8.1 Arrangement of elements
1. How is the Periodic Table organized in terms of the number of protons?
It is arranged in order of increasing proton number or atomic number.
2. In what structures are elements placed within the Periodic Table?
Elements are arranged in periods and groups.
3. Describe the change in character that occurs as you move across a period from left to right.
There is a change from metallic to non-metallic character across a period.
4. What is the relationship between an element's group number and the charge of the ions it forms?
There is a direct relationship between the group number and the charge of the ions formed from elements in that group.
5. Why do elements in the same group of the Periodic Table exhibit similar chemical properties?
They have similar chemical properties because they share similar electronic configurations.
6. How can an element's position in the Periodic Table be used to understand its behavior?
Its position can be used to predict its properties.
7. What should you be able to do if given information about various elements in a specific group?
You should be able to identify trends within that group.
8.2 Group I properties
8. Name the specific Group I alkali metals listed in the syllabus and describe their general physical hardness.
The metals are lithium, sodium, and potassium, and they are relatively soft metals.
9. What is the general trend for melting points as you move down Group I?
There is a trend of decreasing melting point down the group.
10. Describe the general trend for density as you move down the elements in Group I.
There is a trend of increasing density down the group.
11. Describe the general trend for reactivity as you move down the Group I alkali metals.
There is a trend of increasing reactivity down the group.
12. What should you be able to do if provided with information about specific elements in Group I?
You should be able to predict the properties of other elements in Group I.
8.3 Group VII properties
13. Name the three Group VII halogens mentioned in the syllabus and state their molecular nature.
The halogens are chlorine, bromine, and iodine, and they are diatomic non-metals.
14. What is the general trend for density as you move down Group VII?
There is a trend of increasing density down the group.
15. Describe the general trend for reactivity as you move down the elements in Group VII.
There is a trend of decreasing reactivity down the group.
16. State the appearance of chlorine at room temperature and pressure (r.t.p.).
Chlorine is a pale yellow-green gas.
17. State the appearance of bromine at room temperature and pressure (r.t.p.).
Bromine is a red-brown liquid.
18. State the appearance of iodine at room temperature and pressure (r.t.p.).
Iodine is a grey-black solid.
19. Describe and explain the displacement reactions that occur with halogens and other halide ions.
A more reactive halogen will displace a less reactive halogen from an aqueous solution of its halide ions.
20. What should you be able to do if given information about specific elements in Group VII?
You should be able to predict the properties of other elements in Group VII.
8.4 Transition elements
21. List four general physical and chemical properties that characterize transition elements as metals.
They have high densities, have high melting points, form coloured compounds, and often act as catalysts both as elements and in compounds.
22. What unique chemical characteristic do transition elements have regarding their ions?
They have ions with variable oxidation numbers, such as iron(II) and iron(III).
8.5 Noble gases
23. Describe the reactivity and molecular state of Group VIII noble gases.
They are unreactive, monatomic gases.
24. Explain why noble gases are unreactive by referring to their electronic configuration.
They are unreactive because they have a full outer electron shell, which is a stable arrangement.