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Page 1
Q And A
Q1: What are the defects in Modern Periodic Table?
Answer: Following are the defects:
? Position of hydrogen still dicey. It is not fixed till now.
? Position of lanthanides and actinides has not been given inside the main body of periodic
table.
? It does not reflect the exact distribution of electrons of some of transition and inner transition
elements.
Q2: What are the salient features of Modern Periodic Table?
Answer:
? In a period of the periodic table, the number of valence electrons increases as atomic number
increases. As a result, elements change from metal to metalloid to nonmetal to noble gas.
? Atomic size is a periodic property. As atomic number increases in a period, atomic radius
decreases. As atomic number increases in a group, atomic radius increases.
? Positive ions have smaller atomic radii than the neutral atoms from which they derive.
Negative ions have larger atomic radii than their neutral atoms.
? Positive ions in the same group increase in size down the group.
? In a group, each element has the same number of valence electrons. As a result, the
elements
in a group show similar chemical behavior.
? Metallic character decreases from left to right in a period because of the increase in the
effective nuclear charge.
? Non-metallic character increase from left to right in a period because of ncrease in
effective nuclear charge.Non-metallic character decreases down the group because of
increase in the size of the
atom.
Q3: Two elements X and Y have atomic numbers 12 and 16 respectively. Write the electronic
configuration for these elements. To which period of the modern periodic table do these two
elements belong? What type of bond will be formed between them and why?
Answer: Electronic configuration of X (Z=12): 2, 8, 2
Electronic configuration of Y (Z=16): 2, 8, 6
Both these elements belong to third period. An ionic bond is formed between X and Y due to transfer
of two electrons from X to Y.
Q4: The present classification of elements is based on which fundamental property of
elements?
Answer: Atomic Number is the basis.
Q5: Li, Na and K are the elements of a Dobereiners Triad. If atomic mass of Li is 7 and that of K
is 39. What would be the atomic mass of Na?
Answer: According of Dobereiner’s law of triads, the atomic mass of the middle element, in this case
Na, should be the arithmetic mean of Li and K.
Thus,
arithmetic mean of Li and K = (7 + 39)/2 = 23 (Answer)
Q6: Define Dobereiner’s law of triads.
Answer: It states, "when elements are placed in order of the ascending order of atomic masses,
Page 2
Q And A
Q1: What are the defects in Modern Periodic Table?
Answer: Following are the defects:
? Position of hydrogen still dicey. It is not fixed till now.
? Position of lanthanides and actinides has not been given inside the main body of periodic
table.
? It does not reflect the exact distribution of electrons of some of transition and inner transition
elements.
Q2: What are the salient features of Modern Periodic Table?
Answer:
? In a period of the periodic table, the number of valence electrons increases as atomic number
increases. As a result, elements change from metal to metalloid to nonmetal to noble gas.
? Atomic size is a periodic property. As atomic number increases in a period, atomic radius
decreases. As atomic number increases in a group, atomic radius increases.
? Positive ions have smaller atomic radii than the neutral atoms from which they derive.
Negative ions have larger atomic radii than their neutral atoms.
? Positive ions in the same group increase in size down the group.
? In a group, each element has the same number of valence electrons. As a result, the
elements
in a group show similar chemical behavior.
? Metallic character decreases from left to right in a period because of the increase in the
effective nuclear charge.
? Non-metallic character increase from left to right in a period because of ncrease in
effective nuclear charge.Non-metallic character decreases down the group because of
increase in the size of the
atom.
Q3: Two elements X and Y have atomic numbers 12 and 16 respectively. Write the electronic
configuration for these elements. To which period of the modern periodic table do these two
elements belong? What type of bond will be formed between them and why?
Answer: Electronic configuration of X (Z=12): 2, 8, 2
Electronic configuration of Y (Z=16): 2, 8, 6
Both these elements belong to third period. An ionic bond is formed between X and Y due to transfer
of two electrons from X to Y.
Q4: The present classification of elements is based on which fundamental property of
elements?
Answer: Atomic Number is the basis.
Q5: Li, Na and K are the elements of a Dobereiners Triad. If atomic mass of Li is 7 and that of K
is 39. What would be the atomic mass of Na?
Answer: According of Dobereiner’s law of triads, the atomic mass of the middle element, in this case
Na, should be the arithmetic mean of Li and K.
Thus,
arithmetic mean of Li and K = (7 + 39)/2 = 23 (Answer)
Q6: Define Dobereiner’s law of triads.
