Classification of Elements and Periodicity in Properties
89347
Ortho and para- hydrogen have
1 Identical chemical properties but different physical properties
2 identical physical and chemical properties
3 Identical physical properties but different chemical properties
4 different physical and chemical properties.
Explanation:
Ortho and para hydrogen are similar in chemical properties but differ in some of the physical properties. - Melting point of para hydrogen is $13.83 \mathrm{k}$ while that of ordinary hydrogen is $13.95 \mathrm{k}$ - Boiling point of para hydrogen is $20.26 \mathrm{k}$ while that of ordinary hydrogen is $20.39 \mathrm{k}$. - The vapour pressure of liquid para hydrogen is higher than that of ordinary liquid hydrogen.
WB-JEE-2010
Classification of Elements and Periodicity in Properties
89355
The law of triads is applicable to a group of
1 $\mathrm{Cl}, \mathrm{Br}, 1$
2 C,N,O
3 $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$
4 $\mathrm{H}, \mathrm{O}, \mathrm{N}$
Explanation:
According to the law of triads, in a group of three elements, the average atomic masses of the first and last element would be approximately equal to the atomic mass of middle elements. Do bereiner also suggested that the law of triads can also be extended for other quantifiable properties such as density of elements. Bromine must be approximately equal to the average of atomic masses of chlorine and Iodine. Hence, $\mathrm{Cl}, \mathrm{Br}$, I are follow the law of triads. (3.c) Periodic Classification, Periodic Trends
JEE Main
Classification of Elements and Periodicity in Properties
89359
Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements $O, S, F$ and $C l$ ?
1 $\mathrm{Cl}<$ F $<\mathrm{O}<\mathrm{S}$
2 O $<$ S $<$ F $<\mathrm{Cl}$
3 F $<$ S $<\mathrm{O}<\mathrm{Cl}$
4 $\mathrm{S}<\mathrm{O}<\mathrm{Cl}<\mathrm{F}$
Explanation:
Electron gain enthalpy generally increases in a period from left to right and decrease from top to bottom in a group of periodic table. $\mathrm{Cl}$ and $\mathrm{F}$ are belong to 17 group and $\mathrm{O}$ and $\mathrm{S}$ are belong to 16 group. $\mathrm{Cl}$ has higher electron gain enthalpy than $\mathrm{F}$ because the incoming electron experience a greater force of repulsion because of small size of $F$ atom. Similarly, in case of $\mathrm{O}$ and $\mathrm{S}$. Thus, the correct order of electron gain enthalpy is- $$ \mathrm{O}<\mathrm{S}<\mathrm{F}<\mathrm{Cl} $$
NEET-2010
Classification of Elements and Periodicity in Properties
89363
In general, the properties that decrease and increase down a group in the periodic table, respectively are
1 electronegativity and atomic radius
2 electronegativity and electron gain enthalpy
3 electron gain enthalpy and electronegativity
4 atomic radius and electronegativity
Explanation:
Electro negativity is a measure of the tendency of an atom to attract a bonding pair of electron. On moving to down the group electronegativity decrease and increase down the group atomic radius respectively. Electron gain enthalpy becomes more negative from left to right in a period.
Classification of Elements and Periodicity in Properties
89347
Ortho and para- hydrogen have
1 Identical chemical properties but different physical properties
2 identical physical and chemical properties
3 Identical physical properties but different chemical properties
4 different physical and chemical properties.
Explanation:
Ortho and para hydrogen are similar in chemical properties but differ in some of the physical properties. - Melting point of para hydrogen is $13.83 \mathrm{k}$ while that of ordinary hydrogen is $13.95 \mathrm{k}$ - Boiling point of para hydrogen is $20.26 \mathrm{k}$ while that of ordinary hydrogen is $20.39 \mathrm{k}$. - The vapour pressure of liquid para hydrogen is higher than that of ordinary liquid hydrogen.
