The Periodic Table and Periodicity Chemistry Outlin e Outlin e PowerPoint Presentation by Mr. John Bergmann

The Elements elements known to the ancients… Element names come from a variety of sources. place names… famous people… foreign languages… mythology-related names… names related to element properties… S, CuC,Sn, Fr,Po,Ge, Ga, Eu, Am, Cf, Sc Es, Fm,Md,No, Lr,Rf,Bh Hg, Ta,Ti, Nb Pm,Th, W, Fe,Au,Ag, Pb, Sn, Cu I, Br,

atomic number Background on the Periodic Table Dmitri Mendeleev: organized Table by increasing atomic mass left spaces and predicted properties of undiscovered elements Henry Moseley: put elements in order of increasing ____________. Mendeleev Moseley Russian scientist credited with organizing elements into table (1870)

P ZnAs Sb PtBi Midd CrMn Li K NOF Na BBe H AlSiCl CaTiVCoNiSeBr SrYZrNbMoRhPdCdTeI BaTaWOsIr Mg CeTbEr ThU Discovering the Periodic Table C S FeCu AgSn AuHgPb Ancient Times He ScGaGe RbRuIn CsTl PrNdSmGdDyHoTmYb La Ne Ar Kr Xe PoRn Ra EuLu Pa Ac Tc HfReAt Fr Pm NpPuAmCmBkCfEsFmMdNoLr Rf Db SgBhHsMt Journal of Chemical Education, Sept. 1989

MENDELEEV’S PERIODIC TABLE

Why is it called the Periodic Table ? Periodic means a quantity that repeats itself at regular intervals (ex. a month, a year, etc) So the table of elements are periodic in that elements with similar properties are put near each other on the table

Describing the Periodic Table periodic law: the properties of elements repeat every so often period: group (family): horizontal row; there are 7 vertical column; there are

Regions of the Table metals: left side of Table; form cations, 75% of all elements properties: 1) lustrous (shiny) 2) ductile (can pull into wire) 3) malleable (can hammer into shape) 4) good conductors (heat and electricity)

Transition metals: -Are in groups 3-12(middle of periodic table) -Usually have multiple oxidation states: ex. Fe 3+ and Fe 2+ - Form COLORED compounds

nonmetals: right side of Table; form anions properties: 1) good insulators (don’t conduct) 2) gases or brittle(break apart) solids Regions of the Table (cont.) Br 2 I2I2 S8S8 Ne bromineiodinesulfurneon

computer chips metalloids (semimetals): “stair” between metals and nonmetals properties: in-between those of metals and nonmetals; “semiconductors” Regions of the Table (cont.) (B, Si, Ge, As, Sb, Te, Po) Si and Ge computer chips metals nonmetals

Metals and Nonmetals Li 3 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac   METALS Nonmetals Metalloids

Elements in the SAME group have the SAME number of valence electrons: ex. N, P, As, Sb, Bi : all in group 15, all have 5 valence electrons IMPORTANT !!! Elements with the same number of valence electrons have SIMILAR properties

Li: 2-1 Na: Both have 1 valence electron Because Li and Na are in the same group and have the same number of valence electrons, they have similar chemical and physical properties

Periodicity Because the periodic table is arranged according to valence electrons, there are trends in properties of elements Information about different elemental properties are found in Table S

1. atomic radius: the size of a neutral atom RADIUS

Atoms become larger as you go down a group add a new energy level each time you go down a group WHY?

Atomic Radii Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te SbSn In Tl Pb Bi Mg Ca Sr Ba Be F O N C B IA IIA IIIA IVA VA VIA VIIA = 1 Angstrom

Atoms become smaller as you move left to right across a period

Li 3p 4p 5p BeBC Increasing nuclear charge is drawing electrons in closer across a period

Arrange the following elements in order of increasing atomic radius: 1.N, F, C, O 2.Sr, Be, Ca, Mg F, O, N, C Be, Mg, Ca, Sr

ionic radius: cationsanions Ca atomCa 2+ ion Cl atom Cl 1– ion the size of an ION 20 p + 20 e – 20 p + 18 e – 17 p + 17 e – 17 p + 18 e – Ca Ca 2+ Cl Cl – cations are smalleranions are larger

If you LOSE electrons, you become smaller: cations < atoms If you GAIN electrons, you become bigger: anions > atoms + -

Which atom, when it forms an ion, will have an ionic radius larger than its atomic radius : Ca, Na, F, Li F as it is a non-metal, and will form an anion; anions are larger than their atoms

2. IONIZATION ENERGY (IE): the energy required to remove an electron (e – ) from an atom M + 1st I.E. M + + e – removes 1 st e – 3p Add energy to remove the valence electron ATOMCATION

