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AP Chemistry ATOMIC STRUCTURE

AP Chemistry ATOMIC STRUCTURE . DO NOW: Answer the following questions What are the subatomic particles? Where are each subatomic particle located? What is the charge associated with each subatomic particle?. THE ATOM.

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AP Chemistry ATOMIC STRUCTURE

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  1. AP Chemistry ATOMIC STRUCTURE DO NOW: Answer the following questions What are the subatomic particles? Where are each subatomic particle located? What is the charge associated with each subatomic particle?

  2. THE ATOM • Atom – the smallest particle of an element that can enter into a chemical reaction • Can be broken down into subatomic particles

  3. Subatomic particles REMEMBER  P….E….N

  4. All atoms are composed of a dense nucleus surrounded by “empty” space occupied by electrons. Subatomic particles

  5. 1) The nucleus contains two types of particles; protons with a positive charge and neutrons with no charge. 2) The mass of a protons or a neutron is 1 amu. 3) The number of protons in the nucleus of an atom is the atomic number. Subatomic particles

  6. 4) For a neutral atom: atomic # = # protons = # of electrons 5) Each atom must contain the same number of protons but do not always contain the same number of neutrons 6) Electrons are located in orbitals outside the nucleus and have a charge equal to but opposite of, a proton. Subatomic particles

  7. 7) The sum of the number of protons and neutrons in the nucleus is called the mass number. Ex: Mass # - # of protons = # of neutrons Ex: Mass # - # of neutrons = # of protons Subatomic particles

  8. 8) A neutral atom of Magnesium (Mg) contains 12 protons and 12electrons. 9) When the mass # of a neutral atom of Sulfur (S) is 30 then the number of protons / electrons is 16 and the # of neutrons is 14. Subatomic particles

  9. Isotopes and Atomic Masses 1) All atoms of a given element must contain the same # of protons but the # of neutrons may vary. 2) Isotopes are atoms of the same element that have different #s of neutrons, and hence have different mass numbers.

  10. Isotopes and Atomic Masses 3) Isotopes are identified by using a symbol that indicates both the element and its mass number. 4) The mass number of any given element must be an integer because it is the sum of all protons and neutrons

  11. ISOTOPES OF He (________________)

  12. ISOTOPES OF C (________________)

  13. Isotopes and Atomic Masses 5. The average atomic mass is the weighted average of all the isotopes of a given element and is the number in the top left corner of each element on the Periodic Table.

  14. PRACTICE: Determine the average atomic mass of the following mixtures of isotopes 1. 80% 127I, 17% 126I, 3% 128I

  15. PRACTICE: Determine the average atomic mass of the following mixtures of isotopes 2. 50% 197 Au, 50% 198 Au

  16. Important Definitions Nucleons: particles in the nucleus (protons and neutrons) Nuclear Charge: charge of the nucleus (same at # of protons) Examples: How many nucleons are there in an atom with an atomic number of 20 and 23 neutrons? What is the nuclear charge of an Iron atom?

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