Answer: It states, "when elements are placed in order of the ascending order of atomic masses,
groups of three elements having similar properties are obtained. The atomic mass of the middle
element of the triad is equal to the mean of the atomic masses of the other two elements of the triad."
Q7: Why did Dobereiner's system of classification fail?
Answer:
? Major drawback of Deberneir’s classification was that it was valid only for a few groups of
elements known during that time. He was able to identify three triads only.
? Also with more accurate measurements of atomic masses showed that the mid element of the
triad did not really have the mean value of the sum of the other two elements of the triad.
? For elements of very low mass or very high mass, the law did not hold good. For example
Flourine(F), Chlorine (Cl), Bromine(Br). Atomic mass of Cl is not an arithmetic mean of atomic
masses of F and Br
Q8: Explain about position of metalloids in modern periodic table.
Answer: In the Modern Periodic Table, a zig-zag line separates metals from non-metals. The
borderline elements – boron, silicon, germanium, arsenic, antimony, tellurium and polonium – are
intermediate in properties and are called metalloids or semi-metals.
Q9: Why does Silicon classified as metalloid?
Answer: Silicon is classified as a semi-metal or metalloid because it exhibits some properties of both
metals and non-metals.
Q10: State Newland's law of octaves.
Answer: Elements are arranged in increasing order of their atomic masses such that the properties of
the eighth element is repetition of the properties of first element ( similar to eighth note in an octave of
music).
Q11: X and Y are the two elements having similar properties which obey Newlands law of
octaves. How many elements are there in between X and Y?
Answer: The law states there are eight elements in an octave (row). No. of elements between X and
Y is six.
Q12: What are the drawbacks of Newland's law of octaves?
Answer: Following are the major drawbacks:
1. Worked well with lighter elements (upto Calcium). After that elements in eighth column did not
possess properties similar to element in first column.
2. Newland assumed only 56 elements existed so far. Later new elements were discovered
which did not fit into octaves table.
3. Newland adjusted few elements in a same slot though their properties were quite different.
E.g. Cobalt and nickel are in the same slot and these are placed in the same column as
fluorine, chlorine and bromine which have very different properties than these elements. Iron,
which resembles cobalt and nickel in properties, has been placed far away from these
elements.
Q13: What periodic trends do we observe in terms of atomic radii or atomic sizes in Modern
periodic table?
Answer: Following two trends are observed.
Page 3
Q And A
Q1: What are the defects in Modern Periodic Table?
Answer: Following are the defects:
? Position of hydrogen still dicey. It is not fixed till now.
? Position of lanthanides and actinides has not been given inside the main body of periodic
table.
? It does not reflect the exact distribution of electrons of some of transition and inner transition
elements.
Q2: What are the salient features of Modern Periodic Table?
Answer:
? In a period of the periodic table, the number of valence electrons increases as atomic number
increases. As a result, elements change from metal to metalloid to nonmetal to noble gas.
? Atomic size is a periodic property. As atomic number increases in a period, atomic radius
decreases. As atomic number increases in a group, atomic radius increases.
? Positive ions have smaller atomic radii than the neutral atoms from which they derive.
Negative ions have larger atomic radii than their neutral atoms.
? Positive ions in the same group increase in size down the group.
? In a group, each element has the same number of valence electrons. As a result, the
elements
in a group show similar chemical behavior.
? Metallic character decreases from left to right in a period because of the increase in the
effective nuclear charge.
? Non-metallic character increase from left to right in a period because of ncrease in
effective nuclear charge.Non-metallic character decreases down the group because of
increase in the size of the
atom.
Q3: Two elements X and Y have atomic numbers 12 and 16 respectively. Write the electronic
configuration for these elements. To which period of the modern periodic table do these two
elements belong? What type of bond will be formed between them and why?
Answer: Electronic configuration of X (Z=12): 2, 8, 2
Electronic configuration of Y (Z=16): 2, 8, 6
Both these elements belong to third period. An ionic bond is formed between X and Y due to transfer
of two electrons from X to Y.
Q4: The present classification of elements is based on which fundamental property of
elements?
Answer: Atomic Number is the basis.
Q5: Li, Na and K are the elements of a Dobereiners Triad. If atomic mass of Li is 7 and that of K
is 39. What would be the atomic mass of Na?
Answer: According of Dobereiner’s law of triads, the atomic mass of the middle element, in this case
Na, should be the arithmetic mean of Li and K.
Thus,
arithmetic mean of Li and K = (7 + 39)/2 = 23 (Answer)
Q6: Define Dobereiner’s law of triads.
