Questions and Answers
__ Sb + __ Cl₂ → __SbCl₃
synthesis
__ Mg + __O₂ → __MgO
synthesis
__ CaCl₂ → __ Ca + __ Cl₂
decomposition
__ NaClO₃ → __ NaCl + __ O₂
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__ Fe + __ HCl → __ FeCl₂ + __ H₂
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__ CuO + __ H₂ → __ Cu + __ H₂O
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Al + H₂SO₄ → Al₂(SO₄)₃ + H₂
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_ MgBr₂ + _ Cl₂ → _ MgCl₂ + _ Br₂
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__ SnO₂ + __ C → __ Sn + __ CO
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Pb(NO₃)₂ + H₂S → PbS + HNO₃
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__ HgO → __ Hg + __ O₂
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__ KClO₃ → __ KCl + __ O₂
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__ N₂ + __ H₂ → __ NH₃
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_ NaBr + _ Cl₂ → _ NaCl + _ Br₂
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Zn + AgNO₃ → Zn(NO₃)₂ + Ag
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__ Sn + __ Cl₂ → __ SnCl₄
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__ Ba(OH)₂ → ___ Ba + __ H₂O
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Mg(OH)₂ + HCl → MgCl₂ + H₂O
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Na₂CO₃ + HCl → NaCl + H₂CO₃
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__ NH₄NO₂ → __ N₂ + __ H₂O
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__ N₂ + __ O₂ → __ N₂O₅
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__ MgCO₃ → __ MgO + __ CO₂
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__ KBr + __ Cl₂ → __ KCl + __ Br₂
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_ Zn + _ CuSO₄ → _ Cu + _ ZnSO₄
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__ P + __ O₂ → __ P₄O₆
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SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + NH₄Br
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__ AgNO₃ + __ (NH₄)₂CrO₄ → __ Ag₂CrO₄ + __ NH₄NO₃
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_ K + _ H₂O → _ KOH + _ H₂
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Al + Pb(NO₃)₂ → Al(NO₃)₃ + Pb
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__ Fe + __ O₂ → __ Fe₃O₄
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__ Li + __ O₂ → __ Li₂O
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__ ZnCl₂ + __ KOH → __ Zn(OH)₂ + __ KCl
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__ Fe₃O₄ + __ H₂ → __ Fe + __ H₂O
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_ Pb(NO₃)₂ → _ Pb + _ NO₂ + _ O₂
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__ H₂O → __ H₂ + __ O₂
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__ Mg + __ N₂ → __ Mg₃N₂
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Study Notes
Synthesis Reactions
- Formation of compounds from simpler reactants.
- Examples include:
- ( \text{Sb} + \text{Cl}_2 \rightarrow \text{SbCl}_3 )
- ( \text{Mg} + \text{O}_2 \rightarrow \text{MgO} )
- ( \text{N}_2 + \text{H}_2 \rightarrow \text{NH}_3 )
- ( \text{Fe} + \text{O}_2 \rightarrow \text{Fe}_3\text{O}_4 )
- ( \text{Li} + \text{O}_2 \rightarrow \text{Li}_2\text{O} )
- ( \text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2 )
- ( \text{P} + \text{O}_2 \rightarrow \text{P}_4\text{O}_6 )
- ( \text{Sn} + \text{Cl}_2 \rightarrow \text{SnCl}_4 )
Decomposition Reactions
- Breakdown of compounds into simpler substances.
- Examples include:
- ( \text{CaCl}_2 \rightarrow \text{Ca} + \text{Cl}_2 )
- ( \text{HgO} \rightarrow \text{Hg} + \text{O}_2 )
- ( \text{KClO}_3 \rightarrow \text{KCl} + \text{O}_2 )
- ( \text{Ba(OH)}_2 \rightarrow \text{Ba} + \text{H}_2\text{O} )
- ( \text{MgCO}_3 \rightarrow \text{MgO} + \text{CO}_2 )
- ( \text{H}_2\text{O} \rightarrow \text{H}_2 + \text{O}_2 )
- ( \text{NH}_4\text{NO}_2 \rightarrow \text{N}_2 + \text{H}_2\text{O} )
Single Replacement Reactions
- One element replaces another in a compound.
- Examples include:
- ( \text{Fe} + \text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2 )
- ( \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} )
- ( \text{Al} + \text{H}_2\text{SO}_4 \rightarrow \text{Al}_2(\text{SO}_4)_3 + \text{H}_2 )
- ( \text{KBr} + \text{Cl}_2 \rightarrow \text{KCl} + \text{Br}_2 )
- ( \text{Zn} + \text{AgNO}_3 \rightarrow \text{Zn(NO}_3)_2 + \text{Ag} )
- ( \text{SnO}_2 + \text{C} \rightarrow \text{Sn} + \text{CO} )
- ( \text{Fe}_3\text{O}_4 + \text{H}_2 \rightarrow \text{Fe} + \text{H}_2\text{O} )
Double Replacement Reactions
- Exchange of ions between two compounds.
- Examples include:
- ( \text{Pb(NO}_3)_2 + \text{H}_2\text{S} \rightarrow \text{PbS} + \text{HNO}_3 )
- ( \text{Mg(OH)}_2 + \text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2\text{O} )
- ( \text{Na}_2\text{CO}_3 + \text{HCl} \rightarrow \text{NaCl} + \text{H}_2\text{CO}_3 )
- ( \text{SrBr}_2 + (NH_4)_2\text{CO}_3 \rightarrow \text{SrCO}_3 + \text{NH}_4\text{Br} )
- ( \text{AgNO}_3 + (NH_4)_2\text{CrO}_4 \rightarrow \text{Ag}_2\text{CrO}_4 + \text{NH}_4\text{NO}_3 )
- ( \text{ZnCl}_2 + \text{KOH} \rightarrow \text{Zn(OH)}_2 + \text{KCl} )
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Test your knowledge on chemical equations and their classifications with these flashcards. Each card presents a reaction and its type, helping you understand synthesis, decomposition, and replacement reactions.
