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Acids and bases 2017
- 1. Year 11 100Science 4 External Credits AS90944 Ms Gibellini
- 2. https://play.kahoot.it/#/?quizId=248ce6a9- 8476-4133-bf25-915462acb928 Whereto find info on moodle http://learningon.theloop.school.nz/moodle/c ourse/view.php?id=1336
- 3. Aspects of acidsand bases will be selected from: Atomic structure electron arrangement of atoms and monatomic ions of the first 20 elements (a periodic table will be provided) ionic bonding names and formulae of ionic compounds using a given table of ions. Properties acids release hydrogen ions in water reactions (of acids with bases) to form salts pH and effects on indicators. Rates of reaction and particle theory. Uses neutralisation carbon dioxide formation salt formation. Acids and bases are restricted to HCl, H2SO4, HNO3, metal oxides, hydroxides, carbonates and hydrogen carbonates. Other acids may be included in examination questions. The names and formulae of any such acids will be given in the question.
- 5. A neutronwalks into a restaurant and orders a couple of cokes. As she is about to leave, she asks the waiter how much she owes. The waiter replies, "For you, No Charge!!!"
- 6. Describe thestructure of an atom Discuss the key differences between the three sub-atomic particles
- 8. All matteris made up of atoms Chemistry involves the rearrangement of atoms or groups of atoms Recall the structure of an atom
- 10.
- 11. Atoms aremade up of the following sub atomic particles: Electrons negative charge outside nucleus, in shells constant motion very very small (1/2000 of a proton) Neutron No charge, neutral Inside nucleus Same size as proton Proton Positively charged Inside nucleus
- 12. Atoms havean overall neutral charge, therefore: Number of protons = Number of electrons
- 13. Criteria: • Different colourfor each sub atomic particle • Electrons smaller than protons and neutrons • Labels – including charge of particles • Electron clouds – 2, 8
- 14. Complete worksheetsprovided Compete Scipad page 10: Atoms Describe the atomic structure of a lithium atom Explain how the particles within an atom contribute to its overall mass.
- 15. Describe theatomic structure of a lithium atom Explain how the particles within an atom contribute to its overall mass. Overall mass of an atom is made up of protons and neutrons, as the mass of electrons is negligible
- 16. http://chemistry.about.com/library/weekly/blatomqu iz.htm http://ippex.pppl.gov/interactive/matter/elements.ht ml http://www.pbslearningmedia.org/asset/lsps07_int_t heatom/ http://www.bbc.co.uk/education/guides/zt2hpv4/rev ision - read and complete the quiz at the end http://phet.colorado.edu/en/simulation/build-an- atom https://www.youtube.com/watch?v=wRNxrxXkCRQ – only watch the first section on atoms
- 17. Define theterm ‘element’ Name and write symbols of common elements Develop an understanding of the structure of the Periodic Table
- 18. Elements aremade of only one kind of atom ◦ Gold is made of gold atoms ◦ Carbon is made of carbon atoms ◦ Hydrogen is made of hydrogen atoms
- 19. Elements havebeen put in order of: Physical properties Chemical properties Atomic number Mass number Number of electrons in outer shell on the Periodic Table of Elements
- 20.
- 21. 1) Hydrogen 2) Helium 3)Lithium 4) Beryllium 5) Boron 6) Carbon 7) Nitrogen 8) Oxygen 9) Fluorine 10)Neon 11) Magnesium 12)Aluminium 13)Silicon 14)Phosphorus H He Li Be B C N O F Ne Mg Al Si P
- 22. 15)Sulphur 16)Chlorine 17)Argon 18) Calcium 19) Zinc Theless obvious ones: 1) Sodium 2) Potassium 3) Iron 4) Copper 5) Silver 6) Tin 7) Gold 8) Mercury 9) Lead S Cl Ar Ca Zn Na K Fe Cu Ag Sn Au Hg Pb
- 23. Element Song Daniel Radcliff Learn your symbols: http://education.jlab.org/elementflashcards/
- 24.
