1. Describe how elements are arranged in the periodic table

2. Arranged in order of increasing atomic number.
So that elements with the same number of electrons in their outer shell fall in the same vertical column

3. In the periodic table what is a group?

4. A vertical column of elements

5. In the periodic table what is a period

6. A horizontal row of elements

7. Explain the use of the periodic table to predict the properties of elements

8. There is a trend in physical properties down many groups and across a period
we can use these trends to predict the properties of elements

9. How does the character of the elements change as you move across a period

10. Across each period there is a gradual change from non-metallic character to metallic character from right to left
Down each group the elements become more metallic in character
Between the non-metals and metals are elements with some properties of each , the metalloids

11. describe the relationship between the group number and the number of outer shell electrons

12. Elements in the same group have the same number of outer shell electrons
The period number of an element is the number of shells

13. List the general physical properties of metals

14. List the general physical properties of metals

15. Conduct electricity and heat Sonorous
Shiny when freshly cut
High melting and boiling pints
Malleable
Ductile

16. What is the name of the group 1 elements

17. Alkali metals

18. Describe lithium , potassium and sodium and state the trends in their:
melting point
Density
reaction with water

19. Relatively soft metals
Melting point decreases from lithium to potassium (with increasing atomic number)
Density increases from lithium to potassium
Reactivity with water increases from lithium to potassium

20. explain the trends in their reactivity

21. As you go down group 1 reactivity increases because it get easier to loose the outer electron:
As you go down the group atomic radius increase so the outer electron gets further away from the attractive nucleus
There are more electrons between the outer electron and nucleus reducing the attraction of the nucleus and the outer electron (shielding)

22. describe the distinguishing features of the transition metals

23. Physical properties
High melting points
High densities
Form coloured compounds
Strong and hard
Conduct electricity when solid
Chemical properties
Good catalysts
Less reactive than group 1
To not react with cold water
Most react with steam

24. Give examples of 2 transition metal catalysts and their uses

25. Iron: catalyses the synthesis of ammonia
Valadium(V)oxide : catalyses the synthesis of sulphur trioxide

26. Describe the oxidation states of the transition metals

27. They have more than one oxidation state in their compounds
Example: Iron can have an oxidation state of +2 Fe(II) or + 3 Fe(III)

28. Define an alloy

29. An alloy is a mixture made up of either two or more different metals or a metal and non-metals

30. Draw a diagram to compare an alloy to a pure metal

31. Alloy
Pure metal

32. explain in terms of their properties why alloys are used instead of pure metals

33. They are stronger. Brass is stronger than copper and does not corrode
Alloys of iron with chromium or nickel are more resistant to corrosion
Alloys of iron with tungsten are very hard and do not change shape at high temperatures
Aluminium alloyed with copper, manganese and silicon are used for making aircraft bodies because the alloy is stronger than aluminium alone and still has a low density comparable to pure aluminium

34. What word describes the arrangement of atoms in group 7 elements ie
What word describes the arrangement of atoms in group 7 elements ie . Bromine , chlorine and iodine?

35. diatomic

36. Define the term halide

37. halogen atom that has gained an electron to form a negative ion

38. Describe the trend in colour and reaction with halide ions as you go down group 7 from chlorine to iodine

39. Describe the trend in colour from chlorine to iodine

40. The colours get darker and more intense down the group

41. State the colour of chlorine gas

42. Yellow - green

43. State the colour of bromine

44. Red-brown

45. State the difference in colour between iodine as a solid , gas and aqueous

46. Solid iodine = grey-black
Iodine vapour = purple
Aqueous iodine = brown

47. Describe the solubility of iodine

48. Iodine is relatively insoluble in water
But soluble in aqueous potassium iodide

49. Describe the trends in physical properties of the halogens

50. The melting points and boiling points increase down the group
The density (of the liquid) increases down the group

51. Describe how the halogens react with halide ions

52. A displacement reaction is one in which one type of atom or ion replaces another in a compound
A more reactive halogen will replace a less reactive one in a compound
Example:
Cl2 + 2KI  2KCl + I2
chlorine is more reactive than iodine so it displaces it from KI

53. A displacement reaction is one in which one type of atom or ion replaces another in a compound
A more reactive halogen will replace a less reactive one in a compound
Example:
Cl2 + 2KI  2KCl + I2
chlorine is more reactive than iodine so it displaces it from KI

54. What type of reaction occurs between halogens in a displacement reaction

55. A redox reaction

56. Draw a results table for an experiment looking at the relative reactivities of the halogens

57. Draw a results table for an experiment looking at the relative reactivities of the halogens
Potassium chloride
Potassium bromide
Potassium iodide
chlorine
No reaction
reaction
bromine
iodine

58. Describe the noble gases

59. Have a full outer shell so are
Unreactive (already have full outer shell)
Monatomic gases(do not need to form bonds as already have full outer shell)
Their densities increase as you go down the group
Are monoatomic

60. State the uses of the noble gases

61. Helium is used for filling balloons because it is less dense than air and does not burn
A mixture of helium and oxygen is used in breathing apparatus for deep sea divers
Neon, argon and xenon are used in advertising signs
Argon is used in providing an inert atmosphere in welding
Argon is used to fill electric bulbs because it is inert