Revision work 1) Define the term isotopes. 2) How many protons, neutrons and electrons are present in each of the following atoms? In Modern Definition, C-12 is chosen as the standard reference Atomic Mass Unit ( amu) • Mass of one atom of Carbon – 12 = 12 amu Modern Definition of relative atomic mass Old definition of relative atomic mass • Relative atomic mass (Numerical) • 1 Chlorine consists of two isotopes with mass numbers 35 and 37, with their natural abundances 76% and 24% respectively. • Calculate a) average mass of one atom of Chlorine • b) relative atomic mass of Chlorine Isotopes of Chlorine (numerical’s answer) • a) Let us consider 100 Cl atoms found in nature. • Total mass of 100 Cl atoms = 76 x 35 amu + 24 x 37 amu = 3548 amu Therefore, average mass of one atom of Cl = 3548 amu/100 = 35.5 amu b) Relative atomic mass of Chlorine • Problem no 2 • Magnesium consists of three isotopes with mass numbers 24, 25 and 26 , and with natural abundances 79%, 10% and 11% respectively. • Calculate a) average mass of one atom of Magnesium • b) relative atomic mass of Magnesium Problem No 3 • Boron consists of two isotopes with nucleon number 10 and 11, and with natural abundances 20% and 80% respectively. • Calculate relative atomic mass of Boron. Isotopes of Magnesium Isotopes of Chlorine Summary about Chlorine • i) Atomic number of Chlorine is 17. • ii) Mass numbers for first Cl atom is 35 and for 2nd Cl atom is 37. • iii) Average mass for one atom of Chlorine = 35.5 amu. • iv) Average mass of one atom of element in amu is atomic mass. • v) Atomic mass of Chlorine is 35.5 amu. • vi) Relative atomic mass of Chlorine is 35.5. Isotopes of Magnesium Summary about Magnesium • i) Atomic number of Magnesium is 12. • ii) Mass numbers for first Mg atom is 24 , for 2nd Mg atom is 25 and for third Mg atom is 26. • iii) Average mass for one atom of Magnesium = 24.3 amu. • iv) Average mass of one atom of element in amu is atomic mass. • v) Atomic mass of Magnesium is 24.3 amu. • vi) Relative atomic mass of Magnesium is 24.3. • https://youtu.be/0N_CIdmI5Cg Problem No 4 Most elements exist naturally as a mixture of isotopes, each with their own relative isotopic mass. Lead has four stable isotopes. Information about three of these isotopes is given. Isotope Pb-204 Pb-206 Pb-208 Relative isotopic Percentage abundance mass 204.0 1.4 206.0 24.1 208.0 52.4 a) Define the term relative isotopic mass. For example Relative isotopic mass of Pb-208 is equal to ratio of mass of one atom of Pb-208 to 1/12 the mass of one atom of C-12 b) The relative atomic mass of Lead is 207.21. Calculate the percentage abundance and hence the relative isotopic mass of the fourth isotope of Lead. • Percentage abundance of the fourth isotope of Lead = 100 – (1.4 + 24.1 + 52.4) = 100 – 77.9 = 22.1 Relative atomic mass of Lead is 207.12. Let relative isotopic mass of the fourth isotope of Lead is a. • Learners can build and test isotopes using this simulation: phet.colorado.edu/en/simulation/isotopes-and-atomic-mass 1 mole = 6.02 x 1023 particles(Avogadro’s constant) For example 1 mole of e - = 6.02 x 1023 electrons 1 mole of H = 6.02 x 1023 hydrogen atoms 1 mole of H2 = 6.02 x 1023 hydrogen molecules 1 mole of CO2 = 6.02 x 1023 CO2 molecules Comparison Species He C-12 Mg Relative atomic mass/relative isotopic mass 4 12 24.3 Atomic mass/isotopic mass 4 amu 12 amu 24.3 amu 1 mole 4g 12 g 24.3 g No of particles 6.02 x 1023 Helium