H Default Li Be B C N O F Na Mg Al Si P S Cl K Ca Sc Ti V Cr Mn Fe Co

H Default Li Be B C N O F Na Mg Al Si P S Cl K Ca Sc Ti V Cr Mn Fe Co
He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba * Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po At Rn Fr Ra ** Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv us Uuo La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

LONG FORM PERIODIC TABLE
Why Not Make the Periodic Table Symmetrical? H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm H LONG FORM PERIODIC TABLE He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv us Uuo

Pauling Electronegativity(χ)
Δχ Bond Type Example Non-Polar Covalent H2 ≥0.5 to >1 Polar Covalent HCl ≥1 to <2 Very Polar Covalent HF ≥2 Ionic Bond Na+Cl- 1 H 2.20 Pauling Electronegativity(χ) 2 He 3 Li 0.98 4 Be 1.57 5 B 2.04 6 C 2.55 7 N 3.04 8 O 3.44 9 F 3.98 10 Ne 11 Na 0.93 12 Mg 1.31 13 Al 1.61 14 Si 1.90 15 P 2.19 16 S 2.58 17 Cl 3.16 18 Ar 19 K 0.82 20 Ca 1.00 21 Sc 1.36 22 Ti 1.54 23 V 1.63 24 Cr 1.66 25 Mn 1.55 26 Fe 1.83 27 Co 1.88 28 Ni 1.91 29 Cu 30 Zn 1.65 31 Ga 1.81 32 Ge 2.01 33 As 2.18 34 Se 35 Br 2.96 36 Kr 3.00 37 Rb 38 Sr 0.95 39 Y 1.22 40 Zr 1.33 41 Nb 1.6 42 Mo 2.16 43 Tc 1.9 44 Ru 2.2 45 Rh 2.28 46 Pd 47 Ag 1.93 48 Cd 1.69 49 In 1.78 50 Sn 1.96 51 Sb 2.05 52 Te 2.1 53 I 2.66 54 Xe 2.60 55 Cs 0.79 56 Ba 0.89 * 72 Hf 1.3 73 Ta 1.5 74 W 2.36 75 Re 76 Os 77 Ir 78 Pt 79 Au 2.54 80 Hg 2.00 81 1.62 82 Pb 2.33 83 Bi 2.02 84 Po 2.0 85 At 86 Rn 87 Fr 0.7 88 Ra 0.9 ** 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 Ds 111 Rg 112 Cn 113 Uut 114 Fl 115 Uup 116 Lv 117 Uus 118 Uuo 57 La 1.1 58 Ce 1.12 59 Pr 1.13 60 Nd 1.14 61 Pm 62 Sm 1.17 63 Eu 1.2 64 Gd 65 Tb 66 Dy 67 Ho 1.23 68 Er 1.24 69 Tm 1.25 70 Yb 71 Lu 1.27 89 Ac 90 Th 91 Pa 92 U 1.38 93 Np 94 Pu 1.28 95 Am 96 Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr 1.291

