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chem quiz
| Question | Answer |
|---|---|
| What does it mean for a chemical equation to be balanced? | Same number of each type of atom on both sides of the equation. |
| Law of Conservation of Matter | Matter cannot be created or destroyed in a chemical reaction. |
| What is a skeleton equation? | An unbalanced chemical equation. |
| What can you change to balance an equation? | Coefficients ONLY (never subscripts). |
| (aq) | Aqueous (dissolved in water) |
| What does “+” mean in a chemical equation? | Reacts with |
| What does “→” mean? | Produces / yields |
| The 7 diatomic elements | H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂ |
| When do elements exist as diatomic molecules? | When they are one of the 7 diatomic elements. |
| Synthesis reaction definition | Two or more substances combine to form one compound. A + B → AB |
| N₂ + 3H₂ → 2NH₃ | Example of synthesis |
| Decomposition reaction definition | One compound breaks into simpler substances. AB → A + B |
| 2H₂O₂ → O₂ + 2H₂O | Example of decomposition |
| Single replacement definition | One element replaces another in a compound. AB + C → AC + B |
| 2HCl + Mg → H₂ + MgCl₂ | Example of single replacement |
| What table is used to see if single replacement occurs? | Activity Series (Table J) |
| Double replacement definition | Two compounds exchange ions AB + CD → AC + BD |
| What usually forms in double replacement reactions? | A precipitate, water, or gas. |
| Pb(NO₃)₂ + 2HCl → 2HNO₃ + PbCl₂ | Example of double replacement |
| Combustion of a hydrocarbon always produces… | CO₂ and H₂O |
| CH₄ + 2O₂ → CO₂ + 2H₂O | Example of hydrocarbon combustion |
| Simple combustion definition | A metal reacts with oxygen to form a metal oxide. Metal + O₂ → Metal Oxide |
| 4Fe + 3O₂ → 2Fe₂O₃ | Example of simple combustion |
| when does no reaction occur | when everything is AQ |
| what is a net ionic and a complete ioninc | a net ionic is the two things that combine to form the new thing like solid a complete ionic is eveyhting broken down but the solids |
| Conversion from grams to moles | Divide the mass of a sample by its molar mass to obtain the number of moles |
| Excess reactant determination | After identifying the limiting reagent, subtract the amount used from the initial quantity of the other reactant to find what remains |
| Percent yield | A metric of experimental efficiency calculated as Actual yield / Theoretical yield X 100 |
| Actual yield | The measured amount of product obtained from an experiment |
| Yield discrepancy causes | Differences between theoretical and actual product amounts arise from incomplete reactions, side reactions, or experimental loss |
| Molar volume (gas at STP) | The volume occupied by one mole of an ideal gas at standard temperature and pressure, equal to 22.4L |
| Stoichiometric ratio | The proportion of moles of reactants and products as indicated by the coefficients in a balanced equation |
| Conversion from liters of gas to moles at STP | Divide the measured volume by 22.4 L/mol to calculate the amount in moles |
| Avogadro's number | The number of particles contained in one mole, 6.022 ×10^23 |
| Theoretical yield | The maximum possible amount of product calculated from the limiting reagent and stoichiometric ratios |
| Precipitate | The solid material that separates out of a solution because it is insoluble in water |
| Limiting reagent | The reactant that is completely consumed first, determining the maximum amount of product formed |
| Molarity | The concentration of a solution expressed as moles of solute per liter of solution, denoted as mol/L |
| Excess reagent | The reactant that remains after the limiting reagent has been used up |
| Supernatant | The clear liquid remaining above the solid after a precipitate has formed |
| insoluble soluble | insoluble means solid soluble means (AQ) |
| when do you use table F | When you need to make a double reaction you ned to see which one one is insoluble(solid) and soluble |
| 1. What type of reaction is a precipitation reaction? A) Single replacement B) Combustion C) Double replacement D) Synthesis | Answer: C — precipitation reactions are a subclass of double replacement |
| 2. What is a precipitate? A) A gas that forms B) A liquid product C) A solid that forms from two solutions D) Any aqueous compound | ✅ Answer: C |
| 3. A precipitate is always: A) Soluble B) Aqueous C) Insoluble D) A gas | ✅ Answer: C |
| 6. What is the supernatant? A) The solid that forms B) The gas released C) The solution left over after a precipitate forms D) The reactant that runs out | ✅ Answer: C |
| 8. Which ions are spectator ions in the reaction above? Pb(NO₃)₂(aq) + 2 KCl(aq) → PbCl₂(s) + 2 KNO₃(aq) A) KNO₃ A) Pb²⁺ and Cl⁻ B) K⁺ and NO₃⁻ C) Pb²⁺ and NO₃⁻ D) K⁺ and Cl⁻ | ✅ Answer: B |
| What does conservation of mass mean in a chemical equation? | The number of each type of atom must be the same on both sides of the equation. |
| What do coefficients in a balanced chemical equation represent? | Mole ratios between substances. |
| Do coefficients represent mass or electrons? | ❌ No — only moles, not grams or electrons. |
| What makes a reaction a chemical change? | A new substance is formed. |
| Why is 2H₂O → 2H₂ + O₂ a chemical change? | Because water turns into different substances. |
| Is H₂O(l) → H₂O(g) chemical or physical? | Physical — same substance, different state. |
| What does “conserved” mean in chemistry? | Not created or destroyed. |
| What is ALWAYS conserved in chemical reactions? | Mass, charge, and energy |
Created by:
Fernando.Quezada