Periodic Table 1869 Dmitri Mendeleev in Russia Lothar Meyer of Germany Published nearly identical schemes

Note taking time

Henry Moseley 1913 Developed the concept of atomic numbers

Groups Vertical Columns Families Elements have similar properties Same number of valence electrons (the number of electrons in outer most shell)

Periods Horizontal rows Period number corresponds to number of energy levels

Periodic Table Most of the elements are metals Gases – H,N,O,F,Cl and Group 18 Liquids – Hg and Br

Page 4 – Coloring Time GROUP IA GROUP IIA GROUP VIIA GROUP VIII (0) 2 Period    GROUP IA    GROUP IIA Transition Metals GROUP IIIA GROUP IVA GROUP VA GROUP VIA    GROUP VIIA    GROUP VIII (0) 1 2 He -    2 3 Li 1.0 4 Be 1.5 5 B 2.0 6 C 2.5 7 N 3.0 8 O 3.5 9 F 4.0 10 Ne - 3 11 Na 0.9 12 Mg 1.2 13 Al 1.5 14 Si 1.8 15 P 2.1 16 S 2.5 17 Cl 3.0 18 Ar - 4 19 K 0.8 20 Ca 1.0 21 Sc 1.3 22 Ti 1.5 23 V 1.6 24 Cr 1.6 25 Mn 1.5 26 Fe 1.8 27 Co 1.9 28 Ni 1.9 29 Cu 1.9 30 Zn 1.6 31 Ga 1.6 32 Ge 1.8 33 As 2.0 34 Se 2.4 35 Br 2.8 36 Kr - 5 37 Rb 0.8 38 Sr 1.0 39 Y 1.2 40 Zr 1.4 41 Nb 1.6 42 Mo 1.8 43 Tc 1.9 44 Ru 2.2 45 Rh 2.2 46 Pd 2.2 47 Ag 1.9 48 Cd 1.7 49 In 1.7 50 Sn 1.8 51 Sb 1.9 52 Te 2.1 53 I 2.5 54 Xe - 6 55 Cs 0.7 56 Ba 0.9 57 La 1.1 72 Hf 1.3 73 Ta 1.5 74 W 1.7 75 Re 1.9 76 Os 2.2 77 Ir 2.2 78 Pt 2.2 79 Au 2.4 80 Hg 1.9 81 Tl 1.8 82 Pb 1.9 83 Bi 1.9 84 Po 2.0 85 At 2.2 86 Rn - 7 87 Fr 0.7 88 Ra 0.9 89 Ac 1.1 104 Rf - 105 Ha -

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Metals Left of zig zag line Low ionization energy and electronegativity Lose electrons to form positive ions Metallic luster when polished Good conductor of heat and electricity Malleable (made into sheets) Ductile (made into wire) Most are solid at room Temperature (Hg is a liquid)

Lower Left of Table Most Metallic Character Most reactive metal

Nonmetals Right of zig zag line (except group 18 – Noble gases) Gain electrons to form form negative ions High ionization energy (attraction for electrons) and high electronegativity Lack luster and form brittle solids Poor conductors of heat and electricity Exist as gases (mostly) solids (molecular or network) bromine is a volatile liquid at room temperature.

Metalloids Touch zig zag Known as semi-metals At the border of metals and nonmetals Properties are similar to metals and nonmetals Boron, silicon, germanium, arsenic, antimony and tellurium

Metalloids

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Trends Bottom left most reactive metal Top right (excluding group 18) most reactive nonmetal Metals – reactivity increases as you go down a group Nonmetals – reactivity increases as you go up a group

Ionization Energy Energy needed to remove an electron from an atom The greater the attraction for electrons the more energy is needed to remove the electron The smaller the ionization energy, the easier it is to remove an electron

Ionization Energy Li 520 B 801 O 1314 Ne 2081 Trend: Ionization Energy increases across a period.

Ionization Energy C 1086 Si 787 Ge 762 Pb 716 Trend: Ionization Energy decreases down a group.

Electronegativity Is the attraction for electrons. The larger the electronegativity the more the atom attracts electrons. 3 Factors Nuclear charge - # of protons, increase charge greater attraction Principal energy level – The higher the principal energy level of the outermost electrons, the greater the distance from the nucleus, the weaker is the pull Electron Cloud Effect – shields the outermost electrons from the nucleus. The inner electrons repel outermost electron

Electronegativity Li 1.0 B 2.0 O 3.4 Ne ----- Why doesn’t Ne have an Electronegativity? It is not reactive. Does not react with any element. Trend Electronegativity increases across a period.

Electronegativity C 2.6 Si 1.9 Ge 2.0 Pb 1.8 F 4 Cl 3.2 Br 3.0 I 2.7

Electronegativity decreases down a group. Trend: Electronegativity decreases down a group.

Atomic Radius Is half the distance between adjacent nuclei (the distance from the nucleus to the outer most valence electrons). Size of the atom Related to the attraction of the nucleus for its electrons Decreases as the atomic number increase as a result of the force of attraction between the positive nucleus and the negative electrons.

Atomic Radius Li 130 B 84 O 64 Ne 62 Trend: Atomic Radius decreases across a period.

Atomic Radius C 75 Si 114 Ge 120 Pb 145 Trend: Atomic Radius increases down a group.

Ionic Radius Metals lose electrons, ionic radius becomes smaller Nonmetals gain electrons, the ionic radius becomes larger

Notes Now

Group 1 Elements Alkali Metals One valence electron React with acids to product hydrogen gas Form strong bases

Group 2 Metals Alkali earth metals 2 valence electrons Form weak bases

Metals Reactivity increases as we go down a group Reactivity decreases as we go across a period (left to right) Ex. Sodium is more reactive than Magnesium (period 3) Why? Sodium wants to give the one electron away faster. Group 1 – larger atomic size Group 2 – greater nuclear charge

Group 17 Halogens 7 valence electrons Diatomic molecules High electronegativity Very reactive, occurs in nature only as compounds All three phases of matter exist.

Phases Fluorine and chlorine are gases Br is a liquid Iodine and astatine are solids

Group 18 Noble Gases Inert Gases-old name, they were thought to be unreactive. Chemically unreactive Completely filled valence shells Monoatomic

Groups 3-11 Transition elements Positive oxidation states Formed colored compounds d sublevels – lose electrons from an inner energy level Forms ions of more than one stable charge Ex. Fe2+ and Fe3+

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What do all of these have in common?

They are all Carbon.

What do all of these have in common? Graphite Carbon Fiber Clothes Artist’s Charcoal Carbon Fiber Custom Wheel Charcoal Diamond

Allotropes

What is an allotrope? A structurally differentiated form of an element that exhibits allotropy.

What is allotropy? A property of certain elements, as carbon, sulfur, and phosphorus, of existing in two or more distinct forms.

A.K.A. When an element exists in pure forms that differ in the way the atoms are arranged.

Buckminsterfullerene

Sulfur Phosphorous Oxygen P4 and P2 Other Allotropes S4, S5, S8 O2 and O3