic compounds and molecular compounds differ?
2. A.) What laboratory procedure allows you to test a compound is ionic or molecular?
b.) what results would you expect?
3. A.) What do we call the smallest particle of an element?
b.) what do we call the smallest particle in a compound with ionic bonds?
C.) what do we call the smallest particle of a covalently bonded compound?
For each of the following what type of smallest particle would exist? explain your reasoning?
a.) strontium
B.) CaCl2
C.) CCl4
D.) SO2
E.) helium
F.) bromine
G.) MgO
Please help me on these thanks:)
2 answers
You are a lifesaver thank u soooooo much:)!!!!
2 answers