Chapter 14 Chemical Periodicity

The Periodic Table Revisited What did they do: 1. J.W. Doberiener 2. J.A.R. Newlands 3. Dmitri Mendeleev

4. Henry Mosely Periodic Law: The chemical and physical properties of the elements are periodic functions of their atomic number. (Not all elements follow this)

Review Parts of Periodic Table

Trends 1. Atomic radius a. Monatomic atoms – distance from the nucleus to the outermost electron of an atom b. Diatomic – ½ the distance from one adjacent atom to another

Atomic number is directly proportional to the atomic radius c. Rules: Group or family Atomic number is directly proportional to the atomic radius d. Ex. Which has a larger atomic radius? Li Cs 2s1 6s1

e. Rules for: Series or period atomic number is a indirect proportion to the atomic radius f. Ex. Which has a larger atomic radius? Li or Ne

Li Ne 2s1 2p6 What could you look at if they are in the same row Li Ne 2s1 2p6 What could you look at if they are in the same row? # protons 3 p+ 10p+ More protons has a stronger nuclear attraction (pulls in close)

S or Po Mg or Cl Li or Rn g. Special cases 1. Out of the following pairs state which has a larger atomic radius. S or Po Mg or Cl Li or Rn

Summary 2. Look for same configuration, more energy means it is larger 1. Start with the last electron configuration 2. Look for same configuration, more energy means it is larger 3. Look for same last energy level, more protons makes it smaller 4. Look for adjoining element

2. Ionization Energy (IE) a. Energy needed to remove the outermost electron from an atom in its gaseous state b. Unit: kJ/mole

c. Rules: Group or family 1 c. Rules: Group or family 1. Atomic number is indirectly proportional to the IE 2. Increasing atomic number leads to a lower IE

Li Cs Li Cs 2s1 6s1 3. Ex. Which would have a higher IE? (high IE) (low IE) electrons further away, so it’s easier to remove

1. Atomic number is directly proportional to the IE d. Rules: Series or Periods 1. Atomic number is directly proportional to the IE 2. Increasing atomic number equals higher IE

(stronger nuclear attraction) higher 3. Ex. Which would be higher Li or Ne? Li Ne 2s1 2p6 (same energy level) 3 protons 10 protons (stronger nuclear attraction) higher

4. Which is higher? Mg or P Na or Cl

5. Ex. Rank in terms of IE from high to low Sr, C, F

Which has higher IE, N or O? 6. Special cases: Which has higher IE, N or O? **** ONLY TAKE BALANCE INTO CONSIDERATION WHEN DEALING WITH ADJACENT ELEMENTS.

3. Balance of adjacent elements Rank from low to high IE Ca Sr As Se Summary Look at: 1. Energy levels 2. How many protons 3. Balance of adjacent elements Rank from low to high IE Ca Sr As Se

3. Second ionization energy, IE2 a. The energy needed to remove the second outermost electron AFTER the outermost has already been removed. b. What IE1 looks like: Na + IE1  Na+ + e- 11 p+ 11 p+ 11 e- 10 e_

c. What will IE2 look like: Na+ + IE2  Na+2 + e- 11 p+ 10 e- 11 p+ 9 e-

4. Third ionization energy a. Energy needed to remove the third outermost electron after the two outermost electrons have been removed. b. What it looks like: Na+2 + IE3  11p 11p 9e 8e

c. IE3 is always applied to a (+2) ion. d. IE2 is always applied to a (+1) ion. e. How would you rank IE, IE2, IE3? (high to low) IE3 > IE2 > IE

f. Examples: Be, C or F Be+ C+ F+ 2s1 2p1 2p4 4p+ 6p+ 9p+ 1. Which of the following elements would have the higher IE2? Be, C or F Be+ C+ F+ 2s1 2p1 2p4 4p+ 6p+ 9p+ lowest highest

2. Which of these would have the highest IE3 ? Be, C, F Be+2 C+2 F+2 1s2 2s2 2p3 6 p+ 9p+ Highest lowest (closest to nucleus)

3. Rank the following elements in terms of IE2 from high to low O+ S+ F+

1. Look at energy levels (how close to the nucleus) g. Summary of IE 1. Look at energy levels (how close to the nucleus) 2. Consider how many protons 3. Consider adjacent elements (use balance vs unbalance)

4. Ex. Rank in terms of IE from high to low: Ca, Sr, As, Se

b. Which is more reactive? Li, Na, K 5. Chemical activity a. An elements ability to replace another element in a chemical compound b. Which is more reactive? Li, Na, K

a. Group or family – activity increases with increasing atomic number c. Rules 1. Metals a. Group or family – activity increases with increasing atomic number b. Series or Period – activity decreases with increasing atomic number c. Ex. Rank activity from low to high Be, Ca, Ba low high

2. Nonmetals a. Group or family- activity decreases down the group b. Series or period- activity increases as atomic number increases c. Rank from low to high Se, S,Cl

d. What is the most active metal? e. What is the most active nonmetal? 6. Ionic radius a. the distance from the nucleus to the outermost electron of a naturally occurring ion

b. Want to achieve the electron configuration of a noble gas c. Examples: 1. Which would have a larger ionic radius? Sr, Mg, Al

2. Rank in terms of larger ionic radius large to small: N, S, F, Br

d. Cations are SMALLER than the atom from which they naturally come. e d. Cations are SMALLER than the atom from which they naturally come. e. Anions are LARGER than the atom from which they naturally come. f. Cations are positive. g. Anion are negative charge.

7.Electron Affinity b. X + electron + EA  X− a. The energy absorbed or released when an atom gains an electron b. X + electron + EA  X− c. Higher energy less stable or balance d. Lower energy more stable or balance

Noble gas configuration will be the lowest e. Ex. Which will have the highest EA B N F Before 2p1 __ __ __ 2p3 __ __ __ 2p5 __ __ __ After 2p2 __ __ __ 2p4 __ __ __ 2p6 __ __ __ Noble gas configuration will be the lowest

f. Equations using EA or IE 1. Show Mg losing an electron Mg + 738 kJ  Mg+ +e− State whether it is endothermic or exothermic

2. Show Mg gaining an electron Mg + e−  Mg− + 19 kJ Is this endothermic or exothermic?