Sure, let's break this down step-by-step to understand which statement is correct according to Dalton's Atomic Theory.
Dalton's Atomic Theory includes several important postulates, one of which is that atoms of different elements combine in simple whole-number ratios to form compounds.
Let's analyze the given question with this in mind:
1. Case of Copper with +1 charge forming a compound with Chlorine:
- Copper (Cu) has a +1 charge and forms a compound with Chlorine (Cl).
- The chemical formula of the compound is CuCl.
2. Case of Copper with +2 charge forming a compound with Chlorine:
- Copper (Cu) has a +2 charge in this case.
- The chemical formula of the compound is CuCl₂.
According to Dalton's Atomic Theory:
- Atoms combine in fixed, simple, whole-number ratios to form compounds.
- Therefore, if we compare the compounds CuCl and CuCl₂, the ratio of Copper and Chlorine atoms in each compound is simple and whole.
Now, address each option given:
a. The masses of both compounds must be an integer:
- While it may seem intuitive to say that the masses of compounds should be integers, this statement does not directly align with Dalton's Atomic Theory specifics. Dalton's Theory focuses more on the ratios of atoms rather than the absolute masses.
b. The masses of both compounds must be the same:
- This statement is false because CuCl and CuCl₂ will have different masses due to differing numbers of Chlorine atoms present.
c. The ratio of the mass of one compound to another must be a whole number:
- This statement aligns with Dalton's Theory. Because the atoms combine in simple whole-number ratios, the ratio of the masses of the resulting compounds will also reflect these ratios. Hence, the mass ratio of CuCl to CuCl₂ will be a simple whole number.
d. None of the above:
- Since we've established that one of the options is correct, this statement can be ruled out.
Based on these steps, the correct option is:
c. The ratio of the mass of one compound to another must be a whole number
