Group+1Hr7

Lithium
1s^2 2s^1 n= 2 l= 0 ml= 0 ms= + 1/2

Atomic Number: 3 Atomic Mass: 7 Protons: 3 Neutrons: 4 Electrons: 3 Isotopes: 5

Lithium is very soft and is silver and white colored.

Sodium
1s^2 2s^2 2p^6 3s^1 n= 3 l=0 ml=0 ms= +1/2

Atomic Number: 11 Atomic Mass: 23 Protons: 11 Neutrons: 12 Electrons: 11 Isotopes: 13

Sodium is metallic, silver, and white colored and is very soft.

Potassium
1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 n=4 l= 0 ml= 0 ms= +1/2

Atomic Number: 19 Atomic Mass: 39 Protons: 19 Neutrons: 20 Electrons: 19 Isotopes: 24

Potassium is soft, silvery-white and metallic.

Rubidium
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^1 n=4 l= 0 ml= 0 ms= +1/2

Atomic Number: 37 Atomic Mass: 85 Protons: 37 Neutrons: 48 Electrons: 37 Isotopes: 26

Rubidium is sliver-ish, soft white, and metallic.

Cesium
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^1 n=4 l= 0 ml= 0 ms= +1/2

Atomic Number: 55 Atomic Mass: 133 Protons: 55 Neutrons: 78 Electrons: 55 Isotopes: 39

Cesium is a soft, silver-gold metal.

Francium
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^6 7s^1 n=7 l= 0 ml= 0 ms= +1/2

Atomic Number: 87 Atomic Mass: 223 Protons: 87 Neutrons: 136 Electrons: 87 Isotopes: 34

Francium is a dark colored, metallic metal.



= Hyperlinks =

= http://en.wikipedia.org/wiki/Alkali_metal = = http://www.chemicalelements.com/groups/alkali.html = = =

= Physical Properties =

-The alkali metals differ from other metals in several ways. They are soft, with low melting and boiling temperatures. They have low densities -The ionic radii of the alkali metals are all much smaller than the corresponding atomic radii. This is because the atom contains one electron in an s level relatively far from the nucleus in a new quantum shell, and when it is removed to form the ion the remaining electrons are in levels closer to the nucleus. In addition, the increased effective nuclear charge attracts the electrons towards the nucleus and decreases the size of the ion.

=Chemical Properties= -The alkali metals are strong reducing agents. The reaction with oxygen tarnishes the metals in air, so they are stored under oil. They cannot be stored under water because they react with it to produce hydrogen and alkali hydroxides: -Na dissolves in liquid ammonia to give a deep blue solution of sodium cations and solvated electrons. This solution is used as a reducing agent. At higher concentrations the colour of the solution changes to bronze and it conducts electricity like a metal. -The chemistry of Li shows some anomalies, as the cation Li+ is so small it polarises anions and so introduces a covalent character to its compounds. Li has a diagonal relationship with magnesium.

=Periodic Trends=

They are very reactive and they are also never found in their natural form in nature. They are silver colored and have a very low density. They react with halogens to form ionic salts. They have the lowest ionization potential in their period.

=Fun Facts=

Caesium is used in atomic clocks which is accurate to seconds over thousands of years. Lithium is used in batteries. The most common for of sodium is salt which can be found on most of our dinner tables. Potassium is in bananas. Rubidium is used in fireworks to give it a purple color. Francium is the second rarest element.

=Sources= http://www.rsc.org/chemsoc/visualelements/Pages/data/intro_groupi_data.html

= http://en.wikipedia.org/wiki/Alkali_metal = = http://www.chemicalelements.com/groups/alkali.html =