# The Periodic Guide: Study Guide Essay examples

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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
-Covalent bond- Electrons are shared between two atoms, neither atom completely gains or loses electrons. Between two nonmetals.

Relate your knowledge of the periodic trends to the chemical bonding exhibited by various elements.

Lesson 03.05: Ionic Bonding and Writing Formulas
Determine an element’s ionic charge based on its location on the periodic table.
Group 1- 1+
Group 2- 2+
Group 3- 3+
Group 4- 4+
Group 5- 3-
Group 6- 2-
Group 7- 1-
Group 8- non-reactive noble gases
Write the correct ionic formula when given two elements that bond ionically.
Use question above and periodic table

Lesson 03.06: Covalent Bonding and Lewis Structures
Determine how many covalent bonds an atom needs in order to fill its valence shell, using the periodic table.
Must get to 8 valance electrons.
Ex. Group 17 needs one more valance electron; group 6 needs 2 more valance electrons

Draw correct Lewis structures to model covalently bonded molecules when given the name or formula of the molecule.

Describe your observations and conclusions from the virtual lab.

Lesson 03.07: Intermolecular Forces
Use VSEPR theory to predict the shape of a molecule based on its Lewis structure.
The VSEPR theory is about geometry of compounds and electron location.

Compare and contrast intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding, and ion-dipole). London dispersion forces occur between all molecules and particles but are the only