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43 Cards in this Set
- Front
- Back
Accuracy |
Determined by how close a measurement is to a "True" or "Accepted" value. Accuracy is measured in terms of error. |
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Error |
The difference between the measures value of a quantity and the "True" or "accepted" value. Error is classified as either systematic or random. |
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Systematic Error |
Is attributable to definite cause such as an instrument, malfunction, miscalculation, or erroneous technique. |
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Random Error |
Characteristic of a particular device or instrument or an individual's technique. |
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Precision |
Is defined as the reproducibility of results or how many decimal places you can measure with a particular instrument |
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On a ruler, it is point to the 3 in centimeters. What is the marking? |
3.0 cm |
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On a thermometer, it is at the long 63. How would you write that? |
63.0°C |
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On a graduated cylinder, it is filled up to the line of 43. How would you write that? |
43.0 mL |
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What is the formula for Density ? |
Mass ÷ Volume |
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What are the units of density ? |
(g/mL) |
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What is the formula for percent error ? |
Experimental - Accepted ÷ Accepted ×100 |
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Law of Conservation of Mass |
States that the mass of any one element at the beginning of a reaction will equal the mass of the element at the end of the reaction. |
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Law of Definite Proportions |
States that a pure compound will always have the same elements combined in the same proportions by mass |
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Law of Constant Composition |
Applies regardless of how the substance is made, where it is found, or how many different reactions are followed to form the compound. |
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Empirical Formula |
Is the simplest whole number ratio of atoms of each element in the compound |
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Molecular Formula |
Represents the actual number of each type of atoms in a compound |
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Formula for calculating molecular formula |
Molecular molar mass ÷ empirical molar mass |
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Stoichiometry |
The numerical relationships between chemical amounts in a balanced chemical equation |
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Limiting Reactant |
Reactant that is completely consumed in a chemical reaction |
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Reactant in Excess |
Any reactant that occurs in greater quantity than is required to completely react with the limiting reactant |
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Theoretical Yield |
Macimum amount of product that can be produced in a chemical reaction based on the amount of limiting reactant available |
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Actual yield |
The amount of product that is actually produced or recovered experimentally in a lab |
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Percent yield |
The percentage of the theoretical yield thay is obtained experimentally in a lab |
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Precipitate |
The solid is formed as a result of a chemical reaction |
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Supernatant Liquid or Supernate |
the liquid solution that exists above the precipitate in the reaction mixture |
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Filtration |
the use of filter paper to separate an insoluable solid from a liquid in a reaction mixture |
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Residue |
The precipitate thay collects on the filter paper |
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Filtrate |
The liquid that passes through the filter paper and the funnel |
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Formula of % yield |
Mass of actual yield ÷ mass of theoretical yield × 100% |
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Molarity |
A measure of amount of solute in a solution |
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What is the formula for Molarity |
Mol of Solute ÷ L of solution |
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Combination Reaction |
Is a reaction in which two or more reactant are combined to form a single product. |
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What is the formula for a combination reaction ? |
A + B 》 AB |
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Decomposition Reaction |
When a single reactant is decomposed or broken down into two or more products |
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What is the formula for a decomposition reaction |
AB 》 A + B |
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Single Replacement Reaction |
A substitution or displacement reaction occurs when a single free element replaces or is substituted for one of the elements in a chemical compound |
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What is the formula for a single replacement reaction |
A + BC 》 AC + B |
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Double Replacement Reaction |
Is a reaction in which there is an "exchange in partners" |
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What is the formula for a double replacement reaction |
AB + CD 》 AD + CB |
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Molecular equation |
Is the chemical equation that shows the complete neutral formulas for every compound in a reaction 2NH4Cl(aq) + Ca(OH)2(aq) 》 2NH3(g) + 2H2O(l) + CaCl2(aq) |
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Complete ionic equation |
Is the chemical equation that shows all of the species as they are actually present in a solution 2NH4+ + 2Cl- + Ca+2 + 2OH- 》 2NH3 + 2H2O + Ca+2 + 2Cl- |
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Net ionic |
Is an equation thay shows only the species thay change during the reaction NH4+(aq) + OH-(aq) 》 NH3(g) + H2O(l) |
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Spectator ions |
Which do not participate in the reaction and remain unchanged on both sides of a chemical equation are included in the complete ionic equation but are excluded in the net ionic equation |