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All questions of p-Block Elements for JEE Exam
Which of the following statements is true?a)The atomic radius of Ga is less than B.
b)The atomic radius of Ga is more than Al.c)The atomic radius of Ga is less than Al.d)The atomic radius of Ga is equal to AlCorrect answer is option 'C'. Can you explain this answer?
b)The atomic radius of Ga is more than Al.
c)The atomic radius of Ga is less than Al.
d)The atomic radius of Ga is equal to Al
Correct answer is option 'C'. Can you explain this answer?
|
Neha Joshi answered |
The atomic radius of the Ga is less than Al because of poor screening effect. The atomic radius of Ga is slightly lesser than of Al because in going from Al to Ga, the electrons have already occupied 3d sub shell in Ga
The correct statements among the given are
- a)Antimony belongs to 15th group and 5th period
- b)electron gain enthalpy of P > N > S > O
- c)Minimum and maximum oxidation number of phosphorus is -3 and +6
- d)Fluoroapatite, formula is Ca6(PO4)6 CaF2
Correct answer is option 'A'. Can you explain this answer?
The correct statements among the given are
a)
Antimony belongs to 15th group and 5th period
b)
electron gain enthalpy of P > N > S > O
c)
Minimum and maximum oxidation number of phosphorus is -3 and +6
d)
Fluoroapatite, formula is Ca6(PO4)6 CaF2
|
Divey Sethi answered |
Option A: Group 5A (or VA) of the periodic table are the pnictogens: the nonmetals nitrogen (N), and phosphorus (P), the metalloids arsenic (As) and antimony (Sb), and the metal bismuth (Bi).
Option B: The electron gain enthalpy of P< N< S< O.
Option C: Minimum and maximum oxidation number of phosphorus are -3 and +5 respectively.
Option D: Fluorapatite is a phosphate mineral with the formula Ca5(PO4)3F .
Option B: The electron gain enthalpy of P< N< S< O.
Option C: Minimum and maximum oxidation number of phosphorus are -3 and +5 respectively.
Option D: Fluorapatite is a phosphate mineral with the formula Ca5(PO4)3F .
Hence, option A is correct.
HClO is known as- a)chloric acid
- b)Chlorine
- c)bacteria killer
- d)water
Correct answer is option 'A'. Can you explain this answer?
HClO is known as
a)
chloric acid
b)
Chlorine
c)
bacteria killer
d)
water
|
|
Nada Sharin answered |
Hypohalous acid is also known as CHLORIC (I) ACID
Correct answer is '4'. Can you explain this answer?
|
Subhankar Choudhary answered |
Molecular Orbital Theory and Antibonding Orbitals in Nitrogen
Molecular orbital theory (MOT) is a theoretical model that describes the behavior of electrons in molecules based on the principles of quantum mechanics. It is used to explain and predict the properties of molecules, including their electronic and magnetic properties, bond lengths, bond angles, and so on.
In MOT, the electrons in a molecule are treated as waves that are described by molecular orbitals (MOs), which are mathematical functions that represent the probability of finding an electron at a given point in space. These MOs are formed by combining the atomic orbitals of the atoms in the molecule.
Antibonding orbitals are MOs that have a higher energy than the atomic orbitals from which they are formed. When electrons occupy these orbitals, they weaken the bond between the atoms in the molecule, making it more likely to break apart.
Nitrogen has five valence electrons, which are represented by the atomic orbitals s and p. In the molecule N2, these atomic orbitals combine to form five MOs: two bonding MOs, two antibonding MOs, and one nonbonding MO.
The two bonding MOs are lower in energy than the atomic orbitals from which they are formed, and they help to hold the two nitrogen atoms together. The nonbonding MO is filled with two electrons, which are shared equally between the two nitrogen atoms and do not contribute to the bond strength.
The two antibonding MOs are higher in energy than the atomic orbitals from which they are formed, and they weaken the bond between the two nitrogen atoms. When all five valence electrons are placed into the MOs, there are four electrons in the antibonding MOs and one electron in the nonbonding MO.
Therefore, according to molecular orbital theory, there are four electrons present in the antibonding orbitals of nitrogen.
Molecular orbital theory (MOT) is a theoretical model that describes the behavior of electrons in molecules based on the principles of quantum mechanics. It is used to explain and predict the properties of molecules, including their electronic and magnetic properties, bond lengths, bond angles, and so on.
