The object of reflection for this journal is your experience in learning the mat

The object of reflection for this journal is your experience in learning the material during the week. You are required to make one entry per week, each about 250 – 300 words of length. You are advised to make entries regularly rather than completing it right before a submission date, and the quality of reflection should be the emphasis of your entries rather than over-emphasis on the word count.
Chapter 6 Overview and Learning Objectives
OVERVIEW
Lewis structures are representations of molecules (and ions) that shows the bonds between atoms in molecules and non-bonded or lone pair electrons. Only valence or outer-shell electrons are used to draw Lewis structures. The principle is that electrons are shared between atoms so that each has a full outer shell (usually an octet but a duet in the case of hydrogen). Bonds can be single bonds (one pair of electrons shared), double bonds (two pairs shared), or triple bonds (three pairs shared). Electronegativity is a periodic property (increasing as you go left to right and decreasing as you from top to bottom on the Periodic Table) that describes the attraction for the electrons in chemical bonds by one atom or the other. The unequal sharing of electrons results in polar covalent bonds where one atom in the bond has a partial negative charge and the other atom in the bond has a partial positive bond. Exceptions to the octet rule are compounds involving boron and beryllium, species with an odd number of electrons (radicals), and expanded octet (with 10 or 12 electrons around a central atom) for elements in Period 3 and higher. Formal charge is a formalism used to help assess the correctness of a Lewis structure.
Chapter 7 Overview and Learning Objectives
OVERVIEW
Molecules are three-dimensional–they have a shape–and many of the properties of compounds are determined by this three dimensional shape. The shapes of molecules are determined by the steric repulsion of electron groups (lone pairs and chemical bonds) around a central atom. Five main categories result: linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral. If some of the electron groups attached are lone pairs of electrons, there are additional groups–bent, trigonal pyramidal, see-saw, T-shaped, linear, square pyramidal, and square planar. If these shapes are asymmetrical and have polar bonds in the molecule, the whole molecule can be polar. Intermolecular forces are attractions between molecules that come about because of polar bonds and molecules. In this chapter we also discuss orbital hybridization, which seeks to connect the idea of molecular shape with the previous discussion of atomic orbitals.
Write an academic reflection in four paragraphs: describe, interpret, evaluate, and plan.
What did you learn this week?
What activities helped you to learn?
What activities did you find engaging?
How will you do to better understand your muddy points for the week?