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Unit 6: The Mole
The Mole
Term | Definition |
---|---|
Avogadro's number | ( 6.022 141 79 X 10^23) : It is the number of particles in exactly one mole of a pure substances. |
Molar mass | The mass of one mole of a pure substance. |
Mole | ( Mol) It is the amount of a substance that contains as many there are atoms in exactly 12 g of carbon-12 |
Molecule | It is neutral group of atoms that are held together by covalent bonds. |
Scientific notation | They are numbers written in the form M x 10^n, where the factor M is the number greater than or equal to 1 but less that 10, and n is a whole number. |
Formula unit | It is the simplest collection of atoms from which an ionic compound's formula can be written. |
Molecular mass | It is calculated by adding the masses of the element present in a mole of the molecule or a formula unit that makes up the compound. |
Atomic mass | It is the weighted average of the atomic masses of the naturally occurring isotopes of an element. |
Molecular formula | It is the actual formula of a molecular compound. |
Density | The ratio of mass to volume or, the mass divided by volume |
Formula mass | It is the mass of any molecule, formula unit, or iron is the sum of the average atomic masses of all atoms represented in its formula |
Percent composition | The percentage by mass of each element in a compound |
Empirical formula | It consists of the symbols for the element combined in a a compound, with subscripts showing the smallest whole number mole ratio of the different atoms in the compound |