1. Gallery walk Chapter 7

2. 5H2 Station 1 What number is the coefficient?
What number is the subscript?
What element is the H
How many H are there?

3. Station 2
Write the total number of each elements in the following examples:

4. Station 3 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

5. Station 4 Balance the equation using the notecards on the table – write the final balance equation
Now, count the number of molecules of each element present on both sides of the equation.
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

6. Station 5 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

7. Station 6 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

8. Station 7 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

9. Station 8 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

10. Station 9 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

11. Station 10 Balance the equation using the notecards on the table – write the final balance equation
Take the unbalanced equation and make a note of the elements present in each side of the equation.
Now, count the number of molecules of each element present on both sides of the equation.
Here comes the task of balancing the chemical equations. You should see that same numbers of molecules of all elements are present on the reactants side as well as the products side. The equation should follow law of conservation of mass i.e. matter is neither created nor destroyed.
While balancing the equations you should only change the co-efficient of the chemical formula but not the subscripts. Changing the subscripts will change the components.
Start by balancing one element at a time. Finally check if all the elements are balanced.

12. Station 11 Diatomic Atoms
Is Dr. H2O2F2Br2I2N2Cl2 in the house??
There are 7 diatomic molecular elements on the periodic table. When they are in the elemental state (all by themselves, not tied up in a compound) they must have a subscript 2 behind them.
Each molecule is made of two atoms of the substance.
They never exist as single atoms. They are either tied up in a compound, or tied up (chemically bonded) with each other as two packs (diatomic molecules). When balancing equations, you can never have one of these seven elements all by itself as a single atom. Doesn't happen. They can be in a compound however without the subscript two.

13. Station 12 I Never Bring Clay From Our Home upside down backward L and H Write down the saying to help remember the diatomics – then shade in the periodic table with purple

14. Station 13 Law of Conservation of Mass- mass can not be created or destroyed only changed forms.

15. Station 14 Types of reactions
Endothermic
Exothermic
heat is absorbed (feels cold)
heat is released (feels warm)
energy must be added for reaction to occur
reaction occurs spontaneously
Example of Endothermic Process
Photosynthesis is an example of an endothermic chemical reaction. In this process, plants use the energy from the sun to convert carbon dioxide and water into glucose and oxygen. This reaction requires energy (sunlight) for every glucose that is produced:
sunlight + 6CO2(g) + H2O(l) = C6H12O6(aq) + 6O2(g)
Example of Exothermic Processes
An example of an exothermic reaction is the mixture of sodium and chlorine to yield table salt.
Na(s) + Cl2(s) = NaCl(s)

16. How many of each element are on each side of the equation to start
How many of each element are on each side of the equation to start? Is it balance? N H N H