Question

1. potassium and sulfur

• potassium charge: ______
• sulfur charge: ______
• final formula: ______

section e
#\tions used\tformula\twhy the charges balance
10\taluminum + chlorine\t____\t____
11\tcalcium + phosphorus\t____\t____
12\tmagnesium + nitrogen\t____\t____

part 3 — reflection
answer in complete sentences.

1. what happens to the number of ions needed as ion charge increases?

______
______

1. how did the simulator help you understand ionic bonding?

______
______

Explanation:

Step1: Find K and S ion charges

Potassium (Group 1) has charge $+1$; Sulfur (Group 16) has charge $-2$.

Step2: Balance charges for K and S

To balance $+1$ and $-2$, need 2 K⁺ ions: $2(+1) + (-2) = 0$. Final formula: $\text{K}_2\text{S}$.

Step3: Find Al and Cl ion charges

Aluminum (Group 13) has charge $+3$; Chlorine (Group 17) has charge $-1$.

Step4: Balance charges for Al and Cl

To balance $+3$ and $-1$, need 3 Cl⁻ ions: $(+3) + 3(-1) = 0$. Final formula: $\text{AlCl}_3$.

Step5: Find Ca and P ion charges

Calcium (Group 2) has charge $+2$; Phosphorus (Group 15) has charge $-3$.

Step6: Balance charges for Ca and P

To balance $+2$ and $-3$, use 3 Ca²⁺ and 2 P³⁻: $3(+2) + 2(-3) = 0$. Final formula: $\text{Ca}_3\text{P}_2$.

Step7: Find Mg and N ion charges

Magnesium (Group 2) has charge $+2$; Nitrogen (Group 15) has charge $-3$.

Step8: Balance charges for Mg and N

To balance $+2$ and $-3$, use 3 Mg²⁺ and 2 N³⁻: $3(+2) + 2(-3) = 0$. Final formula: $\text{Mg}_3\text{N}_2$.

Answer:

3. Potassium and Sulfur

• Potassium charge: $+1$
• Sulfur charge: $-2$
• Final formula: $\text{K}_2\text{S}$

Section E

1. Aluminum + Chlorine

• Formula: $\text{AlCl}_3$
• Why the Charges Balance: $+3 + 3(-1) = 0$

1. Calcium + Phosphorus

• Formula: $\text{Ca}_3\text{P}_2$
• Why the Charges Balance: $3(+2) + 2(-3) = 0$

1. Magnesium + Nitrogen

• Formula: $\text{Mg}_3\text{N}_2$
• Why the Charges Balance: $3(+2) + 2(-3) = 0$

Part 3 — Reflection

1. As the magnitude of an ion's charge increases, the number of the opposing charge ions needed to balance the overall charge changes inversely: a higher charge on one ion means fewer of that ion are needed relative to a lower-charged counterion to reach a net neutral charge.
2. A simulator helps visualize the transfer of electrons between metal and nonmetal atoms, shows how ions form with specific charges, and demonstrates the ratio of ions required to create a neutral ionic compound, making the abstract concept of ionic bonding concrete and easier to grasp.