Reactivity Series of Metals

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

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

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

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

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

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

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

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

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

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

<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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

Potassium produces a lilac flame when heated in air.

Magnesium burns with a brilliant white flame.

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

Lead forms a yellow powder when heated in air.

Sodium forms a white powder when gently heated in air.

Copper forms copper oxide when heated strongly in air.

A reaction where one element displaces another from a compound.

A more reactive metal displaces copper from a copper sulfate solution

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

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

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

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

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

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

Calcium reacts with water to produce calcium hydroxide and hydrogen.

Zinc reacts with steam to produce zinc oxide and hydrogen.

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

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

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

Magnesium reacts with steam to produce magnesium oxide and hydrogen.

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

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

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

Copper and silver are not reactive with dilute acids.

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

The reaction between aluminium and dilute acids is vigorous.

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