Ready to sharpen your hybridization practice skills? Dive into our free quiz challenge designed to test your understanding of orbital hybridization. Whether you're reviewing for exams or reinforcing lecture concepts, this interactive orbital hybridization quiz offers a series of thought-provoking hybridization practice questions and problem-solving scenarios to elevate your chemistry comfort zone. Throughout this journey, you'll learn to identify orbital mixing, predict molecular shapes, and confidently assign hybridization states in real-world molecules. Curious how well you can apply sp, sp2, and sp3 concepts? Jump in now and put your knowledge to the test! For a quick warm-up, try our molecular geometry quiz or explore another chemistry practice quiz before you begin. Click start and conquer these hybridization orbitals practice problems today!
What is the hybridization of the carbon atom in methane (CH4)?
sp3
sp2
sp
sp3d
The carbon in methane forms four equivalent sigma bonds with hydrogen and has no lone pairs, giving a steric number of 4 and sp3 hybridization. The geometry is tetrahedral. Each hybrid orbital overlaps with an H 1s orbital to form a sigma bond. Learn more.
What is the hybridization of the carbon atoms in ethene (C2H4)?
sp3
sp2
sp
sp3d
Each carbon in ethene forms three sigma bonds (two to H and one to the other C) and one pi bond, for a steric number of 3 and sp2 hybridization. The remaining unhybridized p orbitals on each carbon overlap to form the pi bond. This gives a planar structure. Reference.
What is the hybridization of the carbon atoms in acetylene (C2H2)?
sp3
sp2
sp
sp3d
In acetylene each carbon forms two sigma bonds (one to H and one to the other C) and two pi bonds, giving a steric number of 2 and sp hybridization. Two unhybridized p orbitals on each carbon form the two pi bonds. The molecule is linear. Details.
What is the hybridization of the nitrogen atom in ammonia (NH3)?
sp3
sp2
sp
sp3d
Nitrogen in NH3 has three sigma bonds and one lone pair, giving a steric number of 4 and sp3 hybridization. The lone pair occupies one hybrid orbital, resulting in a trigonal pyramidal shape. Chemguide explanation.
What is the hybridization of the nitrogen atom in molecular nitrogen (N2)?
sp3
sp2
sp
sp3d
In N2 each nitrogen forms one sigma bond and two pi bonds to the other nitrogen, giving a steric number of 2 and sp hybridization. Each nitrogen uses two unhybridized p orbitals for the pi bonds. The molecule is linear. Learn more.
What is the hybridization of the oxygen atom in water (H2O)?
sp3
sp2
sp
sp3d
Oxygen in H2O has two sigma bonds and two lone pairs, giving a steric number of 4 and sp3 hybridization. The two lone pairs occupy hybrid orbitals, creating a bent shape. Reference.
What is the hybridization of the carbon atom in carbon dioxide (CO2)?
sp3
sp2
sp
sp3d
In CO2 the central carbon forms two sigma bonds to oxygen and has no lone pairs, giving a steric number of 2 and sp hybridization. The molecule is linear with two pi bonds formed from unhybridized p orbitals. More information.
What is the hybridization of the boron atom in boron trifluoride (BF3)?
sp3
sp2
sp
sp3d
Boron in BF3 forms three sigma bonds and has no lone pairs, giving a steric number of 3 and sp2 hybridization. The molecule is trigonal planar. Chemguide.
What is the hybridization of the phosphorus atom in phosphorus pentafluoride (PF5)?
sp3
sp2
sp3d
sp3d2
Phosphorus in PF5 forms five sigma bonds and has no lone pairs, giving a steric number of 5 and sp3d hybridization. The geometry is trigonal bipyramidal. Reference.
What is the hybridization of the sulfur atom in sulfur hexafluoride (SF6)?
sp3
sp3d
sp3d2
sp2
Sulfur in SF6 forms six sigma bonds and has no lone pairs, giving a steric number of 6 and sp3d2 hybridization. The molecule is octahedral. Details.
