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Chapter 7
Chemical Reactions
| Question/Term | Answer/Definition |
|---|---|
| Solution | Homogeneous mixture of 2 or more substances. |
| What are 3 examples of a solution? | Ocean, Blood Plasma, Air, Soda, Steel, Lemonade, |
| Solute | The substance that gets dissolved. Minority component. Ex. sugar, salt, zinc, copper, cocoa, flour, cinnamon, oxygen |
| Solvent | Substance that dissolves other materials. Majority component. Ex. water, ethanol. acetone, methanol, |
| Universal Solvent | Water |
| What are 3 types of solutions? | Gaseous, Liquid, Solid |
| What are the most common Solutions? | Aqueous - solid, liquid, or gas AND water Aqua means water. |
| Solvated | when a solute has been surrounded and dispersed by solvent molecules. Ex. salt dissolved in water |
| What is the difference between dissolving ionic compounds vs. molecular compounds in water? Ex. Salt vs Sugar | Dissociation vs. Separation. Ionic compounds dissociate into separate, charged ions that move freely and can conduct electricity. Molecular compounds remain intact as individual molecules separated but not breaking apart into ions, do not conduct. |
| Electrolyte Solutions | Liquid that conducts electricity because it contains dissolved ions (ionic compounds dissolved in water) Ex Salt water |
| Nonelectrolyte Solutions | Liquid that does not conduct electricity because it contains neutral molecules. (Molecular Compounds dissolved in water) |
| What is an exception of a molecular substance that can ionize in water and conduct electricity? | Acids |
| Soluble | Substances that will dissolve in water |
| Insoluble | Substances that will not dissolve in water |
| Solubility | The amount of a compound that dissolves in liquid |
| Saturated solution | Solution that holds the maximum amount of solute under the solution conditions |
| Unsaturated solution | Solution with less than the maximum amount of solute under the solution conditions |
| Why does increasing temperature increase solubility for solids? | The added heat provides energy to overcome the solute's intermolecular forces and helps solvent molecules mix. |
| Why does increasing temperature decrease solubility for gases? | The added kinetic energy allows gas molecules to escape the solvent. |
| polyatomic ions | Group of 2 or more atoms that share electrons (covalent bond) but act as a single unit and carries an overall positive or negative charge. |
| Will a polyatomic ion dissociate in water? | No, it will stay intact due to the covalent bond. If it is part of an ionic compound the overall compound separates but the polyatomic ion remains. Ionic bonds break but covalent bonds don't. |
| Co(C2H3O2)2 | Soluable |
| ZnS | Insoluble |
| PbCO3 | insoluble |
| (NH4)2S | Soluble |
| k3PO4 | Soluble |
| AgI | Insoluble |
| Ni(NO3)2 | Soluble |
| AgBr | Insoluble |
| CaCl2 | Soluble |
| Pb(NO3)2 | Soluble |
| PbSO4 | Insoluble |
| CuS | Insoluble |
| FeSO4 | Soluble |
| NH4Cl | Soluble |
| Dilute solution | Contains small amount of solute |
| Concentrated solution | Contains large amounts of solute |
| Moles | The unit of measure for the amount of solute dissolved in a solution. |
| Molarity | Number of moles of solute per liter of solution. M= moles solute/liters solution |
| Formula for Grams (g) to Moles (m) | g / mm = m grams / molar mass = moles |
| Molarity Formula | M = m / L Molarity = moles / Liters of solution |
| Chemical reactions | Process where one or more substances (reactants) are transformed into different substances (products). Chemical bonds are broken and new bonds are formed. |
| Signs of Chemical reactions | Energy change (change in temperature), change in color, production of gas, formation of a solid, or emission of light. |
| Chemical equations | Representation of chemical reactions. Reactants are on the left and products are on the right. |
| Chemical equations must obey what? | Law of conservation of Mass. matter is neither created or destroyed. The total number of the reactants must equal the total number of the products. |
| What do you use to balance a chemical equation with? | Coefficients. A number added to the front, changing how many molecules there are but not what kind of molecules there are. |
| How do you determine the number of a particular type of atom within a chemical formula in an equation? | Multiply the subscript for the atom by the coefficient for the formula. |
| NEVER change a subscript to balance an equation, only the coefficient! Why? | Changing the subscript changes the number of the individual atom therefore changing the type of molecule altogether! |
| What do the abbreviations (g), (l), (s), and (aq) in chemical reactions stand for? | gas, liquid, solid, and aqueous |
| precipitation reaction | reactions that result in the formation of an insoluble product. |
| precipitate | insoluble solid formed by a reaction that occurs in solution. |
| When do precipitation reactions occur? | When pairs of oppositely charged ions attract each other so strongly that they form an insoluble ionic solid. |
| Only what kind of compounds form precipitates? | Insoluble |
| Molecular equations | equation showing the complete neutral formulas for every compound in the reaction |
| Complete ionic equation | Shows the reactants and products as they are actually present in solution. |
| spectator ions | Ions in a complete ionic equation that appear unchanged on both sides of the equation. |
| How can you simplify an equation to more clearly show what is going on? | Remove the spectator ions. |
| Net ionic equation | equations that show only the species that actually participate in the reaction. What is left after the spectator ions have been removed. |
| Reactions that form water when mixing an acid and a base | Acid-Base reactions |
| reactions that involve gas | Gas-Evolution reactions |
| Molecular compounds that produce H+ ions when dissolved in water | Acids |
| Properties of acids | can dissolve various metals. Typically have a sour taste. food ex. lemons, limes, vinegar |
| Ionic compounds that produce OH-ions when dissolved in water. | Bases |
| Properties of bases | bitter taste and slippery feel |
| What 2 things are usually produced from an acid-base reaction? | Water and salt |
| 4 types of gas-evolution reactions | Sulfide-acid, carbonate-acid, sulfate-acid, ammonium-base |
| What is it called when a substance gains oxygen? | Oxidation |
| a substance that has gained oxygen has been what? | Oxidized |
| When a substance losses oxygen it is what? | Reduced |
| reduction | loss of qxygen |
| Substance that is oxidized | reducing agent |
| Substance that is reduced | Oxidizing agent |
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