1. Periodicity
Periodic Table Trends

2. patterns in e- config = patterns in properties= Periodic Trends.

3. 3 factors that effect Periodic Trends

4. 1. Energy level (front of first flap)
(on back of flap)
Rings/orbits/ shells: “how far out the e- cloud spans”
More E levels= valence e- further away from nucleus

5. 1. Energy level (draw under flap)

6. (on back of sheet) Who has more Energy Levels?
Ca or Ge
Al or Ba
Fr or Cl

7. (2nd flap front) 2. Nuclear Charge (# protons)
(back)
How strong is the nucleus.
The more p+ the greater the charge, the stronger the pull on the e- , which pulls them in closer & makes the atom smaller!!
Ie. More p+ = greater charge= e- pulled closer

8. (under) 2. Nuclear Charge (# protons)

9. (behind) Nuclear Charge- Who has more?
Na or Rb
Ca or Se
S or Mg
Li or O

10. (3rd flap) 3. Shielding effect
Nuclear charge
Inner e-
BLOCKS +
Valence e- from the
nuclear charge( p+)
b/c  E Level
(back)

11. (under) 3. Shielding effect

12. (back) Who has more shielding effect?
Na or Rb
Sn or C
Br or F

13. 4. Atomic Radius

14. (back flap for atomic radius)
Top of a group
No  in E level
 nuclear charge
=  p+ = stronger nucleus = valence e- are pulled closer +
E level

15. Atomic Radius ( under flap)
Fatty Fatty Francium!!!

16. Atomic Radius

17. Which atom is bigger & Why?
Li or Cs
Ga or B
O or C
Be or Ba
Si or S

18. (front) 5. Ionization Energy (IE)

19. Ionization Energy- energy needed to remove 1 e-
(back)
Ionization Energy- energy needed to remove
1 e-
higher IE
Top of a group
Closer to being noble gas = more E (harder)
to remove e-
Bigger = valence e- farther away=
less E (easier) to remove e-
lower IE

20. Ionization Energy
Measured in kJ/mole Ex: It takes 520 kJ to ionize 1 mole of Li

22. Which atom has larger (1st ) Ionization Energy ?
1. Na or S 2. Mg or Ba 3. Ga or Br 4. P or Bi

23. 2nd , 3rd ….Ionization Energies
The 1st electron is the easiest to remove
It take more energy to remove a 2nd electron than it did the 1st and so forth

24. (front) 6. Electronegativity
(back)
Ability to attract e- into a chemical bond
Like tug of war

25. Electronegativity higher Electroneg.
Top of a group
More E level & more e- = less likely to want more e-
The More Valence e- you have the closer you already are to being a noble gas.
Fluorine is the most Electronegative element
Lower
electroneg

26. Does NOT include the Nobel Gases

27. Which atom has higher Electronegativity?
Na or Mg
K or Br
F or Br
Ca or Ga
Li or S
Br or As

28. 7. Octet Rule = 8 (valence e-)
(back)
Gain, lose, or share e- to be STABLE
like Noble gases s2p6
**Exception energy level 1
Hydrogen only wants 1 more e- to be like He (already stable)

29. Ions: atoms trying to obey the octet rule will…
Gain or Lose e- based
on what's EASIER
Cation (+) loses e- = positive ion
Anion (-)
gains e- = negative ion
Group
must
Charge 1
loses 1 e- 1+ 2
Loses 2 e- 2+ 13
Loses 3e- 3+
Group
must
charge 15
Add 3 e-
3 - 16
Add 2 e-
2 - 17
Add 1e-
1 -

30. Metal ION Size 1. Lose valence e- , lose E level
2. Stronger nuclear charge
= becomes smaller

31. Metal ION Size
Atom
Losing e-
Ion
Lost E level

32. Non-Metal ION Size Gain valence e- Weaker nuclear charge
= become BIGGER

33. Non-Metal ION Size
Ion
add e-
Atom
Same #p+ BUT more e-

34. Metal
NonMetal

35. Which ion in each, is smaller?
1. Al3+ or P3- 2. K+ or Cs+ 3. O2- or Te2-

36. Summary Ionization energy decreases Electronegativity decreases
Nuclear charge increases
Atomic radius increases
Shielding increases
Shielding is constant
Atomic Radius decreases
Ionization energy increases
Electronegativity increases
Nuclear charge increases

37. Ranking Elements by Atomic Size
Warm Up 3.1
Ranking Elements by Atomic Size
PROBLEM:
Using only the periodic table (not Figure 8.15), rank each set of main group elements in order of decreasing atomic size:
(a) Ca, Mg, Sr
(b) K, Ga, Ca
(c) Br, Rb, Kr
(d) Sr, Ca, Rb
PLAN:
Elements in the same group increase in size and you go down; elements decrease in size as you go across a period.
SOLUTION:
These elements are in Group 2A(2).
(a) Sr > Ca > Mg
These elements are in Period 4.
(b) K > Ca > Ga
Rb has a higher energy level and is far to the left. Br is to the left of Kr.
(c) Rb > Br > Kr
Ca is one energy level smaller than Rb and Sr. Rb is to the left of Sr.
(d) Rb > Sr > Ca

38. (a) Kr, He, Ar (b) Sb, Te, Sn (c) K, Ca, Rb (d) I, Xe, Cs
Warm Up 3.2
Ranking Elements by First Ionization Energy
PROBLEM:
Using the periodic table only, rank the elements in each of the following sets in order of decreasing IE1:
(a) Kr, He, Ar
(b) Sb, Te, Sn
(c) K, Ca, Rb
(d) I, Xe, Cs
PLAN:
IE decreases as you proceed down in a group; IE increases as you go across a period.
SOLUTION:
(a) He > Ar > Kr
Group 8A(18) - IE decreases down a group.
(b) Te > Sb > Sn
Period 5 elements - IE increases across a period.
(c) Ca > K > Rb
Ca is to the right of K; Rb is below K.
(d) Xe > I > Cs
I is to the left of Xe; Cs is further to the left and down one period.