The History of the Modern Periodic Table November 4th, 2016

During the nineteenth century, chemists began to categorize the elements according to similarities in their physical and chemical properties. The end result of these studies was our modern periodic table.

Johann Dobereiner Model of triads 1829 Classified some elements into groups of three (called triads) The elements in a triad had similar chemical properties and orderly physical properties. (ex. Cl, Br, I and Ca, Sr, Ba)

John Newlands Law of Octaves 1863 Suggested that elements be arranged in “octaves” He noticed (after arranging the elements in order of increasing atomic mass) that certain properties repeated every 8th element

John Newlands Law of Octaves FUN FACT: Newlands' claim to see a repeating pattern was met with savage ridicule on its announcement. His classification of the elements, he was told, was as arbitrary as putting them in alphabetical order and his paper was rejected for publication by the Chemical Society.

Dmitri Mendeleev In 1869 he published a table of the elements organized by increasing atomic mass.

Lothar Meyer At the same time, he published his own table of the elements organized by increasing atomic mass.

Both left vacant spaces where unknown elements should fit. Both Mendeleev and Meyer arranged the elements in order of increasing atomic mass. Both left vacant spaces where unknown elements should fit. So why is Mendeleev called the “father of the modern periodic table” and not Meyer, or both?

Mendeleev... stated that if the atomic weight of an element caused it to be placed in the wrong group, then the weight must be wrong. (He corrected the atomic masses of Be, In, and U) was so confident in his table that he used it to predict the physical properties of three elements that were yet unknown.

After the discovery of these unknown elements between 1874 and 1885, and the fact that Mendeleev’s predictions for Sc, Ga, and Ge were amazingly close to the actual values, his table was generally accepted.

However, in spite of Mendeleev’s great achievement, problems arose when new elements were discovered and more accurate atomic weights determined. By looking at our modern periodic table, can you identify what problems might have caused chemists a headache? Ar and K Co and Ni Te and I Th and Pa

Henry Moseley 1913 Working with X-rays, he determined the actual nuclear charge (atomic number) of the elements* Rearranged the elements in order of increasing atomic number. *“There is in the atom a fundamental quantity which increases by regular steps as we pass from each element to the next. This quantity can only be the charge on the central positive nucleus.”

Henry Moseley Fun Fact: His research was halted when the British government sent him to serve as a foot soldier in WWI. He was killed in the fighting in Gallipoli by a sniper’s bullet, at the age of 28. Because of this loss, the British government later restricted its scientists to noncombatant duties during WWII.

The Periodic Law When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. …. That’s why it’s called the periodic table.

These became known as the Actinide series. Glenn T. Seaborg 1944 Co-discovered 10 new elements Moved 14 elements out of the main body of the periodic table These became known as the Actinide series.

Glenn T. Seaborg Fun Fact: He is the only person to have an element named after him while still alive. "This is the greatest honor ever bestowed upon me - even better, I think, than winning the Nobel Prize."

The Remaining Questions Why could most of the elements be arranged in order of increasing atomic mass but a few could not? What was the reason for chemical periodicity?

The Reason is Valence Electrons The number of electrons in the outermost energy level Determines the chemical behavior of an element Elements in the same vertical column (family) have similar properties because they have the same number of electrons in their outer shell

The Octet Rule • Every element is seeking 8 electrons in its outermost energy level • Nonmetals will take electrons from metals to form negative ions so they have set of 8 • Metals will give up (donate) their e- to form positive ions

Exceptions to Octet Rule • Less than 8 - energy level considered “full” with 2 valence electrons - ”duet” instead of “octet” - Hydrogen (H) - Helium (He)

Charges (as a result of valence electrons & the octet rule)

Basics of the Periodic Table

Periodic Table: Atomic number – the identity of an element Row = Period (Horizontal Rows #1-7)             The atomic # increases as you go from left to right             Atomic# = # protons (p) = # electrons for a neutral atom Properties change somewhat regularly as you go across Column = Group = Family (Vertical Columns #1-18)             Elements in a group have similar chemical properties

Metals, Non metal and metalloids – Summary Table Non metals

To Review: Metals Common Properties - shiny - good electrical/heat conductor - most are solids (room temperature) - malleable (can be hammered) - ductile (can be drawn into fine wire) - high tensile strength (resist breaking when pulled) Unique Properties - mercury (liquid at room temperature) - Group 1 metals can be cut with a knife - variety of colors

- poor conductors of heat & electricity - not as common as metals To Review: Nonmetals Common Properties - poor conductors of heat & electricity - not as common as metals Gases (Room Temperature) - nitrogen, oxygen, fluorine, & chlorine Liquids - bromine Solids - carbon, phosphorous, selenium, sulfur, iodine

- share characteristics with m & nm - all solids at room temperature To Review: Metalloids Common Properties - located between m & nm - share characteristics with m & nm - all solids at room temperature - less malleable than metals - not as brittle as nonmetals - semiconductors of electricity • Metalloid Elements - Boron (B), Antimony (Sb), Silicon (Si), Tellurium (Te), Germanium (Ge), Polonium (Po) - Arsenic (As) (debate-also metal)