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Solids and Liquids
Chapter 14
Intermolecular forces• Bonding forces that hold
atoms together within a molecule
Intramolecular forces• The forces that occur
among molecules that cause them to aggregate to form a solid or a liquid
Intermolecular forces
• Dipole-dipole attraction- molecules with dipole moments can attract each other by lining up so that the positive and the negative ends are close to each other.
• Hydrogen bonding- hydrogen is bound to two highly electronegative atoms, such as nitrogen, oxygen or fluorine.
• London dispersion forces- the forces that exist among noble gas atoms and nonpolar molecules
Solutions
Chapter 15
Soluble vs. Insoluble
Solubility (or Soluble)• Something that is capable
of being dissolved in a solvent
Insolubility (or insoluble)• Incapable of being dissolved
within a given solution
Solubility Rules
Examples
• State which of the following compounds are soluble and which are not– KBr = – PbCO3 =
– BSO3 =– zinc hydroxide =
– KBr = Soluble– PbCO3 = Insoluble
– BSO3 =Insoluble– zinc hydroxide = Insoluble
Types of solutions• Solution-a homogeneous mixture• Solvent-the largest substance that is present within the solution• Solutes-the smallest substance within the solution• Aqueous solution-solutions with water as a solvent• Saturated-a solution that contains as much solute as will dissolve at
the temperature• Unsaturated- a solution that has not reached the limit of solute that
will dissolve• Concentrated-a large amount of solute dissolved• Dilute-a relatively small amount of solute is dissolved• Supersaturated- a solution that contains more dissolved material
than could be dissolved by the solvent under normal circumstances
Molarity vs Molality
Molarity• (M)• Describes the amount of
solute in moles and the volume of the solution in liters.
• The number of moles of solute per volume of solution in Liters
• Moles of Solute = mol Liters of Solution L
Molality• The amount of substance of
solute, divided by the mass of solvent.
• The number of moles of solute divided by the number of kilograms of solvent
• Moles of solute = mol Kg of Solution kg
Example of calculating Molarity
• Calculate the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in enough water to make 1.50L of solution.
• Step 1: calculate the number of moles in NaOH– 11.5g x 1mol = 0.288moles
40 g• Step 2: divide number of moles by the number of
Liters– 0.288moles = 0.192M
1.50 L
Example of calculating Molality
• What is the molality of a solution made from 2.4 moles of NaCl and 0.80 kg of water?
• Divide number of moles by the number of kilograms:– 2.4 moles = 3.0m
0.80 kg
Net Ionic Equation
• Ionic equations are used to describe the chemical reaction while also clearly indicating which of the reactants and products exist primariy as ions in aqueous solutions.
Rules for writing net ionic equations
1. Start with a balanced molecular equation (meaning: an equation that shows the chemical formulas of all reactants and products, but not their physical states)
2. Break all soluble strong electrolytes (compounds with (aq) beside them into their ions
* indicate the correct formula and charge of each ion * indicate the correct number of each ion* write (aq) after each ion
3. Bring down all compounds with (s), (l), or (g) uncharged
For example
Use the following equations to answer the question:2Na3PO4(aq) + 3CaCl2(aq) 6NaCl(aq) + Ca3(PO4)2(s)
Net ionic equation:6Na+ (aq) + 2PO4
-3(aq) + 3Ca+2(aq) + 6Cl-(aq) 6Na+(aq) +6Cl-(aq) + Ca3(PO4)2(s)