Atomic Orbitals and Transition Metals

Question 1

Heisenberg’s uncertainty principle

Answer 1

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

Question 2

pauli exclusion principle

Answer 2

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

Question 3

aufbau principle

Answer 3

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

Question 4

hund’s rule

Answer 4

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

Question 5

principle quantum number (n)

Answer 5

shell of electron

Question 6

second quantum number (l)

Answer 6

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

Question 7

third quantum number (m)

Answer 7

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

Question 8

fourth quantum number (s)

Answer 8

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

Question 9

how many electrons can s orbitals hold?

Answer 9

2

Question 10

how many electrons can p orbitals hold?

Answer 10

6

Question 11

how many electrons can d orbitals hold?

Answer 11

10

Question 12

shape of s orbitals

Answer 12

spherical

Question 13

shape of p orbitals

Answer 13

dumb bell shaped

Question 14

VSEPR

Answer 14

Valence Shell Electron Pair Replusion

Question 15

what is VSEPR for?

Answer 15

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

Question 16

steps of VSEPR

Answer 16

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

Question 17

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

Answer 17

different shapes for molecules and polyatomic ions

Question 18

electron pairs and the arrangement of the electron pairs

Answer 18

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

Question 19

strength of repulsion of electron pairs

Answer 19

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

Question 20

relationship between electron configuration and ionisation energies

Answer 20

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

Question 21

when is a subshell most stable?

Answer 21

when it is filled or half filled

Question 22

transition metal

Answer 22

metal with an incomplete d shell

Question 23

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

Answer 23

4s

Question 24

why aren’t zinc and scandium transition metals?

Answer 24

their d subshells aren’t either filled or half filled

Question 25

oxidation numbers for atoms in elements

Answer 25

0

Question 26

sum of oxidation numbers in compounds

Answer 26

0

Question 27

sum of oxidation numbers in ions

Answer 27

equal to the charge on the ion

Question 28

oxidation number of F

Answer 28

-1

Question 29

oxidation number of O

Answer 29

-2

Question 30

oxidation number of H

Answer 30

+1

Question 31

oxidation number of Cl

Answer 31

-1

Question 32

if oxidation number increases in a reaction

Answer 32

element is oxidised

Question 33

if oxidation number decreases in a reaction

Answer 33

element is reduced

Question 34

compounds containing metals in high oxidation states

Answer 34

oxidising agents

Question 35

compounds containing metals in low oxidation states

Answer 35

reducing agents

Question 36

dative covalent bond

Answer 36

one atom is supplying both electrons for the covalent bond

Question 37

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

Answer 37

yes

Question 38

complex

Answer 38

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

Question 39

ligands

Answer 39

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

Question 40

monodenate

Answer 40

forms a single dative covalent bond with central metal ion

Question 41

bidenate

Answer 41

forms two dative covalent bond with central metal ion

Question 42

hexadenate

Answer 42

forms six dative covalent bond with central metal ion

Question 43

coordination number

Answer 43

number of bonds from ligands to central metal ion

Question 44

naming complex ions using iupac rules

Answer 44

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

Question 45

colour in transition metal complexes

Answer 45

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

Question 46

splitting of d orbitals

Answer 46

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

Question 47

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

Answer 47

the ligand and its position in spectrochemical series

Question 48

heterogenous catalysts

Answer 48

different physical state to the reactants in catalysed reactions

Question 49

homogeneous catalyst

Answer 49

same physical state to the reactants in catalysed reactions

Question 50

strong field ligands

Answer 50

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

Question 51

weak field lignads

Answer 51

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

Question 52

why are transition metals good catalysts?

Answer 52

- 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