| Definition | ||
| #1 | What is the energy required to increase the surface area of a liquid by a unit amount? |
Surface Tension |
| #2 | What are the attractive forces between the positive end of one polar molecule and the negative end of another polar molecule |
Dipole-Dipole Forces |
| #3 | What is superconductivity? |
Frictionless flow of electrons through a substance. |
| #4 | The process by which solvent molecules surround and interact with solute ions or molecules is called... |
Solvation. |
| #5 | What is the degree of randomess or disorder in a system given by a thermodynamic quantity? |
Entropy |
| Tables, Graphs, Pictures | ||
| #1 |
Is this a Polar or a Non-Polar Bond? |
It is very polar. |
| #2 |
What kind of bonding is present here. |
Hydrogen bonding or London dispersion forces . |
| #3 |
|
Polymers |
| #4 |
Which one is more polar? |
C5H11OH |
| #5 | What is this structure? |
Vitamin A! |
| Equations | ||
| #1 | Write a chemical equation that represents the formation of polychloroprene from chloroprene. |
CH2=CClCH=CH2 --> -[-CH2CCl=CHCH2-]-n |
| #2 | Write a chemical equation that represents the formation of polyacrylonitrile from acryonitrile1 |
CH2=CHC*N --> -[-CH2CH(C*N)-]-n |
| #3 | Write a chemical equation for formation of a polymer via a condensation reaction from the monomers succinic acid (HOOCCH2CH2COOH) and ethylenediamine (H2NCH2CH2NH2) |
|
| #4 | ||
| #5 | ||
| Comparison | ||
| #1 | Which member of the following pairs has the stronger intermolecular dispersion force:
Br2 or O2 |
Br2 |
| #2 | Which member of the following pairs has the larger London dispersion forces:
H2O or H2S |
H2S |
| #3 | What is the difference between a monomer and a polymer? |
A monomer is a single structure and has low moleculer weight, while a polymer consists of several monomers and appears like plastic such as shellac and varnish. A polymer has higher molecular weight. |
| #4 | List the three states of matter in order of increasing molecular disorder and increasing intermolecular attractions. |
The solid state has the least amount of disorder, the liquid state is intermediate between the solid and gaseous state, the gas state is the most disordered. The intermolecular forces are the strongest in the solid, intermediate in the liquid phase, and weakest in the gas phase. |
| #5 | For each of the follwing pairs of semiconductors, which one will have the larger band gap: A) CdS or CdTe B) GaN or InP C) GaAs or InAs |
A)CdS B)GaN C)GaAs |
| Calculations | ||
| #1 | Calculate the mass percentage of Na2SO4 in a solution containing 10.6 g Na2SO4 in 483 g water. |
2.15% Na2SO4 by mass |
| #2 | Calculate the molarity of each of the follwing solutions: A)8.66 g benzene (C6H6) dissolved in 23.6 g carbon tetrachloride (CCl4) B) 4.80 g NaCl dissolved in 0.350 L of water |
A) 4.70 M C6H6 B)0.235 M NaCl |
| #3 | You are given 12.0 g of ice at -5.00 °C. How much energy is needed to melt the ice completely to water? q = (mass) (Δt) (Cp)
q = (moles of water) (ΔHvap) |
q = (12.0 g) (5.0 °C) (2.06 J g¯1 °C¯1) q = 123.6 J = 0.1236 kJ + q = (12.0 g) (5.0 °C) (2.06 J g¯1 °C¯1) q = 123.6 J = 0.1236 kJ = 4.14 kJ |
| #4 | For many years drinking water has been cooled in hot climates by evaporating it from the surfaces of canvas bags or porous clay pots. How many grams of water can be cooled from 35 C to 20 C by the evaporation of 60 g of water? (The heat of vaporization of water in this temperature range is 2.4 kJ/g. The specific heat of water is 4.18 J/g-K.)
q = (mass) (Δt) (Cp) q = (moles of water) (ΔHvap) |
2.3*10^3 g H2O |
| #5 | Ethanol (C2H5OH) melts at -144 C and boils at 78 C. Its density is 0.789 g/mL. The enthalpy of fusion of ethanol is 5.02 kJ/mol. The specific heats of solid and liquid ehtanol are 0.97 J/g-K and 2.3 J/g-K, respectively. A)How much ethanol is required to to convert 25.0 g of ethanol at 25 C to the vapor phase at 78 C? B) How much heat is required to convert 5.00 L of ethanol at -140 C to the vapor phase at 78 C? |
A) 24.0 kJ B) 5.57*10^3 kJ |
| Final Question | |
What are these structures representing?