10.1 Chemical Measurement.

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Presentation transcript:

10.1 Chemical Measurement

How do we measure the mass of an atom? Atomic mass: the mass of an atom expressed relative to the mass assigned to carbon-12 Common atomic masses: (we will always use 2 places behind the decimal) Hydrogen: 1.01 amu Carbon: 12.01 amu Oxygen: 16.00 amu

How do we measure the mass of a molecule? Molecules are just several atoms chemically combined together, so… Formula mass: the sum of all atomic masses of all the atoms in a compound Ex: H20 2 H’s, so 2 x 1.01 = 2.02 1 O, so 1 x 16.00 = 16.00 Add them together, you get 18.02, so one molecule of water has a mass of 18.02 amu.

Find the mass of … An atom of bromine Diatomic bromine A molecule of carbonic acid (H2CO3) Answers: Atom of bromine = 79.90 amu Diatomic bromine = 159.80 amu Molecule of carbonic acid = 62.03 amu

But why do we need to measure the mass of atoms and molecules? Well, most of the time we don’t! But we do need to measure bigger amounts. We do this using the concept of a mole! Well, not one quite like this!

Mole: (Def): of any element, the number of atoms of that element equal to the number of atoms in exactly 12.0 grams of carbon-12. This ends up being 6.02 x 1023 atoms. This is the number of atoms in 1 mole of any element. It is called Avogadro’s number (named after an Italian chemist and physicist)

So, how do you find a mole of an atom? Exactly as you found the atomic mass! The only difference is that it is measured in grams. Remember that hydrogen had an atomic mass of 1.01 amu? Well, the mass of one mole of hydrogen is 1.01 grams! This is called the molar mass – the mass, in grams, of one mole of a substance ADDITION: units for molar mass = g/mol

Look at the comparison . . . Element Number of atoms in one mole Mass of one mole Copper 6.02 x 1023 63.55 g Mercury 200.59 g Sulfur 32.07 g Iron 55.85 g

What about molecules? Same thing! Earlier, we found the formula mass of water to be 18.02 amu. Well, one mole of water (which is 6.02 x 1023 molecules) has a mass of 18.02 g.

One last note on particles… Three words that may confuse you… An ATOM is the smallest part of an element. (ex: One mole of carbon has a mass of 12.01 g) A MOLECULE is the smallest part of a covalent or molecular compound. (Ex: one mole of water has a mass of 18.02 g) A FORMULA UNIT is the smallest part of an ionic substance. (Ex: one mole of sodium chloride has a mass of 58.44 g)

Looking at it another way… Smallest particle is… One mole has ___ particles One mole has a mass of … Carbon (C) Atom 6.02 x 1023 atoms 12.01 g Water (H20) Molecule 6.02 x 1023 molecules 18.02 g Sodium Chloride (NaCl) Formula unit 6.02 x 1023 formula units 58.44 g