C1 Atomic Structure and Periodic Table Knowledge Organiser PDF

# C1 ATOMIC STRUCTURE AND THE PERIODIC TABLE KNOWLEDGE ORGANISER ## Question 1. Define atom 2. Draw a labelled diagram of an atom, labelling the subatomic particles 3. Define element 4. Define compound 5. Define molecule 6. Define mixture 7. Describe what filtration is used for 8. Give two example...

# C1 ATOMIC STRUCTURE AND THE PERIODIC TABLE KNOWLEDGE ORGANISER ## Question 1. Define atom 2. Draw a labelled diagram of an atom, labelling the subatomic particles 3. Define element 4. Define compound 5. Define molecule 6. Define mixture 7. Describe what filtration is used for 8. Give two examples of uses of filtration 9. Describe the process of crystallisation 10. Give an example of where we might use crystallisation 11. Describe the process of crystallisation to produce large, regularly shaped crystals 12. Describe what we would use distillation for 13. Describe a use for distillation 14. Explain how simple distillation works 15. Describe what paper chromatography is used for 16. Describe the two 'phases' of chromatography 17. Explain why different inks would move up the chromatography paper by different amounts 18. Describe the difference in appearance of the chromatogram for pure and impure substances 19. Explain these results from the chromatogram 20. Explain how a paper chromatogram can be used to identify two substances that are the same 21. State the three subatomic particles 22. State the masses of the subatomic particles 23. State the relative charges of the subatomic particles 24. How are the subatomic particles arranged in an atom? (3 marks) 25. What is the plum pudding model of the atom? 26. What did the gold foil experiment prove? 27. What is the atomic number of an atom? 28. What is the mass number of an atom? 29. How do you calculate the number of neutrons in an atom? 30. How are the electrons arranged in atoms? 31. How many electrons can go in the first shell? 32. How many electrons can go in the second and third shells? 33. Draw the electronic structure for oxygen (use the periodic table) 34. Write the electronic structure for potassium 35. Draw the electronic structure for magnesium 36. What are groups in the periodic table? 37. What can the group tell you about the electrons in an atom? 38. What are periods in the periodic table? 39. What can the period tell you about the electrons in an atom? 40. How did Mendeleev arrange elements in the periodic table? 41. Why did Mendeleev put some elements in groups? 42. Why did Mendeleev leave gaps in his periodic table? 43. Iodine has a lower atomic weight than tellurium, so iodine should be placed before tellurium in Mendeleev's periodic table. However, he placed iodine after tellurium. Explain why 44. How do isotopes explain the need for the reversal of iodine and tellurium? 45. How is the modern periodic table arranged? - In order of increasing atomic number - elements with similar properties are placed in vertical columns, called groups 46. State the equation for relative atomic mass 47. What is an ion? 48. How many electrons does calcium have? 49. How many electrons does silicon have? 50. How are the electrons in sulphur arranged? 51. How are the electrons in magnesium arranged? 52. How many electrons are in the outer shell of boron? 53. How many electrons are in the outer shell of phosphorous? 54. How many electrons are in the outer shell of sodium? 55. An element has three shells and three electrons in the outer shell. What element is it? 56. How many electrons are in the outer shell of Gallium? 57. In terms of electrons, what do group 1 elements have in common? 58. In terms of electrons, what do group 7 elements have in common? 59. In terms of electrons, what do group o elements have in common? 60. What is more reactive, lithium or sodium? 61. What is more reactive, chlorine or bromine? 62. Define inert 63. Explain why the noble gases are inert 64. What is a trend? 65. State the trend in the melting points of the alkali metals 66. Define isotope 67. State the number of protons, neutrons and electrons in 236C 68. What state is fluorine at room temperature? 69. What state is chlorine at room temperature? 70. What state is bromine at room temperature? 71. What state is iodine at room temperature? 72. Describe the observations when lithium reacts with water 73. Describe the observations when sodium reacts with water 74. Write the word equation for the reaction between sodium and water 75. Describe the observations when potassium reacts with water 76. Balance the equation: Li + H2O→LIOH + H₂ 77. Balance the equation: K + H2O→ KOH + H₂ 78. Name LiOH 79. Name KOH 80. Explain why the group 1 elements are called alkali metals 81. Explain how you would prove that potassium hydroxide had been produced in the reaction between potassium and water 82. What is a displacement reaction? 83. Explain why the following reaction does not proceed: KBr + 12 84. Balance the below equation and explain why it is a displacement reaction: KBr + Cl2→ KCI + Br2 85. Explain why fluorine is more reactive than chlorine 86. Explain why potassium is more reactive than lithium (3 marks) 87. Explain why bromine is less reactive than chlorine (3 marks) 88. Explain why sodium is less reactive than caesium (3 marks) # C2 BONDING, STRUCTURE AND THE PROPERTIES OF MATTER KNOWLEDGE ORGANISER ## Question 1. What charge do electrons have? 2. What charge will an ion of lithium take? 3. What charge will an ion of beryllium take? 4. What charge will an ion of barium take? 5. What charge will an ion of fluorine take? 6. If something has gained electrons, what charge will it have? 7. If something has lost electrons, what charge will it have? 8. What charge will an ion of oxygen take? 9. What charge will an ion of Selenium take? 10. Why do atoms transfer electrons in ionic bonding? 