Transition Metals

Question 1

Transition metals forming positive ions

Answer 1

4s Electrons are lost before the electrons occupying 3d orbitals

Question 2

What kind of d orbitals have a special stability

Answer 2

Half filled or fully filled

Question 3

Transition metals are defined as

Answer 3

Metals with incomplete d sub shell in at least one of their ions

Question 4

Aufbau principle

Answer 4

states that in the ground state of an atom or ion, electrons fill subshells of the lowest available energy, then they fill subshells of higher energy.

Question 5

What are the excpetions to the aufbau principle?

Answer 5

Chromium and Copper atoms, where the added stability of the half filled/ completely filled d orbitals results in 4s being half filled

Question 6

An element has a particular oxidation state when

Answer 6

It had a specific oxidation number

Question 7

Ligands

Answer 7

Negative ions or molecules with non bonding pairs of electrons which they donate to the central metal atom/ion forming DATIVE COVALENT BONDS

Question 8

Ligands can be

Answer 8

Mono-dentate- Donates one pair of electrons to form a dative covalent bond
Bidentate- Donates two pairs of electrons
all the way up to hexadentate

Question 9

Coordination number

Answer 9

The total number of bonds from the ligands to the central transitional metal atom/ion

Question 10

When are d orbitals no longer degenerate?

Answer 10

In a transition metal complex

Question 11

Transition metal complex

Answer 11

Consists of a central metal ion surrounded by ligands

Question 12

Dative covalent bond

Answer 12

One atom provides both electrons of the bonding pair, same as any other covalent bond

Question 13

Oxidation number determines

Answer 13

if oxidation or reduction has occurred

Question 14

Rules for assigining oxidation number

Answer 14

• OXN of an uncombined element is 0
• Ions of single atoms have same OXN as their charge
• Sum of all OXN in molecule has to be 0
• Sum of all OXN numbers on a polyatomic ion is equal to charge on the ion.

Question 15

Why may transition metals have different colours

Answer 15

Differing oxidation states

Question 16

Copper and iron when naming negative complexes

Answer 16

Cuprate and ferrate, everything else add an Ate to the end

Question 17

common ligands with a 2- charge

Answer 17

Oxido 0 2-, Oxalato O4C2 2-

Question 18

Blue light is absorbed

Answer 18

Red and green are transmitted, with a yellow colour complex.

Question 19

The colour being observed is the

Answer 19

Complementary colour to the colour of wave length thats absorbed

Question 20

why will colours of the same transition metal be different ?

Answer 20

When different ligands are attached to the t metal, energy absorbed will change, resulting in different wavelengths of light being transmitted. Ligands produce different crystal field splittings.

Question 21

Ligand field strength is due to iys

Answer 21

Place in the spectrochemical series.

Question 22

Why are transition metals able to absorb light

Answer 22

The 5 d orbitals split in term of energy, they are no longer degenerate, due to electron repulsion when the ligands attach to t metal. When electrons are promoted to the higher energy level d orbitals light is absorbed.

Question 23

Spectrochemical series decreasing

Answer 23

Weaker field
Smaller energy difference
Longer wavelength absorbed

Question 24

Ultraviolet radiation absorbed

Answer 24

Will appear colourless, our eyes are unable to detect the UV radiation thats been removed from the transmitted light.

Question 25

Complexes that absorb ultraviolet radiation

Answer 25

Will have strong field ligans, which cause a greater energy gap and will require higher energy for d-d transitions.

Question 26

Why would zinc not produce coloured compounds?

Answer 26

Zinc does not hace incomplete d orbitals in its io, so no d-d trantions can take place as all orbitals are full.