1. Transition Metals The d-block elements

2. Properties of Transition Metals • Have a wide range of oxidation states (different positively charged ions formed) • Malleable and very hard metals • High melting and boiling points • High electrical conductivity • Low ionization energies • Located in the d-block (groups 3-12)

3. Group 10 Metals • Group 10 includes Nickel, Palladium, and Platinum • Used as catalysts for adding hydrogen to organic compounds • Palladium has the ability to absorb 900 times its own volume of hydrogen • Platinum is considered a precious metal and is quite expensive. • platinum-ore.jpg

4. Group 11 Metals • Often called the “coinage group.” • All are excellent conductors of electricity, but copper is the only one cheap enough to be used in large quantities. • Gold is not very reactive and forms very few compounds. One compound it forms is auric chloride (AuCl3) • Gold is the most malleable and ductile metal known. Also, it is the best conductor of electricity.

5. Tungsten • Comes from the ore Wolframite. • Has a density 19.3 times that of water. • The only 5d block metal known to be found in a few species of bacteria. • Highly corrosion resistive and extremely strong. • Highest melting point of all metals.

6. Molybdenum • Sometimes mistaken for graphite because of its properties. • Used in the production of alloys, electrodes, and catalysts. • Molybdenum disulfide is often used as a lubricant. Was used during the Vietnam War to lubricate sliding parts on weapons. • Pictured on the right is some Molybdenum Ore.

7. Chromium • Forms many toxic compounds. • Cr(VI) is used in the industrial chroming process and is carcinogenic. • Cr(III) is required for lipid and sugar metabolism. • Chromium forms ions with a 1,2,3,4,5, and 6 + charge. • Added to form stainless steel.

8. Yttrium • Has been found in moon rocks. • Used commercially to produce the red color in TV sets. • Discovered near Ytterby, Sweden in 1787. • Forms a 3+ ion only by losing all its s and d outer electrons. • Common product of nuclear fission of Uranium.

9. Multiple Oxidation States Formed By Transition Metals • D- block metals lose their outer s electrons first before losing any d electrons. • Example: Copper’s 4s1 3d10 configuration allows it to form a 1+ state because of the 1 s orbital electron. The second electron is removed from the d sublevel leaving a configuration of 3d9.

10. Effect of Positive Ion Formation on Ion Size • Let’s use Copper as an example: • The atomic radius is 135pm. • 1+ ionic radius is 91pm. • 2+ ionic radius is 87 pm. • 3+ ionic radius is 68pm.