Answer: It states, "when elements are placed in order of the ascending order of atomic masses,
groups of three elements having similar properties are obtained. The atomic mass of the middle
element of the triad is equal to the mean of the atomic masses of the other two elements of the triad."
Q7: Why did Dobereiner's system of classification fail?
Answer:
? Major drawback of Deberneir’s classification was that it was valid only for a few groups of
elements known during that time. He was able to identify three triads only.
? Also with more accurate measurements of atomic masses showed that the mid element of the
triad did not really have the mean value of the sum of the other two elements of the triad.
? For elements of very low mass or very high mass, the law did not hold good. For example
Flourine(F), Chlorine (Cl), Bromine(Br). Atomic mass of Cl is not an arithmetic mean of atomic
masses of F and Br
Q8: Explain about position of metalloids in modern periodic table.
Answer: In the Modern Periodic Table, a zig-zag line separates metals from non-metals. The
borderline elements – boron, silicon, germanium, arsenic, antimony, tellurium and polonium – are
intermediate in properties and are called metalloids or semi-metals.
Q9: Why does Silicon classified as metalloid?
Answer: Silicon is classified as a semi-metal or metalloid because it exhibits some properties of both
metals and non-metals.
Q10: State Newland's law of octaves.
Answer: Elements are arranged in increasing order of their atomic masses such that the properties of
the eighth element is repetition of the properties of first element ( similar to eighth note in an octave of
music).
Q11: X and Y are the two elements having similar properties which obey Newlands law of
octaves. How many elements are there in between X and Y?
Answer: The law states there are eight elements in an octave (row). No. of elements between X and
Y is six.
Q12: What are the drawbacks of Newland's law of octaves?
Answer: Following are the major drawbacks:
1. Worked well with lighter elements (upto Calcium). After that elements in eighth column did not
possess properties similar to element in first column.
2. Newland assumed only 56 elements existed so far. Later new elements were discovered
which did not fit into octaves table.
3. Newland adjusted few elements in a same slot though their properties were quite different.
E.g. Cobalt and nickel are in the same slot and these are placed in the same column as
fluorine, chlorine and bromine which have very different properties than these elements. Iron,
which resembles cobalt and nickel in properties, has been placed far away from these
elements.
Q13: What periodic trends do we observe in terms of atomic radii or atomic sizes in Modern
periodic table?
Answer: Following two trends are observed.
1. Within each column (group), atomic radius tends to increase from top to bottom. This trend
results primarily from the increase in the number of the outer electrons. As we go down a
column, the outer electrons have a greater probability of being farther from the nucleus,
causing the atom to increase in size.
2. Within each row (period), atomic radius tends to decrease from left to right. The major factor
influencing this trend is the increase in the nuclear charge as we move across a row. The
increasing effective nuclear charge steadily draws the valence electrons closer to the nucleus,
causing the atomic radius to decrease.
Q14: Name the scientist who proposed modern periodic law? On which fundamental property
of elements it is based?
Answer: Henry Moseley. He proposed atomic number should be chosen as fundamental property
(instead of atomic mass) to classify elements.
Q15: On what basis did Mendeleev arrange the elements?
Answer: On the basis of atomic masses.
Q16: An element R of atomic number 12 combines separately with NO
3
-
and (SO
4
)
2-
, (PO
4
)
3-
radicals.
a) Write the electronic configuration of element R
b) Write the formulae of the three compounds so formed.
c) To which group of the periodic table does the element ‘R’ belong?
d) Does it form covalent or ionic compound? Why?
Answer:
a) Electronic configuration of R is 2,8,2.
b) Compounds formed are: R(NO
3
)
2
, R(SO
4
) and R(PO
4
)
2
c) R has two valence electrons and hence it belongs to second group.
d) It forms ionic compound by loosing two electrons to attain stable electronic configuration.
Q17: Why do you think the noble gases are placed in a separate group?
Answer: Due to following reasons:
Page 4
Q And A
Q1: What are the defects in Modern Periodic Table?
Answer: Following are the defects:
? Position of hydrogen still dicey. It is not fixed till now.
? Position of lanthanides and actinides has not been given inside the main body of periodic
table.
? It does not reflect the exact distribution of electrons of some of transition and inner transition
elements.
Q2: What are the salient features of Modern Periodic Table?
Answer:
? In a period of the periodic table, the number of valence electrons increases as atomic number
increases. As a result, elements change from metal to metalloid to nonmetal to noble gas.
? Atomic size is a periodic property. As atomic number increases in a period, atomic radius
decreases. As atomic number increases in a group, atomic radius increases.