11. Explain in terms of electrons what occurs when lithium bonds with fluorine 12. Explain in terms of electrons what occurs when magnesium bonds with oxygen 13. Explain in terms of electrons what occurs when magnesium bonds with chlorine 14. Explain in terms of electrons what occurs when sodium bonds with oxygen 15. Why do sodium ions and chlorine ions form an ionic bond? 16. Why don't sulphur ions and oxygen ions form ionic bonds with each other? 17. What is the name for a substance made of billions of oppositely charged ions joined together? 18. State the melting points of ionic substances 19. Explain why ionic substances have high melting points. 20. Will NaCl(s) conduct electricity? 21. Will NaCl (aq) conduct electricity? 22. Will NaCl (l) conduct electricity? 23. What does molten mean? 24. Explain why ionic compounds do not conduct electricity when solid 25. Explain why ionic compounds conduct electricity in solution 26. Explain why ionic compounds conduct electricity when molten 27. What does soluble mean? 28. What does insoluble mean? 29. Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity? 30. Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is 31. Explain why chlorine and fluorine form covalent bonds 32. Complete the sentence: In covalent bonds, electrons are 33. In ionic bonds, electrons are 34. Draw a dot and cross diagram for methane CH4 35. What is the name given to the structure of diamond, graphite and sillicon dioxide? 36. How many bonds does each carbon have in diamond? 37. Explain why diamond has a high melting point 38. Explain why most giant covalent substances do not conduct electricity 39. Explain why graphite conducts electricity 40. Explain why graphite can act as a lubricant 41. What is graphene? 42. What is a fullerene? 43. What type of substance are methane and water? 44. What is a molecule? 45. Describe the structure of simple covalent molecules 46. What are intermolecular forces? 47. Explain why methane has a low melting point 48. What is a polymer? 49. Describe the main features of metals in terms of their structure 50. Explain why metals can conduct electricity 51. Explain why pure metals are soft 52. What is an alloy? 53. Give a reason for alloying a metal 54. Explain why alloys can be harder than pure metals # C3 QUANTITATIVE CHEMISTRY KNOWLEDGE ORGANISER ## Question 1. A sample of magnesium is heated in air and the mass increases. Explain why. 2. A sample of magnesium is added to acid and it starts bubbling. What will happen to the mass? Explain your answer. 3. A student mixes two colourless and clear solutions together, and a white solid forms. The mass stays the same. Explain why. 4. A student reacts 20g of solid with a gas and the mass of the resulting solid is found to be 30g. What mass of gas reacted? 5. The student actually started with 25g of gas. Explain why the mass did not increase to 459. 6. Calculate the relative formula mass of: * KCI * HNO3 * VF5 * KMnO4 * LiO * H2O2 * Ba(OH)2 * (NH4)2SO4 7. In the reaction below, K and LiBr react together to form KBr and a second substance. Calculate the Mr of the reactants and the known product: K + LiBrO KBr + ? - Determine the Mr of the unknown product and identify what it is. 8. How many atoms are in a mole of atoms? 9. How many atoms are in two moles of atoms? 10. How many electrons are in ten moles of electrons? 11. How many electrons are in 0.8 moles of electrons? 12. State the equation linking mass, Mr and moles 13. One mole of atom A has a mass of 32g. What would the mass of 0.06 moles of atom A be? 14. A molecule has 12 electrons. How many electrons are in one mole of that molecule? 15. Calculate the number of electrons in H₂SO₄ 16. How many electrons would be in 2 moles of H₂SO₄? 17. How many electrons would be in 12 moles of (NH4)₃PO₄? 18. What is the Mr of (NH4)₃PO₄? 19. What is the Mr of Li₂O? 20. How many moles are in 40g of K2Cr2O7? 21. What is the Mr of a substance if 3.2 moles has a mass of 100g? 22. What is the mass of 4 moles of a substance with an Mr of 84? 23. Calculate the Mr of a substance with a mass of 250g that contains 8 moles 24. What is the mass of 0.8 moles a substance with an Mr of 25? 25. How many moles are in 25g of CO₂? 26. How many atoms of H are there in 2 moles of HBr? 27. Find the empirical formula of each of the following substances. a) N 82.4%, Η 17.6% 28. Draw a molecule of oxygen gas (O2) 29. How many moles are in 200g of oxygen gas? 30. How many electrons are in 200g of oxygen gas? 31. How many electrons are in 150g of oxygen gas? 32. Ozone has three oxygen atoms all chemically bonded. What is its Mr? 33. What is the mass of 10 moles of O3? 34. The following questions relate to this equation: N2 + H2O NH3 * a. Balance the equation * b. What is the ratio of nitrogen molecules to hydrogen molecules in ammonia NH3? * c. If 6 H₂ molecules are used, how many NH3 molecules can be formed? * d. If 4 moles of N₂ are used, how much H₂ is needed? * e. If 7.2 moles of H₂ are used, how much N₂ is needed and how much NH3 can be formed? 35. What is the mass of 15 moles of NH3? 36. This question relates to this chemical reaction: AICI3 + F2 AIF3 + Cl2 * a. Balance the equation * b. 2 moles of AlCl3 are used. How much F₂ is needed? * c. What is the Mr of AICI3? * d. What mass of AlF3 equates to 43 moles? * e. How many atoms are in 43 moles of AIF3? 37. This question relates to this chemical reaction: KCI + F2 KF + Cl2 * a. Balance the equation * b. 10g of F₂ are used. What mass of KCI is required? 38. 140 g of nitrogen (N2) reacts with 30 g of hydrogen (H2) to form ammonia. Use this information to construct a balanced symbol equation for this reaction. 39. What mass of calcium hydroxide is formed when 10.0 g of calcium oxide reacts with 10.0 g of water? CaO + H2O → Са(ОН)2