Define dipole-dipole
Polar bond and asymmetrical
How do you know if something is polar?
- lone pair on central atom
- different terminal atoms
Define metallic solid
Metal atoms
What are the main properties of metallic solids?
- Malleable/ductile
- Wide range of boiling/melting points
- Good conductors
What are the properties of metallic solids?
- metal atoms
- wide range of boiling/melting points
- good conductors
- malleable/ductile
- metallic bonds
What are the properties of molecular solids?
- dipole-dipole and H bonds
- do not conduct electricity
- variable hardness but mostly soft
- low to moderate boiling point
What are the properties of ionic solids?
- Cation and anion
- Ionic bonds
- High to very high melting points
- Hard
- As a solid = does not conduct electricity
- As a liquid = conducts electricity
What are the properties of covalent network solids?
- covalent bonds
- highest boiling point
- very hard
- conducts electricity
What are the four network covalent solids?
SiO2
SiC
C(diamond)
C(graphite)
When do yours 8.314 for R versus .08206
Always use the 8.314J unless it’s gas laws or osmotic pressure
Determine the coordination number, edge length equation, and how many atoms per cell for a simple cubic unit cell
Simple
- 1 atom per cell
- Coordination number = 6
- Edge length = 2r
Determine the coordination number, edge length equation, and how many atoms per cell for a body-centered cubic unit cell
Body-centered
- 2 atoms per cell
- Coordination number = 8
- Edge length = 4r / sq rt 3
Determine the coordination number, edge length equation, and how many atoms per cell for a face-centered cubic unit cell
Face- centered cubic cell
- 4 atoms per cell
- Coordination number = 12
- Edge length = 4r / sq rt 2
Describe the kinetic molecular thoery
At a given temperature molecules in the gas phase have more energy than molecules in the liquid phase
Define fusion
Fusion = melting
solid –> liquid
What two things do you look for to determine largest lattice energy?
High charge and small size
Ionic size ______ across a period and _____ down a group
decreases across a period, increases down a group
When given a graph, how do you know where the normal boiling point is
Find 1 atm
Phase changes exhibit a change in ____ energy while states of matter exhibit changes in ____ energy
phase change = potential energy
states of matter = kinetic energy
Temperature changes reflect ____ energy changes while ____ energy is from forming or breaking IMFs
kinetic, potential
What does normal boiling point mean for temperature?
100 degrees celcius
373.15 degrees Kelvin
Vapor pressure is _____ affected by changes in volume
NOT
What is the relationship between temperature and phase transitions?
There is no change in temperature during phase transitions (hence the straight line on the graphs)
What are the five things to know about polarizability?
- bigger atoms = more polarizable
- more electrons = more polarizable
- stronger LDF= more polarizable
- lower electronegativity = more polarizable
- anions are more polarizable than cations
