D- and F-Block Elements Quiz
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Questions and Answers

What characteristic is primarily responsible for the variety of oxidation states in transition elements?

  • Completely filled d orbitals
  • Presence of s electrons
  • Partly filled d orbitals (correct)
  • High electronegativity

Which property is NOT typically associated with transition metals?

  • High ionization energies (correct)
  • Formation of colored ions
  • Paramagnetic behavior
  • Catalytic activity

Why is zinc not considered a transition element?

  • It does not form complexes.
  • It has no d electrons.
  • It has a completely filled 3d orbital. (correct)
  • It is an alkaline earth metal.

What trend is observed among transition elements compared to main group elements?

<p>Greater horizontal similarities (B)</p> Signup and view all the answers

Which of the following is NOT a characteristic property of transition metals?

<p>High reduction potentials (C)</p> Signup and view all the answers

Which series of transition metals does not include elements whose d orbitals are progressively filled?

<p>3f series (C)</p> Signup and view all the answers

Which of the following elements is not considered a transition element?

<p>Zinc (B)</p> Signup and view all the answers

What do the f-block elements primarily contribute to in modern technology?

<p>Nuclear energy (B)</p> Signup and view all the answers

What is the primary characteristic of the d-block elements?

<p>They consist of groups 3-12. (D)</p> Signup and view all the answers

What oxidation state is most commonly exhibited by transition metals?

<p>Variable oxidation states (A)</p> Signup and view all the answers

Which pair of elements constitutes the inner transition metals?

<p>Thorium and Uranium (B)</p> Signup and view all the answers

Which of the following compounds is not typically associated with the d-block elements?

<p>NaCl (D)</p> Signup and view all the answers

Which of the following best describes the arrangement of f-block elements within the periodic table?

<p>Separated to form a distinct block (C)</p> Signup and view all the answers

Which series of inner transition metals begins with Ac?

<p>Actinoids (B)</p> Signup and view all the answers

Which elements are not regarded as transition metals due to their filled d orbitals?

<p>Zinc, cadmium, and mercury (B)</p> Signup and view all the answers

Which of the following is true about transition elements?

<p>They must have incompletely filled d orbitals in at least one oxidation state. (A)</p> Signup and view all the answers

Which group of metals includes silver, gold, and platinum?

<p>Precious metals (C)</p> Signup and view all the answers

What do the presence of partly filled d or f orbitals allow in transition elements?

<p>Wider range of oxidation states and complex formation (A)</p> Signup and view all the answers

How can the usual theory of valence be applied to transition elements?

<p>It can be applied successfully, similar to main group elements. (B)</p> Signup and view all the answers

Which metals are considered industrially important among transition metals?

<p>Iron, copper, and titanium (B)</p> Signup and view all the answers

What is the outer electronic configuration of Chromium (Cr)?

<p>4s^2 3d^5 (B)</p> Signup and view all the answers

What is unique about the electronic configuration of the first row (3d) transition metals?

<p>They have partially filled d orbitals. (B)</p> Signup and view all the answers

Which element has the electronic configuration of 5s^2 4d^10?

<p>Cadmium (Cd) (A)</p> Signup and view all the answers

Which of the following correctly identifies the characteristics of transition elements?

<p>They often form colored compounds and possess variable oxidation states. (D)</p> Signup and view all the answers

Why is the study of transition metals significant compared to main group elements?

<p>Their chemistry is more complex due to variable oxidation states. (A)</p> Signup and view all the answers

Which of the following elements is not regarded as a transition element?

<p>Mercury (Hg) (C)</p> Signup and view all the answers

Which element has the highest number of 3d electrons in the first series of transition elements?

<p>Nickel (Ni) (A)</p> Signup and view all the answers

What is the electronic configuration of Silver (Ag)?

<p>5s^1 4d^10 (B)</p> Signup and view all the answers

In terms of electronic configuration, which element has one electron in the 5s subshell?

<p>Molybdenum (Mo) (C)</p> Signup and view all the answers

What is the outer electronic configuration of Yttrium (Y)?

<p>5s^2 4d^1 (C)</p> Signup and view all the answers

Which of the following correctly describes the 4d orbital configuration of Ruthenium (Ru)?

<p>5 (C)</p> Signup and view all the answers

How many d electrons does Manganese (Mn) have?

<p>5 (D)</p> Signup and view all the answers

What is the general electronic configuration of the d-block transition elements?

<p>(n-1)d1–10 ns1–2 (B)</p> Signup and view all the answers

Which transition element configuration is an exception to the standard electronic configuration rules?

<p>3d5 4s1 (A)</p> Signup and view all the answers

What energy level do the d-block metals occupy in relation to the periodic table?

<p>They are flanked by s- and p-block elements. (C)</p> Signup and view all the answers

Why do exceptions occur in the electronic configurations of certain transition metals?

<p>The (n-1)d and ns orbitals have a very small energy difference. (A)</p> Signup and view all the answers

What is the electron configuration of copper (Cu)?

<p>3d10 4s1 (B)</p> Signup and view all the answers

How many electron(s) can the outermost ns orbital of the transition elements accommodate?

<p>1 or 2 electrons (A)</p> Signup and view all the answers

What series of transition elements is still considered incomplete?

<p>6d series (D)</p> Signup and view all the answers

Which statement best describes the position of d-block elements in the periodic table?

<p>They are positioned in the middle of the table. (C)</p> Signup and view all the answers

Which of the following is a characteristic of transition metals?

<p>They have high oxidation states. (C)</p> Signup and view all the answers

Why are half-filled and completely filled sets of orbitals considered more stable?

<p>They have lower energy configurations. (C)</p> Signup and view all the answers

Flashcards

d-block elements

Elements in the periodic table's groups 3-12 where the d orbitals are progressively filled.

f-block elements

Elements in the periodic table where the 4f and 5f orbitals are progressively filled in the latter two long periods.