In MOT, the electrons in a molecule are treated as waves that are described by molecular orbitals (MOs), which are mathematical functions that represent the probability of finding an electron at a given point in space. These MOs are formed by combining the atomic orbitals of the atoms in the molecule.
Antibonding orbitals are MOs that have a higher energy than the atomic orbitals from which they are formed. When electrons occupy these orbitals, they weaken the bond between the atoms in the molecule, making it more likely to break apart.
Nitrogen has five valence electrons, which are represented by the atomic orbitals s and p. In the molecule N2, these atomic orbitals combine to form five MOs: two bonding MOs, two antibonding MOs, and one nonbonding MO.
The two bonding MOs are lower in energy than the atomic orbitals from which they are formed, and they help to hold the two nitrogen atoms together. The nonbonding MO is filled with two electrons, which are shared equally between the two nitrogen atoms and do not contribute to the bond strength.
The two antibonding MOs are higher in energy than the atomic orbitals from which they are formed, and they weaken the bond between the two nitrogen atoms. When all five valence electrons are placed into the MOs, there are four electrons in the antibonding MOs and one electron in the nonbonding MO.
Therefore, according to molecular orbital theory, there are four electrons present in the antibonding orbitals of nitrogen.
Hot conc. H2SO4 acts as moderately strong oxidising agent. It oxidises both metals and nonmetals. Which of the following element is oxidised by conc. H2SO4 into two gaseous products?- a) Cu
- b)S
- c)C
- d)zn
Correct answer is 'C'. Can you explain this answer?
Hot conc. H2SO4 acts as moderately strong oxidising agent. It oxidises both metals and nonmetals. Which of the following element is oxidised by conc. H2SO4 into two gaseous products?
a)
Cu
b)
S
c)
C
d)
zn
|
|
Naina Bansal answered |
C element is oxidised by conc. H2SO4 into two gaseous products.
Which of the following statements is incorrect?- a)Oxidation state of sulphur in its compounds vary from -2 to +8
- b)Tetrahalides of 16th group have see-saw shap
- c)S2CI2 has linear geometr
- d)SCI4 on hydrolysis yields sulphurous acid
Correct answer is option 'C'. Can you explain this answer?
Which of the following statements is incorrect?
a)
Oxidation state of sulphur in its compounds vary from -2 to +8
b)
Tetrahalides of 16th group have see-saw shap
c)
S2CI2 has linear geometr
d)
SCI4 on hydrolysis yields sulphurous acid
|
Priyanka Sharma answered |
Disulphur dichlor
The angle between the
planes is 90°.
The structure is referred to as gauche.
The angle between the
planes is 90°.The structure is referred to as gauche.
Which of the following elements exist as liquid in summer among group 13 elements?
- a) Tl
- b) Al
- c) B
- d) Ga
Correct answer is option 'D'. Can you explain this answer?
Which of the following elements exist as liquid in summer among group 13 elements?
a)
Tlb)
Alc)
Bd)
Ga
|
Krishna Iyer answered |
Galium can occur in liquid state if the room is above 29.76C which is its melting point. So,option d is correct
The correct no. of lone pairs on the central atom of compounds XeF2, XeF4 & XeF6are respectively- [AIEEE-2002]- a)3, 2,1
- b)4, 3, 2
- c)1, 3, 4
- d)1, 2, 3
Correct answer is option 'A'. Can you explain this answer?
The correct no. of lone pairs on the central atom of compounds XeF2, XeF4 & XeF6are respectively- [AIEEE-2002]
a)
3, 2,1
b)
4, 3, 2
c)
1, 3, 4
d)
1, 2, 3
|
|
Krishna Iyer answered |
The correct answer is option A (3,2,1)
XeF2 has a linear shape. Its hybridization is sp3d which means it should have a trigonal bipyramidal shape. Since it has 3 lone pairs, they occupy the equatorial triangle.
XeF4 has sp3d2 hybridization. It has a square planar shape and 2 lone pairs of electrons.
XeF6 has one lone pair of electrons. The 6 out of 8 electrons of Xenon are shared by 6 atoms of fluorine.
XeF2 has a linear shape. Its hybridization is sp3d which means it should have a trigonal bipyramidal shape. Since it has 3 lone pairs, they occupy the equatorial triangle.
XeF4 has sp3d2 hybridization. It has a square planar shape and 2 lone pairs of electrons.
