Properties and Reactions of Metals
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Questions and Answers

Why are metals often combined to create alloys?

  • To reduce their melting point significantly.
  • To improve their properties compared to individual metals. (correct)
  • To decrease their electrical conductivity.
  • To make them completely non-reactive with acids.

    • What happens when an acid is dissolved in water?

  • It releases hydrogen ions ($H^+$). (correct)
  • It releases hydroxide ions ($OH^-$).
  • It forms a metallic bond.
  • It precipitates a solid.

    • How does litmus paper react in the presence of an acid?

  • It remains unchanged.
  • It turns blue.
  • It turns green.
  • It turns red. (correct)

    • What products are formed when an acid reacts with a base?

    <p>A salt and water. (B)</p> Signup and view all the answers

    Which of the following best describes a characteristic property of bases?

    <p>Feeling slippery and releasing hydroxide ions in water. (B)</p> Signup and view all the answers

    Which property is generally associated with metals?

    <p>Lustrous appearance when polished (A)</p> Signup and view all the answers

    What does the reactivity series of metals indicate?

    <p>The order in which metals displace each other from their compounds (A)</p> Signup and view all the answers

    What are the products of a metal reacting with an acid?

    <p>Salt and hydrogen gas (B)</p> Signup and view all the answers

    What observation would most likely confirm that a metal is reacting with an acid?

    <p>Production of hydrogen gas bubbles (D)</p> Signup and view all the answers

    Which factor does not affect the rate of reaction between a metal and an acid?

    <p>The volume of the reaction vessel (A)</p> Signup and view all the answers

    Why is copper commonly used in electrical wiring?

    <p>Due to its high electrical conductivity (A)</p> Signup and view all the answers

    What happens to the temperature of a metal-acid reaction as the reaction proceeds?

    <p>It may increase, indicating an exothermic reaction (D)</p> Signup and view all the answers

    Which of the following metals is expected to react most vigorously with dilute hydrochloric acid?

    <p>Magnesium (C)</p> Signup and view all the answers

    Flashcards

    Alloys

    Metals combined to improve properties compared to individual metals.

    Acids

    Substances that release hydrogen ions (H+) in water, often sour and corrosive.

    Litmus Paper Test

    A test that turns blue paper red in acidic solutions.

    Neutralisation Reaction

    Combining an acid and a base to produce salt and water, typically neutral pH.

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    Common Bases

    Substances that release hydroxide ions (OH-) and feel slippery, like sodium hydroxide.

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    High Melting and Boiling Points

    Metals typically have high temperatures at which they melt and boil.

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    Conductivity

    Metals are excellent conductors of heat and electricity.

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    Malleability and Ductility

    Malleable metals can be shaped; ductile metals can be drawn into wires.

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    Reactivity Series

    The list showing the order of metals based on their reactivity.

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    Reaction with Acids

    Metals react with acids to form salt and hydrogen gas.

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    Key Observations

    Bubbles of gas, temperature changes, and color shifts indicate reactions.

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    Factors Affecting Reactions

    Reactivity, acid concentration, temperature, and surface area influence metal reactions.

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    Metal Uses

    Different metals have specific uses based on their properties.

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    Study Notes

    Properties of Metals

    • Metals generally have high melting and boiling points.
    • Metals are good conductors of heat and electricity.
    • Metals are usually malleable (can be hammered into sheets) and ductile (can be drawn into wires).
    • Metals tend to be lustrous (shiny).
    • Different metals have different strengths and densities.

    Reactivity Series of Metals

    • The reactivity series shows the order in which metals react with other substances.
    • A more reactive metal will displace a less reactive metal from its compound.
    • The most reactive metals are at the top of the series, and the least reactive are at the bottom.
    • Example metals in the reactivity series include potassium, sodium, magnesium, iron, copper, and silver.
    • Knowing a metal's position in the reactivity series helps predict its reactions with acids and other substances.

    Reactions of Metals with Acids

    • Metals react with acids to produce a salt and hydrogen gas.
    • The reaction is more vigorous with more reactive metals.
    • The type of salt produced depends on the metal and the acid.
    • The equation for a general reaction is: Metal + Acid → Salt + Hydrogen
    • Examples of reactions include magnesium reacting with hydrochloric acid producing magnesium chloride.
    • Observing bubbles of gas often indicates that a reaction has taken place.

    Observations in Metal Acid Reactions

    • A visible change in the metal is sometimes observed.
    • The metal may dissolve or disappear during the reaction.
    • Production of hydrogen gas bubbles is a key observation in these reactions.
    • The temperature of the reaction mixture may increase, signifying that heat is released.
    • The solution's appearance may change (color) due to the presence of the new salt.

    Factors Affecting Metal Reactions

    • The reactivity of the metal. More reactive metals react more vigorously.
    • The concentration of the acid. Higher concentrations usually lead to faster reactions.
    • The temperature. Higher temperatures can speed up the rate of reaction.
    • The surface area of the metal. A larger surface area provides more area for reaction.

    Uses of Metals

    • Different metals have specific properties that make them useful for various applications.
    • Iron is used in construction and making tools due to its strength.
    • Copper is used in electrical wiring due to its conductivity.
    • Aluminium is used in food packaging due to its lightweight properties.
    • Metals are often combined to create alloys, which have improved properties compared to the individual metals.

    Acids

    • Acids are substances that release hydrogen ions (H+) when dissolved in water.
    • Acids have a sour taste and can corrode some materials.
    • Common examples include hydrochloric acid, sulfuric acid, and nitric acid.
    • Acid strength differs based on the amount of hydrogen ions released which can be measured using a pH scale.
    • Acids are important in many chemical reactions and industrial processes.

    Identifying Acids

    • Litmus paper turns red in the presence of acid.
    • Universal indicator displays different colours depending on the acid concentration.

    Neutralisation Reactions

    • An acid reacts with a base to form a salt and water.
    • This reaction is known as neutralisation.
    • The reaction often results in a decrease in acidity or basicity.
    • The pH of the resultant solution will be near 7 (neutral).
    • Neutralisation reactions are widely used in various applications.

    Common Bases

    • Bases release hydroxide ions (OH-) when dissolved in water.
    • Bases often feel slippery and can be corrosive like bleach (sodium hypochlorite) or drain unblocker (sodium hydroxide).
    • Common bases include sodium hydroxide and potassium hydroxide.

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    Description

    Explore the fundamental properties of metals, their reactivity series, and the reactions they have with acids. This quiz covers essential concepts in understanding metal characteristics and behavior. Test your knowledge of metals and their properties in various chemical contexts.

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