1. For Test #6: The Periodic Table

2. The Periodic Table
Dimitri Mendeleev – 1st to publish a periodic table.
2) The Periodic Law: When arranged by increasing atomic number, the elements display a regular and repeating pattern of chemical and physical properties.

4. Groups vs Periods
Groups – contain elements with similar chemical properties (vertical columns) because they all have the same number of valence (outer shell) electrons.
Periods – contains elements with the same number of occupied energy levels. Their chemical properties vary.
Note: Know special group names

5. Can YOU name the special groups?

6. Reading the Periodic Table: Classification
Classes of Elements
Nonmetals, Metals, Metalloids, Noble gases
Reading the Periodic Table: Classification

7. Phases of Elements Gases Liquids Most reactive nonmetal
Most Reactive Metal

8. 1) Which is the more reactive metal. A) Potassium or cesium
1) Which is the more reactive metal? A) Potassium or cesium? B) Calcium or barium? 2) Which is the more reactive nonmetal? A) Iodine or Chlorine? B) Carbon or Oxygen?

9. Reading the Periodic Table: Classification
Can you name the symbols for the gases?
Nonmetals, Metals, Metalloids, Noble gases
Reading the Periodic Table: Classification

10. Reading the Periodic Table: Classification
Can you name the metalloids?
Nonmetals, Metals, Metalloids, Noble gases
Reading the Periodic Table: Classification

11. Reading the Periodic Table: Classification
Can you name the 2 liquid elements?
Nonmetals, Metals, Metalloids, Noble gases
Reading the Periodic Table: Classification

12. Atomic Radius
Atomic Radius is the distance from the center of an atom to its outermost electron shell.
Values on Table S
Units are picometers (pm)

13. Atomic Radius Trends
Atomic Radius increases as you move down a group because there are more shells of electrons.
Atomic Radius decreases as you move to the right across a period because the nuclear charge increases & pulls the electrons in closer to the nucleus.
Smaller
Bigger

14. Ionization Energy
Ionization energy is the amount of energy needed to pull an electron from an gaseous atom.
Values on Table S
Units are kilojoules per mole (kJ/mol)
It takes more energy to pull electrons off smaller atoms.
Trends are opposite of that for atomic radius.

15. Ionization Energy Trends
1) Ionization Energy decreases as you move down a group.
2) Ionization Energy increases as you move to the right across a period.
Smaller
Bigger

16. Ionization Energy Trends

17. Electronegativity
Electronegativity measures how much an atom attracts shared electrons in a chemical bond (“electron attraction”)
Linus Pauling – created the electronegativity scale with fluorine having the largest attraction for electrons and it is assigned the biggest value of 4.0
Values on Table S (no units)

18. Electronegativity Trends
Same as ionization energy
Reason: If it takes a lot of energy to remove an electron, the atom must have a big attraction for the electron.
Bigger
Smaller

19. Summary Nuclear Charge is constant Ionization energy decreases
Electronegativity decreases
Atomic Radius increases
Atomic Radius decreases
Nuclear Charge increases
Electronegativity increases
Ionization Energy increases

20. Octet Rule
Atoms will gain, lose, or share valence electrons with other atoms in order to obtain an octet (8 valence electrons).
Hydrogen & Helium are the only exceptions – they want 2 valence electrons.
Recall: Atoms are neutral. Why? _________________
An ion is the charged particle formed when neutral atoms lose or gain electrons.
If an atom gains electrons, it becomes a ____________ charged ion.
If an atom loses electrons, it becomes a ____________ charged ion.

21. Metal Ions
Metal tends to give up electrons and form smaller sized ions that are positively charged.
Atom Ion

22. Nonmetal Ions
Nonmetals tend to gain electrons and form larger sized ions that are negatively charged.
Atom Ion

23. Why?
Metals generally have 1, 2, or 3 valence electrons. For metals it is easier to lose those than gain 5,6,or 7 additional electrons.
Nonmetals generally have 5, 6, or 7 valence electrons. For nonmetals it is easier to gain 1, 2, or 3 more electrons than to lose 5, 6, or 7 electrons.

24. Allotropes

25. Diatomic vs Monoatomic Elements

26. Ground State vs Excited State Special Group Names Isotopes
Don’t Forget
How to find #p, #e, #n
Ground State vs Excited State
Special Group Names
Isotopes