A1 Models of the atom. A2 Size of the atom

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1 A1 Models of the atom 1. Describe the improvements to our understanding of the atom from each of the following scientists: 1.1. Democritus 1.2. Dalton 1.3. Thomson 1.4. Rutherford 1.5. Bohr 1.6. Chadwick 2. What is meant by the term model in a scientific context? 3. Describe what Rutherford saw in his experiment. A2 Size of the atom 1. Give the mass (in kg) of a/an: 1.1. Electron 1.2. Proton 1.3. Neutron 2. How many times heavier is a proton than an electron? 3. What does amu stand for? 4. Which element is used to determine the size of one amu? 5. Give the masses of the following elements in kg: 5.1. Potassium 39 amu 5.2. Chromium 52 amu 5.3. Silicon 28 amu 5.4. Hydrogen 1 amu 6. Give the masses of the following in amu: 6.1. One atom of helium 6, kg 6.2. One atom of magnesium 4, kg 6.3. One molecule of oxygen 5, kg 6.4. An ant kg 6.5. A dog 20 kg

2 A3 Structure of the atom 1. The 3 particles of the atom are: a. b. c. Their respective charges are: a. b. c. 2. The number of protons in one atom of an element determines the atom s, and the number of electrons determines the of the element. 3. The atomic number tells you the number of in one atom of an element. It also tells you the number of in a neutral atom of that element. The atomic number gives the identity of an element as well as its location on the periodic table. No two different elements will have the atomic number. 4. The of an element is the average mass of an element s naturally occurring atom, or isotopes, taking into account the of each isotope. 5. The of an element is the total number of protons and neutrons in the of the atom. 6. The mass number is used to calculate the number of in one atom of an element. In order to calculate the number of neutrons you must subtract the from the. 7. Give the symbol of and the number of protons in one atom of: Lithium Iron Oxygen Krypton Bromine Copper Mercury Helium

3 8. Give the symbol of and the number of electrons in a neutral atom of: Uranium Boron Chlorine Iodine Xenon 9. Give the symbol of and the number of neutrons in one atom of: (Mass numbers are ALWAYS whole numbers show your calculations) Barium Carbon Fluorine Europium Bismuth Hydrogen Magnesium Mercury 10. Name the element which has the following numbers of particles: a. 26 electrons, 29 neutrons, 26 protons b. 53 protons, 74 neutrons c. 2 electrons (neutral atoms) d. 20 protons e. 86 electrons, 125 neutrons, 82 protons f. 0 neutrons 11. If you know ONLY the following information can you ALWAYS determine what the element is? (Yes/No) a. Number of protons b. Number of neutrons c. Number of electrons in a neutral atom d. Number of electrons

4 12. Fill in the missing items in the table below. Unless otherwise stated, all atoms are neutral Name Symbol Z A No of No of No of Standard protons electrons neutrons notation 1 Na Potassium P Iron Silver 36 W

5 A4 Isotopes 1. Define the term isotope 2. In each of the following cases, calculate relative atomic mass of an atom in a sample of the element ,9 % boron 10 and 80,1 % boron % Mg 24, 10% Mg 25 and 11% Mg % lithium 4 and 3% litium-6 3. An element has two stable isotopes, one of which is X-25, which occurs naturally as 18,29%. If the relative atomic mass of an atom of element X is 27,70, determine the atomic mass of the other isotope. 4. For the element Au, use standard notation to give an isotope that has: more neutrons fewer neutrons A5 Electron configuration 1. Complete the following sentence: Electrons with lower energy are found the nucleus, while electrons with a higher energy are found the nucleus. 2. Sketch the shape formed by the 2s orbital and the 2p orbitals. 3. Give the number of electrons that are found in: 3.1. The 1 st energy level 3.2. The 2 nd energy level 3.3. The 3s orbital 3.4. The 2p orbital 3.5. The 3p orbital 4. Sketch the Aufbau diagram for the following atoms/ions 4.1. O 4.2. He 4.3. Na 4.4. S 4.5. F 4.6. C

