Molecular Geometry: VSEPR Theory
Learn about molecular geometry through VSEPR theory, which explains how bonded and lone pair electrons arrange themselves around a central atom to minimize repulsive forces. Explore different molecular shapes such as linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral. Understand concepts like bond angles and the use of wedge and dash notation.
Recommended next
18 questions ready
Start with a quiz
Answer from memory first, then use the existing quiz review flow for anything you miss.
Activities
Quiz18 Questions
Flashcards18 Cards
Study Notes1 Note
Podcast1 Episode
Modules
Learn in sequence
Start with the earlier modules and work forward. Each one builds on the last, so the course gets more advanced as you go.
Molecular Geometry: VSEPR Theory
Quiz • 18 Questions
Molecular Geometry: VSEPR Theory - Flashcards
Flashcards • 18 Cards
Study Notes
1 min • Summary
Molecular Geometry: VSEPR Theory - Podcast
Podcast
Materials
List of Questions18 questions
- Question 1
- 109.5°
- 90°
- 180°
- 120°
- Question 2
- NH3
- CH4
- BF3
- H2O
- Question 3
- 109.5°
- 90°
- 180°
- 120°
- Question 4
- CO2
- CH4
- PCl5
- NH3
- Question 5
- 109.5°
- 180°
- 120°
- 90°
- Question 6
- Polar covalent bond
- Ionic bond
- Hydrogen bond
- Non-polar covalent bond
- Question 7
- Molecular shapes
- Bond angles
- Atomic masses
- Electron configurations
- Question 8
- To determine the mass of the molecule
- To visualize its shape and structure
- To analyze its reactivity
- To calculate its boiling point
- Question 9
- Solubility
- Reactivity
- Hybridization
- Polarity
- Question 10
- Density
- Boiling point
- Solubility
- Color
- Question 11
- Hund's Rule
- Bohr's Theory
- VBT (Valence Bond Theory)
- Aufbau Principle
- Question 12
- It changes its color
- It determines its molar mass
- It impacts its reactivity
- It affects its crystal lattice structure
- Question 13
- Hydrogen bonding
- Dipole-dipole forces
- Instantaneous dipoles induced by moving electrons
- Polarizability of the substance
- Question 14
- Hydrogen bonding
- Covalent bonding
- London dispersion forces
- Dipole-dipole forces
- Question 15
- Viscosity
- Polarizability
- Boiling point
- Surface tension
- Question 16
- Caused by dipole-dipole forces
- Resulting from covalent bonding
- Because of hydrogen bonding
- Due to high viscosity
- Question 17
- Hydrogen bonding
- Dipole-dipole forces
- London dispersion forces
- Ionic bonding
- Question 18
- Homogeneous composite
- Crystalline composite
- Amorphous composite
- Heterogeneous composite
List of Flashcards18 flashcards
- Card 1HintThink straight line.Memory TipLinear = 180
- Card 2HintThink of a flat triangle.Memory TipBF3 is flat
- Card 3HintImagine a pyramid with four sides.Memory TipTetra = 4, 109.5
- Card 4HintThink of a pyramid with a triangular base.Memory TipNH3 has a pyramid shape
- Card 5HintThink of a square with two more points above and below it.Memory TipOcta = 8, 90 degrees
- Card 6HintThink balanced electron sharing.Memory TipEqual sharing
- Card 7HintIt's about how atoms arrange themselves.Memory TipShape prediction
- Card 8HintSee the molecule's arrangement in spaceMemory TipSee it in 3D
- Card 9HintBond angles affect how atoms bond.Memory TipAngle = Hybridization
- Card 10HintPolar or non-polar affects how it dissolvesMemory TipPolar dissolves polar
- Card 11HintLinks hybridization to shapesMemory TipVBT and shapes
- Card 12HintPolarity impacts how atoms arrange.Memory TipPolarity = lattice structure
- Card 13HintMoving electrons create temporary polesMemory TipElectron movement=dipoles
- Card 14HintStrong attraction between moleculesMemory TipStrongest bond
- Card 15HintLarger atoms are more easily polarizedMemory TipSize = Polarizability
- Card 16HintAttraction between water moleculesMemory TipWater's pull
- Card 17HintAttraction at the surfaceMemory TipSurface Hydrogen
- Card 18HintDifferent materials mixed, but not combinedMemory TipSeparate materials