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Questions and Answers
Solutions can be stabilized by addition of ______ in order to prevent hydrolysis.
Solutions can be stabilized by addition of ______ in order to prevent hydrolysis.
acids
The reaction between Fe and S forms ______.
The reaction between Fe and S forms ______.
FeS
Sulphides of transition metals are usually ______ in colour.
Sulphides of transition metals are usually ______ in colour.
black
In a disproportionation reaction, a species is simultaneously ______ and oxidized.
In a disproportionation reaction, a species is simultaneously ______ and oxidized.
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The manganate(VI) ion MnO42- is stable in ______ medium.
The manganate(VI) ion MnO42- is stable in ______ medium.
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The cuprous ion decomposes to give ______ metal and cupric ion Cu2+.
The cuprous ion decomposes to give ______ metal and cupric ion Cu2+.
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Disproportionation is a type of ______ reaction.
Disproportionation is a type of ______ reaction.
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The reaction 3MnO42-(aq) + 4H+(aq) → 2MnO4-(aq) + MnO2(s) + 2H2O(l) is an example of ______.
The reaction 3MnO42-(aq) + 4H+(aq) → 2MnO4-(aq) + MnO2(s) + 2H2O(l) is an example of ______.
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Alloys of transition metals with non-transition metals such as ______ (copper-zinc) and bronze (copper-tin).
Alloys of transition metals with non-transition metals such as ______ (copper-zinc) and bronze (copper-tin).
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The transition metals and their compounds are known for their ______ activity.
The transition metals and their compounds are known for their ______ activity.
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The ability of the d-block metals to show variable ______ states enables the formation of unstable intermediate compounds.
The ability of the d-block metals to show variable ______ states enables the formation of unstable intermediate compounds.
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Transition metals also provide a suitable ______ for the reactions to occur.
Transition metals also provide a suitable ______ for the reactions to occur.
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The d-block elements are important ______ in industry and biological systems.
The d-block elements are important ______ in industry and biological systems.
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The alloys so formed are hard and have often high ______ points.
The alloys so formed are hard and have often high ______ points.
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D orbitals are filled before _____ orbitals in the same principal energy level
D orbitals are filled before _____ orbitals in the same principal energy level
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The _____ sphere is enclosed in brackets in formulas for complex species, and it includes the central metal ion plus the coordinated groups.
The _____ sphere is enclosed in brackets in formulas for complex species, and it includes the central metal ion plus the coordinated groups.
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In coordination chemistry, the donor atom of a ligand is the atom in the ligand that _____ an electron pair with the metal.
In coordination chemistry, the donor atom of a ligand is the atom in the ligand that _____ an electron pair with the metal.
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A coordinate covalent bond exists between _____ and CN- in the coordination compound K2[Cu(CN)4].
A coordinate covalent bond exists between _____ and CN- in the coordination compound K2[Cu(CN)4].
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The oxidation number of the central metal atom in the coordination compound [Pt(NH3)3Cl]Cl is _____.
The oxidation number of the central metal atom in the coordination compound [Pt(NH3)3Cl]Cl is _____.
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There are _____ types of d orbital.
There are _____ types of d orbital.
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The element that exhibits highest number of valences is ______.
The element that exhibits highest number of valences is ______.
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The element with the lowest atomization energy is ______.
The element with the lowest atomization energy is ______.
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The number of dative bonds to the central metal ion is its ______.
The number of dative bonds to the central metal ion is its ______.
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The element that has an equal number of paired and unpaired electrons in the valence shell is ______.
The element that has an equal number of paired and unpaired electrons in the valence shell is ______.
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The ion species that is susceptible to reduction is ______.
The ion species that is susceptible to reduction is ______.
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The compound in which chromium has one electron in the valence shell is ______.
The compound in which chromium has one electron in the valence shell is ______.
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The most stable oxidation state of ______ is +2.
The most stable oxidation state of ______ is +2.
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The anhydride of manganic acid is ______.
The anhydride of manganic acid is ______.
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The higher oxidation states are exhibited when ns and (n-1)d-______ take part in bonding.
The higher oxidation states are exhibited when ns and (n-1)d-______ take part in bonding.
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In the first transition series, ______ shows the maximum oxidation state of +7.
In the first transition series, ______ shows the maximum oxidation state of +7.
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The highest oxidation state shown by any transition metal is ______.
The highest oxidation state shown by any transition metal is ______.
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Ruthenium in second transition series and ______ in the third transition series show +8 oxidation state.
Ruthenium in second transition series and ______ in the third transition series show +8 oxidation state.
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In general, the minimum oxidation state shown by a transition metal is equal to the number of ______-electrons.
In general, the minimum oxidation state shown by a transition metal is equal to the number of ______-electrons.
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The maximum oxidation state shown by titanium is ______ (3d2 4s2).
The maximum oxidation state shown by titanium is ______ (3d2 4s2).
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For chromium and copper, the lowest oxidation state is ______.
For chromium and copper, the lowest oxidation state is ______.
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The common oxidation states for the elements from Fe to Ni are ______ or +3.
The common oxidation states for the elements from Fe to Ni are ______ or +3.
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Study Notes
Oxidation States of Transition Metals
- The lower oxidation state is exhibited when ns electrons participate in bonding, and higher oxidation states are exhibited when ns and (n-1)d-electrons take part in bonding.
- The highest oxidation state of transition metals increases with the increase of atomic number, reaches a maximum in the middle, and then decreases.
- Ruthenium in the second transition series and osmium in the third transition series show +8 oxidation state.
Factors Affecting Oxidation States
- The minimum oxidation state shown by a transition metal is equal to the number of ns-electrons.
- Except for scandium, the +2 oxidation state is the most common in the first transition series, due to the loss of 4s-electrons.
- Chromium and copper have a lowest oxidation state of +1, due to their electronic configurations.
Disproportionation
- Intermediate oxidation states have a tendency to disproportionate in a specific type of redox reaction, where a species is simultaneously reduced and oxidized to form two types of products.
- Example: The disproportionation of potassium manganate compound K2MnO4 in acidic aqueous solution.
Alloys of Transition Metals
- The alloys formed by transition metals are hard and have high melting points.
- Ferrous alloys containing chromium, vanadium, tungsten, molybdenum, and manganese are used in the production of steels and stainless steel.
- Alloys of transition metals with non-transition metals, such as brass (copper-zinc) and bronze (copper-tin), are also formed.
Catalytic Activity
- Transition metals and their compounds are known for their catalytic activity, due to their ability to show variable oxidation states and provide a suitable surface for reactions to occur.
- They enable reactions to proceed faster by providing an alternative reaction pathway of lower activation energy.
Coordination Chemistry
- In coordination chemistry, the donor atom of a ligand is the atom in the ligand that shares an electron pair with the metal.
- The coordination sphere is enclosed in brackets in formulas for complex species and includes the central metal ion plus the coordinated groups.
Properties of Transition Metals
- Transition metals are characterized by hardness, high melting points, and catalytic activity.
- They exhibit variable oxidation states, which enable them to form alloys and compounds with other metals and non-metals.
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Description
This quiz covers the oxidation states of transition elements, including how ns electrons and (n-1)d-electrons participate in bonding, and how the highest oxidation state changes within the transition series.
