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The Periodic Table YAYYYYYYYYYYYYY!!!!!!!!!!!!!!!!!!!!!!!!

The Periodic Table YAYYYYYYYYYYYYY!!!!!!!!!!!!!!!!!!!!!!!!. Dmitri Mendeleev. Russian Chemist In 1869, he published the first periodic table . Organized the elements in a way that would help his students learn them more easily.

dorian-caldwell
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The Periodic Table YAYYYYYYYYYYYYY!!!!!!!!!!!!!!!!!!!!!!!!

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  1. The Periodic TableYAYYYYYYYYYYYYY!!!!!!!!!!!!!!!!!!!!!!!!

  2. Dmitri Mendeleev • Russian Chemist • In 1869, he published the first periodic table. • Organized the elements in a way that would help his students learn them more easily. • Set it up as a card game with the information known about each element listed on a separate card, then arranged them in various ways.

  3. Periodic Law • Mendeleev settled on an organization of elements that was based on the masses of the elements. • Mendeleev found that when the elements were arranged in order of atomic mass, many physical and chemical properties of the elements followed repeating patterns. • Worked for most elements, but not all. • Three pairs of elements had to be switched, but Mendeleev thought these masses were measured incorrectly.

  4. Ekasilicon • Mendeleev was able to accurately predict the existence of elements not yet discovered. These showed up as gaps in his periodic table. • One such element gap, Mendeleev called ekasilicon. He predicted its mass, density, melting point and color based on its location in the periodic table. • Fifteen years after this prediction, a new element was discovered in in Germany and given the name Germanium. Its properties matched the properties of ekasilicon.

  5. Modern Periodic Law • H.G.J Moseley worked in Rutherford’s lab. • Found that metals produce X-rays when bombarded with energetic electrons and that the frequencies differed for each metal. These frequencies, came from differences in a fundamental property of each element; the amount of positive charge in the nucleus. • (The number of protons – The atomic #)

  6. Modern Periodic Law • This proved that the correct way to arrange elements is not by atomic mass, but by atomic number. • When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.

  7. Periodic Table Arrangement • Horizontal rows are called Periods. • The modern periodic table has 7 Periods. • The period tells the number of principal energy levels. (Principal Quantum Number) • Vertical columns are called Groups (or Families) Elements in a group behave similarly to each other. • The modern periodic table has 18 groups. • Group can tell number of valence electrons.

  8. Li = 1s22s1 Na = 1s22s22p63s1 K = 1s22s22p63s23p64s1 *Li, Na, K all have 1 valence e- *All are found in group 1 or IA *Li in row 2 Na in row 3 K in row 4 B = 1s22s22p1 Al = 1s22s22p63s23p1 Ga = 1s22s22p63s23p64s23d104p1 *B, Al, Ga all have 3 valence e- *All are found in group 13 or IIIA *B in row 2 Al in row 3 Ga in row 4

  9. N = 1s22s22p3 P = 1s22s22p63s23p3 As = 1s22s22p63s23p64s23d104p3 *N, P, As all have 5 valence e- *All are found in group 15 or VA *N in row 2 P in row 3 As in row 4 F = 1s22s22p5Cl = 1s22s22p63s23p5 Br = 1s22s22p63s23p64s23d10p5 *F, Cl, Br all have 7 valence e- *All are found in group 17 or VIIA *F in row 2 Cl in row 3 Br in row 4

  10. Periodic Table

  11. Periodic Table H He B C N O F Ne Li Be Na Mg Al Si P S Cl Ar K Ca Fe Cu Zn Sn I Ag Hg Pb Au U

  12. Atomic Number • The number of protons in one atom of a given element. • Increases as you move down a group. • Increases as you move from left to right across a period.

  13. Average Atomic Mass • The average mass of all the isotopes of a given element. • Increases as you move down a group. • Increases as you move from left to right across a period.

  14. Metal, Nonmetal, Metalloid Trend • Elements on the left side of the periodic table are metals. • There are 88 metals on the periodic table. • Elements on the right side are nonmetals. • There are 17 nonmetals on the periodic table. • Elements on the “staircase” between the metals and nonmetals are metalloids. (also known as semimetals) • There are 7 metalloids on the periodic table.

  15. Periodic Table H He B C N O F Ne Li Be Na Mg Al Si P S Cl Ar K Ca Fe Cu Zn Sn I Ag Hg Pb Au Metal Division Line U

  16. Periodic Table H He B C N O F Ne Li Be Na Mg Al Si P S Cl Ar K Ca Fe Cu Zn Sn I Ag Hg Pb Au Metal Division Line U Metalloids

  17. Periodic Table H He B C N O F Ne Li Be Ar Na Mg Al Si P S Cl K Ca Fe Cu Zn Sn I Ag Hg Pb Au Metal Division Line U Metalloids Nonmetals

  18. Periodic Table H He B C N O F Ne Li Be Ar Na Mg Al Si P S Cl K Ca Fe Cu Zn Sn I Ag Hg Pb Au Metal Division Line U Metalloids Nonmetals Metals