- 25. 08/02/2017 Mendeleev The periodic tablearranges all the elements in groups according to their properties. Horizontal rows are called PERIODS Vertical columns are called GROUPS
- 26. 08/02/2017 H He Li BeB C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg Fact 1: Elements in the same group have the same number of electrons in the outer shell (this corresponds to their group number) E.g. all group 1 metals have __ electron in their outer shell These elements have __ electrons in their outer shell These elements have __ electrons in their outer shells
- 27. 08/02/2017 H He Li BeB C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg Fact 2: As you move down through the periods an extra electron shell is added: E.g. Lithium has 3 electron in the configuration 2,1 Potassium has 19 electrons in the configuration __,__,__,__ Sodium has 11 electrons in the configuration 2,8,1
- 28. 08/02/2017 H He Li BeB C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg Fact 3: Most of the elements are metals: These elements are metals This line divides metals from non- metals These elements are non- metals
- 29. 08/02/2017 H He Li BeB C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg Fact 4: (Most important) All of the elements in the same group have similar PROPERTIES. This is how I thought of the periodic table in the first place. This is called PERIODICITY. E.g. consider the group 1 metals. They all: 1) Are soft 2) Can be easily cut with a knife 3) React with water
- 30. Metals onthe _____ Non Metals on the ______ Rows tell us the number of electron shells an element has Groups tell us the number of electrons in the outer shell
- 32.
- 33. Complete Scipadpage 11and 13 http://www.bbc.co.uk/education/guides/z84wjxs/revision - read information, complete activity and quiz http://inteleducationresources.intel.co.uk/content/keystage4/ch emistry/pc/lessons/uk_ks4_elements_periodic_table/h-frame- ns6.htm http://inteleducationresources.intel.co.uk/content/keystage4/ch emistry/pc/lessons/uk_ks4_atoms_periodic_table/h-frame- ns6.htm http://preparatorychemistry.com/Element_name_symbol_Flash1. htm http://lessons.e- learningforkids.org/efk/Courses/EN/Science_Elements/base.htm
- 34. Determine thestructure of an atom based on data from the periodic table Draw the arrangement of electrons around any given atom Use the electron arrangement of an atom to identify which group on the periodic table it belongs too.
- 35. What isthe difference between Gold and Oxygen? Elements are made up of one kind of atom only Elements have been put in order of: Physical properties Chemical properties Atomic number Mass number Number of electrons in outer shell on the Periodic Table of Elements
- 36.
- 37. Atomic Number: Smallernumber Number of protons Number of electrons Atomic Mass or Mass Number: Bigger number of the two Total number of sub atomic particles Number of protons + neutrons.
- 38. How do wework out the number of: Protons = Atomic number Electrons = Atomic number Neutrons = Mass number – atomic number Fill in first 5 columns of Elemental information sheet http://learningon.theloop.school.nz/moodle/mod/quiz/vi ew.php?id=78647
- 39. Electrons arrangethemselves in regular order around the nucleus depending on their energy. Each energy level holds a different number of electrons: ◦ Level 1 – 2 electrons ◦ Level 2 – 8 electrons ◦ Level 3 – 8 electrons Electrons fill from Level 1 shell, or the closet to the nucleus first.
- 40. Calculating electron arrangementusing the periodic table: Row/Period gives us the number of electron shells Group tells us the number of electrons in outside shell Eg Sodium – row 3 – three shells - group 1 – 1 electron in outside shell - electron arrangement = 2,8,1
- 41. Fill incolumns 9, 10, 11 on elemental information sheet. Draw dot diagrams for the first 5 elements H, He, Li, Be, B) (use dots for electrons, and draw shell lines in pencil, use blue pen for protons and red for neutrons) Complete Scipad pages 12, 15, 16
- 42. http://lgfl.skoool.co.uk/content/keystage4/chemistry/pc/lesson s/uk_ks4_atoms_periodic_table/h-frame-ns6.htm http://phet.colorado.edu/en/simulation/build-an-atom http://www.pbs.org/wgbh/aso/tryit/atom/ http://www.learner.org/interactives/periodic/elementary_interac tive.html http://www.sciencequiz.net/jcscience/jcchemistry/atomstruct/at omicstmc1a.htm http://science.widener.edu/svb/tutorial/protons.html http://www.pbs.org/wgbh/aso/tryit/atom/builder.html http://www.classzone.com/books/earth_science/terc/content/in vestigations/es0501/es0501page05.cfm?chapter_no=investigati on http://www.bbc.co.uk/schools/gcsebitesize/science/add_edexce l/atomic_structure/electronsrev3.shtml - read and complete test bite
- 43. Describe therole of electrons in chemical reactions Describe how positive and negative ions are formed Write the name and formula of common ions
- 45. Two atoms arewalking down the street. Says one atom to the other, "Hey! I think I lost an electron!" The other says, "Are you sure??" "Yes, I'm positive!"
