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Intermolecular Forces
Liquids
Solids
Solids Pt.2
Phase Diagrams
100
What is hydrogen bonding, and which elements bonded to hydrogen can have hydrogen bonding?
Hydrogen bonding is a special dipole-dipole attraction where the Hydrogen is more positive than the rest of the compound, creating a more polar molecule. NOF.
100
Define Capillary Action.
Cohesive forces between liquid molecules. Adhesive forces between polar liquid molecules and polar bonds in the material making up the container.
100
Imagine a solid material that consists of a lattice of two different metals: A and Z. The material is an array of A atoms with Z atoms located in the spaces between. This should be classified as a...
Interstitial alloy
100
What differentiates a semiconductor from other metals? (Bonus 500 for example)
Semiconductor has better electrical conductivity as temperature increases, which is the opposite for other metals. (Silicon)
100
True or False: Volatile liquids have weak intermolecular forces.
True
200
What is the strongest form of intermolecular force? What is the weakest?
Hydrogen Bonding. London Dispersion Forces.
200
Name the term: The resistance of a liquid to an increase in surface area.
Surface Tension
200
Do molecular solids have low or high melting points?
High 
200
How do N-Type Semiconductors work?

N-type semiconductors are substances whose conductivity is increased by doping with atoms having more valence electrons than the host crystal

200
What is the critical point of a substance?

The critical temperature is the temperature above which a vapor cannot be liquefied. The critical pressure is the pressure required to liquefy at the critical temperature. The critical point is the critical temperature and pressure of a substance

300
Does CCl4 or CH4 have more london dispersion forces? Why?
CCl4 has more. "Polarizability" increases with the number of electrons in a molecule.
300
Why is there a concave meniscus for water? What is a situation where the meniscus could be convex?
Adhesive forces are greater than cohesive forces. If the opposite occurs.
300
What is the difference between a crystalline and amorphous solid?

Crystalline solids have a highly regular arrangement of their components. Amorphous solids have considerable disorder in their structures

300
Is a solid crystal of NaCl:

a. Soft or Hard?

b. High or low melting point?

c. Good or poor electrical conductor?

hard, high, poor.
300
What is the triple point of a substance?
Where it exists as a gas, liquid, and solid at the same time.
400
Are intermolecular forces or intramolecular forces stronger? Why?
Intramolecular. 
400
What occurs to viscosity of a liquid as intermolecular forces increase?
Increases.
400
What are the three types of crystalline solids?
Network atomic solids, ionic solids, molecular solids
400

Is CH4:

a. Soft or Hard?


b. High or low melting point?



Soft, low.
400
Spell Phase Diagram backwards.
M-A-R-G-A-I-D- -E-S-A-H-P
500
Order the following from strongest to weakest: Dipole-Dipole; Ionic; London Dispersion Forces; Hydrogen Bond; Covalent.

London Dispersion Forces; Dipole-Dipole; Hydrogen Bond; Covalent; Ionic

500
What is viscosity a measure of?
Resistance to flow
500
What is the difference between a substitutional and interstitial alloy? (Bonus 1000 for examples of each)
Substitutional alloys have some atoms replaced. (Brass = Copper + Zinc). Interstitial alloys have atoms in the spaces between other atoms. (Steel = iron + carbon)
500
What the hell is a p-type semiconductor?

P-type semiconductors are substances whose conductivity is increased by doping with atoms having fewer valence electrons than the host crystal

500
Name three differences between vaporization and boiling.
Vaporization (slow, no bubbles, only surface, any temperature)

Boiling (fast, bubbly, throughout, boiling point)