Question 1

Oxides of metals in higher oxidation states tend to be basic.

Accepted Answer

Oxides of metals in higher oxidation states tend to be acidic or amphoteric, not basic. Basicity decreases as the oxidation state of the metal increases.

Question 2

Which of the following metals has the smallest atomic radius?
A) W
B) Co
C) Ta
D) Ag
E) V

Accepted Answer

Cobalt (Co) has the smallest atomic radius among the options given. Atomic radius generally decreases across a period from left to right in the periodic table due to the increase in nuclear charge, which pulls the electrons closer to the nucleus. Cobalt is located to the right of vanadium (V) and thus has a smaller atomic radius than vanadium. Tungsten (W), tantalum (Ta), and silver (Ag) are located in periods below cobalt, and elements generally have larger atomic radii as you move down a group due to the addition of electron shells.

Question 3

The transition metals exhibit significant horizontal similarities in chemistry.

Accepted Answer

The transition metals all have similar properties due to their partially filled d-orbitals, leading to similar chemical behavior across the horizontal rows (periods) of the periodic table.

Question 4

The metals in the lower right corner of the d-block are often called the _____.

Accepted Answer

The answer of The metals in the lower right corner...

Question 5

The electronic configuration of chromium is _____.

Accepted Answer

The answer of The electronic configuration of chromium is _____....

Question 6

Higher oxidation states become more stable across the $d$-block.

Accepted Answer

Higher oxidation states become less stable across the $d$-block from left to right due to increasing nuclear charge, which strengthens the attraction between the nucleus and the electrons, making it harder to remove electrons and thus favoring lower oxidation states.

Question 7

The group 3 elements are powerful reductants.

Accepted Answer

Group 3 elements such as aluminum and boron are known to be powerful reductants as they readily donate electrons to other compounds or elements, leading to their reduction.

Question 8

The transition metals become more reactive from left to right across a row.

Accepted Answer

The transition metals actually become less reactive from left to right across a row due to increasing effective nuclear charge, which makes it harder for the outer electrons to be removed.

Question 9

Why are the transition metals paramagnetic?

Accepted Answer

The answer of Why are the transition metals paramagnetic?...

Question 10

Why do the coinage metals exhibit significant noble character?

Accepted Answer

The answer of Why do the coinage metals exhibit significant...

Question 11

Which of the following elements has the highest electrical conductivity?
A) Sc
B) Au
C) Re
D) Nb
E) Cr

Accepted Answer

Gold (Au) has the highest electrical conductivity among the options listed. It is well known for its excellent conductivity of electricity and heat, making it a valuable material in electronics, jewelry, and various industrial applications.

Question 12

Which of the following metals has the largest atomic radius?
A) Y
B) Tc
C) Ru
D) Rh
E) Zr

Accepted Answer

The answer of Which of the following metals has the...

Question 13

The group 4 transition metals have limited commercial applications.

Accepted Answer

The group 4 transition metals, including titanium, zirconium, and hafnium, have various commercial applications such as in aerospace, biomedical implants, and chemical processing.

Question 14

In transition metals, the ns electrons are always lost before the (n-1)d electrons.

Accepted Answer

In transition metals, the ns electrons are typically lost before the (n-1)d electrons because the ns electrons are higher in energy and further from the nucleus compared to the (n-1)d electrons.

Question 15

The transition metals Nb, Tc, and Mo, when arranged in the increasing order of their electrical conductivities follow the order:
A) Nb < Tc < Mo.
B) Nb < Mo < Tc.
C) Mo < Tc < Nb.
D) Tc < Mo < Nb.
E) Mo < Nb < Tc.

Accepted Answer

The answer of The transition metals Nb, Tc, and Mo,...

Question 16

Which of the following metals has a significant noble character?
A) Titanium
B) Niobium
C) Tantalum
D) Platinum
E) Hafnium

Accepted Answer

Platinum is known as one of the most noble metals due to its high resistance to corrosion and chemical attack, as well as its stability in harsh environments. This makes it an ideal choice for use in jewelry, electronic components, and medical implants.

Question 17

The size of neutral atoms of the d-block elements _____ from left to right across a row, with increasing atomic number.

Accepted Answer

The answer of The size of neutral atoms of the...

Question 18

The electronic configuration of copper is 4s²3d⁹.

Accepted Answer

The correct electronic configuration for copper is 1s2 2s2 2p6 3s2 3p6 4s1 3d10. The given configuration in the question is incorrect.

