
The central atom in a molecule is in \[s{p^2}\] hybrid state. The shape of molecule will be
A) Pyramidal
B) Tetrahedral
C) Octahedral
D) Trigonal planar
Answer
232.8k+ views
Hint: Here, the central atom's hybridization is given. And we have to find the molecule's shape. We know that the \[s{p^2}\] hybridised atom indicates that there will be the presence of three groups surrounding the central atom.
Complete Step by Step Answer:
Let’s discuss how we can identify the hybridization of a molecule. If the hybridization is \[s{p^3}\], the count of groups, that is, bond pairs and lone pairs are four. That means, four groups surround the central atom.
Similarly, we can find out the number of groups that surround the central atom, if the hybridization of the atom is \[s{p^2}\]. So, the number of groups, that is, all bond pairs or the bond-pair and lone pairs are three. So, the electron geometry of the molecule is trigonal planar.
Hence, the option D is right.
Additional Information: If the count of groups surrounding the central atom is five, the electron geometry of the molecule is trigonal bipyramidal. If the count of groups surrounding the central atom is four, the electron geometry of the molecule is tetrahedral. If the count of groups surrounding the central atom is eight, the electron geometry of the molecule is octahedral.
Note: It is to be noted that molecular geometry is different from electron pair geometry. If the count of bond pair and lone pair surrounding an atom is two and one respectively, the electron geometry is trigonal planar but the molecular geometry is bent.
Complete Step by Step Answer:
Let’s discuss how we can identify the hybridization of a molecule. If the hybridization is \[s{p^3}\], the count of groups, that is, bond pairs and lone pairs are four. That means, four groups surround the central atom.
Similarly, we can find out the number of groups that surround the central atom, if the hybridization of the atom is \[s{p^2}\]. So, the number of groups, that is, all bond pairs or the bond-pair and lone pairs are three. So, the electron geometry of the molecule is trigonal planar.
Hence, the option D is right.
Additional Information: If the count of groups surrounding the central atom is five, the electron geometry of the molecule is trigonal bipyramidal. If the count of groups surrounding the central atom is four, the electron geometry of the molecule is tetrahedral. If the count of groups surrounding the central atom is eight, the electron geometry of the molecule is octahedral.
Note: It is to be noted that molecular geometry is different from electron pair geometry. If the count of bond pair and lone pair surrounding an atom is two and one respectively, the electron geometry is trigonal planar but the molecular geometry is bent.
Recently Updated Pages
Area of an Octagon Formula Explained Simply

Absolute Pressure Formula Explained: Key Equation & Examples

Central Angle of a Circle Formula Explained Quickly

Difference Between Vapor and Gas: JEE Main 2026

Difference Between Atom and Molecule: JEE Main 2026

Carbon Dioxide Formula - Definition, Uses and FAQs

Trending doubts
JEE Main 2026: Session 2 Registration Open, City Intimation Slip, Exam Dates, Syllabus & Eligibility

JEE Main 2026 Jan 21 Shift 1 Question Papers with Solutions & Answer Keys – Detailed Day 1 Analysis

JEE Main Response Sheet 2026 Released – Key Dates and Official Updates by NTA

JEE Main 2026 Answer Key OUT – Download Session 1 PDF, Response Sheet & Challenge Link

JEE Main Marks vs Percentile 2026: Calculate Percentile and Rank Using Marks

JEE Main 2026 Jan 22 Shift 1 Today Paper Live Analysis With Detailed Solutions

Other Pages
Happy New Year Wishes 2026 – 100+ Messages, Quotes, Shayari, Images & Status in All Languages

One Day International Cricket

Valentine Week 2026: Complete List of Valentine Week Days & Meaning of Each Day

List of Highest T20 Scores in International Cricket

Makar Sankranti Wishes: Happy Makar Sankranti Wishes in Marathi, Hindi, Kannada, and English

What is the Full Form of UGC? Detailed Guide for Students

