2. Structure of the Atom

3. SC Standards Covered Standard PS-2.1Compare the subatomic particles (protons, neutrons, electrons) of an atom with regard to mass, location, and charge, and explain how these particles affect the properties of an atom (including identity, mass, volume, and reactivity). Standard PS-2.4Use the atomic number and the mass number to calculate the number of protons, neutrons, and/or electrons for a given isotope of an element.

4. Scientific Shorthand Each element can be represented by a one, two, or three letter chemical symbol Each symbol consists of one capital letter plus one or two lower case letters

5. Atomic Components Atom Atom - smallest particle of an element which retains the properties of that element.

6. Atomic Theory Atoms are building blocks of elements Similar atoms in each element Different from atoms of other elements Two or more different atoms bond in simple ratios to form compounds

7. Basic Structure The center of the atom is called the nucleus. Surrounding the nucleus is the electron cloud.

8. ParticleSymbolLocationChargeMass Electron e -1 Space around the nucleus 1/1840 amu Proton n0n0 In the nucleus +1 1 amu Neutron p +1 In the nucleus 0 1 amu Subatomic Particles

9. Quarks Quarks – particles that make up protons and neutrons –Three quarks make up a proton or neutron

10. Fine Points to the Structure of the Atom All of the mass of an atom is located in the nucleus All of the volume of the atom is taken up by the electron cloud

12. Atomic Number Atomic number – counts the number of protons in an atom - Used to identify the element - Periodic Table arranged by it Atoms are electrically neutral (not charged) # of protons = # of electrons

13. Learning Check State the number of protons for atoms of each of the following: A. Nitrogen 1) 5 protons 2) 7 protons 3) 14 protons B. Sulfur 1) 32 protons 2) 16 protons 3) 6 protons C. Barium 1) 137 protons 2) 81 protons 3) 56 protons

14. Solution State the number of protons for atoms of each of the following: A. Nitrogen 2) 7 protons B. Sulfur 2) 16 protons C. Barium 3) 56 protons

15. Mass Number Mass Number – Counts the number of protons and neutrons in an atom Number of Neutrons = Mass Number – Proton Number (atomic #)

16. What is the Mass Number of the following Atoms?

17. Isotopes Isotopes - atoms of the same element with different numbers of neutrons

18. More Examples of Isotopes

19. Notation of Isotopes Potassium - 40 K 40 19 Mass number Atomic number

20. Learning Check Naturally occurring carbon consists of three isotopes, 12 C, 13 C, and 14 C. State the number of protons, neutrons, and electrons in each of these carbon atoms. 12 C 13 C 14 C 6 6 6 #P _______ _______ _______ #N _______ _______ _______ #E _______ _______ _______

21. Carbon - 12Carbon - 13Carbon - 14

22. Atomic mass - weighted average of all the isotopes of a particular element –T–This is the mass indicated on the periodic table. –T–This number will be closest to the most common isotope of the element.

23. Learning Check An atom of zinc has a mass number of 65. A.Number of protons in the zinc atom 1) 302) 353) 65 B.Number of neutrons in the zinc atom 1) 302) 353) 65 C. What is the mass number of a zinc isotope with 37 neutrons? 1) 372) 653) 67

24. Solution An atom of zinc has a mass number of 65. A.Number of protons in the zinc atom 1) 30 B.Number of neutrons in the zinc atom 2) 35 C. What is the mass number of a zinc isotope with 37 neutrons? 3) 67

25. Learning Check Write the isotope (nuclear) notation for atoms with the following: A. 8 p +, 8 n, 8 e - ___________ B.17p +, 20n, 17e - ___________ C. 47p +, 60 n, 47 e - ___________

26. Solution 16 O A. 8 p +, 8 n, 8 e - 8 B.17p +, 20n, 17e - 37 Cl 17 C. 47p +, 60 n, 47 e - 107 Ag 47