Periodic Table and Electron Configurations Honors Chemistry Unit 3

Modern Periodic Table Elements are arranged by increasing atomic number. Elements are arranged by increasing atomic number. –Recall that atomic number gives the number of protons in the nucleus of an atom.

The Periodic Law says: When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. Horizontal rows = periods Horizontal rows = periods –There are 7 periods –Each row (or period) is the energy level Vertical column = group (or family) Vertical column = group (or family) –Similar physical & chemical properties –Identified by number (1 - 18)

Periods

Groups/Families

Areas of the periodic table Three classes of elements are: 1. Metals 2. Nonmetals 3. Metalloids Notice the heavy, stair-step line? This is the dividing line between the Metals and Non-Metals This is the dividing line between the Metals and Non-Metals

Properties of Metals Properties of Metals On the Left side of the table On the Left side of the table Does not include hydrogen Does not include hydrogen Solids at room temperature (except for Mercury) Solids at room temperature (except for Mercury) Shiny Shiny Ductile: can be made into wires Ductile: can be made into wires Malleable: can be pounded & easily shaped, like knives and swords Malleable: can be pounded & easily shaped, like knives and swords Most are silver/grey in color Most are silver/grey in color Conducts heat and electricity Conducts heat and electricity Will lose electrons to form (+) ions (cations) Will lose electrons to form (+) ions (cations)

Properties of Non-metals On the right side of the periodic table On the right side of the periodic table Most are gases (H, He, Ne, etc.) Most are gases (H, He, Ne, etc.) Brittle, or break easily Brittle, or break easily Dull texture Dull texture Poor conductors of heat and electricity Poor conductors of heat and electricity Will Gain electrons to become negative ions (anions) Will Gain electrons to become negative ions (anions) Come in a variety of colors Come in a variety of colors

Properties of Metalloids Properties are intermediate between metals and nonmetals Properties are intermediate between metals and nonmetals Also called semi-metals Also called semi-metals They are on the stair step line in between the metals and non-metals They are on the stair step line in between the metals and non-metals They have a combination of both metallic and non- metallic properties They have a combination of both metallic and non- metallic properties –Ex: they are shiny but don’t conduct electricity Semiconductors – conduct electricity under certain circumstances (some used in computer technology) Semiconductors – conduct electricity under certain circumstances (some used in computer technology)

Metals Metals Nonmetals Nonmetals Metalloids Metalloids Metallic Character Metallic Character

Main Group Elements – groups 1, 2 &13-18 Main Group Elements – groups 1, 2 &13-18 Transition Metals – groups 3-12 Transition Metals – groups 3-12 Inner Transition Metals Inner Transition MetalsBlocks

Sublevel Blocks

Each row (or period) is the energy level for s and p orbitals. Each row (or period) is the energy level for s and p orbitals Period Number

Group 1 metals all end in s 1 Group 1 metals all end in s 1 Group 2 metals all end in s 2 Group 2 metals all end in s 2 –really should include He, but it fits better in a different spot, since He has the properties of the noble gases, and has a full outer level of electrons. s2s2 s1s1 Elements in the s - blocks He 1s 1 2s 2 7s 1 7s 2

The P-block – groups p1p1 p2p2 p3p3 p4p4 p5p5 p6p6 2p 1 3p 1 2p 6 6p 1 6p 6

Transition Metals - d block d1d1 d2d2 d3d3 d4d4 d5d5 d6d6 d7d7 d8d8 d9d9 d 10 Groups d 1 4d 1 5d 1 3d 10

F - block Called the “inner transition elements” Called the “inner transition elements” 4f 1 5f 1

f orbitals start filling at 4f, and are 2 less than the period number f orbitals start filling at 4f, and are 2 less than the period number f 5f

The “f” Block

The “d” orbitals fill up in levels 1 less than the period number, so the first d is 3d even though it’s in row 4. The “d” orbitals fill up in levels 1 less than the period number, so the first d is 3d even though it’s in row d 4d 5d

Writing Electron Configuration from the Periodic Table The way an electron configuration ends will tell you what element you have. The way an electron configuration ends will tell you what element you have.Examples: 1. 3d s p 2 Mn Rb Ge

Chemistry Crash Course video - Periodic Table Chemistry Crash Course video - Periodic Table Chemistry Crash Course video - Periodic Table Chemistry Crash Course video - Periodic Table