Obtaining and Using Metals Flashcards
Describe the reactions of common metals with water and acids.
Metals like potassium, sodium, and calcium react vigorously with water, producing hydrogen gas and metal hydroxides.
Metals such as magnesium, zinc, and iron react with dilute acids to produce a salt and hydrogen gas.
Describe the reactions of metals with salt solutions.
More reactive metals displace less reactive metals from their salt solutions, forming a new metal and a new salt.
Explain why displacement reactions are redox reactions.
In displacement reactions, one metal is oxidized (loses electrons) and the other metal ion is reduced (gains electrons).
Deduce the order of metals in the reactivity series based on their reactions.
The reactivity series is deduced by observing how metals react with water, acids, and salt solutions, with more reactive metals displacing less reactive ones.
Explain the reactivity series in terms of the tendency of metal atoms to form cations.
More reactive metals lose electrons easily, forming cations more readily, which places them higher in the reactivity series.
Recall the meaning of the term ‘ore’.
An ore is a type of rock that contains sufficient metal content to make extraction economical.
Recall some metals found uncombined in Earth’s crust.
Metals like gold and platinum are found in pure form because they are unreactive.
Explain how and why some metals are extracted from their ores by heating with carbon.
Metals below carbon in the reactivity series can be extracted by heating with carbon, which reduces the metal oxide to metal.
Explain how and why some metals are extracted from their ores by electrolysis.
Metals above carbon in the reactivity series require electrolysis because they cannot be reduced by carbon.
Describe two biological methods of metal extraction.
Phytomining (using plants to absorb metals) and bioleaching (using bacteria to extract metals from ores).
Evaluate biological methods of metal extraction.
Biological methods are environmentally friendly and reduce energy use, but are slower than traditional methods and can be less efficient.
Explain why reactions at the electrodes during electrolysis are redox reactions.
Oxidation occurs at the anode, where ions lose electrons, and reduction occurs at the cathode, where ions gain electrons.
Describe the meanings of oxidation and reduction in terms of oxygen.
Oxidation is the gain of oxygen, while reduction is the loss of oxygen.
Explain which substance has been oxidized and which has been reduced in a reaction.
The substance that gains oxygen is oxidized, and the one that loses oxygen is reduced.
Recall that all metals are extracted by reduction of their ores
Metals are obtained by reducing their ores, typically through heating with carbon or electrolysis.
