Do Now: Location on Periodic Table Lose or Gain electrons to obtain noble gas electron configuration? Form cations or anions? Relative ionization energy Relative electronegativity Metals Nonmetals If an element has a LOW ionization energy, what does that tell you about its tendency to lose electrons? If an element has a HIGH electronegativity and electron affinity, what does that tell you about its tendency to gain electrons? ~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~ Ionization Energy First Ionization Energy energy required to Second Ionization Energy energy required to Third Ionization Energy energy required to In general 1 st I.E. 2 nd I.E. 3 rd I.E. Based on the relative jump between ionization energies, you can tell how many the element has 1. 2. a. Between which 2 ionization energies do you see the biggest jump? b. How many valence electrons would this element have? c. What group would this element be found in?
Properties of Metals vs. Nonmetals Metals (can be hammered/molded into sheets) (can be drawn/pulled into a wire) Have (are shiny when polished) Good (allow heat & electricity to flow throw them) Nonmetals malleable or ductile; instead, they are (shatter easily) luster; instead, they are They are either or conductors Reactivity of Metals vs. Nonmetals Reactivity of a metal is related to its o The, the the metal o Trend (within the metals on the periodic table): Going down a group: Going across a period: o Most reactive metal: Reactivity of a nonmetal is related to its o The, the the nonmetal o Trend (within the nonmetals on the periodic table): Going down a group: Going across a period: o Most reactive nonmetal:
Ions and Ionic Radius When an atom loses electrons and becomes a cation, its radius becomes than that of the neutral atom o # protons # electrons, therefore increasing the effective nuclear charge, meaning that there is a stronger pull of the electrons towards the nucleus. When an atom gains electrons and becomes an anion, its radius becomes than that of a neutral atom o When electrons get added to the same energy level, they repel each other Isoelectronic Species: Atoms/ions that have the Atom/Ion C Cl Mn 2+ B Ar Zn Fe 3+ Ge 2+ Atomic Number (# protons) Lost or Gained Electrons? # of electrons *Which ones are isoelectronic to each other? *Group the species above in order of increasing radius. (Remember: for isoelectronic species, the one with a larger nuclear charge will have a smaller radius)
Directions 1. The following page represents a blank periodic table, containing elements from groups 1, 2 and 13-18 in periods 1-4. Elements with atomic numbers 21 30 have been omitted from this activity. It may be helpful to draw in a staircase before you start placing elements 2. The elements below represent elements with atomic numbers 1 36. However, these elements have been coded with letters A-Z. Using the clues below, identify squares A Z as one of the elements in the first four periods of the periodic table. Once you have identified all of the squares (letters) as an element from period 1 4, write the letter in the appropriate period and group on the blank periodic table in the space provided. 3. In the blanks next to each clue, indicate the element from the Periodic Table it represents. Clues 1. The following groups of letters have similar properties: S, T, M B, U, J P, K, Z, H O, V, E L, Q, W, G D, A, F C, N, Y R, I, X 2. Element A has the largest radius in its group 3. Element B has valence electrons in the 3 rd shell. 4. Element C has the smallest electron shielding effect in its 5. Element D has an atomic # eight times that of the atomic # of Z. 6. Element E has the smallest radius in its 7. The ion for Element F is isoelectronic to element P. 8. The ion for Element G is isoelectronic to element Z. 9. Element H has a full 4 th energy level (shell). 10. Element I is the second most reactive in its 11. Element J has the lowest electronegativity in its 12. Element K is an inert (unreactive) gas with 3 electron shells. 13. Element L has the smallest nuclear charge in its period 14. Element M is a nonmetal with the second highest electron affinity in its 15. Element N has a higher electronegativity than L. 16. Element O has the lowest ionization energy in its 17. Element P is a stable gas with the 2 nd highest ionization energy of its 18. Element Q loses an electron most easily in its 19. Element R is a metalloid. 20. Element S has the largest electron shielding effect in its 21. Element T is the most electronegative element. 22. Element U is a brittle solid. 23. Element V is a metal even though it touches the staircase. 24. Element W is the only nonmetal and gas in this 25. Element X is the only diatomic element in its 26. Element Y has the biggest jump between its 2 nd and 3 rd ionization energies and has the highest mass in this 27. Element Z has a complete valence shell of 2 electrons.
Name Date Block **On the back of this page, write a short paragraph explaining your thought process and how you determined where to place the letters corresponding to each element.