Higher Tier: count bonds before calculating the energy change
導入済み| English | 意味 |
|---|---|
| overall energy change/ˌəʊvəˈrɔːl ˈenədʒi tʃeɪndʒ/ | 全エネルギー変化 |
| bond energy/bɒnd ˈenədʒi/ | 結合エネルギー |
What would explain this observation?
- Higher Tier: Breaking a bond needs energy. An exothermic reaction releases energy overall because formation of new bonds releases more than was needed to break the old ones.
- Start with a prediction. State the quantities or features you would compare, then decide what evidence could distinguish two explanations.
Build the model
- Energy must be supplied to break bonds in reactants. Energy is released when bonds form in products. Using supplied bond energies, overall energy change 总能量变化=total energy needed for bonds broken−total energy released for bonds formed. A negative answer means bond formation releases more than breaking requires, so the reaction is exothermic. A positive answer means the reverse and the reaction is endothermic.
- bond energy 键能: Energy required to break a mole of the stated bonds in the supplied model; overall energy change: Total bond-breaking energy minus total energy released by bond formation.
Breaking costs 700 kJ and forming releases 950 kJ. What is the signed overall change?
難易度 1/5 · 100 コイン + 今日初回完了時に小ボーナス付与
Overall change = energy taken in to break bonds minus energy released forming them = 700 - 950 = -250 kJ. The negative sign means a net release - exothermic.
Match each technical term to its precise meaning.
難易度 2/5 · 140 コイン + 今日初回完了時に小ボーナス付与
Use the definitions to distinguish related quantities and processes.
Choose evidence that can test it
- Use the balanced equation and actual bond types. A coefficient multiplies all bonds in that molecule. For H₂ + Cl₂ → 2HCl, break one H–H and one Cl–Cl and form two H–Cl bonds. For 2H₂ + O₂ → 2H₂O, break two H–H bonds and one O=O bond, and form four O–H bonds. An O=O double bond uses its supplied double-bond value once; do not double a single-bond value.
- Make separate broken and formed lists with counts, multiply each supplied value by its count, total each list, then subtract in the stated order. These values give an approximate model for the reaction quantities represented by the equation. Check units and sign and interpret the result in words. Do not infer this calculated value from a thermometer reading without a different model; AQA’s solution practical does not require that calculation.
Which two habits make the investigation or model in this case more defensible?
難易度 2/5 · 140 コイン + 今日初回完了時に小ボーナス付与
Stating the conditions and assumptions lets others repeat the work exactly, and recording the supporting evidence lets them check the conclusion. Hiding disagreeing results removes the evidence that could challenge a wrong conclusion, and one measurement can never establish a wider claim.
Work from known quantities
- State the known values and their units. Choose the relation because its assumptions fit this case, then rearrange before substitution.
- Known: supplied bond energies are H–H 436, Cl–Cl 243 and H–Cl 431 $\dfrac{\text{kJ}}{\text{mol of bonds}}$. For H₂ + Cl₂ → 2HCl, breaking requires 436+243=679 kJ; forming releases 2×431=862 kJ. Overall change=679−862=−183 kJ for the equation amounts: exothermic. The released magnitude is 183 kJ, but the signed change is negative. The balanced equation is essential to the count.
For H₂ + Cl₂ → 2HCl, use H–H 430, Cl–Cl 240, H–Cl 420 $\dfrac{\text{kJ}}{\text{mol of bonds}}$. Find the signed change for the equation amounts. Use the same sequence: known quantities → model → relation → substitution → unit and interpretation.
For H₂ + Cl₂ → 2HCl, use H–H 430, Cl–Cl 240, H–Cl 420 kJ per mole of bonds. Find the signed change for the equation amounts.
難易度 2/5 · 140 コイン + 今日初回完了時に小ボーナス付与
The result is -170 kJ. Known: H-H 430, Cl-Cl 240, H-Cl 420 kJ per mole of bonds; H2 + Cl2 -> 2HCl. Breaking: 430 + 240 = 670 kJ. Forming: 2 x 420 = 840 kJ. Change = 670 - 840 = -170 kJ for the equation amounts - exothermic. The equation tells you TWO H-Cl bonds form.
Check the conclusion and its limits
- Do not call breaking bonds exothermic, subtract formed from broken in the reverse order, or count atoms as if each were a bond. A negative energy change is not negative activation energy. This entire source section is Higher-only, while drawing the profiles remains common-tier content.
- Return to the original observation. Explain what the result supports, which conditions it assumes, and one way to test a competing explanation.
Breaking a chemical bond releases energy. This claim is false: Breaking bonds always REQUIRES energy to separate the atoms; energy is released when bonds FORM. Reversing this flips the sign of every energy calculation.
Higher Tier: count bonds before calculating the energy change: Use the balanced equation and actual bond types. A coefficient multiplies all bonds in that molecule. For H₂ + Cl₂ → 2HCl, break one H–H and one Cl–Cl and form two H–Cl bonds. For 2H₂ + O₂ → 2H₂O, break two H–H bonds and one O=O bond, and form four O–H bonds. An O=O double bond uses its supplied double-bond value once; do not double a single-bond value.
Breaking a chemical bond releases energy.
難易度 1/5 · 100 コイン + 今日初回完了時に小ボーナス付与
Breaking bonds always REQUIRES energy to separate the atoms; energy is released when bonds FORM. Reversing this flips the sign of every energy calculation.
Energy required to break a mole of the stated bonds in the supplied model: write the technical term.
難易度 1/5 · 100 コイン + 今日初回完了時に小ボーナス付与
bond energy means Energy required to break a mole of the stated bonds in the supplied model.