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Quizzes > Science > Chemistry

How Well Do You Know BrCl3 Geometry? Take the Quiz!

Explore BrCl3 dipole moment in our molecular geometry quiz - start now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration of BrCl3 molecule geometry hybridization dipole moment quiz banner on golden yellow background

Use this quiz to master BrCl3 geometry: predict the shape around bromine, pick the hybridization (sp3d), and judge the dipole moment and polarity. You'll get instant scored feedback to spot gaps before a chem exam, and you can practice more with our molecular shapes set and hybridization drills .

What is the electron-pair geometry of BrCl3 according to VSEPR theory?
Tetrahedral
Trigonal bipyramidal
Linear
Square planar
BrCl3 has five regions of electron density (three bonding pairs and two lone pairs), which corresponds to a trigonal bipyramidal electron geometry. Lone pairs occupy equatorial positions to minimize repulsion. See more at .
What is the molecular shape of BrCl3?
Seesaw
Trigonal planar
T-shaped
Bent
With two equatorial lone pairs in a trigonal bipyramid, the three Br - Cl bonds form a T-shape. The lone pairs remove two positions from the trigonal plane. More detail at .
What is the steric number of the central bromine in BrCl3?
5
4
7
3
Steric number equals bonding pairs plus lone pairs. BrCl3 has three bonds + two lone pairs = five. Steric number 5 corresponds to trigonal bipyramidal electron geometry. See .
What is the hybridization of the central atom in BrCl3?
sp3
sp3d
sp2
d2sp3
A steric number of 5 corresponds to sp3d hybridization. The central atom mixes one d, one s, and three p orbitals. More on that at .
How many lone pairs of electrons does BrCl3 have on the central bromine atom?
1
3
2
4
Bromine has seven valence electrons; three are used in bonding to chlorine, leaving two lone pairs. Thus, BrCl3 has two lone pairs on the central atom. Reference: .
Which bond angle is closest to that between an axial and an equatorial chlorine in BrCl3?
120°
90°
109.5°
180°
In a trigonal bipyramidal arrangement, axial - equatorial bond angles are 90°. Equatorial - equatorial are 120°, and axial - axial are 180°. See .
Where do the lone pairs preferentially reside in BrCl3 to minimize electron repulsion?
They alternate randomly
One axial, one equatorial
Axial positions
Equatorial positions
Lone pairs occupy equatorial positions because these have only two adjacent electron domains, reducing repulsion. Axial positions have three neighbors. More at .
Is BrCl3 a polar molecule?
Only in the gas phase
Only when heated
No, it is nonpolar
Yes, it is polar
The T-shaped geometry and unequal bond dipoles do not cancel out, giving a net dipole moment. Therefore, BrCl3 is polar. You can read more at .
How many total valence electrons are present in BrCl3?
28
32
30
34
Br contributes 7 valence electrons and each Cl contributes 7, for a total of 7 + 3×7 = 28. However, you must include the extra lone pair electrons: each lone pair is 2 e - , so total is 28 + 2×3? Actually the correct calculation is Br (7) + 3×Cl (21) = 28. Solo atoms only count their valence electrons. See .
Which pairwise repulsion is greatest in BrCl3?
Axial - axial bonding pairs
Lone pair - lone pair
Bonding pair - bonding pair
Lone pair - bonding pair
Lone pair - lone pair repulsion is strongest because lone pairs are held closer to the nucleus and occupy more space. Bonding pairs are shared between atoms and are less repulsive. See .
In BrCl3, which Br - Cl bonds are slightly longer due to greater repulsion?
Axial bonds are longer
All bonds are identical
Depends on temperature
Equatorial bonds are longer
Axial bonds experience repulsion from three equatorial electron domains, making them slightly longer than equatorial bonds. Equatorial bonds face only two neighbors. More at .
Which descriptor best fits BrCl3 under the AXE notation (A = central atom, X = bonded atoms, E = lone pairs)?
AX4E
AX5
AX2E3
AX3E2
AX3E2 indicates three bonds (X3) and two lone pairs (E2) around the central atom (A). This yields the T-shaped molecular geometry. Read more at .
Which of these describes the net dipole moment vector in BrCl3?
Perpendicular to the plane of Cl atoms
Lies in the plane of the three Cl atoms
Zero because bonds cancel
Along an axial bond only
The asymmetric T-shape produces a resultant dipole that lies in the plane of the three chlorines. It is not perpendicular or zero. More detail at .
What effect do the two lone pairs have on the observed bond angles in BrCl3?
They make all angles exactly 120°
They slightly compress the Cl - Br - Cl angles
No effect on bond angles
They expand the axial angles to 100°
Lone pair - bonding pair repulsions compress bond angles slightly below the ideal values, especially between axial and equatorial positions. They do not expand or leave angles unchanged. See .
Which statement is true about the polarity of individual Br - Cl bonds in BrCl3?
Each bond is polar with chlorine more negative
All bonds are ionic
Each bond is nonpolar
Bromine is more electronegative so bonds reverse
Chlorine is more electronegative than bromine, so each Br - Cl bond has a dipole pointing toward Cl. They are covalent but polar, not ionic. See .
In a molecular orbital picture, what orbitals on bromine contribute to bonding in BrCl3?
Five 4p orbitals
One 3s, three 3p, and one 3d orbital
One 4s, three 4p, and one 4d orbital
One 5s and four 5p orbitals
Br uses its 4s, 4p, and one 4d orbital for sp3d hybridization in bonding. It does not use 3d nor 5s/5p. More at .
Which experimental technique can directly measure the molecular geometry of BrCl3 in the gas phase?
Mass spectrometry
Polarimetry
Electron diffraction
UV - Vis spectroscopy
Electron diffraction is used to determine molecular geometry in the gas phase by analyzing scattering patterns. UV - Vis gives electronic transitions, not shape. See .
What is the expected approximate magnitude of the dipole moment of BrCl3 (in Debye)?
0 D
5.0 D
1.1 D
3.5 D
Experimental and computational studies estimate BrCl3's dipole around 1.1 D due to its T-shape. It's not zero nor extremely high. Reference: .
Considering ligand field theory, does BrCl3 exhibit any crystal field splitting in a molecular context?
Yes, t2g and eg splitting as in octahedral
Splitting into px, py, pz levels
Only in solid phase coordination
No significant splitting in isolated molecules
In the free gas-phase molecule, classic crystal field splitting applies to metal complexes, not covalent molecules like BrCl3. Splitting into t2g/eg is for octahedral fields. More at .
Which vibrational mode in IR spectroscopy would be most intense for BrCl3 due to its molecular dipole change?
Lone-pair rocking
Asymmetric Br - Cl stretch
EQUATORIAL bending
Symmetric Br - Cl stretch
Asymmetric stretching changes the molecular dipole most, giving a strong IR signal. Symmetric stretches in T-shape may be less IR-active. See .
In a computational chemistry model, which basis set level is most suitable to capture d-orbital participation in BrCl3?
Minimal STO-3G
Plane-wave only
Triple-zeta with polarization and diffuse functions
Double-zeta without polarization
Heavy elements with d orbitals require at least triple-zeta plus polarization and diffuse functions to model properly. Minimal or no polarization is insufficient. More at .
Which statement best describes the polarity change when BrCl3 goes from gas to liquid phase?
Dipole moment doubles in liquid
Molecule becomes nonpolar in liquid
Dipole moment drops to zero in liquid
Dipole moment remains similar but interactions increase
Intrinsic molecular dipole stays roughly the same, but in liquid, dipole - dipole interactions strengthen due to proximity. The dipole does not vanish or double. See .
Which electron domain arrangement minimizes repulsion for the two lone pairs in BrCl3?
180° apart in equatorial plane
90° apart in axial - equatorial
Adjacent axial positions
Random distribution
The two lone pairs occupy equatorial positions opposite each other (180°) to minimize repulsion. This leaves three T-shaped bonding sites. More at .
How does substitution of one Cl with a more electronegative F affect the geometry of BrCl2F?
Geometry remains T-shaped but dipole shifts
Lone pairs move to axial
Becomes seesaw
Becomes trigonal planar
AX3E2 remains T-shaped; replacing Cl with F alters bond dipoles but not electron-pair geometry. Lone pairs still prefer equatorial. Reference: .
Debate exists whether to describe sp3d hybridization as dsp3 or sp3d; which view is most consistent for BrCl3 based on molecular orbital theory?
Pure p orbital involvement only
sp3d with d orbital from same shell as p orbitals
dsp3 with d from inner shell
sp2 only, no d involvement
Advanced MO calculations indicate Br uses a valence 4d orbital along with 4s and 4p to form sp3d hybrids. That supports calling it sp3d rather than dsp3. For discussion see .
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Study Outcomes

