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25 Cards in this Set
- Front
- Back
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Law of Conservation of Mass |
In a chemical reaction, matter is neither created nor destroyed. |
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Law of Definite Proportions |
All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. |
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Law of Multiple Proportions |
When two elements (call them A and B) form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers. |
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Charge on an Electron |
-1.60*10^-19 |
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Atomic Number |
Number of protons in an atom's nucleus. |
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Chemical Symbol |
One or two letter abbreviation for an element. |
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Natural Abundance |
The relative amount of each different isotope in a naturally occurring sample of a given element (usually constant). |
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Mass Number |
Sum of the number of neutrons and protons in an atom. |
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Alkali Metals |
Group 1A, all reactive metals. |
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Alkaline Earth Metals |
Group 2A, fairly reactive, although not as reactive as the alkali metals. |
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Halogens |
Group 7A, highly reactive non-metals. |
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Atomic Mass |
Average mass for an element. |
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Mass Spectrometry |
Way to measure the masses of atoms and percent abundances of isotopes. |
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Mole |
6.022*10^23 particles; the value of the mole is equal to the number of atoms in exactly 12 grams of pure carbon |
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Nitrate |
NO3 - |
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Sulfate |
SO4 2- |
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Carbonate |
CO3 2- |
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Bicarbonate |
HCO3 - |
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Phosphate |
PO4 -3 |
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Ammonium |
NH4 + |
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Hydroxide |
OH - |
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Acetate |
C2H3O2 - |
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Hydrocarbon |
Organic compounds that only contain C and H. |
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Functional Group |
Organic compound containing C, H, and other atoms |
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Naming of Ions |
Cation name + anion name + ide |
