Procedure:

1. The number of protons, neutrons, and electrons determines the properties of atoms.
2. Obtain a baggie from your instructor.
3. Baggies contain the following:
- Red bead: represents a proton
- Green bead: represents a neutron
- Blue bead: represents an electron
4. Count the number of protons, neutrons, and electrons and fill out the data table below:

| Bag # | # of Protons | # of Neutrons | # of Electrons | Atomic # | Mass # | Charge | Symbol | Name |
|-------|--------------|---------------|----------------|----------|--------|--------|--------|----------|
| 1 | 29 | 35 | 29 | 29 | 64 | 0 | Cu | Copper |
| 2 | 20 | 21 | 20 | 20 | 41 | 0 | Ca | Calcium |
| 3 | 17 | 18 | 17 | 17 | 35 | 0 | Cl | Chlorine |
| 4 | 8 | 8 | 8 | 8 | 16 | 0 | O | Oxygen |

Conclusions:

1. What are the three main subatomic particles?
2. What is the relationship between protons and atomic number?
3. What is the relationship between protons, neutrons, and the mass number?
4. How could you determine the number of neutrons in a carbon-14 atom? How many are there?
5. What is the definition of an isotope? Which of your bags were isotopes?

Atoms are made up of protons, neutrons, and electrons, with the atomic number representing the number of protons. The mass number is calculated by adding protons and neutrons, and isotopes are variations of elements with differing neutron counts. For example, carbon-14 has 6 protons and 8 neutrons, making it an isotope of carbon.

Explanation:

Understanding Atomic Structure

Atoms are composed of three main subatomic particles: protons, neutrons, and electrons. The atomic number is defined as the number of protons in an atom, which also equals the number of electrons in a neutral atom. The mass number is the total number of protons and neutrons in an atom's nucleus, while the atomic mass accounts for the average mass of an element's isotopes.

Key Concepts

The three main subatomic particles are:

Protons (positively charged, found in the nucleus)
Neutrons (neutral charge, found in the nucleus)
Electrons (negatively charged, orbiting the nucleus)

The relationship between protons and atomic number is that the atomic number uniquely identifies an element. For instance, carbon has an atomic number of 6 because it has 6 protons. The relationship between protons, neutrons, and mass number can be described mathematically: mass number = protons + neutrons.

To determine the number of neutrons in a carbon-14 atom, subtract the atomic number (6) from the mass number (14): 14 - 6 = 8. Thus, carbon-14 has 8 neutrons.

An isotope is defined as an atom of the same element with a differing number of neutrons. For instance, if you had a bag that represented carbon-12 and another for carbon-14, they would be considered isotopes of carbon.

Learn more about Atomic Structure here:

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