Chemistry 30
CH30-MS1
Examine the role of valence electrons in the formation of chemical bonds.
SI
Indicators for this outcome
| (a) | Trace the historical development of the model of the atom from Bohr to the modern quantum understanding, including the contributions of Einstein, Planck, Heisenberg and DeBroglie. (STSE, K) |
| (b) | Discuss the value of representing scientific understanding of the atom using various types of models, including molecular formula, structural formula, space-filling molecular model, ball-and-stick molecular model and Lewis structure. (STSE, A) |
| (c) | Examine how evidence and experimentation inform the development and refinement of theories in chemistry. (STSE) |
| (d) | Explain the relationship between the position of an element on the periodic table and its number of valence electrons with reference to the octet rule. (K) |
| (e) | Explain the formation of ions and predict their charge in group 1 and 2 elements and non-metals, based on an understanding of valence electrons and the octet rule. (K, S) |
| (f) | Draw Lewis structures (electron dot structures) for group 1 and 2 elements and non-metals, and their ions, based on an understanding of valence electrons. (STSE, S) |
| (g) | Discuss the role of valence electrons in the formation of covalent and ionic bonds, including the connection to metals and non-metals. (K) |
| (h) | Predict the arrangement of atoms and draw Lewis structures (electron dot structures) to represent covalent- and ionic-bonded molecules. (S) |
| (i) | Predict the geometry and draw the shapes of molecules with a single central atom using valence shell electron pair repulsion (VSEPR) theory. (K, S) |
| (j) | Predict the nature of chemical bonds within a molecule using the property of electronegativity. (K, S) |
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