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Discussed Points
Term 1
Chapter 4
Chapter 5
Chapter 6
| 189 | Condensed phases of matter are solid and liquid. |
| 190 | Gaseous elements (under room conditions) are found at the top right hand side of the Periodic Table. |
| 191 | One gram of steam, H2O (g) causes more severe burns than one gram of water, H2O(l) at 100oC. At the same temperature, both have the same average kinetic energy but steam has a higher potential energy than water. |
| 192 | A volatile liquid is a liquid that evaporates at room temperature. A liquid with a low boiling point is easy to vaporize |
| 193 | Vapor pressure of a liquid: is the pressure of the gas above the liquid with which it is at equilibrium (Both liquid and gas exist indefinitely). |
| 194 | Vapor pressure of a liquid in a sealed container depends on temperature of the flask. As the temperature increases the vapor pressure of a liquid increases. |
| 195 | At the boiling point, the temperature of a pure substance stays constant as the liquid is being heated until all the liquid changes into gas. The heat given to the liquid causes more liquid to change into gas. |
| 196 | Molar heat of vaporization is the minimum energy required to change one mole of a substance from liquid to gas at the same temperature. |
| 197 | General equation for Molar heat of vaporization: X (l) + heat ⇌ X (g) |
| 198 | General equation for Molar heat of condensation: X (g) ⇌ X (l) + heat |
| 199 | In general, a substance that has a higher boiling point is expected to have a higher molar heat of vaporization. |
| 200 | Minimum conditions for liquid molecules to vaporize: |
| 1) Molecules are supposed to be on the surface. | |
| 2) Molecules are supposed to have an average kinetic energy greater than the energy keeping the molecules in the liquid state. | |
| 201 | Boiling point: is the temperature at which the liquid vaporizes anywhere in the solution. |
| 202 | At the boiling point: |
| a. Vapor pressure is equal to the surrounding pressure. | |
| b. Bubbles of vapor can form anywhere within the liquid. | |
| c. Molecules escape from the surface of the liquid to enter the gas phase as vapor (this also happens at room temperature). | |
| d. With increasing altitude, atmospheric pressure decreases and so does boiling point. | |
| 203 | Normal boiling point: is the temperature at which the vapor pressure is exactly 1 atm or 760 mmHg. |
| 204 | Molar heat of fusion: is the energy required to change one mole of a substance from solid to liquid at the same temperature and constant pressure |
| 205 | Molar heat of fusion is less than the molar heat of vaporization. Molar heat of vaporization of water is 7 times molar heat of fusion of water. |
| 206 | In general, a pure substance that has a high melting point is expected to have a high molar heat of fusion. |
| 207 | Comparison between the energy of the molecules on the three states of matter. |
| Highest PE in gases and lowest PE in solids. The PE of liquid is less than in gases and more than in solids. |
Term 2
| 253 | SELF STUDY: the electric model of atoms, direction of electric current, meaning of fundamental property, effect of distance on electric force | SQ 47 – 50 |
| 254 | Conductor: a material that completes an electric circuit | |
| 255 | Electric current: is the movement of electric charge. | SQ 52 |
| 256 | Electrolyte: a substance that dissolves in water producing electrically conducting solutions, example: aqueous solution of sodium chloride. | |
| 257 | DEMONSTRATION for conductors and non-conductors | SQ51 |
| 258 | Non-electrolyte: a substance that dissolves in water producing electrically non-conducting solutions, example aqueous solution of sugar and distilled water. Water itself is a bad conductor of electricity. When small quantities of a certain substance are dissolved in water, water becomes a good conductor of electricity. | |
| 259 | Examples of electrolytes: | |
| · All acids are electrolytes e.g acetic acid CH3COOH, sulphuric acid H2SO4... | ||
| · All ionic compounds are electrolytes e.g NaCl, CaCl2, MgBr2.... | ||
| 260 | Brief introduction to section 6.6.3 | |
| 261 | Ions: are charged particles( charged atoms or groups of atoms) | SQ54 |
| 262 | Cations: positively charged ions (usually metal ions eg Na+, Ca2+..) | SQ65 |
| 263 | Anions: negatively charged ions ( non-metal ions, eg Cl-, CO32-) | SQ64 |
