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Advanced Chemistr > inorganic chem flash - red > Flashcards

inorganic chem flash - red Flashcards

1
Q

what is ems

A

electromagnetic radiation includes x rays and tv signals, different types of ems make up the ems

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2
Q

what produces ems waves

A

waves are produced by electrically charged particles

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3
Q

what are photons

A

electromagnetic radiation can be absorbed, when this occurs electromagnetic radiation behaves more like a stream of particles than as a wave. these particles caked photons. therefore say that electromagnetic raduatuin has a dual nature; wave motion and streams of photons

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4
Q

fromula to calc energy of 1 photon

A

e=hf

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5
Q

what is atomic process that produces atomic emission spectrum

A

when an atom gains energy it gets promoted to a higher energy level. When the excited electron drops back down to the lower energy level a photon is emitted.

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6
Q

Definition of transition metal

A

A transition metal has a partially filled d-sub shell in at least one of its valencies, ie when it is an ion

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7
Q

Why are zn and sc not considered a transition metal

A

Sc has an empty 3D orbital so doesn’t fit the tm definition

Zn has a full d orbital so doesn’t fit the tm definition

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8
Q

Electron configuration within a trans metal

A

(Fe) => [AR] 4s3 3d6.
As there is special stability, associated with half-filled/ completed filled d orbitals when transition metals atoms form ions electrons form the 4s orbitals are lost first

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9
Q

Oxidation state of a transition metal

A

Ox state is a change on an ion. TM’s show variable valency. Ie ionisable oxidation states/numbers

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10
Q

The preferred ox state depends on the stability of the ion

A

.

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11
Q

Why is Fe3+ the preferred ox state of iron

A

Fe3+ is the most stable as it is half filled

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12
Q

Rules for determining oxidation number of a trans metal

A
  • all free elements have an ox number = 0
  • for montomic ions, the ox number is the same as the charge on the ion
  • in compounds oxygen has an oxidation number of 2
  • hydrogen has an oxidation number of …
  • in polyatomic ions the sun of all the oxidation number is equal to the overall charge of the ion
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13
Q

What is oxidation / reduction

A

Oxidation is an increase I. Oxidation number

Reduction is a decrease in oxidation number

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14
Q

What compounds tend to be ox/reduce agents

A

Compounds containing metals high oxidation states tend to be good oxidising agents as rhe ions are easily reduced to lower oxidation states, compounds containing metals in low oxidation states tend to be reducing agents

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15
Q

What is a trans metal complex

A

A TM complex consists of a central metal ion surrounded by ligands, the metal ion is positive and acts as an electrophile

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16
Q

What is a Ligand

A

Ligands are negative ions with one or more lone pair of electrons that they can donate to the central metal ion, forming dative covalent bonds. A dative covalent bond is one in which both electrons in a bond are donated by one of the atoms.

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17
Q

What are the most common types of ligands

A

H20 - aqua
Nh3 - ammine (double m)
Fluorine - Flurido
Chlorine - chlorido

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18
Q

Different types of ligands

A

Monodentate ligands attach to the TM at one point. (Ie donate one pair of electrons)
A bidentate attaches at two points
Hexadentate at 6

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19
Q

Formula for a TM complex

A

Practice drawing

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20
Q

Rules for naming a TM metal

A
  • number of ligands
  • name ligand (if more than one then alphabetical order)
  • TM
  • oxidation state of TM
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21
Q

Practice negative TM complexes

A

Sound but x

22
Q

What causes a line in the emission spectrum

A

An exited electron returns to ground state, emitting energy difference as visible light of a specific wavelength

23
Q

Why do the lines converge as they reach the continuum

A

The energy gaps between energy levels decrease with increasing energy. Ie the higher energy levels get closer and closer together

24
Q

what does the shape of a tm depend on

A

the shape depends on the coordination number

25
Q

why d orbitals in a tm are no longer degenerate

A

in TM complexes the ligands approach the central metal ion along the x,y,z axis. the electrons in d-orbitals if the metal ion are repelled by the electrons of the approaching ligands, there d-orbitals therefore have higher energy then the d-orbitals that lie between axes. the d-orbitals are no longer degenerate. this is known as the splitting of d-orbitals

26
Q

what are strong/weak field ligands

A

strong field ligands are ligands which cause a large difference in energy between the d-orbitals, weak field ligands cause a small difference in energy between d-orbitals (ie orbitals are split less)

27
Q

what is the spectrochemical series

A

ligands can be placed in order of their ability to split d-orbitals, this is the electrochemical series