Melting Point (C) Δχ Bond Type Example 0.0-0.5 Non-Polar Covalent H2
Δχ Bond Type Example Non-Polar Covalent H2 ≥0.5 to >1 Polar Covalent HCl ≥1 to <2 Very Polar Covalent HF ≥2 Ionic Bond Na+Cl- 1 H 2.20 Melting Point (C) 2 He 3 Li 0.98 4 Be 1.57 5 B 2.04 6 C 2.55 7 N 3.04 8 O 3.44 9 F 3.98 10 Ne 11 Na 0.93 12 Mg 1.31 13 Al 1.61 14 Si 1.90 15 P 2.19 16 S 2.58 17 Cl 3.16 18 Ar 19 K 0.82 20 Ca 1.00 21 Sc 1.36 22 Ti 1.54 23 V 1.63 24 Cr 1.66 25 Mn 1.55 26 Fe 1.83 27 Co 1.88 28 Ni 1.91 29 Cu 30 Zn 1.65 31 Ga 1.81 32 Ge 2.01 33 As 2.18 34 Se 35 Br 2.96 36 Kr 3.00 37 Rb 38 Sr 0.95 39 Y 1.22 40 Zr 1.33 41 Nb 1.6 42 Mo 2.16 43 Tc 1.9 44 Ru 2.2 45 Rh 2.28 46 Pd 47 Ag 1.93 48 Cd 1.69 49 In 1.78 50 Sn 1.96 51 Sb 2.05 52 Te 2.1 53 I 2.66 54 Xe 2.60 55 Cs 0.79 56 Ba 0.89 * 72 Hf 1.3 73 Ta 1.5 74 W 2.36 75 Re 76 Os 77 Ir 78 Pt 79 Au 2.54 80 Hg 2.00 81 1.62 82 Pb 2.33 83 Bi 2.02 84 Po 2.0 85 At 86 Rn 87 Fr 0.7 88 Ra 0.9 ** 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 Ds 111 Rg 112 Cn 113 Uut 114 Fl 115 Uup 116 Lv 117 Uus 118 Uuo 57 La 1.1 58 Ce 1.12 59 Pr 1.13 60 Nd 1.14 61 Pm 62 Sm 1.17 63 Eu 1.2 64 Gd 65 Tb 66 Dy 67 Ho 1.23 68 Er 1.24 69 Tm 1.25 70 Yb 71 Lu 1.27 89 Ac 90 Th 91 Pa 92 U 1.38 93 Np 94 Pu 1.28 95 Am 96 Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr 1.291

The Periodic Table is Arranged With Metals on the Left
Metals (conductors): conduct Electricity and Heat well, high melting points, malleable, ductile. Non-metals (non-conductors): pretty much the opposite of metals (don’t conduct heat well, etc). Metalloids (semi-conductors): have properties similar to both metals and non-metals. The Periodic Table is Arranged With Metals on the Left Metals Mealloids Non-Metals Stepped-Line Separates Metals and Non-metals * **

Most Elements are Solids under Ambient Conditions
The majority of the periodic table consists of solid metals. Only one is a liquid (Mercury) at room temperature. Most of the Non-metals tend to all be gasses as room temperature with the exception or Bromine (a dark red liquid). Several are solids (e.g. carbon) Most Elements are Solids under Ambient Conditions Solid Liquid Gas Br * Hg **

He Ne Ar Kr Xe Rn Covalent Radii in Nanometers (1x10-9nm)
0.037 He 0.123 .089 0.088 0.077 0.070 0.066 0.064 Ne 0.157 0.136 0.125 0.117 0.110 0.104 0.099 Ar 0.203 0.174 0.122 0.121 0.114 Kr 0.216 0.192 0.150 0.140 0.141 0.137 0.133 Xe 0.235 0.198 0.155 0.154 0.152 0.153 Rn Covalent Radii in Nanometers (1x10-9nm) Noble Gases are inert and their covalent radius can’t be measured in the same way H H Li Be B C N O F Na Mg Al Si P S Cl Size Decreases Energy Levels are constant but nuclear charge increases. K Ca Ga Ge As Se Br Increasing Electron Energy Levels Size Increases Rb Sr In Sb Te Sn I Cs Ba Tl Pb Bi Po At

H1+ He Li1+ Be2+ N3- O2- F1- Ne Na1+ Al3+ P3- S2- Cl1- Ar K1+ Ca2+
2s22p6 Nitride N3- Oxide O2- Fluoride F1- Ne Na1+ Mg2+ Al3+ 3s23p6 Phosphide P3- Sulfide S2- Chloride Cl1- Ar K1+ Ca2+ Sc+3 Ti+4 V2+ V3+ V4+ V5+ Cr2+ Cr3+ Mn2+ Mn3+ Mn4+ Mn6+ Mn7+ 4s03p6 Fe2+ 4s03d7 Co2+ 4s03d8 Ni2+ 4s03d10 Cu1+ 3d10 Zn2+ 4s24p6 Selenide Se2- Bromide Br1- Kr 4s03p5 Fe3+ 4s03d6 Co3+ 4s03d9 Cu2+ Rb1+ Sr2+ 5s04d10 Ag1+ 4d10 Cd2+ 4d105s2 Sn2+ 5s25p6 Iodide I1- Xe Sn4+ Cs1+ Ba2+ 6s04f145d10 Au+1 4f145d10 Hg2+ 4f145d106s2 Pb2+ Bi3+ Rn 6s26p6 5d10

