1. LT2: Periodic Table Basics

2. How is the periodic table arranged?
Mendeleev first arranged it by average atomic mass.
Mosley then arranged it by increasing ATOMIC NUMBER

3. Columns= Families or Groups
Rows= Periods
The transition metals are not considered a “family”

4. Blue= METALS Yellow= NONMETALS Pink= Semimetals (Metalloids)

5. Transition Metals G8: Noble Gases G7: Halogens G3: Boron Group
G1: Alkali Metals
G4:Carbon Group
G5:Nitrogen
G6: Oxygen
G2: Alkaline Earth Metals
Transition Metals
Inner Transition Metals

6. Compare electron configurations down a group and across a period
Compare electron configurations down a group and across a period. What do they have in common?
Group Ca Sr
Common:
Period Ga

8. Don’t forget the blocks on the periodic table!

9. FLIP TO THE BACK OF YOUR PAGE FOR NOTES ON…
LABEL YOUR PAPER LIKE THIS:
PROPERTIES OF METALS
PROPERTIES OF NONMETALS
PROPERTIES OF SEMIMETALS (METALLOIDS)
Additional Information about Specific Groups:

10. METALS PROPERTIES OF METALS DUCTILE MALLEABLE LUSTEROUS
SOLIDS AT ROOM TEMP
SMOOTH
CONDUCTORS

11. PROPERTIES OF NONMETALS
NOT CONDUCTORS
NOT MALLEABLE
NOT DUCTILE
NOT LUSTEROUS--DULL
BRITTLE SOLIDS OR GASES AT ROOM TEMPERATURE

12. PROPERTIE S OF SEMIMETALS (METALLOIDS)

13. ADDITIONAL INFORMATION ABOUT EACH GROUP…

14. ALKALI METALS GROUP 1 VALENCE ELECTRONS—1
MOST REACTIVE METALS ON THE TABLE

15. ALKALINE EARTH METALS GROUP 2 2 VALENCE ELECTRONS
2ND MOST REACTIVE METAL GROUP ON THE TABLE

16. HALOGENS
GROUP 7
7 VALENCE ELECTRONS
MOST REACTIVE GROUP ON THE TABLE

17. NOBLE (INERT) GASES GROUP 8 8 VALENCE ELECTRONS
DO NOT REACT (HARDLY EVER)

18. VALENCE NUMBER FOR EACH GROUP

19. LT3: Periodic Trends
Atomic Radius- half the distance between 2 adjacent nuclei.
Illustration

20. Reasoning
Period- As you move across a period valence electrons occupy the SAME ENERGY LEVEL. However, the pull from the nucleus increases as more protons are added pulling the electrons in DECREASING the size of the atom.
Group- As you move down a group the valence ENERGY LEVEL INCREASES which causes the atom to get larger.

21. Ionic Size- when atoms gain or lose electrons they become IONS
CATION
ANION
FROM A LOSS OF ELECTRONS= POSITIVE CHARGE
SMALLER THAN NEUTRAL ATOM
LOSE ENERGY LEVELS
DECREASE IN ELECTROSTATIC REPULSION
FROM A GAIN OF ELECTRONS= NEGATIVE CHARGE
LARGER THAN NEUTRAL ATOM
INCREASES THE ELECTROSTATIC REPULSION

22. IONIZATION ENERGY- ENERGY NEEDED TO REMOVE AN ELECTRON FROM AN ATOM
Illustration

23. Reasoning
Periods- As you move across the period, the atoms are getting smaller and closer to having a full valence shell (8 electrons) so it is HARDER or requires HIGHER Ionization Energy to remove electrons because atoms tend to keep their electrons.
Groups- As you move down a group, the atoms are getting larger so it is EASIER or requires LOWER Ionization Energy to steal electrons because the attraction between p+ and e- is decreasing.

24. Electronegativity- ability to attract electrons in a bond.
Most Electronegative
Illustration
Least Electronegative

25. Reasoning
Period- Across a period the elements are closer to having a full octet (8 valence electrons) so they attract electrons more to reach the full valence shell. (excluding the Noble Gases)
Group- Going down a group there is less attraction from inside the nucleus to outside on the valence shell due to a larger size which decreases the electronegativity down a group.

27. Practice
Which of the following is the smallest? Highest Ionization energy?
Cl, Se, Br
Which of the following is the largest? Highest Ionization energy?
P, S, Se
Which of the following is the largest atom? Smallest Ionization energy?
Sc, Y, La
Which of the following is the smallest? Highest electronegativity?
V, Cr, W

28. Practice Which of the following is the largest?
Te 2-, I1-, Xe
Which of the following is the smallest?
Li, Li1+, Na
Put these in order from largest to smallest electronegativity.
B, Na, K, Al

29. Successive Ionization Energy- What do you think this term means and why does it change like this?

30. Energy needed to remove successive electrons from an atom
Energy needed to remove successive electrons from an atom. (the first, the second, the third, etc.)
It changes based on valence electron number.