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Explore the history and organization of the periodic table, from Dobereiner's triads to Mendeleev's modern layout. Learn about element families, oxidation numbers, Lewis dot structures, and trends in atomic size and activity.
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History • Dobereiner • Created a table of triads (Groups of three elements)
Newlands • Designed a table called “Law of Octaves” (Groups of 8 elements)
Mendeleev • Considered the “Father of our Modern Table” • Arranged the elements according to increasing atomic mass • Left blank spaces for elements not yet discovered.
Problems with Mendeleev’s chart • Some elements did not fall into a group with other elements like it
Moseley • Fixed problems in Mendeleev’s Table • Arranged the elements by increasing atomic number
Each element in a box Element Name Number of Atomic Number electrons in each shell Element Symbol Average atomic Mass 2 8 18 2
Horizontal Rows • Called Periods or Series • Indicate: • outermost energy levels being filled
Vertical Columns • Called families or groups • Indicate: • Chemical Properties • Same number of electrons in outer shell (valence electrons) • Number at the top of each column indicates the number of electrons in the outer shell
Group 1 – Alkali Metals • Have 1 electron in outer shell (valence electron) • Fills “s” orbital with one electron • Most reactive metals
Group 2 – Alkaline Earth Metals • Has 2 electrons in the outer shell (valence electrons) • Fills s orbital with 2 electrons
Group 3 – Boron Family • Has 3 electrons in the outer shell • Fills p orbital with 1 electron • Contains both metals and metalloids
Group 4 – Carbon Family • Has 4 electrons in outer shell • Fills p orbital with 2 electrons • Contains metals, metalloids, and nonmetals
Group 5 – Nitrogen Family • Has 5 electrons in outer shell • Fills p orbital with 3 electrons • Contains metals, metalloids, and nonmetals
Group 6 – Chalcogen (oxygen) Family • Has 6 electrons in outer shell • Fills p orbital with 4 electrons • Contains metals, metalloids, and nonmetals
Group 7 – Halogen Family • “Salt Producers” • Has 7 electrons in outer shell • Fills p orbital with 5 electrons • Contains all nonmetals
Group 8 – Noble Gases • Has an octet in outer shell • Except helium – has only 2 electrons (s orbital full) • Fills p orbitals with 6 electrons • Inert gases (not reactive) • Contains all nonmetals
Transition Elements • All metals • Fill the d orbitals • Members of importance • W, Fe, Co, Pt, Cu, Ag, Au, Zn, Hg • Hg – is the only liquid at room temperature
Nonmetals (20%) • All on the right side of the table
Noble Gases (5%) All elements are trying to be like the noble gases. Lewis Dot for Noble Gas .. : x : ..
Oxidation Numbers • Number of electrons lost, gained, or shared to form bonds All atoms trying to get 8 electrons
If atoms lose electrons, they go down to a lower energy level that is filled • The atom will take on a positive charge • A positively charged atom = cation
If atom gains electrons, they fill up the outer shell • The atom takes on a negative charge • Negatively charged atom = anion
Oxidation Numbers for the families • Group 1 • +1 (lose 1 electron rather than gaining 7) • Group 2 • +2 (lose 2 electron rather than gaining 6) • Group 3 • +3 (lose 3 electron rather than gaining 5)
Oxidation Numbers for the families • Group 4 • +4 or -4 (can gain or lose 4. It is halfway to 8; tends to share)
Oxidation Numbers for the families • Group 5 • -3 (gains 3 electron rather than losing 5) • Group 6 • -2 (gains 2 electron rather than losing 6) • Group 7 • -1 (gains 1 electron rather than losing 7) • Group 8 • 0 (has an octet)
Transition Metals • Have more than 1 oxidation number • Cu • + 1 or +2 • Fe • +2 or +3
Atomic Size • Down a family: size increases • More shells are being added • Across a period: size decreases • Nuclear charge pulls electrons in slightly
Activity • Down the family • On the right side of the table • Activity decreases • Down the family • On the left side of the table • Activity increases
Activity • Across the period • On the top of the table, the activity increases • Across the period • On the bottom of the table, the activity decreases
Chemical Activity • Key elements • Francium: most active metal • Fluorine: most active nonmetal
Bonding • 2 types • Covalent: sharing electrons • Ionic: Transfer of electrons • Forming ions (cations and anions)
Electronegativity • The tendency of an atom to attract electrons when bonding • Metals of low electronegativity form cations • Metals of high electronegativity form anions
Ionization Energy (IE) • Energy required to remove an electron • Metals: low IE (e- easily removed) • Nonmetals: high IE (e- hard to remove)
Across periods: • IE increases • Down a group: • IE decreases
4 factors affecting IE • Nuclear charge: The greater the nuclear charge, the greater the IE • Shielding Effect: The greater the number of inner electrons, the less the IE