atoms 6.02 x 1023 Carbon -12 atoms 6.02 x 1023 Magnesium atoms Molar mass • Mass of 1 mole of substance is called molar mass. • Molar mass of Helium is 4 g mol-1 • Molar mass of Magnesium is 24.3 g mol-1 Molar mass of Calcium is 40.1 g mol-1 Copy and complete the following table Element Molar mass Na 23 g mol-1 Cu Ar Fe Ba Answer Element Molar mass Na 23 g mol-1 Cu 63.5 g mol-1 Ar 39.9 g mol-1 Fe 55.8 g mol-1 Ba 137.3 g mol-1 Revision • Relative atomic mass of Lithium (Ar) = 6.9 • Atomic mass of Lithium = 6.9 amu • Molar mass of Lithium = 6.9 g mol-1 • 6.9 g of Lithium contains 6.02 x 1023 Lithium atoms Calculate the no of moles present in each of the following samples. a) 30.0 g carbon b) 24.0 g Sulphur c) 16.0 g Magnesium • a) Mass = 30 g • Molar mass of Carbon = 12 g mol-1 • No of moles = Mass/Molar mass • = 30 g/12 g mol-1 • = 30 g/12 g mol-1 • = 2.5 mol Mole or Mol ? • Rupees in short is written as Rs •mole in short is written as mol •5 mole or 5 mol How many atoms are present in each of the following samples? i) 1.5 mol of H ii) 3.99 gram of Argon iii) 48.6 gram of Magnesium Answer • i) 1 mol of H contains 6.02 x 10 23 H atoms Therefore 1.5 mol of H contains 1.5 x 6.02 x 10 23 H atoms = 9.03 x 1023 H atoms ii) No of mol = mass/molar mass = 3.99 g/ 39.9 g mol-1 = 0.1 mol Therefore No of Argon atoms = 0.1 x 6.02 x 10 23 = 6.02 x 1022 What is the mass (in gram) in each of following samples? i) 0.1 mol of Mg ii) 10 mol of Li iii) 6.02 x 1021 atoms of Iron iv) 6.02 x 1025 atoms of Helium Answer • i) No of mol (n) = 0.1 mol • Molar mass of Magnesium = 24.3 g mol-1 No of mole (n) = mass (m)/Molar mass(M) Therefore, m = n x M = 0.1 mol x 24.3 g mol-1 = 0.1 mol x 24.3 g mol-1 = 2.43 g Answer of q. no. iii) No of mol of iron = 6.02 x 1021 / 6.02 x 1023 n = 0.01 mol molar mass of iron (M) = 55.8 g mol-1 mass (m) = n x M = 0.01 mol x 55.8 g mol-1 = 0.558 g Which one of the following samples contains highest no of atoms? • a) 2 g of hydrogen. • b) 9.03 x 1023 atoms of oxygen • C) 16.0 g of oxygen • d) 7 g of Helium gas Definition Calculate relative molecular mass (Mr) of following. (Relative atomic mass (Ar) of H= 1, C = 12, N= 14, O = 16) i) CO2 • ii) NH3 • iii) C3H7OH • Iv) C6H12O6 Answer • iii) Relative molecular mass (Mr) of C3H7OH = 3 x 12 + 8 x 1 + 1 x 16 = 36 + 8 + 16 = 60 Note: Like Ar , Mr also does not have any unit. Answers i) 44 ii) 17 iii) 60 iv) 180 Calculate relative formula mass (Mr) of following. • i) KCl • iii) BaCl2. 2H2O ii) MgSO4 iv) CuSO4. 5 H2O • v) (NH4)2SO4 • Note: Compounds given above are not made up of molecules. • They are made up of ions. • (Ar of K = 39.1, Mg = 24.3, Ba = 137.3 , Cl = 35.5 , Cu = 63.5 , S = 32.1) Answer • i) Mr of KCl = 1x 39.1 + 1 x 35.5 = 39.1 + 35.5 = 74.6 iv) Mr of CuSO4. 5 H2O = 1 x 63.5 + 1 x 32.1 + 4 x 16 + 5 x 18 = 63.5 + 32.1 + 64 + 90 = 249.6 Other answers: ii) 120.4 iii) 244.3 iii) 132.1 Revision • i) Relative molecular mass (Mr) of CO2 = 44 • Molecular mass of CO2 = 44 amu • Molar mass of CO2 = 44 g mol-1 • 44 g of CO2 contains 6.02 x 1023 molecules of CO2 Calculate the no of moles present in each of the following samples. a) 90 g of H2O(l) b) 36 g of C6H12O6 (s) c) 51 g of NH3 (g) Answers • a) 5 mol of H2O • b) 0.2 mol of glucose • C) 3 mol of NH3 A drop of water weighs 0.04 g. Calculate the number of H2O molecules present in the drop of water. Mass (m) = 0.04 g Molar mass of water (M) = 18 g mol-1 No of mol of H2O (n) = m/M = 