- 46. Chemical reactionsoccur when atoms gain or lose electrons The fewer electrons that are gained or lost the more reactive atoms are.
- 47. Atoms requiretheir outer shells to be full in order to be chemically stable Atoms either lose or gain electrons to get a full outer shell (2,8,8) When atoms lose or gain electrons they become electrically charged and are then called ions Gaining electrons (-ve) results in a ________ ion Losing electrons results in a __________ ion The number of protons (+ve) stays the same
- 48. E.g Na Na++ e- Sodium atom sodium ion Free electron 2, 8, 1 2, 8, Cl + e- Cl- Chlorine atom electron Chlorine ion 2, 8, 7 2, 8, 8 The charge on an ion is called its valency. Valency always has a sign (+ or -) and a numerical value. (although we don’t write 1) Complete ion information on elemental sheet
- 49. How doyou know if an atom will gain or lose electrons? Eg. Na 2,8,1 - is it easier to lose one electron or gain 7? - Hence Na looses a negative electron to become: - Na+ Eg. Cl 2,8,7 - is it easier to gain one electron or lose 7? - Hence Cl gains a negative electron to become: - Cl-
- 50. Information Na BeCl Atomic Number Mass Number Protons Neutrons Electrons Electron Config. Gain/Lose Electrons +ve/-ve charge Ion Formed Ion electron config. Protons: Electrons in Ion
- 51. Complete Scipadpages 17-19 Magnesium and calcium atoms both form ions with a charge of +2. Magnesium atoms form Mg2+ ions, and calcium atoms form Ca2+ ions. Explain why magnesium and calcium atoms form ions with the same charge of +2. In your answer, you should: define an ion explain why atoms form ions identify the group on the periodic table where the two atoms are found explain why both magnesium and calcium ions have a charge of +2.
- 52. Definition of anion: An ion is an atom or group of atoms that have lost or gained an electron and therefore carry a charge. Explanation of formation of ions: If the outer shell (valence) of an atom is not filled, the atom is unstable. It will react to gain a full outer shell to become more stable, by either losing or gaining electrons and making it into an ion. Identification of Group: Magnesium and calcium are in the same group on the periodic table Group 2 – both have two electrons in outside shell.
- 53. Explanation of whyboth form+2 ions: The atoms have the same number of electrons (two) in their outer shell. 2,8,2 and 2,8,8,2 Both Mg and Ca need to lose two outer electrons to become stable by having a full outer shell. Each ion (Mg2+ and Ca2+) ends up with two less electrons(negative) than there are protons(positive) in its nucleus, so the ion has a charge of +2.
- 54. http://learningon.theloop.school.nz/moodle/mo d/quiz/view.php?id=78656 http://education- portal.com/academy/lesson/ions-predicting- formation-charge-and-formulas-of- ions.html#lesson Kahoots - https://play.kahoot.it/#/?quizId=2cac1ec6- 82e3-4ba2-b5e2- 70de7c141537&user=ngibellini&token=3888d93 5-6c6c-456b-a1eb-6c979d632e41
- 55. Describe ionicbonding Use ions to write the name and formula of compounds A sign outside the chemistry hotel reads "Great Day Rates, Even Better NO3 -'s"
- 56. Ionic compounds: Have equal numbers of + and – charges Made up of metal and non metal Named by the ions they contain Metal part goes first, then non metal If non metal ion is made up of two or more elements change end to ate, SO4 – sulphate only 1 element in non metal ion it ends in ide NaCl = sodium chloride
- 57. Positive Ions NegativeIons +1 +2 +3 -3 -2 -1 H+ Hydrogen Ion Mg 2+ Magnesium Ion Al3+ Aluminium Ion N3- Nitrite Ion O2- Oxygen ion Cl- Chloride ion Li+ Lithium Ion Ca2+ Calcium Ion Fe3+ Iron III ion P3- Phosphide ion S2- Sulphide ion Br- Bromide ion Na+ Sodium Ion Fe2+ Iron II ion PO3- 4 Phosphate Ion CO2- 3 Carbonate ion I- Iodide ion K+ Potassium Ion Cu2+ SO2- 4 Sulphate Ion NO- 3 Nitrate ion Ag+ Silver Ion Zn2+ HCO- Hydrogen carbonate ion NH+ 4 Ammonium Ion Pb2+ OH- Hydroxide ion
- 59. Ionic compounds havean overall neutral charge. Therefore there must be equal numbers of positive and negative charges. ◦ Magnesium Nitrate Mg2+NO3 -1 Mg+ Mg+ NO3 -1 ◦ 2 positives and one negative what is needed to balance the charges? ◦ Another negative or (NO3 -1)2 Mg2+(NO3 -1)2 - we need another whole anion so use brackets
- 60. Write outsymbols from table Put brackets around ions with two elements (two capitals) eg SO2- 4 Count the number of positives and negatives Balance charges by multiplying ion Check it balances Rewrite without charges
- 62. Formulas show howmany atoms of each type are in a compound The bottom right hand number tells us how many of the atoms directly before it there are. ◦ H20 = 2 hydrogen atoms, one oxygen atom We don’t write 1 in as we are lazy!
