Actinoids

__**Actinoids:**__

(grams per cubic centimetre) || 156.1 pico m || **1913** by Kasimir Fajans and Otto H. Göhring. || (grams per cubic centimetre) || 138.5 pico m || Martin Klaproth discovered Uranium in **1789**. || (grams per cubic centimetre) || 155 pico m ||  || E.M McMillan discovered Neptunium in **1940.** ||
 * **//Element//** || **//Symbol//** || **//Appearance//** || **//Atomic Number//** || **//Atomic Mass//** || **//# of Protons//** || **//#of Neutrons//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//# of Electrons//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//# of Valence Electrons//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//# of Shells//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//Melting Point// (vary according to source)** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//Boiling Point//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//Physical State at Room Temperature//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//Density//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//Atomic Radius//** || <span style="color: #365f91; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**//Discovery Date//** ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Thorium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Th || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Pure thorium is a silvery-white, air stable metal which retains its lustre/ shine for several months. When contaminated with oxygen, however, Thorium slowly tarnishes, becoming grey and then black. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">90 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">232.0381 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">90 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">142 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">90 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">6d2 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1755°C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">4788 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Thorium is a solid metal || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">11.72 g·cm−3 (grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">179 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**1828** by Jöns Jacob Berzelius. ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Protactinium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Pa || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Protactinium is an element with a bright metallic lustre that stays for some time after contact with air. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">91 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">231.0359 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">91 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">140 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">91 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">5f2 6d1 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || 1568 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">4027 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Protactinium is a solid metal || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">15.37 g·cm−3
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Uranium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">U || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Uranium is a dense, silvery-white, slightly paramagnetic, radioactive metal. It is also ductile and malleable. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">92 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">238.0289 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">92 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">146 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">92 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">6 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1405.3  1132.2 ° C  2070 ° F || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">4404 K, 4131 °C, 7468 °F || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Solid || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">19.1 g·cm−3
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Neptunium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Np || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Neptunium is a ductile, silvery, radioactive metal. Neptunium forms numerous chemical compounds. Chemically it is extremely reactive and is attacked by oxygen, steam and acids, but not by alkalis. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">93 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">237.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">93 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">144 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">93 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">NA || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">640.0 °C 913.15 K 1184.0 °F || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">4273 K, 4000 °C, 7232 °F || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Solid || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">20.45 g·cm−3

<span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">151.3 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**1940** by a team lead by Glenn T. Seaborg and Edwin McMillan. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">173 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**1944** by Glenn T. Seaborg, Ralph A. James, Leon O. Morgan, and Albert Ghiorso. ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Plutonium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Pu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Plutonium has a bright silvery appearance at first, but it oxidizes very quickly into a dull grey (yellow and olive green are also present). || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">94 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">244.0642 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">94 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">150 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">94 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">5f6 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">639.4 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">3228 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, plutonium is in its ‘α form’. This is about as hard and brittle as grey cast iron (unless it is alloyed with other metals to make is soft and malleable. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">19.84 g·cm−3
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Americium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Am || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Pure americium has a silvery and white lustre. It is more silvery than plutonium or neptunium and easier to work with than neptunium or uranium. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">95 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">243.0614 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">95 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">148 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">95 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">5f7 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1176 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">2607 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Americium is a solid metal, and it tarnishes in dry air. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">13.69 g·cm−3
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Curium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Cm || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Curium is a synthetic chemical element and is silvery in colour. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">96 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">247.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">96 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">151 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">96 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">NA || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1340.0 °C 1613.15 K 2444.0 °F || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">3383 K || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Curium is a solid metal. || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">13.51 g·cm−3 <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">174pico m ||   || <span style="color: black; font-family: Calibri; font-size: 8pt; line-height: normal; margin: 0in 0in 0pt;">Curium was discovered in **1944** by Glenn Seaborg, Ralph A. James, and Albert Ghiorso. ||