0.04 g/18 g mol-1 = 2.22 x 10-3 mol Therefore, number of H2O molecules = 2.22 x 10-3 x 6.02 x 1023 = 1.34 x 1021 What is the mass of each of the following samples? • a) 1.5 moles of MgSO4 • b) 0.333 moles of AlCl3 • c ) 0.25 mole of CaCO3 d) 4 mol of CH4 Answer i) relative molecular mass (Mr ) of MgSO4 = 1 x 24.3 + 1 x 32.1 + 4 x 16 = 120.4 1.5 mol of MgSO4 = 180.6 g ii) Mr of AlCl3 = 133.5 mass of 0.333 mol of AlCl3 = 44.45 g iii) Mr of CaCO3 = 100.1 0.25 mol of CaCO3 = 25.025 g iv) Mr of CH4 = 16 4 mol of CH4 = 64 g A gas syringe contains 64 g of Oxygen gas. Calculate the number of moles of Oxygen. Relative atomic mass of O (Ar) = 16 Mass (m) = 64 g Molar mass(M) = 16 g mol-1 n = m/M = 64 g/16 g mol-1 = 4 mol of O Relative molecular mass of O2 (Mr) = 32 Mass (m) = 64 g Molar mass(M) = 32 g mol-1 n = m/M = 64 g/32 g mol-1 = 2 mol of O2 A mole of ? Be specific • 1 molecule of H2O is made up of 2 atoms of H and 1 atom of O • 1 mol of H2O contains 2 mol of H and 1 mol of O. • 1 mol of H2O contains 2 x 6.02 x 10 23 atoms of H and 6.02 x 1023 atoms of O. • 1 mole of CaCl2 contains 1 mol of Ca++ ion and 2 mol of Clion Fill in the blanks about ethane (C2H6 ) • 1 molecule of ethane is made up of ….. atoms of C and ….. atoms of H. • 1 mol of ethane is made up of …… mol of C and ….. mol of H. 1 mol of C2H6 contains ………………… atoms of C and …………….. atoms of H. Relative molecular mass (Mr ) of C2H6 is …………….. Molar mass of ethane is ………….. Answer for fill in the blanks about ethane (C2H6 ) • 1 molecule of ethane is made up of 2 atoms of C and 6 atoms of H. • 1 mol of ethane is made up of 2 mol of C and 6 mol of H. 1 mol of C2H6 contains 2 x 6.02 x 1023 atoms of C and 6 x 6.02 x 1023 atoms of H. Relative molecular mass (Mr ) of C2H6 is 30 Molar mass of ethane is 30 g mol-1 What is the mass of each of the following samples in gram? • a) 1 mol of H • b) 1 mol of H2 c) 1 mol of C2H5OH d) 5 mol of CaCl2 Answer • a) 1 g of Hydrogen • b) 2 g of Hydrogen • c) 46 g • d) 555.5 g Suppose you wrote your name with a stick of chalk (CaCO3) on the ground. 0.05 g of calcium carbonate is deposited on the ground. • a) Calculate how many mol of calcium carbonate is deposited on the ground after writing your name with a stick of chalk. • b) Calculate how many particles of calcium carbonate are deposited on the ground c) Calculate how many individual atoms of oxygen are deposited. First 20 elements and their normal form S.No Name of element Symbol/ formula Mass of 1 mol S.no Name of element Symbol/ formula Mass of 1 mol 1 Hydrogen H2 (g) 2g 11 Sodium Na (s) 23 g 2 Helium He (g) 4g 12 Magnesium Mg (s) 24.3 g 3 Lithium Li (s) 6.9 g 13 Aluminium Al (s) 27 g 4 Beryllium Be (s) 9g 14 Silicon Si (s) 28.1 g 5 Boron B (s) 10.8 g 15 Phosphorous P (s) 31 g 6 Carbon C (s) 12 g 16 Sulphur S (s) 32.1 g 7 Nitrogen N2 (g) 28 g 17 Chlorine Cl2 (g) 71 g 8 Oxygen O2 (g) 32 g 18 Argon Ar (g) 39.9 g 9 Fluorine F2 (g) 38 g 19 Potassium K (s) 39.1 g 10 Neon Ne (g) 20.2 g 20 Calcium Ca (s) 40.1 Ions formed by the first 20 elements S. No. Name of element Electron arrangement Formula of Ion/s formed S.No Name of . element Electron arrangemen t Formula of Ion/s formed 1 Hydrogen 1 H + or H - 11 Sodium 2,8,1 Na + 2 Helium 2 None 12 Magnesium 2,8,2 Mg ++ 3 Lithium 2,1 Li + 13 Aluminium 2,8,3 Al +++ 4 Beryllium 2,2 Be ++ 14 Silicon 2,8,4 Si ++++ or Si ---- 5 Boron 2,3 B +++ 15 Phosphorous 2,8,5 6 Carbon 2,4 C ++++ or C ---- 16 Sulphur 2,8,6 7 