- 63. The numberdirectly outside a bracket is a multiplier of everything inside the bracket. ◦ Al(OH)3 = 1 Al, 3 O, 3 H ◦ (NH4)3PO4 = 3N, 12 (3x4) H , 1P, 4 O To get the total number of atoms we work out how many of each atoms there are and then add them ◦ (NH4)3PO4 = 3N, 12 (3x4) H , 1P, 4 O ◦ 3+12(3x4)+1+4 = 20 atoms
- 64. A bignumber in front means two of the whole compound – so work out how many of each atom there is, add them up and then multiply this by the big number at the front. ◦ 2(NH4)3PO4 = 3N, 12 (3x4) H , 1P, 4 O ◦ 3+12+1+4 = 20 atoms ◦ 20 x 2 = 40 atoms
- 65. Complete Scipadpages 20-27 Explain why the ions in sodium hydroxide combine to give the formula NaOH but the ions in beryllium hydroxide combine to give the formula Be(OH)2. In your answer, you should: compare the charges on the individual ions found in the compounds sodium hydroxide and beryllium hydroxide explain why the ions combine in the ratios the way they do to form the compounds NaOH and Be(OH)2.
- 66. Comparison of chargeson ions: When these elements react, Na loses one electron and forms a +1 ion, while Be loses two electrons and forms a +2 ion in order to adopt the stable electron configuration. The hydroxide carries a charge of -1. Explanation of formation of compounds: An ionic compound is electrically neutral therefore all the positive charges must balance the negative charges. Therefore it requires one OH-1 for each Na+ ion but two OH-1 ions for each Be2+ ion to form a neutral compound/ balance the charges.
- 67. Explain why theions formed by sodium and oxygen both have the same electron arrangement. In your answer you should: • describe an ion • describe the atomic structures of a sodium ion and an oxide ion • state the charge on the sodium ion and the oxide ion • explain the charges on both ions in terms of electron arrangement and number of protons
- 68. Element X isbetween numbers 11 and 18 on the Periodic Table. An atom of element X forms an ion. This ion combines with the hydroxide ion to form a neutral compound, X(OH)3. Determine what element X is and justify your answer. In your answer you should: • consider the ratio of X ions to hydroxide ions • use the formula X(OH)3 to determine the charge of the X ion • explain how you would use the Periodic Table in your Resource Booklet to find out which group element X is in • name element X.
