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Introduction to the Periodic Table

Introduction to the Periodic Table. ● Atoms ● Symbol ● Elements ● Atomic Mass ● Protons, Neutrons, and Electrons ● Valence Electrons ● Groups and Periods ● Metals ● Non metals ● Metalloids. https://www.youtube.com/watch?v=uPkEGAHo78o. I am Dmitri Mendeleev!.

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Introduction to the Periodic Table

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  1. Introduction to the Periodic Table ● Atoms ● Symbol ● Elements ● Atomic Mass● Protons, Neutrons, and Electrons ● Valence Electrons ● Groups and Periods ● Metals ● Non metals ● Metalloids https://www.youtube.com/watch?v=uPkEGAHo78o

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

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

  4. The Periodic Table is a useful way to arrange elements. • The vertical columns (↕) are called groups. • The horizontal rows (↔) are called periods. • Elements in the same group have similar properties. • Three quarters of the elements are metals. • One quarter of the elements are non-metals.

  5. Remember how to use the periodic table of elements

  6. How do you read the PERIODIC TABLE?

  7. 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.

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

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

  10. Reading the Elemental Box

  11. 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 MASS - ATOMIC NUMBER

  12. Practice! 2 He Atomic number the number of protons (p+) in an atom 4 Atomic mass the number of protons (p+) and neutrons (n) in an atom number of electrons =number of protons

  13. What is an ELEMENT? • A substance composed of a single kind of atom. • Cannot be broken down into another substance by chemical or physical means.

  14. The most abundant element in the earth’s crust is oxygen.

  15. Bohr’s model of the Atom electrons in orbits = Electron Cloud nucleus

  16. Protons ( p+ ) • Part of the nucleus • Have positive (+) charge

  17. Neutron ( 0 ) • Part of the nucleus • Have neutral charge

  18. Electrons ( e- ) • Orbit around the nucleus • Have negative (-) charge

  19. HELIUM ATOM + Electron Cloud (Electrons) proton N + - + N - N - neutron electron Nucleus (Protons + Neutrons)

  20. Atomic Structure • Atoms have 2 regions 1) Nucleus: the center of the atom that contains mostof the mass of the atom. 2) Electron cloud: surrounds the nucleus & takes up most of the space of the atom. Nucleus (Protons and Neutrons) Electron Cloud (Electrons)

  21. Atomic Structure There are two basic components in every atom: Electron Cloud Nucleus

  22. Valence Electrons https://www.youtube.com/watch?v=YbpsDiTBejI

  23. What is a Valence Electron? Valence electrons are the electrons in the outer shell that bond with other atoms = + 6 Valence Electrons 1 Valence Electron

  24. What is a Valence Electron? = valence electron

  25. What is a Valence Electron? = valence electron

  26. What is a Valence Electron? Valence electrons are the electrons in the outer shell that bond with other atoms Core electrons are under valence electrons = valence electron

  27. Outer Shells of Electrons The number of valence electrons determines an element’s chemical properties For example, the noble gases on the right side of the periodic table are inert Inert = do not react with other atoms

  28. Main Group Valence shells Group 1 2 13 14 15 16 17 18 As we move from left to right we add one electron at a time To the outermost Principal energy level – the Valence shell (1VE) (2VE) (3VE) (4VE) (5VE) (6VE) (7VE) (8VE)

  29. Noble Gases Noble gases are inert because they have 8 outer shell (=valence) electrons Having 8 outer shell electrons means the outer shell is full, and therefore can’t react

  30. Periodic Table Groups Columns on the periodic table are called GROUPS Elements in the same group have similar chemical properties. This is because each group has the same number of valence electrons

  31. Valence Electrons in Groups Elements in the periodic table are arranged in groups. Each group has the same number of valence electrons…. Group 5A Group 7A Group 1A Group 2A Group 4A Group 6A Group 8A Group 3A Group 1A has 1 valence electron, group 2A has 2 valence electrons, group 3A has 3 valence electrons……….

  32. Importance of Valence Electrons https://www.youtube.com/watch?v=cAnOUwPfHlk The entire periodic table is arranged according to the number of valence electrons each element has!! The reason they arrange the periodic table this way is because elements in each group react similarly (=same)

  33. Metals, Metalloids, and Non metals https://www.youtube.com/watch?v=QdajjpfwZEM

  34. Metals, Metalloids, andNonmetals

  35. Notice the difference between the appearance of the metals and nonmetals.

  36. Physical properties of METALS • Metals are SOLIDS. (except mercury) • Metals are HARD. (except Lithium, Potassium, Sodium)

  37. Physical Properties of METALS Metals have shiny luster. (or metallic luster) LUSTER – the way an object’s surface reflects light

  38. When you leave a spoon in a cup of hot drink, the bit poking out of the drink gets hot. Why? Conduction! METALS are the best conductors of heat. Best conductors: silver and copper

  39. Physical Properties of METALS • Metals are good conductors of electricity. Copper, silver, and gold are good electrical conductors. In a conductor, electric current can flow freely. Since metals have free electrons, they can carry a charge easily. Copper Wiring

  40. Physical Properties of METALS Metals are malleable. Malleable or Malleability - metals ability to be shaped or formed as by hammering or pressure; can be beaten into thin sheets Aluminum is malleable.

  41. Physical Properties of METALS Metals are ductile. Ductility or ductile – can be drawn into a wire

  42. Overview of Metals • Lustrous (Shiny) • Solids (at room temp) • Malleable – can be hammered flat • Ductile – can be pulled into wire • High Conductivity – ability to transfer heat or electricity to another object

  43. Physical Properties of NONMETALS Nonmetals have a dull luster. (They are not shiny!) Example: Phosphorus

  44. Physical Properties of NONMETALS Nonmetals are insulators. They do not conduct electricity or heat well.

  45. Physical Properties of NONMETALS Nonmetals are soft (except for diamonds and brittle. Example: Sulfur

  46. Nonmetals • Opposite of properties of metals • Not shiny (Not lustrous) • Poor conductors • Mostly gases (at room temperature) • Solids are brittle Sulfur

  47. METALLOIDS The elements contained in the classification of Metalloids:

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