Ionization energy decreases down a group as the valence electrons move further away from the nucleus This valence electron is easier to remove because it is further away from the nucleus, so ionization energy is less

Ionization energy increases across a period as the valence electrons are held more tightly by increasing nuclear charge 3p 4p 5p This valence electron takes the most energy to remove because it is held more tightly by nucleus

Ionization Energies (in kilojoules per mole) joules are a unit of energy… H Li Na K Be Mg Ca B Al Ga C Si Ge N P As O S Se F Cl Br Ne Ar Kr He Rb Sr In Sn Sb Te I Xe Smoot, Price, Smith, Chemistry A Modern Course  1987, page 188

3.ELECTRONEGATIVITY Linus Pauling invented the the electronegativity scale. a) the tendency for a bonded atom to attract e – to itself b) the GREEDINESS for electrons

As we go, electronegativity… decreases. increases. electronegativity increases

So the most electronegative element (the element GREEDIEST for electrons) is… The least electronegative element (the element most likely to GIVE UP electrons is)…. F Cs

4. METALLIC CHARACTER: a) elements that behave the most like a metal (shiny, ductile, malleable, etc) b) ability to lose electrons

Metallic Characteristic metallic character increases nonmetallic character increases metallic character increases nonmetallic character increases MOST METALLIC ELEMENT MOST NONMETALLIC ELEMENT

Summary of Periodic Trends Ionic size (cations) Ionic size (anions) decreases Atomic radius decreases Ionization energy increases Electronegativity increases Metallic character decreases Atomic radius increases Ionization energy decreases Electronegativity decreases Metallic character increases 1A 2A3A4A 5A 6A7A 0

shielding effect: kernel e – “shield” valence e – from attractive force of the nucleus Li v.e – K -- caused by kernel and valence e – repelling each other As we go, shielding effect increases. tougher to remove easier to remove

alkali metals: alkaline earth metals: halogens: noble gases: contain f orbitals lanthanides: coinage metals: transition elements: main block (representative) elements: group 1 (except H); 1+ charge; very reactive group 2; 2+ charge; less reactive than alkalis group 17; 1– charge; very reactive group 18; no charge; unreactive elements 58–71 actinides: elements 90–103 group 11 groups 3–12; variable charges groups 1, 2, 13–18

Table S supplies important information about the elements

To tell what phase of matter an element is at a certain temperature, use the “melting” and “boiling” point data on Table S For an element, at temperature LESS than melting point, it will be a Between the melting point and the boiling point, it will be : And above the boiling point, it will be a: SOLI D LIQUID GAS

S L G

Temperature scales Temperature given on Table S is Kelvin (K) Kelvin temperature is Celsius temperature (K = o C + 273) STP stands for “Standard Temperature and Pressure” and is 273K (0 o C) and 101.3kPa

Which element would be a liquid at 500K: Mg, Na or Ar ? Which element is a gas at STP ? Zn, Ne, or Si ? Which element will float in water ? K, Sc or S ? Na Ne K

CHEMISTRY OF THE DIFFERENT GROUPS

Alkali Metals, Group 1 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

Group 1: 1.Known as “alkali metals” 2.Have 1 valence electron 3.Lose electrons VERY easily (never found in nature as atoms; only in compounds) 4.Low ionization energies and electronegativity values 5.Hydrogen not considered an alkali metal

Alkaline Earth Metals, Group 2 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

Group 2: 1.Known as “alkaline earth metals” 2.Have 2 valence electrons 3.Also lose electrons easily (never found in nature as atoms; only in compounds) 4.Low ionization energies and electronegativity values (not as low as alkali metals though…)

Group 15 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi Po At Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

GROUP 15 1.Doesn’t have particular group name 2.Have both metal and non-metal properties 3.Gain electrons to form 3- anions 4.Nitrogen will form triple bonds to form diatomic N 2

Group 16 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi Po At Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

GROUP 16 1.Have 6 valence electrons 2.Contain metals and nonmetals 3.Tend to gain electrons (2) to form 2- anions 4.Larger ionization energy and electronegativity values

Halogens, Group 17 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

GROUP 17 1.Known as the “halogens”, which means “salt formers” 2.Elements in this group like to gain one electron to become 1- anions. 3.The salts these compounds form are called “halides” 4.Contain all 3 states of matter: F and Cl are gases, Br is a liquid, and At is a solid 5.Are very reactive and are not found as free elements in nature.

Noble Gases, Group 18 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

GROUP 18 1.Are known as the Noble or Inert Gases 2.Have 8 valence electrons and are extremely stable (non-reactive) 3.Are all gases at room temperature 4.Have the largest ionization energy values of any group

Lanthanide Series H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr La

Actinide Series H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr La

alkaline earth metals halogens noble gases lanthanides alkali metals actinides coinage metals transition elements main block elements metalloids hydrogen more nonmetals more metals