H. CHEMISTRY
REVIEW – LIQUIDS AND SOLIDS, Unit 10
How liquids and solids differ from gases
1) Distances between particles
2) Attractive forces
Characteristics of liquids and solids - shape and volume
Heat of fusion, heat of vaporization
1) how they differ in the same substance, calculations with
Dynamic equilibrium
Equilibrium vapor pressure (vapor pressure)
- Effect of amount of liquid, volume of flask, nature of liquid, temperature on
vapor pressure
Relative humidity:
- Solve problems
Boiling
- When does a liquid boil?
- *Boiling point can change, depending on ________________
- Normal boiling point:
Intermolecular forces of attraction
1) Van der Waals – Dipole-dipole, dispersion forces
*Increase with increasing _____________________________
∴*Boiling point increases with increasing ________________________
2) Hydrogen bonds – Explain WHAT they are & WHEN they occur
*Result in high _________________________
Melting
Melting point
Phase change diagram
Identify MPt, BPt, area of (l), (s), (g), increasing KE, same KE, increasing PE
Entropy
*Processes tend to go to __________ entropy and _________energy
(enthalphy)
Energy(enthalphy) factors involved in a process occurring
Types of solids – KNOW CHART – Types of Solids
CONDUCTIVITY FOR ALL OF THE TYPES
Ionic: MPt, examples
Types and equations for how they decompose
Molecular: MPt, examples
Sublimation: examples
Water: D(ice) vs. D(liquid). Why?
Network solids
Macromolecules
MPt., examples
Graphite, diamond structures, buckyballs (fullerenes)
Metallic solids: MPt, examples, explain structure
Be able to use charts, diagrams
1. ***Finish Questions #17-23 and Problems 8,9,18,19,21 in packet as well as the
rest of this packet
2. Define each of the following terms clearly and completely.
(a) Van der Waals Forces(b) Hydrogen Bond(c) Dipole-dipole force(d) Dispersion force –
(e) Covalent- network solid –
(f) Ionic Solid –
(g) Molecular Solid –
(h) Metallic Solid -
(i) Sublimation –
(j) Vaporization –
(k) Condensation –
(l) Freezing –
(m) Melting –
(n) Heat of Fusion –
(o) Heat of Vaporization –
(p) KMT of Matter *hint why are liquids and solids different from gases? –
(q) Dynamic Equilibrium –
(r) Vapor Pressure –
(s) Boiling –
(t) Melting Point –
(u) Entropy –
(v) Enthalpy –
(w) Electron Sea Model –
(x) Relative Humidity –
3. Explain the following in one to three sentences.
(a) Zinc is a conductor but a diamond is an insulator.
(b) H2O has a higher boiling point than CO2.
(c) Which liquid, HCl or HF, has a higher boiling point?
4. For each of the solids listed, give
I.
the type of solid (ionic, molecular, metallic, or network)
II.
the bond or force that holds the solid together.
(a) NH3
(b) Ag
(c) SiC (Silicon Carbide)
(d) N2
(e) KBr
5. Which type are each of the solids described below?
(a) crystalline solid with slight odor that melts at 78◦C
(b) solid that conducts in the solid phase
(c) solid with a very high melting point that does not conduct
(d) solid that does not conduct but dissolves in water to make a conducting
solution.
Type of Solid
Ionic
Molecular
Polar/ Nonpolar
Metallic
Covalent Network
Examples
Conducts in
solid state
(yes or no)
Conducts in
liquid state
(yes or no)
Melting
point range