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Consider two metals: M and N. A strip of solid N is placed into 2mL of a 0.10 M M(NO3)2 solution. The solution changes from blue to green.
Six-coordinate CR(3) complexes of the type trans-(CrL4A2)n+, generally have magnetic moments consistent with three unpaired electrons.
Determine the oxidation state of the metal in each of the following complexes. Draw all linkage isomers and stereoisomers for each complex.
Expensive electronic equipment use gold-coated parts. Explain why this is based on chemical behavior.
How do you estimate the percentage covalent nature of different compounds using the Pauling's Electronegativity Scale?
In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y^4-) and metal chelate (abbreviated MY^n-4) can buffer the free metal ion.
The 3dxy orbital has its high probability regions lying between the x and y axes. The 3dz2 orbital has its high probability regions mainly on the z axis.
A plot ofthe lattice energies for MClz salts for M : Ca to Znand a drawing of the rmit cell are shown to the right. In the elechostatic model.
Calculate the number of miligrams of each metal (Mn2+, Zn2+, and Mg 2+) in the 25.00 mL sample of unknown.
Discuss the 6 major groups of chemical reactions and provide an example and the general formula of each type.
Determine the point group for each of the following molecules, ions and objects. Draw a clear picture of each molecule.
Determine the point group for each of the following molecules and items. Draw a clear picture of each molecule or item and show.
Assume the internuclear axis is the y axis and the incoming atom has the same axis system as the atom with the fx(x2-3y2) orbital projection.
For each series of octahedral complexes, predict which will have the largest and which will have the smallest value for Do. Briefly explain your answers.
Three elements are listed below. How many electrons does each have in its outermost electron shell?
Nearly every compound of silicon has this element in the +4 oxidation state. In contrast, most compounds of lead have this element in the +2 oxidation state.
When chemists discuss the periodic nature of the elements they focus on mainly the 'representative elements'.
Consider the placement of Na, K, Ca, Cu, Mg and Z on the periodic table. Does their placement reflect their physical properties? How?
In the early days of the periodic table, the 1870s, both silicon and tin were known elements, but germanium was unknown.
What happens to the atomic radii as you go down a column in the periodic table,e.g. from Li to Fr?
How do you determine the oxidation state of an element in a compound? Two well-known compounds KMnO4 and K2Cr2O7 are used as examples.
To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes.
In general, as you go across a period in the periodic table from left to right: (1) the atomic radius __________; (2) the electron affinity.
As you go down a column in the periodic table, atomic size increases. Explain why in terms of principle quantum number and effective nuclear charge.
What is the relationship between first ionization energies and metallic and non-metallic properties?