Between you and a partner, grab one textbook…

1. Turn to p. 193 (Organize Elements minilab) Cut a piece of construction paper into 10 squares and write the information for each element on each separate sheet Follow the instructions and answer the questions on a separate sheet (one sheet per pair) Between you and a partner, grab one textbook…

2. For quiz b 3 2

3. Chapter 6 Periodic Table

4. J.W. Dobereiner • Early 1800’s, classify elements in sets of 3 • This trend didn’t work for most of the elements known at the time Development of the Periodic Table

5. 1865 – noticed trend that every 8th element had same properties (law of octaves) • Unfortunately, this didn’t work for all the known elements at the time, and it was dismissed John Newlands

6. Considered the father of the modern Periodic table Mendeleev arranged by increasing atomic mass (1869)

7. Discovered that the # of protons = atomic number Developed concept of arranging PT by atomic number Periodic law – there is a periodic repetition of properties when elements are arranged by atomic # Moseley

8. Periods vs. groups/families • Metals vs. nonmetals vs. metalloids • What are some properties? • Are all nonmetals gases? • Representative elements vs. transition metals vs. inner transition metals Parts of the Periodic Table

9. What do all elements in the same group have in common? Valence electrons All elements in the same group exhibit similar characteristics Sodium and Potassium are both highly reactive in water So, what subatomic particle is responsible for determining properties of an element? Electrons

10. How many valence electrons? Alkali metals: 1 valence electron, s block Alkaline earth metals: 2 valence electrons, s block Halogens: 7 valence electrons, s and p block Noble gases: 8 valence, totally filled s and p block, except for which element? Helium – his s block is filled with only 2

11. Transition metals: (Groups 3B – 12B) 2 s-block electrons, and various d block electrons Called transition metals b/c electrons can move around the d block Inner transition metals: 2 s-block electrons and various f block electrons Representative elements: (Groups 1A – 8A) any of the s or p-block elements

12. SHIELDING Shielding • Which atom has more shielding? • We’ll be coming back to this idea of shielding often

13. Half the distance between the nuclei of 2 like atoms No definite edge of electron cloud Atomic Radius atomic radius

14. Trends in Atomic Radius Be C • Down the Groups • What is changing about the atom as we go down? • # of shells = energy level • More shells = bigger atom • Across the Periods • Same period means same # of shells • What is changing as we go across a period? F Li Na K Rb

15. Who is larger? • Mg or S? • Br or K? • C or Sn? • Who is smaller? • Li or N? • F or I? • Put the following elements in order of increasing atomic radius Ca, Fe, Br, O, Ba

16. An ion is an atom with a charge (+ or -) • In a sodium atom, how many protons and electrons do we have? How many valence e-? • 11 p+ and 11 e- • 1 valence e- • Can we lose protons? • No, that would change the element What is an ion?

17. An atom is most stable when it has a full outer shell • How many valence electrons = full? • An atom will lose or gain electrons to achieve this – whichever is easiest • Sodium has 1 valence electron. Do you think he loses or gains? • Loses, then there will be 1 more proton than electrons Octet rule

18. If an atom has 2 valence e-, what will it do? • What group is this? What charge? • What charge does aluminum form? Lose or gain? • +3, loses 3 electrons If an ion is positive it has ______ e- If an ion is negative it has ______ e-

19. Size of Ions (Ionic Radius) Na Na+ e- F- F e-

20. Who is larger? • Mg or Mg2+? • S or S2-? • O2- or F1-? • First, determine if you have lost or gained electrons… Which particle do you have more of (who has the power?)

21. IE is the energy required to remove an electron from an atom (and make it an ION) KEEP SHIELDING IN MIND Babysitter analogy A couple First Ionization Energies: Li = 520 kJ/mol O = 1310 kJ/mol Who is harder to take an electron from? Ionization energy

22. Which has the higher ionization energy? • Li or N? • Cs or Li? • O or S? • Which has the lower ionization energy? • K or Fe? • F or Br?

23. Warm up: As we go down the groups on the PT, the size of the atom __________, making it __________ to take an electron away, making the ionization energy __________ As we go left to right across a period, the size of the atom _________, making the ionization energy __________. Turn in projects up front…

24. Arrange in decreasing ionization energies: Cr, Br, I, Li, N

25. How well an element can attract electrons from another element in a bond • Atoms fill their outer shells when they bond with another atom • How might EN relate to IE? • If it’s hard to take an electron away, what kind of attraction do you think it has? • What do you think the electronegativity of a noble gas might be? Do they want to bond? • Zero Electronegativity (EN)

26. Arrange in order of increasing electronegativity: Mg, F, Ne, Cs, Al

27. NOW THE EASY WAY… & OVER IE and EN increase RaDius Decreases UP But it is good to understand the WHY so you can double check yourself…

28. Put in order of decreasing atomic radius: Ca, Al, Ne, Rb, Br, Au, Zn, C What order is this for ionization energy? (increasing or decreasing)

29. Skip #8 Add this question (doesn’t matter where): Determine the larger radius in the following: a. Mg or Mg2+ (whatare thethe b. Cl or Cl1- things with charges c. Cl1- or P3- called, and how do they get those charges?)

30. Between you and a partner, grab a textbook: Turn to p. 193 (Organize Elements minilab) Cut a piece of construction paper into 10 squares and write the information for each element on each separate sheet Follow the instructions and answer the questions on a separate sheet (one sheet per pair) When finished, turn it in and grab a BINGO card Continue from yesterday…