- 69. http://www.learner.org/interactives/periodic/ basics_interactive.html http://www.sciencegeek.net/Chemistry/tater s/Unit2IonicCompoundFormulas.htm http://preparatorychemistry.com/Bishop_ani on_nom_Flash1.htm http://preparatorychemistry.com/Bishop_cati on_nom_Flash1.htm
- 70. Write wordequations for chemical reactions Balance chemical equations
- 71. Reactant Product There has to be the same number and type of each atom on both sides of the arrow – this is how you check you have balanced the equation correctly! There are three types of equations ◦ Word equations (don’t need atoms balanced) ◦ Symbol equations ◦ Ionic equations (not need for level 1)
- 72. Step 1: Writeout word equation Magnesium + oxygen Magnesium oxide Step 2: Write out symbol formula Mg + O2 MgO Step 3: Count atoms of each kind on each side 1 Mg 2 O 1 Mg 1O
- 73. Step 4: Identifythe atoms with different numbers 2 oxygen atoms on left one on right Step 5: Increase atoms by putting number: in front of compound (2H2O) – makes 4 H & 2 O after an ion (Mg2) – makes 2 Mg brackets and a subscript around polyatomic ions (SO4)2 –makes 2 S & 8 O Do hydrogen then oxygen atoms first Mg + O2 2MgO
- 74. Step 6: Countatoms of each kind on each side – they will have changed as a result of step 5!!!! 1 Mg 2 O 2 Mg 2O Step 7: Identify the atoms with different numbers 1 Mg on left & 2 on right Step 8: Increase atoms numbers 2Mg + O2 2MgO
- 75. Step 1: Writeout word equation Sodium + Water Sodium Hydroxide + Hydrogen Step 2: Write out symbol formula Na + H2O NaOH + H2 Step 3: Count atoms of each kind on each side 1 Na, 2 H, 1 O 1 Na, 1 O, 3 H Step 4: Identify the atoms with different numbers 2 H 3 H Step 5: Increase atoms by putting number: Na + 2H2O 2NaOH + H2
- 76. Step 6: Countatoms of each kind on each side 1 Na 4H 2 O 2 Na 2 O 4H Step 7: Identify the atoms with different numbers 1 Na on left and 2 on right Step 8: Increase atoms numbers 2Na + 2H2O 2NaOH + H2
- 77. Step 12: Countatoms of each kind on each side 2 Na 4H 2 O 2 Na 2 O 4H Same type of atoms and same number of atoms on both sides – DONE! Nobody said it’d be easy but it does get easier, and remember practice makes perfect!
- 79. http://misterguch.brinkster.net/eqnbalance.html http://www.files.chem.vt.edu/RVGS/ACT/notes/scripts/bal_eq1.html http://www.sciencegeek.net/Chemistry/taters/EquationBalancing.htm http://preparatorychemistry.com/Bishop_bal_eq_Flash1.htm http://education.jlab.org/elementbalancing/ http://funbasedlearning.com/chemistry/chemBalancer/default.htm http://phet.colorado.edu/sims/html/balancing-chemical-equations/latest/balancing- chemical-equations_en.html http://www.creative-chemistry.org.uk/gcse/revision/equations/02.htm Kahoots: https://play.kahoot.it/#/?quizId=891a4988-2b62-4650-a6ad- 2448a3185aa4&user=ngibellini&token=3888d935-6c6c-456b-a1eb-6c979d632e41 https://play.kahoot.it/#/?quizId=b9a2e1f9-e174-4a17-904f- 772c3d8ca5d7&user=ngibellini&token=3888d935-6c6c-456b-a1eb-6c979d632e41 https://play.kahoot.it/#/?quizId=a12c2b2d-859b-49cf-a878-10344ebc6639 Complete Sci pad pages 28-31
- 80. Complete Scipadpages 8-9, 32-35 http://www.nobraintoosmall.co.nz/students/ science/NCEA_Level1/pdfs/90944_collated_a tom_questions.pdf#zoom=100 Complete purple book pages: Complete worksheets:
- 83. http://www.youtube.com/watch?v=_rsqBNhFG1Y http://inteleducationresources.intel.co.uk/conten t/keystage3/chemistry/pc/learningsteps/particle _theory/launch.html http://www.bbc.co.uk/bitesize/ks3/science/che mical_material_behaviour/particle_model/activity / https://www.youtube.com/watch?v=eSInI1xHvh4
- 84. In orderfor a reaction to occur particles need to collide Particles need to collide with enough force to break bonds and form new ones The more successful collisions the faster a reaction occurs Complete Rates of Reaction Experiments
- 85. More successful collisionscan be caused by: ◦ Increasing the temperature (particles move faster so collide more) ◦ Increasing the concentration (more particles to collide) ◦ Increasing surface area (small particles have greater surfaces for collisions to occur) ◦ Use a catalyst (holds chemicals so collisions can occur, lowers activation energy needed to break bonds) ◦ Increase pressure (particles are closer together therefore collide more often) Increasing collisions increases rate of reaction!
- 86. What isthe difference between particle theory and collision theory Complete Rates of Reactions Experiments Complete worksheets Complete scipad pages 37-39, 48-53 Complete pages 40-47 (all the equipment you need is up the front) http://www.kscience.co.uk/animations/collision.h tm
- 87. Particle theory– all matter is made up of particles which are in constant motion Collision theory – particles need to collide with enough force and energy to break bonds and form new ones More particles more collisions faster rate of reaction More movement more collisions faster rate of reaction
- 88. Calcium carbonate (marblechips) and hydrochloric acid react together in a conical flask. The word equation for this reaction is: calcium carbonate + hydrochloric acid → calcium chloride + water + carbon dioxide gas (a) Describe an observation you would make when this reaction occurs. (b) Explain why the mass decreases with time. When more concentrated hydrochloric acid is used, the reaction is faster. © Explain the difference in the rate of reaction. In your answer you should refer to: • particles • collisions • reaction rate.
