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Liquids and Solids How do the strengths of the intermolecular attraction compare btw solids, liquids, and gases at room temperature? What is the difference btw intermolecular bonds and intramolecular bonds? Explain how dispersion forces form. Explain how dipole-dipole and hydrogen bonds form How does viscosity change with increasing and decreasing temperature? Why is boiling a cooling process How does pressure effect the boiling point of a substance?
How do intermolecular bonds effect the boiling point of a substance? Calculate the following Molarity prob: Make sure you know how to prepare the solutions. Calculate the molarity of a solution prepared by dissolving 95. 5 grams of KNO 3 in enough water to make a 0. 75 L solution. How many grams of chlorine are needed to prepare a 0. 50 liters of a 0. 100 M solution of chlorine dissolved in water? How do you make 2. 5 L of HCl with a concentration of 3. 0 M from a 12. 0 M solution? How many ml of an 18. 0 M solution of sulfuric acid would you use to make 3. 8 L of a 4. 0 M solution?
According to Le Chateliers Principle, predict the direction the reaction will shift 2 NO (g) = 2 H 2 (g) N 2 (g) = 2 H 2 O (l) (a) NO is added (b) water is removed (c) nitrogen gas is removed (d) nitrogen gas is added 4 HCl (g) = O 2 (g) 2 H 2 O (g) = 2 Cl 2 (g) (a) oxygen is added (b) hydrochloric acid is removed (c) chlorine gas is added (d) water is added If the reaction shifts to the right, will the products of the reactants increase in concentration? If the reaction shifts to the left, will the products of reactants increase in concentration? Write a balanced equation showing the following dissolved in water Sr (NO 3) 2 CaCl 2 What would happen if you added calcium phosphate to the following equation? Sr 3 (PO 4) 2 3 Sr 2 + + 2 PO 43 - Solutions and Equilibrium What are ion-dipole attractions and how are they involved in the process of solvation What does crystallization or precipitation mean? What is a supersaturated solution? How is this kind of solution made?
What happens to the boiling point and freezing point of water when salt is added? How can you increase the rate at which a solute dissolves in a solvent? What kinds of compounds are electrolytes and why What two processes are equal when solubility equilibrium is reached? Carbon tetrachloride and water are immiscible in each other. Explain How does temp effect the solubility of a gas and solid Why do cities add salt to the roads in the winter? When is a reaction at chemical equilibrium?
Chapter 15 Properties of Solutions Solute Solvent Example Soluble Insoluble Example How can you tell which subs is the solute and which is the solvent Types of Solutions Solid Solutions Alloys = How are alloys formed? Gaseous Solutions Liquid Solutions Miscible Immiscible: Example Aqueous Solutions Aqueous solution = water as solvent Electrolyte = substance that dissolves in water to form solution that conduct electricity EX Why do electrolytes conduct electricity? Ionic compound Non -electrolyte = substance dissolve in water doe not conduct electricity Concentration of Solutions A concentrated solution contains: Large amt. of solution to amt.
of solvent Ex punch syrup sugar to water Dilute solution = small amt. Concentration of a solution is amt. of solution to amt. of solvent Molarity (M) Most common expression of solution concentration Number of moles to solvent dissolve in e? of solvent molarity = moles of solvent L of solution? A volumetric flask is used to make solution of a precise molarity?
Practice problem Vinegar is a solution of acetic acid. What is the molarity of the solution produced when 125 g of acetic acid (C 2 H 4 O 2) is dissolved in sufficient water to prepare 1. 5 L of solution? 1. 3 grams How many grams of bromine are needed to prepare 0. 500 L of a 0. 0100 M solution of bromine in water? . 79 grams Try to figure these out on your own molarity V = volume (liters) If you have a 12 M solution of HCl how many liters of it should you use if you want to make 2 liters solution of HCl with a molarity of 3 M? You want to make a 7. 5 -L solution of 4 M sulfuric acid. You have 6 M solution available. What would you do? Freezing Point Depression = colligating property which describe the ability of a solute to lower t Ex slt Why does it help to add salt to water cooking = increased the boiling point On cold winter days unprotected radiator water can freeze and expand which can ruin the engine by cracking the engine block.