Common Polyatomic Ions and their Charge
Acetate Ammonium Carbonate Chlorate Chlorite Chromate Cyanide Dichromate C2H3O2- NH4+ CO32- ClO3- ClO2- CrO42- CN- Cr2O72- Bicarbonate Bisulfate Bisulfite Hydronium Hydroxide Hypochlorite Nitrate Nitrite HSO4- HSO3- H3O+ OH- ClO- NO3- NO2 Oxalate Perchlorate Permanganate Phosphate Silicate Sulfate Sulfite Thiosulfate C2O42- ClO4- MnO4- PO43- SiO32- SO42- SO33- S2O32- 1s0 H1+ He 1s2 Li1+ Be2+ 2s22p6 Nitride N3- Oxide O2- Fluoride F1- Ne Na1+ Mg2+ Al3+ 3s23p6 Phosphide P3- Sulfide S2- Chloride Cl1- Ar K1+ Ca2+ Sc+3 Ti+4 V2+ V3+ V4+ V5+ Cr2+ Cr3+ Mn2+ Mn3+ Mn4+ Mn6+ Mn7+ 4s03p6 Fe2+ 4s03d7 Co2+ 4s03d8 Ni2+ 4s03d10 Cu1+ 3d10 Zn2+ 4s24p6 Selenide Se2- Bromide Br1- Kr 4s03p5 Fe3+ 4s03d6 Co3+ 4s03d9 Cu2+ Rb1+ Sr2+ 5s04d10 Ag1+ 4d10 Cd2+ 4d105s2 Sn2+ 5s25p6 Iodide I1- Xe Sn4+ Cs1+ Ba2+ 6s04f145d10 Au+1 4f145d10 Hg2+ 4f145d106s2 Pb2+ Bi3+ Rn 6s26p6 5d10 Monatomic Ions

H 1s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d10 He 1s2 Li 2s1 Be
C 2p2 N 2p3 O 2p4 2p5 Ne 2p6 Na 3s1 Mg 3s2 Al 3p1 Si 3p2 3p3 3p4 Cl 3p5 Ar 3p6 K 4s1 Ca 4s2 Sc 3d1 Ti 3d2 V 3d3 Cr 3d5 Mn Fe 3d6 Co 3d7 Ni 3d8 Cu 3d10 Zn Ga 4p1 Ge 4p2 As 4p3 Se 4p4 Br 4p5 Kr 4p6 Rb 5s1 Sr 5s2 Y 4d1 Zr 4d2 Nb 4d4 Mo 4d5 Tc Ru 4d7 Rh 4d8 Pd 4d10 Ag Cd In 5p1 Sn 5p2 Sb 5p3 Te 5p4 I 5p5 Xe 5p6 Cs 6s1 Ba 6s2 * Hf 5d2 Ta 5d3 W 5d4 Re 5d5 Os 5d6 Ir 5d7 Pt 5d9 Au 5d10 Hg 6p1 Pb 6p2 Bi 6p3 Po 6p4 At 6p5 Rn 6p6 Fr 7s1 Ra 7s2 ** Rf 6d2 Db 6d3 Sg 6d4 Bh 6d5 Hs 6d6 Mt 6d7 Ds 6d8 Rg 6d10 Cn La 5d1 Ce 4f15d1 Pr 4f3 Nd 4f4 Pm 4f5 Sm 4f6 Eu 4f7 Gd 4f75d1 Tb 4f9 Dy 4f10 Ho 4f11 Er 4f12 Tm 4f13 Yb 4f14 Lu Ac 6d1 Th Pa 5f26d1 U 5f36d1 Np 5f46d1 Pu 5f6 Am 5f7 Cm 5f76d1 Bk 5f9 Cf 5f10 Es 5f11 Fm 5f12 Md 5f13 No 5f14 Lr

