Questions: Complete the table below. For example, in the first row decide whether Sc^3+ is a cation or anion. In the second row, write the symbol for the ion that an atom of potassium is mostly likely to form and then decide what type of ion it is.

Complete the table below. For example, in the first row decide whether Sc^3+ is a cation or anion. In the second row, write the symbol for the ion that an atom of potassium is mostly likely to form and then decide what type of ion it is.

Transcript text: Complete the table below. For example, in the first row decide whether $\mathrm{Sc}^{3+}$ is a cation or anion. In the second row, write the symbol for the ion that an atom of potassium is mostly likely to form and then decide what type of ion it is.

Solution

Solution Steps

Step 1: Determine the Ion for Potassium

Potassium (K) is an alkali metal located in Group 1 of the periodic table. Alkali metals typically lose one electron to achieve a stable electron configuration, forming a cation with a charge of $+1$. Therefore, the most likely ion for potassium is $ \mathrm{K}^+ $.

Step 2: Determine the Ion for Phosphorus

Phosphorus (P) is a non-metal located in Group 15 of the periodic table. Non-metals in this group typically gain three electrons to achieve a stable electron configuration, forming an anion with a charge of $-3$. Therefore, the most likely ion for phosphorus is $ \mathrm{P}^{3-} $.

Step 3: Determine the Ion for Calcium

Calcium (Ca) is an alkaline earth metal located in Group 2 of the periodic table. Alkaline earth metals typically lose two electrons to achieve a stable electron configuration, forming a cation with a charge of $+2$. Therefore, the most likely ion for calcium is $ \mathrm{Ca}^{2+} $.

Step 4: Determine the Ion for Fluorine

Fluorine (F) is a halogen located in Group 17 of the periodic table. Halogens typically gain one electron to achieve a stable electron configuration, forming an anion with a charge of $-1$. Therefore, the most likely ion for fluorine is $ \mathrm{F}^- $.

Final Answer

\[ \begin{array}{|c|c|c|} \hline \text{element} & \text{symbol of ion} & \text{type of ion} \\ \hline \text{scandium} & \mathrm{Sc}^{3+} & \text{cation} \\ \hline \text{potassium} & \mathrm{K}^+ & \text{cation} \\ \hline \text{phosphorus} & \mathrm{P}^{3-} & \text{anion} \\ \hline \text{calcium} & \mathrm{Ca}^{2+} & \text{cation} \\ \hline \text{fluorine} & \mathrm{F}^- & \text{anion} \\ \hline \end{array} \]

\[ \boxed{ \begin{array}{c} \text{Potassium: } \mathrm{K}^+ \text{ (cation)} \\ \text{Phosphorus: } \mathrm{P}^{3-} \text{ (anion)} \\ \text{Calcium: } \mathrm{Ca}^{2+} \text{ (cation)} \\ \text{Fluorine: } \mathrm{F}^- \text{ (anion)} \end{array} } \]

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