Question

1. choose the best answer.which of these is the correct formula for aluminum oxide?aioai₂o3ai₃oai₃o₂4) type in each blank the charges for the ions based on their location using the periodic table. (see companion material attached.)lialmgfonne

Explanation:

Question 3

To determine the correct formula for aluminum oxide, we use the charges of the ions. Aluminum (Al) typically has a charge of \(+3\) (\( \text{Al}^{3+} \)) and oxygen (O) typically has a charge of \(-2\) (\( \text{O}^{2-} \)). To balance the charges, we use the criss - cross method: the magnitude of the charge of one ion becomes the subscript of the other ion. So, for \( \text{Al}^{3+} \) and \( \text{O}^{2-} \), we get \( \text{Al}_2\text{O}_3 \) (because \( 2\times(+3)+3\times(-2)=0 \), which satisfies the charge neutrality of a compound). Let's check the other options:

• For \( \text{AlO} \): The charge would be \(+3+(-2)= + 1\), which is not neutral.
• For \( \text{Al}_3\text{O} \): The charge would be \(3\times(+3)+(-2)=+7\), not neutral.
• For \( \text{Al}_3\text{O}_2 \): The charge would be \(3\times(+3)+2\times(-2)=+9 - 4 = + 5\), not neutral.

• Lithium (Li): Lithium is in Group 1 of the periodic table. Group 1 elements lose 1 electron to form ions with a charge of \(+1\) (\( \text{Li}^+ \)).
• Aluminum (Al): Aluminum is in Group 13. It loses 3 electrons to form an ion with a charge of \(+3\) (\( \text{Al}^{3+} \)).
• Magnesium (Mg): Magnesium is in Group 2. It loses 2 electrons to form an ion with a charge of \(+2\) (\( \text{Mg}^{2+} \)).
• Fluorine (F): Fluorine is in Group 17. It gains 1 electron to form an ion with a charge of \(-1\) (\( \text{F}^- \)).
• Oxygen (O): Oxygen is in Group 16. It gains 2 electrons to form an ion with a charge of \(-2\) (\( \text{O}^{2-} \)).
• Nitrogen (N): Nitrogen is in Group 15. It gains 3 electrons to form an ion with a charge of \(-3\) (\( \text{N}^{3-} \)).
• Neon (Ne): Neon is a noble gas. Noble gases are stable and do not form ions easily, so its charge is \(0\).

Answer:

B. \( \text{Al}_2\text{O}_3 \)

Question 4