Chapter 10 Flashcards
Molecules in a gas have complete freedom of motion.
KE overcomes the attractive forces between molecules.
Molecules in a liquid have limited freedom of motion.
Have enough KE to overcome some of the forces.
Molecules in a solid have no freedom of motion.
Though they vibrate, they can’t overcome the forces.
How strong are gas IM forces?
Weak
How strong are liquid IM forces?
Moderate
How strong are solid IM forces?
Strong
One state of matter can be transformed into another
by changing the
temperature, pressure, or both.
When you change the temperature, you change the
kinetic energy of the particles
− When you change the pressure, you change the
strength of the attractions between the particles
Covalent bonds are held together by _________
forces. Are these strong or weak?
intramolecular, Strong
Intermolecular attractions exist
between molecules
Where do intermolecular attractions happen in molecules?
+ ion/end of polar molecule to - ion/end of polar molecule
Are inter or intra molecular forces stronger? Why?
Usually intra, greater distance=less force to break attractions
What determines Physical properties? EG boiling/melting points, vapor pressure, viscosity
Intermolecular forces
Stronger Intermolecular forces can be correlated to
Higher melting/boiling point
What are intermolecular forces also known as?
Van der Waals forces
What are the 3 types of attractions between neutral molecules?
Dipole-dipole, Hydrogen bonding, London Dispersion
What type of bonding involves ions?
Ion-dipole force
Can nonpolar atoms have dipole-dipole attraction? Can nonpolar gases be liquefied?
No, Yes
Who proposed London Dispersion forces?
Fritz London
How do London Dispersion forces happen? How does this affect other atoms?
E- can end up on the same side of atom (normally try to repel each other), creating temporary polarity, which influences its neighbors. + wants to bind to -
What are London Dispersion forces? Where are they found?
Attractions between an instantaneous
dipole and an induced dipole. All molecules, regardless of their polarity
What is the trend of molecular weight and dispersion forces?
As MW increases, dispersion forces increase.
Do long or short molecules have stronger London forces? Why
Longer, more surface area so they have more interactions
What molecules have dipole dipole forces? Why?
All polar molecules, because they have permanent dipole moments
What is a dipole?
A molecule with charged ends
What is a dipole dipole force?
Dipoles interacting via opposite end attraction
18 onward(Just highlighted stuff)
What is hydrogen bonding?
A type of dipole dipole force where H (H bond donor) is directly bonded to N, O, or F (H bond acceptor). This interacts with a lone pair of e- on an N, O, or F atom in another molecule.
What are ion dipole forces?
Solvent pulling the ions from an ionic substance from the crystal, solvating them
What does an anion dipole look like?
What does a cation dipole look like?
Ammonia and hydrogen fluoride both have unusually high boiling points due to _____
hydrogen bonding, because it causes have strong Intermolecular forces (which correlate to high boiling points)
Is hydrogen bonding inter or intra molecular?
Inter
What is Hydrogen bonding?
Strong intermolecular forces that happen between molecules with a very strong permanent dipole moment.
What are ion dipole forces, and how are they formed?
When an ionic substance dissolves in H2O, the solvent pulls ions and solvates (surrounds) them. Solvent has +/- charged ends, which are attracted to the ions.