? Positive ions have smaller atomic radii than the neutral atoms from which they derive.
Negative ions have larger atomic radii than their neutral atoms.
? Positive ions in the same group increase in size down the group.
? In a group, each element has the same number of valence electrons. As a result, the
elements
in a group show similar chemical behavior.
? Metallic character decreases from left to right in a period because of the increase in the
effective nuclear charge.
? Non-metallic character increase from left to right in a period because of ncrease in
effective nuclear charge.Non-metallic character decreases down the group because of
increase in the size of the
atom.
Q3: Two elements X and Y have atomic numbers 12 and 16 respectively. Write the electronic
configuration for these elements. To which period of the modern periodic table do these two
elements belong? What type of bond will be formed between them and why?
Answer: Electronic configuration of X (Z=12): 2, 8, 2
Electronic configuration of Y (Z=16): 2, 8, 6
Both these elements belong to third period. An ionic bond is formed between X and Y due to transfer
of two electrons from X to Y.
Q4: The present classification of elements is based on which fundamental property of
elements?
Answer: Atomic Number is the basis.
Q5: Li, Na and K are the elements of a Dobereiners Triad. If atomic mass of Li is 7 and that of K
is 39. What would be the atomic mass of Na?
Answer: According of Dobereiner’s law of triads, the atomic mass of the middle element, in this case
Na, should be the arithmetic mean of Li and K.
Thus,
arithmetic mean of Li and K = (7 + 39)/2 = 23 (Answer)
Q6: Define Dobereiner’s law of triads.
Answer: It states, "when elements are placed in order of the ascending order of atomic masses,
groups of three elements having similar properties are obtained. The atomic mass of the middle
element of the triad is equal to the mean of the atomic masses of the other two elements of the triad."
Q7: Why did Dobereiner's system of classification fail?
Answer:
? Major drawback of Deberneir’s classification was that it was valid only for a few groups of
elements known during that time. He was able to identify three triads only.
? Also with more accurate measurements of atomic masses showed that the mid element of the
triad did not really have the mean value of the sum of the other two elements of the triad.
? For elements of very low mass or very high mass, the law did not hold good. For example
Flourine(F), Chlorine (Cl), Bromine(Br). Atomic mass of Cl is not an arithmetic mean of atomic
masses of F and Br
Q8: Explain about position of metalloids in modern periodic table.
Answer: In the Modern Periodic Table, a zig-zag line separates metals from non-metals. The
borderline elements – boron, silicon, germanium, arsenic, antimony, tellurium and polonium – are
intermediate in properties and are called metalloids or semi-metals.
Q9: Why does Silicon classified as metalloid?
Answer: Silicon is classified as a semi-metal or metalloid because it exhibits some properties of both
metals and non-metals.
Q10: State Newland's law of octaves.
Answer: Elements are arranged in increasing order of their atomic masses such that the properties of
the eighth element is repetition of the properties of first element ( similar to eighth note in an octave of
music).
Q11: X and Y are the two elements having similar properties which obey Newlands law of
octaves. How many elements are there in between X and Y?
Answer: The law states there are eight elements in an octave (row). No. of elements between X and
Y is six.
Q12: What are the drawbacks of Newland's law of octaves?
Answer: Following are the major drawbacks:
1. Worked well with lighter elements (upto Calcium). After that elements in eighth column did not
possess properties similar to element in first column.
2. Newland assumed only 56 elements existed so far. Later new elements were discovered
which did not fit into octaves table.
3. Newland adjusted few elements in a same slot though their properties were quite different.
E.g. Cobalt and nickel are in the same slot and these are placed in the same column as
fluorine, chlorine and bromine which have very different properties than these elements. Iron,
which resembles cobalt and nickel in properties, has been placed far away from these
elements.
Q13: What periodic trends do we observe in terms of atomic radii or atomic sizes in Modern
periodic table?
Answer: Following two trends are observed.
1. Within each column (group), atomic radius tends to increase from top to bottom. This trend
results primarily from the increase in the number of the outer electrons. As we go down a
column, the outer electrons have a greater probability of being farther from the nucleus,
causing the atom to increase in size.
2. Within each row (period), atomic radius tends to decrease from left to right. The major factor
influencing this trend is the increase in the nuclear charge as we move across a row. The
increasing effective nuclear charge steadily draws the valence electrons closer to the nucleus,
causing the atomic radius to decrease.
Q14: Name the scientist who proposed modern periodic law? On which fundamental property
of elements it is based?
Answer: Henry Moseley. He proposed atomic number should be chosen as fundamental property
(instead of atomic mass) to classify elements.
