<p>Chem 113 – Week 9 (Chapter 8)</p><p>Not a whole lot of math today. Here’s the list of topics we should have down by the end of the week:</p><p>1. Electron configurations of ions: Ex. Write ground state electron configurations for the following transition metal ions: a) Sc3+; b) Ti4+; c) V5+; d) Cr3+; e) Mn2+; f) Fe2+; g) Co2+; h) Fe3+; i) Ni2+; j) Cu+; k) Cu2+; l) Ag+; m) Au+; n) Au3+; o) Pt2+.</p><p>Ex. Write ground state electron configurations for the following ions: a) Li+; b) H-; c) N3-; d) F-; e) S2-; f) Al3+; g) Se2-; h) Br-; i) Rb+; j) Sr2+; k) Sn2+; l) Te2-; m) Ba2+; n) Pb2+; o) In3+; p) Tl+; q) Tl3+.</p><p>Ex. Group the species that are isoelectronic with each other: C, Cl-, Mn2+, B-, Ar, Zn, Fe3+, Ge2+.</p><p>2. Screening and shielding of electrons:</p><p>3. Periodic Trends: -Atomic Radius increases from right to left and from top to bottom -Ionic Radius isn’t a general trend. Cations are generally smaller than their atoms and anions are generally larger than their atoms. -Ionization Energy increases from bottom to top and from left to right. -Electron Affinity increases from bottom to top and from left to right. Ex. Arrange the following in order of increasing first ionization energy: Na, Cl, Al, S and Cs.</p><p>Ex. Arrange the following atoms in order of decreasing atomic radius: Na, Al, P, Cl, Mg</p><p>Ex. Explain which of the following cations is larger, and why: Cu+ or Cu2+.</p><p>Ex. Arrange the elements in each of the following groups in order of the most positive electron affinity: a) Li, Na, K; b) F, Cl, Br, I</p><p>Ex. (Test 3 2003)Rank the following in order of increasing (left to right): (a) atomic radii Mg, Sr, Rb (b) ionic radii Mg2+, Na+, Al3+ (c) ionic radii Cl-, K+, S2- (d) first ionization energy Ge, C, As (e) electronegativity S, O, P</p><p>Ex. (Test 3 2004) The following questions relate to periodic trends. a) Which has the larger atomic radius, Mg or Al (b) Which has the smaller ionic radius, Fe2+ or Fe3+ 1- 1- (c) Which has the larger ionic radius, ClO4 or BrO4 (d) Which has the larger 2nd Ionization Energy, Na or Mg (e) Which has the smaller electronegativity, C or H (f) Which element is more metallic, Ge or Sn (e) Which has the greater electron affinity, Cl or F</p><p>Ex. (Test 3 2003) (i) Explain why the 1st ionization energy of Na is less than that of Li even though the nuclear charge has increased. (ii) Explain why the ionization energy of O is less than that of N (both in the gas phase) even though the nuclear charge has increased.</p><p>4. Predicting Reaction Products: Ex. (Final 2003) Complete and balance the following equations: (a) ____ HNO3 (aq) + ____ NaOH (aq) (b) ____ B (s) + ____ O2 (g) → (c) ____ Al (s) + ____ Cl2 (g) → (d) ____Mg (s) + ____ N2 (g) → (e) ____ Mg (s) + ____ CO2 (g) → </p><p>Ex. (Final 2004) Complete and balance the following reactions</p><p>(a) ___ Na2O(s) + ___ H2O(l)  </p><p>(b) ___ SO3(s) + ___ H2O(l)  (c) ___ P4O10(s) + ___ H2O(l) </p><p>(d) ___ K(s) + ___ H2O(l) </p><p>(b) ___ Al(s) + ___ O2(g) </p><p>(e) ___ CaCO3(s) + heat </p><p>(f) ___ Si(s) + ___ F2 (g) </p><p>(g) ___ BaH2(s) + ___ H2O(l) </p><p>Ex. (Test 3 2003) Complete and balance the following equations. (a) ___ Mg (s) + ___H2O(l) → (b) ___ Cs2O(s) + ___ H2O(l) → (c) ___ SO2(g) + ___ H2O(l) → (e) ___ CaC2(s) + ___ H2O(ll) </p><p>Ex. (Test 3 2004) Complete and balance the following reactions</p><p>(a) K2O(s) + H2O(l)  </p><p>(d) CO2(g) + H2O(l) </p><p>(e) XeO3(s) + H2O(l)  </p>