I did an experiment where You will place five metals in different metal ion solutions to see which combinations of metals and ions result in single displacement reactions. The metal are Mg(s) (MgSO4 )

Khizra Malik Chemistry lab report

Grade: 11 month date year

Determining what combinations of metals and ions

result in a single displacement reactions

Purpose:

To determine what combination of metals and ions result in a single displacement reaction.

Hypothesis:

From the most reactive metal ion to the least reactive metal ion:

Mg> Zn>Sn Fe> Cu

The most reactive metal ion is Magnesium (Mg) and the least reactive is copper (Cu).

Variables

Oxidizing agents

Reducing agents

Reactivity series of the metals and their ions

Equipment and Materials

• chemical safety goggles - clean strips of magnesium,Zinc,Iron,Tin and copper.

• lab apron - dropper bottles of dilute solutions of

• well plat magnesium sulfate, MgSO4 (0.1 mol/L)

• sandpaper zinc sulfate, ZnSO4 (0.1 mol/L)

iron(II) sulfate, FeSO4 (0.1 mol/L)

tin(II) chloride, SnCl2 (0.1 mol/L)

copper(II) sulfate, CuSO4 (0.1 mol/L)

Procedure

A procedure was designed to determine which metal/metal ion solution combinations result in a single displacement reaction; the procedure was to place five metals in different metal ion solutions to see which metal/ion combinations result in single displacement reactions; and then it was continued with the teacher's approval. The reaction was recorded only when a new solid was formed, regardless of any gas bubbles that might form. Only 8 reactions took place and then the contents of the well plate was disposed of as per the teacher's instructions. The last step was to clean the workstation and wash hands.

Observation table

Ions

a) It was recorded whether a reaction happened by observation significant charges after adding the metals to different solutions

• Colour change of solutions

• Formation of precipitate

The experiment aims to determine which of the metals is the most reactive. It is

important to recall that metals can give electrons in an oxidation-reduction reaction,

which is why they are called reducing agents. This is why we can classify metals

according to their strength as reducing agents or their reactivity.

b) The reactivity of metals ions increases as we go from top to bottom. Based upon the data the elements from most reactive to least reactive: 1. Mg, 2. Zn. 3.Sn, 4.Fe, and 5. Cu (least reactive)

Explanation:

Mg reacted to displace Zn2+, Cu2+, Sn2+ and Fe2+. This represents all 4 of the other ions so Mg is the most reactive.

Zn reacted to displace Sn+2 and Cu+2. Based on the data it is the second most reactive replacing only 2 of the other ions.

Fe and Sn reacted to displace Cu+2. Therefore, based on the data, we have no evidence to place them one above the other and we must list them as a tie for the next most reactive one.

Cu did not displace any of the other ions so is least active.

c) The atomic size of metal increases while going down in periodic table due to which they tend to lose electrons easily, and from moving left to right in A periodic table, the atomic size of metal decrease hence;

• Reactivity of metal increases while going down in the periodic table.

• Reactivity of metal decreases while moving left to right in the periodic table.

Same trend follows for the reactivity of ions.

d) The order if reactivity of metal ions is;

Ba+2 > Ni+2 > Hg+2

Justification: Barium is present in 2A group which is on the left side of periodic table followed by Nickel atom in 10 group and Mercury in 12, therefore barium will have most reactive ions and then nickel and then mercury.

e) Writing a chemical equation for each single displacement reaction recorded

1. Mg(s)  + ZnSO4(aq) → Zn(s) + MgSO4(aq)

Mg(s) + Zn+2(aq) + SO4-2(aq) → Zn(s) + Mg+2(aq) + SO4-2 (aq)

Mg(s) + Zn+2(aq) → Zn(s) + Mg+2(aq)

2. Mg(s)  + CuSO4(aq) → Cu(s) + MgSO4(aq)

Mg(s) + Cu+2(aq) + SO4-2(aq) → Cu(s) + Mg+2(aq) + SO4-2(aq)

Mg(s)  + Cu+2(aq) → Cu(s) + Mg+2(aq)

3. Mg(s)  + SnCl2(aq) → Sn(s) + MgCl2(aq)

Mg(s) + Sn+2(aq) + 2Cl-(aq) → Sn(s) + Mg+2(aq) + 2Cl-(aq)

Mg(s) + Sn+2(aq) → Sn(s) + Mg+2(aq)

.

4. Mg(s)  + FeSO4(aq) → Fe(s) + MgSO4(aq)

Mg(s) + Fe+2(aq) + SO4-2(aq) → Fe(s) + Mg+2(aq) + SO4-2 (aq)

Mg(s) + Fe+2(aq) → Fe(s) + Mg+2(aq)

5. Zn(s) + CuSO4(aq) → Cu(s) + ZnSO4(aq)

Zn(s) + Cu+2(aq) + SO4-2(aq) → Cu(s) + Zn+2(aq) + SO4-2(aq)

Zn(s) + Cu+2(aq) → Cu(s) + Zn+2(aq)

6. Zn(s) + SnCl2(aq) → Sn(s) + ZnCl2(aq)

Zn(s) + Sn+2(aq) + 2Cl-(aq) → Sn(s) Zn+2(aq) + 2Cl-(aq)

Zn(s) + Sn+2(aq)→ Sn(s) Zn+2(aq)

7. Sn(s) + CuSO4(aq) → Cu(s) + SnSO4(aq)

Sn(s) + Cu+2(aq) + SO4-2(aq) → Cu(s) + Sn+2(aq) + SO4-2 (aq)

Sn(s) + Cu+2(aq)→ Cu(s) + Sn+2(aq)

8.Fe(s) + CuSO4(aq) → Cu(s) + FeSO4(aq)

Fe(s) + Cu+2(aq) + SO4-2(aq) → Cu(s) + Fe+2(aq) + SO4-2 (aq)

Fe(s) + Cu+2(aq) → Cu(s) + Fe+2(aq)

Source of error

f) No, copper piping is not a suitable choice because copper is above silver and gold on the activity series. Metals that are higher up on the activity series are more likely to exist as ions because they more readily lose electrons (they are more easily oxidized). Any metal will reduce ions below it on the activity series, meaning copper will lose electrons and these would be gained by the silver and gold ions. Since copper loses electrons, Cu(s) changes to Cu2+(aq) and the copper piping would fall apart over time so no, copper piping is not a suitable choice.

Conclusion

The combination of what metals and ions cause in a single displacement reaction in this experiment resulted in only 8 reactions occurring and they were between Mg(s) and Zn2+ ,

Mg(s) and CU2+(aq) , Mg(s) and Sn2+(aq) , Mg(s) and Fe2+(aq) , Zn(s) and CU2+(aq) , Zn(s) and Sn2+(aq) ,

Sn(s) and CU2+(aq) , Fe(s) and CU2+(aq).