Periodic Groups and Trends. Periodic Table PERIODIC GROUPS 9/18/2013
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1 Periodic Groups and Trends Periodic Table Periodicity: regular variations (or patterns) of properties with increasing atomic weight. Both chemical and physical properties vary in a periodic (repeating pattern). Get out your periodic tables and label the metals, nonmetals, and metalloids. Another name for metalloid is semi-metal. Group: vertical column of elements ( family ) Period: horizontal row of elements Color and label the groups/families of elements on the other side of your paper. Remember to create a legend. PERIODIC GROUPS alkali metals alkaline earth metals Transition metals lanthanides halogens noble gases alkali metals alkaline earth metals transition metals halogens noble gases lanthanides actinides actinides 1
2 Alkali Metals Group 1 on periodic table Very reactive Soft solids Readily combine with halogens (ex. NaCl) Tendency to lose one electron (+1 ion) sodium and water potassium and water Alkaline Earth Metals Group 2 on periodic table Abundant metals in the earth Not as reactive as alkali metals Higher density and melting point than alkali metals Generally form a +2 ion Transition Metals Groups 3-12 on periodic table Important for living organisms (think vitamins: multivitamins (they have iron, zinc, chromium, etc.) Halogens Group 7A on periodic table (***or GROUP 17) Salt former combines with groups 1 and 2 to form salts (ionic bonds) Form a -1 ion Noble Gases Group 8 on periodic table (** or GROUP 18) Relatively inert, or nonreactive Gases at room temperature Lanthanides Part of the inner transition metals Soft silvery metals Tarnish readily in air React slowly with water 2
3 Actinides Radioactive elements Part of the inner transition metals Forming Ions Atoms will gain or lose electrons to reach a more stable state Try to be like noble gases Those on the right of the periodic table will gain electrons (form negative ions) Those on the left will lose electrons (form positive ions) PERIODIC TRENDS Atomic radii Ionization energy Ionic radii Trend: increases down a group The atomic radius gets bigger because electrons are added to energy levels farther away from the nucleus. Plus, the inner electrons shield the outer electrons from the positive charge ( pull ) of the nucleus; known as the SHIELDING EFFECT Trend: decreases across a period As the # of protons in the nucleus increases, the positive charge increases and as a result, the pull on the electrons increases. 3
4 Definition: energy required to remove outer electrons Definition: energy required to remove outer electrons Trend: decreases down a group Electrons are in higher energy levels as you move down a group; they are further away from the positive pull of the nucleus and therefore easier to remove. Trend: increases across a period The increasing charge in the nucleus as you move across a period exerts greater pull on the electrons; it requires more energy to remove an electron. Ionic Radii Cations are always smaller than the metal atoms from which they are formed. (fewer electrons because metals LOSE electrons) Definition: the tendency of an atom to attract electrons to itself when chemically combined with another element Anions are always larger than the nonmetal atoms from which they are formed. (more electrons because nonmetals GAIN electrons) 4
5 Trend: decreases down a group Although the nuclear charge is increasing, the larger size produced by the added energy levels means the electrons are farther away from the nucleus; decreased attraction, so decreased electronegativity; plus, shielding effect Trend: increases across a period (noble gases excluded!) Nuclear charge is increasing, atomic radius is decreasing; attractive force that the nucleus can exert on another electron increases. Summing Up Periodic Trends 5
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