1.
atomic mass unit: amu, exactly 1/12 the mass of a carbon-12 atom, or 1.660 540 x 10^ -23
2.
atomic number: (Z) of an element is the number of protons in the nucleus of each atom of that element
3.
atoms to grams: multiply 1/Avogadros' # by the molar mass of the element=________
4.
atoms to moles: multiply __________ by 1/Avogadro's # = _______________
5.
average attomic mass: the weighted average of the stomic masses of the naturally occuring isotopes of an element
6.
Avogadro's number: 6.022 1367 x 10^23-is the number of particles in exactly one mole of a pure substance, 6.022 x 10^23
7.
grams to atoms: multiply ______________by 1/molar mass of element by Avogadro's # = _________
8.
grams to moles: multiply _______________by 1/molar mass of element
9.
hyphen notation: name of the element-mass number
10.
isotopes: atoms of the same element that have different masses
11.
mass number: total number of protons and neutron in the nucleus of an isotope
12.
molar mass: the mass of one mole of a pure substance
13.
mole: (mol) the amount of a substance that contains Avogadro's number of particles
14.
mole: the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12
15.
moles to atoms: multiply __________ by Avogadro's # =_________
16.
moles to grams: multiply __________by molar mass of element=________
17.
nuclide: general term for any isotope of any element