1. Atoms, Isotopes, & Ions

2. An atom consists of a nucleusnucleus –protons and neutrons electrons in orbitals around the nucleus.electrons in orbitals around the nucleus. The Structure of the Atom Nucleus Electron cloud

3. Atomic Number vs Mass Number Atomic # = # of protons in an atom Mass # = # of protons + neutrons in an atom He 4242 Mass Number  Atomic Number 

4. Isotopes Isotopes - Atoms of the same element but different mass number.Isotopes - Atoms of the same element but different mass number. Boron-10 ( 10 B) has 5 p and 5 nBoron-10 ( 10 B) has 5 p and 5 n Boron-11 ( 11 B) has 5 p and 6 nBoron-11 ( 11 B) has 5 p and 6 n 10 B 11 B

5. Isotopes? Which of the following represent isotopes of the same element? Which element? 234 X 234 X 235 X 238 X 92 93 9292

6. Isotopes & Their Uses Bone scans with radioactive technetium-99.

7. Isotopes & Their Uses The tritium content of ground water is used to discover the source of the water, for example, in municipal water or the source of the steam from a volcano.

8. Counting Protons, Neutrons, and Electrons Protons: Atomic Number (from periodic table) Neutrons: Mass Number minus the number of protons (mass number = protons +neutrons) Electrons: –If it’s an atom, the protons and electrons must be the SAME so that it is has a net charge of zero (equal numbers of + and - charges) –If it does NOT have an equal number of protons & electrons, it is NOT an atom, it is an ION.

9. 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 o _______ _______ _______ #e - _______ _______ _______

10. Answers 12 C 13 C 14 C 6 6 6 #p + 6 6 6 #n o 6 7 8 #e - 6 6 6

11. IONS IONS are atoms or groups of atoms with a positive or negative charge.IONS are atoms or groups of atoms with a positive or negative charge. Taking away an electron from an atom gives it a positive charge.Taking away an electron from an atom gives it a positive charge. Adding an electron to an atom gives it a negative charge.Adding an electron to an atom gives it a negative charge. To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na + Ca +2 I - O -2To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na + Ca +2 I - O -2 Na Ca I O Na Ca I O

12. Forming Cations & Anions A CATION forms when an atom loses one or more electrons and therefore has an overall positive charge. An ANION forms when an atom gains one or more electrons and therefore has an overall negative charge.

13. QUESTIONS What is the result when the number of electrons for a given atom changes? What is the result when the number of neutrons for a given atom changes? What is the result when the number of protons for a given atom changes?

14. Learning Check An atom has 14 protons and 20 neutrons. A.Its atomic number is 1) 142) 203) 34 B. Its mass number is 1) 142) 203) 34 C. The element is 1) Si2) Ca3) Se D.Another isotope of this element is 1) 34 X 2) 34 X 3) 36 X 16 14 14

15. Visualizing Isotopes & Ions Hydrogen Ion: http://web.visionlearning.com/custom/chemis try/animations/CHE1.3-an-ions.shtml Hydrogen Isotope: http://web.visionlearning.com/custom/chemis try/animations/CHE1.3-an-isotopes.shtml http://web.visionlearning.com/custom/chemis try/animations/CHE1.3-an-isotopes.shtml

16. Learning Check State the number of protons, neutrons, and electrons in each of these ions. 39 K + 16 O -241 Ca +2 198 20 #p + ___________________ #n o ___________________ #e - ___________________

17. One Last Learning Check Write the nuclear symbol form for the following atoms or ions: A. 8 p +, 8 n, 8 e - ___________ B.17p +, 20n, 17e - ___________ C. 47p +, 60 n, 46 e - ___________

18. Isotopes and Average Atomic Mass -A sample of any element consists of one or more isotopes of that element. -Each isotope is a different weight. -The relative amounts of each isotope for any element represents the isotope distribution for that element. -The atomic weight is the average of the isotope weights weighted for the isotope distribution Atomic Mass =[(mass of isotope) (%abundance) ] + [(mass of isotope) (%abundance)] + [….] 100%

19. Practice Problem The natural abundance for boron isotopes is: 19.9% 10 B (10.013 amu) and 80.1% 11 B (11.009amu). Calculate the atomic weight of boron.

20. Some Humor A neutron walks into a restaurant and orders a couple of drinks. As she is about to leave, she asks the waiter how much she owes. The waiter replies, “For you, No Charge!!!”

22. Next week…how does atomic structure relate to the periodic table?