XeF6 has one lone pair of electrons. The 6 out of 8 electrons of Xenon are shared by 6 atoms of fluorine.
- a)
- b)
- c)
- d)
Correct answer is option 'B'. Can you explain this answer?
a)
b)
c)
d)
|
|
Nikita Singh answered |
The second ionization energy refers to the energy required to remove the electron from the corresponding monovalent cation of the respective atom.
It is expected to increase from left to right in the periodic table with the decrease in atomic size.
Since the Oxygen atom gets a stable electronic configuration, 2s22p3 after removing one electron, the O+ shows greater ionization energy than F+ as well as N+.
Thus, correct order will be: O > F > N > C
In trivalent state, for example, the trichlorides, being covalent are hydrolysed in water form- a)pentagonal structure
- b)planar structure
- c)trigonal structure
- d)tetrahedral structure
Correct answer is option 'D'. Can you explain this answer?
In trivalent state, for example, the trichlorides, being covalent are hydrolysed in water form
a)
pentagonal structure
b)
planar structure
c)
trigonal structure
d)
tetrahedral structure
|
Riya Banerjee answered |
trihalides hydrolysis to form tetrahedral structure
The maximum oxidation state shown by a p-block element is equal to the:- a)Total number of valence electrons (i.e., the sum of the s and p-electrons)
- b)Total number of s electrons
- c)Total number of p electrons
- d)None of these
Correct answer is option 'A'. Can you explain this answer?
The maximum oxidation state shown by a p-block element is equal to the:
a)
Total number of valence electrons (i.e., the sum of the s and p-electrons)
b)
Total number of s electrons
c)
Total number of p electrons
d)
None of these
|
|
Preeti Khanna answered |
- The oxidation state of an element is related to the number of electrons that an atom loses, gains, or appears to use when joining with another atom in compounds.
- It also determines the ability of an atom to oxidize (to lose electrons) or to reduce (to gain electrons) other atoms or species.
- They should release the total valence electrons to attain stability, so the maximum possible oxidation state is the number of valence electrons.
In the third period of the periodic table the element having smallest size is - a)Na
- b)CI
- c)Ar
- d)Si
Correct answer is option 'B'. Can you explain this answer?
In the third period of the periodic table the element having smallest size is
a)
Na
b)
CI
c)
Ar
d)
Si
|
Aarav Sharma answered |
The third period contains eight elements: sodium, magnesium, aluminium, silicon, phosphorus, sulfur, chlorine, and argon.
In a period from left to right atomic size decreases due to Increase in nuclear charge.
but the noble gases are bigger than the halogens as they have octet and sort of repulsion occurs in the shells.
so the smallest element in a period is the halogen.so chlorine Cl is the smallest.
The exhibition of highest co-ordination number depends on the availability of vacant orbitals in the central atom. Which of the following elements is not likely to act as central atom in MF3-6?- a)B
- b)Al
- c)Ga
- d)In
Correct answer is option 'A'. Can you explain this answer?
The exhibition of highest co-ordination number depends on the availability of vacant orbitals in the central atom. Which of the following elements is not likely to act as central atom in MF3-6?
a)
B
b)
Al
c)
Ga
d)
In
|
|
Anjana Sharma answered |
The element M in the complex ion MF6^3- has a coordination number of six. Since B has only s- and p-orbitals and no d – orbitals, therefore, at the maximum it can show a coordination number of 4. Thus, B cannot form complex of the type MF6^3-, i.e., option (a) is correct.
Maximum number of compounds are known in case of :- a)Krypton
- b)Helium
- c)Argon
- d)Xenon
Correct answer is option 'D'. Can you explain this answer?
Maximum number of compounds are known in case of :
a)
Krypton
b)
Helium
c)
Argon
d)
Xenon
|
Aaditya Ghoshal answered |
Only xenon is well known to form chemical compounds, because xenon is large in size and having higer atomic mass.Due to having larger atomic radius the force of attraction between the outer electron and the protons in the nucleus is weaker.
Which is incorrectly matched ?- a)CsBr3
Cs+ + Br3– - b)I4O9 I3+ + (IO3–)3
- c)AgBrO3 Ag+ + BrO3–
- d)I2O4 IO2– + IO2+
Correct answer is option 'D'. Can you explain this answer?
