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).

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g

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