How do the properties of metals differ from those of both ionic and molecular compounds?

Answer and Explanation:

Metals are lustrous (shiny), malleable (that means that can be hammered) and ductile. They are usually solid at room temperature (except mercury which is liquid). They are good conductors of heat and electricity. They are made of metallic bonds. Examples:   iron (Fe), silver (Ag).

Ionic compounds are hard and usually brittle. They form crystals (solid at room temperature) and they have high melting points. They only conduct electricity when are dissolved in water. They are made of ionic bonds Examples: sodium chloride (NaCl), magnesium oxide (MgO).

Molecular compounds are gases, liquids or low-melting solids. They are poor conductors of heat and electricity. They have low melting and boiling points. They are made of covalent bonds. For example: methane (CH₄) and ozone (O₃).

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.