By the end of the unit, the students will be able to:

1 - Explain how atoms combine to form compounds through metallic, ionic, and covalent bonding. (4.1)

2 - Predict chemical formulas based on the number of valence electrons. (4.1)

3 - Define:  sea of electrons, alloy

4 - Use the term "sea of electrons" to explain why metals are good conductors of heat and electricity, are shiny, and are malleable and ductile.

5 - Use electronegativity to explain the difference among ionic, polar and nonpolar covalent bonds. (4.3)

6 - Determine the charges for metallic and nonmetallic ions within ionic compounds, based on the number of valence electrons.

7 - Draw Lewis dot diagrams for ionic and covalent compounds. (4.2)

8 - Use valence-shell electron-pair repulsion theory (VSEPR) to predict the molecular geometry (linear, bent, triangular planar, triangular pyramidal, and tetrahedral) of simple molecules (4.4)

9 - Identify how hydrogen bonding in water affects a variety of physical, chemical, and biological phenomena (e.g. surface tension, capillary action, density, boiling point). (4.5)