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Unit 6
The Mole
Term | Definition |
---|---|
Avogadro´s number | 6.022 141 79 x 10^23 - is the number of particles in exactly one mole of a pure substance |
molar mass | The mass of one mole of a pure substance is called the molar mass of that substance. |
mole | A mole (abbreviated mol) is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon - 12. |
molecule | A molecule is a neutral group of atoms that are held together by covalent bonds |
Scientific notation | In science notation, numbers are written in the form M x 10^n, where the factor M is a number greater than or equal to 1 but less than 10, and n is a whole number. |
formula unit | A formula unit is the simplest collection of atoms from which an ionic compound ´s formula can be written. |
molecular mass | The molar mass of a compound is calculated by adding the masses of the elements present in a mole of the molecules or formula units that make up the compound. |
atomic mass | Average atomic mass is the weighted average of the atomic masses of the naturally occuring isotopes of an element. |
molecular formula | A molecular formula shows the types and numbers of atoms combined in a single formula of a molecular compound. |
density | Density is the ratio of mass to volume, or mass divided by volume. |
Formula mass | Formula mass of any molecule, formula unit , or ion is the sum of the average atomic masses of all atoms represented in it´s formula. |
Percent composition | The percentage by mass of each element in a compound is known as the percentage composition of the compound. |
Empirical formula | An empirical formula consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole-number mole ratio of the different atoms in the compound. |