Atomic structure

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Atomic structure

  1. 1. ATOMIC STRUCTURE Take these notes on page 31 in your notebook. Use the Cornell Method of Note taking. Label and Date the page.
  2. 2. SUBATOMIC PARTS Electrons Represented with lower case (e) In electron shells or energy levels around the nucleus Negatively charged (-)
  3. 3. SUBATOMIC PARTS Protons -Represented with lower case (p) -In nucleus -Positively charged (+)
  4. 4. SUBATOMIC PARTS Neutrons -Represented with lower case (n) -In nucleus -No charge (neutral)
  5. 5. SUBATOMIC PARTS Atoms have no charge The # of protons = # of electrons The proton (+) and electron(-) cancel each other out. Neutrons have no charge.
  6. 6. SUBATOMIC PARTS Draw an atom and label the subatomic parts in your notes!
  7. 7. ATOMIC NUMBER Represented by capital Z. Z = the number of protons in an atom
  8. 8. ATOMIC NUMBER
  9. 9. ATOMIC NUMBER  Use the periodicTable on page 288-289 in your textbook to find the symbols and atomic number of the following elements: Selenium Zinc Caesium Chromium
  10. 10. MASS NUMBER “Electrons are to protons as fleas are to an elephant – the proton being the elephant. When we calculate the mass of an elephant, we don’t add on the mass of the elephant‘s fleas, and when we calculate the mass of an atom, we don’t add the mass of the electrons.” ~Joy of Chemistry, Cobb & Fetterrolf ~it takes the mass of 1837 electrons to equal the mass of 1 neutron or proton
  11. 11. MASS NUMBER Since electrons weigh so little they are not included in calculating atomic mass. Mass number is represent by capital (A) Mass Number is calculated by adding the number of protons and the number of neutrons Mass number = atomic number + number of neutrons A = Z + number of neutrons
  12. 12. MASS NUMBER
  13. 13. MASS NUMBER Use the periodicTable on page 288-289 in your textbook to find the symbols and mass number of the following elements: Molybdenum Osmium Titanium Sulphur
  14. 14. MASS NUMBER We can use the mass number to calculate the number of neutrons: Number of neutrons = mass number – atomic number Neutrons = A - Z
  15. 15. NUMBER OF NEUTRONS Using the atomic numbers and mass numbers you found to calculate the number of neutrons in: Molybdenum Osmium Titanium Sulphur Selenium Zinc Caesium Chromium
  16. 16. IONS Ions are electrically charged particles If an atom loses one or more electrons it becomes positively charged (K+) If an atom gains one or more electrons it becomes negatively charged (Cl-)
  17. 17. DIDYOU LABEL AND DATEYOUR PAGE? Complete your Notes with a Summary and Main Ideas or Questions in the Left column!

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