LECTURE 5 (Coordinating compounds) Flashcards

1
Q

Describe Ionic compounds

A
  • Consist of positive and negative ions
  • Ions held together by ionic bonds (strong attractions between oppositely charged ions)
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2
Q

What is a Covalent bond?

A

When atoms of two non-metals share electrons

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3
Q

What does the high ionisation energies of the non-metals cause?

A

Electrons are not transferred between atoms but shared to achieve stability

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4
Q

What is the difference between a covalent bond and molecules?

A

Covalent bond = when atoms share electrons

Molecules = when two or more atoms share electrons

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5
Q

What is a dipole?

A

A polar covalent bond that has a separation of charges

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6
Q

Describe how the polarity of a bond depends on the electronegativity difference

A

In a polar covalent bond, the shared electrons are attracted to the more electronegative electron -> makes it partially -ve -> other atom with lower electronegativity becomes partially +ve due to lack of electrons at that atom -> bond becomes MORE POLAR as the ELECTRONEGATIVITY DIFFERENCE increases

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7
Q

Who was the first to formulate the ideas of the structures of coordination compounds?

A

Alfred Werner (1866-1919)

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8
Q

What are coordination compounds?

A

Chemical compounds that consist of an array of anions or neutral molecules that are bound to a central atom via coordinate covalent bonds

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9
Q

What are the molecules/ions that are bound to the central atom in coordination compounds referred to as?

A

Ligands/Complexing agents

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10
Q

How strong is the bond between metal and ligand?

A

Stronger than intermolecular forces (because they form directional bonds between the metal ion and the ligand) but are weaker than covalent bonds and ionic bonds

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11
Q

What is the difference between a double salt and a complex?

A

Double salt = dissociate into simple ions completely when dissolved in water

Complex ions = do not dissociate

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12
Q

What do double salts and a complex have in common?

A

Both are formed by the combination of two or more stable compounds in stoichiometric ratio

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13
Q

What are Isomers?

A

Two or more compounds that have the same chemical formula but a different arrangement of atoms

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14
Q

What are the two principal types of isomerism known among coordination compounds?

A
  • Stereoisomerism
  • Structural isomerism
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15
Q

What are the two types of Stereoisomerism?

A
  • Geometrical isomerism
  • Optical isomerism
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16
Q

What are the different types of Structural isomerism?

A
  • Linkage isomerism
  • Coordination isomerism
  • Ionisation isomerism
  • Solvate isomerism
17
Q

What are Stereoisomers?

A

Have the same chemical formula and chemical bonds but have different spatial arrangement

18
Q

What are Optical isomers/Enantiomers?

A

Mirror images that cannot be superimposed on one another

19
Q

What is the Valence bond theory?

A

The metal atom or ion under the influence of ligands can use its orbitals for hybridisation to yield a set of equivalent orbitals of definite geometry (e.g octahedral tetrahedral)

20
Q

What is the Crystal field theory?

A

An electrostatic model which considers the metal-ligand bond to be ionic arising purely from electrostatic interactions between the metal ion and the ligand

21
Q

What are the advantages and disadvantages of the Crystal field model?

A

ADVANTAGES:
- explains the formation, structures, colour and magnetic properties of coordination compounds

DISADVANTAGES:
- does not take into account the covalent character of bonding between the ligand and central atom

22
Q
A