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Unlocking the Periodic Table: Mendeleev's Vision and Element Organization

Discover the genius of Dmitri Mendeleev and the significance of the Periodic Table in organizing elements by chemical properties, making predictions, and understanding atomic structure. Learn about isotopes, ions, atomic number, and more.

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Unlocking the Periodic Table: Mendeleev's Vision and Element Organization

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  1. Unit 5 Section 2 Notes A Guided Tour of the Periodic Table

  2. Who is Dmitri Mendeleev? (1834-1907) • In 1869,Dmitri Ivanovitch Mendeléev created the first accepted version of the periodic table.

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

  4. The Periodic Table • The periodic table groups similar elements together. This organization makes it easier to predict the properties of an element based on where it is in the periodic table.

  5. Elements • Elements in the periodic table are represented by their symbols. • The first letter is ALWAYS capital • If there is a second letter, it is ALWAYS lowercase • Every element has itsown unique symbol Cu C Carbon Copper

  6. How is the Periodic Table Organized? • The elements are arranged based on the number of protons in the nucleus. • Periodic Law: states that when elements are arranged in order of increasing atomic number, similarities in their properties will occur in a regular pattern.

  7. Periods in the Periodic Table • Period: a horizontal row of elements in the periodic table • As you move from left to right in a period, the number of protons and electrons increases by one • Elements in the same period DO NOT have similar properties; in fact, they change greatly across the row • The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

  8. Groups or Families in the Periodic Table • Group or family: a vertical column of elements in the periodic table • All elements in a family have the same number of valence electrons, so they have similar properties • For example, lithium (Li), sodium (Na), potassium (K), and other members of group 1 are all soft, white, shiny metals. • These elements are NOT exactly alike because they have different numbers of protons

  9. Ions • Ionization: the process of adding electrons to or removing electrons from an atom • Ion: an atom that has lost or gained one or more electrons and has a net electric charge • Cation: an ion with a positive charge • Anion: an ion with a negative charge

  10. Goal of Atoms • All atoms want to have a FULL octet (8 e- in outer shell) • They do this by gaining, losing, or sharing electrons

  11. 3 p+ 4 n0 3 p+ 4 n0 Metals and Electrons • Metals LOSE electrons to form cations • Example: Lithium loses one electron to become a lithium ion, written as Li+ Second energy level can hold up to 8 e-. It is easier to lose 1 e- than gain 7 more. After lithium loses an electron, it has a full outermost energy level. 2 electrons 3 electrons

  12. 9 p+ 10 n0 9 p+ 10 n0 Nonmetals and Electrons • Nonmetals GAIN electrons to form anions • Example: Fluorine gains one electron to become a fluoride ion, written as F- Second energy level can hold up to 8 e-. It is easier to gain 1 e- than lose 7 more. After fluorine gains an electron, it has a full outermost energy level. 9 electrons 10 electrons

  13. So, how do compounds form?

  14. So, how do compounds form?

  15. So, how do compounds form?

  16. Atomic Number • Atomic Number: how many protons are in the nucleus of an atom • Remember that ATOMS are neutral, so they have equal numbers of protons and electrons • Therefore, atomic number also tells the number of electrons for atoms only

  17. Mass Number (Atomic Mass) • Mass Number: the number of protons and neutrons in an atom • Mass number is ONLY protons and neutrons because they provide most of an atoms mass • The same element can have different mass numbers because they may have different numbers of neutrons.

  18. Isotopes • Isotopes: atoms of the same element having the same number of protons but different numbers of neutrons • Each “version” of the atom has the same number of protons and electrons

  19. Isotopes • Some isotopes are more common than others • For example, protium is found most often

  20. Calculating Neutrons in an atom • To calculate the number of neutrons in an atom, take mass number minus atomic number. Mass Number - Atomic Number # of Neutrons

  21. Average Atomic Mass • In the periodic table, the atomic mass is a decimal because it is an average of all the naturally occurring isotopes • When calculating neutrons from average atomic mass, round to the nearest whole number • Example: How many neutrons are in Zinc? (Atomic Number 30; Average atomic mass 65.39) • 65-30 = 35 neutrons

  22. How do you read the Periodic Table?

  23. Periodic Table Song • http://www.youtube.com/watch?v=zUDDiWtFtEM

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