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Started with a chemistry primer to see the knowledge we had of chemistry before any teaching.

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Introduced the multiple activities that would be assigned through out the semester and syllabus. Examples: Mastering Chemistry, recitations, exams, quiz, etc.

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Learned how to identify number of significant figures based on the information given. Started to use conversion factors to convert units. Example: Kj=1000 joules.

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Learned how to classify matter by state and composition. Example: homogenous mixture, heterogeneous mixture. Learned to distinguish matter from extensive/intensive, physical, or chemical. Learned how to identify atomic mass/number. Converting mass to moles and vice-versa. Converting between mass and particles and vice-versa

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Laws of conservation of mass and multiple/definite proportions. Scientific Theories.

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Laws of conservation of mass and multiple/definite proportions. Scientific Theories.

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Matter is not created or destroyed. Dalton's theory: Each element is composed of tiny, indestructible particles
called atoms.(Just one of the many concepts)

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Example of proper ration of proportions: 16g of Oxygen/2g of Hydrogen=8.0 or 8:1 ratio.

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Matter must not be as uniform as it appears. It must contain large regions of empty space dotted with small regions of very dense matter. The structure of an atom is not completely full of some matter, it has empty spaces and different components. Example: Nucleus, protons, electrons.

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Example of identifying atomic mass/number: Neon.

Atomic mass of 20 and atomic number 10.

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Learned how to calculate wavelength, frequency, and energy of a photon.

Learned the Balmer-Rydberg equation, to calculate the wavelength, frequency, and/or energy of a photon absorbed or released for an electron transition in the hydrogen atom.

Learned to describe and identify each of the s, p, and d groups.

Learned how to assign quantum numbers to each other and to their corresponding orbital. Assign quantum numbers for an electron in an atom.

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Identifying core and valence electrons, f block (transition metals) is introduced. Electro configurations: Alkali metals, Alkaline metals, metalloids, Halogens, etc.

(Zeff) use of effective nuclear charge.

The larger the effective nuclear charge an electron
experiences, the stronger the attraction it will have
for the nucleus.

Atoms in the same group increase in size down the
column.

Ionization of energy.

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Decrease as we move down a column in the Periodic table. Increases moving from left to right. Greater effective nuclear charge.

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For an overall view of Elemental periodic properties 

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For an overall view of Elemental periodic properties 

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Table 3.2 "Summary of Periodic Properties" page 92, Chapter 3 PPT presentation.

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Identifying covalent and Ionic bonds.

Writing empirical formulas.

Lewis model.

Octet rule. And outcasts: H, Li, Be, and B [Make octet rule more complicated 😊 ]

Naming compounds.

Polyatomic Ions.

Hydrates and their prefixes.

Bonding and lone pair electrons. Double bonds. Triple Bonds.

Learned to convert mass to molecules.

Combustion analysis.

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Metal & Non-Metal= Ionic

Non-Metal & Non-Metal= Covalent

When a metal interacts with a nonmetal, it can transfer
one or more of its electrons to the nonmetal.
– The metal atom then becomes a cation.
– The nonmetal atom becomes an anion.

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Chapter 4 PPT slides Table 4.4 "Some Common Polyatomic Ions" page 49.

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[(molecular mass of element)/(mass of 1 mol of compound)] x100

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Classified bonds as nonpolar (pure) covalent, polar covalent, or ionic using either a periodic table or electronegativity values

Drew Lewis Diagrams for molecules and polyatomic ions.

Learned VSEPR (Valence Shell Electron Pair
Repulsion) to determine the electron-pair and molecular geometries as well as basic bond angles for an atom in any molecule.

Used bond polarity and molecular shape to determine polarity of molecule

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Illustrations of Molecular Geometries of Molecules Using 3-D Notations

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Illustrations of Molecular Geometries of Molecules Using 3-D Notations

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Image showing name and geometry of molecules in Chapter 5 PPT slides page 68.

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Used Valence Bond Theory (VB) to predict hybridization of atoms in a molecule.

Learned how to identify and determine the number of sigma and pi bonds in a molecule.

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Table of Hybridization Scheme from
Electron Geometry

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Table of Hybridization Scheme from
Electron Geometry

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Useful infographic on chapter 6 PPT slides page 30.

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Theres a lecture video and practice problem in "Sections 6.1-6.3" for better understanding of how to use VSEPR to also find pi and sigma bonds.

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Learned about chemical change or reactions.

Types of reactions.

Writing and balancing chemical equations to represent the change.

LOTS OF STOICHIOMETRY PROBLEMS.

Finding limiting and excess reactant.

Finding theoretical and percent yield.

Oxidation numbers.

OH.... DID I MENTION STOICHIOMETRY PROBLEMS??? JUST IN CASE YOU FORGOT!

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Use the "Stoichiometry and Problem Solving Notes" document to get an overview and refresher of the types of reactions there is. As well as how to work an stoichiometry problem. Reading the solution and dilution part won't hurt anybody👍.

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Learned reactions in solution, solution concentration, and making and diluting solutions.

Solubility of ionic compounds.

The difference between ionic and net ionic equations.

Oxidation numbers

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Helpful information about acids and bases in Chapter 8 PPT slides page 68.

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GOOD EXAMPLE OF Writing Acid–Base
Reactions

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GOOD EXAMPLE OF Writing Acid–Base
Reactions

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In page 81 of the Chapter 8 PPT slides there's a good example of how to write the acid-base reactions with the complete ionic and net ionic equation. (May be useful for better comprehension).

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Thermodynamic system.

The first law of thermodynamics.

Heat, calorimetry, enthalpy of reaction, Hess's law, and bond energies.

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BEST WAY TO LEARN THERMODYNAMICS= SOLVE PROBLEMS AND WATCH THE SECTION VIDEOS

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BEST WAY TO LEARN THERMODYNAMICS= SOLVE PROBLEMS AND WATCH THE SECTION VIDEOS

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Watch the videos and then try the practice problems to test the your personal understanding of the material covered of thermodynamics.

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WHY WATCH THE VIDEOS AND NOT JUST READ THE PPT?

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WHY WATCH THE VIDEOS AND NOT JUST READ THE PPT?

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The powerpoint slide is not very clear organizing the information on the thermodynamics problems. And so watching the lecture videos posted by the professor might be more efficient to understand unit 9.

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Learned the properties of gasses.

Gas laws.

Kinetic Molecular Theory.

Behavior of gasses.

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In Chapter 10 PPT slides page 9 there's a table that provides information on what some units are equal to.

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P= pressure

V= Volume

T= Temperature

n= Amount of moles

R= ideal gas law constant [0.0821 (L x atm)/(mol x K)]

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Really good formula to use to find whatever unknown value needed. Flexible, just have to adjust the unknown on one side and the knowns on the other and solve.

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USE VIDEOS AND PRACTICE PROBLEMS POSTED IN CHAPTER 10 UNIT 

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USE VIDEOS AND PRACTICE PROBLEMS POSTED IN CHAPTER 10 UNIT 

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Getting the terms down is important but knowing how to apply them is also vital. Use the videos and practice problems to test your knowledge and information processing.