4: d-Block Metal Chemistry
- Page ID
- 428428
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)The d-block elements are found in groups 3, 4, 5, 6, 7, 8, 9, 10, 11, and 12 of the periodic table; d-block elements are also known as the transition metals. The d orbital is filled with the electronic shell “n-1.”
- 4.1: Properties of Transition Metals
- 4.1.1: A Brief Survey of Transition-Metal Chemistry
- 4.1.2: Electron Configuration of Transition Metals
- 4.1.3: General Trends among the Transition Metals
- 4.1.4: Introduction to Transition Metals I
- 4.1.5: Introduction to Transition Metals II
- 4.1.6: Metallurgy
- 4.1.6.1: An Introduction to the Chemistry of Metal Extraction
- 4.1.6.2: The Extraction of Copper
- 4.1.6.3: The Extraction of Iron
- 4.1.6.3.1: Iron Production
- 4.1.6.4: The Extraction of Silver
- 4.1.6.4.1: Preparation and uses of Silver chloride and Silver nitrate
- 4.1.7: Oxidation States of Transition Metals
- 4.1.8: Transition Metals in Biology
- 4.2: Group 3 Transition Metals
- The observed trends in the properties of the group 3 elements are similar to those of groups 1 and 2. Due to their ns2(n − 1)d1 valence electron configurations, the chemistry of all four elements is dominated by the +3 oxidation state formed by losing all three valence electrons. As expected based on periodic trends, these elements are highly electropositive metals and powerful reductants, with La (and Ac) being the most reactive.
- 4.3: Group 4 Transition Metals
- Because the elements of group 4 have a high affinity for oxygen, all three metals occur naturally as oxide ores that contain the metal in the +4 oxidation state resulting from losing all four ns2(n − 1)d2 valence electrons.
- 4.4: Group 5 Transition Metals
- All group 5 metals are normally found in nature as oxide ores that contain the metals in their highest oxidation state (+5). Because of the lanthanide contraction, the chemistry of Nb and Ta is so similar that these elements are usually found in the same ores.
- 4.5: Group 6 Transition Metals
- The group 6 metals are slightly less electropositive than those of the three preceding groups, and the two heaviest metals are essentially the same size because of the lanthanide contraction.
- 4.6: Group 7 Transition Metals
- All three group 7 elements have seven valence electrons and can form compounds in the +7 oxidation state. The chemistry of the group 7 metals (Mn, Tc, and Re) is dominated by lower oxidation states. Compounds in the maximum possible oxidation state (+7) are readily reduced.
- 4.7: Group 8 Transition Metals
- The chemistry of groups 8, 9, and 10 is dominated by intermediate oxidation states such as +2 and +3.
- 4.8: Group 9 Transition Metals
- All group 9 elements are relatively rare in the earth's crust, with the most abundant, cobalt, only accounting for 0.0029% of the Earth's crust. Rhodium and iridium are two of the rarest naturally occurring elements in the earth, only found in platinum ores.
- 4.9: Group 10 Transition Metals
- Group 10 metals are white to light grey in color, and possess a high luster, a resistance to tarnish (oxidation), are highly ductile, and enter into oxidation states of +2 and +4, with +1 being seen in special conditions.
- 4.10: Group 11 Transition Metals
- The “coinage metals”, copper, silver, and gold, have held great importance in societies throughout history, both symbolically and practically. For centuries, silver and gold have been worn by royalty to parade their wealth and power. On occasion, these metals were even used in art. Although the most important oxidation state for group 11 is +1, the elements are relatively unreactive, with reactivity decreasing from Cu to Au.
- 4.11: Group 12 Transition Metals
- Group 12 elements have partially filled (n − 1)d subshells, and hence are not, strictly speaking, transition metals. Nonetheless, much of their chemistry is similar to that of the elements that immediately precede them in the d block. The group 12 metals are similar in abundance to those of group 11, and they are almost always found in combination with sulfur. Group 12 metals tend have low melting and boiling points (due to the weak metallic bonding of the ns2 electrons) and charges of +2 or +1.