Nitrogen 2,5 Chlorine 2,8,7 Cl - 8 Oxygen 2,6 N O -- 17 18 Argon 2,8,8 None 9 Fluorine 2,7 F- 19 Potassium 2,8,8,1 K+ --- P --S -- Monoatomic ion contains only one atom in the ion. Polyatomic ion contains 2 or more atoms in the ion. S.No Name of ion 1 hydroxide Formula S.No Name of ion Formula of ion of ion OH 6 sulphite SO3 -- 2 carbonate CO3 -- 3 4 Bicarbonate/ HCO3 hydrogencarbonate sulphate SO4 -- 5 Phosphate --PO4 7 nitrate NO3 - 8 nitrite NO2 - 9 ammonium NH4 + Rule for writing formula of ionic compound • i) Positive ion is written in the left side of the formula • ii) Polyatomic ion is enclosed in a bracket if the number of the polyatomic ion in the compound is more than 1. • Write down molecular formula of aluminium sulphate 3 2 Al SO 4 Al2(SO4)3 Examples of ionic compounds Compound name formula Cation anion Calcium chloride CaCl2 Ca++ Cl - Sodium chloride NaCl Na+ Cl - Lithium fluoride LiF Li+ F- Iron(II) oxide FeO Fe++ O -- Aluminium sulphide Al2S3 Al+++ S -- Fe2(SO4)3 Fe+++ SO4 -- Iron(III) sulphate Correct following molecular formulae if necessary • i) MgOH2 ii) (NH4)Cl • iii) Cl3Al iv) Cu(II)SO4 Water is a covalent compound • Water is a covalent compound. • If you take water in a glass, there will be large no of seperate seperate H2O molecules Water is made up of large number of separate H2O molecules. Sodium chloride is an ionic compound Sodium chloride is made up of ions. It does not contain separate NaCl molecules Na +Cl Na +Cl- Na +Cl - Na +Cl Na +Cl - Na +Cl- Na +ClNa +Cl- X Na +Cl- Ionic compound like sodium chloride are not made up of molecules. Hence we use the term relative formula mass for them. Formula of sodium chloride is NaCl because ratio of Na+ ion and Cl- ion is 1:1 in the compound. Sodium Chloride is made up of ions. A precipitation reaction is a reaction that yields an insoluble product—a precipitate— when two solutions are mixed. • i) NaCl(aq) + AgNO3 (aq) AgCl(s) + NaNO3(aq) • White ppt. • Here, Silver Chloride produced is insoluble in water and its colour is white. Convert a molecular equation into net ionic equation • i) NaCl (aq) + AgNO3 (aq) Na+(aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq) Omit spectator ions. Na+(aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq) Ag + (aq) + Cl – (aq) AgCl (s) This is the net ionic equation. AgCl(s) + NaNO3 (aq) AgCl (s) + Na+ (aq) + NO3- (aq) AgCl (s) + Na+ (aq) + NO3- (aq) Convert following molecular reaction into net ionic equation. ii) BaCl2 (aq) + Na2SO4 (aq) iii) FeCl3 (aq) + 3 NaOH (aq) iv) KOH (aq) + HNO3 (aq) v) Zn (s) + H2SO4 (aq) BaSO4 (s) + 2 NaCl (aq) White ppt Fe(OH)3 (s) + 3 NaCl (aq) reddish brown ppt KNO3 (aq) + H2O (l) ZnSO4 (aq) + H2 (g) https://youtu.be/uaBHB5GSgHU • While converting molecular equations into ionic equations, do not convert solid, liquid and gaseous substances into ions. Some more examples H2SO4 (aq) + 2 KOH (aq) K2SO4 (aq) + 2 H2O (l) 2H+ (aq) + SO4- - (aq) + 2K+ (aq) + 2OH– (aq) 2K+ (aq) + SO4- - (aq) + 2 H2O (l) Omit spectator ions. 2H+ (aq) + SO4- - (aq) + 2K+ (aq) + 2OH– (aq) 2K+ (aq) + SO4- - (aq) + 2 H2O (l) 2H+ (aq) + 2OH– (aq) 2 H2O (l) H+ (aq) + OH– (aq) H2O (l) Some more examples Na2CO3 (s) + 2 HCl (aq) 2 NaCl (aq) + H2O (l) + CO2 (g) Na2CO3 (s) + 2H+ (aq) + 2Cl- (aq) Omit spectator ions. Na2CO3 (s) + 2H+ (aq) + 2Cl- (aq) 2Na + (aq) + 2Cl -(aq) + H2O(l) + CO2(g) 2Na + (aq) + 2Cl -(aq) + H2O(l) + CO2(g) Na2CO3 (s) + 2H+ (aq) 2Na + (aq) + H2O(l) + CO2(g)