Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Georges chem > Transition elements chp 24 > Flashcards

Transition elements chp 24 Flashcards

1
Q

what similarities do the d-block elements share

A
  • all metallic
  • display typical physical properties of metals
  • high melting and boiling points
  • shiny in appearance
  • conduct both heat and electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what are some common uses for d-block elements

A
  • tools, coins, construction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is special about the electron configuration of chromium and copper
why is this

A
  • they do not have full 4s orbtials
  • its more stable to have a d5/d10 and 4s1 sub-shells than to have d4/d9 and 4s2 sub shells
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is unique about the 4s and 3d sub shells

A
  • 3d is at a higher energy level than 4s
  • 4s sub-shell fills up and empties before 3d sub-shell
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what is the definition of a transition element

A
  • d-block elements that form at least 1 ion with partially filled d-orbitals
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

which d-block elements are not transition elements

A
  • scandium and zinc
  • scandium only forms 3+ by losing its 4s electrons and its only 3d electron
  • zinc only forms 2+ by the loss of its 4s electrons leaving it with a full 3d orbital
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what are the properties of transition elements that differ from other metals

A
  • transition elements have different oxidation States within certain compounds
  • form coloured compounds
  • elements and their compound can act as catalysts
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what are the colours and oxidation states formed from the first period of d-block elements

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is the trend in number of different oxidation states across the transition elements

A

increase to manganese then decrease again

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what are some examples of were transition metals and their compounds are used as catalysts

A
  • iron catalyst in the haber process
  • vanadium oxide catalyst in the contact process
  • nickel in hydrogenation
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what is a complex ion

A
  • formed when one or more molecules or negatively charged ions bond to a central metal ion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what is the definition of a ligand

A
  • a molecule or ion that donates a pair of electrons to a central metal ion to form a coordinate/dative covalent bond
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what is meant by the coordination number

A
  • indicates the number of coordinate bonds attached to the central metal ion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

how should you represent complex ions

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is a monodentate ligand

A
  • able to donate one pair of electrons to central ion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what are some examples of ligands and what would they be called in nomenclature

A
  • water: aqua
  • ammonia: ammine
  • carbon monoxide: carbonyl
  • cyanide ion: cyano
  • chloride ion: chloro
  • hydroxide ion: hydroxy
  • oxygen molecule: oxo
  • nitrogen monoxide: nitroso
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what are bidentate ligands

A

ligands that can donate 2 lone pairs of electron to the central metal ion (forms 2 dative bonds)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what are some examples of bidentate ligands

A
  • 1,2-diaminoethane (en)
  • ethanedioate (oxalate)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what does the shape of a complex ion depend upon

A
  • depends upon the coordination number
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what shape does a complex ion with a coordination number of 6 have

A

octahedral shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what 2 shapes can complex ions with coordination numbers of 4 give

A
  • tetrahedral (common)
  • square planar
22
Q

when are square planar complexes formed

A

occur in complex ions of transition metals with 8 d-electrons in the highest energy d sub-shelled

23
Q

what does the colour of the complex ions depend upon

A
  • depends upon the metal at the centre of the complex, its oxidation state, and the ligands bonded to It
24
Q

what types of steroisomerisms can complex ions display

A
  • cis-trans isomerism
  • optical isomerism
25
Q

what does the type of stereoisomerism of complex ions depend on

A
  • some 4 coordinate and 6 coordinate complex ions containing 2 different different monodenate ligands show cis-trans isomerism
  • some 6 coordinate complex ions containing monodentate and bidentate ligands can show both cis-trans and optical isomerism
26
Q

what is different between organic stereoisomerism and stereoisomerism in complex ions

A
  • in organic, requires the presence of a C=C bond
  • in complex ions, shape of complex holds groups in different orientations about central ion
27
Q

when would cis isomer complex ions occur

A
  • ligands are adjacent to one another
28
Q

when would trans isomer complex ions occur

A
  • ligands are opposite one another
29
Q

on what octhedral complex can optical isomerism occur

A

has to contain 2 or more bidentate ligands

30
Q

what is another name for optical isomers

A
  • enantiomers
31
Q

whats the definition of optical isomer

A
  • non-superimposable mirror images of each other (like left hand and right hand)
32
Q

what is a ligand substitution reaction

A

reaction is one in which one ligand in a complex ion is replaced by another ligand

