5: Properties of Transition Metals and Ligands Flashcards

1
Q

What is the definition of a transition metal?

A

Metals that can form one or more stable ions with an incomplete D sub shell.

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2
Q

Which 2 elements do not count as transition elements?

A

Scandium and Zinc

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3
Q

Why are scandium and zinc not considered transition metals?

A

They do not form ions with incomplete d subshells.

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4
Q

Give the shortened electron configuration of chromium.

A

[Ar] 4s1, 3d5

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5
Q

Give the shortened electron configuration of copper.

A

[Ar] 4s1 3d10

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6
Q

For copper and chromium, why does the 4s subshell not fill fully?

A

The atom is more stable when the 3d subshell is either full or half full.

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7
Q

Give the shortened electron configuration of Cu2+

A

[Ar] 3d9

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8
Q

Give 2 physical properties of transition metals.

A

High density
High melting/boiling point

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9
Q

What type of ions can transition elements form?

A

Complex

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10
Q

What can transition metal ions do that normal metal ions can’t do?

A

They can form coloured ions.

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11
Q

Why can transition metals form ions with different charges?

A

They have variable oxidation states

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12
Q

What is a complex ion?

A

An ion formed when a transition metal is surrounded by ligands that bond to it by donating lone pairs into vacant d orbitals

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13
Q

Ligands always form which type of bonds?

A

Coordinate bonds

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14
Q

What are ligands?

A

Atoms or ions that have a lone pair to form a coordinate bond with other metals.

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15
Q

What is the coordination number?

A

The number of coordinate bonds formed by ligands to metal ions.

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16
Q

What is a unidentate ligand?
Give some examples.

A

Ligands that form one coordinate bond.
NH3, :Cl-, :CN-

17
Q

In Ag+ complexes, what shape will the ion be?
What will the bond angle be?
What will the coordination number be?

A

Linear
180 degrees
Coordination number 2

18
Q

In large ligands (eg: :Cl-), what shape will the ion be?
What will the bond angle be?
What will the coordination number be?

A

Tetrahedral
Bond angle 109.5
Coordination number 4

19
Q

In Pt2+ complexes, what shape will the ion be?
What will the bond angle be?
What will the coordination number be?

A

Square planar
90 degrees bond angle
Coordination number 4, 2 lone pairs

20
Q

In most complex ions, what shape will the ion be?
What will the bond angle be?
What will the coordination number be?

A

Octahedral
Bond angle 90
Coordination number 6

21
Q

What are bidentate ligands?

A

Ligands that form 2 coordinate bonds

22
Q

Give 2 examples of bidentate ligands.

A

En, (C2O4 2-)

23
Q

What is another name for complex ions that form a multidentate ligand?

A

Chelate

24
Q

Chelates can be used to remove d block metal ions from what?

A

Remove them from solution

25
Q

Name the element that creates a ligand in haem groups.
This atom froms the complex called g_____

A

Nitrogen. Forms part of the globin complex.

26
Q

Why is the binding of oxygen to haemoglobin reversible?

A

The bond between the iron ion and oxygen is weak, so oxygen easily be unloaded where needed.

27
Q

Why is the binding of CO to haemoglobin irreversible?

A

CO is a ‘better ligand’.

28
Q

Describe how optical isomerism works in ligands with different atoms.

A

Ligands will be on different atoms.

29
Q

Finish the substitution reaction equation for
[Co(H2O)6]2+ + 6NH3

A

[Co(H2O)6]2+ + 6NH3 -> [Co(NH3)6]2+ + 6H2O

30
Q

Finish the substitution reaction equation for [Cu(H2O)6]2+ + 4Cl-

A

[Cu(H2O)6]2+ + 4Cl- -> [CuCl4]2- + 6H2O

31
Q

Finish the substitution reaction equation for [Cu(H2O)6]2+ + 4NH3

A

[Cu(H2O)6]2+ + 4NH3 -> [Cu(H2O)2(NH3)4]2+ + 4H2O

32
Q

Why is the reaction with CN- ligands irreversible?

A

It forms strong bonds

33
Q

What type of isomerism can complex ions with a square planar shape and octahedral shape show?

A

E/Z

34
Q

Describe arrangement of ligands in a cis isomer of an octahedral complex ion.

A

If the 2 different ligands to the other 4 are next to each other, it is cis.

35
Q

Describe arrangement of ligands in a trans isomer of an octahedral complex ion.

A

If the 2 ligands that are different to the other 4 are opposite each other, it is trans.

36
Q

Finish the ligand substitution equation for this reaction:
[Fe(H2O)6]3+ + 6CN-

A

[Fe(H2O)6]3+ + 6CN- -> [Fe(CN)6]3- + 6H2O

37
Q

For most substitution reactions, is enthalpy likely to be positive or negative?

A

Negative

38
Q

Finish the substitution equation for this reaction.
[Cu(H2O)6]2+ + 3en

A

[Cu(H2O)6]2+ + 3en -> [Cu(en)3] + 6H2O

38
Q

Explain why entropy increases for this reaction:
[Ni(NH3)6]2+ + 3en -> [Ni(en)3]2+ + 6NH3
State the feasibility of this reaction.

A

There are more molecules on the right than the left. This means the reaction will always be feasible.