Reactivity Series Metals Reactions with Water and Acid
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Describe and explain what determines the reactivity of a certain metal in the reactivity series.
Metal atoms form positive ions by loss of electrons when they react with other substances The tendency of a metal to lose electrons is a measure of how reactive the metal is A metal that is high up on the series loses electrons easily and is thus more reactive than one which is lower down on the series
Note that although carbon and hydrogen are non-metals, they are included in the reactivity series, why is this?
Note that although carbon and hydrogen are non-metals, they are included in the reactivity series as they are useful in extracting metals from their oxides by reduction processes
Reactivity Series: In order of least to most reactive, denote the reactivity of the 13 metals in the reactivity series.
Reactivity Series: Most reactive 1 - Potassium (K) 2 - Sodium (Na) 3 - Lithium (Li) 4 - Calcium (Ca) 5 - Magnesium (Mg) 6 - Aluminium (Al) 7 - Carbon (C) 8 - Zinc (Zn) 9 - Iron (Fe) 10 - Hydrogen (H) 11 - Copper (Cu) 12 - Silver (Ag) 13 - Gold (Au) Least reactive “Please Send Lions, Cats, Monkeys and Cute Zebras Into Hot Countries Signed Gordon”
Metals Reacting with Cold Water: In order of least to most reactive, denote the reactivity of the 13 metals in the reactivity series with cold water.
Metals Reacting with Cold Water: Most reactive 1: Potassium - Reacts violently 2: Sodium - Reacts quickly 3: Lithium - Reacts less strongly 4: Calcium - Reacts less strongly 5: Magnesium - No reaction 6: Zinc - No reaction 7: Iron - Slow rusting 8: Copper - No reaction Least reactive Other metals are unreactive; only metals above hydrogen in the reactivity series will react with water
Metals Reacting with Cold Water: (1) Metals that react with cold water form a metal hydroxide and hydrogen gas: metal + water → metal hydroxide + hydrogen For example, calcium: Ca + 2H₂O → _______ + ___
Metals Reacting with Cold Water: (1) Metals that react with cold water form a metal hydroxide and hydrogen gas: metal + water → metal hydroxide + hydrogen For example, calcium: Ca + 2H₂O → Ca(OH)₂ + H₂
Metals Reacting with Cold Water: (2) Magnesium reacts very slowly with cold water when finely divided Magnesium reacts with gaseous water to form a metal oxide and hydrogen gas: Mg + H₂O → _____ + ___
Metals Reacting with Cold Water: (2) Magnesium reacts very slowly with cold water when finely divided Magnesium reacts with gaseous water to form a metal oxide and hydrogen gas: Mg + H₂O → MgO + H₂
Metals Reacting with Dilute Acid: In order of least to most reactive, denote the reactivity of the 13 metals in the reactivity series with dilute acid.
Metals Reacting with Dilute Acid: Most reactive 1: Potassium - Reacts violently 2: Sodium - Reacts violently 3: Lithium - Reacts vigorously 4: Calcium - Reacts vigorously 5: Magnesium - Reacts vigorously 6: Zinc - Reacts less strongly 7: Iron - Reacts less strongly Least reactive Other metals are unreactive; only metals below hydrogen in the reactivity series will not react with acids.
Metals Reacting with Dilute Acid: When acids and metals react, the hydrogen atom in the acid is replaced by the metal atom to produce a salt and hydrogen gas: metal + acid → metal salt + hydrogen For example iron: Fe + 2HCI → ______ + ___
Metals Reacting with Dilute Acid: When acids and metals react, the hydrogen atom in the acid is replaced by the metal atom to produce a salt and hydrogen gas: metal + acid → metal salt + hydrogen For example iron: Fe + 2HCI → FeCl₂ + H₂ In both these types of reactions (water and acids) the metals are becoming positive ions.