Which diagram shows the correct way to represent an ionic compound of magnesium oxide?

Element X reacts with element Y to give a product containing X3+ ions and Y2− ions.

Maksim231197 [3]

Answer:

X₂Y₃

Explanation:

X⇒X³⁺ + 3e⁻ /×2

Y + 2e⁻ ⇒ Y²⁻ /×3

2X⇒2X³⁺ 6e⁻

3Y + 6e⁻⇒ 3Y²⁻

2X + 3Y ⇒2X³⁺ + 3Y²⁻ ⇒ X₂Y₃

Electron from one side and from other side can be shortened so we multiply half equations to get equivalent number of electrons on both side. Next step is summing these two half equations. Element Y takes two electrons from element X, so X become positive charged, and Y become negatively charged. It is very likely that element Y have greater electronegativity.

5 0

2 years ago

According to the lab guide, which changes below will you look for in order to test the hypothesis? check all that apply. changes

viktelen [127]

Answer:

All of them are.

Explanation:

8 0

2 years ago

Read 2 more answers

Using only the following elements P, Br, and Mg, give the formulas for:A. an ionic compound. B. a molecular compound with polar

Talja [164]

Answer:

<h2>1. Ionic compound- $MgBr_2$ </h2><h2>2. Polar molecular compound- $PBr_3$ </h2>

Explanation:

Mg is a metal that has 12 atomic numbers and thus its electronic configuration is $1s^22s^22p^63s^2$ . The outer most shell of this element has 2 electrons so it loses 2 electrons and thus form $Mg^2^+$ ions. Br is a nonmetal and has 35 atomic number so its electronic configuration is $1s^22s^22p^63s^23p^64s^23d^1^04p^5$ . Since its outermost shell has 7 electrons so it can accept one electron and thus forms $Br^-$ . So magnesium ion and bromide ion combine and forms an ionic compound $MgBr_2$ .