  19. Periodic Table 1 18 H He 2 13 14 15 16 17 B C N O F Ne Li Be Ar Na Mg Al Si P S Cl 3 4 5 6 7 8 9 10 11 12 K Ca Fe Cu Zn Sn I Ag Hg Pb Au Metal Division Line U Metalloids Groups Columns 1-18 (#e- in outside shell) Nonmetals Metals

  20. IA Periodic Table VIIIA 1 IVA VIA 18 H IIA IIIA VA VIIA He 2 13 14 15 16 17 B C N O F Ne Li Be Ar Na Mg Al Si P S Cl 3 4 5 6 7 8 9 10 11 12 K Ca Fe Cu Zn Sn I Ag Hg Pb Au Metal Division Line U Metalloids Groups Columns 1-18 (#e- in outside shell) Nonmetals Metals

  21. IA Periodic Table VIIIA 1 IVA VIA 18 H IIA 1 IIIA VA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 5 5 Sn I Ag Hg Pb 6 Au 6 7 Metal Division Line U Metalloids Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Metals

  22. Atomic Radius Trend • Radius – The distance from the center of an atom’s nucleus to its outermost electron. • The electron cloud does not have an exact boundary, so we typically measure atomic radius by measuring the distance from the centers of two bonded atoms, then halving that measurement.

  23. Atomic Radius Trend • On the periodic table: • the atomic radius increases as you go down a group. • The principal quantum number increases (an energy level is added for additional electrons) • The atomic radius decreases as you go across a period. • As protons are added, the pull on electrons increases. This shrinks the orbital and makes the atom smaller. Full shells occupy less space.

  24. IA Periodic Table VIIIA 1 IVA VIA 18 H IIA 1 IIIA VA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 5 5 Sn I Ag Hg Pb 6 Au 6 7 Metal Division Line U Metalloids Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Atomic Radius Nonmetals Metals

  25. Groups of the Periodic Table • Remember that elements in a group on the periodic table have similar properties to each other. • This is due to the number of valence electrons. Having the same number of valence electrons makes them bond to similar atoms in the same ratios. • If you know the properties of one element in a group, you know the properties of all the elements in that group!!!

  26. IA Periodic Table VIIIA 1 IVA VIA 18 H IIA 1 IIIA VA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Metal Division Line Most active metal U Metalloids Atomic Radius Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Metals

  27. IA Alkali Metals Periodic Table VIIIA 1 IVA VIA 18 H IIA 1 IIIA VA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Metal Division Line Most active metal U Metalloids Periods Rows 1-7 (# of shells) Atomic Radius Groups Columns 1-18 (#e- in outside shell) Nonmetals Metals

  28. Alkali Metals IA Periodic Table VIIIA 1 Alkaline Earth Metals IVA VIA 18 H IIA 1 IIIA VA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 Transition Metals 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Metal Division Line Most active metal U Metalloids Periods Rows 1-7 (# of shells) Atomic Radius Groups Columns 1-18 (#e- in outside shell) Nonmetals Metals

  29. Alkali Metals IA Periodic Table Halogens VIIIA 1 Alkaline Earth Metals 18 H IIA 1 IIIA IVA VA VIA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 Transition Metals 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Metal Division Line Most active metal U Metalloids Atomic Radius Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Metals

  30. Alkali Metals IA Periodic Table Noble Gases 1 VIIIA Alkaline Earth Metals Halogens 18 H IIA 1 IIIA IVA VA VIA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 Transition Metals 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Metal Division Line Most active metal U Metalloids Atomic Radius Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Metals

  31. Alkali Metals IA Periodic Table Noble Gases 1 VIIIA Alkaline Earth Metals Halogens 18 H IIA 1 IIIA IVA VA VIA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 Transition Metals 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Most active metal Lanthanide U Metalloids Atomic Radius Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Metals

  32. Alkali Metals IA Periodic Table Noble Gases 1 VIIIA Alkaline Earth Metals Halogens 18 H IIA 1 IIIA IVA VA VIA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 Transition Metals 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Most active metal Lanthanide Actinide U Metalloids Atomic Radius Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Metals

  33. Alkali Metals IA Periodic Table Noble Gases 1 VIIIA Alkaline Earth Metals Halogens 18 H IIA 1 IIIA IVA VA VIA VIIA He 2 13 14 15 16 17 1 B C N O F Ne 2 Li Be 2 Ar 3 Na Mg Al Si P S Cl 3 3 4 5 6 7 8 9 10 11 12 4 K Ca Fe Cu Zn 4 Transition Metals 5 5 Sn I Ag Hg Pb 6 Au 6 7 Most active nonmetal Most active metal Lanthanide Actinide U Metalloids Inner Transition Metals Groups Columns 1-18 (#e- in outside shell) Periods Rows 1-7 (# of shells) Nonmetals Atomic Radius Metals

  34. Alkali Metals • Group 1 or 1A. • These elements have 1 valence electron which they will give up when bonding to become more stable. (full valence shell) Therefore, they will become +1 ions. • Alkali means “ashes.” Sodium and potassium are present in the ashes of burned plants.