28
Q

why do TM absorb light

A

light is absorbed when electrons in a lower d-orbital are promoted to a d-orbital of higher energy. if light of one colour is absorbed, the complimentary colour will be observed

29
Q

explain why TM are used as catalysts

A

TMs are used as catalysts because unpaired d electrons or unfilled d orbitals allows intermediate complexes to occur. twos weal’s the covalent bonds inside the reactant molecules, this can provide reaction pathways with lower EA. another reaction is because TM have variable oxidation states, this allows TM to provide an alternative reaction pathway with lower Ea

30
Q

what is a homogeneous/hetergeneous catalyst

A

homogeneous catalysts are in the same physical state as the reactants,
the heterogeneous catalysts are in a different physical states to reactants

31
Q

what is the valency shell electron pair Repulsion rule

A

VSEPR
states that a molecule will adapt the shape that results in the minimum repulsion between the valency electrons. bonds space out as far as possible from each other to give minimum repulsion forces.

32
Q

what is the hierarchy of repulsion between electron pairs

A

LP:LP>LP:BP>BP:BP

33
Q

what are the rules when working out the shape of a molecule that has no lone pairs

A
  • write formula
  • workout how many valency electrons the central atom and other atoms contribute to bonding
  • divide by 2 to get the number of bonding pairs
  • decide on the basic shape of the molecule.
34
Q

draw a table showing different shapes of molecules

A

memorise table

35
Q

what happens to the shape of molecules when there are lone pairs.

A

when lone pairs are inverted, the basic shapes are modified because the LP. has greater repulsion than the BP. where all the positions are not equal the LP goes to the site with the least repulsion, ie in the trigonal bipyrimdal this is the equational position. when there is more than one LP they try to get as far apart as possible from each other.

36
Q

What is continuous spectrum

A

Continuous spectrum includes all wavelengths of light, it consists of a continuum of wavelengths

37
Q

What is emission spectrum

A

The emission spectrum includes only specific wavelengths of light

38
Q

What is absorption spectrum

A

The absorption spectrum includes all wavelengths of light with the exception of a small number of specific wavelengths of light. The absorption spectrum of an element is the converse of the emission spectrum of that element

39
Q

Explain diagram of emission spectrum supports atomic model

A

When an electron gains energy an electron in the general state can be promoted to a higher energy level ( an excited state). When the excited electron relaxes it drops back to the ground state and gives that energy (emits energy). In the form of a photon of light. The photon of light is a specific wavelength that corresponds to the difference in energy. The greater the energy the shorter the wavelength

40
Q

Explain diagram of emission spectrum supports atomic model

A

At higher energy (shorter wavelength) the emission lines become closer together, this evidence supports the modern atomic model - as energy levels get further from the nucleus they become closer together until eventually they merge and form a continuum at n= infinity. The energy gaps between energy levels decrease with increasing energy, i.e. higher energy levels get closer together.

41
Q

What are orbitals

A

The area in space where an electron is likely to be forced is called an orbital. Different orbitals are different shapes. S,p,d,f. Each orbital can hold a maximum of 2 electrons

42
Q

What is an s-type orbital

A

Spherical shape like a ball. The S orbital in the first shell is smaller than s orbital in the second shell

43
Q

What is a p-type orbital

A

The second shells all have p orbitals, in addition to an s orbital. The p subshell has three different p orbitals of the same energy. Orbitals that have equal energy are said to be degenerate. The shape of p orbitals is a dumbbell shape.
What is a d-type orbital

44
Q

quantum numbers

A

write out now on paper

45
Q

State aufbau’s principle

A

Electrons fill the orbitals in order of increasing energy meaning that the lowest energy subshells are filled first. Of course some sub-shells such as p-subshells and d-subshells have degenerate orbitals

46
Q

What does hund’s rule state

A

When there are degenerate orbitals that are available, electrons fill each degenerate orbital singly, and with parallel spins, before pairing up to fill the orbitals

47
Q

Pauli’s exclusion

A

No two electrons within the same atom can have the same four quantum numbers. This means that two electrons in the same orbital must have ….. spins

48
Q

Ionisation energies

Explain the trend in 1st ionisation energy of elements as you go across the period

A

The general trend as you go across a period is an increase in 1st ionisation energies. However, a decrease can be seen between Be and B, as well as between N and O.

49
Q

shapes of molecules

A

go into screenshots now and do it

50
Q

Order of increasing ems

A

Gamma ray, X-ray, ultraviolet, visible, infrared, microwave, radio waves

Advanced Chemistr (32 decks)

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