Chemistry Study Guide Module 3

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.

Lesson 03.03
Predict the properties of an element based on the patterns of the periodic table.

Lesson 3.04
Define ionic and covalent bonding.
Ionic Bond: A chemical bond that results from electrostatic attraction between positive and negative ions.
Covalent Bond: A chemical bond in which electrons are shared between two atoms.
Relate knowledge of the periodic trends to chemical bonding.