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Building Atoms! AP Biology On your paper • Label Notes 2.1 Categories • Cheerios – Electrons • Smarties – Protons • Starbursts - neutrons Build a Helium Atom 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? Build Hydrogen 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? How many electrons fit each orbital? • First – 2 • Second -8 • Third -8 Build Nitrogen • Is nitrogen electrically stable? • What does nitrogen need to be electrically stable? Build Oxygen • Is oxygen electrically stable? • What does oxygen need to be electrically stable? • Is oxygen more reactive than nitrogen? Build Fluorine. • Is Fluorine electrically stable? • What does Fluorine need to be electrically stable? • Is fluorine more reactive than nitrogen? Oxygen? 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? PDQ 2.1 1. Atom vs. Element Atom • Basic unit of matter • Composed of protons, neutrons and electrons 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 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 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 3. Continued. Label and define Electron Cloud nucleus Center of an atom where the protons and neutrons are located. Neutron Proton Electron Cloud – Darker areas show probable location of where electrons would be. 3. Continued. Label and Define electron proton neutron Orbital/ Electron Shell Paths where electrons travel have varying distances from nucleus 4. Atomic Mass vs. Atomic Number Atomic Mass • 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 Atomic Number • Equal to the number of protons • Unique to each element • Oxygen is number 8 and therefore has 8 protons. 5. Atomic mass vs. Atomic Weight Atomic Mass • Mass of a single atom or an individual isotope 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. 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. 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) 8. What determines interactions between atoms? • Number of electrons 8. Continued… Valence electrons • Valence electrons are the electrons that are on the outermost electron shell. • They determine how reactive the atom will be. 8. Continued… One covalent bond. Carbon – 4 Nitrogen – 3 Oxygen - 2 Phosphorus –3 Sulfur - 2 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…..