Reactivity Series of Metals
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Questions and Answers

Which metal burns with a lilac flame when heated in the air?

  • Potassium (correct)
  • Magnesium
  • Calcium
  • Sodium

What is the color of the flame observed when magnesium is heated in the air?

  • Brilliant white (correct)
  • Golden yellow
  • Brick red
  • White

What is the product formed when iron is heated strongly in the air?

  • Zinc oxide
  • Lead oxide
  • Iron oxide (correct)
  • Copper oxide

What is the observation when lead is heated strongly in the air?

<p>A yellow powder is formed on the surface (C)</p> Signup and view all the answers

Which metal reacts with oxygen to form a white powder when heated gently in the air?

<p>Sodium (A)</p> Signup and view all the answers

What is the product formed when copper is heated strongly in the air?

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

Which of the following is an example of a displacement reaction?

<p>Zn + CuSO4 → ZnSO4 + Cu (A)</p> Signup and view all the answers

Which of the following metals is most likely to displace copper from a copper sulfate solution?

<p>Mg (B)</p> Signup and view all the answers

What is the nature of aluminum oxide?

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

Which of the following metals is least reactive, according to the reactivity series?

<p>Au (B)</p> Signup and view all the answers

What is the oxidation state of iron in a reaction where it forms a compound with oxygen?

<p>+3 (A)</p> Signup and view all the answers

Which metal can displace copper from a copper(II) sulfate solution according to the reactivity series?

<p>Zinc (Zn) (B)</p> Signup and view all the answers

What is the oxidation state of sodium in a reaction where it forms a compound with chlorine?

<p>+1 (C)</p> Signup and view all the answers

What is the outcome of a metal displacement reaction involving a more reactive metal and a less reactive metal?

<p>The more reactive metal loses electrons and becomes a positive ion, while the less reactive metal gains electrons and becomes a neutral atom (B)</p> Signup and view all the answers

What happens when calcium is added to water?

<p>A colourless solution is produced. (B)</p> Signup and view all the answers

What is the product of the reaction between steam and zinc?

<p>Zinc oxide and hydrogen. (D)</p> Signup and view all the answers

What is the observation when potassium is added to water?

<p>It moves around on the surface of water. (C)</p> Signup and view all the answers

What is the product of the reaction between steam and iron?

<p>A black powder is produced. (D)</p> Signup and view all the answers

What happens when sodium is added to cold water?

<p>It dissolves and a colourless solution is produced. (B)</p> Signup and view all the answers

What is the product of the reaction between steam and magnesium?

<p>A white powder is produced. (C)</p> Signup and view all the answers

What happens when very reactive metals like potassium react with dilute acids?

<p>They react vigorously and produce a large amount of hydrogen gas. (A)</p> Signup and view all the answers

What is the reason for the lack of observable change when aluminium reacts with dilute acids at first?

<p>The protective oxide layer on the surface of the aluminium is reacting with the acid. (C)</p> Signup and view all the answers

What happens when the oxide layer on the surface of aluminium is completely reacted with the dilute acid?

<p>The acid reacts with the aluminium to form salt and hydrogen. (D)</p> Signup and view all the answers

Which of the following metals do not react with dilute acids?

<p>Copper and silver (B)</p> Signup and view all the answers

What is the product formed when aluminium oxide reacts with hydrochloric acid?

<p>Aluminium chloride and water (C)</p> Signup and view all the answers

What is the characteristic of the reaction between aluminium and dilute acids?

<p>It is a vigorous reaction. (B)</p> Signup and view all the answers

What is the purpose of heating the metal in the set-up?

<p>To vent with the steam (B)</p> Signup and view all the answers

What happens when calcium is added to water?

<p>Calcium hydroxide and hydrogen are produced (C)</p> Signup and view all the answers

What is the product of the reaction between steam and zinc?

<p>Zinc hydroxide and hydrogen (D)</p> Signup and view all the answers

Why should the mineral wool not be heated?

<p>It might explode (B)</p> Signup and view all the answers

What is the product of the reaction between steam and iron?

<p>A black powder is produced (C)</p> Signup and view all the answers

What is the observation when potassium is added to water?

<p>A colourless gas is evolved and it burns with a lilac flame (A)</p> Signup and view all the answers

Flashcards

Potassium flame color

Potassium produces a lilac flame when heated in air.

