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Displacement reaction is a type of reaction that replaces part of one reactor with another. It mean a more reactive element displacement a less reactive element, for example :Mg+ZnSO4=MgSO4+Zn.  Mg is more reactive than Zn, therefore Zinc have been displace by Mg

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A displacement reaction is a type of reaction in which part of the less reactive element is replaced by the more reactive reactant.

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A displacement is the one wherein the atom or set of atoms is displaced by another atom in a molecule

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A displacement is the one wherein the atom or set of atoms is displaced by another atom in a molecule

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Tina

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A reaction where part of a reactant is replaced by another more reactive reactant

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Displacement reaction is when the more reactive element displaces the less reactive element.

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A displacement reaction occurs when a more reactive metal displaces the less reactive metal.

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A displacement reaction is the one wherein the atom or a set of atoms is displaced by another atom in a molecule.

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Mg+ZnSO4=MgSO4+Zn

Mg+FeSO4=MgSO4+Fe

Mg+CuSO4=MgSO4+Cu

Zn+FeSO4=ZnSO4+Fe

Zn+CuSO4=ZnSO4+Cu

Fe+CuSO4=FeSO4+Cu

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A reaction where part of a less reactive element is replaced by another more reactive element.

Eg: Mg + FeSO4 --> MgSo4 + Fe

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Displacement reaction is when a more reactive element displaces an other less reactive element in a compound

Example:Mg+FeSO4—>MgSO4+Fe

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To find the reactivity of 4 different metal, definition of displacement, displacement reaction

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Displacement reaction refers to the reaction between the ionic root of an element or compound and an ionic compound

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Mg>Zn>Fe>Cu

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To understand displacement reactions through examining the reactivity of four metals, and redox reactions.

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Use displacement reactions to find the reactivity of four metals.

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Mg + ZnSO4 --> MgSO4 + Zn

Mg + FeSO4 --> MgSO4 + Fe

Mg + CuSO4 --> MgSO4 + Cu

Zn + FeSO4 --> ZnSO4 + Fe

Zn + CuSO4 --> ZnSO4 + Cu

Fe + CuSO4 -->FeSO4 + Cu

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To find the reactivity of four metals

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To understand how to use the displacement reaction to find the reactivity of metals

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Mg > Zn > Fe > Cu

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ZnSO4 + Mg → Zn + MgSO4

FeSO4 + Mg → Fe + MgSO4

CuSO4 + Mg → Cu + MgSO4

FeSO4 + Zn → Fe + ZnSO4

CuSO4 + Zn → Cu + ZnSO4

CuSO4 + Fe → Cu + FeSO4

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To find the definition of displacement and the reactivity of the 4 metals, Mg, Zn, Cu, Fe.

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To fine the define of  displacement reaction. The reactivity of four metal.

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Mg + ZnSO4 -> MgSO4 + Zn
Mg + FeSO4 -> MgSO4 + Fe
Mg + CuSO4 -> MgSO4 + Cu

Zn + FeSO4 -> ZnSO4 + Fe
Zn + CuSO4 -> ZnSO4 + Cu

Fe + CuSO4 -> FeSO4 + Cu

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Mg > Zn > Fe > Cu

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1.Have a paper of table of four Metal Salt Solution(MgSO ZnSO FeSO CuSO) and Metal
2. Add Mg Zn Fe Cu to the table (Have almost same amount in each box)
3.Add Metal Salt Solution to metal
4.Wait for a while to see reaction
5.Record the data

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Mg ( most reactive ) > Zn > Fe > Cu ( least reactive )

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find 4 metals reactivity by displacement reaction

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To find the definition of displacement and reactivity

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Mg+ZnSO4=MgSO4+Zn

Mg+FeSO4=MgSO4+Fe

Mg+CuSO4=MgSO4+Cu

Zn+FeSO4=ZnSO4+Fe

Zn+CuSO4=ZnSO4+Cu

Fe+CuSO4=FeSO4+Cu

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Mg>Zn>Fe>Cu

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Mg+ZnSO4—>MgSO4+Zn
Mg+FeSO4—>MgSO4+Fe
Mg+CuSO4—>MgSO4+Cu
Zn+FeSO4—>SnSO4+Fe
Zn+CuSO4—>ZnSO4+Cu
Fe+CuSO4—>FeSO4+Cu

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Mg+ZnSO4—> MgSo4+Zn
Mg+FeSO4—> MgSo4+Fe
Mg+CuSO4—> MgSo4+Cu
Zn+FeSO4—>ZnSo4+Fe
Zn+CuSO4—>ZnSo4+Cu
Fe+CuSO4—>FeSo4+Cu

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Mg+ZnSO4—>MgSO4+Zn
Mg+FeSO4—>MgSO4+Fe
Mg+CuSO4—>MgSO4+Cu
Zn+FeSO4—>SnSO4+Fe
Zn+CuSO4—>ZnSO4+Cu
Fe+CuSO4—>FeSO4+Cu

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Mg>Zn>Fe>Cu

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Mg>Zn>Fe>Cu

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Mg > Zn > Fe > Cu

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1. Have 4 different metals and metal solutions ready (Eg. CuSO4, MgSO4)
2. Place the 4 different metals in the different solutions
3. See if there is a reaction for each metal
4. The metal that reacts with most of the solutions is the most reactive

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ZnSO4 + Mg → Zn + MgSO4

FeSO4 + Mg → Fe + MgSO4

FeSO4 + Zn → Fe + ZnSO4

CuSO4 + Zn → Cu + ZnSO4

CuSO4 + Mg → Cu + MgSO4

CuSO4 + Fe → Cu + FeSO4

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Oxidising agent, it mean  a substance that has the ability to oxidize other substances.(Example: such as chlorine and fluorine), itself reduce. Reducing agent, it mean a substance that has the ability to reduce other substances.(Example :oxalic acid, and sulfite compounds)itself oxidised.

