Chem 341

Spring 2000

1. Know what is meant by (1) a ligand, and (2) the coordination number
2. Know that complex ions have an ionic charge and that coordination compounds are neutral but these terms are often used interchangeably. They both deal with ligands attached to a central metal atom, usually a transition metal.
3. Know the names of the two inorganic chemists most responsible for the development of the chemistry of coordination compounds. Know which one won the Nobel prize.
4. Know how, in general, conductivity measurements lead Werner to conclude that the coordination number of his series of Pt complexes was six.
5. Be able to plot the conductivity of a series of Pt salts of the type "K_xPt(NH₃)_y(Cl)_z, with y = 6 to 0, x = 0 to 2, z = x + 4 and z + y = 6 .
6. Know the following abbreviations and be able to write the names, chemical and structural formulas for the ligands: aq, en, acac-, ox^2-, py, dipy (or bipy), o-phen, Hdmg, dmso, Cp-, trien, triflate ion, and edta^4-.
7. Be able to sketch isomers of optically active, octahedral complex ions.
8. For octahedral complexes, know that only two bidentate ligands are sufficient to produce optical isomers.
9. Be able to sketch cis & trans and fac & mer isomers of octahedral geometries.
10. Be able to state the common geometries found for coordination numbers of 2, 3, 4, 5, and 6.
11. Know what is meant by (and be able to correctly pronounce) each of the following:
• coordinate bond 
•  the coordination number 
• a chelate complex
• a chelating ligand 
• an ambidentate ligand
•  a "n-dentate" ligand
• kinetically labile
• kinetically inert
• chiral
12. Know the following types of isomerism. Given a chemical formula, be able to write the formulas of the other isomers: polymerization, ionization, hydrate, ligand, linkage, coordination, geometric, and optical.
 

Unit 2 - Electron Configurations, Periodic Trends, and Geometries

1. Know how the atomic mass is related to the number of protons and neutrons. Know how the atomic number is related to the number of electrons and protons. Know what an isotope is.
2. Know and be able to use the three common forms of numbering the columns of the periodic table.
3. Know what is meant by each of the following: a family or group of elements, a period, triads, representative (or main group) elements, transition elements (including Sc, Y, & La), lanthanide elements, actinide elements, metallic elements, semi-metals (or metalloids), nonmetal elements, the "s", "p", "d", and "f" block elements, and alkali metals, alkaline earth elements, halogens, chalcogens, pnicogens, and coinage metals. Know that terms "rare earth elements" and "inert gases" should not be used and be able to give a reason why.
4. Know a statement of the periodic law.
5. Know the name, symbols, and range of allowed values for the four quantum numbers.
6. Know that the electron's radius can be said to increase with increasing values of the "n". Know that it shrinks with increasing nuclear charge (Z) at a fixed outer "n". Know that anions are larger than the neutral element and cations are smaller than the neutral species. Be able to give a reason for this.
7. Know how the assignment of quantum number values corresponds with each element's unique electronic configuration. Be able to give the "expected" (i.e. predicted) ground state electronic configuration of any element based on its position on the periodic chart. Know the "exceptions" of Cr, Mo, Cu, Ag, Au, Nb, Tc, Ru, Rh, Pd, & Pt. Know that there are other "exceptions" among the lanthanide elements.
8. Know what an oxidation number is and be able to assign them using the standard rules.
9. Know the trends in atomic sizes of the elements both down the columns and across the rows. Be able to give simple reasons for these trends.
10. Know what is meant by electronegativity and the general trends among the nonmetals. Know what is meant by electropositivity. Know the general periodic trends for these two properties.
11. Know the common geometric shapes found for coordination numbers 2, 3, 4, 5, 6, and 8. Be able to use the VSEPR method to predict geometries from the chemical formula. Know that this means that the correct Lewis Picture must first be drawn.

 

Unit 3 - Hydrogen, Water and Acids

1. Know the three ways that the text lists for hydrogen to enter into chemical combination. Know which one really doesn't happen and why. Know the difference between hydrogen and dihydrogen.
2. Know that hydrogen is the most abundant element in the universe (and why), tenth in abundance in the earth's crust, and present in more different compounds than any other element.
3. Be able to write balanced chemical equations for the "water gas" reaction and the subsequent "shift" reaction to produce dihydrogen. Know that dihydrogen is currently obtained industrially from natural gas (and other light hydrocarbons).
4. Know the usual laboratory method of generating dihydrogen (including the balanced chemical equation).
5. Know the reason why dihydrogen is usually a rather unreactive species even though it usually has a negative DGš for reaction.
6. Know the three isotopes of hydrogen, their chemical symbols, and the differences in their nuclei. Know which one is radioactive.
7. Know what is meant by the class of compounds termed "hydrides". Know the three general classes. Know the "ionic" class also as "saline hydrides". Know three good examples of each class.
8. Know the common reaction of all ionic hydrides with water. Know also that they will always react with any positively polarized proton (of which, water is just one specific case).
9. Know what is meant by the "hydrogen bond". Know that it only occurs in connection with covalent compounds with F, O, N, and perhaps Cl.
10. Be able to predict the relative aqueous acidity of binary acids of the nonmetals.
11. Be able to predict the relative aqueous acidity of neutral, hydroxy acids based on the "bare oxygen rule".
12. Be able to use electronegativities to predict aqueous acidities of species with the same number of 'bare" oxygens.
13. Be able to predict the relative aqueous acidities of ions of polyprotic acids.