- 89. Fizzing / bubblingoccurs, marble chips decrease in size, heat is produced. Why mass decreases The marble chips decreases as one of the products is CO2 gas. This gas escapes and so the mass of the flask and contents is reduced. What’s happening As the reactant particles collide, they form product particles. As the reaction proceeds, there are fewer and fewer reactant particles left to collide and so the rate of reaction becomes slower. At the start (section X) of the reaction, more product particles are being formed, then more gas is being formed, therefore more gas escapes at first and so the mass of the flask and contents decreases more rapidly. At X, the rate of reaction is fast but decreasing with time. In section Y there are now fewer (less) reactants and so there are fewer collisions per second (unit time) and so less product is formed, ie less gas being released, so the mass does not decrease as rapidly. At Y, the rate of reaction is slow and slowing. In section Z the reaction has stopped, as one of the reactants (marble chips or HCl) has run out, so there are no particles left to react.
- 90. When more concentratedacid is used, there are more acid particles in the same volume of the acid. Because of this, there are more particles to collide with the calcium carbonate. Because there are more to collide, the rate of reaction is faster. Explains why the reaction is faster, by linking the idea that there are more acid particles in the same unit volume available for collisions, and hence there will be more collisions, causing the faster reaction rate
- 91.
- 93. Define theterms acid, base and alkali Name and write the formula of three common laboratory acids Classify acids and alkalis as chemicals with distinct properties and uses.
- 94.
- 95. Taste sour pH less than 7 Turn litmus red Contain hydrogen ion H+ Conduct electricity Acid rain (oxides of sulphur and nitrogen from factories dissolve in water to form acid rain) citric juice, stomach acid (HCl), vinegar, battery acid Acid reactions: ◦ Acid + base salt + water ◦ Acid + metal salt + hydrogen gas ◦ Acid + carbonate salt + water + carbon dioxide
- 96. Taste bitter,Feel slippery pH greater than 7 Turn litmus blue Alkali is a base that is soluble in water Metal oxides and metal hydroxides Most contain OH- ion, hydroxide ion Conduct electricity Soaps, oven cleaners (NaOH) Antacids (Mg(OH)2) – neutralise stomach acids Floor cleaners, bleach (ammonium hydroxide) Calcium hydroxide is limewater Calcium hydrogen carbonate – limestone caves Used to neutralise acids: ◦ Neutralisation ◦ HCl + NaOH NaCl + H2O = pH 7 ◦ Acid + Base salt + water
- 97. Common Name Chemical Name FormulaAcid Base Vinegar Lemon juice Grape juice Soda Water Antacids Floor Cleaner Battery Acid Stomach Acid Nitric Acid Hydrochloric Acid Magnesium oxide
- 98. Common Name ChemicalName Formula Acid Base Vinegar Acetic Acid C2H4O2 Lemon juice Citric Acid C6H8O7 Grape juice Tartaric Acid C4H6O6 Soda Water Carbonic Acid H2CO3 Antacids Magnesium Hydroxide MgOH Floor Cleaner Ammonium Hydroxide NH4OH Battery Acid Sulphuric Acid H2SO4 Stomach Acid Hydrochloric Acid HCl Nitric Acid Nitric Acid HNO3 Hydrochloric Acid Hydrochloric Acid HCl Magnesium oxide Magnesium oxide MgO
- 99. Complete Scipadpages 58-59 What is an Acid, What is a Base List three common household acids and their formulas List three common household bases and their formulas
- 100. http://inteleducationresources.intel.co.uk/co ntent/keystage4/chemistry/pc/lessons/uk_ks 4_acids_alkalis_salts/h-frame-ns6.htm http://preparatorychemistry.com/Bishop_acid _base_Flash1.htm http://preparatorychemistry.com/Bishop_typ e_sub_Flash1.htm
