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Building Atoms!

This activity explores the structure of atoms using everyday objects like Cheerios, Smarties, and Starbursts. Students will learn about protons, neutrons, and electrons and how they contribute to an atom's stability. They will also discover the concepts of isotopes, radioisotopes, and electronegativity.

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Building Atoms!

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  1. Building Atoms! AP Biology

  2. On your paper • Label Notes 2.1

  3. Categories • Cheerios – Electrons • Smarties – Protons • Starbursts - neutrons

  4. Build a Helium Atom Draw & Label in notebook

  5. Suppose…. What is it called now? • The number of protons change? • The number of electrons change? • The number of neutrons change? • What is a radioisotope? New element! Ion Isotope Radioactive; unstable nucleus

  6. Build Hydrogen Draw & Label in notebook

  7. Predict in your notebook… • If Hydrogen gained a proton, what would it be called…. • If hydrogen lost an electron, what would it be called… • If hydrogen gained a neutron? Helium Hydrogen ion “oxidized” Isotope deuterium

  8. How many electrons fit each orbital? • First – 2 • Second -8 • Third -8

  9. Build Nitrogen • Is nitrogen electrically stable? • What does nitrogen need to be electrically stable?

  10. Build Oxygen • Is oxygen electrically stable? • What does oxygen need to be electrically stable? • Is oxygen more reactive than nitrogen?

  11. Build Fluorine. • Is Fluorine electrically stable? • What does Fluorine need to be electrically stable? • Is fluorine more reactive than nitrogen? Oxygen?

  12. What is electronegativity? • Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons • What is the trend of electronegativity on the periodic table? • Electronegativity increases from left to right and decreases from top to bottom down a column • Which elements are the most stable? • Which elements are the most reactive?

  13. PDQ 2.1

  14. 1. Atom vs. Element Atom Element Pure substance Contains only 1 kind of atom Has unique characteristics that distinguish it from other elements 94 elements in nature More than 24 have been made in laboratories • Basic unit of matter • Composed of protons, neutrons and electrons

  15. 2. 6 elements common in bio • SPONCH • Sulfur – found in certain proteins • Phosphorus – found in DNA • Oxygen – required for aerobic organisms • Nitrogen – found in DNA and protein • Carbon – basic atom in all organic molecules • Hydrogen – also in all organic molecules

  16. 3. Describe atom structure • Composed of • Protons – in nucleus, positive charge • Neutrons – in nucleus, no charge • Electrons – in orbitals/electron cloud, negative charge • Most atoms are electrically neutral, which means the number of electrons = number of protons

  17. 3. Continued. Label and define Electron Cloud nucleus Neutron Center of an atom where the protons and neutrons are located. Proton Electron Cloud – Darker areas show probable location of where electrons would be.

  18. 3. Continued. Label and Define electron proton neutron Orbital/ Electron Shell Paths where electrons travel  have varying distances from nucleus

  19. 4. Atomic Mass vs. Atomic Number Atomic Mass Atomic Number Equal to the number of protons Unique to each element Oxygen is number 8 and therefore has 8 protons. • Protons + Neutrons • Example – Oxygen has an atomic mass of 16. Because it has 8 protons and 8 neutrons. • The mass written on periodic tables refers to the average atomic mass. You would round this number to determine number of neutrons

  20. 5. Atomic mass vs. Atomic Weight Atomic Mass Atomic Weight Is the average mass of all naturally occuring isotopes of an element Also called average atomic mass. This is what is on the periodic table. • Mass of a single atom or an individual isotope

  21. 6. How to calculate number of neutrons • Number of neutrons = atomic mass (rounded) – number of protons • For example, nitrogen. • Protons = 7 • Atomic mass is 14. • Number of neutrons = 14-7 = 7.

  22. 7. Isotopes • Have a different number of neutrons than it’s element • Each isotope has a different mass number. • Radioactive isotopes are radioactive and have an unstable nucleus. (They have excess nuclear energy)

  23. 8. What determines interactions between atoms? • Number of electrons

  24. 8. Continued… Valence electrons • Valence electrons are the electrons that are on the outermost electron shell. • They determine how reactive the atom will be.

  25. 8. Continued… All atoms thrive to have 8 electrons in their outer shell – octet rule. They will react to get it! Some want it more than others…..

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