SOLIDS.

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Presentation transcript:

SOLIDS

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

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

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

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 http://www.chem.purdue.edu/gchelp/liquids/vpress.html

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

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

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

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

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

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

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

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)

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

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

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

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

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

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*

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

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

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

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

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

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

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.

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