- 101. Use thepH scale to compare the acidity and alkalinity of different solutions http://inteleducationresources.intel.co.uk/content/keystage3 /chemistry/pc/learningsteps/acids_alkalis/launch.html http://inteleducationresources.intel.co.uk/content/keystage3 /chemistry/pc/learningsteps/acid_base_reactions/launch.htm l http://inteleducationresources.intel.co.uk/content/keystage3 /chemistry/pc/learningsteps/neutral_react/launch.html http://inteleducationresources.intel.co.uk/content/keystage3 /chemistry/pc/learningsteps/ph_scale/launch.html
- 102. We use apH scale to tell us how acidic, basic or neutral a substance is. Acids have a pH range from 1-6 Alkalis or bases have a pH range from 8-14 Neutral substances have a pH of 7
- 103. Strong acidscontain more free H+ ions Strong bases contain more free OH- ions Most naturally occurring substances are weak eg. Citric acid in citrus fruit
- 105. Complete ScipadInvestigations pages 61-62 Testing pH and Making Indicators Complete Scipad page 63
- 106. Name andwrite the formula for various metal oxides, metal hydroxides, metal carbonates and hydrogen carbonate
- 107. Metal oxides contain oxide ion O2- Rust Iron oxide FeO, Zinc oxide (sunscreen) ZnO Basic Acid + Metal Oxide Metal Salt + Water Metal Hydroxide Contain hydroxide ion OH- Antacids Magnesium hydroxide MgOH Form when metal or metal oxide reacts with water Acid + Metal Hydroxide Metal Salt + Water
- 108. Metal Carbonates Contain the carbonate ion CO3 - Calcium carbonate CaCO3 - marble chips Release carbon dioxide when react with acids Acid + Metal Carbonate Metal Salt + Water + Carbon Dioxide Metal Hydrogen Carbonates Contain hydrogen carbonate ion HCO3 - Neutralise acids Produce carbon dioxide when reacted with acids Calcium hydrogen carbonate CaHCO3 Acid + Metal Hydrogen Carbonate Metal Salt + Water + Carbon Dioxide
- 109. Name Metal TypeFormulae Copper oxide CuCO3 Lithium hydroxide FeO Zinc carbonate MgOH Calcium hydrogen carbonate
- 110. Describe neutralisationreactions Identify the products of neutralisation reactions
- 111. When weadd base to an acid, a chemical reaction takes place. The acid and base are used up in the reaction. We say they are neutralised. They make a salt and water. When a substance has been neutralised or is neutral it has a pH of around 7. Acid + Base Salt + Water
- 112. Aim: To neutralisean acid using a base. Method: Step 1: Add four drops of sodium hydroxide to a test tube. Step 2: Add one drop of universal indicator to the test tube and shake. Step 3: Stop when the solution is green, if the solution turns red or orange add a very small drop of NaOH until the liquid turns green.
- 113. Complete Scipadpractical page 64 Neutralisation Complete scipad page 65
- 114. What causes indigestion? -tomuch acid in the oesophagus What do we need to add to neutralize that acid? - Base! – Antacid, quickeze, mylanta, gaviscon etc
- 115. Iron Magnesium ZincCopper Lead Hydrochloric Acid Sulphuric Acid Zinc Sulphate ZnSO4 No Reaction Nitric Acid Salts are named after the acids from which they are formed. • Hydrochloric acid forms chloride salts • Sulphuric acid forms sulphate salts • Nitric acid forms nitrate salts
- 116.
- 117. Complete pages93, 94, 95 A student puts 5 mL of dilute hydrochloric acid into a boiling tube and adds five drops of universal indicator to the solution. The student then takes a solution of sodium hydroxide of the same concentration as the acid and adds it one drop at a time to the acid until the colour stops changing. Describe the colour of the universal indicator solution: ◦ in the hydrochloric acid before any sodium hydroxide was added. ◦ when the sodium hydroxide was added and the colour of the solution stopped changing. As the sodium hydroxide is added several colour changes occur. Explain how the colour changes relate to pH AND what ions are present in the solution colour changes.
