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A/B RxN
A) When acid and base react with each other, the cation of the base and anion of the acid will combines and form salt.
B) HA + B >>> BH(+) + A
C) H3O(+) + OH(-) >>> 2H2O

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Lab Reaction
A) NaH + Cl2
B) The amount of HCl in each trials
C) If we increased the concentration of HCl, then more precipitation will form

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1) Does increasing the amount of the acid or base affect how they react with the can?
2) Why does the can with a scratch have a faster and more effective reaction?
3) Do some other factors such as temperature or pressure affect how intense the acid or base in general?
4) Why is it that the base react better with the cola can and the acid doesn't seems to have as great result of the bubbles as the base?
5) If we change the size of the can, will the reaction be faster or stronger?

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Equilibrium Experiment
a) Apparently, the change in volume of the plastic container did’t appears that much, and it mostly because of the cups that we use for the experiment have the exact same volume. So at the end we end up having a nearly same amount of water in both container
b) As the experiment goes on, it seems that the player who got a bigger cups slowly overcome the player with the small one, and at the end we can clearly see that the player who get the bigger cups eventually won because they can fill up their opponent’s plastic container faster due to the large volume of their cup.
c) Surprisingly,  for the entire experiment both container seems to be at constants volume. Even if the player got a different cups size it still appears that the amount of water that both players attempts to fill their opponent are done equally every single round. Each size of the cups has their advantage and disadvantage, so at the end they both end up as the same volume before we run the experiment.
d) The dynamic equilibrium will occurs once a reversible reaction is exist, and it is a process where substances transition between the reactants and products at equal rates, meaning there is no net change.

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Food energy ( high to low )
The energy from experiment
- Lay ( 324.87 Cal/g )
- Popcorn ( 372.56 Cal/g )
- Corn Puff ( 278.46 Cal/g )
The Actual Energy
- Lay ( 340 Cal/g )
- Corn Puff ( 190 Cal/g )
- Popcorn ( 120 Cal/g )

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Energy
Where is energy stored in a molecule?
- The energy stored in a covalent bond that occurs in the reaction.
What can you change about your graph to make it more accurate?
- Add in some more details such as explanation and the number of substance, reactants and product.

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Sucrose dehydration
A.) After mixing sucrose with sulfuric acid then  the reaction will occurs. The sulfuric acid will removes water from the sugar in exothermic reaction, and that mean the reaction will release the heat. After the reaction is done, we can see that the products of this reaction are the separate of the chemical elements of sucrose, which is the pure carbon, water and the solid carbonaceous.
B.) C12H22O11 >>> 12 C + 11 H2O
C.) Questions
- Why is adding a little amount of water help the reaction to occurs faster?
- Why is it an exothermic reaction?
- Can we add something more for the reactants to make the reaction last longer?
- Is sulfuric acid considered as a reactant or catalyst?
- Why does the color of the reactants change so much during the reaction?

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Activation Energy Graph

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Question for the Experiment
-  Does changing the amount of catalyst change how affective it is toward the reaction rate?

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KMT & Collision Theory
A) Collision theory states that the rate of a chemical reaction depend on the number of collisions between reactant molecules. So the more often reactant molecules collide, the  faster the reaction rate will be
B) Spontaneous is the process or events that occur naturally without any external cause. The relationship between spontaneous and chemical reactions is that there are processes of chemical reactions that occurs without input of matter or electrical energy into the system, which is called spontaneous process.

