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Questions and Answers
Which electronic configuration characteristic is most typical for d-block elements?
Which electronic configuration characteristic is most typical for d-block elements?
- Half-filled _p_ orbitals and completely filled _s_ orbitals.
- Random filling of _s_ and _d_ orbitals without any specific pattern.
- Complete filling of _s_ orbitals with two electrons, followed by gradual filling of _d_ orbitals. (correct)
- Complete filling of _p_ orbitals before filling _s_ orbitals.
Why are elements in group 12 (Zn, Cd, Hg) not considered transition metals, according to the definition provided?
Why are elements in group 12 (Zn, Cd, Hg) not considered transition metals, according to the definition provided?
- They react vigorously with water.
- They exhibit multiple oxidation states.
- They do not form colored compounds.
- They have completely filled _d_ orbitals in their ground state and common oxidation states. (correct)
What is the general valence shell electron configuration of d-block elements, according to the content?
What is the general valence shell electron configuration of d-block elements, according to the content?
- $(n-2)f^{1-14}(n-1)d^{0-1}ns^{2}$
- $ns^{2}np^{1-6}$
- $(n-1)d^{1-10}ns^{1-2}$ (correct)
- $(n-1)s^{2}p^{6}$
Chromium (Cr) exhibits an electron configuration of $[Ar]3d^54s^1$ instead of the expected $[Ar]3d^44s^2$. What is the most likely reason for this?
Chromium (Cr) exhibits an electron configuration of $[Ar]3d^54s^1$ instead of the expected $[Ar]3d^44s^2$. What is the most likely reason for this?
Copper (Cu) has an electron configuration of $[Ar]3d^{10}4s^1$. How does this configuration contribute to its chemical properties?
Copper (Cu) has an electron configuration of $[Ar]3d^{10}4s^1$. How does this configuration contribute to its chemical properties?
How many d-block elements are present in the fourth through seventh periods of the periodic table?
How many d-block elements are present in the fourth through seventh periods of the periodic table?
Vanadium (V) has an electron configuration of $[Ar]3d^34s^2$. Based on this information and the provided data, what are the possible oxidation states of Vanadium?
Vanadium (V) has an electron configuration of $[Ar]3d^34s^2$. Based on this information and the provided data, what are the possible oxidation states of Vanadium?
Manganese (Mn) is listed as having an electron configuration of $[Ar]3d^54s^2$. What implications does this have regarding its possible oxidation states?
Manganese (Mn) is listed as having an electron configuration of $[Ar]3d^54s^2$. What implications does this have regarding its possible oxidation states?
How does electronegativity generally change across the 3d series (Sc to Zn)?
How does electronegativity generally change across the 3d series (Sc to Zn)?
What distinguishes d-block elements from other elements in the periodic table?
What distinguishes d-block elements from other elements in the periodic table?
Flashcards
What are d-block elements?
What are d-block elements?
Elements in which valence electrons are in the ns1-2 a (n-1) d1-10 orbitals, where n is 4 to 7.
Where are d-block elements located?
Where are d-block elements located?
d-block elements found between the s and p blocks.
What is the general electron configuration of d-block elements?
What is the general electron configuration of d-block elements?
Generally, (n-1)dx nsx, where x + y is the group number.
What are transition elements?
What are transition elements?
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Which elements are not transition elements?
Which elements are not transition elements?
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What is stable electron configuration for d-elements?
What is stable electron configuration for d-elements?
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Why is chromium an exception?
Why is chromium an exception?
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Why is copper an exception?
Why is copper an exception?
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Study Notes
- d-elements are those in which the valence electrons are located in the ns1-2 a (n-1) d1-10 orbitals, where n is 4 to 7 (period number).
- These elements are found in groups 3 to 12 of the periodic table.
- In the periodic table, d-elements are located between the s-block and p-block elements.
- d-element atoms generally have a valence layer electron configuration of (n-1)dx nsx, where the sum of x + y gives the order number of the group in which the element is located.
- d-elements are also called transition elements, because in the unbound state or in some of their oxidation states, they have incompletely occupied d-orbitals.
- According to this definition, the elements of group 12 (Zn, Cd, Hg) do not belong to the transition elements, because their d-orbitals are completely filled.
- However, their properties are very similar to transition elements.
- d-elements are located in the fourth to seventh periods of the periodic table, there are forty of them.
d-elements in the Periodic Table
- The d-elements in the periodic table are shown.
Electronic Configuration of d-element Atoms
- A characteristic feature of the electronic configuration of d-element atoms is that the electronic configurations in which the s orbitals are filled with two electrons and the d orbitals gradually, are stable for them.
- Atoms of chromium and copper are exceptions.
- For a chromium atom, it is energetically more advantageous if there is one electron in the 4s orbital and the d orbitals are half-filled.
- A chromium atom has a smaller energy value with the electronic configuration [Ar]3d54s¹ than with the configuration [Ar]3d44s².
- For a copper atom, it is energetically more advantageous if the d-orbitals are fully occupied and the 4s-orbital contains only one electron [Ar]3d104s1 and not [Ar]3d94s².
- In the case of 4d to 6d elements, there are even more exceptions.
Basic Characteristics of 3d-elements
| Symbol | Slovak name | Z | Electronic configuration of the atom | Electronegativity (Pauling) | Molar mass/ g·mol-1 | Melting point/°C | Boiling point/°C | Density/ g·cm-3 |
|---|---|---|---|---|---|---|---|---|
| Sc | Scandium | 21 | [Ar]3d¹4s² | 1.4 | 44.956 | 1539 | 3.00 | |
| Ti | Titanium | 22 | [Ar]3d²4s² | 1.5 | 47.867 | 1668 | 4.51 | |
| V | Vanadium | 23 | [Ar]3d³4s² | 1.6 | 50.942 | 1900 | 6.10 | |
| Cr | Chromium | 24 | [Ar]3d⁵4s¹ | 1.66 | 51.996 | 1857 | 7.19 | |
| Mn | Manganese | 25 | [Ar]3d⁵4s² | 1.55 | 54.938 | 1245 | 7.43 | |
| Fe | Iron | 26 | [Ar]3d⁶4s² | 1.8 | 55.845 | 1535 | 7.86 | |
| Co | Cobalt | 27 | [Ar]3d⁷4s² | 1.9 | 58.933 | 1495 | 8.90 | |
| Ni | Nickel | 28 | [Ar]3d⁸4s² | 1.9 | 58.693 | 1453 | 8.90 | |
| Cu | Copper | 29 | [Ar]3d¹⁰4s¹ | 1.9 | 63.546 | 1083 | 8.96 | |
| Zn | Zinc | 30 | [Ar]3d¹⁰4s² | 1.65 | 65.38 | 419.5 | 7.14 |
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