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Chapter 10

Chapter 10. Periodic Trends Density Atomic and Ionic Radii. Density. Iridium (Z = 77) has the highest density. We can predict that an element is more dense if it is closer to Iridium. Density. Effective Nuclear Charge (Z eff ).

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Chapter 10

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  1. Chapter 10 Periodic Trends Density Atomic and Ionic Radii

  2. Density • Iridium (Z = 77) has the highest density. • We can predict that an element is more dense if it is closer to Iridium.

  3. Density

  4. Effective Nuclear Charge (Zeff) • The effective nuclear charge (Zeff) of an atom is basically how well it is able to hold on to its most loosely held electron.

  5. Atomic radius (radii) • The atomic radius is essentially the size of an atom.

  6. Atomic radius (radii) • Theatomic radius is essentially the size of an atom. • The largest atom is Francium (Z = 87).

  7. Atomic radius (radii) • The atomic radius is essentially the size of an atom. • The largest atom is Francium (Z = 87). • We can predict that an atom is larger if it is closer to Francium.

  8. Atomic Radius Xylophone monkey

  9. Atomic Radius and Effective Nuclear Charge • The atomic radius decreases as effective nuclear charge increases.

  10. Effective Nuclear Charge (Zeff) • The effective nuclear charge of an atom is primarily determined by: • The nuclear charge • The shielding effect

  11. The Nuclear Charge (Z) • Based on the number of protons in the nucleus. • Example: Carbon vs. Nitrogen

  12. The Nuclear Charge (Z)

  13. The Nuclear Charge (Z) • The greater the number of protons in the nucleus the greater the effective nuclear charge.

  14. Conclusion: Nitrogen is a smaller atom than carbon because nitrogen has 7 protons to pull in its electrons whereas carbon only has 6.

  15. Nuclear charge explains why atoms get smaller across a period Atomic Radius Xylophone monkey

  16. Shielding Effect. • The shielding effect is when electrons between the nucleus and the outermost electrons in an atom shield or lessen the hold of the nucleus on the outermost electrons.

  17. Shielding Effect. He Ne

  18. Conclusion: Neon is larger than helium because it has an increased shielding effect from having two energy levels whereas helium only has one energy level. He Ne

  19. Rank the atoms from smallest to largest • Na, K, O, N

  20. Chemical Reactivity • Metals tend to lose electrons when reacting • Nonmetals tend to gain electrons when reacting • Effective nuclear charge allows us to use the periodic table to predict reactivity.

  21. Chemical Reactivity • Metals increase in reactivity left and down. • Nonmetals become more reactive up and to the right. • Most reactive metal is? • Most reactive nonmetal is? Fr F

  22. Shielding Effect explains why atoms get larger down a group Atomic Radius Xylophone monkey

  23. Ionic Radius • Ionic Radius is the size of an ion.

  24. Size Change in Ion Formation

  25. Rules for Ionic Radius • Ionic Radius goes by the same rules as atomic radius however it is necessary to treat anions and cations seperately. • Anions are “always” larger than cations.

  26. Rank the ions from smallest to largest • K+, N3-, Na+, O2-

  27. Homework • Worksheet: Density, Atomic and Ionic Radii

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