Question:
Boron halides behave as Lewis acids because they
Boron halides behave as Lewis acids because they
Updated On: Jul 6, 2022
- are covalent compounds
- are ionic compounds
- have only six electrons in the valence shell
- have a lone pair of electrons on the B atom
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The Correct Option is C
Solution and Explanation
Boron halides, $BX_3$ have only six electrons (three from B atom and three from three halogen atoms) around central B atom and thus B octet is not complete. Hence, boron halides behave as electron deficient compounds or Lewis acids.
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Concepts Used:
P-Block Elements
- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
- P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.
P block elements consist of:
- Group 13 Elements: Boron family
- Group 14 Elements: Carbon family
- Group 15 Elements: Nitrogen family
- Group 16 Elements: Oxygen family
- Group 17 Elements: Fluorine family
- Group 18 Elements: Neon family