Periodic Table of the Elements Notes
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1 Periodic Table of the Elements Notes Arrangement of the known elements based on atomic number and chemical and physical properties. Divided into three basic categories: Metals (left side of the table) Nonmetals (right side of the table) Metalloids (touching the zig zag line) Basic Organization by: Atomic structure Atomic number Chemical and Physical Properties Uses of the Periodic Table Useful in predicting: chemical behavior of the elements trends properties of the elements Atomic Structure Review: Atoms are made of protons, electrons, and neutrons. Elements are atoms of only one type. Elements are identified by the atomic number (# of protons in nucleus). Energy Levels Review: Electrons are arranged in a region around the nucleus called an electron cloud. Energy levels are located within the cloud. At least 1 energy level and as many as 7 energy levels exist in atoms Energy Levels & Valence Electrons Energy levels hold a specific amount of electrons: 1st level = up to 2 2nd level = up to 8 3rd level = up to 8 (first 18 elements only) The electrons in the outermost level are called valence electrons. Determine reactivity - how elements will react with others to form compounds Outermost level does not usually fill completely with electrons
2 Using the Table to Identify Valence Electrons Elements are grouped into vertical columns because they have similar properties. These are called groups or families. Groups are numbered Group numbers can help you determine the number of valence electrons: Group 1 has 1 valence electron. Group 2 has 2 valence electrons. Groups 3 12 are transition metals and have 1 or 2 valence electrons. Groups have 10 fewer than the group number. For example: Group 13 has 3 valence electrons. Group 15 has 5 valence electrons. Group 18 has 8 valence electrons (except He) Elements & Reactivity Reactivity is a chemical property that determines how elements will react with others to form compounds. What makes an element reactive? Number of valence electrons of each atom When outer levels are full, atoms are stable. When they are not full, they react: gain, lose, or share 1 or 2 electrons The most reactive metals are the elements in Groups 1 and 2. Elements in Group 1 generally lose an electron so their outer energy level is empty. Elements in Group 2 generally lose two electrons so their outer energy level is empty. These groups easily give up their valence electrons to make a compound. The most reactive nonmetals are the elements in Groups 16 and 17. Elements in Group 16 need two more electrons to fill their outer energy level. Elements in Group 17 need one more electron to fill their outer energy level. These groups gain valence electrons to make a compound. Groups Groups run vertically in the periodic table. They are numbered from Elements in the same groups have the same number of valence electrons in the outer energy level. Grouped elements behave chemically in similar ways.
3 Group 1: Alkali Metals Contains: Metals Valence Electrons: 1 Reactivity: Very Reactive most reactive group on the Periodic Table solids soft react violently with water shiny low density Group 2: Alkaline-Earth Metals Contains: Metals Valence Electrons: 2 Reactivity: very reactive, but less reactive than alkali metals (Group 1) Solids Silver colored More dense than alkali metals Groups 3-12 Transition Metals Contain: Metals Valence electrons: 1 or 2 Reactivity: less reactive than alkali and alkaline-earth metals Higher density Good conductors of heat and electricity Groups 3-12 Transition Metals--Below Main Table Contain: The Lanthanide and Actinide Series These two rows are pulled out of sequence and placed below the main table to keep the table from being too wide. Lanthanides are atomic numbers Actinides are atomic numbers Groups 3-12 Rare Earth Elements ~ Lanthanides Lanthanides follow the transition metal atomic number 57 Lanthanum in Period 6. Valence electrons: 3 Reactivity: Very reactive High luster, but tarnish easily High conductivity for electricity Very small differences between them
4 Groups 3-12 Rare Earth Elements ~ Actinides Actinides follow the transition metal atomic number 89 Actinium in Period 7 Valence electrons: 3 (but up to 6) Reactivity: unstable All are radioactive Most made in laboratories Metalloids A zig-zag line that separates metals from metalloids Elements from Groups contain some metalloids. Metalloids are Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium and Polonium These elements have characteristics of metals and nonmetals. Group 13: Boron Group Group 13: Boron Group Contains: 1 metalloid and 4 metals Valence Electrons: 3 Reactivity: Reactive Solid at room temperature Group 14: Carbon Group Contains: 1 non-metal, 2 metalloids, and 2 metals Valence Electrons: 4 Reactivity: Varies Solid at room temperature Group 15: Nitrogen Group Contains: 2 non-metals, 2 metalloids, and 1 metal Valence electrons: 5 Reactivity: Varies All but N are solid at room temperature
5 Group 16: Oxygen Group Contains: 3 non-metals, 2 metalloids Valence Electrons: 6 Reactivity: Reactive All but O are solid at room temperature. Groups 17: Halogens Contain: Nonmetals Valence Electrons: 7 Reactivity: Very reactive Other shared properties Poor conductors of electric current React violently with alkali metals to form salts Never found uncombined in nature Group 18 Noble Gases Contains: Nonmetals Valence Electrons: 8 (2 for He) Reactivity: Nonreactive (least reactive group) Colorless, odorless gases at room temperature Outermost energy level full All found in atmosphere Hydrogen Stands Apart H is set apart because its properties do not match any single group. Valence electrons: 1 Reactivity: very, but loses the 1 electron easily Similar to those of non-metals rather than metals Periods Periods run horizontally across the Periodic Table Periods are numbered 1 7 All the elements in a period will have the same number of energy levels, which contain electrons. Examples: Period 1 atoms have 1 energy level. Period 2 atoms have 2 energy levels. Period 5 atoms have 5 energy levels.
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