Activity #2

Activity 2: Atom and Atomic Structure
For this activity review the Content Slides (Atoms and Atomic Structure) and complete the activities/questions below.

Make a model of your three favorite elements on the Periodic Chart.  The models must be 3-dimensional and be made out of common objects around your home.  Place photos of your three models with descriptions on your blog. Your models must include the appropriate number and positioning of protons, neutrons and electrons.

Name: Carbon
Symbol: C
Atomic Number: 6
Atomic Mass: 12.0107 amu
Melting Point: 3500.0 °C (3773.15 K, 6332.0 °F)
Boiling Point: 4827.0 °C (5100.15 K, 8720.6 °F)
Number of Protons/Electrons: 6
Number of Neutrons: 6
Classification: Non-metal
Crystal Structure: Hexagonal

Name: Sodium
Symbol: Na
Atomic Number: 11
Atomic Mass: 22.98977 amu
Melting Point: 97.72 °C (370.87 K, 207.9 °F)
Boiling Point: 883 °C (1156 K, 1621 °F)
Number of Protons/Electrons: 11
Number of Neutrons: 12
Classification: Alkali Metal
Crystal Structure: Cubic

Name: Chlorine
Symbol: Cl
Atomic Number: 17
Atomic Mass: 35.4527 amu
Melting Point: -100.98 °C (172.17 K, -149.764 °F)
Boiling Point: -34.6 °C (238.55 K, -30.279997 °F)
Number of Protons/Electrons: 17
Number of Neutrons: 18
Classification: Halogen
Crystal Structure: Orthorhombic

Questions:

1. What is the atomic number for each of your models?

Carbon= 6
Sodium= 11
Chlorine= 17


2. What is the atomic mass number for each of your models?

Carbon= 12.0107 amu
Sodium= 22.98977 amu 
Chlorine= 35.4527 amu


3. In your models, which two subatomic particles are equal in number?

 The Protons and Electrons.


4. How would you make an isotope for one of your models?  What would change with the model?

I would have to have the same number of protons and neutrons. This would change the mass number. In order to have an Isotope you need the the same atomic number but a different mass number. 

5. Considering the overall volume of your element models, what makes up most of the volume of an atom?

 Considering the nucleus makes up most of the mass then empty space takes up most of the volume when looking at the atom structure I created.

6. For one of your models, show with another image what happens when energy excites an electron.

 This can happen through photoexcition or excitation.  It absorbs the photon and takes on its energy. It moves to the outer wall.


7. Once the electron is excited, what do we typically observe when the electron returns to the ground-state?

When going back to ground state they release energy and throw it back out to become neutral again.


8. Why are some elements different colors when they are excited? Hint: when electrons are excited (by something like heat from an explosive) they move up to another orbital and when they fall back they release the energy in the form of light. 

It has a photon moved to the outer level of the atom and it gives off a different color.  The color depends on the amount of energy beging released into the atom. The different numbers of electrons in an element lossing energy causes it to change colors.

9. With the Fourth of July coming up quickly, explain how the colors of fireworks arise.

 The level of heat admitted to the element has a big part in why they are the colors they are. The elements all react differently to heat and electrons gain energy at different levels. The metal salts in a firework burn better. Raw metallic metals burn and emits a light.


10.  Explain the overall organizational structure of the periodic table.

The periodic table is arranged in rows and columns.  It goes up according to the elements atomic number. There are 18 vertical columns, or groups and the horizontal rows of the table are called periods. The rows are organized by the number of electron shelves the have. Then it is broken down into groups or classes: Alkali Metals, Alkaline Earth, Halogens, Noble Gases, Transition Metals, Non-Metals, and Metalloids.

11. List two example elements for each of these groups or classes: Alkali Metals, Alkaline Earth, Halogens, Noble Gases, Transition Metals, Non-Metals, and Metalloids.

Alkali Metals:Lithium, Sodium
Alkaline Earth: Magnesium, Calcium

Halogens: Chlorine, Iodine
Noble Gases: Helium, Neon
Transition Metals: Cobalt, Copper
Non-Metals: Carbon, Hydrogen
Metalloids:  Boron, Tellurium