1. Periodic Trends Barbara A. Gage PGCC CHM 1010

2. Atomic Properties Depend on: – Number of protons – attractive nuclear force – Number of electrons – shielding effect of electron shells – Distance of electrons from nucleus – distance decreases nuclear force Barbara A. Gage PGCC CHM 1010

3. Atomic Properties Atomic radius Barbara A. Gage PGCC CHM 1010 Metallic and covalent radii.

4. Atomic Properties Click on image above to go to the Periodic Trends excelet Barbara A. Gage PGCC CHM 1010

6. Ranking Elements by Atomic Size SOLUTION: PROBLEM:Using the periodic table, rank each set of main group elements in order of decreasing atomic size: (a) Ca, Mg, Sr(b) K, Ga, Ca(c) Br, Rb, Kr(d) Sr, Ca, Rb Elements in the same group increase in size and you go down; elements decrease in size as you go across a period. (a) Sr > Ca > MgThese elements are in Group 2A(2). (b) K > Ca > GaThese elements are in Period 4. (c) Rb > Br > KrRb has a higher energy level and is far to the left. Br is to the left of Kr. (d) Rb > Sr > CaCa is one energy level smaller than Rb and Sr. Rb is to the left of Sr.

7. Atomic Properties Ionization energy energy required to remove an electron from a neutral, gaseous atom Cl (g)  Cl 1+ + e - K (g)  K 1+ + e - Barbara A. Gage PGCC CHM 1010

8. First ionization energies of the main-group elements.

9. Barbara A. Gage PGCC CHM 1010 Ranking Elements by First Ionization Energy SOLUTION: PROBLEM:Using the periodic table only, rank the elements in each of the following sets in order of decreasing IE 1 : (a) Kr, He, Ar(b) Sb, Te, Sn(c) K, Ca, Rb(d) I, Xe, Cs IE decreases as you proceed down in a group; IE increases as you go across a period. (a) He > Ar > Kr (b) Te > Sb > Sn (c) Ca > K > Rb (d) Xe > I > Cs Group 8A(18) - IE decreases down a group. Period 5 elements - IE increases across a period. Ca is to the right of K; Rb is below K. I is to the left of Xe; Cs is furtther to the left and down one period.

10. Barbara A. Gage PGCC CHM 1010

12. Atomic Properties Electron affinity energy change when an electron is added to a neutral atom to form a negative ion Cl + e -  Cl - K + e -  K 1- Barbara A. Gage PGCC CHM 1010

13. Electron affinities of the main-group elements.

14. Barbara A. Gage PGCC CHM 1010 Figure 8.15 and 8.16 Trends in four atomic properties.

15. Ionic Properties Ionic radius radius of the ionic form of an atom Barbara A. Gage PGCC CHM 1010

16. Ionic vs. atomic radii Cations

17. Barbara A. Gage PGCC CHM 1010 Ionic vs. atomic radii Anions

18. Barbara A. Gage PGCC CHM 1010 Ranking Ions by Size SOLUTION: PROBLEM:Rank each set of ions in order of decreasing size, and explain your ranking: (a) Ca 2+, Sr 2+, Mg 2+ (b) K +, S 2-, Cl - (c) Au +, Au 3+ Compare positions in the periodic table, formation of positive and negative ions and changes in size due to gain or loss of electrons. (a) Sr 2+ > Ca 2+ > Mg 2+ (b) S 2- > Cl - > K + These are members of the same Group (2A/2) and therefore decrease in size going up the group. The ions are isoelectronic; S 2- has the smallest Z eff and therefore is the largest while K + is a cation with a large Z eff and is the smallest. (c) Au + > Au 3+ The higher the + charge, the smaller the ion.