WB-JEE-2010
Classification of Elements and Periodicity in Properties
89355
The law of triads is applicable to a group of
1 $\mathrm{Cl}, \mathrm{Br}, 1$
2 C,N,O
3 $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$
4 $\mathrm{H}, \mathrm{O}, \mathrm{N}$
Explanation:
According to the law of triads, in a group of three elements, the average atomic masses of the first and last element would be approximately equal to the atomic mass of middle elements. Do bereiner also suggested that the law of triads can also be extended for other quantifiable properties such as density of elements. Bromine must be approximately equal to the average of atomic masses of chlorine and Iodine. Hence, $\mathrm{Cl}, \mathrm{Br}$, I are follow the law of triads. (3.c) Periodic Classification, Periodic Trends
JEE Main
Classification of Elements and Periodicity in Properties
89359
Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements $O, S, F$ and $C l$ ?
1 $\mathrm{Cl}<$ F $<\mathrm{O}<\mathrm{S}$
2 O $<$ S $<$ F $<\mathrm{Cl}$
3 F $<$ S $<\mathrm{O}<\mathrm{Cl}$
4 $\mathrm{S}<\mathrm{O}<\mathrm{Cl}<\mathrm{F}$
Explanation:
Electron gain enthalpy generally increases in a period from left to right and decrease from top to bottom in a group of periodic table. $\mathrm{Cl}$ and $\mathrm{F}$ are belong to 17 group and $\mathrm{O}$ and $\mathrm{S}$ are belong to 16 group. $\mathrm{Cl}$ has higher electron gain enthalpy than $\mathrm{F}$ because the incoming electron experience a greater force of repulsion because of small size of $F$ atom. Similarly, in case of $\mathrm{O}$ and $\mathrm{S}$. Thus, the correct order of electron gain enthalpy is- $$ \mathrm{O}<\mathrm{S}<\mathrm{F}<\mathrm{Cl} $$
NEET-2010
Classification of Elements and Periodicity in Properties
89363
In general, the properties that decrease and increase down a group in the periodic table, respectively are
1 electronegativity and atomic radius
2 electronegativity and electron gain enthalpy
3 electron gain enthalpy and electronegativity
4 atomic radius and electronegativity
Explanation:
Electro negativity is a measure of the tendency of an atom to attract a bonding pair of electron. On moving to down the group electronegativity decrease and increase down the group atomic radius respectively. Electron gain enthalpy becomes more negative from left to right in a period.
Classification of Elements and Periodicity in Properties
89347
Ortho and para- hydrogen have
1 Identical chemical properties but different physical properties
2 identical physical and chemical properties
3 Identical physical properties but different chemical properties
4 different physical and chemical properties.
Explanation:
Ortho and para hydrogen are similar in chemical properties but differ in some of the physical properties. - Melting point of para hydrogen is $13.83 \mathrm{k}$ while that of ordinary hydrogen is $13.95 \mathrm{k}$ - Boiling point of para hydrogen is $20.26 \mathrm{k}$ while that of ordinary hydrogen is $20.39 \mathrm{k}$. - The vapour pressure of liquid para hydrogen is higher than that of ordinary liquid hydrogen.
WB-JEE-2010
Classification of Elements and Periodicity in Properties
89355
The law of triads is applicable to a group of
1 $\mathrm{Cl}, \mathrm{Br}, 1$
2 C,N,O
3 $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$
4 $\mathrm{H}, \mathrm{O}, \mathrm{N}$
Explanation:
According to the law of triads, in a group of three elements, the average atomic masses of the first and last element would be approximately equal to the atomic mass of middle elements. Do bereiner also suggested that the law of triads can also be extended for other quantifiable properties such as density of elements. Bromine must be approximately equal to the average of atomic masses of chlorine and Iodine. Hence, $\mathrm{Cl}, \mathrm{Br}$, I are follow the law of triads. (3.c) Periodic Classification, Periodic Trends
JEE Main
Classification of Elements and Periodicity in Properties
89359
Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements $O, S, F$ and $C l$ ?