<span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">186 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**1950** by Stanley G. Thompson, Kenneth Street Jr., and Albert Ghiorso. || (grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">186 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**1952** by Albert Ghiorso & Berkely Lab. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">287pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Mendelevium was discovered by Albert Ghiorso and S.T Seaborg in 1955. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre) || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">285 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**1958** by Nobel Institute of Physics in Stockholm and later by Albert Ghiorso, Torbjorn Sikkeland, J. R. Walton, and Glenn T. Seaborg. ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Berkelium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Bk || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">The appearance of berkelium is not known, since no one has managed to isolate the element in a pure form. It is presumed to be silvery-gray like its neighbours on the periodic table. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">97 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">247.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">97 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">150 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">96 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">NA || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">2 || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1259 K 986 °C 1807 °F || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Berkelium is a solid metal. || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">14.78 g·cm−3 <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(grams per cubic centimetre)  || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">170 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Berkelium was discovered in **1949** by G.T Seaborg. ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Californium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Cf || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Californium is a silvery-white metal (metallic californium has not been produced yet). || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">98 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">251.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">98 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">153 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">98 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">5f10 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">900 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1470 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Californium is a solid metal || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">15.1 g·cm−3
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Einsteinium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Es || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Though only small amounts of Einsteinium have been produced, it is said to be silver in colour. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">99 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">252.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">99 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">153 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">99 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">5f11 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">860 °C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, the element Einsteinium is a solid metal || 8.84 g·cm−3
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Fermium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Fm || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Fermium has a very short life-span, so scientists doubt that enough of the element will ever be obtained to be weighed or seen. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">100 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">257.09 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">100 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">157 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">100 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">NA || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;"> 1800K 1527°C <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">2781 °F || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, the element Fermium is a solid metal || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">290 pico m || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Fermium was discovered by G. R. Choppin, S.G. Thompson, A. Ghiorso and B.G. Harvey in **1952**. ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Mendelevium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Md || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">The appearance of Mendelevium is unknown to scientists however they presume that it is probably silvery, white or metallic gray. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">101 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">258.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">101 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">157 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">101 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">NA || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1100 K 827 °C 1521 °F || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Solid || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Nobelium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">No || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">The appearance of nobelium is unknown; however it is most likely silvery-white or grey and metallic. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">102 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">259.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">102 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">157 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">102 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">5f14 7s2 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">827°C || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">At room temperature, Nobelium is a solid metal || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">**Lawrencium** || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Lr || <span style="color: black; font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">The appearance of Lawrencium is unknown but experts suggest that its colour varies from a silvery, white to a metallic gray like the other elements from the Actinoides. || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">103 || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">262.0 amu || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">103 Protons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">159 Neutrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">103 Electrons || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">NA || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Seven || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">1900 K 1627°C 2961°F ||   ||
 * <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">(presumably) Solid || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Unknown || <span style="font-family: 'Calibri','sans-serif'; font-size: 8pt; line-height: 115%;">Albert Ghiorso discovered Lawrencium in 1961. ||

THE ACTINOID FAMILY: //** Actinoides: **//
The group of elements known as the Actinoides are the elements from actinium (element 89) to lawrencium (element 103). All members of the series resemble actinium in their chemical and electronic properties, and so they form a separate group within the periodic table.

TRENDS DOWN THE ACTINOID FAMILY:
 * As we look across the Periodic Table, the atomic number of each of the elements increases steadily by one. As the atomic number of the elements increase, so do the number of protons. In terms of electrons, all electrons increase by a factor of one as we go from one element to another; the number of valence electrons however, stay the same regardless of where they are positioned in their ‘family.’ When looking at the number of neutrons, we see that there is no pattern and that they increase or decrease quite randomly. However, it was interesting to see that Californium and Einsteinium shared the same amount of neutrons and the same atomic radius. Fermium, Mendelevium and Nobelium also shared the same number of neutrons. Regarding the atomic mass, it was very difficult to determine a specific pattern due to the fact that the atomic mass did not increase or decrease by a specific amount – the mass increased and decreased quite unsystematically. This was the same with the atomic radius for the rest of the elements. We found that the atomic radius decreased, and then increased before decreasing and increasing again. All elements in this family had the same number of shells (7) and the same physical state at room temperature (solid). The boiling and melting points were all extremely varied across the table, and, in terms of Nobelium and Einsteinium, a boiling point had not even been established. The density of all elements continuously varied also. **
 * This table seems to apply to real life too. When we are viewed with our families, there are many similarities between us and our relatives, however, along with these similarities come infinite differences. **


 * Interesting Fact: Due to the fact that this family is the actinoid family, they are able to handle more than eight electrons in their inner shells, unlike other families in the periodic table. **

