1. Entry Task: Friday November 2 nd Which of the following pair has a smaller radius? Sr or Sr +2 P or P -3 Na or Na +

2. Periodic Trends Handout Answers

3. Define periodic law. Periodic Law- is the periodic repetition of chemical and physical properties of elements by atomic number

4. Provide 5 properties of a metal Conductive Have Luster- shiny Malleable (smack it with hammer and it will flatten out) Solids at room temperature (except for Mercury) Loses valence electrons easy.

5. Provide 5 properties of a nonmetal Non-Conductive Lack Luster- dull Not Malleable (as a solid- if smack it with hammer it will shatter) Most are gases at room temperature. Does not lose valence electrons easy.

6. What are metalloids? Elements that have both metal and nonmetal properties

7. Identify each element as a metal, metalloid, or nonmetal. Nonmetal a)fluorine______ b)germanium______ c)zinc______ d)phosphorous______ e)lithium______ Metalloid Metal Nonmetal Metal

8. a)noble gases ______ b)halogens ______ c)alkali metals ______ d)alkaline earth metals ______ Give two examples of elements for each category. He, Ne, Ar, Kr, Xe, Rn F, Cl, Br, I Li, Na, K, Rb, Cs, Fr Be, Mg, Ca, Sr, Ba, Ra

9. What are valence electrons They are the outer most set of electrons. OR the electrons in the highest principle orbit.

10. What happens to the reactivity of an element as you move from left to right across the periodic table? EXPLAIN WHY THIS HAPPENS. What happens to the reactivity of an element as you move from left to right across the periodic table? EXPLAIN WHY THIS HAPPENS. The reactivity decreases, because they are gaining valence electron Or becoming more stable.

11. What is the octet rule? The octet rule states that elements that have a filled valence orbit, 8 electrons, will have a stable (non-reacting) arrangement.

12. What trend in atomic radius do you see as you go down a group/family on the periodic table? Its increases (gets bigger). What causes this trend? The orbit size increases as move down a group.

13. What trend in atomic radius do you see as you go across a period on the periodic table? Its decreases (gets smaller). What causes this trend? The electrons/protons increases and the nucleus pulls the electrons to it.

14. a)Al or B ______ b)S or O ______ c)Br or Cl______ d)Na or Al ______ e)O or F ______ f)Mg or Ca ______ Circle the atom in each pair that has the largest atomic radius Al - larger orbit S - larger orbit Br - larger orbit Na - less pull from nucleus O - less pull from nucleus Ca - larger orbit

15. Which ions are larger, cations or anions? Explain why. Anions are larger. They have gained electrons therefore making them larger.

16. a)N or N -3 ______ b)Li or Li +1 ______ c)O or O -2 ______ d)Mg or Mg +2 ______ e)Al or Al +3 ______ Circle the atom or ion that is LARGER of the pair. N -3 - gained electrons Li - did NOT lose electrons O -2 - gained electrons Mg - did not lose electrons Al - did not lose electrons

17. Define ionization energy. Define ionization energy. It is the energy required to remove one electron.

18. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? Explain. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? Explain. It is easier with a low ionization energy. These element with low ie are trying to get rid of electrons to become stable.

19. What trend in ionization energy do you see as you go down a group/family on the periodic table? Its decreases (gets less). What causes this trend? Large orbits have lots of electrons- easy pickin’s.

20. What trend in ionization energy do you see as you go across a period on the periodic table? Its increases (needs more energy). What causes this trend? Increasing the # of valence OR becoming more nonmetals so they don’t want to give up electrons.

21. a)Li or Be ______ b)Na or K ______ c)Cl or Si ______ d)Ca or Ba ______ e)P or Ar ______ f)Li or K ______ Circle the atom in each pair that has the greater ionization energy. Be - closer to nonmetals Na - have fewer electrons Cl - need one more to be stable Ca - have fewer electrons Ar - its got the set- back off Li - fewer electrons

22. Define Electronegativity. Define Electronegativity. The ability of an atom to attract electrons in a chemical bond.

23. What trend in electronegativity do you see as you go down a group/family on the periodic table? Its decreases (gets less). What causes this trend? Large orbits have lots of electrons not really needing electrons.

24. What trend in electronegativity do you see as you go across a period on the periodic table? Its increases. What causes this trend? Moving towards the nonmetals and they want to fill valence orbit.

25. a)Ca or Ga ______ b)Li or O ______ c)Cl or Si ______ d)Br or As ______ e)Ba or Sr ______ f)O or S______ Circle the atom in each pair that has the greater electronegativity. Ga - closer to nonmetals O - closer to nonmetals Cl - need one more to be stable Br - closer to nonmetals Sr - Fewer electrons O - fewer electrons

26. To Know list Concentration of MOSTLY Ch. 6 (75%) ◦Groups/Families verses periods ◦Metals, nonmetals and metalloid properties ◦# of valence electrons for groups ◦Atomic Radius trends ◦Ion trends (cation + and anion -) ◦Ionization energy- define and trends ◦Electronegativity- define and trends

27. To Know list Concentration of MOSTLY Ch. 6 (75%) ◦Energy levels-light, E-dot/valence-Ch. 5 ◦Particles- Protons, Electrons Neutrons-Ch. 4 ◦Physical chemical properties/changes-Ch. 3 ◦Scientific notation and Significant Figs- Ch. 2 25%