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The Periodic Table Basics & Naming & Formulas of Compounds

The Periodic Table Basics & Naming & Formulas of Compounds. Chemistry-CP Periods 4 & 6. J.W. Dobereiner. In 1860, there were only 63 elements known Classified some elements into triads--groups of three

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The Periodic Table Basics & Naming & Formulas of Compounds

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  1. The Periodic Table Basics & Naming & Formulas of Compounds Chemistry-CP Periods 4 & 6

  2. J.W. Dobereiner • In 1860, there were only 63 elements known • Classified some elements into triads--groups of three • Triads had: Similar chemical properties & physical properties that varied in an orderly way • Important because: He grouped elements with similar properties revealing an orderly pattern in the elements’ properties.

  3. Examples of Triads • Halogen Triad: Chlorine, Bromine and Iodine • Coinage Triad: Copper, Silver & Gold • Metal Triad: Calcium, Strontium & Barium

  4. J.A.R. Newlands (1865) • Realized that when the elements were arranged by increasing atomic mass, the properties of the 8th element were similar to the 1st element. • Law of Octaves: The periodic pattern repeats itself every 8 elements

  5. Dmitri Mendeleev • Russian chemist who developed the first periodic table • Listed the elements according to atomic mass • Important because: He showed the properties of the elements repeat in an orderly way from row to row of the table

  6. Periodicity: the tendency to recur at regular intervals • Things that are periodic:

  7. Mendeleev’s periodic table was so successful because it allowed him to predict the properties of still unknown elements • Eka-Aluminum (Gallium) • Eka-Silicon (Germanium)

  8. Lothar Meyer (1869) • Published almost the same element classification scheme as Mendeleev but did not receive credit because Mendeleev revealed his first and Mendeleev was more successful at demonstrating its usefulness

  9. Henry Moseley • Realized that the periodic table was not in the perfect order • Arranged the modern periodic table. • Listed the elements according to atomic number • Important because: once arranged by atomic number all the elements were in order by their chemical & physical properties • The modern periodic table is listed in order of atomic number

  10. Periodic Law • The physical and chemical properties of the elements repeat in a regular pattern when they are arranged in order of increasing atomic number

  11. Periodic Table • Arrangement of the elements in order of their atomic numbers so that the elements are periodic functions of their atomic numbers.

  12. Element Key: • Includes the element symbol, element name, atomic mass and atomic number • May include other information

  13. Groups (also called Families) • The vertical columns on the periodic table • There are 18 groups, labeled with the numbers 1-18. 1 18 2 13 14 15 16 17 3 4 5 6 7 8 9 10 11 12

  14. Group Names Alkal i Metals Noble Gases Alkal ine Earth Met. Boron Group Carbon Group Nitrogen Group Oxygen Group Halogens Transition Metals Lanthanides Actinides

  15. Periods • Horizontal Rows on the Periodic Table • There are 7 periods labeled with the numbers 1-7. 1 2 3 4 5 6 7

  16. Examples

  17. States of Matter (at Room Temp.) Solids: Black lettering on the wall periodic table Liquids: Blue lettering on the wall periodic table (Hg & Br) Gases: Red lettering on the wall periodic table (noble gases, F, Cl, O, N, H)

  18. METALSLeft of the zig-zag lineException: Hydrogen

  19. PROPERTIES OF METALS • Typically solids at room temperature • Good conductors of heat & electricity • High melting points • Luster (shiny) • Malleable (can be hammered into sheets) • Ductile (can be pulled into wires)

  20. Nonmetals-Located right of the zig-zag line Exception: hydrogen

  21. Nonmetals • Make up 99% of Earth’s atmosphere (Oxygen & Nitrogen) • Do not conduct electricity and poor conductors of heat • Brittle when solids • Many are gases at room temperature • Lack luster • Low melting points

  22. MetalloidsElements bordered by the zig-zag line (exception: Al is a metal)

  23. Metalloids • Properties of the Metalloids • Have some chemical and physical properties of metals and other properties of nonmetals • Some are semiconductors • Semiconductor: An element that does not conduct electricity as well as a metal but does conduct slightly better than a nonmetal • Computers, Handheld electronic devices, calculators

  24. Radioactive Elements • Elements with atomic numbers higher than 82 • Radioactivity: Spontaneous emission of radiation • Elements are radioactive because they have too many or too few neutrons • The protons in the nucleus naturally repel each other. The neutrons are the “glue” that hold the nucleus together.

