1. Chapter14: Periodic Trends
Modern Chemistry; Holt, Rinehart, & Winston

2. Dmitri Mendeleev (1834-1907) Russian chemist
Arranged his periodic table according to atomic mass so that elements with similar properties were in the same group
Predicted the properties of elements that had not yet been discovered using his periodic table

3. Henry Moseley (1887-1915) English chemist
Proved Mendeleev’s arrangement of the periodic table to be correct – only, the periodic table was arranged according to atomic number, not atomic mass

4. The Periodic Law
States that when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern

5. Distance between nuclei
Atomic Radii
Atomic radius – the distance between the center of the nucleus and the outer most energy level
Atomic Radius
Distance between nuclei

6. Atomic Radius Decreases across a row
Higher effective nuclear charge – more protons being added to the nucleus at the same time electrons are being added to the same energy level

7. Why?
Protons are added to the nucleus moving across a period from left to right
This increases the charge of the nucleus (effective nuclear charge – Zeff)
As a result, it compacts the atom

8. Group Trends Increase down a group
Although more protons are being added to the nucleus going down a period, energy levels are also being added. The inner energy levels create a shielding effect from the attractive nuclear forces.

9. Why?
The addition of shells increases the electrons’ distance from the nucleus and the size of the atom
This makes the atom larger
n=3
n=2
n=1

10. Ionization Energy
The energy required to remove one electron from a neutral atom of an element creating an ion

11. Period Trends Increase across a row Why?
Zeff increases across the period
There is stronger attraction between the positive and negative particles more difficult to remove them.

12. Group Trends Decrease down the column Why?
Electrons are far away from positive nucleus, making it easier to remove
Electrons have higher PE as the energy level increases
Shielding effect – outer electrons are shielded from the nuclear charge attractive forces by the electrons in the inner energy shells

13. Electronegativity
A measure of the ability of an atom in a chemical compound to attract a bonding pair of electrons
A MEASURE OF GREEDINESS!

14. Trends Increase across a period Decrease down a group
EXCEPTIONS: NOBLE GAS (GROUP 18). They do not have an electronegativity value because they do not form chemical compounds.