Classification of Elements and Periodicity in Properties
89372
The screening effect of d-electrons is
1 Equal to p-electrons
2 Much more than p-electrons
3 Same as f-electrons
4 Less than p-electrons
Explanation:
The screening effect of inner electron of the nucleus is due to decrease in ionization potential, therefore the order of the screening effect is $\mathrm{f}<\mathrm{d}<\mathrm{p}<\mathrm{s}$ Hence, the screening effect of d-election is less than pelectron.
BITSAT-2013
Classification of Elements and Periodicity in Properties
89373
Identify the wrong statement in the following.
1 Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
2 Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
3 Atomic radius of the elements increases as on moves down the first group of the periodic table.
4 Atomic radius of the elements decreases as on moves across from left to right in the $2^{\text {nd }}$ period of the periodic table.
Explanation:
The positive charge on the cation increases, the effective nuclear charge increases. Thus, the atomic size decreases. Since the number of the shell increases, So atomic radius increases. Against isoelectronic species, ionic radius increases with increases in negative charge or decrease in positive charge.
NEET-2012
Classification of Elements and Periodicity in Properties
89375
As we move from left to right in the 3d-series elements
1 electropositive character decreases
2 electropositive character increases
3 electropositive character decreases and electronegative character increases
4 electropositive character increases and electronegative character decreases.
Explanation:
As we move in the row from left to right, electrons are added to the $3 \mathrm{~d}$ subshell to neutralize the increase in the positive charge of the nucleus as the atomic number increase so, we move from left to right in $3 \mathrm{~d}$ series element electropositive character decrease and electronegative character increases.
COMEDK-2011
Classification of Elements and Periodicity in Properties
89377
Number of elements presents in the fifth period of Periodic Table is
1 32
2 10
3 18
4 8
Explanation:
The fifth period is from rubidium (37) to xenon (54). The last electron enters in $5 \mathrm{~s}, 4 \mathrm{~d}$ or $5 \mathrm{p}$ orbitals. Therefore, the fifth period has $(2+10+6) 18$ elements.
Classification of Elements and Periodicity in Properties
89372
The screening effect of d-electrons is
1 Equal to p-electrons
2 Much more than p-electrons
3 Same as f-electrons
4 Less than p-electrons
Explanation:
The screening effect of inner electron of the nucleus is due to decrease in ionization potential, therefore the order of the screening effect is $\mathrm{f}<\mathrm{d}<\mathrm{p}<\mathrm{s}$ Hence, the screening effect of d-election is less than pelectron.
BITSAT-2013
Classification of Elements and Periodicity in Properties
89373
Identify the wrong statement in the following.
1 Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
2 Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
3 Atomic radius of the elements increases as on moves down the first group of the periodic table.
4 Atomic radius of the elements decreases as on moves across from left to right in the $2^{\text {nd }}$ period of the periodic table.
Explanation:
The positive charge on the cation increases, the effective nuclear charge increases. Thus, the atomic size decreases. Since the number of the shell increases, So atomic radius increases. Against isoelectronic species, ionic radius increases with increases in negative charge or decrease in positive charge.
NEET-2012
Classification of Elements and Periodicity in Properties
89375
As we move from left to right in the 3d-series elements
1 electropositive character decreases
2 electropositive character increases
3 electropositive character decreases and electronegative character increases
4 electropositive character increases and electronegative character decreases.
Explanation:
As we move in the row from left to right, electrons are added to the $3 \mathrm{~d}$ subshell to neutralize the increase in the positive charge of the nucleus as the atomic number increase so, we move from left to right in $3 \mathrm{~d}$ series element electropositive character decrease and electronegative character increases.
COMEDK-2011
Classification of Elements and Periodicity in Properties
89377
Number of elements presents in the fifth period of Periodic Table is
1 32
2 10
3 18
4 8
Explanation:
The fifth period is from rubidium (37) to xenon (54). The last electron enters in $5 \mathrm{~s}, 4 \mathrm{~d}$ or $5 \mathrm{p}$ orbitals. Therefore, the fifth period has $(2+10+6) 18$ elements.