Which is incorrectly matched ?
a)
CsBr3 Cs+ + Br3–
Cs+ + Br3–b)
I4O9 I3+ + (IO3–)3
I3+ + (IO3–)3c)
AgBrO3 Ag+ + BrO3–
Ag+ + BrO3–d)
I2O4 IO2– + IO2+
IO2– + IO2+
|
Gunjan Lakhani answered |
It is strictly covalent does not shows cationic & anionic form.
Which of the outer electronic configuration represent argon?- a)ns2np4
- b)ns2
- c)ns2np2
- d)ns2np6
Correct answer is option 'D'. Can you explain this answer?
Which of the outer electronic configuration represent argon?
a)
ns2np4
b)
ns2
c)
ns2np2
d)
ns2np6
|
Aadhar Academy answered |
The correct answer is option D
Outer electronic configuration represents argon ns2,np6.
Atomic no. of argon is 18. Its electronic configuration will be
1s2 2s2 2p6 3s2 3p6.
As the outermost shell is full (3s23p6) it is called noble gas.
Outer electronic configuration represents argon ns2,np6.
Atomic no. of argon is 18. Its electronic configuration will be
1s2 2s2 2p6 3s2 3p6.
As the outermost shell is full (3s23p6) it is called noble gas.
Partial hydrolysis of XeF6 yields:- a)Xenon trioxide
- b)Xenon tetrafluoride
- c)Xenon dioxydifluoride
- d)Xenon oxyfluoride
Correct answer is option 'D'. Can you explain this answer?
Partial hydrolysis of XeF6 yields:
a)
Xenon trioxide
b)
Xenon tetrafluoride
c)
Xenon dioxydifluoride
d)
Xenon oxyfluoride
|
|
Anjana Sharma answered |
Partial hydrolysis of XeF6 yields xenon oxyfluoride.
XeF6 + H2O → XeOF4 + 2HF
The order of ionization enthalpy for B, Al and Ga is:- a)B>Al<Ga
- b)B
- c)B>Al>Ga
- d)Ga
Correct answer is option 'A'. Can you explain this answer?
The order of ionization enthalpy for B, Al and Ga is:
a)
B>Al<Ga
b)
B
c)
B>Al>Ga
d)
Ga
|
Ayush Joshi answered |
(A) B>Al<Ga
The trend in ionization enthalpy is because there is decrease in Ionisation enthalpy from B to Al due to increase in size and from Al to Ga. Ga has more ionisation energy than Al due to uneffective screening effect.
Nitrogen dioxide is dissolved in water to produce- a)HNO3 and HNO2
- b)Only HNO3
- c)Only HNO2
- d)HNO2 and N2
Correct answer is option 'A'. Can you explain this answer?
Nitrogen dioxide is dissolved in water to produce
a)
HNO3 and HNO2
b)
Only HNO3
c)
Only HNO2
d)
HNO2 and N2
|
Uday Chakraborty answered |
NO2 + H2O → HNO3 + HNO2
Mixed
anhydride
Mixed
anhydride
Which of the following gaseous molecule is monoatomic?- a)Oxygen
- b)Helium
- c)Nitrogen
- d)Chlorine
Correct answer is option 'B'. Can you explain this answer?
Which of the following gaseous molecule is monoatomic?
a)
Oxygen
b)
Helium
c)
Nitrogen
d)
Chlorine
|
Swara Sharma answered |
Explanation:
Monoatomic molecules are the molecules that consist of only one atom of an element. They are rare because most elements tend to bond with other atoms to form molecules. However, some elements are stable in their monoatomic form.
The given options are:
a) Oxygen (O2) - Oxygen molecule is diatomic, which means it consists of two atoms of oxygen.
b) Helium (He) - Helium is a rare example of a monoatomic molecule. It exists as a single atom and does not bond with other atoms.
c) Nitrogen (N2) - Nitrogen molecule is diatomic, which means it consists of two atoms of nitrogen.
d) Chlorine (Cl2) - Chlorine molecule is diatomic, which means it consists of two atoms of chlorine.
Therefore, the correct answer is option 'B', Helium, which is a monoatomic molecule.
Monoatomic molecules are the molecules that consist of only one atom of an element. They are rare because most elements tend to bond with other atoms to form molecules. However, some elements are stable in their monoatomic form.
The given options are:
a) Oxygen (O2) - Oxygen molecule is diatomic, which means it consists of two atoms of oxygen.
b) Helium (He) - Helium is a rare example of a monoatomic molecule. It exists as a single atom and does not bond with other atoms.
c) Nitrogen (N2) - Nitrogen molecule is diatomic, which means it consists of two atoms of nitrogen.
d) Chlorine (Cl2) - Chlorine molecule is diatomic, which means it consists of two atoms of chlorine.
