Question

Using only the following elements P, Br, and Mg, give the formulas for:A. an ionic compound. B. a molecular compound with polar covalent bonds that obeys the octet rule and has no formal charges.

Answer 1

Answer:

1. Ionic compound- $MgBr_2$

2. Polar molecular compound- $PBr_3$

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 $MgBr_2$.

P is also a nonmetal and combine with Br with covalent bond and due to electronegativity differences form polar covalent compound such as $PBr_3$.

Answer 2

Ionic bond exists between magnesium and chlorine while a polar covalent bond exists between phosphorus and bromine.

An ionic compound is formed between metals and nonmetals while covalent compounds are formed between two nonmetals. In ionic compounds one atom transfers electrons to another atom while covalent bonds are shared.

• An ionic compound is formed between magnesium and bromine and the formula of the compound is MgBr2
• A polar covalent bond is formed between phosphorus and bromine and the formula of the compound is PBr3

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