| 264 | Ionic compounds: are compounds in which oppositely charged ions are held together strongly by an electrostatic force of attraction. They are formed from the reaction between a metal and a non-metal. Examples of ioninc compounds are sodium chloride (table salt), NaCl, calcium chloride, CaCl2, and silver nitrate, AgNO3. | |
| 265 | Sodium chloride NaCl is made from the combination of sodium ions Na+ and chloride ions Cl- in a ratio of 1:1. When one mole of sodium chloride dissolves in water it provides the solution with two moles of ions( 1mole of sodium ions and 1 mole of chloride ions) as per the equation: NaCl(s) →Na+(aq)+Cl-(aq) | SQ53 |
| 266 | Calcium chloride is made from the combination of calcium ions Ca2+ and chloride ions Cl- in a ratio of 1:2. When one mole of calcium chloride dissolves in water it provides the solution with three moles of ions( 1mole of calcium ions and 2 moles of chloride ions) as per the equation: CaCl2(s) → Ca2+(aq) + 2Cl–(aq). | SQ56 |
| 267 | Silver nitrate AgNO3 is made from the combination of silver ions Ag+ and nitrate ions NO3- in a ratio of 1:1. When one mole of silver nitrate dissolves in water it provides the solution with two moles of ions( 1mole of silver ions and 1 mole of nitrate ions) as per the equation: AgNO3 (s) → Ag+(aq) + NO3-(aq) | SQ57 |
| 268 | Sodium chloride and all other ionic compounds are electrolytes because they provide the solution with freely moving ions which can carry electric charge | |
| 269 | An electric current flows when we have a complete circuit. Current flows outside the battery from the positive terminal to the negative terminal. If an ionic solution is connected to a battery, all positive ions move in the direction of the current, away from the positive electrode and towards the negative electrode. All negative ions move in a direction opposite to the current, away from the negative electrode and towards the positive electrode. | SQ55 |
| 270 | Not all ionic compounds are soluble in water and ionize completely in it. Examples include: calcium carbonate, silver chloride, silver bromide, silver iodide and barium sulphate. | SQ58 |
| 271 | Memorize name and formulae of cations and anions listed p. 47 part2 textbook. | SQ66 |
| 272 | Naming ionic compounds: cation is always named first followed by the anion | BQ9, SQ67 |
| 273 | Writing the formulae of ionic compounds | BQ10 |
| 274 | Properties of an ionic solid: ionic solids have high mpt and bpt, do not conduct electricity when solid, conduct electricity when molten or aqueous. Ionic solids form clear crystals | SQ63 |
| 275 | Write dissociation reactions of ionic compounds in water. The equations must be balanced for atoms and for charge | SQ61 |
| 276 | Precipitate: is solid formed when mixing two aqueous solutions. | |
| 277 | Precipitation reaction: is a reaction where a precipitate (solid) is formed. | SQ59 |
| 278 | Demonstration: Different precipitation reactions: | |
| 279 | Write a complete formula equation, a complete ionic equation, a net-ionic equation to represent a precipitation reaction. | BQ 8 |
| 280 | Predominant ions: is that take part in the reaction | |
| 281 | Spectator ions: ions that do not take part in a reaction | SQ60 |
| 282 | Molecular solids are made up of molecules. Examples of molecular solids are wax, sugar, hydrogen chloride, ammonia ... | |
| 283 | Discuss properties of molecular solids: | SQ62 |
| 284 | Other types of solids: metallic solids and network solids | |
| 285 | Metallic solids: e.g Cu, Ag, Na | |
| 286 | Network solids / giant molecular/ giant covalent solids are atomic solids made up of atoms joined together by strong covalent bonds. Network solids are characterized by their high melting point and boiling point. e.g Sand (SiO2) , graphite (C) and diamond(C) | SQ68 |
| 287 | Determine [ions] present given number of moles of salt and volume of solution. | BQ11, 12, CR25 |
| 288 | Determine the concentration of each ion present in a solution prepared by mixing two other solutions without precipitate formation | BQ12, CT 23 |
| 289 | Determine the concentration of each ion present in a solution prepared by mixing two other solutions resulting in the formation of a precipitate. Calculate the mass of precipitate formed | BQ13 |
Pending Points
Term 2
Term 3
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