COMPOUNDS AND USES OF THE ACTINOID FAMILY: Thorium is a member of the actinide family which is located in Row 7 of the periodic table. The actinide family all have atomic numbers between 90 and 103 and is named after element 89 actinium. The element was named after Thor, the Scandinavian god of war. In terms of physical properties, to elaborate on what is written on the table, thorium is a silvery white, soft metal similar to lead. It can be hammered, rolled, bent, cut, shaped and welded rather easily. . It is soluble in acids and reacts slowly with oxygen at room temperature. Thorium is an abundant element in the Earth’s crust and more than two dozen isotopes of thorium are known. All are **radioactive**. Most people would have heard of thorium in portable glass lanterns. These lanterns contain a delicate material known as a mantle. Gas that passes through the mantle is ignited to produce a very hot and bright white flame. Thorium dioxide (ThO2) and thorium nitrate (Th(NO3)4) were used in a type of lantern mantle called a Welsbach mantle. Thorium dioxide can also be used as a catalyst (a substance used to speed up or slow down a chemical reasction without undergoing any change itself) when converting ammonia into nitric acid, in petroleum cracking and in producing sulphuric acid. ** Hydrides: ** Thorium dihydride: ThH2 ** Fluorides: ** Thorium trifluoride: ThH2 Thorium tetrafluoride: ThF4 ** Chlorides: ** Thorium tetrachloride: ThCl4 ** Iodides: ** Thorium diiodide: ThI2 Thorium triiodide: ThI3 Thorium tetraiodide: ThI4 ** Oxides: ** Thorium dioxide: ThO2 ** Sulphides: ** Thorium sulphide: ThS Thorium disulphide: ThS2 Dithorium trisulphide: Th2S3 ** Selenides: ** Thorium diselenide: ThSe2 ** Nitrides: ** Thorium nitride: ThN ** Complexes: ** Thorium sulphate nonahydrate: Th(SO4)2.9H2O When looking at Thorium itself, is used as an alloying agent to improve magnesium’s strength at high temperatures. As well as this, it is also a source of nuclear power.
 * // Thorium: //**
 * USES: ** Thorium and its compounds have relatively few uses. The most well known thorium compound is thorium dioxide (ThO2). This compound has the highest melting point of any oxide, about 3300 degrees Celsius. It is used for high temperature ceramics. When added to glass, ThO2 assists in increasing the refractive index and decreasing dispersion. This glass is used to make lenses for high quality cameras and scientific equipment.
 * __ Here is a list of some of the examples of Thorium compounds: __**

In 1913, Kasimir Fajans and his colleague, O.H. Göhring suggested to name the element brevium because the half life of the isotope they found was very “brief.” After this, it was given the name “protoactinium” meaning “first actinium.” In 1949, the name was changed to protactinium. It is a bright, shiny metal that forms a whitish coating of protactinium when exposed to air. There are tiny, tiny amounts of protactinium found in the Earth’s crust with 20 known isotopes. It is a rare, poisonous and expensive element (US$300 per gram). > Protactinium(V) fluoride PaF5 > Protactinium(V) chloride PaCl5 > Protactinium(V) bromide PaBr5 > Protactinium(IV) iodide PaI4 > Protactinium(V) iodide PaI5 > Protactinium(IV) oxide PaO2 > Protactinium(V) oxide Pa2O5 ** USES: ** Unfortunately, neither Protactinium nor its compounds have any commercial uses.
 * // Protactinium: //**
 * __ Some of its compounds include: __**
 * ** Fluorides: ** Protactinium(IV) fluoride PaF4
 * ** Chlorides: ** Protactinium(IV) chloride PaCl4
 * ** Bromides: ** Protactinium(IV) bromide PaBr4
 * ** Iodides: ** Protactinium(III) iodide PaI3
 * ** Oxides: ** Protactinium(II) oxide PaO

//** Uranium: **// - Uranium boride - Uranium dioxide - Uranium sulfate - Uranium tetrachloride - Uranium tetrafluoride - Uranium borohydride - Uranium carbide - Uranium hexafluoride - Uranium hydride - Uranium nitride - Uranium pentafluoride - Uranium(III) chloride - Uranous
 * USES: ** Uranium is mined for several purposes. The most common uses of uranium are in nuclear weapons and in nuclear power stations. It has been used to produce nuclear weapons for more than 50 years and electricity for more than 40 years. The radioactive element is additionally used to make atomic bombs (nuclear fissure bombs). Scientists have also found traces of the element in some ceramics and paints.
 * Uranium compounds and structures: **

