Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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Multiple Choice

After drawing the Lewis structure of BrF3, what is the ideal bond angle around the central bromine atom?

109.5°

120°

90° and 180°

104.5°

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Verified step by step guidance

Identify the central atom in BrF3, which is bromine (Br), and count the total number of valence electrons from bromine and the three fluorine atoms.

Draw the Lewis structure by placing bromine in the center and connecting it to three fluorine atoms with single bonds, then distribute the remaining electrons to satisfy the octet rule, noting that bromine can have an expanded octet.

Determine the electron pair geometry around the bromine atom by counting the number of bonding pairs (3 Br-F bonds) and lone pairs on bromine (2 lone pairs), giving a total of 5 regions of electron density.

Use the VSEPR theory to predict the molecular shape based on 5 electron pairs: the electron geometry is trigonal bipyramidal, but the presence of 2 lone pairs changes the molecular shape to T-shaped.

Identify the ideal bond angles in a trigonal bipyramidal arrangement: equatorial positions have 120° angles, axial positions have 90° angles with equatorial atoms, and because the lone pairs occupy equatorial positions, the bond angles between bonded atoms are approximately 90° and 180°.