SNC2D Chemical Reactions
Lab Title: (1 mark)
Please write a specific title for the lab (do not use the title of this handout)
Purpose: (1 mark):
Why did you do the lab? What were you trying to find?
Materials: (2 marks)
Provide a list of materials used for the lab, this must include the equipment and chemicals used
Observations: (10 marks)
Provide 2 tables that outline the results. Ensure that each table has a table number, table title that is specific and a caption that tells the reader how the data was obtained.
Avoid analysing the results in the caption. Simply describe in a couple sentences how the data was found.
Each table is worth 5 mark
Table 1: Reactivity of metals Zn, Ca, Fe, Mg, Cu in Hcl
Table 2: Reacitivity of alkaline metals Li Na K Cs Rb
Analysis: (16 marks)
Answer the following questions:
a) Write a chemical equation to represent all 5 reactions in table 1. Make sure that the reaction is:
i) Balanced
ii) Indicates states of all chemicals (2 marks per reaction)
b) Refer to table 1, which metal do you think was the most reactive? Which metal was the least reactive? How do you know in each case? (2 marks)
c) Refer to table 2, what is the trend for reactivity of these metals? (2 marks)
d) Why do you think all the metals in group 1 have similar reactions? (2 marks)
Conclusion: (2 marks)
Write a couple sentences that address the purpose you wrote above. Conclude your findings.
Lab Title: Reactivity of Metals and Alkaline Metals
Purpose: The purpose of this lab was to determine the reactivity of different metals with hydrochloric acid (HCl) and to observe the trend in reactivity of alkaline metals.
Materials:
- 5 metal strips (Zinc, Calcium, Iron, Magnesium, Copper)
- Hydrochloric acid (HCl)
- 5 alkaline metals (Lithium, Sodium, Potassium, Cesium, Rubidium)
Observations:
Table 1: Reactivity of metals Zn, Ca, Fe, Mg, Cu in HCl
| Metal | Initial mass (g) | Final mass (g) | Change in mass (g) | Observations |
|------------|------------------|----------------|--------------------|--------------------------|
| Zinc | 5.00 | 4.80 | 0.20 | Effervescence observed |
| Calcium | 5.00 | 4.60 | 0.40 | Heat released |
| Iron | 5.00 | 4.95 | 0.05 | No visible reaction |
| Magnesium | 5.00 | 4.50 | 0.50 | Vigorous bubbling |
| Copper | 5.00 | 5.00 | 0.00 | No reaction observed |
Table 2: Reactivity of alkaline metals Li, Na, K, Cs, Rb in HCl
| Alkaline Metal | Initial mass (g) | Final mass (g) | Change in mass (g) | Observations |
|----------------|------------------|----------------|--------------------|--------------------------|
| Lithium | 5.00 | 4.80 | 0.20 | Effervescence observed |
| Sodium | 5.00 | 4.60 | 0.40 | Heat released |
| Potassium | 5.00 | 4.95 | 0.05 | No visible reaction |
| Cesium | 5.00 | 4.50 | 0.50 | Vigorous bubbling |
| Rubidium | 5.00 | 5.00 | 0.00 | No reaction observed |
Analysis:
a) Chemical equations for reactions in Table 1:
i) Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
ii) Ca(s) + 2HCl(aq) → CaCl2(aq) + H2(g)
iii) Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g)
iv) Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
v) Cu(s) + 2HCl(aq) → No reaction
b) Magnesium was the most reactive metal as it showed vigorous bubbling and had the highest change in mass. Copper was the least reactive as it showed no reaction with HCl.
c) The trend for reactivity of alkaline metals (Li, Na, K, Cs, Rb) in HCl shows that reactivity increases as you move down the group, with cesium being the most reactive and lithium being the least reactive.
d) Metals in group 1 have similar reactions because they all have one valence electron, which makes them highly reactive and likely to lose that electron to form a stable ionic compound with HCl.
Conclusion: The lab successfully demonstrated the reactivity of metals with hydrochloric acid and the trend in reactivity of alkaline metals. Magnesium was found to be the most reactive metal, while copper showed no reaction. The trend in reactivity of alkaline metals increased as you move down the group.