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Atoms Key Terms
Chapter 3 Key Terms
14
Chemistry
Not Applicable
03/16/2004

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Term
Law of conservation of mass
Definition
states that mass is neither destroyed nor created during ordinary chemical reactions or physical changes
Term
law of multiple proportions
Definition
If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers
Term
law of definite proportions
Definition
The fact that a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound
Term
atom
Definition
the smallest particle of an element that retains the chemical properties of that element
Term
nuclear forces
Definition
these short-range proton-neutron, proton-proton, and neutron-neutron forces hold the nuclear particles together
Term
atomic number
Definition
the number of protons and neutrons in the nucleus of each atom of that element
Term
isotopes
Definition
atoms of the same element that have different masses
Term
mass number
Definition
the total number of protons and neutrons in the nucleus of an isotope
Term
nuclide
Definition
a general term for any isotope of any element
Term
atomic mass unit
Definition
or 1 amu, is exactly 1/12 the mass of a carbon-12 atom
Term
average atomic mass
Definition
the weighted average of the atomic mases of the naturally occuring isotopes of an element
Term
mole
Definition
the amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12
Term
Avogadro's number
Definition
6.0221236 x 10^23--is the number of particles in exactly one mole of a pure substance
Term
molar mass
Definition
the mass of one mole of a pure substance
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