QQuestionChemistry
QuestionChemistry
Rank the following atoms according to their size. 1st attempt I See Periodic Table o se Cations (5 items) (Drag and drop into the appropriate area)
# Cations (5 items) (Drag and drop into the appropriate area)
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Step 1:I will rank the given cations from smallest to largest based on their ionic radii.
The cation with the smallest ionic radius will be ranked first, and the one with the largest ionic radius will be ranked last. The cations are:
Step 2:Al^{3 +}
2. $$Mg^{2+}
Step 3:Na^{+}
4. $$K^{+}
Step 4:Ca^{2 +}
To rank these cations, I will use the general trend that, for the same group in the periodic table, cations with higher charges have smaller ionic radii, and within the same period, cations with higher atomic numbers have larger ionic radii.
Step 5:: Compare Al^{3 +} and Mg^{2 +}
- Both are from the same period (3rd period), but $$Al^{3+}$$ has a higher charge than $$Mg^{2+}$$.
Therefore, Al^{3 +} has a smaller ionic radius than Mg^{2 +}.
Step 6:: Compare Mg^{2 +} and Na^{+}
- $$Mg^{2+}$$ and $$Na^{+}$$ are from the same group (2nd group), but $$Mg^{2+}$$ has a higher charge than $$Na^{+}$$.
Therefore, Mg^{2 +} has a smaller ionic radius than Na^{+}.
Step 7:: Compare Na^{+} and K^{+}
- $$Na^{+}$$ and $$K^{+}$$ are from the same period (4th period), but $$Na^{+}$$ has a smaller atomic number than $$K^{+}$$.
Therefore, Na^{+} has a smaller ionic radius than K^{+}.
Step 8:: Compare K^{+} and Ca^{2 +}
- $$K^{+}$$ and $$Ca^{2+}$$ are from the same period (4th period), but $$Ca^{2+}$$ has a higher charge than $$K^{+}$$.
Therefore, Ca^{2 +} has a smaller ionic radius than K^{+}.
Final Answer
1. Al^{3 +} 2. Mg^{2 +} 3. Na^{+} 4. K^{+} 5. Ca^{2 +}
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