Transition metals

Elements of the d-block.

Inner Transition Metals

Elements of the f-block.

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Electronic Configuration

The arrangement of electrons in the orbitals of an atom.

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Oxidation States

Different positive charges an element can have in a compound.

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Lanthanides

Elements in the 4f series of the f-block.

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Actinides

Elements in the 5f series of the f-block.

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Transition Elements Definition

Elements with incompletely filled d orbitals in their ground state or any oxidation state.

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Zinc, Cadmium, Mercury

Not considered transition metals because they have completely filled d orbitals.

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Occurrence

The natural abundance and distribution of an element.

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General Characteristics

Common properties of a group of elements like high melting and boiling points, variable oxidation states etc.

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Valence Theory

A theory used to understand the chemical bonding

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Transition Elements

Elements in the d-block of the periodic table, positioned between s- and p-block elements.

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d-block

The section of the periodic table containing transition elements.

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Electronic Configuration (general)

The arrangement of electrons in the atoms of the transition elements; typically (n-1)d^1-10 ns^1-2.

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n-1

Refers to the inner d orbitals in an atom's electron configuration.

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ns

Refers to the outermost s orbitals in an atom's electron configuration.

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3d,4d,5d Series

Series of transition metals where the d-orbitals in the atoms of the third, fourth and fifth rows of the transition metal blocks, respectively, receive electrons.

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Electronic Configuration Exception (Cr)

Chromium's electron configuration (3d5 4s1) deviates from the general rule due to the stabilization of half-filled orbitals.

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Electronic Configuration Exception (Cu)

Copper's electron configuration (3d10 4s1) deviates from the general rule due to the stabilization of completely filled orbitals.

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Stability of Configurations

Electron configurations are more stable when the d and s orbitals are either half filled or completely filled.

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Penultimate Energy Level

The energy level before the outermost energy level in an atom.

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Transition Element Defining Feature

Transition elements have a partially filled d orbital in their ground state or any common oxidation state.

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Transition Element Properties

Transition elements exhibit diverse properties like variable oxidation states, colored ions, complex formation, catalytic activity, and paramagnetism due to their partially filled d orbitals.

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Transition Element vs. Main Group Elements

Transition elements show greater similarities within a horizontal row (period) than main group elements.

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Why is Scandium a Transition Element?

Scandium has a partially filled 3d orbital in its ground state (3d1), making it a transition element.

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Why is Zinc NOT a Transition Element?

Zinc has a completely filled 3d orbital in both its ground state and its oxidized state, disqualifying it as a transition element.

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General Electronic Configuration

The general formula that represents the electronic configuration of most transition elements. It is (n-1)d1-10 ns 1-2.

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Zn, Cd, Hg

These elements are not considered transition elements even though they are in the d-block. They have completely filled d and s orbitals in both their ground state and common oxidation states.

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1st Series

The first row of transition elements in the periodic table, from Scandium (Sc) to Zinc (Zn).

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2nd Series

The second row of transition elements in the periodic table, from Yttrium (Y) to Cadmium (Cd).

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3rd Series

The third row of transition elements in the periodic table, from Lanthanum (La) to Mercury (Hg).

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4th Series

The fourth row of transition elements in the periodic table, from Actinium (Ac) to Ununbium (Uub).

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Electronic Configuration (Sc)

Sc has an electronic configuration of [Ar] 3d1 4s2, where the 3d orbital has one electron and the 4s orbital has two electrons.

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Electronic Configuration (Ti)

Ti has an electronic configuration of [Ar] 3d2 4s2, where the 3d orbital has two electrons and the 4s orbital has two electrons.

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Electronic Configuration (V)

V has an electronic configuration of [Ar] 3d3 4s2, where the 3d orbital has three electrons and the 4s orbital has two electrons.

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Study Notes

D- and F-Block Elements

  • Transition elements (iron, copper, silver, gold) have been crucial to human development and are important sources of nuclear energy
  • The d-block elements (groups 3-12) have progressively filled d orbitals in the four long periods
  • The f-block elements involve filling 4f and 5f orbitals in the last two long periods.
  • They're conventionally part of group 3, but are separate in the table
  • "Transition metals" and "inner transition metals" refer to d- and f-block elements respectively

Electronic Configurations

  • Transition elements' general electronic configuration is (n-1)d1-10ns1-2
  • The (n-1) refers to the inner d orbitals, which can contain 1 to 10 electrons
  • The outermost ns orbital can have 1 or 2 electrons
  • Exceptions exist due to slight energy differences between (n-1)d and ns orbitals, leading to more stable half- or completely filled orbitals

Transition Metal Series

  • There are three main transition metal series: 3d (Sc to Zn), 4d (Y to Cd), and 5d (La to Hg, omitting Ce to Lu)
  • A 6d series (starting with Ac) is incomplete
  • Lanthanides (4f) and Actinides (5f) are inner transition series
  • Transition elements are defined by incompletely filled d orbitals (either in ground state or oxidation states)
  • Elements Zn, Cd, and Hg, despite being in group 12, are not considered transition metals since they have completely filled d orbitals (in ground and oxidation states).

General Properties

  • Transition elements have varying oxidation states.
  • Formation of colored ions.
  • Entering into complex compound formations with diverse ligands
  • Catalytic properties
  • Paramagnetic behaviour
  • Greater horizontal similarities in properties compared to the main group elements
  • Show some group similarities as well

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Related Documents

Unit 8: The d- and f-Block Elements PDF

Description

Test your knowledge on the d- and f-block elements, including transition metals and their electronic configurations. Understand the significance of these elements in human development and their roles in nuclear energy. Dive into the details of transition metal series and their properties.

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