Question 19

The ions Sc³⁺, Mn³⁺, and Cr³⁺ when arranged in the increasing order of their ionic radius, follow the order _____. A) Sc³⁺ < Mn³⁺ < Cr³⁺ B) Cr³⁺ < Mn³⁺ < Sc³⁺ C) Mn³⁺ < Cr³⁺ < Sc³⁺ D) Cr³⁺ < Sc³⁺ < Mn³⁺ E) Sc³⁺ < Cr³⁺ < Mn³⁺

Accepted Answer

The trend in ionic radii is generally determined by the effective nuclear charge (the number of protons in the nucleus) and the electron configuration of the ion. As we move from left to right across a period in the periodic table, both the effective nuclear charge and the number of electrons in the outermost shell increase, resulting in a smaller ionic radius.

In this case, Sc, Mn, and Cr are all transition metals that are located in the same period of the periodic table (row 4). Therefore, the trend in ionic radii is largely determined by the effective nuclear charge of each ion.

Sc3+ has 21 protons in its nucleus, Mn3+ has 25, and Cr3+ has 24. Therefore, the effective nuclear charge increases in the order Sc3+ < Cr3+ < Mn3+. This suggests that the trend in ionic radii should be Mn3+ < Cr3+ < Sc3+ with Mn3+ having the smallest ionic radius and Sc3+ having the largest ionic radius.

Since the question is asking for the trend in increasing order of ionic radius, we need to reverse the trend we just found. Therefore, the correct answer is that the trend in ionic radii for Sc3+, Mn3+, and Cr3+ is Sc3+ < Cr3+ < Mn3+.

Question 20

The transition metals are generally characterized by partially filled _____ subshells in the free elements or their cations.

Accepted Answer

The answer of The transition metals are generally characterized by...

Quiz 23: The D-Block Elements

Oxides of metals in higher oxidation states tend to be basic.

Which of the following metals has the smallest atomic radius?

The transition metals exhibit significant horizontal similarities in chemistry.

The metals in the lower right corner of the d-block are often called the _____.

The electronic configuration of chromium is _____.

Higher oxidation states become more stable across the $d$ -block.

The group 3 elements are powerful reductants.

The transition metals become more reactive from left to right across a row.

Why are the transition metals paramagnetic?

Why do the coinage metals exhibit significant noble character?

Which of the following elements has the highest electrical conductivity?

Which of the following metals has the largest atomic radius?

The group 4 transition metals have limited commercial applications.

In transition metals, the ns electrons are always lost before the (n-1)d electrons.

The transition metals Nb, Tc, and Mo, when arranged in the increasing order of their electrical conductivities follow the order:

Which of the following metals has a significant noble character?

The size of neutral atoms of the d-block elements _____ from left to right across a row, with increasing atomic number.

The electronic configuration of copper is 4s²3d⁹.

The ions Sc³⁺, Mn³⁺, and Cr³⁺ when arranged in the increasing order of their ionic radius, follow the order _____.

The transition metals are generally characterized by partially filled _____ subshells in the free elements or their cations.

Quiz 23: The D-Block Elements

Oxides of metals in higher oxidation states tend to be basic.

Which of the following metals has the smallest atomic radius?

The transition metals exhibit significant horizontal similarities in chemistry.

The metals in the lower right corner of the d-block are often called the _____.

The electronic configuration of chromium is _____.

Higher oxidation states become more stable across the ddd -block.

The group 3 elements are powerful reductants.

The transition metals become more reactive from left to right across a row.

Why are the transition metals paramagnetic?

Why do the coinage metals exhibit significant noble character?

Which of the following elements has the highest electrical conductivity?

Which of the following metals has the largest atomic radius?

The group 4 transition metals have limited commercial applications.

In transition metals, the ns electrons are always lost before the (n-1)d electrons.

The transition metals Nb, Tc, and Mo, when arranged in the increasing order of their electrical conductivities follow the order:

Which of the following metals has a significant noble character?

The size of neutral atoms of the d-block elements _____ from left to right across a row, with increasing atomic number.

The electronic configuration of copper is 4s23d9.

The ions Sc3+, Mn3+, and Cr3+ when arranged in the increasing order of their ionic radius, follow the order _____.

The transition metals are generally characterized by partially filled _____ subshells in the free elements or their cations.

Higher oxidation states become more stable across the $d$ -block.

The electronic configuration of copper is 4s²3d⁹.

The ions Sc³⁺, Mn³⁺, and Cr³⁺ when arranged in the increasing order of their ionic radius, follow the order _____.