Slaked lime (Ca(OH)₂), is a commonly used flocculant. How can you prepare Ca(OH)2 from calcium metal?

Two second-series transition metals can form [M(Br)₄]⁻ complex ions with three unpaired electrons. Determine the oxidation state of the metals and their identities.

Find the transition metals on the periodic table that correspond to these electron configurations. Name each metal.

1. [Kr] 5s²4d²

2. [Kr] 5s²4d⁵

Provide the electron configuration of free Ni²⁺ ion and determine the number of unpaired electrons.

Identify the oxidation number of each metal center in the following coordination compounds.

i. [Cr(en)₂(CO)Cl]²⁺

ii. Co(H₂O)₃(CN)₃

iii. [Ni(C₂O₄)₂(NH₃)₂]^2–

iv. [Fe(OH)₅]^3–

v. Cr(CO)₆

Draw the Lewis structure of [Ni(NH₃)₆]²⁺

Is the given ligand monodentate? If not, what is its denticity? Is it capable of forming chelate rings?

In the coordination complex, [Co(CN)₆]^3-, which species acts as the Lewis base during its formation with cobalt ion? Furthermore, determine the oxidation number of Co and the coordination number of the formed complex.

Name the following compounds. 

a) Na₂[Fe(CN)₅NO]

b) [Pt(NH₃)₂]Cl₂

c) [Co(NH₃)₄Cl₂]Br

Deduce the formula, with the charge, for the coordination compounds below:

i. A nickel(II) complex with four ammonia ligands and two nitrate ligands

ii. A palladium(II) complex with two dien ligands

iii. A cobalt(III) complex with three ethylenediamine ligands and three chloride ligands

Consider the following isomers of iron(II) coordination compound:

What are the names and formulas for the compounds?

Those whose lobes point directly at the ligands or those whose lobes do not–which set of d-orbitals will have higher energy when ligands approach a central metal ion?

Explain why Pd²⁺(aq) appears brown while Cd²⁺ appears colorless.

Draw the crystal field energy-level diagram for the below-given square planar complex. How many unpaired electrons are present?

[Pt(H₂O)₄]²⁺

Match the crystal-field splitting diagrams to the following descriptions:

i. a square planar complex of Pt²⁺

ii. a tetrahedral complex of Pt²⁺

iii. a weak-field octahedral complex of Co³⁺

vi. a strong-field octahedral complex of Co³⁺

Accomplish the following to give a valence bond description of [Fe(H₂O)₂F₄]^2- (high-spin):

i. Sketch the orbital diagram for the free metal ion and the orbital diagram for the metal ion in the coordination complex.

ii. Determine the hybrid orbitals used by the metal.

iii. Count the number of unpaired electrons.

At 480 nm, the ion, [Cr(CN)₆]^3-, displays one absorption peak. Determine its crystal field splitting energy, Δ (kJ/mol), and the color of that ion. Is CN^- a stronger or weaker field ligand compared to NH₃?

Consider the complexes given below. Identify which are diamagnetic.

i. [Zn(H₂O)₄]²⁺ (tetrahedral)

ii. [Rh(NH₃)₆]³⁺

iii. [Pt(CN)₄]^2– (square planar)

iv. [PdBr₆]^2–