6 4.7. Cl 4.8. Be 4.9. Li P H Ca He 5. Write out the electron configuration for the following atoms/ions B 5.2. N 5.3. O 5.4. Al 5.5. H 5.6. Ne 5.7. Na 5.8. Cl B F - 6. State Pauli s exclusion principle 7. For each of the following atom, state the number of: i) Valence electrons ii) Core electrons iii) Lone pairs iv) Unpaired electrons 7.1. C 7.2. S 7.3. N 7.4. O 7.5. Li 7.6. Al 7.7. Cl 7.8. Ar 7.9. H Ca 8. Explain why, on the right side of the table, fluorine is most reactive element in its column. 9. Explain why, on the left side of the table, caesium is most reactive element in its column.

7 A6 The periodic table 1. Give the names of 3 elements that are in the: 1.1. Same group of the periodic table as sulphur 1.2. Same period of the periodic table as zinc 1.3. Nobel gases 1.4. Alkali metals 1.5. Halogens 1.6. Alkaline-earth metals 2. With regards to their electron structure, what do the following elements all have in common: 2.1. O, S and Se 2.2. Li, B and F 3. Explain why the size of atoms decreases across a period from left to right 4. Explain what is meant by the term electronegativity. 5. Explain why the electronegativity of atoms decreases down a group. 6. Explain why the ionization energy increases across a period from left to right. A7 Bonding Name the following ionic compounds: 1. NaBr 2. CaO 3. Li 2S 4. MgBr 2 5. Be(OH) 2 Write the formulas for the following ionic compounds: 6. potassium iodide 7. magnesium oxide 8. aluminum chloride 9. sodium nitrate 10. calcium carbonate 11. lithium sulfate 12. beryllium phosphide 13. magnesium hydroxide 14. sodium phosphate 15. aluminum carbonate 16. calcium chloride 17. aluminum oxide

8 18. ammonium chloride 19. chromium (VI) phosphate 20. vanadium (IV) carbonate 21. tin (II) nitrite 22. cobalt (III) oxide 23. vanadium (V) sulphide 24. chromium (III) hydroxide 25. lithium iodide 26. lead (II) nitride Write the names of the following covalent compounds: 27. SO N 2S 29. PH BF P 2Br CO 33. SiO SF NH NO 2 Write the formulas of the following covalent compounds: 37. nitrogen trichloride 38. boron carbide 39. dinitrogen trioxide 40. phosphorus pentafluoride 41. sulfur dibromide 42. diboron tetrahydride 43. oxygen difluoride 44. carbon disulphide 45. nitrogen monoxide Draw Lewis diagrams for the following atoms 46. N 47. Cl 48. K 49. Na 50. Al 51. H 52. P 53. Ne 54. O

9 55. Define the term covalent bond and give an example of three substances that contain only covalent bonds. 56. Consider the list below, and decide whether the following substances are held together by COVALENT, IONIC or METALLIC bonds. MgO, NH 3, water, H 2, LiCl, CuSO 4, PbSn, NO, HBr, carbon dioxide, NaCO 3, AlN, K 2Cr 2O 7, AgAu, SiO With the aid of a sketch, explain how atoms are held together in a metallic bond. 58. Use Lewis diagrams to show how the following substances combine by forming covalent bonds: H and N C and O C and Cl H and O 59. Use Lewis diagrams to show how the following substances combine by forming ionic bonds: Li and O Mg and Cl Na and P K and Br Ca and N 60. Write down the formulae (including charge) for the following compound ions: Sulphate Carbonate Nitrate Hydroxide Ammonium 61. Calculate the relative molecular mass of the following covalent substances: CO HCN H 2O B 2O H 2SO Calculate the relative formula mass of the following ionic substances: CuSO CaO Zn(NO 3) Li 2O

10 62.5. Al 2(Cr 2O 7) Fe(MnO 4) NH 4NO 3

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