In this unit, students are introduced to the idea that the electrons surrounding the nucleus can either be gained, lost or shared to form ionic/ metallic or covalent bonds. Students will learn how to use the electronegativity values to predict whether two atoms will form an ionic or a covalent bond.

By the end of this unit, Students will be able to:

• • Distinguish between the locations of metal atoms versus non-metal atoms on the periodic table.

  • Use electronegativity values to predict whether an ionic or covalent bond is most likely to form.

  • Identify compounds as ionic, covalent, or metallic based on their chemical formula.

  • Predict the number of atoms needed in a molecular formula.

  • Examine ratios of atoms in compounds.

  • List some properties of ionic, covalent, and metallic bonds.

  • Compare and contrast the basic structure of ionic and molecular compounds.

  • Determine the number of valence electrons for an atom.

  • Create a Lewis dot structure for an atom, covalent compound, and ionic compound.

  • Predict the charge of an ion.

  • Predict the molecular shape of a covalent molecule based upon its Lewis dot structure.

  • Explain why stable, neutral ionic compounds are formed from cations and anions.

  • Explain why different quantities of ions combine to make different compounds.

  • Explain the purposes of superscripts and subscripts in chemical formulas.

  • Name and write the formulas for binary and ternary ionic compounds.

Time: 16 Hours

Assessments:

Naming Chemical Compounds Assign.

Blog Based Assignment

Unit 3 Cumulative Assignment