
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
164.4k+ 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
Complex Numbers and Quadratic Equations Chapter For JEE Main Maths

Polymers Chapter for JEE Main Chemistry

Difference Between Electrophile and Nucleophile: JEE Main 2024

Hydrocarbons Chapter for JEE Main Chemistry

Chemistry in Everyday Life Chapter for JEE Main Chemistry

Chemical Thermodynamics Chapter for JEE Main Chemistry

Trending doubts
JEE Main Marks Vs Percentile Vs Rank 2025: Calculate Percentile Using Marks

JEE Mains 2025 Cutoff: Expected and Category-Wise Qualifying Marks for NITs, IIITs, and GFTIs

NIT Cutoff Percentile for 2025

JoSAA JEE Main & Advanced 2025 Counselling: Registration Dates, Documents, Fees, Seat Allotment & Cut‑offs

JEE Main 2025 Session 2: Application Form (Out), Exam Dates (Released), Eligibility, & More

JEE Main 2025 CutOff for NIT - Predicted Ranks and Scores

Other Pages
Total MBBS Seats in India 2025: Government and Private Medical Colleges

NEET Total Marks 2025

Neet Cut Off 2025 for MBBS in Tamilnadu: BC, MBC, SC & Government Colleges

Karnataka NEET Cut off 2025 - Category-wise Cut-off and Previous Year Trends

NEET Marks vs Rank 2024

NEET 2025 – Every New Update You Need to Know