- 4.1: Properties of Transition Metals
- 4.1.1: A Brief Survey of Transition-Metal Chemistry
- 4.1.2: Electron Configuration of Transition Metals
- 4.1.3: General Trends among the Transition Metals
- 4.1.4: Introduction to Transition Metals I
- 4.1.5: Introduction to Transition Metals II
- 4.1.6: Metallurgy
- 4.1.6.1: An Introduction to the Chemistry of Metal Extraction
- 4.1.6.2: The Extraction of Copper
- 4.1.6.3: The Extraction of Iron
- 4.1.6.3.1: Iron Production
- 4.1.6.4: The Extraction of Silver
- 4.1.6.4.1: Preparation and uses of Silver chloride and Silver nitrate
- 4.1.7: Oxidation States of Transition Metals
- 4.1.8: Transition Metals in Biology
- 4.2: Group 3 Transition Metals
- The observed trends in the properties of the group 3 elements are similar to those of groups 1 and 2. Due to their ns2(n − 1)d1 valence electron configurations, the chemistry of all four elements is dominated by the +3 oxidation state formed by losing all three valence electrons. As expected based on periodic trends, these elements are highly electropositive metals and powerful reductants, with La (and Ac) being the most reactive.
- 4.3: Group 4 Transition Metals
- Because the elements of group 4 have a high affinity for oxygen, all three metals occur naturally as oxide ores that contain the metal in the +4 oxidation state resulting from losing all four ns2(n − 1)d2 valence electrons.
- 4.4: Group 5 Transition Metals
- All group 5 metals are normally found in nature as oxide ores that contain the metals in their highest oxidation state (+5). Because of the lanthanide contraction, the chemistry of Nb and Ta is so similar that these elements are usually found in the same ores.
- 4.5: Group 6 Transition Metals
- The group 6 metals are slightly less electropositive than those of the three preceding groups, and the two heaviest metals are essentially the same size because of the lanthanide contraction.
- 4.6: Group 7 Transition Metals
- All three group 7 elements have seven valence electrons and can form compounds in the +7 oxidation state. The chemistry of the group 7 metals (Mn, Tc, and Re) is dominated by lower oxidation states. Compounds in the maximum possible oxidation state (+7) are readily reduced.
- 4.7: Group 8 Transition Metals
- The chemistry of groups 8, 9, and 10 is dominated by intermediate oxidation states such as +2 and +3.
- 4.8: Group 9 Transition Metals
- All group 9 elements are relatively rare in the earth's crust, with the most abundant, cobalt, only accounting for 0.0029% of the Earth's crust. Rhodium and iridium are two of the rarest naturally occurring elements in the earth, only found in platinum ores.
- 4.9: Group 10 Transition Metals
- Group 10 metals are white to light grey in color, and possess a high luster, a resistance to tarnish (oxidation), are highly ductile, and enter into oxidation states of +2 and +4, with +1 being seen in special conditions.
- 4.10: Group 11 Transition Metals
- The “coinage metals”, copper, silver, and gold, have held great importance in societies throughout history, both symbolically and practically. For centuries, silver and gold have been worn by royalty to parade their wealth and power. On occasion, these metals were even used in art. Although the most important oxidation state for group 11 is +1, the elements are relatively unreactive, with reactivity decreasing from Cu to Au.
- 4.11: Group 12 Transition Metals
- Group 12 elements have partially filled (n − 1)d subshells, and hence are not, strictly speaking, transition metals. Nonetheless, much of their chemistry is similar to that of the elements that immediately precede them in the d block. The group 12 metals are similar in abundance to those of group 11, and they are almost always found in combination with sulfur. Group 12 metals tend have low melting and boiling points (due to the weak metallic bonding of the ns2 electrons) and charges of +2 or +1.