1. Ch 6: The Periodic Table and Periodic Law
Honors Chemistry

2. Section 6.1 Development of the Modern Periodic Table
Chemist’s first began to organize known elements in the 1700’s. Many have made contributions over the years.
Dmitri Mendeleev, a Russian
chemist developed the first Periodic
Table of elements in 1869.
There were about 60 known
Elements at this time.

3. “I began to look about and write down the elements with their atomic weights and typical properties, analogous elements and like atomic weights on separate cards, and this soon convinced me that the properties of elements are in periodic dependence upon their atomic weights.”  --Mendeleev, Principles of Chemistry, 1905, Vol. II

4. Mendeleev’s Predictions
When creating his periodic table, Mendeleev left blank spaces for elements that had not yet been discovered.
Using periodic properties of the other elements, he correctly predicted the properties of scandium, gallium, and germanium.

5. Mendeleev’s Predictions…
Mendeleev predicted 5 elements.
Within 15 yrs, 3 of the 5 elements had been discovered!!!

6. Our Modern Periodic Table…
Moseley rearranged the table by increasing atomic number, and resulted in a clear periodic pattern – our modern periodic table.
Periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number is called periodic law.
Interactive Periodic Table

7. Elements in groups 1,2, and possess a wide variety of chemical and physical properties and are called the representative elements.
Elements in groups 3-12 are known as the transition metals.
Elements are classified as metals, non-metals, and metalloids.

8. Metals…
Metals are elements that are generally shiny when smooth and clean, solid at room temperature, good conductors of heat and electricity, malleable, and ductile.
Alkali metals are all the elements in group 1 except hydrogen, and are very reactive.
Alkaline earth metals are in group 2, and are also highly reactive.

9. Metals…
The transition elements are divided into transition metals and inner transition metals.
The two sets of inner transition metals are called the lanthanide series and actinide series and are located at the bottom of the periodic table.

10. Group 17 is composed of highly reactive elements called halogens.
Nonmetals…
Non-metals are elements that are generally gases or brittle, dull-looking solids, and poor conductors of heat and electricity.
Group 17 is composed of highly reactive elements called halogens.
Group 18 gases are extremely unreactive and commonly called noble gases.

11. Metalloids…
Metalloids have physical and chemical properties of both metals and non-metals, such as silicon and germanium.
The metalloids form a staircase that separates the metals from the nonmetals, with the exception of aluminum which is a metal.

13. Section 6.2 Classification of the Elements
Recall electrons in the highest principal energy level are called valence electrons.
Groups can help determine how many valence electrons an atom has.

14. Remember…
Group 1 elements have 1 valence e- and group 2 elements have 2 valence e-.
The number of valence electrons for elements in groups is ten less than their group number.
Remember, the maximum number of valence e- is 8.
The Noble Gases are the only elements that have completely filled orbitals. He has 2 valence e- and the other noble gases all have 8 valence e-.

15. Electron Dot Structures…

16. Atomic size is a periodic trend influenced by electron arrangement.
Section 6.3 Periodic Trends
Atomic Radius…
Atomic size is a periodic trend influenced by electron arrangement.
Atomic radius is half the distance between adjacent nuclei.

17. Atomic Radius Trends…
There is a general decrease in atomic radius from left to right because the nucleus pulls the electrons in tighter.
Atomic radius generally increases as you move down a group, since an energy level is being added.

18. Ionic Radius…
An ion is an atom or bonded group of atoms with a positive or negative charge.
When atoms lose electrons and form positively charged ions, they always become smaller.
When atoms gain electrons and form negatively charged ions, they always become larger.

19. Ionic Radius Trends…
The ionic radii of both positive ions and negative ions generally decrease from left to right.
Both positive and negative ions increase in size moving down a group.

20. Ionic Radius Trends…

21. In terms of IE, electrons are removed one at a time.
Ionization Energy…
Ionization energy is defined as the energy required to remove an electron from a gaseous atom.
In terms of IE, electrons are removed one at a time.
The energy required to remove the first electron is called the first ionization energy.

22. Ionization Energy…

23. Ionization Energy…
What trend do you see each time an electron is removed?

24. Ionization Energy…
First ionization energy increases from left to right across a period because metals tend to lose their valence and nonmetals want to keep their valence.
First ionization energy decreases down a group because atomic size increases and less energy is required to remove an electron farther from the nucleus.

25. Ionization Energy…

26. Ionization Energy…
The octet rule states that atoms tend to gain, lose or share electrons in order to acquire a full set of eight valence electrons.
The octet rule is useful for predicting what types of ions an element is likely to form.

27. Electronegativity…
The electronegativity of an element indicates its relative ability to attract electrons in a chemical bond.
Electronegativity decreases down a group and increases left to right across a period.
Metals have low electronegativites and nonmetals have high electronegativites.

28. Electronegativity…
Why don’t the noble gases have EN values listed?