  25. Synthetic Elements • The synthetic elements are the elements with the outlined symbols on the wall periodic table. • Synthetic elements are not found in nature. They are man-made elements.

  26. Atomic Model Diagram

  27. ENERGY Electrons with the most energy are located farthest from the nucleus Electrons with the lowest energies are located close to the nucleus.

  28. ENERGY lEVELS The 4th energy level contains a maximum of 32 electrons Energy level 3 contains a maximum of 18 electrons Level 2 contains a maximum of 8 electrons Level 1 contains a maximum of 2 electrons

  29. EXAMPLES Draw an atomic diagram of:

  30. Atomic Model Diagram

  31. Valence Electrons • The # of electrons in the highest (outermost) energy level • Transition Metals: The # of valence electrons for a transition metal can vary due to the closeness of their s & d sublevels • Exceptions: • Silver is always 1 valence electron • Zinc is always 2 valence electrons • Inner Transition Metals: Typically have 3 valence electrons

  32. Lewis Dot Diagrams • The element symbol, used to represent the element’s inner level electrons, is surrounded by dots to represent the element’s valence electrons • The # of dots must equal the # of valence electrons, no more than 2 dots per side • Remember: The valence electrons can never be greater than 8, therefore, there can never be more than 8 dots.

  33. Oxidation Number • The charge an atom acquires when it gains or loses electrons to become stable • Ion: Atom that has a charge due to the loss or gain of electrons • Octet Rule: Atoms tend to gain, lose or share electrons so that each atom has a full outermost energy level which is typically 8 valence electrons (octet)

  34. ION • An atom becomes an ion when it gains or loses electrons • The protons in an atom never change—an atom CANNOT gain or lose protons

  35. ION An ion does not have equal numbers of protons and electrons (the positive does not = the negative)…therefore… an ION is a CHARGEDatom ATOM ION

  36. Oxidation Number • If an element loses electrons, its oxidation # is a _______________ number because: there are more positive protons than negative electrons Ca+ion (a positively charged ion) • Elements with 1-3 valence electrons: • Lose electrons to become stable • Form ions with a positive charge

  37. ATOM vs. CATION Positively charged proton Negatively charged electron

  38. Oxidation Number If an element gains electrons, its oxidation # is a _______________ number because: there are more negative electrons than positive protons. A n ion • Elements with 5-7 valence electrons: • Gain electrons to become stable • Form ions with a negative charge • Elements with 4 valence electrons: • Metals will lose electrons, becoming positive ions • Nonmetals will gain electrons, becoming negative ions egative

  39. ATOM vs. ANION Positively charged proton Negatively charged electron

  40. Oxidation Number

  41. Oxidation Number • Transition Metals • Oxidation #s may vary • Except: Ag+1 & Zn+2 • Inner Transition Metals: • Typically a +3 Oxidation Number

  42. Examples

  43. CA+IONS • To Name a Cation: Name the Metal • Transition Metals: Name the Metal followed by a Roman Numeral in Parentheses to Indicate the Metal’s charge • Remember: The oxidation number can change for transition metals, so it is important to indicate the metal’s charge • Exceptions: • Zinc is always +2 and Silver is always +1 so they are transition metals that do not require Roman Numerals

  44. ROMAN NUMERALS

  45. ANIONS • To Name: Change the ending of the nonmetal’s name to –ide. Examples: Sulfide, Iodide, Selenide

  46. ION SYMBOL • ElementSymbolOxidation# • The oxidation # is the charge the atom acquires when it gains or loses electrons to become stable (acquire 8 electrons) OXIDATION NUMBERS ARE PERIODIC

  47. EXAMPLES • Write the ion symbol for the ions formed from the following elements. a) Lithium b) Aluminum c) Silver d) Phosphorus e) Selenium f) Bromine

  48. MORE EXAMPLES • Name the following ions a) Fe2+ b) Cl- c) N3- d) K+ e) Zn2+ f) P3-

  49. POLYATOMIC IONS Common Polyatomic Ions—This table is on your periodic tables

  50. Polyatomic Ions • Names typically end in: • The only positively charged ion is: • Where should you look to find the polyatomic ions? -ate or -ite Ammonium (NH4+) Polyatomic Ion Chart on your Periodic Table

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