1. Chapter 5 The Periodic Law

3. History of the Periodic Table
1869 – Dmitri Mendeleev published his periodic table. He had arranged it by grouping together the elements that had
similar properties and by increasing atomic masses. His periodic table left empty spaces for new elements that would be discovered.

4. Mendeleev’s List of elements in Russian Circa 1869

5. Periodic Table circa 1898

6. History of the Periodic Table
1911 – Henry Moseley (a student of Ernest Rutherford) rearranged a few elements on the periodic table so that elements were
arranged by increasing atomic number rather than by atomic mass.

8. History of the Periodic Table
1944 – Glenn T. Seaborg rearranged the periodic table to make it look like it does today. He moved the Actinide Series and
the Lanthanide Series elements to the bottom of the periodic table.

9. Modern Periodic Table

10. The Periodic Law
The physical and chemical properties of the elements are periodic functions of their atomic numbers

11. What are the trends among the elements for atomic radius?
The atomic radius of an element is one half of the distance between the nuclei of two atoms of the same element when the atoms are joined.
Atomic radii are often measured in picometers (pm).
1. Interpret Diagrams Which element in the figure above has the largest atomic radius?

12. Summary: trends in atomic radius
6. Compare If a halogen and an alkali metal are in the same period, which element will have the larger atomic radius?

13. Group trends H Li
Atomic radius increase as you move down because each atom has another energy level, so the atoms get bigger. Na K Rb

14. Periodic Trends
As you go across a period, the radius gets smaller.
Electrons are in same energy level.
Increasing number of positive protons within the nuclei pull on the valence electrons. Na Mg Al Si P S Cl Ar

15. Learning Check According to their positions on the
Periodic Table, which of the
following neutral atoms has the
largest atomic radius? A
Beryllium B
Magnesium C
Calcium D
Strontium

16. CATIONS Cations are positively charged ions
Cations form by losing electrons.
Cations are smaller than the atom they come from.
Metals form cations.
Cations of representative elements have noble gas configuration.

17. ANIONS Anions are negatively charged ions
Anions form by gaining electrons.
Anions are bigger than the atom they come from.
Nonmetals form anions.
Anions of ‘main’ groups elements have noble gas configuration.

18. Group trends Li1+ Na1+ K1+ Rb1+ Cs1+ Adding energy level
Ions get bigger as you go down.
Na1+
K1+
Rb1+
Cs1+

19. Ionic Radius
A greater number of protons will cause an ion to become smaller due to attractive forces between the nucleus and the valence electrons
greater number of electrons will cause an ion to become larger due to electron repulsion.
N3-
O2-
F1-
Li1+
B3+
Be2+
C4+

20. Period trends in ionic radius

21. Learning Check
2 Which of the following statements is true about the trend for ionic radii?
A When electrons are lost forming positive ions, the ionic radius is larger than its corresponding neutral atom.
B When electrons are lost forming positive ions, the ionic radius is smaller than its corresponding neutral atom.
C When electrons are gained forming positive ions, the ionic radius is larger than its corresponding neutral atom.
D When electrons are gained forming positive ions, the ionic radius is smaller than it’s corresponding neutral atom.

22. What are the trends among the elements for ionization energy?
The energy required to remove an electron from an atom is called ionization energy.
This energy is measured when an element is in its gaseous state.
The energy required to remove the first electron from an atom is called the first ionization energy.

23. Ionization Energy Decreases as we move down the periodic table.
The outermost energy level is farther from the nucleus. Therefore, it is easier to remove an electron.

24. Ionization Energy Increases as you move across the periodic table
The nuclear charge(atomic #) increases across the period because you have more protons and your atomic radius is getting smaller. As a result, there is an increase in the attraction of the nucleus for an electron.
The outermost electrons are just a little closer to the nucleus and so they are harder to remove.

25. Summary: trends in ionization energy
11. Compare Which element would have a larger first ionization energy: an alkali metal in Period 2 or an alkali metal in Period 4?

26. Learning Check
3 Which element in group 17 (group 7A), the halogens, has the highest ionization energy?
A Fluorine
B Chlorine
C Bromine
D Iodine

27. Learning Check
4 Based on the periodic trend for ionization energy, which element in Period 3 has the greatest tendency to lose an electron?
A Sodium
B Aluminum
C Phosphorus
D Argon

28. Atoms with large ionization energy values are
A. more likely to form positive ions
B. less likely to form positive ions
C. most likely to lose their outer electrons
D. lacking valence electrons

29. Electronegativity
The tendency for an atom to attract electrons to itself when it is chemically combined with another element.
High electronegativity means it pulls the electron toward it.

30. Electronegativity
The further down a group, the farther the electron is away, and the more electrons an atom has.
More willing to share.
Low electronegativity.

31. Electronegativity
Metals let their electrons go easily resulting in a low electronegativity
Nonmetals want more electrons and take them away from others resulting in a high electronegativity.

32. Electronegativity Values for Selected Elements
H 2.1 He
Li 1.0
Be 1.5
B 2.0
C 2.5
N 3.0
O 3.5
F 4.0 Ne
Na 0.9
Mg 1.2
Al 1.5
Si 1.8
P 2.1
S 2.5
Cl 3.0 Ar
K 0.8
Ca 1.0
Ga 1.6
Ge 1.8
As 2.0
Se 2.4
Br 2.8 Kr
Rb 0.8
Sr 1.0
In 1.7
Sn 1.8
Sb 1.9
Te 2.1
I 2.5 Xe
Cs 0.7
Ba 0.9
Tl 1.8
Pb 1.9
Bi 1.9

33. Learning Check
Which diagram below correctly depicts the increase in electronegativity across periods and down groups?

34. Summary: periodic trends
15. Explain Periodic Trends In general, how can the periodic trends exhibited by the elements be explained?

35. Reactivity
Reactivity increases as you go down the columns of metallic elements.
Reactivity decreases as you go down the columns of non-metallic elements.
Flourine is the most reactive nonmetal

36. Valence Electrons
The electrons available to be lost, gained, or shared in the formation of compounds.
The electrons in the highest energy level
Label valence electrons on periodic table

37. Extra Slides

38. 1+ 2+ 3+ 3- 2- 1- H He 4- 4+ Li Be B C N O F Ne Na Mg Al Si K Ca Ga Rb1+ H He 2+ 4- 4+ 3+ 3- 2- 1- Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Ga Ge As Se Br Kr Rb Sr In Sn Sb Te I Xe Cs Ba Tl Pb Bi Po At Rn Fr Ra