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Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

Where are transition metals located on the periodic table?

A

d block, outer e- are on the d block

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2
Q

When TM ions form, which orbital is emptied first?
And why?

A

4s
- 4s and 3d orbitals very close together
-4s and 3d orbitals have been filled, the energy levels swapped over
-due to the addition of electrons in the energies in the orbital

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3
Q

Explain why scandium and zinc aren’t transition metals?

A

Scandium ion (III) has no electrons in the d orbital
Zinc (II) ion has a full d orbital

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4
Q

Criteria for TM

A

A transition metal that can form an atom or an ion with an incomplete d orbital

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5
Q

Characteristic Properties of TM, and what causes them?

A

-form coloured ions/compounds
-catalysts
-variable oxidation states
-forms complexes

-incomplete D-orbital

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6
Q

Describe how colour arises in TM?

A

-The electrons move from the ground to an excited state
-Visible light is absorbed to promote d electrons to a higher energy level
-Absorbs colour, rest of the colours reflected, forms the complementary colour

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7
Q

Why Li+ and Na+ not used as catalysts?

A

Only one oxidation state

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8
Q

What is a nucleophile?

A

electron pair donor

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9
Q

Define coordinate bond

A

covalent bond in which both electrons are donated by one atom

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10
Q

Define Complex

A

A molecule with a transition metal ion in the middle with ligands covalently bonded to them

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11
Q

Define Ligand

A

A ligand is a molecule or ion that forms a co-ordinate bond with a transition metal by donating a pair of electrons.

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12
Q

Define co-ordination number?

A

Co-ordination number is number of co-ordinate bonds to the central metal atom or ion.

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13
Q

Define Monodentate Ligand

A

One atom
That can donate a lone pair of electrons to form 1 co-ordinate bond
e.g H2O, NH3 (positively charged)
Cl- , CN- (negatively charged)

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14
Q

Define Bidentate Ligands

A

Two lone pairs
Each donates a lone pair of electrons to form 2 co-ordinate bonds with the central metal ion
e.g C2O42 (ethanedioate from ethanedioic acid)
H2NCH2CH2NH2

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15
Q

Define Multidentate Ligand

A

several atoms
Each donating a lone pair of electrons to form several co-ordinate bonds to the central metal ion
e.g EDTA4- (hexadentate specifically)

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16
Q

Why does H2 not act as a ligand?

A

No lone pairs

17
Q

What influences the shape of a complex ion?

A

-size of ligands attached
-coordination number

18
Q

What is a simple size?

A

atoms dating lone pair of electrons have similar size

19
Q

Features of an octahedral complex

A

-Coordination number of 6
-H2O and NH3 are small ligands so can easily fit around the metal ion

20
Q

What is an octahedral complex surrounded by water?

A

hexaaqua ion

21
Q

Features of a tetrahedral complex?

A

-Coordination number of 4
-Cl- is a large ligand so only 4 can fit around the central metal ion

22
Q

Square Planar Complex and Bond Angle

A

-coordination number of 4
-for Pt2+ and Ni2+
-90*
e.g (NH3)2PtCl2 (cisplatin)

23
Q

Linear Complex

A

-Coordination number of 2
-For Ag+
-180*
e.g [Ag(NH3)2]+ (Tollen’s reagent)

24
Q

Stereoisomers

A

-Molecules with the same structural formula but different spatial arrangement

25
Q

Optical Isomers

A

Non-superimposable mirror images

26
Q

What type of isomerism do octahedral complexes show?

A

-cis and trans
-2 identical monodentate ligands are
completely opposite to each other
-180 degrees

27
Q

How does trans isomerism manifest in octahedral complexes?

A

2 identical monodentate ligands are completely opposite to each other
180 degrees

28
Q
A
29
Q

What colour precipitate would you see when dilute HNO3 and AgNO3 are added to Cl-?

A

White ppt of AgCl

30
Q

How to calculate a redox titration

A

1- write out 2 half equations
2- combine
3- calculate MOLES of chemical in a burette
4- calculate MOLES of chemical in the flask
5- work out MOLES of ORIGINAL SOLUTION
6- work out the mass/concentration of ORIGINAL SAMPLE, using moles=concentration x vol OR mass=moles x mr

31
Q
A

Chemistry (6 decks)

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