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XI Chem _New Chapter-3 Periodic Classification of Elements[True or False Statement Questions]
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XI_Chem_New Chap-3_Periodic Classification of Elements_[True or False Statement Questions]Sl # Statements [3.0 Introduction _ Need to classify elements; Genesis of periodic classificaiton] TRUE/FALSE
Dmitri Mendeleev's Periodic Law was based on the color of elements rather than their atomic
1 FALSE
weights. (Skill Level: 2)
Dmitri Mendeleev's Periodic Law, stating that elements' properties depend on their atomic
2 TRUE
weights, led to the Modern Periodic Table.
Isotopes of an element have identical chemical properties due to variations in the number of
3 FALSE
protons in their nuclei. (Skill Level: 4)
Johann Dobereiner observed similarities in physical and chemical properties among groups of
4 TRUE
three elements, known as Triads.
John Alexander Newlands proposed the Law of Octaves, noting similarities among every eighth
5 TRUE
element, although it was limited in scope.
John Alexander Newlands proposed the Law of Octaves, which perfectly described the behavior of
6 FALSE
all elements. (Skill Level: 3)
Lothar Meyer's table of elements based on atomic weights resembled the Modern Periodic Table,
7 TRUE
providing an early visualization of periodic trends.
Mendeleev arranged elements by atomic weight, placing those with similar properties together
8 TRUE
and predicting undiscovered elements.
Mendeleev arranged elements haphazardly on the table without considering their properties.
9 FALSE
(Skill Level: 2)
Mendeleev's genius lay in predicting properties of undiscovered elements like gallium and
10 TRUE
germanium, demonstrating the Table's predictive utility in chemistry.
11 Mendeleev's Periodic Table arranged elements by properties and atomic weights, predicting TRUE
missing elements, setting a foundation for understanding element relationships and behaviors.
Mendeleev's Periodic Table was disorganized and failed to predict any missing elements. (Skill
12 FALSE
Level: 2)
Mendeleev's predictions for gallium and germanium, including atomic weight and properties,
13 TRUE
were validated by their later discovery.
Scientists classified elements systematically to rationalize chemical facts, predict new properties,
14 TRUE
and facilitate further study.
Scientists randomly classified elements, leading to the organization of the Periodic Table. (Skill
15 FALSE
Level: 3)
The Modern Periodic Table categorizes elements arbitrarily, with no basis in properties or atomic
16 FALSE
weights. (Skill Level: 2)
The Modern Periodic Table, developed primarily by Mendeleev, categorizes elements into rows
17 TRUE
and columns based on properties and atomic weights, aiding chemical understanding.
The Periodic Table, a fundamental concept in chemistry, organizes elements based on atomic
18 TRUE
weights, enabling predictions of their properties.
The Periodic Table's development had no connection to Dobereiner's triads, Newlands' octaves,
19 FALSE
or Mendeleev's work. (Skill Level: 3)
The Periodic Table's development involved Dobereiner's triads, Newlands' octaves, and
20 TRUE
Mendeleev's arrangement, revealing periodic relationships among elements.
1 OF 8 RI_Best Wishes
, XI_Chem_New Chap-3_Periodic Classification of Elements_[True or False Statement Questions]
Statements [3.3 Modern Periodic Law, 3.4 Nomenclature of Elements with Atomic Numbers >
Sl # TRUE/FALSE
100, 3.5 Electronic Configuration, and the Periodic Table]
The Modern Periodic Law states that the physical and chemical properties of elements are
1 TRUE
periodic functions of their atomic numbers.
Elements in the same group or family in the Periodic Table have similar valence shell electronic
2 TRUE
configurations and exhibit similar chemical behavior.
Hydrogen is placed separately at the top of the Periodic Table because it has only one s-electron
3 TRUE
and can exhibit properties of both alkali metals and halogens.
Elements in the s-block, p-block, d-block, and f-block are categorized based on the type of atomic
4 TRUE
orbitals being filled with electrons.
The Periodic Table consists of seven periods, each corresponding to the highest principal quantum
5 TRUE
number (n) of the elements in that period.
The lanthanoid series, also known as the 4f-inner transition series, starts with cerium (Z = 58) and
6 TRUE
ends at lutetium (Z = 71).
Lanthanoids and actinoids, which are part of the 6th and 7th periods, respectively, are placed
7 TRUE
separately in the Periodic Table as the 4f and 5f inner transition series.
The atomic number of an element corresponds to the number of protons in its nucleus, reflecting
8 TRUE
the element's quantum configuration.
The 3d transition series of elements begins with scandium (Z = 21) and continues until zinc (Z =
9 TRUE
30).
Helium, although strictly belonging to the s-block, is positioned in the p-block along with other
10 TRUE
noble gases due to its completely filled valence shell.
The IUPAC provides a systematic nomenclature for elements with atomic numbers above 100,
11 TRUE
using numerical roots and adding "ium" at the end.
Elements within the same group or family on the Periodic Table may have vastly different valence
12 FALSE
shell electronic configurations, leading to diverse chemical behaviors.
Hydrogen's unique position on the Periodic Table results from its extreme reactivity, causing it to
13 FALSE
belong to multiple groups simultaneously.
Elements in the s-block, p-block, d-block, and f-block are arbitrarily categorized with no relevance
14 FALSE
to their atomic orbitals, causing confusion in the Periodic Table.
The Periodic Table is an arbitrary arrangement of elements with no correlation between the
15 FALSE
number of periods and quantum numbers.
The lanthanoid series, often called the 4f-inner transition series, starts and ends randomly with
16 FALSE
elements like bromine and nickel, making it structurally inconsistent.
Placing lanthanoids and actinoids separately in the Periodic Table as inner transition series
17 FALSE
disrupts the table's logical structure and confuses element placement.
The atomic number of an element bears no relation to the number of protons in its nucleus,
18 FALSE
creating a fundamental flaw in atomic theory.
Helium's positioning in the p-block alongside noble gases is an arbitrary decision with no scientific
19 FALSE
basis, introducing confusion into the Periodic Table.
2 OF 8 RI_Best Wishes
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