Magnesium flame color

Magnesium burns with a brilliant white flame.

Iron heated in air

Iron forms iron oxide (rust) when heated strongly in air.

Lead heated in air

Lead forms a yellow powder when heated in air.

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Sodium heated in air

Sodium forms a white powder when gently heated in air.

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Copper heated in air

Copper forms copper oxide when heated strongly in air.

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Displacement reaction example

A reaction where one element displaces another from a compound.

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Metal displacing copper

A more reactive metal displaces copper from a copper sulfate solution

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Aluminum oxide nature

Aluminum oxide is amphoteric, meaning it can react with both acids and bases.

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Least reactive metal

Gold (Au) is the least reactive metal in the reactivity series.

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Iron oxidation state

Iron can have an oxidation state of +3 when it forms a compound with oxygen.

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Metal displacing copper(II)sulfate

Zinc (Zn) can displace copper from copper(II) sulfate.

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Sodium oxidation state

Sodium has an oxidation state of +1 when forming a compound with chlorine.

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Metal displacement reaction outcome

A more reactive metal loses electrons and becomes a positive ion, while a less reactive metal gains electrons and becomes a neutral atom.

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Calcium reaction with water

Calcium reacts with water to produce calcium hydroxide and hydrogen.

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Steam and zinc product

Zinc reacts with steam to produce zinc oxide and hydrogen.

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Potassium reaction with water

Potassium reacts vigorously with water, moving on the surface and producing a lilac flame, along with hydrogen.

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Steam and iron product

Iron reacts with steam to produce iron(III) oxide (a black powder) and hydrogen.

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Sodium reaction with cold water

Sodium reacts with cold water to form sodium hydroxide and hydrogen.

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Steam and magnesium product

Magnesium reacts with steam to produce magnesium oxide and hydrogen.

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Reactive metals and dilute acids

Very reactive metals (like potassium) react vigorously with dilute acids, producing a large amount of hydrogen gas.

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Aluminium reaction with dilute acids (initial)

Initially, aluminum does not react visibly with dilute acids because of a protective oxide layer.

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Aluminium oxide layer reaction

Once the aluminium's protective oxide layer is reacted, the acid reacts with aluminium, producing salt and hydrogen.

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Metals unreactive with dilute acids

Copper and silver are not reactive with dilute acids.

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Aluminum oxide and hydrochloric acid reaction

Aluminium oxide reacts with hydrochloric acid to produce aluminium chloride and water.

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Aluminum and dilute acids reaction

The reaction between aluminium and dilute acids is vigorous.

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Purpose of heating metal

Heating metal (in particular with steam) is done to increase the reaction.

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Study Notes

Reactivity Series

  • A list of metals in order of their reactivity, with the most reactive at the top and the least reactive at the bottom
  • The series is based on the metal's ability to lose electrons and form ions
  • The reactivity series consists of, in order: potassium (K), sodium (Na), calcium (Ca), magnesium (Mg), aluminium (Al), zinc (Zn), iron (Fe), tin (Sn), lead (Pb), copper (Cu), silver (Ag), and gold (Au)

Oxidation States

  • The oxidation state of an element is the number of electrons it has lost or gained to form a bond
  • Metals tend to lose electrons to form a positive ion (cation) and have a positive oxidation state
  • The oxidation state of a metal can vary depending on the reaction it is involved in
  • Examples of oxidation states include:
    • Sodium (Na) typically having an oxidation state of +1
    • Iron (Fe) having oxidation states of +2 or +3
    • Copper (Cu) having oxidation states of +1 or +2

Metal Displacement

  • A reaction in which a more reactive metal displaces a less reactive metal from its compound
  • The more reactive metal loses electrons and becomes an ion, while the less reactive metal gains electrons and becomes a neutral atom
  • The reactivity series can be used to predict the outcome of metal displacement reactions
  • Examples of metal displacement reactions include:
    • Zinc (Zn) displacing copper (Cu) from copper(II) sulfate solution
    • Iron (Fe) not displacing copper (Cu) from copper(II) sulfate solution because iron is less reactive than copper

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Test your knowledge of the reactivity series of metals, including potassium, sodium, calcium, and magnesium. Learn how they react with oxygen and observe the different flames produced.

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