1. SOLIDS

2. Changes Build the foldable into the notes
Have them draw the picture after you give the notes
Have them do the practice by writing the formulas under the picture as examples

3. What you need to be able to do: given any one, figure out the rest
Formula
Properties – predict and explain
Particle view

4. Properties of Solids
Melting point – T at which a substance changes from a solid to a liquid
Vapor pressure – definition on next slide
Conducts heat or insulator
Conducts electricity
Brittle – force applied causes it to shatter
Hard – resists changes in shape
Malleable/Ductile – can change shapes without breaking

5. Vapor Pressure
the pressure of the vapor resulting from evaporation of a liquid (or solid) above a sample of the liquid (or solid) in a closed container

6. Make your foldable Ionic Molecular Metallic Network
Draw a picture representation for each of the 4 types of solids
Ionic
Molecular
Metallic
Network

7. 4 Types of Solids – write these as examples on the ‘door’ of your foldable
Ionic
NaCl
CuSO4
Metallic
Atomic (Na or Fe)
Alloys (Bronze=Cu+Sn)
Molecular
Most nonmetals (helium, sulfur)
Most covalent compounds (P4O10, NH3, CO2)
Network - rare
Atomic = Carbon and Silicon
Molecular = SiO2 and SiC

8. Ionic Solids 11.6 Lattice points occupied by cations and anions
Held together by electrostatic attractions (an intramolecular force)
Hard, high melting point, brittle
Poor conductor of heat and electricity in SOLID state (although ionic compounds do conduct in LIQUID state or when dissolved in water  can help with identification)
CsCl
ZnS
CaF2
11.6

9. Strength of ionic bonds
Use Coulomb’s Law!
Smaller ions (little r)
Larger charges (big q)
They’ll usually only ask about one at a time
Example: LiF vs NaCl
Example: LiF vs BeO

10. Metallic
Lattice points occupied by metal atoms (could be 1 type or 2)
Held together by metallic bonds (nondirectional covalent bonds; share electrons with everyone; sea of electrons)
Wide range of hardnesses/melting points
Good conductor of heat and electricity due to delocalized/free electrons
Shiny
Malleable/Ductile – doesn’t change the environement immediately surrounding the metal core
Readily alloyed
2 diff metals
nucleus &
inner shell e-
mobile “sea”
of e-
11.6

11. Molecular Solids
Lattice points occupied by nonmetals, diatomic molecules, covalent molecules, and polymers
Held together by intermolecular forces (much weaker than intramolecular forces)
Soft, low melting point (because held together by weaker intermolecular forces)
Poor conductor of heat and electricity because electrons are trapped in covalent bonds
11.6

12. Network Solids carbon atoms 11.6
Lattice points occupied by atoms (usually carbon/silicon or silicon dioxide and silicon carbide)
Held together by directional covalent bonds (an intramolecular force that is very strong)
Hard, high melting point
Poor conductor of heat and electricity (insulator) – electrons are trapped in covalent bonds
carbon
atoms
graphite
diamond
11.6

13. Practice - Identify the type of solid each substance would form
CaO Cu He
SiO2
CO2 Zn
SrCl2
Brass
Ionic
Metallic
Molecular
Network
Which would have the highest melting point? Narrow it down to one or two…. Ionic and Network will always be the highest. In this case CaO is 4662°F while SiO2 is 2912°F. Which do you think would be third? SrCl2 (~1600°F)

14. Add these properties to the correct solid; include terms like high/low or good/bad if appropriate
Melting point
Vapor pressure
Conducts heat
Conducts electricity
Brittle
Hard or soft
Malleable/Ductile

15. IONIC High melting point* Low vapor pressure*
Do not conduct heat (insulator)
Do not conduct electricity*
Brittle*
Hard
Not malleable or ductile

16. Metallic Low vapor pressure Good conductor of heat/electricity*
Malleable/Ductile*

17. Molecular Low melting point* High vapor pressure Do not conduct heat
Do not conduct electricity*
Not hard (they’re soft)
Not malleable/Ductile

18. Network High melting point* Low vapor pressure
Do not conduct heat (they’re insulators)
Some conduct electricity (Si gets more conductive with increased temperatures)
Hard*
Not malleable or Ductile

19. Explain the following properties
Ionic
High melting point*
Low vapor pressure*
Nonconductors of electricity*
Brittle*
Metallic
Good conductor of heat/electricity*
Malleable/Ductile*
Molecular
Low melting point*
Do not conduct electricity*
Network
High melting point*
Hard*

20. IONIC High melting point Low vapor pressure*
Held together by strong coulombic forces / intramolecular force
Low vapor pressure*
Do not conduct electricity*
Electrons are trapped onto atoms (to form ions with full octet)
Brittle*
Repulsion of like charges when one layer slides across another

21. Metallic Good conductor of heat/electricity* Malleable/Ductile*
Electrons are delocalized and relatively free to move
Malleable/Ductile*
Deforming the solid doesn’t change the environment immediately surrounding each metal core

22. Molecular Low melting point* Do not conduct electricity*
Weak intermolecular forces hold them together
Do not conduct electricity*
Electrons are tightly held within covalent bonds of constituent molecules

23. Network High melting point* Hard* All atoms are covalently bonded
Covalent bond angles are fixed

24. Practice You may work this individually or with ONE partner
Go to socrative.com
Classroom: LOZANOE122
Your name should be your first and last name
Teams: use both last names
When you’re done: study your foldable and wait patiently

25. Paired Poster Review Get a cup question and tape it to your poster.
Answer it 
Repeat (a bunch of times….)
Help
6. Viscous means resistance to flow (honey is viscous, water is not)
Misnomer – named incorrectly
Omit 2b
5. One of those was in the lab, another I’ve written on a post-it by the cup

26. Practice! What type of solid am I?
CaO
I’m brittle and have a low melting point
Brass
Sulfur
I conduct heat and am malleable
I have intermolecular forces holding me together
I have intramolecular forces holding me together
Carbon– would I have a low or high melting point? Explain.
Potassium nitrate – would I be brittle or malleable? Explain.
In 3 words or less, explain why metals conduct electricity.

27. Answers! What type of solid am I?
ionic
Molecular
metallic
Metallic or ionic
Network – high melting point because you must break strong INTRAmolecular forces
Ionic – brittle, a force would cause a shift in the planes of ions, introducing repulsive forces
Sea of electrons