Atoms and Isotopes

Atoms and Isotopes

Introduction to Nuclear Energy

Multiple Select

What are atoms composed of?

• Neutrons

• Protons

• Electrons

• Gammons

Multiple Select

Which of the following is true about the Bohr-Rutherford Model of an atom?

• Protons and electrons are densely packed in the nucleus.

• Neutrons orbit around the nucleus.

• Neutrons and protons are densely packed in the nucleus.

• Most of the mass of an atom exists in its electrons.

Multiple Select

Which of the following are true about the Bohr-Rutherford Model of an atom?

• Most of the atom is empty space.

• There can up to two electrons in the innermost shell of any atom.

• Tiny electrons orbit the nucleus.

• Each shell of electrons represents a different energy level.

Multiple Select

Which quantity determines the type of atom we are dealing with?

• Number of Protons

• Number of Neutrons

• Number of Electrons

• Total Number of Subatomic Particles

Bohr-Rutherford Model

• The dense nucleus contains the atom's protons and neutrons.

• The relatively tiny electrons orbit the nucleus (much smaller than protons and neutrons).

• The electrons only occupy certain energy levels.

• Most of the atom consists of empty space.

Excited Electrons

• Electrons are said to be in their ground state when they have the lowest energy possible.

• Electrons are said to be in an excited state when they have received enough energy to allow them to jump to the next energy level (move to the next shell).

• Electrons then drop back down to their ground state (where they like to be) and emits energy in the process.

Isotope

• An Isotope is a form of an element that has the same atomic number but a different atomic mass.

• The atomic number (the number of protons in the nucleus) determines the element, so the element remains the same.

• Because the mass is different, however, the number of neutrons in the nucleus of each atom is not the same.

• When there is an element that can exist with a different number of neutrons, it is an isotope.

Carbon

• Carbon is an element that has isotopes.

• Carbon-12 has 6 protons and 6 neutrons; a mass number of 12.

• Carbon-14 has 6 protons and 8 neutrons; a mass number of 14.

• Both isotopes of carbon exist naturally. Carbon-12 is more common than Carbon-14.

Radioisotopes

• Some isotopes (radioisotopes) are unstable and spontaneously change their structure.

• They want to be in a stable state so they change their structure to become more stable.

• During the change, they release various particles and energy in the form of radiation.

• The radiation that is released is potentially dangerous if not handled safely. The radiation can also be used to benefit us in various ways.

Benefits of Radioisotopes

• Medical Applications of Radioisotopes

• Nuclear Medical Imaging: Radioactive dyes (ie, technetium-99m) can be injected into patients to detect differences in organ function.

• The differences located by the radioactive tracing (we can detect the energy emissions) are more detailed than those detected by X-rays . They can detect differences in soft tissue as well as bones while X-rays are used primarily for bone fractures.

Benefits of Radioisotopes

• Medical Applications of Radioisotopes

• Radionuclide Therapy (RNT) is a field in medicine in which the properties of certain radioactive materials are used to treat ailments such as thyroid disease and cancer.

• An example of this is the use of Iodine-131 to identify and treat thyroid disease.

Open Ended

What did you learn from today's lesson?

Open Ended

Is there anything that you already know about radioactive decay? Is there anything you want to learn more about? We will be looking at the particles and energy released from radioactive isotopes tomorrow in class.

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