Types of Chemical Reactions Writing Chemical Reactions Chemical reactions, or chemical changes, happen when the atoms in one or more chemicals split up and join together in new ways. For example, hydrogen can react with oxygen : hydrogen + oxygen wate r Before the reaction the oxygen atoms go round in pairs, and the hydrogen atoms go round in pairs. When they react we get two new
molecules, of the compound water. Each of these molecules has three atoms, two hydrogen atoms joined to one oxygen atom. We can write this as H2O. Types of Reactions Many chemical reactions have defining characteristics which allow them to be
classified as to type. Types of Chemical Reactions The five types of chemical reactions in this unit are: Combination Decomposition Single Replacement Double Replacement Combustion The reaction of sugar with
concentrated sulphuric acid. Combination Reactions Two or more substances combine to form one substance. The general form is A + X AX Example:
Magnesium + oxygen magnesium oxide 2Mg + O2 2MgO Combination Reactions Combination reactions may also be called composition or synthesis reactions. Some types of combination reactions: Combination of elements
K + Cl2 One product will be formed Combination Reactions K + Cl 2 Write the ions: K+ Cl-
Balance the charges: KCl Balance the equation: 2K + Cl2 2KCl Combination Reactions Some types of combination reactions: Oxide + water Nonmetal oxide + water acid
SO2 + H2O H2SO3 Metal oxide + water base BaO + H2O Ba(OH)2 Combination Reactions Some types of combination reactions: Metal oxides + nonmetal oxides Na2O + CO2 Na2CO3 CaO + SO2 CaSO3 Decomposition Reactions
One substance reacts to form two or more substances. The general form is AX A + X Example: Water can be decomposed by electrolysis. 2H2O 2H2 + O2
Decomposition Reactions Types of Decomposition Reactions: Decomposition of carbonates When heated, some carbonates break down to form an oxide and carbon dioxide. CaCO3 CaO + CO2 H2CO3 H2O + CO2 Decomposition Reactions Types
of decomposition reactions: Some metal hydroxides decompose into oxides and water when heated. Ca(OH)2 CaO + H2O Note that this is the reverse of a similar combination reaction. Decomposition Reactions Types of decomposition reactions:
Metal chlorates decompose into chlorides and oxygen when heated. 2KClO3 2KCl + 3O2 Zn(ClO3)2 ZnCl2 + 3O2 Some of these reactions are used in explosives. Decomposition Reactions Some substances can easily decompose: Ammonium hydroxide is actually
ammonia gas dissolved in water. NH4OH NH3 + H2O Some acids decompose into water and an oxide. H2SO3 H2O + SO2 Decomposition Reactions Some decomposition reactions are difficult to predict. The decomposition of nitrogen
triiodide, NI3, is an example of an interesting decomposition reaction. Nitrogen triiodide Single Replacement Reactions A metal will replace a metal ion in a compound. The general form is A + BX AX + B
A nonmetal will replace a nonmetal ion in a compound. The general form is Y + BX BY + X Single Replacement Reactions Examples: Ni + AgNO3
Nickel replaces the metallic ion Ag+. The silver becomes free silver and the nickel becomes the nickel(II) ion. Ni + AgNO3 Ag + Ni(NO3)2 Balance the equation: Ni + 2AgNO3 2Ag + Ni(NO3) Single Replacement Reactions Not all single replacement reactions that can be written actually happen. The metal must be more active than the metal ion.
Aluminum is more active than iron in Al + Fe2O3 in the following reaction: Thermite Reaction Al + Fe2O3 Aluminum will replace iron(III) as was seen in the video. Iron(III) becomes Fe and aluminum metal becomes Al3+. 2Al + Fe O 2Fe + Al O 2 3
2 3 Single Replacement Reactions An active nonmetal can replace a less active nonmetal. The halogen (F2, Cl2, Br2, I2) reactions are good examples. F2 is the most active and I2 is the least. Cl2 +2 NaI 2 NaCl + I2 Double Replacement
Reactions Ions of two compounds exchange places with each other. The general form is AX + BY AY + BX Metathesis is an alternate name for double replacement reactions. Double Replacement
NaOH + CuSO4 The Na+ and Cu2+ switch places. Na+ combines with SO 2- to form Na SO 4 2 4. Cu2+ combines with OH- to form Cu(OH)2
NaOH + CuSO4 Na2SO4 + Cu(OH)2 2NaOH + CuSO4 Na2SO4 + Cu(OH)2 Double Replacement CuSO + Na2CO3 Cu2+ combines with CO 2- to form 3 CuCO3.
Na+ combines with SO 2- to form 4 Na2SO4. CuSO + Na CO CuCO + 4 2 3 3 Na2SO4 4 Double Replacement Na CO3 + HCl
Notice that gas bubbles were produced rather than a precipitate. What was the gas? Write the double replacement reaction first. 2 Double Replacement Na CO3 + HCl Na+ combines with Cl- to form NaCl. H+ combines with CO 2- to form
3 H2CO3. Na CO + 2HCl 2NaCl + H CO 2 3 2 3 H CO breaks up into H O and CO . 2 3 2 2 2 Double Replacement
The gas formed was carbon dioxide. The final balanced reaction is: Na2CO3 + HCl NaCl + H2O + CO2. Balance the equation. Na CO + 2HCl 2NaCl + H O + 2 3 2 CO2 Combustion Reaction
When a substance combines with oxygen, a combustion reaction results. The combustion reaction may also be an example of an earlier type such as 2Mg + O2 2MgO. The combustion reaction may be burning of a fuel. Combustion
Reaction Methane, CH4, is natural gas. When hydrocarbon compounds are burned in oxygen, the products are water and carbon dioxide. CH + O CO + H O 4 2 2 2 CH + 2O CO + 2H O 4
2 2 2 Combustion Reactions Combustion reactions involve light and heat energy released. Natural gas, propane, gasoline, etc. are burned to produce heat energy. Most of these organic reactions produce water and carbon
dioxide. Practice Classify each of the following as to type: H 2 + Cl2 2HCl Combination
Ca + 2H2O Ca(OH)2 + H2 Single replacement Practice 2CO + O2 2CO2 Combination and combustion 2KClO 3
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