33
Q

when copper (II) sulphate is dissolved in water what is seen

A

pale blue complex ion [Cu(H2O)6] 2+, is formed

34
Q

what happens when excess aqueous ammonia is added to a solution containing [Cu(H2O)6] 2+

A
  • pale blue changes colour to form a dark blue solution
  • 4 ammonia ligands have replaced 4 of the water ligands
35
Q

if ammonia is added drop wise to a solution containing [Cu(H2O)6] 2+ what reactions and colour will be seen

A
  • pale blue precipitate of Cu(OH)2 is formed in first stage
  • Cu(OH)2 precipitate then dissolves in excess ammonia to for dark blue solution
36
Q

what is seen when excess conc HCl is added to a solution containing [Cu(H2O)6] 2+

A
  • pale blue solution changes to form yellow solution
  • example of ligand substitution reaction
  • 6 H2O molecules replaced by 4 Cl molecules
  • Cl ligands are bigger than H2O ligands so fewer can fit round central ion
37
Q

what is produced when chromium (III) potassium sulphate, KCr(SO4)2 - 12(H2O) is dissolved in water

A
  • [Cr(H2O)6] 3+ is formed
    ^pale purple solution formed
38
Q

what occurs when chromium (III) sulfate is dissolved in water

A
  • green solution formed
  • [Cr(H2O)5SO4]-
39
Q

How does [Cr(H2O)6] 3+ reaction with excess ammonia

what can be observed

A
  • forms complex ion [Cr(NH3)6]3+
  • when excess added drop wise
    ^initally a grey-green precipitate of Cr(OH)3 is formed
    ^Cr(OH)3 dissolves in excess ammonia to form the complex ion [Cr(NH3)6] 3+
40
Q

explain how carbon monoxide can effect haemoglobin

A
  • When carbon monoxide is inhaled, it binds to hemoglobin to form carboxyhemoglobin
  • this bond is much stronger than the bond between hemoglobin and oxygen.
  • presence of carbon monoxide reduces the oxygen-carrying capacity of blood.
41
Q

what is a precipitation reaction

A
  • occurs when 2 aqueous solutions containing ions react together to form an insoluble ionic solid called a precipitate
42
Q

how do transition metal ions aqueous solutions react with aqueous sodium hydroxide and aqueous ammonia

A
  • they react by forming precipitates
  • some of these will dissolve in excess sodium hydroxide or ammonia to form complex ions
43
Q

what are some examples of precipitates that do not dissolve in excess of aqueous sodium hydroxide

A

Cu(OH)2, Fe(OH)s, Fe(OH)3 and Mn(OH)2 do not disssolve in excess sodium hydroxide

44
Q

what can be seen when Fe2+ reacts with sodium hydroxide

write reaction

A
  • pale green solution reacts to form green precipitate of iron (II) hydroxide
  • precipitate is insoluble in excess sodium hydroxide but turns brown at its surface as Fe(II) is oxidised to Fe(III)
45
Q

what can be seen as Fe 3+ reacts with sodium hydroxide

write reaction

A
  • pale yellow solution reacts to form an orange-brown precipitate of iron (III) hydroxide
  • precipitate is insoluble in excess
46
Q

what can be seen if Mn2+ reacts with sodium hydroxide (NaOH)

write reaction

A
  • pale pink solution reacts to form light brown precipitate of manganese hydroxide
  • precipitate is insoluble in excess sodium hydroxide
47
Q

what be seen if chromium (III) Cr3+ is reacted with (aq) NaOH

write reaction

A
  • [Cr(H2O)6]3+ violet solution reacts to grey-green Cr(OH)3 precipitate
    ^is soluble in excess NaOH forms dark green [Cr(OH)6]3- solution
48
Q

How does Fe 2+ react with MnO4 -

what colour is the reactants and products

A
49
Q

How does Fe 3+ react with iodide ions

what colour are reactants and products

A
50
Q

what type of reaction is the reaction of Cu+ with hot dilute sulfuric acid

A
  • disproportionation reaction
51
Q

what’s the test for transition metal ions

A
  • aq NaOH producers precipitates with aq transition metal ions

Georges chem (29 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions