First Ionization Energy Periodic Trends of Atomic Properties requires E to strip e - from atom First Ionization Energy •Always (+) value = e - attracted to p + •E it takes to remove an e - from a gaseous atom producing a gaseous ion E + M → M + + 1e - •Measured in kJ/mole How does IE change within a period? IE ↑ from left to right: Electronegativity Metals- •The relative ability of an atom to attract e - Nonmetals- •unitless First Ionization Energy Two atoms in the same period: •Always (+) value = requires E to strip e - from atom E + M → M + + 1e - How does IE change within a period? - + IE ↑ from left to right: + Metals- low IE - large atom w/ few valence e - held less tightly by nuclear charge Nonmetals- high IE nonmetal metal smaller atoms w/ valence e - held more tightly by nuclear charge More difficult to Easier to pull off e- pull off e- Graph 4: Atomic # vs. 1st ionization energy How does IE change within a group? atomic atomic # # vs. vs. 1st IE IE Li Na K Rb Cs Fr 30 Outermost 2s 3s 4s 5s 6s 7s orbital: Small atom Large atom 25 20 increases 1st IE IE 15 1 H He 2 Li Be B C N O F Ne 10 3 Na Mg Al Si P S Cl Ar 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr increase 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 5 6 Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Rf Ha Sg Ns Hs M t Uun 0 (6) La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (7) Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 0 10 20 30 40 atomic atomic # e - held more loosely Further from nucleus, ___________________ less E Takes _______ to remove e - from 7s than 1s 1
Electronegativity Which element has the highest value for The relative ability of an atom to attract First Ionization Energy? electrons within a chemical bond He Which are more likely to attract an e - , metals or nonmetals? nonmetals Metals Which element has the lowest value for large atoms: e - in valence shell feel First Ionization Energy? weaker pull _____________ from nucleus Cs (or Fr) lose e - generally __________ to make ion w/octet Nonmetals smaller atoms: e - in valence shell feel stronger pull _________________ from nucleus gain or share e - generally _________________ to make ion w/octet Atomic # vs. electronegativity atomic # # vs. vs. EN EN H increases He 1 2 Li Be B C N O F Ne 4.5 3 Na Mg Al Si P S Cl Ar 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 9 4 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 5 6 Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn increases 7 Fr Ra Rf Ha Sg Ns Hs M t Uun 3.5 8 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 17 (6) (7) Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 3 7 35 How does EN change across period: 1 6 2.5 EN EN •EN ↑ across row (other than noble gases) 5 2 4 1.5 •# p + in nuclei ↑ , so valence e - feel strong (+) pull from nucleus 1 38 3 11 19 37 0.5 How does EN change within group: 0 •EN ↓ down column 0 10 20 30 40 atomic # •larger atoms, valence e- further from nucleus, weak pull on e - Which element has the highest Increasing size electronegativity? F Which element has the lowest electronegativity (neglecting noble gases)? Fr 2
Trend: Atomic # vs. radius 1. Atomic radii _____down a group ↑ atomic atomic # # vs. vs. atomic atomic radius radius 3.5 2. Atomic radii _____across period ↓ 3 2.5 Why? atomic radius radius 2 Increase 1. __________ in orbital sizes as energy level ↑ atomic 1.5 2. Across a period: 1 • Same # core e - blocking pull from nucleus 0.5 • Nuclear charge ↑ due to more p + 0 • Valence e - _____________________ drawn closer to nucleus 0 10 atomic atomic number 20 30 40 • The atomic radius __ ↓ Periodic Trends of Atomic Properties Which nonmetal is most likely to take electrons from a metal? Metals = Elements that have partially filled s- or d-sublevel orbitals F is the most active nonmetal: • High EN lose Tend to ______ electrons • High IE • Very small radius = nuclear charge close to valence e - Low IE, low EN, large atoms Which metal will most easily lose its Nonmetals = Elements that have partially filled valence electrons to a nonmetal? p-sublevel orbitals Fr is the most active metal: gain Tend to _______ electrons • Low EN high IE, high EN, small atoms • Low IE • Very large radius = nuclear charge far from valence e - trend in nonmetal reactivity trend in metal reactivity increases H He H He 1 1 2 Li Be B C N O F Ne 2 Li Be B C N O F Ne 3 Na Mg Al Si P S Cl Ar increases 3 Na Mg Al Si P S Cl Ar 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr increases 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 6 6 7 Fr Ra Rf Ha Sg Ns Hs M t Uun 7 Fr Ra Rf Ha Sg Ns Hs M t Uun (6) La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (6) La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (7) Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (7) Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr increases 3
trend in nonmetallic nature: trend in metallic nature: 1 H He Li Be B C N O F Ne 2 3 Na Mg Al Si P S Cl Ar increases 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Rf Ha Sg Ns Hs M t Uun 7 increases 1 H He (6) La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 2 Li Be B C N O F Ne Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Na Mg Al Si P S Cl Ar (7) 3 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr increases 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn increases 7 Fr Ra Rf Ha Sg Ns Hs M t Uun (6) La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (7) Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 4
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