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Elephant toothpaste
A)*The picture*
B) Decomposition
C) The foam bubble is the result from the hydrogen peroxide getting decompose by sodium iodide, potassium iodide and yeast that were used as a catalyst
D) Sodium iodide, Potassium iodide and Yeast

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Lab Variables
Independent variables
- The amount of vinegar
- The amount of baking soda
- Amount of vinegar added per time
- Amount of baking soda added per time
Dependent variables
- The bubble
- The gas

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Chemical Reaction Experiment
The differences between reactant and product
- The product contain 4 atoms
- The reactant contain 2 atoms
- The temperature inside the bag
- The mass of substances
- The air in plastic bag
The similarity between reactant and product
- Both contain calcium
- Both contain sodium

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A) Baking Soda - 10 g
Calcium Chloride - 20 g
Temperature - 26 degree Celsius
Water - 20 mL
B) *The Picture*
C) Baking Soda and Calcium Chloride is both ionic compound so they aren't going to react until we add water because after water dissolve both of them, the positive and negative ions are going to be separate and then will attach with the water's ions instead. Then the chemical reaction will start to work by making both of the compound that are currently mixing together form a bubble and start to fill up the plastic bag. After the experiment, the temperature changed from 26°c to 22°c and the mass decrease from 68.9g to 66.7g

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3 Videos
1. Gay-Lussac's Law
https://www.youtube.com/watch?v=N6DZRiSIK3s
2. Charles's Law
https://www.youtube.com/watch?v=NplVuTrr59U
3. Boyle's Law
https://www.youtube.com/watch?v=eR49g3ubTBg

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Questions

1. Why do the amount of the water increase?
2. Why does the temperature cooling down?
3. How did the red water goes up into the glass?
4. What kind of reaction make the process work?
5. Why did the gas suddenly disappear?
6. Does the interaction relate to the intermolecular force?
7. How did the glass lose their heat?
8. How does the interaction work without chemical substances?
9. If we change water into another liquid will this process work?
10. What type of gas law is this?

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Intermolecular Forces

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Play Game

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Planning for Project

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Lab
- Boiling point
- Melting point
- Intermolecular Forces

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Review
- Intermolecular Forces

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Intermolecular Forces
- Work sheet
- Do some reflection

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Hydrogen Bonding
- Learn about Dipole
- Hydrogen

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Intermolecular Forces
- Dipole-Dipole
- Slide and Doc

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Arrangement & Movement & Force
- States of Matter
- Forces between Particles
- Properties and Forces
- A model of Solid Liquid Gas

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Polar Molecules
- Molecule Polarity
- Polar Molecules
- Atom Investigation

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Lewis Structure
- Unpaired electron
- Lone pairs
- Bonds in each atom

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Lewis Structure
- Practice drawing

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Lewis Structures
* insert the drawing* (later)

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Covalent Bonding
- Forms between two non-metal
- Lower energy = More stable
- Single bond = 2 shared electrons
- Double bond = 4 shared electrons

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Ionic Compounds
- Quiz 1.2

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Ionic compound
- Learn the two types of elements
- Learn how to balance an electron

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Ionic Compound
- Naming the chemical compounds
- Observe the valence electron
- Matching two elements together

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Ionic Compound
- Draw dot diagram
- Metal and Non-metal elements
- The positive and negative sign

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Ionic & Molecular Compounds
- Learn about Chemical bond
- Neutral Atom
- Bohr Ions
- Types of Bonds

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Exam
- Unit 1.1 Test
- The periodic Trends

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Exam
- Unit 1.1 Test
- The periodic Trends

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Final Report
- Do the Graph
- Making data table
- Response the Hypothesis
- Do observation paragraph

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Lab Report
- Compare Data with group
- Working on Final Report

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Lab Report
- Do the Experiment
- Discuss with group
- Collecting Data

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Lab Report Planning
- Description of Experiment
- Diagram of Experiment
- Prepare for Al+NaOH Experiment

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Periodic table Trend
- Ionization Energy
- Electronegativity
- Atomic Radius
- Melting Point

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Reviewing the Quiz
- Discuss the correct answers
- Prepare for lab experiment

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Quiz
- We have a quiz about the size of particles
- The interaction of protons and electrons
- How does the interaction effect the size

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Periodic table
- Atomic radius
- Positive and Negative of proton
- Observe the electrons in element
- Define and compare the size of elements

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Periodic table
- Learn about the Atomic Radius
- Learn about Electronegative
- And the process of Ionization of how it's  steal the electron

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Observe the periodic table
- The principle quantum number
- The valence electron

- The periodic table with the element's group labelled