Atomic Models, Isotopes & Radioactivity

Name the three main subatomic particles and state their charges.

What does the atomic number tell you about an atom?

What does the mass number tell you about an atom?

Define isotope.

How are carbon-12 and carbon-14 similar and different?

What is radioactivity?

Why did scientific models of the atom change over time?

State one piece of evidence that showed atoms have internal structure.

Give one useful application of a radioactive isotope.

Correct this misconception: “All radiation is artificial and always dangerous.”

Compare Dalton’s solid-sphere model with the modern atomic model. Explain what changed and why.

Use atomic number and mass number to determine the numbers of protons, neutrons and electrons in a neutral atom.

Explain how isotopes of the same element can have the same chemical identity but different mass numbers.

Describe how Rutherford’s gold foil experiment changed the model of the atom.

Explain why radioactive isotopes can be useful in medicine, industry or archaeology, while still requiring careful control.

Compare alpha, beta and gamma radiation in terms of particle/energy type and penetrating ability.

A student says, “Radioactive atoms are different elements because they are radioactive.” Evaluate and correct this statement.

Create a timeline of atomic model development from Dalton to Thomson, Rutherford, Bohr and the modern model.

Explain how new evidence can support, modify or replace a scientific model using the atom as your example.

Write a full explanation of one isotope, including its structure, stability or radioactivity, and one real use or risk.