Term
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Definition
| The total mass remains constant during a chemical change |
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Term
| A chemical reaction that illustrates the Law of Conservation |
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Definition
| 2.53 grams of Mercury + 0.20 grams of Oxygen = 2.73 grams of red-orange residue |
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Term
| Describe the differences between the states of matter |
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Definition
Solid- rigidity, they maintain their shapes when subjected to outside forces
Liquids- relatively incompressible fluid, fixed volume but no shape
Gas- easily compressible fluid, any quantity will fit in a container of any size or shape |
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Term
| Example of each state if matter |
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Definition
Solid- ice
Liquid- water
Gas- steam |
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Term
| Definition of a physical property |
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Definition
| A characteristic that can be observed for a material without changing its chemical identity |
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Term
| Three examples of a physical property |
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Definition
| Physical state, melting point, color |
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Term
| Definition if a chemical property |
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Definition
| A characteristic of a material involving its chemical change |
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Term
| Three examples of a chemical property |
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Definition
| Heat combustion, reactivity, Ph factor |
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Term
| Definition of a physical change |
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Definition
| A change in the form if matter but not in its chemical identity |
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Term
| Two examples of a physical change |
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Definition
| Dissolving one material into another, crumpling a piece if paper, breaking a bottle |
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Term
| Definition of a chemical change |
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Definition
| A change in which one more kinds if matter are transformed into new matter or several new kinds of matter |
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Term
| Two examples of a chemical change |
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Definition
| Rusting of iron, burning paper |
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Term
| What is the difference between Pure and Impure substances? |
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Definition
Pure substances- uniform composition, only one kind of particle
Impure substance- have particles of other substances mixed in that can be separated by physical means |
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Term
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Definition
| A substance that cannot be decomposed by any chemical reaction into a simpler substance |
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Term
| Three examples of elements |
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Definition
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Term
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Definition
| A substance composed of two or more elements chemically combined. A pure compound always contains a definite or constant proportions of the elements by mass |
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Term
| Three examples of a compound |
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Definition
| Sodium chloride, water, salt |
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Term
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Definition
| A material that can be separated by physical means into two or more substances |
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Term
| What is the difference between heterogeneous and homogenous mixtures? |
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Definition
Heterogenous- a mixture that consists of physically distinct parts, each with different properties
Homogeneous- a mixture that is uniform in is properties throughout given samples |
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Term
| Define intensive properties? |
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Definition
| Does not depend on the amount of material present |
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Term
| Two examples of intensive properties |
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Definition
| Density and boiling point |
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Term
| Definition of an extensive property |
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Definition
| Directly proportional to the amount of material present |
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Term
| Two examples of the extensive property |
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Definition
| amount of heat it takes to melt the substance completely, the mass of the object |
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Term
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Definition
| a collective term for separating mixtures |
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Term
| Describe three different kinds of Chromatography |
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Definition
Paper Chromatography-place a spot of the mixture on the chromatography paper, then place the paper in the solvent, the mixture will separate as it travels up the paper
Gas- gases stick to the walls of the capillary tube differently, separating them
Liquid-The liquids stick to the walls of a tube a different heights separating them |
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Term
| Describe how paper chromatography can be applied to a lab station |
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Definition
| It can be applied when we have pigments to separate or other mixtures that are able to be visibly separated when made into a concentrated paste on the papaer |
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