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Quizzes > Science > Chemistry

Molecular Structure Quiz: Test Your Chemistry Mastery

Ready for a molecular geometry quiz? Challenge your electron configuration skills!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Layered paper art molecules atoms electrons orbitals resonance arrows on teal background for molecular structure quiz

Ready to unlock the secrets of chemical bonding? Dive into our molecular structure quiz, a fun molecular geometry quiz designed to challenge your understanding of shapes and interactions. In this electron configuration quiz, you'll apply VSEPR theory, spot trigonal bipyramidal arrangements, and explore resonance effects. You'll reinforce key concepts like bond angles, hybridization, molecular polarity, and resonance phenomena along the way. Perfect for chemistry students prepping for exams or anyone eager for a brain-teasing challenge, you'll gain instant feedback and boost your confidence with each question. Start now: try the free molecular structure quiz or test your skills further in our molecular shape quiz today!

What is the molecular geometry of CH4?
Tetrahedral
Trigonal planar
Bent
Linear
CH4 has four bonding pairs around the central carbon and no lone pairs, which arranges the atoms as far apart as possible in three dimensions, resulting in a tetrahedral geometry. This shape minimizes electron pair repulsion according to VSEPR theory. Carbon in CH4 is sp3 hybridized, leading to bond angles of approximately 109.5. Learn more.
Which electron pair geometry describes NH3?
Tetrahedral
Trigonal pyramidal
Bent
Trigonal planar
NH3 has three bonding pairs and one lone pair around nitrogen, giving four regions of electron density. VSEPR theory classifies four electron domains as tetrahedral electron pair geometry. The lone pair occupies one vertex of the tetrahedron, while the three hydrogens occupy the others. Reference.
What hybridization does the central carbon in CO2 exhibit?
sp
sp2
sp3
dsp2
CO2 is a linear molecule with two regions of electron density around the central carbon atom. VSEPR theory indicates that two domains correspond to sp hybridization. The 180 bond angle and linear arrangement arise from mixing one s and one p orbital. Further reading.
What is the bond angle in H2O?
104.5
109.5
120
90
Water has two bonding pairs and two lone pairs on the central oxygen atom. The lone pairs repel more strongly than bonding pairs, compressing the HOH angle to about 104.5. This gives water a bent molecular shape. Chemguide reference.
Which of the following molecules exhibits resonance?
Benzene (C6H6)
Methane (CH4)
Ammonia (NH3)
Water (H2O)
Benzene has a cyclic conjugated ? system in which electrons are delocalized over all six carbon atoms. This delocalization is represented by resonance structures. Neither methane, ammonia, nor water have such conjugated ? networks. Read more.
Which molecule contains a central atom that expands its octet?
SF6
BF3
CH4
NH3
In SF6, sulfur forms six SF bonds, using 12 valence electrons and exceeding the octet rule. This is possible because sulfur has available d orbitals to accommodate extra electron density. BF3 actually has an incomplete octet, while CH4 and NH3 follow the octet rule. Learn more.
Which of the following molecules has a net dipole moment?
SO2
CO2
BF3
CH4
SO2 has a bent geometry with unequal distribution of electron density, giving it a net dipole moment. CO2 and BF3 are linear and trigonal planar respectively with symmetric charge distribution, resulting in no net dipole. CH4 is also nonpolar due to its tetrahedral symmetry. Reference.
What is the molecular geometry of XeF4?
Square planar
Tetrahedral
See-saw
Square pyramidal
XeF4 has six electron domains: four bonding pairs and two lone pairs on xenon. VSEPR theory places the lone pairs opposite each other in an octahedral arrangement, leaving the fluorine atoms in a square plane. This gives a square planar molecular geometry. More info.
What is the formal charge on the central nitrogen atom in the nitrate ion, NO3-?
+1
0
-1
+2
In one resonance form of NO3-, nitrogen is bonded to three oxygens (one double bond and two single bonds) with no lone pairs. The formal charge is calculated as valence electrons (5) minus nonbonding electrons (0) minus half the bonding electrons (6 pairs = 12 electrons/2 = 6), giving +1. The overall negative charge resides on the oxygens. See calculation.
Predict the molecular shape and electron pair geometry of ClF3.
T-shaped (trigonal bipyramidal)
See-saw (trigonal bipyramidal)
T-shaped (octahedral)
Trigonal planar (trigonal planar)
ClF3 has five regions of electron density (three bonding pairs and two lone pairs) around the central chlorine, leading to a trigonal bipyramidal electron geometry. According to VSEPR theory, the lone pairs occupy equatorial positions to minimize repulsion, resulting in a T-shaped molecular geometry. Bond angles are compressed slightly from idealized positions due to lone pair repulsions. Detailed explanation.
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Study Outcomes

  1. Analyze molecular geometries -

    Identify and distinguish shapes such as trigonal bipyramidal, tetrahedral, and linear in the molecular geometry quiz to better grasp three-dimensional structures.

  2. Predict bond angles -

    Estimate bond angles using VSEPR theory and understand how electron pair repulsion influences molecular shape and geometry.

  3. Determine electron configurations -

    Assign electron configurations for atoms within molecules and relate these configurations to overall structure and reactivity.

  4. Interpret resonance structures -

    Compare and evaluate resonance forms to assess their contribution to molecular stability and delocalized electron distribution.

  5. Apply VSEPR principles -

    Use valence shell electron pair repulsion theory to deduce three-dimensional arrangements and predict the most stable molecular geometry.

  6. Predict molecular polarity -

    Determine molecule polarity by combining knowledge of geometry, bond polarity, and electron distribution to anticipate dipole moments.

Cheat Sheet

  1. VSEPR Shapes and Bond Angles -

    Dive into VSEPR theory (IUPAC guidelines) to predict molecular geometries by minimizing electron-pair repulsions, like the trigonal bipyramidal structure with 120° equatorial and 90° axial bonds. A catchy mnemonic - "three in the equator, two at the poles" - helps cement those angles. This trick transforms even the trickiest molecular structure quiz questions into quick recall.

  2. Hybridization and Steric Number -

    Determine an atom's hybridization by counting its steric number: the sum of bonded atoms and lone pairs dictates sp, sp², sp³, sp³d or sp³d² hybridization (as detailed in MIT OpenCourseWare). For example, PCl₅ exhibits sp³d hybridization forming a trigonal bipyramid, while CH₄ is classic sp³. Mastering this link makes any molecular geometry quiz smoother.

  3. Electron Configuration & Molecular Orbitals -

    Apply the Aufbau principle and Hund's rule from reputable sources like the University of California to fill atomic and molecular orbitals - 1s→2s→2p→σ2p<π2p→π*2p<σ*2p. Remember O₂'s paramagnetism arises from two unpaired electrons in π*2p, a common electron configuration quiz staple. Sketching MO diagrams boosts confidence for molecular structure quiz sections.

  4. Resonance Structures and Delocalization -

    Use resonance to depict electron delocalization in molecules such as benzene (C₆H₆) and carbonate (CO₃²❻), following arrow-pushing rules from ACS resources. Favor structures with full octets and minimal charge separation to identify the major contributor. This strategy reinforces your answers in resonance quiz problems.

  5. Bond Order, Length & Strength -

    Understand that bond order = (bonding electrons − antibonding electrons)/2 (as explained by Chemistry LibreTexts); increasing bond order shortens and strengthens bonds (e.g., C≡C vs C=C vs C - C). Recognizing this trend helps predict molecular stability and reactivity in both molecular geometry and resonance quizzes. Drawing correlations between bond order and bond length makes your quiz answers stand out.

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