Mole - Calculating moles PDF

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Calculating moles...

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The Biochemical Foundation of Life. Introduction: In this topic you will be learning about: 

Structure of the atom: protons, neutrons, electrons; electrons and orbitals; metals and nonmetals, ions, radicals.

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Structure of molecules; from small organics to large biomolecules, identification and naming of common functional groups.

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Atomic and molecular measurements; molecular mass, moles, concentration

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3D molecular shape and isomerism: optical and geometrical isomerism, configuration and conformations.

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Bonding within molecules (covalent) and between molecules (ionic, hydrogen, Van der Waals).

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Distribution of electrons within molecules; electronegativity; inductive and resonance effects.

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Movement of electrons between molecules; making and breaking of bonds; equilibrium, substitution, elimination, reduction and oxidation reactions.

Unit: Moles, concentrations & dilutions -

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Mole (ml) is an amount of stuff The mole is a convenient way of scaling down large numbers: one mole of atoms represents 6 × 1023 atoms–that is 600 000 000 000 000 000 000 000 atoms. We call the value 6 × 10 23 the Avogadro constant. One mole of any element contains the same number of atoms: 1 mol of Na contains 6 × 10 23 atoms of sodium; 1 mol of N contains 6 × 1023 atoms of nitrogen. A mole is a way of referring to numbers of any type of particle (atom, ion, or molecule) not just numbers of atoms. So, there are as many molecules in one mole of H2O as there are atoms in one mole of elemental hydrogen: 1 mol of H2O = 6 × 1023 molecules, 1 mol of H = 6 × 1023 atoms While one mole of two different elements contains the same number of atoms, each has a different mass. Carbon has an atomic mass of 12 amu, while hydrogen has an atomic mass of 1 amu, therefore an atom of 12C is twelve times heavier than an atom of hydrogen. Because one atom of carbon has a mass that is twelve times heavier than one atom of hydrogen, we can deduce that one mole of carbon (6 × 1023 atoms) has a mass that is twelve times heavier than one mole of hydrogen (also 6 × 1023 atoms). We call the mass of one mole of a substance (atom, ion, or molecule) its molar mass, with the unit g mol−1 (which can also be written g/mol) To calculate moles present in a sample of 24g of C: -

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