CourseReview1-Nov.2020
.pdf
School
Georgetown High School**We aren't endorsed by this school
Course
SCIENCE 123
Subject
Chemistry
Date
Dec 18, 2024
Pages
6
Uploaded by JusticeCrocodile3663
SCH3U Nov 2020 Here are some tips for getting ready for the summative evaluation: 1.Review each unit one at a time by reading through your notes then trying the unit test again without looking at the correct answers until you have finished it. If you did not make corrections to your test when you first got it back now would be a good time. 2.Make a list of topics you need to work on and questions you need to get some help on. 3.Try the multiple choice questions from the tests again. 4.Complete the review below. Review for Summative Evaluation Atomic Theory and the Period Table You will need to: ✓Know the trends on the periodic table- ionization energy, atomic radius, electron affinity ✓Describe models of the atom: Rutherford, Bohr, Quantum Mechanical model ✓Write standard atomic notation, electron configurations✓Calculate average atomic mass1.The atomic radius of the elements _____________ as you go left to right across the periodic table. 2.The electron affinity of the elements ____________ as you go down a family. 3.The most reactive metals are found _______________________________________ on the periodic table. 4.The least reactive non-metals are found ____________________________________ on the periodic table. 5.Metals have low ____________________ ______________________ while non-metals have high ________________ ____________________. 6.Write the standard atomic notation for argon. 7.Write the electron configuration for chromium.
Bonding and NomenclatureYou will need to: ✓Draw Lewis diagrams for ionic, polyatomic ions and covalent substances ✓Draw structural diagrams and shapes for covalent substances and determine the polarity of the molecules ✓Name and write formulas for ionic and covalent substances 8.Draw Lewis diagrams for the following: a)aluminum sulfide b) PH3c)CCl4, d) C2H2e)SrCl2f) H2Se g)OH-h) C2H29.Draw structural diagrams for the following: a)CH3Cl b) Cl2O b)CO32-d) CO2e)HCN f) O210.Now draw and name the 3-D shape for #9. 11.Which of the above molecules is polar? 12.Name the following compounds: a)LiHCO3b) Sn(OH)2c)ICl3d) H3PO4(aq)d)HNO2(aq)f) NaClO3f)CaSO3h) KCN 13.Write formulas for the following: a)ammonium sulfate b) magnesium hydride b)diphosphorus pentasulphide d) hydrofluoric acid e)iron (III) sulfide f) hydrosulfuric acid
Types of Reactions You will need to ✓Identify types of chemical reactions, balance chemical equations, write ionic and net ionic equations, identify precipitates formed using the solubility chart, know how to use the activity series14.Write a balanced chemical equation for each of the following types of reactions: a)Synthesis b) decomposition c)single displacement with metals d) single displacement with non-metals f)double displacement with a precipitate formation g)Neutralization h) combustion 15.Write the ionic and net ionic equation for the reaction: Mg(s)+ H2SO4(aq)→MgSO4(aq)+ H2(g)16.What are spectator ions? 17.Will a precipitate form between a) sodium chloride and barium sulfate? b) barium chloride and sodium sulfate? c) calcium nitrate and sodium hydroxide? The Mole You will need to: ✓Make the following calculations: n→m, N→n, N→m ✓Determine percent composition of a compound ✓Determine empirical and molecular formulas ✓Give answers to the correct number of significant digits 18.Calculate the number of moles and the number of molecules in 150 g of water. 19.Calculate the mass of 2.43 moles of C2H2. 20.Calculate the number of atoms of each element present in 0.84 moles of CH4. 21.Which contains the greatest number of molecules: 252 g of sulfuric acid OR 300 g of carbonic acid?
22.Which represents the greatest amount of silver: 25 g OR 0.25 mol OR 2.0 x 1023atoms? 23.Calculate the percent by mass of carbon in lithium carbonate. 24.What mass of carbon is in 25 g of lithium carbonate? 25.A sample of a compound was analyzed and found to contain the following: Carbon: 66.6%; Hydrogen: 11.2%; Oxygen: 22.2%. Determine the empirical formula of the compound. The molar mass of the compound was found to be 144.21 g/mol. Determine the molecular mass of the compound. Stoichiometry and Solutions You will need to: ✓Using balanced equations: carry out calculations involving mole to mole, mass to mass, percent yield, limiting reactant ✓Determine concentration in mol/L using the formulas c=n/v and c1V1=c2V2✓Solve stoichiometric problems using solutions and gases ✓Know the properties of acids and bases ✓Determine pH, pOH, [H+] and [OH-] ✓Do titration problems 26.Write the balanced chemical equation for the reaction between sodium hydroxide and phosphoric acid. 27.Which is the limiting reactant if a) 1.5 g of sodium hydroxide is mixed with 15 g of phosphoric acid? b) 100 mL of 0.10M sodium hydroxide is mixed with 150 mL of 0.10M phosphoric acid? 28.21.0 g of sodium hydroxide is added to water for a final volume of 500 mL. What is the concentration of sodium hydroxide? 29.What mass of NaCl needs to be added to water to make 100 mL of 1.0M NaOH? 30.What volume of 18.0M sulfuric acid is needed to prepare 500 mL of 0.750 M sulfuric acid? 31.15.0 g of sodium is added to water. The final volume of the solution formed is 350 mL. After writing out the balanced chemical equation, determine the concentration of sodium hydroxide formed.
32.10.0 mL of H2CO3is titrated with 0.50 M NaOH. a)Write the chemical equation that represents the reaction. b)Complete the chart: Trial Initial reading on burette Final reading on burette Volume of NaOH added (mL) 1 0.0 12.4 2 12.4 24.2 3 24.2 36.5 Average volume NaOH added c)How many moles of NaOH were required to neutralize the acid? d)How many moles of carbonic acid were neutralized? e)What is the concentration of the carbonic acid? f)If phenolphthalein is used as the acid-base indicator, what colour will the endpoint be? 33.What is the pH of a)0.0052M HCl? b)0.15M NaOH? 34.What is the [H+] in a solution with a pH of 2.6? 35.What is the colour of phenolphthalein in a)Water b) acid c) base 36.A solution tastes sour and is corrosive. Is it an acid or base? 37.A solution turns red litmus paper blue and tastes bitter. Is it an acid or base?
Gases:You will need to: ✓Describe the properties unique to gases and using the KMT explain these properties ✓Understand the terms: pressure, STP and molar volume ✓Convert temperature from Celsius to Kelvin and vice versa ✓Describe the relationship between pressure, temperature, volume and moles of a gas ✓Perform calculations using the combined gas law (P1V1/T1=P2V2/T2), Dalton’s Law of Partial Pressures (Ptotal= P1+ P2+ …), n = V/mV, and the ideal gas law (PV=nRT) ✓Use the gas laws in stoichiometric calculations 38.Convert a)120oC to Kelvin b) 1.5L of a gas at 25oC and 110 kPa to STP conditions 39.What is the impact of a)Increasing the pressure of a gas on its volume (n and T remaining constant) b)Decreasing the temperature of a gas on its pressure (n and V remaining constant) c)Increasing the number of moles of a gas on its pressure (T and V remaining constant) 40.What volume does 1.00 g of hydrogen gas collected at 102 kPa and 30oC occupy? 41.10.0 g of magnesium is allowed to react in 500.0 mL of 0.400M hydrochloric acid. What volume of hydrogen gas is produced at STP? (Hint: first you must consider which reactant is limiting) 42.A gas mixture contains 5.0 moles of nitrogen and 10.0 moles of helium. The total pressure of the gas mixture is 90 kPa. What is the partial pressure of each gas?