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__**Instruction **__
 * You are to work in pairs
 * You will be assigned a group in the periodic table to research.
 * Research the group, using the checklist below.
 * Once you have finished your research you are to add your information into this Wikispaces page.
 * DO NOT CHANGE information that another member of the class has added.
 * Include a bibliography of at least two different sources of information other than the textbook.

__**Checklist** __ Your presentation must include the following:

1. Information on each element (Name, discovery date, chemical symbol, atomic number, atomic mass, number of protons, electrons, neutrons, physical state at room temperature and pressure, density, melting point, boiling point and atomic radius) You can use the Ms Excel spreadsheet below to collate the information you have collected for 1.  2. Images of the elements in your group 3. Trends down the group 4. Common compounds these elements form 5. Uses of these elements and/or their compounds. <span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">6. A scientific explanation why they are suitable for that particular use

__**<span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">Sources **__ <span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">Information on the different groups can be found from pages 28 to 32 of your textbook. <span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">You might also want to search the internet and Mrs Adams Blog for further resources to help you. <span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">The dynamic Periodic Table (link attached below) provides a good source of information on each element, which would then help you to recognise trends down a group.



Dynamic Periodic table

__**<span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">Organisers **__ <span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">Before you get started, it might be a good idea for you to use one of the graphic organisers below to help you get organised!

<span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">

__**<span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">Rubric **__ <span style="font-family: 'Comic Sans MS',cursive; font-size: 130%;">The rubric for this assessment task can be found here ->


 * <span style="font-family: 'Comic Sans MS',cursive; font-size: 160%;">These Web pages will be due on 15 November 2010 **

<span style="font-family: 'Tahoma','sans-serif'; font-size: 14pt; margin: 0cm 0cm 0pt;">Alkali Metals: <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Alkali metals also known as alkaline metals, Group I. This family consists of the elements Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr). They are all very reactive because they all have only one electron on their outer shell, making them unbalanced. You will find that alkali metals are shiny and light in weight, they are never found in elemental forms in nature, and are soft metals of low density.

__<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Element: Rubidium __ <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Symbol: Rb <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Appearance: Rubidium is a soft, silvery-white metallic element, solid at room temperature.

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">State: Solid

<span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">Rubidium in a glass tube.

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Atomic Number: 37 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Atomic Mass: 85,4678g <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Number of Protons/electrons: 37 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Density: <span style="font-family: 'Arial','sans-serif';"> 1.532 g/cm3 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Number of shells: 5 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Melting point: 312 <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">oC <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Boiling Point: 961 <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">oC

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Discovery Date: Rubidium was discovered by Robert Bunsen and Gustav Kirchhoff in 1861. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">The Uses of the Element: Rubidium has been used in dating rocks, gives a purple colour for fireworks and Rubidium salts are used in glasses and ceramics. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Reactivity: Rubidium reacts violently in water, forming corrosive rubidium hydroxide (RbOH) and hydrogen gas, which is formed by the heat of the reaction. Rubidium burns with a reddish-violet flame colour. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">[|http://www].Chemicool.com/elements/rubidium.html

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Element: Cesium <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Symbol: Cs <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Appearance: Cesium is silvery-gold <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">State: solid

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Atomic Number: 55 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Number of protons/electrons: 55 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Density: <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;"> 1.873 g/cm3 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Number of shells: 6 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Melting Point: 28.4 <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">oC <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Boiling Point: 670 <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">oC <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Discovery: Cesium was discovered by Robert Bunsen and Gustav Kirchhoff in 1860. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Uses of the Element: Cesium is used in atomic clocks which are extremely accurate, also used in photoelectric cells and used as a getter in vacuum tubes. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Reactivity: Cesium is extremely reactive; it reacts explosively to water producing Cesium Hydroxide (CsOH), an extremely strong base that can rapidly corrode glass.

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">http://www.chemicalelements.com/elements/cs.html

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Element: Francium <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Symbol: Fr <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Appearance: Francium is metallic, it a heavy unstable, radioactive metal. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">State: solid

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Atomic Number: 87 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Number of protons/Electrons: 87 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Density: <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;"> 1.873 g/cm3 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Number of shells: 7 <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Melting Point: 27 <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">oC <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt;">Boiling Point: 677 <span style="color: #29303b; font-family: 'Arial','sans-serif'; font-size: 11pt;">oC

<span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Discovery: Francium was discovered by Marguerite Perey in 1939. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Uses of the Element: There are no uses for Francium due to it being rare and unstable. <span style="font-family: 'Tahoma','sans-serif'; font-size: 11pt; margin: 0cm 0cm 0pt;">Reactivity: Francium is not available in sufficient quantities to show it reacting in water, because Francium is the second rarest element in the Earth’s crust because there is less than thirty grams Francium exists on Earth. In theory Francium would be more reactive than cesium and sodium.