Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies &

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1 Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & electronegativity

2 The Periodic Table What is the periodic table? What information does the table provide? How can one use the periodic table to predict the properties of the elements? Dmitri Mendeleev 2

3 Early Table 3

4 Alternative Models 4

5 Modern Periodic Table 5

The electron configurations are inherent in the periodic table H 1s 1 Li 2s 1 Na 3s 1 Be 2s 2 Mg 3s 2 B 2p 1 Al 3p 1 B 2pC 1 2p 2 Si 3p 2 N 2p 3 P 3p 3 O 2p 4 S 3p 4 F 2p 5 Cl 3p 5 He 1s 2 Ne 2p 6 Ar

6 The electron configurations are inherent in the periodic table H 1s 1 Li 2s 1 Na 3s 1 Be 2s 2 Mg 3s 2 B 2p 1 Al 3p 1 B 2pC 1 2p 2 Si 3p 2 N 2p 3 P 3p 3 O 2p 4 S 3p 4 F 2p 5 Cl 3p 5 He 1s 2 Ne 2p 6 Ar 3p 6 K 4s 1 Rb 5s 1 Cs 6s 1 Fr 7s 1 Ca 4s 2 Sr 5s 2 Ba 6s 2 Ra 7s 2 Sc 3d 1 Y 4d 1 La 5d 1 Ac 6d 1 Ti 3d 2 Zr 4d 2 Hf 5d 2 Rf 6d 2 V 3d 3 Nb 4d3 Ta 5d 3 Db 6d 3 Cr Mn 4s 1 3d 5 3d 5 Mo 5s 1 4d 5 W 6s 1 5d 5 Sg 7s 1 6d 5 Tc 4d 5 Re 5d 5 Bh 6d 5 Fe 3d 6 Ru 4d 6 Os 5d 6 Hs 6d 6 Co 3d 7 Rh 4d 7 Ir 5d 7 Mt 6d 7 Ni 3d 8 Ni 4d 8 Ni 5d 8 Cu Zn 4s 1 3d 10 3d 10 Ag Cd 5s 1 4d 10 4d 10 Au Hg 6s 1 5d 10 5d 10 Ga 4p 1 In 5p 1 Tl 6p 1 Ge 4p 2 Sn 5p 2 Pb 6p 2 As 4p 3 Sb 5p 3 Bi 6p 3 Se 4p 4 Te 5p 4 Po 6p 4 Be 4p 5 I 5p 5 At 6p 5 Kr 4p 6 Xe 5p 6 Rn 6p

7 Trends in Atomic Size Where are the largest atoms found? First problem: Where do you start measuring from? The electron cloud doesn t have a definite edge. They get around this by measuring more than 1 atom at a time.

8 Atomic Size Atomic Radius = half the distance between two nuclei of a diatomic molecule.

9 Trends in Atomic Size Influenced by three factors: 1. Energy Level Higher energy level is further away. 2. Charge on nucleus More charge pulls electrons in closer. 3. Shielding effect electron-electron repulsion

10 H Li Na K Rb Group trends As we go down a group... each atom has another energy level, so the atoms get bigger.

11 Periodic Trends As you go across a period, the radius gets smaller. Electrons are in same energy level. More protons = holding electrons tighter Outermost electrons are closer. Na Mg Al Si P S Cl Ar

12 Atomic Radii Trend

13 Atomic Radii

14 Ionization Energy The minimum amount of energy required to completely remove the outermost electron from a gaseous atom of the element. Removing an electron makes a +1 ion. The energy required to remove the first electron is called the first ionization energy.

15 Ionization Energy The second ionization energy is the energy required to remove the second electron. Always greater than first IE. The third IE is the energy required to remove a third electron. Greater than 1st or 2nd IE.

16 Symbol First H 1312 Second Third He Li Be B C N O F Ne

17 What determines IE Think about whether the electron wants to give up that electron! Greater distance from nucleus decreases IE Shielding effect (inter-electron repulsion)

18 Shielding The electron in the outermost energy level experiences more inter-electron repulsion (shielding). Second electron experiences the same shielding, if it is in the same period

19 Group trends As you go down a group, first IE decreases. The outer electron is further away from the nucleus because there are more energy levels. Shielding increases as does nuclear charge.

20 Periodic trends All the atoms in the same period have the same energy level. Same shielding. But, increasing nuclear charge So IE generally increases from left to right.

21 He First Ionization energy H He has a greater IE than H. same shielding greater nuclear charge Atomic number

22 He First Ionization energy H Li l l l Li has lower IE than H Outer electron further away outweighs greater nuclear charge Atomic number

23 He First Ionization energy H Li Be l l l Be has higher IE than Li same shielding greater nuclear charge Atomic number

24 Driving Force Full Energy Levels require lots of energy to remove their electrons. Noble Gases have full orbitals. Atoms behave in ways to achieve noble gas configuration.

25 First Ionization Energies

26 Trends in Ionic Size Cations form by losing electrons. Cations are smaller that the atom they come from. Metals form cations. Cations of representative elements have noble gas configuration.

27 Ionic size Anions form by gaining electrons. Anions are bigger that the atom they come from. Nonmetals form anions. Anions of main groups elements have noble gas configuration.

28 Configuration of Ions Ions have noble gas configurations (not transition metals). Na is: 1s 2 2s 2 2p 6 3s 1 Forms a 1+ ion: 1s 2 2s 2 2p 6 Same configuration as neon. Metals form ions with the configuration of the noble gas before them - they lose electrons.

29 Configuration of Ions Non-metals form ions by gaining electrons to achieve noble gas configuration. They end up with the configuration of the noble gas after them.

30 Group trends Adding energy level Ions get bigger as you go down. Li 1+ Na 1+ K 1+ Rb 1+ Cs 1+

31 Periodic Trends Across the period, nuclear charge increases so they get smaller. Energy level changes between anions and cations. N 3- O 2- F 1- Li 1+ B 3+ Be 2+ C 4+

32 Size of Isoelectronic ions Iso- means the same Iso electronic ions have the same number of electrons Al 3+ Mg 2+ Na 1+ Ne F 1- O 2- and N 3- all have 10 electrons all have the configuration: 1s 2 2s 2 2p 6

33 Size of Isoelectronic ions Isoelectronic ions that have more protons would be smaller. Al 3+ Na 1+ Ne F1- O2- N3- Mg 2+

34 Electronegativity The tendency for an atom to attract electrons to itself when it is chemically combined with another element. High electronegativity means it pulls the electron toward it. Atoms with large negative electron affinity have larger electronegativity.

35 Group Trend The further down a group, the farther the electron is away, and the more electrons an atom has. More willing to share. Low electronegativity.

36 Periodic Trend Metals are at the left of the table. They let their electrons go easily Low electronegativity At the right end are the nonmetals. They want more electrons. Try to take them away from others High electronegativity.

37 Periodic Trend 37

Trends in the Periodic Table

Trends in the Periodic Table OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret group and period trends in atomic radii, ionization energies and electronegativity The Periodic Table