Classification of Elements and Periodicity in Properties
89372
The screening effect of d-electrons is
1 Equal to p-electrons
2 Much more than p-electrons
3 Same as f-electrons
4 Less than p-electrons
Explanation:
The screening effect of inner electron of the nucleus is due to decrease in ionization potential, therefore the order of the screening effect is $\mathrm{f}<\mathrm{d}<\mathrm{p}<\mathrm{s}$ Hence, the screening effect of d-election is less than pelectron.
BITSAT-2013
Classification of Elements and Periodicity in Properties
89373
Identify the wrong statement in the following.
1 Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
2 Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
3 Atomic radius of the elements increases as on moves down the first group of the periodic table.
4 Atomic radius of the elements decreases as on moves across from left to right in the $2^{\text {nd }}$ period of the periodic table.
Explanation:
The positive charge on the cation increases, the effective nuclear charge increases. Thus, the atomic size decreases. Since the number of the shell increases, So atomic radius increases. Against isoelectronic species, ionic radius increases with increases in negative charge or decrease in positive charge.
NEET-2012
Classification of Elements and Periodicity in Properties
89375
As we move from left to right in the 3d-series elements
1 electropositive character decreases
2 electropositive character increases
3 electropositive character decreases and electronegative character increases
4 electropositive character increases and electronegative character decreases.
Explanation:
As we move in the row from left to right, electrons are added to the $3 \mathrm{~d}$ subshell to neutralize the increase in the positive charge of the nucleus as the atomic number increase so, we move from left to right in $3 \mathrm{~d}$ series element electropositive character decrease and electronegative character increases.
COMEDK-2011
Classification of Elements and Periodicity in Properties
89377
Number of elements presents in the fifth period of Periodic Table is
1 32
2 10
3 18
4 8
Explanation:
The fifth period is from rubidium (37) to xenon (54). The last electron enters in $5 \mathrm{~s}, 4 \mathrm{~d}$ or $5 \mathrm{p}$ orbitals. Therefore, the fifth period has $(2+10+6) 18$ elements.
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Classification of Elements and Periodicity in Properties
89372
The screening effect of d-electrons is
1 Equal to p-electrons
2 Much more than p-electrons
3 Same as f-electrons
4 Less than p-electrons
Explanation:
The screening effect of inner electron of the nucleus is due to decrease in ionization potential, therefore the order of the screening effect is $\mathrm{f}<\mathrm{d}<\mathrm{p}<\mathrm{s}$ Hence, the screening effect of d-election is less than pelectron.
BITSAT-2013
Classification of Elements and Periodicity in Properties
89373
Identify the wrong statement in the following.
1 Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
2 Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
3 Atomic radius of the elements increases as on moves down the first group of the periodic table.
4 Atomic radius of the elements decreases as on moves across from left to right in the $2^{\text {nd }}$ period of the periodic table.
Explanation:
The positive charge on the cation increases, the effective nuclear charge increases. Thus, the atomic size decreases. Since the number of the shell increases, So atomic radius increases. Against isoelectronic species, ionic radius increases with increases in negative charge or decrease in positive charge.
NEET-2012
Classification of Elements and Periodicity in Properties
89375
As we move from left to right in the 3d-series elements
1 electropositive character decreases
2 electropositive character increases
3 electropositive character decreases and electronegative character increases
4 electropositive character increases and electronegative character decreases.
Explanation:
As we move in the row from left to right, electrons are added to the $3 \mathrm{~d}$ subshell to neutralize the increase in the positive charge of the nucleus as the atomic number increase so, we move from left to right in $3 \mathrm{~d}$ series element electropositive character decrease and electronegative character increases.
COMEDK-2011
Classification of Elements and Periodicity in Properties
89377
Number of elements presents in the fifth period of Periodic Table is
1 32
2 10
3 18
4 8
Explanation:
The fifth period is from rubidium (37) to xenon (54). The last electron enters in $5 \mathrm{~s}, 4 \mathrm{~d}$ or $5 \mathrm{p}$ orbitals. Therefore, the fifth period has $(2+10+6) 18$ elements.