What is the hybridization of the chlorine atom in chlorine trifluoride (ClF3)?
sp3
sp3d
sp3d2
sp2
Chlorine in ClF3 has five regions of electron density (three bonds and two lone pairs), giving a steric number of 5 and sp3d hybridization. The shape is T-shaped. Learn more.
What is the hybridization of the central carbon in formaldehyde (H2C=O)?
sp3
sp2
sp
sp3d
Carbon in formaldehyde forms three sigma bonds and has no lone pairs, giving a steric number of 3 and sp2 hybridization. One unhybridized p orbital overlaps with oxygen to form a pi bond. The molecule is planar. Reference.
What is the hybridization of the nitrogen atom in the nitrate ion (NO3–)?
sp3
sp2
sp
sp3d
The nitrogen in NO3– has three sigma bonds and no lone pairs, giving a steric number of 3 and sp2 hybridization. One p orbital on nitrogen overlaps with oxygen p orbitals in resonance to delocalize the pi electrons. The ion is planar. Learn more.
What is the hybridization of the carbon atom in carbonic acid (H2CO3)?
sp3
sp2
sp
sp3d
In H2CO3, the central carbon forms three sigma bonds (two to OH and one to O) and one pi bond, giving a steric number of 3 and sp2 hybridization. The molecule is planar around carbon. Reference.
What is the hybridization of the sulfur atom in sulfur dioxide (SO2)?
sp3
sp2
sp
sp3d
Sulfur in SO2 has two sigma bonds and one lone pair, giving a steric number of 3 and sp2 hybridization. The lone pair occupies one hybrid orbital and the molecule is bent. One unhybridized p orbital forms a pi bond with oxygen. More info.
What is the hybridization of the phosphorus atom in the phosphate ion (PO4 3–)?
sp2
sp3
sp3d
sp3d2
Phosphorus in PO4 3– forms four sigma bonds and has no lone pairs, giving a steric number of 4 and sp3 hybridization. The geometry is tetrahedral. Reference.
What is the hybridization of the xenon atom in xenon tetrafluoride (XeF4)?
sp3
sp3d
sp3d2
sp2
Xe in XeF4 has six regions of electron density (four bonds and two lone pairs), giving a steric number of 6 and sp3d2 hybridization. The geometry is square planar. Learn more.
What is the hybridization of the sulfur atom in sulfur tetrafluoride (SF4)?
sp3
sp3d
sp3d2
sp2
Sulfur in SF4 has five electron domains (four bonds and one lone pair), giving sp3d hybridization and a seesaw shape. One lone pair occupies an equatorial position. Details.
What is the hybridization of the central carbon atom in allene (C3H4)?
sp3
sp2
sp
sp3d
In allene, the central carbon forms two double bonds and has no lone pairs, giving a steric number of 2 and sp hybridization. The terminal carbons are sp2. This results in orthogonal pi systems. Reference.
What is the hybridization of the carbon atoms in benzene (C6H6)?
sp3
sp2
sp
sp3d
Each carbon in benzene forms three sigma bonds and has one unhybridized p orbital, giving a steric number of 3 and sp2 hybridization. The p orbitals overlap to form a delocalized pi system. The molecule is planar. Learn more.
What is the hybridization of the oxygen atom in the hydronium ion (H3O+)?
sp3
sp2
sp
sp3d
In H3O+, oxygen has three sigma bonds and one lone pair, giving a steric number of 4 and sp3 hybridization. The geometry is trigonal pyramidal. Reference.
What is the hybridization of the central atom in ozone (O3)?
sp
sp2
sp3
sp3d
The central oxygen in O3 has two sigma bonds and one lone pair, giving a steric number of 3 and sp2 hybridization. One unhybridized p orbital overlaps in resonance to delocalize electrons. The molecule is bent. More info.
What is the hybridization of each oxygen atom in the carbonate ion (CO3 2–)?
sp3
sp2
sp
sp3d
In CO3 2–, each oxygen is bonded to carbon with one sigma bond and two lone pairs, giving a steric number of 3 and sp2 hybridization. The pi bonds are delocalized over the three oxygens. The ion is planar. Read more.
