Below is a description of how to download you iBook to your iPad. It will take some time to download, so please do not begin the download until you are in a place where you can be connected to wifi and a power source for up to an hour.
The book will be a valuable resource for you to refer to as well as for us to use in class.
Biology:
Open your iBooks App
Click ‘Store’ in the top left
When the store opens, click the tab at the top that says ‘More’
Scroll through that drop-down menu and find textbooks
When that page opens, scroll down until you see ‘Life Sciences’
The textbook we will use is called “Biology” and is $14.99
Chemistry:
Open your iBooks App
Click ‘Store’ in the top left
When the store opens, click the tab at the top that says ‘More’
Scroll through that drop-down menu and find textbooks
When that page opens, scroll down until you see ‘Physical Sciences’
The textbook we will use is called “Chemistry” and is $14.99
Welcome to Mr. Kubuske’s Class Blog. First, please set a bookmark or a link to your home screen. After that feel free to browse this page. At the top are links to class pages where notes, assignments, and documents will be posted for you to download as we work through our curriculum. There’s a page for students, a page about Mr. K, and a soon to come weekly agenda page. On the right is links to my twitter and other info that will help you.
Next, there are 3 papers on the back lab table I’d like you to pick up. You will need to bring these papers back to class tomorrow so put them in a safe place. Eventually, these papers will need to go in your Class 3-ring binder.
Last, for today’s class activity, you’ll need to get a piece of string. The strings are on the old pencil sharpener near the bookcase. Please go ahead and pick up a piece of string and come back to your seat. At that point please put all your papers and other materials away and wait for further instructions.
As a reminder, you will need to download your iBook at home or in a place where you can be on a wifi network for a long period of time.
Thanks for participating and we look forward to working with you this year!
Today we’re going to begin studying Gas Laws… (and that doesn’t mean the rules on Dutch Oven or letting one go in a crowded elevator).
We’re going to try some new classroom techniques for this final unit and create an “Open” classroom. Below are the expectations of you the student and of me the teacher.
Student Values:
You are encouraged to collaborate (share) ideas, information, and how to complete problems with fellow classmates. This means sharing information, not giving answers. The point of collaboration is to better understand the material ourselves and be of service to a colleague. The only thing you may not share are the puzzle pieces; they must be received individually and documented by the instructor.
If you are sharing a resource digitally on the blog or Google Doc you should use your first initial and last name to identify you. Posing as another student is considered fraudulent and does not follow the mission of the school. Any student posing as a colleague will face loss of points and other possible disciplinary actions.
You are tasked with completing 10 topics before you are permitted to attempt the final test. For each topic you complete, you will receive a piece of the puzzle that you are literally and figuratively completing during this unit. You may work at your own pace provided you meet the deadlines set by the teacher.
Since you will be permitted to use the internet and technology as you see fit, you may come across material that is inappropriate for a high school. When this occurs, close your iPad and raise your hand. Do not draw attention to yourself or share the text or images with others.
You are permitted to move about the room as needed to complete tasks and collaborate with colleagues. But in a working environment you must respect the workspace and work ethics of those colleagues by not becoming a distraction.
Failure to follow these values will result in a deduction of points from your Unit 10 score.
Be of service to my students by providing a framework digitally and within the classroom to allow for free flow of ideas and learning.
Provide guiding questions to show students direction they should look to complete their sections.
Be available for mentoring and guidance through challenging material.
As you complete each section you will be asked a set of questions to prove your knowledge of the subject. You must score a 100% to receive your piece of the puzzle then move on to the next section. You are permitted to attempt these questions as many times as needed to receive a score of 100%. You will only lose points by failing to follow the values listed above. You can receive extra consideration for extra points or returning lost points by helping fellow students or providing useful sources for fellow students.
Describe and site4 examples of how gases are different than solids and liquids at the molecular level.
Completeeach of these conversions: atm → mmHg // atm → kPa // atm → torr
2. Boyle’s Law
DescribeBoyle’s Law
Complete4 problems using Boyle’s law
Create an explanation of how you can remember the formula for Boyle’s Law.
3. Charles Law
DescribeCharles law
Complete 4 problems using Charles’ law
Create an explanation of how you can remember the difference between Boyle’s and Charles. OR
Watchthis video and explain how it proves Charles’ Law.
4. Gay-Lussac’s Law
DescribeGay-Lussac’s law
Before receiving completion for this section you should have: Postedat least 1 source of your information (that was not previously posted) , with your name to this Google Doc… OR… Posta question you have and/or Posta response to another students question.
5. Combined Gas Law
Complete 4 problems using the Combined Gas Law.
Write and submit an explanation of what the combined gas law is and why it is useful in the box below. You can see the text from other respondents by clicking this link. Combined Gas Law Responses
6. Standard Temperature & Pressure (STP)
Complete2 problems using the Combined Gas Law at STP.
