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Unit 6: The Mole
Chemistry
Term | Definition |
---|---|
Avogadro's Number | The number of atoms, molecules, or particles in a mole. |
Molar Mass | The mass of one mole of a pure substance, the mass in grams of 1 mol of a substance, molar mass is usually written in "g/mol" |
Mole | A mole (abbreviated mol) is the amount of substance that has 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 | Numbers are written in the form M x 10(n) ; the factor M is a # greater than or equal to 1 but less than 10, & N is a whole #. |
Formula Unit | Simplest collection of atoms from which an ionic compound's formula can be written. |
Molecular Mass | The sum of atomic masses of all atoms in a molecule. |
Atomic Mass | It is a weighted value and average of the atomic masses of the naturally occurring isotopes of an element. |
Molecular Formula | A chemical formula that shows the number and kinds of atoms in a molecule but not the arrangement of the atoms. |
Density | Density is the ratio of mass to volume, or mass divided by volume. |
Formula Mass | The sum of the average atomic masses of a compound's elements. |
Percent Composition | Percentage composition is the number of grams in one mole of a compound. |
Empirical Formula | Consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole number ratio of the different atoms in a compound. Shows the whole-number ratio of elements in a compound. |