What is the effective hybridization of the carbon atoms in cyclopropane?
sp3
sp2
sp
sp2d
Although cyclopropane C–C bonds are often drawn as sigma bonds between sp3 carbons, the ring strain forces the C–C bonds to have increased p-character. The effective hybridization is closer to sp2, with bond angles around 60°. Detailed explanation.
In the guanidinium ion (C(NH2)3+), what is the hybridization of each nitrogen atom?
sp3
sp2
sp
sp3d
In guanidinium each nitrogen is involved in resonance delocalization of the positive charge across the C–N bonds, giving a steric number of 3 around each nitrogen and sp2 hybridization. The molecule is planar. Learn more.
0
{"name":"What is the hybridization of the carbon atom in methane (CH4)?", "url":"https://www.quiz-maker.com/QPREVIEW","txt":"What is the hybridization of the carbon atom in methane (CH4)?, What is the hybridization of the carbon atoms in ethene (C2H4)?, What is the hybridization of the carbon atoms in acetylene (C2H2)?","img":"https://www.quiz-maker.com/3012/images/ogquiz.png"}
Study Outcomes
Identify Hybrid Orbital Types -
You will be able to recognize sp, sp2, sp3, and other hybrid orbitals in various molecules based on their electron domain counts and connectivity.
Predict Molecular Geometry -
You can predict molecular shapes and bond angles by applying hybridization principles to determine the arrangement of electron pairs around central atoms.
Apply Hybridization Practice to Bonding -
You will apply hybridization practice strategies to classify bonds as sigma or π and to solve orbital hybridization problems more accurately.
Analyze Sigma and π Interactions -
You will analyze how different hybrid orbitals overlap to form sigma and π bonds, improving your understanding of covalent interactions.
Differentiate Hybridization States in Complex Molecules -
You will differentiate hybridization states in multi-atom structures by evaluating electron domain geometries and resonance effects.
Evaluate Your Mastery with the Quiz -
You will assess your performance through the orbital hybridization quiz to pinpoint areas for further practice and mastery.
Cheat Sheet
Hybrid Orbital Types and Geometries -
Review sp, sp2, and sp3 hybrid orbitals by correlating each with its geometry: linear (180°), trigonal planar (120°), and tetrahedral (109.5°). Use the mnemonic "S,P3=Tree, S,P2=Plane, S,P=Line" to recall shapes easily (source: MIT OpenCourseWare). Practice identifying these in diverse molecules through hybridization practice questions.
Electron Domains and VSEPR -
Master the link between electron domain count and hybridization by using VSEPR theory: count bonding and lone pairs to assign the right orbital set (source: University of Illinois Department of Chemistry). Remember that five and six domains require sp3d and sp3d2 hybridization respectively, offering new shapes like trigonal bipyramidal and octahedral. Regularly solve hybridization orbitals practice problems to reinforce this mapping.
Sigma and Pi Bond Formation -
Distinguish sigma (σ) bonds formed by head-on overlap of hybrid orbitals from pi (π) bonds formed by side-on overlap of unhybridized p orbitals (source: McMurry's Organic Chemistry). Recognize that single bonds are σ only, while double and triple bonds add one or two π bonds on top of the σ framework. Applying this concept in orbital hybridization quiz scenarios strengthens your bond-counting and hybridization skills.
Real-World Molecule Examples -
Analyze molecules like methane (sp3), ethene (sp2), and acetylene (sp) to see hybridization in action, and extend to compounds such as PCl5 (sp3d) and SF6 (sp3d2) using examples from research repositories (source: Journal of Chemical Education). Drawing Lewis structures then mapping each atom's electron domains will guide you to the right hybridization. Use these examples in your hybridization practice to build confidence before tackling more complex systems.
Effective Hybridization Practice Strategies -
Boost retention by mixing hybridization practice questions with orbital hybridization exercises, starting with simple molecules and progressing to polyatomic ions and coordination compounds. Time yourself with an orbital hybridization quiz to simulate exam conditions and review mistakes immediately (source: Khan Academy). Regular, spaced repetition of these exercises solidifies patterns in orbital selection and geometry assignments.
