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Periodic Table

Periodic Table. Periodic Table- An arrangement of elements in columns based on properties that repeat from row to row. First organized by Dimitri Mendeleev, mo deled after the card game solitaire Elements were arranged into rows by increasing mass

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Periodic Table

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  1. Periodic Table

  2. Periodic Table-An arrangement of elements in columns based on properties that repeat from row to row. • First organized by DimitriMendeleev, modeled after the card game solitaire • Elements were arranged into rows by increasing mass • Similar properties were placed in the same column

  3. Today’s periodic table is arranged by atomic number • The atomic number increases as you move left to right • PERIOD - rows across • GROUP – columns up & down

  4. Review - ELEMENTS • Can not be chemically broken down into simpler substances • Arranged into 3 groups on table: metals, metalloids, non- metals • From left to right on the table elements become less like metals

  5. METALS • good conductors of electricity and heat, usually solid at room temperature, malleable, reactive • Blue elements on YOUR table • TRANSITION METALS – special group of metals found in the middle section of the table, (groups 3-12)

  6. METALLOIDS • Properties are in between the properties of metals and non- metals • All elements that share a border on the “Staircase” on your table

  7. Non- Metals • Poor conductors. Can be solid liquid or gas at room temperature, not reactive • Red elements on YOUR table

  8. Matter &The Atom

  9. Matter The term matter describes all of the physical substances around us Matter is anything that has mass and takes up space The Universe is made up of matter and energy

  10. *Matter is made up of atoms.*An atom is the smallest whole particle of matter. Atoms are the building blocks of matter.* Sub-Atomic particles are the tiny particles that make up an atom.

  11. Atomic Structure • NUCLEUS • The center of the atom. • All the particles are inside or around the nucleus

  12. Atomic Structure proton (p+) neutron (no) electron (e-)

  13. Atomic Structure • Proton (p+) • Located in the nucleus of the atom • Protons have a positive charge (+) • Much larger and heavier than electrons • Number of protons is different for each element. If the number of protons changes, the element changes.

  14. Atomic Structure • Neutron (n0) • Located in the nucleus of the atom • Neutral particle (has no electrical charge) • Largest particle, a bit bigger than a proton

  15. Atomic Structure • Electron (e-) • Found in a cloud outside the nucleus • Electrons have a negative charge (-) • Smallest particle • Orbit nucleus on energy levels

  16. Atomic Number = number of protons in each atom of any element • All atoms want to balance their protons and electrons to be NEUTRAL (no electrical charge) • In a neutral atom, the # of protons = the # of electrons

  17. Atomic Mass– the sum of the mass of all the protons and neutrons in an atom • -- measured in Atomic Mass Units (amu)

  18. Mass Number – sum of protons and neutrons in the nucleus • --can be used to find the number of neutrons in the nucleus • Mass # = atomic # + n or n = mass # - p

  19. ATOMIC NUMBER the number of (p+) and (e-) (+) = (-) ATOMIC MASS (MASS NUMBER) PROTONS (+) + NEUTRONS (0) PROTONS AND NEUTRONS = NUCLEUS 79 Au 197

  20. Isotope – when an atom has a different number of neutrons than other atoms of the same element • Example: 2 Oxygen Atoms, one has 8 neutrons one has 9.

  21. Isotopes • The number of protons for a given atom never changes. • The number of neutrons can change. • Two atoms with different numbers of neutrons are called isotopes • Isotopes have the same atomic # • Isotopes have different atomic Mass #’s

  22. Electrons • Electrons can be found in the electron cloud. • Energy Levels – electrons are located on these levels based on their energy

  23. The lowest energy level is closest to the nucleus • --It holds 2 e- • The 2nd energy level holds 8 e- • The 3rd energy level holds 8 e- • ELECTRONS FILL THE LEVELS FROM INSIDE OUT.

  24. Electrons can change levels when energy is added to or removed from the atom • If an e- gains energy it is in “excited state” and moves out an energy level • If it loses energy it goes in an energy level

  25. Valence Electrons - Number of electrons in outside row • Identified with a Roman numeral number at the top of each group • All elements in each group have the same number • Column VIII (group 18) has 2, 8 or 18 – it is FILLED! • Transition metals have no specific roman numeral

  26. PT COMMANDMENTS For atoms and elements

  27. 1. All atoms want to fill their outer energy level.

  28. 2. The roman numeral columns tell you how many electrons an atom has currently in its outside level.

  29. 3. • THE SUBATOMIC PARTICLES ARE: ELECTRONS(-)NEGATIVE electrical charge PROTONS (+) POSITIVE electrical charge NEUTRONS (0) NO electrical charge

  30. 4. • Protons have a mass of 1 atomic mass unit (AMU) • Electrons have almost zero mass (0 amu).

  31. 5. 79 ATOMIC NUMBER Au (the number of (p+) and (e-) ) 197 (+) = (-) 6. ATOMIC MASS PROTONS (+) + NEUTRONS (0) **don’t forget, protons and neutrons are in the nucleus!

  32. maximum number of 2 electrons electrons in each orbit 8 electrons 18 electrons Nucleus p+ and n0

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