Understanding Electron Configuration and the Periodic Table Structure
This resource provides an in-depth look at electron configurations according to the periodic table. It explains how elements are organized into groups and periods based on their electron configuration, highlighting the properties of s-block, d-block, and p-block elements. It emphasizes the reactivity trends among groups, including alkali and alkaline earth metals, as well as transition metals and nonmetals. Practice problems are included to reinforce knowledge of element classification by their group, period, and block, enhancing comprehension of chemical behavior.
Understanding Electron Configuration and the Periodic Table Structure
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Presentation Transcript
Honors Chemistry Section 5.2 Electron Configuration and the Periodic Table
Periodic Table • Arranged in groups and periods • Groups – similar chemical properties • Period – length determined by # of electrons added to the shell.
S - block • Chemically reactive metals • Group 1 more reactive than Group 2 • Group 1 – alkali metals • Configuration ns1 • Soft • Silvery • So reactive don’t exist in nature as elements • React vigorously with nonmetals • React strongly with water • As you go down the group Tmelt decreases • H not an alkali metal
S – block (cont.) • Group 2 – alkaline earth metals • Configuration ns2 • Harder, denser and stronger than alkali metals • Higher melting point than alkali metals • Less reactive than alkali metals – but still not found in nature as elements • He has an alkaline earth configuration but is a noble gas
Practice • Give the group, period and block of the element with the configuration [Rn] 7s1 • Give the group, period and block of the element with the configuration [He] 2s2 • How does the reactivity of [He] 2s2 compare with [He] 2s1?
D-block • Fills Groups 3 to 12 • Starts filling in the 4th Period (3d) • Configuration ns2 (n-1)dx • Examples • Group 3 - ns2 (n-1)d1 • Group 12 - ns2 (n-1)d10 • D – block are metals • Called Transition Metals or Transition Elements • Good conductors of heat and electricity • Have high luster • Less reactive than alkali or alkaline earth elements • Some don’t easily form compounds (Pd, Pt, Au)
Practice • What is the period, block and group of the element with the configuration [Ar] 3d10 4s1? • What is this element? • What other elements are in the same group?
P - Block • Groups 13 to 18 (Except He) • S – block + P – Block = Main Group Elements • # valence electrons = Group # - 10 • Contains all metalloids • Group 17 – Halogens – most reactive nonmetals • Halogens react with metals to form salts
P – Block (cont.) • Metals – harder and denser than s – block metals but softer and less dense than d – block. • Most p – block metals are not found as elements in nature. • Metalloids – brittle solids/intermediate conductivity
Practice • What is the outer configuration for Group 16, Period 3? What is the name of the element? Is it a metal/nonmetal/metalloid? • What is the period block and group of the element [Kr] 4d10 5s2 5p3? What is the name of the element? Is it a metal/nonmetal/metalloid?
F - Block • Between Groups 3 and 4 • In the 6th and 7th Periods • 4f and 5f are being filled • Lanthanides • Shiny • Metals • Reactivity similar to alkaline earth metals • Actinides • Radioactive • All but first 4 - synthetic
Practice • For each of the following determine block, period, and group. What is the name of the element and determine if the reactivity is high or low. • [He] 2s2 2p3 • [Xe] 4f14 5d10 6s1 • [Rn] 7s1 • [Ar] 3d10 4s2 4p5
