Entry Task: Friday November 2 nd

1. Entry Task: Friday November 2nd 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. Periodic Law- is the periodic repetition of chemical and physical properties of elements by atomic number Define periodic law.

4. 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. Provide 5 properties of a metal

5. 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. Provide 5 properties of a nonmetal

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

7. fluorine______ • germanium ______ • zinc ______ • phosphorous______ • lithium______ Nonmetal Metalloid Metal Nonmetal Identify each element as a metal, metalloid, or nonmetal. Metal

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

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

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

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

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

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

14. Al - larger orbit • Al or B ______ • S or O ______ • Br or Cl ______ • Na or Al ______ • O or F ______ • Mg or Ca ______ S - larger orbit Br - larger orbit Na - less pull from nucleus O - less pull from nucleus Circle the atom in each pair that has the largest atomic radius Ca - larger orbit

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

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

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

18. It is easier with a low ionization energy. These element with low ie are trying to get rid of electrons to become stable. 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.

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

20. 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. What trend in ionization energy do you see as you go across a period on the periodic table?

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

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

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

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

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

26. 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 To Know list

27. 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% To Know list