Unit 4 - The Alkali Metals

1. Know why the Group IA elements are not found in nature in their native state. Know why they cannot be recovered from their compounds by thermal decomposition. Know why their deposits are only found in arid regions of the world.
2. Know that all compounds of Na - Cs have ionic bonding (only M⁺ cations exist).
3. Know the method of preparation of the metals from their salts. Be able to write the equation for this.
4. Know the two binary compounds formed only by Li and Na during direct combustion (Li₂O and Na₂O₂). Know the class not formed by Li or Na (their superoxides).
5. Know the chemical formula and industrial names for the following: soda (Na₂O), caustic soda or lye (NaOH), soda ash (Na₂CO₃), potash (K₂CO₃), sodium bicarbonate (NaHCO₃), and brine (aqueous NaCl).
6. Know the trend in basicities of MO and M(OH) compounds down the column.
7. Know that the trend in hydrated radii of the alkali metal cations is opposite that of the bare ionic radii trend. Be able to give a reason for this. Be able to define hydration number and hydration enthalpy.
8. Know what is meant by a primary and secondary hydration sphere (and higher). Be able to illustrate how this disperses the ionic charge.
9. Be able to describe both the solubility in, and the reaction with, the metals of Groups IA and IIA and liquid ammonia (and other small amines).
10. Know, and be able to write the equation for, the slow decomposition reaction for metals dissolved in liquid ammonia. Know that Fe(III) and certain other transition metals catalyze this reaction.
11. Know why lithium is more covalent in its bonding than the other Group IA elements.
12. Know lithium is the only Group IA element to form stable M-R type compounds (R = organic alkyl or aryl group).
13. Know the reaction for forming LiR (R = some organic group) and also the latter's reactions with covalent Cl and Br compounds, with water, with O₂, with CO₂, with alcohols, and with aldehydes. Know the coupling reaction for its slow decomposition.
14. Know what crown ethers are, how they form complexes with the alkali metal cations, and some of their uses. Also know what a cryptate ligand is.
15. Know at least five of the ways in which Li differs chemically from the other members of its family.
16. Know what an amalgam is and that the alkali metals form rather concentrated amalgams.
17. Know how amalgams of the Group IA metals can be formed by electrolysis reactions.
18. Know what is meant by the "diagonal effect" as applied to Li and Mg.
19. Know that the more positive the E^o value, the greater the tendency for the reaction to proceed as written.
20. Know the trend in E^o values down the column of Group IA elements and a reason for the "unusual" value for Li.

Unit 5 - The Alkaline Earth Metals

1. Know why the chemistry of Be stands apart from that of the rest of the group. Be able to cite at least three examples of this. Know that even Mg is somewhat different from the remaining elements.
2. Know that all Be compounds should be considered to be covalently bonded (i.e. NOT ionic!). Know that Mg's compounds are somewhat covalent (to varying degrees) and the other elements are always ionic in their compounds.
3. Know how the numerical values of the following for the Group IIA elements compare with similar values for the Group IA elements: ionization energies, hydration energies, and reactivity of the metal with water (i.e. thermodynamics and kinetics). Know the trends in these properties down the Group IIA column.
4. Know the trend in reactivities of these metals when added to water.
5. Know the nature of the hydrides of each of these elements.
6. Be able to list three similarities in chemical properties of Be and Al and two important differences.
7. Know what is meant by the statement that Be, BeO and Be(OH)₂ are amphoteric. Be able to illustrate this behavior with balanced chemical equations. Be able to give a reason for this property.
8. Know what a "refractory" material is and the properties of a good refractory material.
9. Know BeO and MgO by their ceramic names berylia and magnesia. Know how their rather reactive oxides are converted into refractories.
10. Know that all Be compounds are toxic and special care needs to be exercised in handling them. Know that the dust of Be compounds is especially bad for the lungs.
11. Know the trend in basicity and solubility of M(OH)₂ compounds down the periodic group.
12. Know the structures of (BeCl₂)_x and (BeH₂)_x and why one requires 3c-2e bonding and the other, the more normal 2c-2e bonding. Be able to predict which of these types occurs in other linear polymers of Be such as [Be(OH)₂]_x and [Be(R)₂]_x.
13. Know the reaction for the combustion of Mg metal.  Know why Mg metal doesn't spontaneously combust.
14. Know the chemical formulas and chemical names of: lime or quicklime ( CaO), slaked lime or hydrated lime (Ca(OH)₂),  milk of lime, limestone (CaCO₃) and gypsum (CaSO₄).
15. Know the chemical process by which CaCl₂ acts as a desiccant.
16. Know why adding a limited amount of water to CaO may boil the water but adding it to CaCl₂ doesn't boil the water.
17. Know the preparation reaction for a Grignard reaction. Know at least five different species present in equilibrium in an ether solution of a Grignard reagent X-Mg-R.