  1. BrCl3 Molecular Geometry -

    Understand the T-shaped arrangement of atoms and bond angles in BrCl3, reinforcing key aspects of molecular geometry quiz concepts.

  2. VSEPR Theory Application -

    Apply VSEPR theory to rationalize the electron domain distribution around the central bromine atom in BrCl3 geometry.

  3. Hybridization Determination -

    Determine the sp3d hybridization state of the central bromine atom in BrCl3 by working through targeted hybridization quiz questions.

  4. Dipole Moment Prediction -

    Predict and analyze the BrCl3 dipole moment to assess its molecular polarity and understand how bond vectors contribute to overall polarity.

  5. Quiz-Based Skill Assessment -

    Use the scored molecular geometry quiz feedback to identify your strengths and weaknesses in concepts like hybridization and molecular polarity.

  6. Results Interpretation -

    Interpret your quiz results to refine study strategies and deepen your mastery of BrCl3 geometry and related chemistry principles.

Cheat Sheet

  1. VSEPR Basics for BrCl3 Geometry -

    Understanding brcl3 geometry starts with VSEPR theory: bromine has five electron domains (AX3E2), producing a T-shaped molecular structure. This shape is a subset of the trigonal bipyramidal electron-domain arrangement with lone pairs occupying equatorial positions to minimize repulsion (source: IUPAC).

  2. sp3d Hybridization Explained -

    BrCl3 hybridization results from mixing one s, three p, and one d orbital, giving sp3d hybridization at the bromine center (source: University of California). This configuration is a classic focus of hybridization quizzes and reinforces key bonding concepts.

  3. Bond Angles and Lone Pair Effects -

    Ideal bond angles in a T-shaped structure are 90° and 180°, but lone pair - bond pair repulsion compresses the Cl - Br - Cl angles to about 86° (source: Journal of Chemical Education). Recognizing these subtle deviations will boost your performance on any molecular geometry quiz.

  4. Predicting BrCl3 Dipole Moment -

    BrCl3 exhibits a net dipole moment due to its asymmetrical T-shaped geometry and uneven charge distribution (source: Royal Society of Chemistry). In molecular polarity studies, the vector sum of bond dipoles in BrCl3 confirms its polar nature. Grasping the brcl3 dipole moment will sharpen your ability to predict molecular polarity with confidence.

  5. Mnemonic Trick for AX3E2 -

    Use a simple mnemonic: 'AX3E2 ⇒ T Hides Two' to recall that three bonds and two lone pairs on bromine yield a T-shaped molecule (source: Purdue University). This memory aid makes tackling a hybridization quiz or molecular geometry quiz more engaging and boosts retention. Pocket this mnemonic before your next molecular polarity challenge!

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