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Chapter 7 PS
This is a review over chapter 7 in the Physical Science 6th edition textbook.
| Question/Term | Answer/definition |
|---|---|
| Exploding fireworks are an example of what? | Chemical reactions |
| All of what depends on chemical reactions? | All of life |
| What are three things chemical reactions provide for us? | Heat in our homes; produce fibers for our clothes; Power our cars. |
| Define Chemical reaction: | A process that changes a substance into one or more different substances |
| What is broken and rearranged in a chemical reaction? | Chemical bonds |
| When a chemical change takes place through a chemical reaction, there are usually what? | clear signes |
| 8 Evidences of a chemical change: | 1. Precipitate 2. Bubbles 3. Energy released 4. Color Change 5. Odor 6. Temperature change 7. Composition change 8. Burning |
| Define precipitate: | When two liquids mix to form a solid |
| Define Chemical equation: | A combination of chemical formulas and symbols that make it a chemical reaction. |
| Define reactants: | Substances that enter into a chemical reaction |
| Define products: | Substances that combine to produce |
| Define yields: | The arrow in a chemical equation |
| Define coefficient | Numbers placed in front of a chemical formula within a chemical equation |
| We valance equations based on the: | Conservation of matter |
| 5 step process for balancing equasions: | 1.Write the word equation for the reaction 2.write the chemical equation for the reaction 3.Balance the chemical equation with coefficients 4.Check to see whether the addition of the coefficient balances the equation 5.Repeat steps if necessary |
| Define mole unit | A unit of measurement that describes 6.02 x 10^23 of particles, atoms, ions, or molecules |
| Balanced chemical equations can tell us how many individual atoms, ions, molecules and ______ take part in a reaction | moles |
| Define molar mass: | The mass of one mole |
| Define Synthesis reaction: | combination of two or more reactants into a single, more complex product: X+Y yields XY |
| Define decomposition reaction: | A reaction in which a single reactant breaks down into two or more products: XY yields X+Y |
| Define Double-replacement reaction: | A reaction in which two compounds swap cations or anions with each other: WX+YZ yields WZ+YX |
| Define Single-replacement reaction: | A reaction in which one element in a compound is replaced by another element: XY+Z yields ZY+X |
| Define Combustion reaction | A reaction in which a substance reacts with oxygen: CH+2O yields CO+2H2O |
| Define oxidation | Any instance in which electrons are lost |
| Define reduction | Gaining of electrons during a chemical reaction |
| Define Exothermic reaction: | Reactions that release energy as heat |
| Define endothermic reactions | reactions that absorbs more energy than it releases |
| Define activation energy | energy needed to get a chemical reaction started |
| Define law of conservation of energy: | During a chemical reaction no energy is created or destroyed, but only changed from one form to another. |
| Define collision model | we need three things to happen before reactants will react: first the reactant particles must collide with each other. Then, when they collide, they must be aligned properly in order to rearrange their bonds. Finally, there must be enough energy. |
| Factors that affect reaction rates: | Surface area: more reactants in contact Stirring: more reactants in contact; slightly more energy Temperature: More collisions; collisions have more energy Concentration: More collisions Catalysts: higher percentage of collisions have enough energy |
| Define enzymes | a special group of catalysts |
| define inhibitor | a catalyst that slows the rate of a reaction by reducing the effectiveness of catalysts. |
| Define reaction rate | the speed of a reaction |
| Define reversible reactions | Reactions that not only form products, but the products can also react together to re-form the original reactants. |
| Define chemical equilibrium | occurs when the forward and reverse reactions each happen at the same rate |
| Changes in chemical equalibrium: | Concentration; temperature, and pressure |
| Define Le chatelier's principle: | states that any chemical system in equilibrium will adjust its equilibrium state in such way as to reduce the effect of any changes made to the system. |
| Define equilibrium | A state in which multiple influences cancel each other out. |
| Define physical equilibrium | When the number of vapor and liquid molecules remains constant. |
| Concentration | Adding any of these substances will shift the equilibrium state toward the other side of the reaction. Removing any substance will shift the equilibrium state toward the side of the reaction from which we removed the substance. |
| Temperature | Increasing the temperature will shift the reaction toward the side of the equation that absorbs energy. Lowering the temperature will shift the system toward the side that releases energy; it will cause more ammonia to be produced. |
| Pressure | The pressure inside a closed container is related to the number of particles it contains; the greater the number of particles the greater the pressure. If the pressure is increased a response that results in fewer gas particles needed. |
| Applying magnetic field | Does not effect reaction rates. |
| Reactants: | are found at the beginning part of the graph |
| Activation energy: | is found as the rising point of the hill |
| Energy in or energy out: | is found in between the reactants and products |
| Products: | Found at the end of the chart |
| Reaction rate: | Is found as the overall line on the chart; from the reactants at the beginning, to the products of the reactions at the end of the graph. |
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hihello2007
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