Writea Definition of Standard Temperature & Pressure.
7. Universal Gas Constant (R)
Find ‘R’s value for :
L·Torr/mol·K (L·mmHg/mol·K)
liter·atm/mol·K
Determine what formula is ‘R’ used in.
8. Ideal Gas Law: Volume
Write out the formula of the Ideal Gas Law.
Complete4 problems finding the value of the Universal Gas constant using the Ideal Gas Law.
9. Ideal Gas Law: Moles
Determine how many liters are equal to 1 mole of any substance at STP (#19 on the Gas Laws Calculations)
Reminder, tomorrow is your Unit 9 Test. The Practice test and it’s answer key are posted for you to review with.
On top of that, you’ll be receiving your first review for semester 2. Today’s version is in outline form as a guideline for you to start pilfering through your handouts, notes, and other materials that may help you review for the final since I’m sure by now you sorta feel like this guy on the left.
We have one Unit left to sort through before we take on this exam fill boar. But until then, use your time wisely as we prepare for our last Test and Final of this School year.
Now that you have completed the simple VSEPR diagrams and made your models of Linear, Trigonal, and Tetrahedral molecular geometry… it’s time to break the rules.
The rule we’re breaking is the Octet rule. To this point you have limited the central atom to sharing up to 8 electrons. But, If your Lewis Dot Diagram has too few electrons, you add pairs of electrons to the central atom.
Let me show you what I mean. Let’s say that we have XeF2.If you calculate the valence electrons you should have 22.
But when you make the Lewis Dot Diagram, it only has 20 ve–.
So, we add a pair of electrons to the Xe central atom giving us a total of 22 ve–This creates a new Ideal Geometry known as Triangular Bipyramidal,which means it has placement for 5 parts (attached atoms or free electron pairs) around the central atom.
Like Tetrahedrons, we are working now in 3-dimensions instead of 2.
There is also an Ideal Geometry for 6 parts known as Octahedron. Think of the central atom as a 6 -sided die. So atoms can be bonded in 6 places and in 3-dimensions!
Now that we know how to find the general structure of a molecule using Lewis Dot diagrams, we can actually find the three-dimensional shape of a molecule AND BUILD IT! We can find the shapes of molecules using the VSEPR (Valence Shell Electron Pair Repulsion) Theory.
The idea is that atoms and electrons found around a central atom are repelled by each other because of the negative charges of the electrons surrounding each (remember opposites attract +/- and similar charges repel -/- or +/+). In other words, everything bonded or attached to the central atom wants to be as far away from everyone else as possible.
So let’s look at NH3 for example.
Step 1: Calculate the valence electrons
1 x N = 1 x 5 = 5 3 x H = 3 x 1 = 3 5+3 = 8 ve–
Step 2: Draw the Lewis Dot Structure
Step 3: Calculate the ABE type
Each letter of ABE stands for a part of the molecule
A= A central atom. If it has a central atom, write an A
B= Attached atoms. Count the number of atoms attached to the central atom and write that as a subscript of B example: B3
E= Free Electron Pairs. If their are extra electron pairs on the central atoms we count them as pairs and write that as a subscript of E (if there are no pairs, do not write E. If there’s only 1 pair, just write E) example: E2
NH3 has a central atom, three attached atoms, and 1 electron pair. So the ABE structure would be AB3E
Step 4: Find the Ideal Geometry.
I like to think of the ideal geometry as places on the central atom with thing happening. If there is only 2 places where things are happening (attached atoms or free electrons) then it’s Linear. If there’s three places, it’s Trigonal. If there’s four, it’s Tetrahedral.
Below is a great link to a video explaining the different shapes and where they come from.
Since NH3 is an AB3E structure there are 4 places where things are happening (B 3 + 1 E) so NH3 is Tetrahedral.
Step 5: Molecular Shape.
Along with the ABE chart is the list of Ideal Geometry and Molecular shape. The shape is based on the idea that the other atoms want to be as far apart as possible AND that free electron pairs need a lot of space to roam.
NH3 has 1 free pair of electrons that float to the top of the molecule as if they were in a balloon. The three Hydrogens then act as a tripod for the entire molecule holding it up. Therefore we say the shape of NH3 is pyramidal.
Lots to do today so lets go over our agenda: 1. Turn in assignment from yesterday 2. Take the Unit 9 Discovery Quiz below. 3. Copy the table on the board to your notes. 4. Take The last of our notes 5. Complete today’s assigmnent.
If you do not see the quiz below, click the link at the top of this post to be directed directly to the quiz.
By the way… this is the 100th post on our blog so… congrats to us.
eriously though, here is the video on Bonding. Use this link if the video does not play –> 
MrKubuske.com 