1. Sb + Cl 2 SbCl Mg + O 2 MgO _. 3. CaCl 2 Ca + Cl NaClO 3 NaCl + O Fe + HCl FeCl 2 + H CuO + H 2 Cu + H 2 O

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1 Year 11 Chemistry Balancing Equations 1. Sb + Cl 2 SbCl 3 2. Mg + O 2 MgO _ 3. CaCl 2 Ca + Cl 2 4. NaClO 3 NaCl + O 2 5. Fe + HCl FeCl 2 + H 2 6. CuO + H 2 Cu + H 2 O 7. Al + H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 8. MgBr 2 + Cl 2 MgCl 2 + Br 2 9. SnO 2 + C Sn + CO 10. Pb(NO 3 ) 2 + H 2 S PbS + HNO HgO Hg + O KClO 3 KCl + O N 2 + H 2 NH NaBr + Cl 2 NaCl + Br Zn + AgNO 3 Zn(NO 3 ) 2 + Ag 16. Sn + Cl 2 SnCl Ba(OH) 2 BaO + H 2 O 18. Mg(OH) 2 + HCl MgCl 2 + H 2 O 19. Na 2 CO 3 + HCl NaCl + H 2 CO NH 4 NO 2 N 2 + H 2 O 21. N 2 + O 2 N 2 O MgCO 3 MgO + CO KBr + Cl 2 KCl + Br Zn + CuSO 4 Cu + ZnSO P + O 2 P 4 O SrBr 2 + (NH 4 ) 2 CO 3 SrCO 3 + NH 4 Br 27. AgNO 3 + (NH 4 ) 2 CrO 4 Ag 2 CrO 4 + NH 4 NO K + H 2 O KOH + H Al + Pb(NO 3 ) 2 Al(NO 3 ) 3 + Pb 30. Fe + O 2 Fe 3 O 4 1

2 Chemistry: Atomic Number and Mass Number Complete the following chart and answer the questions below. Element Name Atomic Number Number of Protons Number of Neutrons Mass Number 23 Na 11 Mass Number Symbol for Sodium Atomic Number 11 Protons carbon hydrogen hydrogen 2 nitrogen cesium tungsten silver 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

3 Complete the following questions 1. Isotope Element Atomic Number Mass Number Number of Neutrons Number of Electrons Electron Shell Configuration 12 6 C Carbon , C 2, C H Ca Al Argon 20 Silicon 30 Iodine 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 d. An atom with Period 3, Group V b. An atom with atomic number 17 e. A sulfur atom c. An atom in Period 2, Group III 3

4 7. Draw the electronic arrangement for the following elements a. oxygen b. sodium c. sulfur d. potassium 8. 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

5 12. 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) 13. 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

6 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 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 V 20 10W a Which two atoms have the same number of neutrons? b c d 40 19X 39 19Y Z Which atom has the smallest mass number? Which two atoms belong to the same element? 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. CO 2 does not change when you balance the equation but you may have 2CO 2 or 3CO 2 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 MgCl 2. b. Dilute nitric acid HNO 3 is added to solid calcium carbonate CaCO 3, producing bubbles of carbon dioxide, water, and the soluble salt calcium nitrate Ca(NO 3 ) 2 c When dilute sodium sulfate Na 2 SO 4 solution is added to dilute barium nitrate Ba(NO 3 ) 2 solution, barium sulfate BaSO 4 precipitates, leaving sodium nitrate NaNO 3 in solution. d Dilute sodium hydroxide is added to dilute sulfuric acid H 2 SO 4, producing water and the soluble salt sodium sulfate Na 2 SO 4 e Dilute sulfuric acid is poured over solid sodium carbonate Na 2 CO 3, producing carbon dioxide, water and the soluble salt sodium sulfate. 6

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