- 118. Description of colourchanges: red /pink to start with blue /purple /violet at end. Explanation of colour changes: At the beginning the red indicated a low pH due to excess H+ ions in the solution. As the NaOH was added, a yellow /green colour indicates a pH of around 7, due to the OH- ions combining with the H+ ions to form a neutral solution. As more NaOH is added the blue /purple indicated a pH of 11 plus, due to excess OH- ions in the solution. Identification of reaction type: Acid-base (or acid-carbonate) neutralisation (the carbonate ions react with the H+ ions of the acidic solution and neutralise the solution). Description of observations: Bubbling in the solution /fizzing /effervescence /frothing /foaming Ca2CO3 disappears. Linking observations to products: The products are CO2, H2O and a salt. The CO2 gas causes the bubbles /fizzing /etc. Writing a word equation: Nitric acid + sodium carbonate sodium nitrate + water + carbon dioxide Writing a symbol equation: 2HNO3 + Na2CO3 2NaNO3 + H2O + CO2
- 119. A student put10 ml of dilute nitric acid in a boiling tube with five drops of universal indicator. Sodium hydroxide of the same concentration was then added. The following observations were recorded. Discuss the reaction occurring as sodium hydroxide is added to the nitric acid. In your answer you should: • explain the relationship between the colours observed and the pH of the solution • explain which ions cause the different colours of the solution • write a word equation for the reaction AND a balanced symbol equation for the reaction.
- 120. Write wordand symbol equations for a range of reactions involving acids and bases Describe some everyday uses of acids, alkalis and neutralisation
- 121. Acid +Base Salt + Water Hydrochloric acid + sodium hydroxide sodium chloride + water Test to see if reaction is complete by using indicator – solution should turn Green
- 122. Complete scipadpages 66-68 Writing chemical equations Complete Scipad practical Making Salts, page 69
- 123. Acid +Carbonate Salt + Water + Carbon dioxide Sulphuric Acid + Copper Carbonate Copper sulphate + water + Carbon dioxide We test for Carbon dioxide by bubbling the gas into lime water which turns milky
- 124. Limewater (calcium hydroxide)reacts with carbon dioxide to produce a precipitate of calcium carbonate: Ca(OH)2 (aq) + CO2 (g) → CaCO3 (s) + H2O (l) Limewater + carbon dioxide calcium carbonate + water If excess CO2 is added, the following reaction takes place: CaCO3 + H2O + CO2 --> Ca(HCO3)2 (colourless) Calcium Carbonate + water + carbon dioxide calcium bicarbonate
- 125. Complete Scipadpractical page 70 Carbonates and Acids Complete Scipad page 71-73
- 126. Acid +Metal Salt + Hydrogen Gas Nitric Acid + magnesium magnesium nitrate + hydrogen gas We test for hydrogen gas by doing the POP test
- 127. Acid +Base Salt + Water Acid + Carbonate Salt + Water + Carbon dioxide Acid + Metal Salt + Hydrogen Gas
- 128. A student wantedto make the salt, magnesium chloride. Discuss how the student would make magnesium chloride salt from hydrochloric acid and magnesium oxide. In your answer you should: • state what type of reaction occurs • write a word equation AND a balanced symbol equation for the reaction between hydrochloric acid and magnesium oxide • explain how you would make magnesium chloride in a school lab from hydrochloric acid and solid magnesium oxide (this can be done by drawing labelled diagrams).
- 129. Type of reaction Acid-Basereaction or neutralisation. Word Equation hydrochloric acid + magnesium oxide → magnesium chloride + water. Balanced Equation 2HCl + MgO → MgCl2 + H2O How to make it Add magnesium oxide to hydrochloric acid in a beaker. Heat slightly and pour this into an evaporating dish and leave somewhere warm (e.g. window sill) for a few days or heat over Bunsen to speed up the reaction, so that the water can evaporate, leaving magnesium chloride salt. Safe lab procedure would include dealing appropriately with chemicals such as HCl or the wearing of safety glasses
- 130. Complete Scipadpages 74-79 Brainstorm connecting words Read the question and answer on the sheet, ◦ highlight the connecting terms, ◦ use the marking schedule to mark it. Swap and complete one more question Complete questions on worksheet ◦ Use connecting terms! Complete Scipad practice NCEA exam under exam conditions pages 80-85, mark it!!
- 131. Online Tutorialsand Quizzes ◦ http://inteleducationresources.intel.co.uk/keystage 3.aspx?id=64
- 132. Atoms andions ◦ Structure of an atom, number of protons, neutrons, elections, electron configuration ◦ Isotopes ◦ Ion formation ◦ Ionic compounds Rates of reactions ◦ Particle theory ◦ Factors affecting rate ◦ Observations and tests for gases Acids reactions ◦ Properties of acids and bases ◦ Common acid equations ◦ pH, indicators and neutralisation ◦ Word equations and balanced equations
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