The Periodic Guide: Study Guide
Lesson 03.01: History of the Periodic Table
Explain how scientific observations led to the development of, and changes to, the periodic table.
-Dmitri Mendeleev- first periodic table, organized 63 known elements according to properties, organized into rows and columns and wrote name, mass, and chemical properties on each
-Julius Lothar Meyer- independently worked in Germany, similar to Mendeleev
-Henry Gwyn Jeffreys Moseley- Worked with Ernest Rutherford, experimented with 38 metals, he found that the positive charge of each element’s nucleus increased by one from element to element as they were arranged in Mendeleev’s periodic table, lead to modern definition of atomic number (# of protons in atom’s nucleus) and the recognition the atomic number was basis for organization of periodic table.
Describe the organization of the modern periodic table.
Arranged from left to right in rows (periods) by increasing atomic number and top to bottom in columns (groups) based on similar chemical properties
Lesson 03.02: Group Names and Properties
Compare and contrast the properties of metals, metalloids, and nonmetals.
-Metals- good conductors of heat and electricity and reflect light and heat, most luster (shine) and most are malleable (hammered or rolled into sheets)
-Non-metals- poor conductors of heat and electricity, most are gas at room temperature, those that are solid are not malleable
-Metalloids- a semiconductor (conduct electricity better than non-metals but not as good as metals), some characteristics of metals but more like nonmetals Identify groups and sections of the periodic table by group name and common properties.
3.02 notes
Lesson 03.03: Periodic Trends
Describe and explain the trends for effective nuclear charge, atomic radius, ionic radius, and ionization energy across a period and down a group.
-Effective Nuclear Charge- the charge (from the nucleus) felt by the valence electrons after you have taken into account the number of
Explain how scientific observations led to the development of, and changes to, the periodic table.
-Dmitri Mendeleev- first periodic table, organized 63 known elements according to properties, organized into rows and columns and wrote name, mass, and chemical properties on each
-Julius Lothar Meyer- independently worked in Germany, similar to Mendeleev
-Henry Gwyn Jeffreys Moseley- Worked with Ernest Rutherford, experimented with 38 metals, he found that the positive charge of each element’s nucleus increased by one from element to element as they were arranged in Mendeleev’s periodic table, lead to modern definition of atomic number (# of protons in atom’s nucleus) and the recognition the atomic number was basis for organization of periodic table.
Describe the organization of the modern periodic table.
Arranged from left to right in rows (periods) by increasing atomic number and top to bottom in columns (groups) based on similar chemical properties
Lesson 03.02: Group Names and Properties
Compare and contrast the properties of metals, metalloids, and nonmetals.
-Metals- good conductors of heat and electricity and reflect light and heat, most luster (shine) and most are malleable (hammered or rolled into sheets)
-Non-metals- poor conductors of heat and electricity, most are gas at room temperature, those that are solid are not malleable
-Metalloids- a semiconductor (conduct electricity better than non-metals but not as good as metals), some characteristics of metals but more like nonmetals Identify groups and sections of the periodic table by group name and common properties.
3.02 notes
Lesson 03.03: Periodic Trends
Describe and explain the trends for effective nuclear charge, atomic radius, ionic radius, and ionization energy across a period and down a group.
-Effective Nuclear Charge- the charge (from the nucleus) felt by the valence electrons after you have taken into account the number of