//** Neptunium: **//
 * USES: ** Neptunium and its compounds of neptunium have been made for research purposes. They are used in specialized detection devices and in nuclear reactors. Neither the element nor its compounds have any commercial uses as it is a very hazardous material. It must be handled with great caution.
 * Neptunium compounds and structures: **
 * -**Neptunium Oxide

Plutonium is an artificial element and member of the actinide family. Naturally, it exists in only the smallest amounts. It was first prepared by a team of researchers at the University of California in 1941, however news of this discovery was only released in 1946. The element was named in honour of the planet Pluto. Plutonium is highly reactive and is found in very small amounts in the Earth’s crust. Fifteen isotopes of plutonium are known to exist. ** Hydrides: ** Plutonium dihydride: PuH2 Plutonium trihydride: PuH3 ** Fluorides: ** Plutonium trifluoride: PuF3 Plutonium tetrafluoride: PuF4 Plutonium hexafluoride: PuF6 ** Chlorides: ** Plutonium trichloride: PuCl3 ** Bromides: ** Plutonium tribromide: PuBr3 ** Iodides: ** Plutonium triiodide: PuI3 ** Oxides: ** Plutonium oxide: PuO Plutonium dioxide: PuO2 Diplutonium trioxide: Pu2O3 ** Sulphides: ** Plutonium sulphide: PuS Plutonium disulphide: PuS2 Diplutonium trisulphide: Pu2S3 ** Selenides: ** Plutonium selenide: PuSe ** Nitrides: ** Plutonium nitride: PuN No plutonium compounds have any commercial application.
 * // Plutonium: [[image:http://www.webelements.com/_media/elements/element-pics-theo/94_Pu_1.jpg width="216" height="232" align="right" caption="Plutonium"]] //**
 * USES: ** Plutonium has two major uses. First of all, some of its isotopes (different types of atoms of the same chemical element) will undergo nuclear fission – a process in which an element is bombarded with neutrons. Then, the element breaks apart into simpler elements, releasing large amounts of energy. Plutonium has used this process to create nuclear weapons (such as atomic bombs) and it is used in nuclear power plants to produce electricity. It has also been used as a portable energy source in space probes and other space vehicles.
 * __ Some examples of Plutonium compounds include: __**

The name Americium was given to the element in honour of the continent of America due to the fact that it occurs just below Europium (named after Europe) in the periodic table. To elaborate on its physical properties, enough americium has been produced to determine a few of its properties which are all listed in the table above. Americium is artificially produced – it does not occur in nature and all isotopes are radioactive, with the most stable being Americium-241. Americium-241 is also used in smoke detectors. ** Fluorides: ** Americium trifluoride: AmF3 Americium tetrafluoride: AmF4 ** Chlorides: ** Americium dichloride: dichloride: AmCl2 Americium trichloride: AmCl3 ** Bromides: ** Americium tribromide: AmBr3 ** Iodides: ** Americium diiodide: AmI2 Americium triiodide: AmI3 ** Oxides: ** Americium Oxide: AmO Americium dioxide: AmO2 Diamericium trioxide: Am2O3 ** Complexes: ** Hexaaquodichloroamericum chloride: AmCl3.6H2O There are no known uses for Americium compounds.
 * // Americium:[[image:http://64.202.120.86/upload/image/articles/2006/americium-power-source/americium-element.jpg width="358" height="226" align="right" caption="Americium"]] //**
 * USES: ** Americium-241 is the only isotope of Americium that has any practical uses. When is decays, it gives off alpha and gamma rays. These alpha rays do not travel very far in air but gamma rays are very penetrating, similar to X-Rays. Therefore, the gamma rays from Americium are used in portable X-Ray machines. These machines can, for example, be taken into oil fields to help determine where new wells can (or should) be dug. Aside from this, americium can also measure the thickness of materials (when more radiation gets through the material and into the detector, the material is thinner; when less gets through, it is thicker).
 * __ Some compounds of Americium include: __**

//** Curium **// -Curium Nitrate - Curium hydroxide - Curium oxide
 * USES: ** Curium is sometimes used to analyze materials taken from mines and is a portable source of electrical power. It gives off a large amount of energy that can be used to generate electricity for space vehicles. A recent use of curium was in the Mars Pathfinder that was sent to Mars in 1997 to study that planet's surface. Some of the equipment on the spacecraft was powered by a curium battery.
 * Curium compounds and structures: **

