Si(OH)4+NaBr=SiBr4+NaOH

Chem 11 Periodic Trends Name: 1. Attract or repel? a. positive and positive₨ b. negative and negative R c. positive and negative A 2. Place arrowheads in the correct direction on the horizontal and vertical lines below. Ionization energy increases Ionization energy increases 3. Which member of each of the following pairs should have a greater ionization energy? a) BronC b) Al or Cl c) Noor Xe d) Mgor Ba e) For No 1) Rb or 4. The ionization energies (IE) of the first 20 elements are given in the table below. Atom Atomic # IE (kJ) Atom 0 Atomic # IE (kJ) Atom Atomic # IE (kJ) H 1 1312 8 1314 P 15 1012 Ho 2 2372 F 9 1681 S 16 1000 Li 3 520 Ne 10 2081 C1 17 1251 Be 4 899 Na 11 496 Аг 18 1521 B 5 801 Mg 12 738 K 19 419 C 6 1086 Al 13 578 Ca 20 590 N 7 1402 Si 14 787 Plot the ionization energy versus atomic number on the following graph and connect each point to the next with a straight line. Then answer the following questions. 2500- 2000- 1500- lentiation 1000- 500- electrons have to our versy removed from full 0 difficult a) Why are the ionization 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 (H) (He) (L) (B) (8) He, Ne, and Ar so () ( high? Atomik )()()( )(A) (57 ) (P) (B) (C) (Ar) ( K) (0) number b) Why do the ionization energies decrease going from He to Ne to Ar? c) Why is there a general increase in ionization energy going from Li to No?elutrons closer to ruckens, ining. acter most electrons are further. from nucleus attention smaller, easy licen d) "Filled subshells and half-filled subshells have a special stability which requires extra energy to be applied before electron removal can occur". This general statement is supported by the existence of the electron configuration exceptions found for Cu and Cr. What expérimental evidence exists in the graph "ionization energy versus atomic number"? 3. Consider two atoms: O and Te. a) Which atom has the larger atomic radius? Te b) Which atom has the larger ionization energy? O c) Which atom has more shells? Te d) How many valence electrons does Te have? 6 e) What is the valence of Te? 2 f) Which atom has a greater electrostatic attraction between its nucleus and outermost electrons?   O 6. Consider two atoms: Ga and Br. a) Which atom has the larger atomic radius? Ga b) Which atom has the larger ionization energy? Br c) Which atom has more shells? Same d) How many valence electrons does each atom have? Ga:   3, Br: 7 e) What is the valence of each atom? Ga: 3, Br: -1 f) Which atom has a greater electrostatic attraction between its nucleus and outermost electrons? Br 7. Consider two atoms: Li and F. a) Which atom is larger? Li b) Which atom has the stronger attraction to the outer electrons on a neighbouring atom, based only on the atomic radius? F c) Which atom has the greater nuclear charge? F d) Which atom can attract electrons from an adjacent atom most strongly, based on both size and nuclear charge? F e) Fill in the blanks: In general, when going from left to right across the periodic table the electronegativity of the atoms will increase.   8. Consider two atoms: F and I. a) Which atom is larger? I b) Which atom has a stronger attraction to the outer electrons of another atom? F c) Fill in the blanks: In general, when going down a family of the periodic table the electronegativity of the atoms will decrease.   9. Place arrowheads in the correct direction on the horizontal and vertical lines below. [Image of a periodic table with arrows indicating trends in electronegativity] 10. a) Ignoring the noble gases, which atom is the most electronegative? F b) Ignoring the noble gases, which atom is the least electronegative? Fr c) Which is more electronegative,   K or Be? Be d) Which is more electronegative, Pb or S? S