We think you have liked this presentation. If you wish to download it, please recommend it to your friends in any social system. Share buttons are a little bit lower. Thank you!
Presentation is loading. Please wait.
Published byLora Bond
Modified over 3 years ago
The Periodic Table Chapter 5 Notes
Mendeleev ● Designed first periodic table (1869) ● Arranged mostly by increasing atomic mass ● Elements in the same column have similar properties
Moseley ● Arranged by increasing atomic number
Periodic Law ● Elements’ physical and chemical properties show a periodic [“repeating”] pattern when arranged by atomic number
● COLUMN = Group or Family o Similar properties based on the same number of valence electrons o Numbered 1-18 or with Roman numerals ● ROW = Period
Valence electrons ● Electrons in the outermost shell ● Octet Rule = all atoms want 8 valence electrons to achieve stability o Exceptions: H, He
Families of the Periodic Table
Alkali Metals ● Soft ● Most reactive metals
Noble Gases ● very UNreactive ● “inert”
Halogens ● Most reactive nonmetals
Metals ● luster/shiny, good conductors of heat & electricity, malleable, ductile ● LEFT SIDE of periodic table
Nonmetals ● not shiny, poor conductors, not malleable or ductile, brittle ● RIGHT SIDE of periodic table
Metalloids ● “semi-metals” ● some properties of metals, some of nonmetals ● touch ZIG-ZAG LINE
Atomic Radius ● Distance from the nucleus to the outer electrons ● Decreases across a row ● Increases down a column
Explanation of Atomic Radius increasing down a column
Explanation of Atomic Radius decreasing across a row
Electronegativity ● Ability of an atom to attract electrons to itself o Increases across a row o Decreases down a column
Ionization Energy ● Energy needed to remove an electron ● Increases across a row ● Decreases down a column
Electron Affinity ● How much an atom wants to gain an electron o Decreases down a column o Increases across a row
Think about Corners
Practice- Circle your answer choice Larger atomic radius? 1) Mg or Sr 2) Mg or S Larger electronegativity? 3) P or Sb 4) Ge or Br Larger ionization energy? 5) Ca or Se 6) Ca or Ra
Ion Size ● Cation – atom loses electron o Atom gets smaller ● Anion – atom gains electron o Atom gets bigger
Exampl e of Ion Size
Anatomy of the Periodic Table
Periodic Table. Atom Neutral atom has equal number of protons and electrons + charges = - charges Overall charge of zero (neutral)
TMI the periodic table is telling you more than you want to know.
Periodic Table and Trends
CHAPTER 6 NOTES: The Periodic Table
The Periodic Table.
Chapter 6 Periodic Table and Periodic Law. The Periodic Table got its name because of the repeating pattern of chemical & physical properties. Mendeleev.
Russian Chemist Dmitri Mendeleev produced the first periodic table of elements He arranged them in order of increasing atomic mass and noticed a periodic.
Periodic Table & Trends
Chapter 6 The Periodic Table and Periodic Law The elements, which make up all living and non-living matter, fit into a orderly table. When interpreted.
Properties of Elements and Trends
Periodic Table Chapter 4.
Periodic Table Chapter 6.
Chapter 4 The Periodic Table.
Chapter 6 Periodic Trends
Organization of the Periodic Table. Demetry Mendeleev organized the elements in the first periodic table by order of mass in Found repetition in.
History of the Periodic Table Dimitri Mendeleev published a periodic table that arranged elements by increasing atomic mass Dimitri Mendeleev published.
Unit 6 – The Periodic Table
Organization of the Periodic Table. Columns of the periodic table Atoms of elements in the same group have the same # of valence electrons and therefore.
© 2019 SlidePlayer.com Inc. All rights reserved.