  35. Alkali Metals • Alkali metals are very reactive. Will react with water and air! (Stored in oil.) • They are soft enough to be cut by a knife. • The members of this group are: (Not Hydrogen.) Li [He]2s1 Na [Ne]3s1 K [Ar]4s1 Rb [Kr]5s1 Cs [Xe]6s1 Fr [Rn]7s1

  36. Alkaline Earth Metals • Group 2 or 2A. • These elements have 2 valence electrons which they will give up when bonding to become more stable. (full valence shell) Therefore they will become +2 ions. • Obtained from alkaline earths. Earths were substances unchanged by fire.

  37. Alkaline Earth Metals • Alkaline Earth Metals are also very reactive. (Not as reactive as group I or 1A) • They have higher densities and melting points than the alkali metals. • Found in mineral deposits. • The members of this group are: Be [He]2s2 Mg [Ne]3s2 Ca [Ar]4s2 Sr [Kr]5s2 Ba [Xe]6s2 Ra [Rn]7s2

  38. Transition Metals • Groups 3 – 12 • Play an important role in living organisms, are extremely valuable as strong structurally useful materials. • Vary greatly in properties and abundance. • Most have high densities and high melting points. • Number of valence electrons varies, therefore ionic charge varies.

  39. Inner Transition Metals • Lanthanide and Actinide Series elements (“f” block elements) • Properties similar to Transition Metals • Many are man-made • Many are naturally radioactive (Large, unstable nuclei. Ratio of neutrons to protons is high) • Have two valence electrons. (after 6s2, 7s2)

  40. The Boron Group • Group 13 or 3A. • These elements have 3 valence electrons which they will give when bonding to become more stable. (full valence shell) Therefore they will become +3 ions. • The members of this group are: B [He]2s22p1 Al [Ne]3s23p1 Ga [Ar]4s24p1 In [Kr]5s25p1 Tl [Xe]6s26p1

  41. The Carbon Group • Group 14 or 4A. • These elements have 4 valence electrons which they can give up, share or accept to become more stable. (full valence shell) Therefore they can become +4 or –4 ions. • The members of this group are: C [He]2s22p2 Si [Ne]3s23p2 Ge [Ar]4s24p2 Sn [Kr]5s25p2 Pb [Xe]6s26p2

  42. The Nitrogen Group • Group 15 or 5A. • These elements have 5 valence electrons. They will accept 3 more to become stable. (full valence shell) Therefore they become –3 ions. • The members of this group are: N [He]2s22p3 P [Ne]3s23p3 As [Ar]4s24p3 Sb [Kr]5s25p3 Bi [Xe]6s26p3

  43. The Oxygen Group • Group 16 or 6A. • These elements have 6 valence electrons. They will accept 2 more to become more stable. (full valence shell) Therefore they become –2 ions. • The members of this group are: O [He]2s22p4 S [Ne]3s23p4 Se [Ar]4s24p4 Te [Kr]5s25p4 Po [Xe]6s26p4

  44. The Halogen Group • Group 17 or 7A. • These elements have 7 valence electrons. They will accept 1 more to become more stable. (full valence shell) Therefore they become –1 ions. • Comes from the Greek word which means “salt former.”

  45. The Halogen Group • The Halogens are very reactive nonmetals and exist in elemental form as diatomic molecules. (F2, Cl2, Br2, I2, At2) • The members of this group are: F [He]2s22p5 Cl [Ne]3s23p5 Br [Ar]4s24p5 I [Kr]5s25p5 At [Xe]6s26p5

  46. The Noble Gases • Group 18 or 8A. • These elements have 8 valence electrons.(Except helium, which has 2) They are already stable, so they do not accept or receive electrons. They do not typically form ions. • These elements are very stable.

  47. The Noble Gases • Members of this group include: Helium 1s2 Neon [He] 2s22p6 Argon [Ne] 3s23p6 Krypton [Ar] 4s23d104p6 Xenon [Kr] 5s24d105p6 Radon [Rn] 6s24f145d106p6

  48. Ionization Energy Trend • Ionization Energy – the energy needed to remove one electron from an atom. (How strongly an atom holds onto its outermost electron.) • 1st ionization energy – energy to remove one e- • 2nd ionization energy – energy to remove a second e- • 3rd ionization energy – energy to remove a third e- etc…

  49. Ionization Energy Trend • An atoms successive ionization energies do not increase smoothly. For example: Magnesium Its 1st ionization energy is 738 kJ/mol. Its 2nd ionization energy is 1451 kJ/mol. Its 3rd ionization energy is 7733 kJ/mol. Find magnesium on the periodic table. Does this trend make sense based on the position of magnesium in the periodic table? (2 s electrons, then a full p block)

  50. Ionization Energy Trend • Would you expect the ionization energy of sodium to be higher or lower than magnesium? • 1st ionization energy of Na = 496 kJ/mol • 2nd ionization energy of Na = 4562 kJ/mol There was a great increase in energy required to remove an electron after the first, due to the location of the next electron. Look up sodium on the periodic table… (1 s electron, then a full p block)

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