6 - Shapes of Molecules and Intermolecular Forces
Cards (49)
- What does electron pair repulsion theory explain?
- Why do electron pairs repel one another?
- What determines the shape of a molecule or ion?
- How are electron pairs arranged in a molecule?
- What is the result of minimizing electron pair repulsion?
- What shape does methane (CH4) have?
- How many C-H covalent bonds does methane have?
- What is the bond angle in methane?
- How are 3D shapes represented in molecular diagrams?
- What is a lone pair of electrons?
- How does a lone pair affect molecular shape?
- What shape do CH4, NH3, and H2O have?
- How does the presence of lone pairs affect bonding angles?
- How are multiple bonds treated in electron pair repulsion theory?
- What shape does CO2 have?
- What happens to bond angles with more electron pairs?
- What shape do three bonding pairs (e.g., BF3) have?
- What is the bond angle in an octahedral shape?
- What shape do six electron pairs give?
- How many bonded pairs does ammonia have?
- What shape do carbonate and nitrate ions have?
- What is electronegativity?
- What does the Pauling scale measure?
- Which element is the most electronegative?
- What indicates an ionic bond based on electronegativity difference?
- What characterizes non-polar bonds?
- What is a dipole in a polar covalent bond?
- How do polar molecules behave with dipoles?
- Why is water considered a polar molecule?
- How does carbon dioxide behave as a molecule?
- How does water dissolve sodium chloride?
- What are intermolecular forces?
- What are the types of intermolecular forces?
- What is the strength range of London forces?
- What is the strength range of hydrogen bonds?
- What happens to induced dipoles in London forces?
- How does the number of electrons affect London forces?
- What are simple molecular substances?
- What state do simple molecular substances exist in?
- Why do simple molecular substances have low melting and boiling points?
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