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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 |
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