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Definition
| A measuring unit representing 6.02x10^23 representative particles of a substance |
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| Spcies present in a substance (atoms, molecules, formula units) |
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| What is the representative particle for diatomic elements? |
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Definition
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| What is the representative particle for molecular compounds? |
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Definition
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| What is the representative particle for ionic compounds? |
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Definition
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| Atomic mass of an element expressed in grams |
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| Gram Molecular Mass (gmm) |
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Definition
| Mass of 1 mole of that compound |
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| Mass of one mole of an ionic compound |
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| Mass (in grams) of one mole of the substance |
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| What is Standard Temperature and Pressure (STP)? |
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Definition
The default temperature and pressure levels for measuring gas.
Standard Temperature = 0°C
Standard Pressure = 101.3 kPa, or 1 atmosphere (atm). |
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| At STP, how much volume does one mole of gas occupy? (in litres)? |
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Definition
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| The percent by mass of each element in a compound |
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Definition
Lowest whole-number ratio of the atoms of the elements in a compound
ex. CO |
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| Can the molecular formula be the same as the Empirical formula? |
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Definition
| Yes of course. The compound Carbon Monoxide, has a molecular formula of CO. It's empirical formula is also CO. |
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| How do you determine the Molecular formula? |
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Definition
Once you have the empirical formula, you need to find the empirical formula mass(efm).
This is smiply molar mass of the empirical formula. Divide original molar mass by this.
This gives empirical formula units in a molecule - it is the multiplier to converter empirical formula to the molecular formula. |
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