Q15: On what basis did Mendeleev arrange the elements?
Answer: On the basis of atomic masses.
Q16: An element R of atomic number 12 combines separately with NO
3
-
and (SO
4
)
2-
, (PO
4
)
3-
radicals.
a) Write the electronic configuration of element R
b) Write the formulae of the three compounds so formed.
c) To which group of the periodic table does the element ‘R’ belong?
d) Does it form covalent or ionic compound? Why?
Answer:
a) Electronic configuration of R is 2,8,2.
b) Compounds formed are: R(NO
3
)
2
, R(SO
4
) and R(PO
4
)
2
c) R has two valence electrons and hence it belongs to second group.
d) It forms ionic compound by loosing two electrons to attain stable electronic configuration.
Q17: Why do you think the noble gases are placed in a separate group?
Answer: Due to following reasons:
1. Similar inert behaviour
2. Similar electronic configuration
3. Available in low concentration.
Q18: Besides gallium, which other elements have since been discovered that were left by
Mendeléev in his Periodic Table? (any two)
Answer: Scandium (Sc) and Germanium(Ge)
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FAQs on Q And A Q1: What are the defects in Modern Periodic Table? - Class 11
| 1. What are the defects in Modern Periodic Table? |  |
Ans. The defects in Modern Periodic Table are:
1. Position of Hydrogen: Hydrogen is placed in group 1 but it does not resemble alkali metals nor does it resemble halogens. It has its own unique properties, therefore, there is no fixed position for hydrogen in the table.
2. Position of isotopes: The isotopes of an element have the same atomic number but different atomic masses. The modern periodic table does not give any information about isotopes and their arrangement.
3. Position of Lanthanides and Actinides: Lanthanides and Actinides elements are placed separately at the bottom of the periodic table, which breaks the continuity of the periodic table. They should be placed in their respective positions in the periodic table.
4. Incomplete shells: The elements with incomplete electron shells are placed in the same group as the elements with completely filled shells. For example, Copper and Chromium are placed in the same group as Zinc and Titanium, respectively, but they have different electron configurations.
5. No provision for the discovery of new elements: The modern periodic table does not provide any provision for the discovery of new elements. It is designed to accommodate only the known elements.
| 2. What is the importance of the periodic table? | |
Ans. The periodic table is important because:
1. It organizes the elements: The periodic table is a systematic arrangement of elements according to their atomic number, electronic configuration, and chemical properties. It helps to organize the elements in a meaningful way.
2. Prediction of properties: The position of elements in the periodic table can help predict their properties. For example, elements in the same group have similar chemical properties.
3. Discovering new elements: The periodic table provides a framework for discovering new elements. Scientists can use the periodic table to predict the properties of undiscovered elements.
4. Understanding chemical reactions: The periodic table helps to understand chemical reactions by showing the valence electrons of each element and how they react with other elements.
5. Industrial Applications: The periodic table is used in various industries such as pharmaceuticals, metallurgy, and chemical manufacturing. It helps to understand the properties of elements and compounds used in these industries.
| 3. How are elements arranged in the periodic table? | |
Ans. Elements are arranged in the periodic table according to their atomic number. The atomic number of an element is the number of protons in the nucleus of its atom. The elements are arranged in order of increasing atomic number in rows and columns. The rows are called periods and the columns are called groups. The elements in the same group have similar chemical properties. The modern periodic table has 7 periods and 18 groups.
| 4. Why are elements grouped in the periodic table? | |
Ans. Elements are grouped in the periodic table based on their electron configurations and chemical properties. Elements in the same group have similar electronic configurations, meaning they have the same number of valence electrons. Valence electrons are responsible for the chemical properties of an element. Elements in the same group have similar chemical properties because they have the same number of valence electrons. For example, the alkaline earth metals (group 2) have two valence electrons and are highly reactive. They have similar properties because they all lose two electrons to form a +2 ion.
| 5. What is the significance of electronic configuration in the periodic table? | |
Ans. The electronic configuration is the arrangement of electrons in the energy levels or shells of an atom. The electronic configuration is significant because it determines the chemical properties of an element. The number of valence electrons, which are the electrons in the outermost shell, determines how an element will react chemically. The position of an element in the periodic table is determined by its electronic configuration. The elements in the same group have the same number of valence electrons and similar chemical properties. Therefore, the electronic configuration plays a crucial role in the periodic table.
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The content of Q And A Q1: What are the defects in Modern Periodic Table? is prepared as per the latest Class 11 syllabus.
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