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1. Atomic Structure

1. Atomic Structure. Objectives: Describe properties of subatomic particles Recall how element / nuclear symbols work Explain the existence of isotopes. The atom model from GCSE:. The subatomic particles from GCSE:. The subatomic particles from GCSE:. THE STRUCTURE OF ATOMS.

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1. Atomic Structure

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  1. 1. Atomic Structure Objectives: Describe properties of subatomic particles Recall how element / nuclear symbols work Explain the existence of isotopes.

  2. The atom model from GCSE:

  3. The subatomic particles from GCSE:

  4. The subatomic particles from GCSE:

  5. THE STRUCTURE OF ATOMS Atoms consist of a number of fundamental particles, the most important are ...

  6. Subatomic particles Atoms consist of a number of fundamental particles, the most important are ... 1 +1 1.672 x 10-27 1.602 x 10-19 1 0 1.675 x 10-27 0 1 1836 -1 9.109 x 10-31 1.602 x 10-19 Calculate the mass of a carbon-12 atom; it has 6 protons, 6 neutrons and 6 electrons

  7. Subatomic particles Atoms consist of a number of fundamental particles, the most important are ... 1 +1 1.672 x 10-27 1.602 x 10-19 1 0 1.675 x 10-27 0 1 1836 -1 9.109 x 10-31 1.602 x 10-19 Calculate the mass of a carbon-12 atom; it has 6 protons, 6 neutrons and 6 electrons 6 x 1.672 x 10-27+6 x 1.675 x 10-27+6 x 9.109 x 10-31 =

  8. Subatomic particles Atoms consist of a number of fundamental particles, the most important are ... 1 +1 1.672 x 10-27 1.602 x 10-19 1 0 1.675 x 10-27 0 1 1836 -1 9.109 x 10-31 1.602 x 10-19 Calculate the mass of a carbon-12 atom; it has 6 protons, 6 neutrons and 6 electrons 6 x 1.672 x 10-27+6 x 1.675 x 10-27+6 x 9.109 x 10-31 = 2.0089 x 10-26 kg

  9. Mass number and atomic number Atomic Number (Z) Mass Number (A)

  10. Mass number and atomic number Atomic Number (Z) Number of protons in the nucleus of an atom Mass Number (A) Sum of the protons and neutrons in the nucleus

  11. 23 Na 11 Mass number and atomic number Atomic Number (Z) Number of protons in the nucleus of an atom Mass Number (A) Sum of the protons and neutrons in the nucleus Mass Number (A) PROTONS + NEUTRONS Atomic Number (Z) PROTONS

  12. 23 Na 11 Mass number and atomic number Atomic Number (Z) Number of protons in the nucleus of an atom Mass Number (A) Sum of the protons and neutrons in the nucleus Mass Number (A) PROTONS + NEUTRONS THERE WILL BE 12 NEUTRONS IN THE NUCLEUS 23 – 11 = 12 Atomic Number (Z) PROTONS

  13. Atoms and Ions • What is an ion? • How is a negative ion made? • How is a positive ion made? • Describe: Br- • Describe Mg2+

  14. Mass number and atomic number

  15. Mass number and atomic number

  16. Isotopes Definition:

  17. Isotopes Definition: Isotopes of an element are atoms with the same number of protons, but different numbers of neutrons • Chemical properties of isotopes are identical • Physical properties (such as density) can differ

  18. Isotopes Example: Chlorine-35 and Chlorine-37

  19. Isotopes - calculations There are two common isotopes of chlorine. Calculate the average relative atomic mass of chlorine atoms Method 1 Three out of every four atoms will be chlorine-35 Average = 35 + 35 + 35 + 37 = 35.5 4 Method 2 Out of every 100 atoms 75 are 35Cl and 25 are 37Cl Average = (75 x 35) + (25 x 37) = 35.5 100

  20. Questions (actual exam ones) • Hydrogen, deuterium and tritium are all isotopes of each other. • Identify one similarity and one difference between these isotopes. • Deuterium can be written as 2H. Determine the number of protons, neutrons and electrons in a neutral deuterium atom. • Write a nuclear symbol for tritium, given that it has 2 neutrons. 2. A certain atom X has one less proton and two more neutrons than K. What are its atomic number and mass number? • Explain in terms of sub atom particles, why C-12 and C-14 are isotopes

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