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Year 11 Chemistry Balancing Equations 1. ____ Sb + ____ Cl2 ____SbCl3 2. ____ Mg + ____O2 ____MgO 3. ____ CaCl2 ____ Ca + ____ Cl2 4. ____ NaClO3 ____ NaCl + ____ O2 5. ____ Fe + ____ HCl ____ FeCl2 + ____ H2 6. ____ CuO + ____ H2 ____ Cu + ____ H2O 7. ____ Al + ____ H2SO4 ____ Al2(SO4)3 + ____ H2 8. ____ MgBr2 + ____ Cl2 ____ MgCl2 + ____ Br2 9. ____ SnO2 + ____ C ____ Sn + ____ CO 10. ____ Pb(NO3)2 + ____ H2S ____ PbS + ____ HNO3 11. ____ HgO ____ Hg + ____ O2 12. ____ KClO3 ____ KCl + ____ O2 13. ____ N2 + ____ H2 ____ NH3 14. ____ NaBr + ____ Cl2 ____ NaCl + ____ Br2 15. ____ Zn + ____ AgNO3 ____ Zn(NO3)2 + ____ Ag 16. ____ Sn + ____ Cl2 ____ SnCl4 17. ____ Ba(OH)2 ____ BaO + ____ H2O 18. ____ Mg(OH)2 + ____ HCl ____ MgCl2 + ____ H2O 19. ____ Na2CO3 + ____ HCl ____ NaCl + ____ H2CO3 20. ____ NH4NO2 ____ N2 + ____ H2O 21. ____ N2 + ____ O2 ____ N2O5 22. ____ MgCO3 ____ MgO + ____ CO2 23. ____ KBr + ____ Cl2 ____ KCl + ____ Br2 24. ____ Zn + ____ CuSO4 ____ Cu + ____ ZnSO4 25. ____ P + ____ O2 ____ P4O6 26. ____ SrBr2 + ____ (NH4)2CO3 ____ SrCO3 + ____ NH4Br 27. ____ AgNO3 + ____ (NH4)2CrO4 ____ Ag2CrO4 + ____ NH4NO3 28. ____ K + ____ H2O ____ KOH + ____ H2 29. ____ Al + ____ Pb(NO3)2 ____ Al(NO3)3 + ____ Pb 30. ____ Fe + ____ O2 ____ Fe3O4 _ 1 Mass Number Chemistry: Atomic Number and Mass Number 23 Na 11 Complete the following chart and answer the questions below. Element Name Atomic Number Number of Protons Symbol for Sodium Atomic Number 11 Protons Number of Neutrons carbon Mass Number 12 8 8 hydrogen 1 6 hydrogen 14 2 nitrogen 14 1 92 2 146 cesium 82 11 12 47 tungsten 108 110 45 24 80 52 89 silver 152 107 76 114 How are the atomic number and the number of protons related to each other? How do the number of protons, number of neutrons, and the mass number relate to each other? What is the one thing that determines the identity of an atom (that is, whether it is an oxygen atom or a carbon atom, etc.)? 2 Complete the following questions 1. Isotope 12 6 C Element Atomic Number Mass Number Carbon 6 12 Number of Neutrons Number of Electrons Electron Shell Configuration 6 2, 4 2, 4 13 6 C 14 6 C 12 23 H 1 Ca 20 1 1 40 20 27 13 Al Argon Silicon Iodine 20 30 127 74 2. If an element has two electrons in its outer shell, is it a metal or non-metal? Explain your answer __________________________________________________________________________________ __________________________________________________________________________________ ___________________________________________________________________________________ 3. What is special about elements that have eight electrons in their outer shell? ___________________________________________________________________________________ ________________________________________________________________________________ 4. How many shells are filled or partly-filled for a Period 3 element? ______________________________________________________________ 5. State the number of outer shell electrons for elements in: a. Group 1 ________ b. Group 3 ________ c. Group 7 ________ d. Group 5 ________ 6. How many electrons do the following have? a. An atom with 6 protons ________ b. An atom with atomic number 17________ c. d. An atom with Period 3, Group V ________ e. A sulfur atom ________ An atom in Period 2, Group III ________ 3 7. Draw the electronic arrangement for the following elements a. oxygen b. sodium c. sulfur 8. d. potassium What is the difference between an element and a compound? 9. Explain the following terms: A isotopes B mass number C subshell D valence electron E orbital F ground state 10. Compare the mass and charge of protons, electrons and neutrons. 11. What is the maximum number of electrons in the second shell?___________________ 4 12. 13. Discuss the contributions made to our understanding of the atom by the following scientists: A John Dalton B J J Thompson C James Chadwick D Ernest Rutherford E Niels Bohr F Erwin Schrodinger (write your answers in your chemistry module) Write out the electron configuration for each of the following elements. 1. H 2. Li 3. Na 4. K 5. Rb 6. Be 7. Mg 8. Ca 9. Sr 10. C 11. O 12. S 13. F 14. Cl 15. Br 16. I 17. He 18. Ne 19. Ar 20. Kr 21. Xe 22. F Looking over your electron configurations, are there any elements above that have similar valence electron configurations to those of other elements? If so, list below the elements that are similar (in terms of valence electrons) and state the similarity for each of the groups. 5 14. Give the chemical symbol for any element: a in the same group as fluorine (F) _______________ b in the same period as sodium (Na) ________________ c in the group known as the alkali metals _____________ d that would form ions of charge 3 _________________ 15. List three properties of non-metals 16. List three properties of metals. 17. Listed below are five atoms using symbols that are not the usual symbols of the elements. Use the letters V to Z to answer the following questions. 40 18 V 20 10 W 40 19 X 39 19 Y 40 20 Z a Which two atoms have the same number of neutrons? ________________ b Which atom has the smallest mass number? ____________________ c thesameelement? _____________________ Which two atoms belong to d Which two symbols represent noble gases? _______________________ 18. State one way in which helium (He) is: a like all other gases in Group VIII b different from all other gases in Group VIII 19. Write balanced chemical equations, including subscripts, for each of the following reactions. Follow these steps: • Write the word equation for the reaction. • Directly underneath the word equation, write the unbalanced formula equation. • Add subscripts—(s), (l), (g) or (aq). • Balance the equation. (don’t change any FORMULA e.g. CO2 does not change when you balance the equation but you may have 2CO2 or 3CO2 etc.) Note: ‘Dilute’ means a water solution, and therefore the appropriate subscript is (aq) Write these equations in your moodule a. Dilute hydrochloric acid HCl is added to solid magnesium hydroxide Mg(OH)2, producing water and the soluble salt magnesium chloride MgCl2. b. Dilute nitric acid HNO3 is added to solid calcium carbonate CaCO3, producing bubbles of carbon dioxide, water, and the soluble salt calcium nitrate Ca(NO3)2 c When dilute sodium sulfate Na2SO4 solution is added to dilute barium nitrate Ba(NO3)2 solution, barium sulfate BaSO4 precipitates, leaving sodium nitrate NaNO3 in solution. d Dilute sodium hydroxide is added to dilute sulfuric acid H2SO4, producing water and the soluble salt sodium sulfate Na2SO4 e Dilute sulfuric acid is poured over solid sodium carbonate Na2CO3, producing carbon dioxide, water and the soluble salt sodium sulfate. 6 7 8