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Advanced Higher Chemistry > Atomic Orbitals and Transition Metals > Flashcards

Atomic Orbitals and Transition Metals Flashcards

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1
Q

Heisenberg’s uncertainty principle

A

you can probably say a region of space that an electron would most likely be found in

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2
Q

pauli exclusion principle

A

orbitals can only hold 2 electrons and they must be spinning in opposite directions

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3
Q

aufbau principle

A

electrons will fill the orbitals that occupy the lowest energy level before the further away ones

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4
Q

hund’s rule

A

when degenerate orbitals are available, these are filled singly before pairing up to fill orbitals

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5
Q

principle quantum number (n)

A

shell of electron

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6
Q

second quantum number (l)

A

orbital of electron (0,1,2,3)

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7
Q

third quantum number (m)

A

orientation in space of the orbital that the electron is found in

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8
Q

fourth quantum number (s)

A

spin of the electron (+1/2 or -1/2)

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9
Q

how many electrons can s orbitals hold?

A

2

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10
Q

how many electrons can p orbitals hold?

A

6

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11
Q

how many electrons can d orbitals hold?

A

10

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12
Q

shape of s orbitals

A

spherical

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13
Q

shape of p orbitals

A

dumb bell shaped

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14
Q

VSEPR

A

Valence Shell Electron Pair Replusion

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15
Q

what is VSEPR for?

A

to determine how many electron pairs are surrounding the central atom and therefore how they are oriented in space as the electron pairs repel eachother

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16
Q

steps of VSEPR

A
  1. how many outer electrons on central atom?
  2. how many electrons present due to bonding pairs?
  3. for polyatomic ions, how many electrons gained or lost?
  4. divide total by 2 to determine no of pairs that surround the atom
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17
Q

what does the repulsion of electron pairs surrounding central atom result in?

A

different shapes for molecules and polyatomic ions

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18
Q

electron pairs and the arrangement of the electron pairs

A 
2- linear
3- trigonal planar
4- tetrahedral
5- trigonal bipyramidal
6- octrahedral
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19
Q

strength of repulsion of electron pairs

A

bonded- bonded (least repulsion), bonded- lone, lone-lone (greatest repulsion)

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20
Q

relationship between electron configuration and ionisation energies

A

the more stable the electron configuration, the higher the ionisation energy

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21
Q

when is a subshell most stable?

A

when it is filled or half filled

22
Q

transition metal

A

metal with an incomplete d shell

23
Q

when transition metals lose electrons to form ions, which subshell are electrons lost from first?

A

4s

24
Q

why aren’t zinc and scandium transition metals?

A

their d subshells aren’t either filled or half filled

25
Q

oxidation numbers for atoms in elements

A

0

26
Q

sum of oxidation numbers in compounds

A

0

27
Q

sum of oxidation numbers in ions

A

equal to the charge on the ion

28
Q

oxidation number of F

A

-1

29
Q

oxidation number of O

A

-2

30
Q

oxidation number of H

A

+1

31
Q

oxidation number of Cl

A

-1

32
Q

if oxidation number increases in a reaction

A

element is oxidised

33
Q

if oxidation number decreases in a reaction

A

element is reduced

34
Q

compounds containing metals in high oxidation states

A

oxidising agents

35
Q

compounds containing metals in low oxidation states

A

reducing agents

36
Q

dative covalent bond

A

one atom is supplying both electrons for the covalent bond

37
Q

can compounds of the same transition metal but in different oxidation states have different colours?

A

yes

38
Q

complex

A

consists of a central metal ion surrounded by a number of negatively charged ions or neutral molecules possessing lone pair of electrons , surrounding are ligands

39
Q

ligands

A

electron donors, donate non bonding electrons into unfilled metal orbitals to form dative covalent bonds

40
Q

monodenate

A

forms a single dative covalent bond with central metal ion

41
Q

bidenate

A

forms two dative covalent bond with central metal ion

42
Q

hexadenate

A

forms six dative covalent bond with central metal ion

43
Q

coordination number

A

number of bonds from ligands to central metal ion

44
Q

naming complex ions using iupac rules

A
  1. number of ligands using mono-, bi-…
  2. identify ligands in alphabetical order sing ending -o for - ions
  3. name central metal ion, if + or neutral= english name but if - = latin name with ending -ate
45
Q

colour in transition metal complexes

A

in split d-d orbitals, electrons in lower energy d orbitals can absorb energy and move to higher energy d orbitals- if energy absorbed in d-d transitions is in visibile part of electro spectrum, colour of transition metal will be complemetary colour of absorbed colour

46
Q

splitting of d orbitals

A

electrons in degenerate d orbitals are replled by the electrons in the ligand molecules- orbitals have higher enegy that d orbitals that lie between axes and are no longer degenerate

47
Q

what does energy difference between different subsets of d orbitals depend on?

A

the ligand and its position in spectrochemical series

48
Q

heterogenous catalysts

A

different physical state to the reactants in catalysed reactions

49
Q

homogeneous catalyst

A

same physical state to the reactants in catalysed reactions

50
Q

strong field ligands

A

cause the greatest splitting of d orbitals and d-d transitions are likely to occur in UV region- 200 to 400nm

51
Q

weak field lignads

A

d-d transitions are likely to occur in visible region, complexes are likely to be coloured

52
Q

why are transition metals good catalysts?

A
  • transiton metal atoms on surface of catalyst active sites form weak bonds with reactant molecules using partially filled or empty d orbitals forming intermediate compounds which weakens covalent bonds within the reactant molecules- provides an alternative pathway with lower activation energy increasing the rate of reaction
  • having variable oxidation states allow the transition metal to provide an alternative pathway with a lower activation energy

Advanced Higher Chemistry (8 decks)

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