Which antifreeze mixture would you want in your engine of a cold winter day? One with the lowest freezing point. Chemical equilibrium The concept of equilibrium What is equilibria? 2 opposing processes take place at the same time Reversible reactions products aft Are all reactions reversible ex? Yes some cant do it on their own or havent been dis What is the standard convention with a reversible reaction? Chemical Equlibria = the rate at which the What do chemist use to dente the concentration of a substance It is important to recognize that reaching equilibrium does not mean that Chemical equilibria is a constant or changing process Le Chateliers Principle = Changes in Concentration If more of a particular substance is added to a reaction at equilibrium, the reaction will return to equal by... Consuming same of the added subs If a substance was removed, the reaction will return to email by...
Producing more of the subst that was removed Practice Problems Predict the direction of the shift in email if: As 4 O 6 + 6 C As 4 + 6 CO CO is added left As 4 is removed right Which change will increase the production of water vapor in this reaction? SO 2 a adding SO 2 b removing H 2 S c removing O 2 d removing SO 2 Chap 17 Solubility and Precipitation Dissolution and Precipitation Just as you did with chemical reactions, you can write an equation to show the dissolution (dissolving) os... An ionic solid place in water Write an equation showing the dissolving of Na Cl in water? ... NaCl (s) D Na (aq) + Cl (aq) Write a balanced equation showing the dissolving of Ba Cl 2 in water...
Ba Cl 2 D Ba 2 (aq) = Cl 2 - (aq) Write a balance equation showing the Fe (OH) 3? ? ? Precipitate = the process in which ions have a solution Solubility equilibrium = The common ion effect = a shift in equilibrium that occurs Practice prob 17 - 3 p 580 Saturation Saturated solution = Chapter 14 Kinetic-molecular theory of matter explains the physical properties of liquids and solids. (According to the kinetic-molecular theory, the state of a substance at room temp depends on the strength of the attractions between its particles. ) Intramolecular forces: Covalent bonds exist within the molecule, holding the atoms together in a specific shape. Intermolecular forces include: Dispersion forces: Force of attraction between induced dipole. Temporary (- +). Present in all molecular substances.
Dipole-dipole forces: Some molecules have a permanent (- +) charges. Hydrogen bonds: Stronger bonds (hydrogen, florine, oxygen, or nitrogen) Large particle results in a strong bond. Properties of Liquids Surface tension Viscosity The Nature of Solids Crystalline solid highly ordered, repeating pattern Example: Diamonds Amorphous solid without form (supercooled liquids) Examples: Glass, rubber, plastic Bonding in Solids Physical properties of a solid depend on the did of particles and the strength of attractive forces that hold them together. Types of bonds: Metallic metals Molecular organic compounds Ionic salts Covalent-network solid diamonds, graphite, silicon, quartz Changes of State To change state, must overcome bond. Vaporization change liquid to gas Condensation change gas to liquid Sublimation solid to gas (dry ice) Deposition gas to solid (snow, water vapor to solid) Chapter 16 Concept of Equilibrium Reversible reaction chemical reactions in which the products can reform the original reactants. 2 NO 2 (g) N 2 O 4 (g) Chemical equilibrium is reached when the rate of the forward reaction is equal to the rate of the reverse reaction.
The Law of Chemical Equilibrium Law of Mass Action ratio of concentrations of reactants and products of a reversible reaction in terms of the equilibrium constant (Equilibrium expression) Law of chemical equilibrium every reaction that reaches equilibrium has a specific equilibrium constant, which indicates the extent of the reaction. Equilibrium position relates to the equilibrium concentrations of the component of a reaction and depends upon the initial concentrations. Pure solids and liquids involved in heterogeneous equilibria do not appear in the equilibrium expression. Equilibrium constant. (do not change) Reaction quotient (Q) Used to determine if the reaction is at equilibrium. (Q = Key) Le Chanteliers Principal A system that is disturbed from equilibrium will shift in order to reduce the disturbance. Factors that disturb a system are change in concentration of reactants and / or products, changes in pressure or temperature. Harbor process industrial process ammonia, uses Le Chanteliers Principal to maximize production of ammonia.
Chapter 17 Solubility Equilibria When an ionic solid is placed in water, attractions between the polar water molecules and the ions of the solid cause the solid to dissociate. The ions spread throughout the solution during dissolution. At the same time the ions in the solution collide with the remaining ionic solid and become part of it during precipitation. Dissolution and Precipitation are reverse processes.
A solution attains solubility when dissolution and precipitation occur at the same rate. The ion concentration in solution are constant at equilibrium. Precipitate if the ion concentration is greater than the concentration at equilibrium (supersaturated) Common ion an ion contained in more than one solute in a solution. Common ion effect the solubility of an ionic solid added to a solution already containing a concentration of common ions is decreased.
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Research essay sample on 2 H 2 O Hydrogen Bonds
