Quiz on Coordination Compounds

What is the reason that metals in coordination compounds love to accept a pair of electrons?

• They have a positive charge

• They have a negative charge

• They complete their octet rule

• They have a full shell

What is the definition of a coordination compound?

• A compound with only one type of ligand

• A compound with a central metal atom bonded to a single molecule

• A compound with no counter ions

• A compound with a metal atom bonded to a number of ions or molecules

What is the role of a ligand in a coordination compound?

• Accepting a pair of electrons from the central metal atom

• Providing stability to the compound

• Acting as a counter ion

• Donating a pair of electrons to the central metal atom

According to Warner's Theory, what are the two types of valencies that a metal atom in a coordination compound has?

• Primary and secondary

• Inner and outer

• Positive and negative

• Ionic and covalent

What is the coordination number of a metal atom in a coordination compound?

• The number of ligands attached to the metal atom

• The total number of electrons in the metal atom

• The number of counter ions present

• The charge of the metal atom

Which type of ligand can donate two pairs of electrons?

• Bidentate

• Impedentate

• Polidentate

• Unidentate

What is the nomenclature rule for naming coordination compounds with multiple ligands?

• Follow alphabetic order of ligands

• Use the name of the central atom only

• Follow the order of ligands in the compound

• Use the same name for all ligands

In Crystal Field Theory, why does the energy of d orbitals increase when ligands approach?

• To increase the coordination number

• Due to attraction between ligands and orbitals

• To stabilize the compound

• Due to repulsion between ligands and orbitals

What is the hybridization of a coordination compound with the formula [Co(NH3)6]Cl3?

• sp3d2

• dsp2

• d2sp3

• sp3

What is the geometry of a coordination compound with the coordination number 6?

• Trigonal bipyramidal

• Octahedral

• Square planar

• Tetrahedral