1 $\mathrm{Cl}<$ F $<\mathrm{O}<\mathrm{S}$
2 O $<$ S $<$ F $<\mathrm{Cl}$
3 F $<$ S $<\mathrm{O}<\mathrm{Cl}$
4 $\mathrm{S}<\mathrm{O}<\mathrm{Cl}<\mathrm{F}$
Explanation:
Electron gain enthalpy generally increases in a period from left to right and decrease from top to bottom in a group of periodic table. $\mathrm{Cl}$ and $\mathrm{F}$ are belong to 17 group and $\mathrm{O}$ and $\mathrm{S}$ are belong to 16 group. $\mathrm{Cl}$ has higher electron gain enthalpy than $\mathrm{F}$ because the incoming electron experience a greater force of repulsion because of small size of $F$ atom. Similarly, in case of $\mathrm{O}$ and $\mathrm{S}$. Thus, the correct order of electron gain enthalpy is- $$ \mathrm{O}<\mathrm{S}<\mathrm{F}<\mathrm{Cl} $$
NEET-2010
Classification of Elements and Periodicity in Properties
89363
In general, the properties that decrease and increase down a group in the periodic table, respectively are
1 electronegativity and atomic radius
2 electronegativity and electron gain enthalpy
3 electron gain enthalpy and electronegativity
4 atomic radius and electronegativity
Explanation:
Electro negativity is a measure of the tendency of an atom to attract a bonding pair of electron. On moving to down the group electronegativity decrease and increase down the group atomic radius respectively. Electron gain enthalpy becomes more negative from left to right in a period.
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Classification of Elements and Periodicity in Properties
89347
Ortho and para- hydrogen have
1 Identical chemical properties but different physical properties
2 identical physical and chemical properties
3 Identical physical properties but different chemical properties
4 different physical and chemical properties.
Explanation:
Ortho and para hydrogen are similar in chemical properties but differ in some of the physical properties. - Melting point of para hydrogen is $13.83 \mathrm{k}$ while that of ordinary hydrogen is $13.95 \mathrm{k}$ - Boiling point of para hydrogen is $20.26 \mathrm{k}$ while that of ordinary hydrogen is $20.39 \mathrm{k}$. - The vapour pressure of liquid para hydrogen is higher than that of ordinary liquid hydrogen.
WB-JEE-2010
Classification of Elements and Periodicity in Properties
89355
The law of triads is applicable to a group of
1 $\mathrm{Cl}, \mathrm{Br}, 1$
2 C,N,O
3 $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$
4 $\mathrm{H}, \mathrm{O}, \mathrm{N}$
Explanation:
According to the law of triads, in a group of three elements, the average atomic masses of the first and last element would be approximately equal to the atomic mass of middle elements. Do bereiner also suggested that the law of triads can also be extended for other quantifiable properties such as density of elements. Bromine must be approximately equal to the average of atomic masses of chlorine and Iodine. Hence, $\mathrm{Cl}, \mathrm{Br}$, I are follow the law of triads. (3.c) Periodic Classification, Periodic Trends
JEE Main
Classification of Elements and Periodicity in Properties
89359
Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements $O, S, F$ and $C l$ ?
1 $\mathrm{Cl}<$ F $<\mathrm{O}<\mathrm{S}$
2 O $<$ S $<$ F $<\mathrm{Cl}$
3 F $<$ S $<\mathrm{O}<\mathrm{Cl}$
4 $\mathrm{S}<\mathrm{O}<\mathrm{Cl}<\mathrm{F}$
Explanation:
Electron gain enthalpy generally increases in a period from left to right and decrease from top to bottom in a group of periodic table. $\mathrm{Cl}$ and $\mathrm{F}$ are belong to 17 group and $\mathrm{O}$ and $\mathrm{S}$ are belong to 16 group. $\mathrm{Cl}$ has higher electron gain enthalpy than $\mathrm{F}$ because the incoming electron experience a greater force of repulsion because of small size of $F$ atom. Similarly, in case of $\mathrm{O}$ and $\mathrm{S}$. Thus, the correct order of electron gain enthalpy is- $$ \mathrm{O}<\mathrm{S}<\mathrm{F}<\mathrm{Cl} $$
NEET-2010
Classification of Elements and Periodicity in Properties
89363
In general, the properties that decrease and increase down a group in the periodic table, respectively are
1 electronegativity and atomic radius
2 electronegativity and electron gain enthalpy
3 electron gain enthalpy and electronegativity
4 atomic radius and electronegativity
Explanation:
Electro negativity is a measure of the tendency of an atom to attract a bonding pair of electron. On moving to down the group electronegativity decrease and increase down the group atomic radius respectively. Electron gain enthalpy becomes more negative from left to right in a period.