//** Berkelium: **// -Berkelium bromide (BkBr3) -Berkelium chloride (BkCl3) -Berkelium dioxide: (BkO2) -Berkelium fluoride (BkF3) -Berkelium iodide (BkI3) -Berkelium oxide (BkO) -Berkelium trifluoride: (BkF3) -Berkelium tetrafluoride: (BkF4) -Berkelium trichloride: (BkCl3) - Berkelium triiodide: (BkI3) -Berkelium trifluoride: BkF3 -Berkelium tetrafluoride: (BkF4) -Berkelium trichloride: (BkCl3) -Diberkelium trioxide: (Bk2O3)
 * USES: **It is extremely rare and has no technological biological or commercial uses.
 * Berkelium compounds and structures: **

This element was named after the state of California (it was discovered by a research team at the University of California). Californium’s isotopes are all radioactive and it does not occur naturally. Californium-252 has been used to look for oil and to test materials without breaking them apart or destroying them. Neutrons from this isotope of californium can be used to inspect airline baggage. Californium is also used in medicine. When injected into the body, it is deposited into the bones. The radiation given off can determine how strong the bone is. Californium-252 is also used to treat ovarian and cervical cancer. ** Fluorides: ** Californium trifluoride: CfF3 Californium tetrafluoride: CfF4 ** Chlorides: ** Californium dichloride: CfCl2 Californium trichloride: CfCl3 ** Bromides: ** Californium tribromide: CfBr3 ** Iodides: ** Californium diiodide: CfI2 Californium triiodide: CfI3 ** Oxides: ** Californium dioxide: CfO2 Dicalifornium trioxide: Cf2O3 There is, once again, no commercial use for Californium compounds.
 * // Californium:[[image:http://gotexassoccer.com/elements/098Cf/Cf_bromid.jpg width="286" height="176" align="right" caption="Californium (we had a better picture, but it did not upload)"]] //**
 * USES: ** When neutrons collide with an atom, they become part of the nucleus, making the atom unstable. The radioactive copper gives off radiation and particles that can be measured.
 * Interesting fact: ** Californium is only made in milligram amounts. It costs US$10 per millionth of a gram.
 * __ Compounds of Californium include: __**

Einsteinium was named after German-American physicist, Albert Einstein. Too little of Einsteinium has been prepared to allow scientists to determine its physical and chemical properties. Like Californium, Einsteinium does not occur naturally in the Earth’s crust and all isotopes of this element are radioactive. There are no commercial uses for these compounds of Einsteinium.
 * // Einsteinium:[[image:http://www.webqc.org/elements-photo/Einsteinium.jpg align="right" caption="Einsteinium Iodide"]] //**
 * USES: ** Since only small amounts of Einsteinium have been produced, it currently has no uses outside of basic scientific research (such as being a step in the production of other elements).
 * __ The following is a list of known compounds of einsteinium: __**
 * Es2O3 einsteinium(III) oxide
 * EsF3 einsteinium(III) fluoride
 * EsCl3 einsteinium(III) chloride
 * EsBr3 einsteinium(III) bromide
 * EsI3 einsteinium(III) iodide
 * EsCl2 einsteinium(II) chloride
 * EsBr2 einsteinium(II) bromide
 * EsI2 einsteinium(II) iodide

-Fermium Chloride
 * // Fermium: //**
 * USES: ** Due to the small amounts produced and its short half-life, there are currently no uses for fermium outside of basic scientific research.
 * Fermium compounds and structures: **

//** Mendelevium: **// ** USES: **Since only small amounts of mendelevium have ever been produced, it currently has no uses outside of basic scientific practices.
 * Mendelevium compounds and structures: ** Mendelevium forms no compounds or structures.

**//Nobelium: (//**  The appearance of Nobelium is unknown; however, it is most likely silvery-white or gray and metallic**// ) //** hexaaquanobelium(II): [No(H2O)6]2+ hexaaquanobelium(III): [No(H2O)6]3+
 * USES: ** Due to the fact that only tiny amounts of Nobelium have ever been produced, there are currently no uses for it, or its compounds, outside of scientific research.
 * __ Compounds of Nobelium: __**

//** Lawrencium: **// ** USES: **Lawrencium has no uses outside of scientific research as it is radioactive and toxic. ** Lawrencium compounds and structures: ** Lawrencium forms no compounds or structures.

Bibliography: [] [] [|www.periodic.lanl.gov/elements] [|www.education,jlab.org/itselemental] [|www.chemicalelements.com/elements] [|www.environmentalchemistry.com/yogi] [|www.experiencefestival.com/plutonium-compounds] [] (for all elements)

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