Question

question 1. determine the correct formulas for the compounds formed between the following:

a. mg²⁺ and oh⁻

b. k⁺ and so₄²⁻

c. nh₄⁺ and cl⁻

d. li⁺ and po₄³⁻

:: mgoh₂ :: mg(oh)₂ :: mg₂oh :: mg₂(oh)₂ :: k₂so₄ :: k₂(so₄)₂ :: k(so₄)₂ :: kso₄ :: (nh₄)₁cl :: (nh₄)₁cl₁ :: nh₄cl :: (nh₄)₂cl :: li₃po₄ :: li(po₄)₃ :: lipo₄ :: li₃(po₄)₃

Explanation:

Step1: Solve for \( \text{Mg}^{2+} \) and \( \text{OH}^- \)

To form a neutral compound, the total positive charge must equal the total negative charge. \( \text{Mg}^{2+} \) has a +2 charge, and \( \text{OH}^- \) has a -1 charge. We need 2 \( \text{OH}^- \) ions to balance the +2 charge of \( \text{Mg}^{2+} \). So the formula is \( \text{Mg(OH)}_2 \).

Step2: Solve for \( \text{K}^+ \) and \( \text{SO}_4^{2-} \)

\( \text{K}^+ \) has a +1 charge, and \( \text{SO}_4^{2-} \) has a -2 charge. We need 2 \( \text{K}^+ \) ions to balance the -2 charge of \( \text{SO}_4^{2-} \). So the formula is \( \text{K}_2\text{SO}_4 \).

Step3: Solve for \( \text{NH}_4^+ \) and \( \text{Cl}^- \)

\( \text{NH}_4^+ \) has a +1 charge, and \( \text{Cl}^- \) has a -1 charge. The charges are equal in magnitude (1+ and 1-), so we need 1 of each ion. The formula is \( \text{NH}_4\text{Cl} \).

Step4: Solve for \( \text{Li}^+ \) and \( \text{PO}_4^{3-} \)

\( \text{Li}^+ \) has a +1 charge, and \( \text{PO}_4^{3-} \) has a -3 charge. We need 3 \( \text{Li}^+ \) ions to balance the -3 charge of \( \text{PO}_4^{3-} \). So the formula is \( \text{Li}_3\text{PO}_4 \).

Answer:

a. \( \text{Mg(OH)}_2 \)
b. \( \text{K}_2\text{SO}_4 \)
c. \( \text{NH}_4\text{Cl} \)
d. \( \text{Li}_3\text{PO}_4 \)