Term
| What is the prefix for 7? |
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Definition
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Term
| What is the prefix for 9? |
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Definition
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Term
| What suffix is always used in covalent nomenclature? |
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Definition
The prefix of -ide is always used in covalent nomenclature. |
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Term
| What is Avogadro's Number and what is significant about it? |
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Definition
Avogadro's Number is 6.022 x 1023. This number is special because it is the number of atoms or molecules in a mole of an element or compound (respectively). |
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Term
| What is the exact definition of a mole? |
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Definition
A mole is the amount of that contains exactly the number of atoms contained 12g of Carbon-12. |
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Term
| What is the technical definition of "atomic mass"? |
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Definition
Atomic mass equals the mass of 1 mole of an element or compound. Specific decimal places are due to the presense of mutliple isotopes within atoms. |
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Term
| What is the first step in balancing chemical equations? |
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Definition
Write the reaction with blank spaces before ther formulas. |
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Term
| What is the second step of balancing equations? |
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Definition
Check if the equation if already balanced. |
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Term
| What is the third step of balancing equations? |
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Definition
Create a graph. Left = reactants, right = products. |
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Term
| What is the fourth step of balancing chemical reactions? |
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Definition
| Inspect for discrepencies in the graph. |
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Term
| What trick should be used when balancing chemical equations? |
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Definition
| Start with the element in lowest abundance (typcially a metal) and leave hydrogen for second to last and always balance oxygen last. |
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Term
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Definition
A molecular formula is something that displays the actual mole-to-mole ratio between elements in a single structural unit. |
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Term
| Define empirichal formula (aka simplest formula) |
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Definition
The empirichal formula displays the smallest whole-number ratio between elements in a formula (compound). Divide through by the greatest common factor. |
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Term
| How do you determine the molecular and/or empirichal formula from mass % data? |
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Definition
| 1. Assume there is 100g (unless some other mass is given). 2. Replace % with grams. 3. Convert grams to moles. 4. Divide each mole value by the smallest from step 3. 5. Insert mole as a subscript. 6. If molecular formula is desired divide the mass of the empirichal formula into the given molar mass. 7. Multiply quotient of step 6 by the subscripts in the empirichal formula. |
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