Page WHO CREATED THE PERIODIC TABLE? DMITRI MENDELEEV
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1 Page WHO CREATED THE PERIODIC TABLE? DMITRI MENDELEEV Russian chemistry professor Wrote name of element & properties on separate cards Arranged cards in order of increasing atomic mass Also grouped elements by similar properties SOME ELEMENTS WERE MISSING Mendeleev postulated the existence of yet to be discovered elements. Table included some irregularities o Mendeleev thought irregularities were due to poor measurements of atomic mass
2 HENRY MOSELEY English Scientist Arranged table according to Atomic Number rather than Atomic Mass This took care of irregularities Moseley s improvements gave us today s Periodic Table REGIONS OF THE PERIODIC TABLE MAIN BLOCK properties vary symmetrically (the most predictable) Hydrogen - H sits on top of the table behaves unlike any other element basis of acids considered a family in itself
3 FAMILY CHARACTERISTICS NOBLE GASES inert unreactive, an element or compound that does not react with others stable non- flammable They form monatomic (single atom) gases. full outer shells (this is why they are unreactive)
4 GROUP 1 ALKALI METALS explosive reactions with water (stored in oil) extremely unstable on their own soft metal cut with a knife like cheese name derived from Arab word for ashes outer shell has one electron stable if it loses an electron What are the ALKALI METALS?
5 GROUP 2 ALKALINE-EARTH METALS harder than alkali metals more dense than alkali metals stronger than alkali metals outer shell has two electrons stable if it loses two electrons less reactive due to # of electrons in outer shell forms a skin with oxide to protect itself What are the ALKALINE-EARTH METALS?
6 GROUPS 3-12 TRANSITION METALS harder than alkaline-earth metals more dense than alkaline-earth metals stronger than alkaline-earth metals outer most electrons in d orbitals all conduct electricity, heat EXCEPTION : Hg is the only non-solid metal LANTHANIDES Shiny, metallic elements Numbers 58 through 71 Outer electrons in f orbital Uses- inside of televisions sets ACTINIDES Metallic elements Numbers 90 through 103 Unstable nuclear decay Best known Uranium
7 GROUP 17 HALOGENS Combine with most metals to form salts Halogen Latin for salt-former Most reactive non-metal Outer shell one electron short of being full Halogens gain an electron for stability What are the HALOGENS?
8 OTHER MAIN BLOCK GROUPS B Al Ga Named after element at top of column Outer shell has the same number of electrons Forms the same charge ion Similar behavior in reactions Similar stability In Tl What are the other families? BORON FAMILY CARBON FAMILY NITROGEN FAMILY OXYGEN FAMILY
9 4-2 TRENDS WITHIN THE PERIODIC TABLE Definition ION an ion is an atom which has gained or lost electrons to obtain stability. Since Atoms would like to have a full outer shell they may get a full shell by either gaining or losing electrons. Example: Lithium SKETCH OF THE LITHIUM ATOM: To become stable Lithium gives up its electron in the outer shell Prior to losing the electron what is the charge of a Lithium atom? +3 (protons) + -3(electrons) = 0 or NEUTRAL
10 What is charge of Lithium ion (after it has lost the electron)? +3 (protons) + -2(electrons) = +1 charge Definition CATION an ion which has lost an electron(s) to become stable, its overall electrical charge is positive. Another Example: Fluorine SKETCH THE FLUORINE ATOM: 9 protons surrounded by 2 electrons in the first shell and 7 in the second shell. To become stable Fluorine gains an electron in the outer shell Prior to losing the electron what is the charge of a Fluorine atom? +9 (protons) + -9(electrons) = 0 or NEUTRAL What is charge of Fluorine ion (after it has gained the electron)? +9 (protons) + -10(electrons) = -1 charge
11 Definition ANION an ion which has gained an electron(s) to become stable, its overall electrical charge is negative. Definition IONIZATION ENERGY the energy required to remove an electron from the neutral atom this is measured in the units of energy (Joules) SIZE OF THE ATOM : INCREASES DOWN A FAMILY DECREASES FROM LEFT TO RIGHT (counterintuitive) DRAW ARROWS ALONG THE TOP AND LEFT SIDE TO INDICATE WHICH DIRECTION THE SIZE OF THE ATOMS ARE INCREASING INCREASING RADIUS INCREASING IONIZATION ENERGY
12
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