Potassium manganate: an oxidising agent,  Mn(+7)O-4(purple)---reduction---Mn-2(+2) (colorless)

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An oxidising agent oxidise another substance - it was reduced
A reducing agent reduces another substance - it was oxidised
E.g. Cl2 + 2Br- --> 2Cl- + Br2
Br loses electrons, so it is oxidised, it is the reducing agent
Cl2 gains electrons, it is reduced, it is the oxidising agent.

Potassium manganate is an oxidising agent. : MnO4(purple) -> reduction -> Mn2+(colorless)

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Mg > Zn > Fe > Cu

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Oxidising agents oxidise another substance. Meanwhile, itself is reduced. Reducing agents reduce another substance. Itself is oxidised.

E.g. Chlorine: Cl2 + 2e- -> 2Cl ( reduction )
E.g. Bromide Ion: 2Br- -> Br2 + 2e- ( oxidation )

POTASSIUM - OXIDISING AGENT:
Potassium is a purple compound. Its formula is KMnO4. In it, the manganese is in oxidation state + VII. But it is much more stable in oxidation state +II.

This is why potassium manganate (VII) acts as a powerful oxidising agent.

MnO4 ( purple manganate ion ) ——> Mn2+ ( colourless manganese ion )

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1.Prepare magnesium, zinc, iron, copper solutions

2.Make a table and put the solution and the metals that you wanted to test if its more reactive or less reactive with each other

3.Record the data of did one metal displace the other metal in the solution, if it does displace it, its more reactive

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2Mg + O2 --> 2MgO

In this equation, oxygen is the oxidizing agent as it is being reduced.
Magnesium is the reducing agent as it is being oxidized by oxygen.

Potassium manganate is an oxidising agent,  MnO-4(+7 oxidation state)(purple)---reduction---Mn-2(+2 oxidation state) (colorless)

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1. Prepare 4 different metals and metal solutions.
2. Put the metals in the metal salt solutions.
3. Wait to see the reactions.
4. More solutions the metal react with, the more reactive it is.

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Oxidising regent is element that can oxidise others and itself reduces
Example: Cl+e- —->Cl-
Reducing agent is when the element can reduce others and it self oxidises
Example: 2Mg—>2Mg+2e-
Potassium Manganate is a is a oxidising agent
Usually manganate(VII)
More stable with manganate(II)
MnO4——>Mn2+

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1) Prepare Mg, Zn, Fe and Au solutions
2) Place them in metal salt solutions
3) Observe the reaction

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1.prepare the metal
2. put all the 4 metals with salt solution together
3. give some time and see reaction
4. if the metal has less solution, than it not reactive, it more, than it is reactive

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Tina
1.Table four different metals and metal solutions(Mg Zn Fe Cu)
2.Put the metals in the metal salt solutions
3. Sea the reactions
4. The more reactive it is the more solutions the metal react with.

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Oxidising agent itself reduces, and Reducing agent itself oxidised.

example:Chlorine: Cl2 + 2e- -> 2Cl-

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1.Have magnesium zinc iron copper and metal solutions
2.Put the 4 different metals(Mg Zn Fe Cu) in the metal solutions
3.wait to see reaction
4.Record the data

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Oxidizing agents oxidize another substance with reduced itself.reducing agents reduce another with oxidized with itself.

2Mg + O2—>2MgO

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oxidising agent is a substance that can reduce itself and oxidise others
reducing agent is a substance that can oxidise itself and reduce others
example: Chlorine is an oxidising agent since it needs one electron in its valence shell to occupy the one empty space.

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Oxidant oxidizes another substance to reduce itself, and reductant oxidizes itself to reduce other substances

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Potassium manganate(VII) is a powerful oxidising agent.
The purple colour will fade after the reduction

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2Na+2HCl-->2NaCl+H2

Oxidation: 2Na=Na+ +2e-
Reduce: H2+2e=H2

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Zn+2HCl—>ZnCl2+H2

Oxidised: Zn—>Zn+2e-
Reduced:H2+2e—->H2

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Zn+2H+—>Zn2+ + H2
Oxidation: Zn—> Zn2+ +2e-
Reduction: 2H+ +2e- —> H2

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2Mg + Br2 -->2 MgBr

Oxidized: Mg--->Mg+2e-
Reduced: Br2 + 2e--->2Br

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Oxidation: 2Br - —> Br2 + 2e-
Reduction: Cl2 + 2e- —> 2Cl-

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oxidation: Zn -> Zn + 2e-

reduction: H2 + e -> 2H

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Zn + 2HCl —> ZnCl2 + H2

Oxidised: Zn —> Zn + 2e-

Reduced: H2+2e —> H2

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Zn+2H+—>Zn2+ + H2
Oxidation: Zn—> Zn2+ +2e-
Reduction: 2H+ +2e- —> H2

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Zn+2H+—>Zn2+H2

Oxidation: Zn-> Zn2+ +2e-
Reduction: 2H+ +2e- -> H2

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Zn+2H+->Zn2++H2

Oxidation Zn-> Zn^2+2e-

Reduction : 2H+ ->H2