1. Warm-Up 10/5/2016 Place the following in increasing atomic size
1. N, Sr, I, Be 2. Li, Hg, Cs, F 3. Fr, Ga, K, Br

2. Write down the electronic configuration of the following elements in long hand formV Zr S Cr I

3. Ionization Energy is the energy needed to remove an electron
1st Ionization Energy: energy required to remove the outermost electron

4. Ionization Energy depends on: a. Distance an electron is from nucleus
The further the electron is away, the easier it is to remove
Begin 7th

5. Ionization Energy Continued
Nuclear charge: refers to the attraction between the nucleus and electrons
A.K.A the Shielding Effect
The further away the electrons are, the less the attraction is between the nucleus and electrons
Begin 5th

6. Trends with Ionization Energy
The first Ionization energy decreases as you move down a group
The first Ionization energy increases as you move across the periodic table

7. Ionization Energy Problems
Arrange the following in terms of increasing ionization energy:
A. Li, K, Cs, Na
B. Ca, Zn, Ge, Br
C. In, B, Al, Ga
D. Mg, P, Na, Cl
Begin 5th

8. Practice
Place the following in increasing Ionization Energy
Rb, Mo, Br, Fr
Cs, O, C, Be, F
Au, Hf, Ba, Po, At

9. Electronegativity is the tendency of elements to attract electrons
Nonmetals attract electrons more than metals 9

10. Electronegativity
Electronegativity is really the strength of an element to “steal and keep” electrons 10

11. Electronegativity is measured on a scale from 0 to 4
The most electronegative element is given a value of 4.0
Begin 5th, & 7th 11

12. Electronegativity Continued
Fluorine is the most electronegative and given a value of 4.0
O = 3.5 Cl = 3.0
S = 2.5 H = 2.1
Li = 1.0 Na = 0.9 12

13. Effects of Electronegativity
The more electronegative an element is, the more non-metallic it is

14. Electronegativity
The strength of other elements to steal electrons is compared to the most electronegative element
Begin 4th 14

15. Trends in Electronegativity
Electronegativity increases as you move across the table
Electronegativity decreases as you move down the table
Electronegativity can be used to predict which type of bond that atoms will form

16. Arrange the following in terms of increasing electronegativity:
Problems
Arrange the following in terms of increasing electronegativity:
a. K, As, Cr, Zn
b. Sr, Y, Ag, I
c. F, O, N, Li
d. Ga, Ca, Fe, K
e. F, At, Cl, Br

17. Electron Affinity
Electron affinity is defined as the neutral atom's likelihood of gaining an electron.

18. Electron Affinity of Metals
Metals have a lower EA than nonmetals because they give up electrons to have a stable octet.

19. Electron Affinity of Nonmetals
Nonmetals like to gain electrons to form anions to have a fully stable octet.

20. Electron Affinity Trend
As the you go down the periodic table it decreases
As you go across the periodic table it increases

21. Na, Rb, Al, P, Cl Fr, K, Na, Cs K, Mg, Si, S Cl, At, I, F
Review Questions
Place the following in increasing Electron Affinity
Na, Rb, Al, P, Cl
Fr, K, Na, Cs
K, Mg, Si, S
Cl, At, I, F

22. Begin 3rd 3-27-01 , 4th Trends with Ionic Size What are Ions?
Ions form when electrons are gained or lost
Metals lose electrons (called Cations) ; non-metals gain electrons( called Anions)
Begin 3rd , 4th 22

23. The metal ions are usually smaller than the metal atoms
Trends with Ionic Size
The metal ions are usually smaller than the metal atoms
The non-metal ions are larger than the non-metal atoms 23

24. The size of the ions increase going down the periodic table
Ionic Size Trend
The size of the ions increase going down the periodic table
The size of cations decreases as you move across the table
The size of anions decreases as you move across the table 24

25. Cations are smaller than their corresponding atoms
Ionic Size Continued
Cations are smaller than their corresponding atoms
Na atom is larger than Na+
Anions are larger than their corresponding atoms
F atom is smaller than F-
Begin 5th , 7th 25

26. Begin 1st 2-26-2000 Ionic Size Problems
State which particle would have the largest radius in each pair:
a. Ca, Ca+2
b. Br, Br -
c. Cl -, Br -,
d. Na+, K+
Begin 1st 26

27. Place the following in increasing electronegativity: Fr, S, Na, Cl
Practice
Place the following in increasing electronegativity:
Fr, S, Na, Cl
Place the following in increasing ionization energy:
Cl , As, Ca, Ni
Place the following in increasing atomic radius:
I, Rb, Cs, Ru

29. For the following pairs of atoms, tell which one of each pair has the largest ionic radius
a. Al, B b. S, O c. Br, Cl d. Na, Al e. O, F

30. For the following pairs of atoms, tell which one of each pair has the largest ionic radius
a. Al b. S c. Br d. Na e. O

31. Indicate which element of the following pairs is the most electronegative.
a. calcium, gallium b. lithium, oxygen c. chlorine, sulfur d. bromine, arsenic

32. a. gallium b. oxygen c. chlorine d. bromine
Indicate which element of the following pairs is the most electronegative.
a. gallium b. oxygen c. chlorine d. bromine