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Chapter 8: Problem 70

Which one of the following statements regarding \(\mathrm{BF}_{3}\) is not correct? (a) It is a Lewis acid (b) It is an ionic compound (c) It is an electron deficient compound (d) It forms adducts

Short Answer

Expert verified
Option (b) is not correct; \(\mathrm{BF}_{3}\) is not ionic.

Step by step solution

01

Understand the Nature of BF3

Boron trifluoride (\(\mathrm{BF}_{3}\)) is a compound composed of boron and fluorine. Boron typically has three valence electrons and forms three covalent bonds with three fluorine atoms. This results in a total of six electrons around boron, rather than the octet (eight electrons) that many atoms strive for.
02

Evaluate Each Option

- **Option (a):** Lewis acids are species that can accept electron pairs. Since \(\mathrm{BF}_{3}\) is electron-deficient, it can accept electrons, making it a Lewis acid.- **Option (b):** Ionic compounds are formed of cations and anions with ionic bonds. \(\mathrm{BF}_{3}\) forms covalent bonds, not ionic, as boron shares electrons with fluorine.- **Option (c):** Electron-deficient compounds have fewer electrons than needed for a complete octet. \(\mathrm{BF}_{3}\) is electron-deficient as boron only has six electrons surrounding it.- **Option (d):** Adducts are formed when a Lewis acid such as \(\mathrm{BF}_{3}\) accepts an electron pair from a donor, forming a coordination complex.
03

Identify the Incorrect Statement

Comparing our analysis from Step 2, the correct options (a, c, d) align with \(\mathrm{BF}_{3}\)'s properties. Option (b) stating that it is an ionic compound is incorrect because \(\mathrm{BF}_{3}\) is covalent.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Lewis Acid
A Lewis acid is a chemical species that can accept a pair of electrons. This is an important concept in chemistry, particularly in understanding reactions where electron pairs are transferred. In the case of boron trifluoride (\( \mathrm{BF}_{3} \)), its structure enables it to function as a Lewis acid.
  • As \( \mathrm{BF}_{3} \) is electron-deficient, it has an unfulfilled need for electrons.
  • This electron deficiency makes it eager to accept electron pairs from other molecules or ions, classifying it as a Lewis acid.
  • A typical reaction would involve \( \mathrm{BF}_{3} \) accepting an electron pair from a donor, like a nitrogen atom in ammonia (\( \mathrm{NH}_{3} \)).
By understanding the concept of Lewis acids, we can better appreciate the kinds of reactions \( \mathrm{BF}_{3} \) engages in, like the formation of adducts.
Covalent Bond
Covalent bonds form when two atoms share one or more pairs of electrons. In boron trifluoride, each boron atom bonds with three fluorine atoms through covalent bonding.
  • The boron atom has three valence electrons and forms a single covalent bond with each of the three fluorine atoms, which need one more electron to achieve a full outer shell.
  • These shared pairs of electrons constitute the covalent bonds in \( \mathrm{BF}_{3} \).
  • This sharing allows all involved atoms to attain a more stable electronic configuration.
This fundamental aspect demonstrates why \( \mathrm{BF}_{3} \) is not an ionic compound; instead, it relies on covalent interactions between boron and fluorine.
Electron Deficient Compound
An electron-deficient compound, like \( \mathrm{BF}_{3} \), has fewer electrons around an atom than required for a stable octet configuration. Boron, in this case, finds itself with only six electrons in total after forming bonds with fluorine.
  • Boron's tendency is to pursue the electron configuration similar to a noble gas, which typically means having eight electrons.
  • This deficiency marks \( \mathrm{BF}_{3} \) as an electron-deficient compound, motivating it to seek extra electrons from other chemicals.
  • As a result, it can readily take part in reactions where electron pairs are donated by other species.
Understanding this deficiency is key to predicting how \( \mathrm{BF}_{3} \) behaves chemically, as it often leads to forming complexes with electron-rich compounds.
Adduct
An adduct forms when a Lewis acid and a Lewis base combine, sharing one or more electron pairs. \( \mathrm{BF}_{3} \) often forms adducts due to its nature as a Lewis acid.
  • When a compound like ammonia, which can donate electron pairs, interacts with \( \mathrm{BF}_{3} \), an adduct is formed as the nitrogen atom donates a pair of electrons to the boron.
  • This forms a stable complex or adduct, which can alter properties and reactivities of the initial substances.
  • Adduct formation highlights \( \mathrm{BF}_{3} \)'s role in chemical synthesis and coordination chemistry.
This aspect of chemistry showcases the dynamic interactions within molecules, illustrating new conduction pathways and stability through adduct formation.

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Most popular questions from this chapter

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Which of the following has the lowest melting point? (a) B \(\square\) (b) Ga (c) \(\mathrm{Al}\) (d) \(\mathrm{Tl}\)
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