Activity 2

Activity 2

Key for Models

Protons: Red/Pink

Neutrons: Green

Electrons: Blue

Models

Hydrogen Model

Atomic Mass: 1

Atomic Weight: 1.008

                                                                                     Lithium Model

                                                                                     Atomic Mass: 3

                                                                                     Atomic Weight: 6.94

Boron Model

Atomic Mass: 5

Atomic Weight: 10.81

Questions

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

Hydrogen: 1

Lithium: 3

Boron: 5

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

Hydrogen: 1.008

Lithium: 6.94

Boron: 10.81

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

Protons and neutrons should be equal. However, the rule is that you take the atomic mass minus the atomic weight to find the number of neutrons. For Lithium, this would mean 6. 94 (or 7) minus 3, which is 4. Lithium would then have one more neutron than proton. The same goes for Boron, which would be 10.81 (or 11) minus 5 equals 6 neutrons. As for Hydrogen, there would be no neutrons, because one minus one is zero.

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

I would add or subtract a Q-tip depending on the number of isotopes needed.

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

The nucleus, which consists of the protons and neutrons, takes up the most volume of an atom.

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

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

We see light when the electron returns to the ground-state.

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.

When the electrons get excited the jump up to a higher orbital level. Once they lose some of that energy, the electrons fall back down to their original state. Depending on how far the electron falls, it changes what type of wavelength is created or what color light is shone.

9. You may observe fireworks over the New Year's, explain how the different colors of fireworks arise.

When atoms inside the firework are heated, their electrons get very excited and jump to a higher orbital level. Once the electrons drop back down, it produces several different colors of light.

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

The periodic table is organized in a grid-like fashion with row and column holding different characteristics. Each row is called a period and each element in a given period has the same number of atomic orbitals as the rest of the elements in that period. Each column is called a group; elements in each group have the same number of valence electrons (electrons in the outer orbital).

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 and Sodium

Alkaline Earth: Barium and Radium

Halogens: Chlorine and Iodine

Noble Gases: Neon and Radon

Transition Metals: Iron and Nickel

Non-Metals: Carbon and Oxygen

Metalloids: Antimony and Boron