Atomic mass in [brackets] is for the most stable isotope .
1 H Hydrogen 1.0079 Alkali Metals Alkaline Earth Metals Transition Metals Lanthanides Actinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium 4.003 3 Li Lithium 6.941 4 Be Beryllium 9.0122 5 B Boron 10.811 6 C Carbon 12.011 7 N Nitrogen 14.007 8 O Oxygen 15.999 9 F Fluorine 18.998 10 Ne Neon 20.180 11 Na Sodium 22.990 12 Mg Magnesium 24.305 13 Al Aluminum 26.982 14 Si Silicon 28.086 15 P Phosphorus 30.974 16 S Sulfur 32.066 17 Cl Chlorine 35.453 18 Ar Argon 39.948 19 K Potassium 39.098 20 Ca Calcium 40.078 21 Sc Scandium 44.956 22 Ti Titanium 47.88 23 V Vanadium 50.942 24 Cr Chromium 51.996 25 Mn Manganese 54.938 26 Fe Iron 55.933 27 Co Cobalt 58.933 28 Ni Nickel 58.693 29 Cu Copper 63.546 30 Zn Zinc 65.39 31 Ga Gallium 69.732 32 Ge Germanium 72.61 33 As Arsenic 74.922 34 Se Selenium 78.09 35 Br Bromine 79.904 36 Kr Krypton 84.80 37 Rb Rubidium 85.468 38 Sr Strontium 87.62 39 Y Yttrium 88.906 40 Zr Zirconium 91.224 41 Nb Niobium 92.906 42 Mo Molybdenum 95.94 43 Tc Technetium 98.907 44 Ru Ruthenium 101.07 45 Rh Rhodium 46 Pd Palladium 106.42 47 Ag Silver 48 Cd Cadmium 49 In Indium 50 Sn Tin 118.71 51 Sb Antimony 52 Te Tellurium 127.6 53 I Iodine 54 Xe Xenon 131.29 55 Cs Cesium 132.91 56 Ba Barium 137.33 * 57-71 72 Hf Hafnium 178.49 73 Ta Tantalum 74 W Tungsten 183.85 75 Re Rhenium 76 Os Osmium 190.23 77 Ir Iridium 192.22 78 Pt Platinum 195.08 79 Au Gold 80 Hg Mercury 200.59 81 Tl Thallium 82 Pb Lead 207.2 83 Bi Bismuth 84 Po Polonium [ ] 85 At Astatine 86 Rn Radon 87 Fr Francium [223] 88 Ra [226] ** 89-103 104 Rf Rutherfordium [261] 105 Db Dubnium [262] 106 Sg Seaborgium [266] 107 Bh Bohrium [264] 108 Hs Hassium [269] 109 Mt Meitnerium [268] 110 Ds Darmstadtium 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium 116 Lv Livermorium [298] 117 Uus Ununseptium 118 Uuo Ununoctium 57 La Lanthanum 58 Ce Cerium 59 Pr Praseodymium 60 Nd Neodymium 144.24 61 Pm Promethium 62 Sm Samarium 150.36 63 Eu Europium 64 Gd Gadolinium 157.25 65 Tb Terbium 66 Dy Dysprosium 162.50 67 Ho Holmium 68 Er Erbium 167.26 69 Tm Thulium 70 Yb Ytterbium 173.04 71 Lu Lutetium 89 Ac Actinium 90 Th Thorium 91 Pa Protactinium 92 U Uranium 93 Np Neptunium 94 Pu Plutonium 95 Am Americium 96 Cm Curium 97 Bk Berkelium 98 Cf Californium 99 Es Einsteinium [254] 100 Fm Fermium 101 Md Mendelevium 258.1 102 No Nobelium 103 Lr Lawrencium 2 2A 1 H Hydrogen 1.0079 Atomic Number Element Symbol Element Name Atomic Mass 13 3A A A A A Periodic Table Atomic mass in [brackets] is for the most stable isotope .

1s22s22p63s23p64s23d104p65s24d10 4p6 3p6 2p6 4d10 3d10 1s2 2s2 3s2 4s2 5s2 Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding) 4f14

1s22s22p63s23p64s23d10 4p65s24d105p66s24f145d106p67s25f146d107p6 1s2
Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

We are going to talk about bonding Bonding between atoms is CIM
Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

__ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s s p s p s d p s d p s f14

H Default Li Be B C N O F Na Mg Al Si P S Cl K Ca Sc Ti V Cr Mn Fe Co

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H Default Li Be B C N O F Na Mg Al Si P S Cl K Ca Sc Ti V Cr Mn Fe Co

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