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Introduction to the Periodic Table

Introduction to the Periodic Table. Atomic Number ● Symbol ● Atomic Mass. I am Dmitri Mendeleev!. I made the PERIODIC TABLE !. Mendeleev. Late 1800’s Arranged table by atomic mass Since chemical properties repeated periodically, he called the table the Periodic Table. HOW HIS WORKED…

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Introduction to the Periodic Table

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  1. Introduction to the Periodic Table Atomic Number ● Symbol ● Atomic Mass

  2. I am Dmitri Mendeleev! I made the PERIODIC TABLE !

  3. Mendeleev • Late 1800’s • Arranged table by atomic mass • Since chemical properties repeated periodically, he called the table the Periodic Table.

  4. HOW HIS WORKED… Put elements in rows by increasing atomic mass. Put elements in columns by the way they reacted. SOME PROBLEMS… left blank spaces for undiscovered elements. (Turned out he was right!) broke the pattern of increasing atomic weight to keep similar reacting elements together. Dmitri Mendeleev: Father of the Table

  5. Weird!!! Mendeleev left blank spaces in his table to keep the elements lined up according to their chemical properties. He predicted properties and mass numbers of elements yet to be discovered. And later, THEY WERE!!!! Creepy!

  6. The Current Periodic Table • Mendeleev wasn’t too far off. But there was room for improvement! • Mass doesn’t always increase from left to right in Mendeleev's table. • Now the elements are put in rows by increasing atomic numbers.

  7. Henry Moseley • 1913 • British • Corrected Mendeleev’s table by arranging elements by atomic number.

  8. Glenn T. Seaborg • co-discovered 10 new elements • in 1944 he moved 14 elements out of the main body of the periodic table to their current location below the Lanthanide series and Actinide series.

  9. Glenn T. Seaborg He is the only person to have an element named after him while still alive.

  10. Al Si Ne Li He P H Periodic Table Basics Be O Mg F Na N B C Cl

  11. What is the PERIODIC TABLE? • Shows all known elements in the universe. • Organizes the elements by chemical properties.

  12. Elements by Discovery Year

  13. How do you read the PERIODIC TABLE?

  14. What is the SYMBOL? • An abbreviation of the element name.

  15. What is the ATOMIC WEIGHT? • The number of protons and neutrons in the nucleus of an atom.

  16. What is the ATOMIC NUMBER? • The number of protons found in the nucleus of an atom Or • The number of electrons surrounding the nucleus of an atom.

  17. Again, how do I find the number of protons, electrons, and neutrons in an element using the periodic table? • # of PROTONS= ATOMIC NUMBER • # of ELECTRONS= ATOMIC NUMBER • # of NEUTRONS= ATOMIC _ ATOMIC WEIGHT NUMBER

  18. Atoms, Electrons & Energy Levels Electrons are the bonds that hold the world together!

  19. Periodic Law:When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties.

  20. Periodic Table Navigation

  21. The Current Periodic Table • The modern periodic table is organized into periods and families. • The horizontal rows are called periods and are labeled from 1 to 7. • The vertical columns are called families or groups and are labeled from 1 to 18.

  22. Periods • The horizontal rows on the Periodic Table are called periods. • Each row is its own period. • Elements in the same period increase by atomic number. • There are seven periods on the Periodic Table.

  23. Electron Cloud Structure Electrons within the electron cloud have different amounts of energy. Energy levels closer to the nucleus have lower levels of energy than those farther away.

  24. Levels • These energy levels are named using numbers 1 – 7. • The period the element is in determines the number of energy levels the element will have. • A complete and stable energy level will contain a maximum of eight electrons. More on this later…don’t freak!

  25. Rows are Periods and Periods are energy levels! There are 7 periods!

  26. The horizontal rows of the periodic table are called PERIODS.

  27. Each new period (row) represents an energy level added. 1 2 3 4 5 6 7

  28. Periods Do you see that the elements increase by one electron and one proton as you move across the table, left to right?

  29. Groups • Vertical columns on the Periodic Table are known as groups or families. • There are 18 groups on the Periodic Table

  30. Members of the same group have many similarities. • Physical and chemical properties • Valence electrons (hang on…I’m getting there!) • Oxidation numbers (I’m getting here too!) • Trends

  31. Valence and Oxidation Number • OK, since you could not wait… Valence is the number of electrons that an element has in its outermost energy level. NO questions now! • Oxidation number is the number of electrons that an element gains or loses when it forms a bond. Guess what? NO questions now either!

  32. The elements in any group of the periodic table have similar physical and chemical properties! The vertical columns of the periodic table are called GROUPS, or FAMILIES.

  33. 1 2 13 14 15 16 17 18 The GROUP provides information about the number of valence electrons.

  34. Periodic Table Trends

  35. Metal trivia Au was the first metal used, 6000 years ago. Ag and Cu followed a few thousand years later. Al not until the 1800’s.

  36. Metals Metals are found to the left of the stair-step line. Tend to give up (lose) electrons. Like to combine with non-metals to form ionic bonds. (wait…more later)

  37. Metals • Usually have 1 – 3 valence electrons • Good conductors of heat and electricity • Malleable – can be flattened into sheets • Ductile – can be pulled into a wire • Shiny • Solid at room temperature (except Mercury)

  38. Nonmetals Found to the right of the stair-step line. Only the noble gases are all nonmetals.

  39. Bonding in nonmetals Electrons are strongly attracted to the nucleus. Can form ionic or covalent bonds. Again, more later! ionic covalent

  40. Nonmetals • Usually have 4 – 8 valence electrons • Can be a solid, liquid, or gas at room temperature • Brittle (if a solid), so not ductile or malleable • Dull, not shiny • Poor conductors of heat and electricity

  41. Metalloids • Have properties of metals and nonmetals. • Can form covalent or ionic bonds. • semiconductors

  42. Exhibit characteristics of metals and nonmetals Semi-conductors – conduct electricity under special conditions The metalloids are: Boron Silicon Germanium Arsenic Antimony Tellurium Polonium Astatine Metalloids

  43. Families

  44. Hydrogen Makes up 99% of the universe. Most H on Earth is found in water. The word hydrogen means “water forming”. Can be diatomic H2

  45. Hydrogen – the weird kid • Commonly has an oxidation number of +1 and one valence electron, so it is grouped with the alkali metals. • But its natural state is a gas, so it really isn’t an alkali metal. • Sometimes has an oxidation number of -1, so it is occasionally grouped with group 17 – the halogens. • Happy now?

  46. Alkali Metals • 1 electron in outer energy shell • React with water to release H2 gas • The most reactive metals

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