1. Periodic Properties of the Elements Chapter 7 Periodic Properties of the Elements Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice Hall, Inc.

2. Periodic Properties of the Elements Development of Periodic Table Elements in the same group generally have similar chemical properties. Properties are not identical, however.

3. Periodic Properties of the Elements Development of Periodic Table Dmitri Mendeleev and Lothar Meyer independently came to the same conclusion about how elements should be grouped.

4. Periodic Properties of the Elements Development of Periodic Table Mendeleev, for instance, predicted the discovery of germanium (which he called eka- silicon) as an element with an atomic weight between that of zinc and arsenic, but with chemical properties similar to those of silicon.

5. Periodic Properties of the Elements Periodic Trends In this chapter, we will rationalize observed trends in  Effective nuclear effects  Sizes of atoms and ions.  Ionization energy.

6. Periodic Properties of the Elements Effective Nuclear Charge In a many-electron atom, electrons are both attracted to the nucleus and repelled by other electrons. The nuclear charge that an electron experiences depends on both factors.

7. Periodic Properties of the Elements Shielding effect Inner electrons “shield” the force of the nucleus on outer valence electrons  Force of the nucleus decreases on valence electrons, as the number of energy levels increases  Inner electrons repel outer energy levels of electrons Follows Coulomb’s Law Explains –Size of atoms –Energy required to remove a valence electron

8. Periodic Properties of the Elements Effective Nuclear Charge The effective nuclear charge, Z eff, is found this way: Z eff = Z − S where Z is the atomic number and S is a shielding constant, usually close to the number of inner electrons.

9. Periodic Properties of the Elements Sizes of Atoms The bonding atomic radius is defined as one-half of the distance between covalently bonded nuclei.

10. Periodic Properties of the Elements Sizes of Atoms Bonding atomic radius tends to… …decrease from left to right across a row due to increasing effective nuclear charge (more protons means greater force due to Coulomb’s Law pulling electrons closer) …increase from top to bottom of a column due to increasing number of energy levels

11. Periodic Properties of the Elements Sizes of Ions Ionic size depends upon:  Nuclear charge. Coulomb’s Law  Number of electrons.  Orbitals in which electrons reside.  Energy level in which electrons reside

12. Periodic Properties of the Elements Sizes of Ions Cations are smaller than their parent atoms.  The outermost electron is removed and repulsions are reduced.  Last electron is now in a lower energy level closer to the nucleus

13. Periodic Properties of the Elements Sizes of Ions Anions are larger than their parent atoms.  Electrons are added and repulsions are increased.  Since same effective nuclear charge but more electrons, electrons cannot be drawn as close making the ions larger

14. Periodic Properties of the Elements Sizes of Ions Ions increase in size as you go down a column.  Due to increasing number of energy levels

15. Periodic Properties of the Elements Sizes of Ions In an isoelectronic series (period), ions have the same number of electrons. Ionic size decreases with an increasing nuclear charge.

16. Periodic Properties of the Elements Ionization Energy Amount of energy required to remove an electron from the ground state of a gaseous atom or ion.  First ionization energy is that energy required to remove first electron.

17. Periodic Properties of the Elements Trends in First Ionization Energies As one goes down a column, less energy is required to remove the first electron.  For atoms in the same group, Z eff is essentially the same, but the valence electrons are farther from the nucleus.

18. Periodic Properties of the Elements Trends in First Ionization Energies Generally, as one goes across a row, it gets harder to remove an electron.  As you go from left to right, effective nuclear charge increases making it more difficult to pull away an electron.

19. Periodic Properties of the Elements Properties of Metal, Nonmetals, and Metalloids

20. Periodic Properties of the Elements Metals versus Nonmetals Differences between metals and nonmetals tend to revolve around these properties.

21. Periodic Properties of the Elements Metals versus Nonmetals Metals tend to form cations. Nonmetals tend to form anions.

22. Periodic Properties of the Elements Metals Tend to be lustrous, malleable, ductile, and good conductors of heat and electricity.

23. Periodic Properties of the Elements Metals Compounds formed between metals and nonmetals tend to be ionic. Metal oxides tend to be basic.

24. Periodic Properties of the Elements Nonmetals Dull, brittle substances that are poor conductors of heat and electricity. Tend to gain electrons in reactions with metals to acquire noble gas configuration.

25. Periodic Properties of the Elements Nonmetals Substances containing only nonmetals are molecular compounds. Most nonmetal oxides are acidic.

26. Periodic Properties of the Elements Metalloids Have some characteristics of metals, some of nonmetals. For instance, silicon looks shiny, but is brittle and fairly poor conductor.