Therefore, the correct answer is option 'B', Helium, which is a monoatomic molecule.
Ammonia can be dried using- a)CaO
- b)H2SO4
- c)P4O10
- d)CaCl2
Correct answer is option 'A'. Can you explain this answer?
Ammonia can be dried using
a)
CaO
b)
H2SO4
c)
P4O10
d)
CaCl2
|
Anoushka Chopra answered |
CaO is used to dry NH3
Which of the following group 13 elements oxide is acidic in nature?- a)Al2O3
- b)B2O3
- c)Tl2O3
- d)Ga2O3
Correct answer is option 'B'. Can you explain this answer?
Which of the following group 13 elements oxide is acidic in nature?
a)
Al2O3
b)
B2O3
c)
Tl2O3
d)
Ga2O3
|
|
Naina Bansal answered |
The acidic character of oxides of group 13 decreases down the group, because non-metallic character of elements decreases down the group and metallic character increases.
And we know that oxides of metals are basic in nature and oxides of non-metals are acidic in nature. So acidic character of oxides of group 13 decreases down the group.
For example boron (1st element of group 13) is non-metal, so its oxide is acidic.
Aluminum (2nd element of group 13) shows characteristics of both metal and non-metal, so its oxide shows amphoteric nature.
As we go down the group, indium and thalium (4th and 5th element of group 13) show metallic properties, so their oxides are basic.
One of the following p-block elements has unusually low melting point- a)Indium
- b)boron
- c)gallium
- d)aluminium
Correct answer is option 'C'. Can you explain this answer?
One of the following p-block elements has unusually low melting point
a)
Indium
b)
boron
c)
gallium
d)
aluminium
|
|
Preeti Iyer answered |
Argon
Argon is most abundant in composition of air percent by volume. It is in 0.934% in composition of air and is one of the major gas in the Earth's atmosphere.
XeF2 is isostructural with- a)SbCl3
- b)BaCl2
- c)TeF2
- d)ICl2–
Correct answer is option 'D'. Can you explain this answer?
XeF2 is isostructural with
a)
SbCl3
b)
BaCl2
c)
TeF2
d)
ICl2–
|
Arya Dasgupta answered |
C) TeF2
XeF2 and TeF2 have the same structure, which is linear with a bond angle of 180 degrees. SbCl3 has a trigonal pyramidal structure, BaCl2 has a linear structure, and ICl2 has a bent structure.
XeF2 and TeF2 have the same structure, which is linear with a bond angle of 180 degrees. SbCl3 has a trigonal pyramidal structure, BaCl2 has a linear structure, and ICl2 has a bent structure.
A brown ring is formed in the ring test for NO3– ion. It is due to the formation of- a)[Fe(H2O)5 (NO)]2+
- b) FeSO4.NO2
- c)[Fe(H2O)4(NO)2]2+
- d)FeSO4.HNO3
Correct answer is option 'A'. Can you explain this answer?
A brown ring is formed in the ring test for NO3– ion. It is due to the formation of
a)
[Fe(H2O)5 (NO)]2+
b)
FeSO4.NO2
c)
[Fe(H2O)4(NO)2]2+
d)
FeSO4.HNO3
|
Sushil Kumar answered |
When freshly prepared solution of FeSO4 is added in a solution containing NO3– ion, it leads to formation of a brown coloured complex. This is known as brown ring test of nitrate.
Which one of the following statements regarding helium is incorrect
[AIEEE 2004]
- a)It is used to produce and sustain powerful superconducting magnets
- b)It is used as a cryogenic agent for carrying out experiments at low temperatures
- c)It is used to fill gas balloons instead of hydrogen because it is lighter and non-inflammable
- d)It is used in gas-cooled nuclear reactors
Correct answer is option 'C'. Can you explain this answer?
Which one of the following statements regarding helium is incorrect
[AIEEE 2004]
a)
It is used to produce and sustain powerful superconducting magnets
b)
It is used as a cryogenic agent for carrying out experiments at low temperatures
c)
It is used to fill gas balloons instead of hydrogen because it is lighter and non-inflammable
d)
It is used in gas-cooled nuclear reactors
|
|
Shreya Gupta answered |
Helium is twice as heavy as hydrogen, its lifting power is 92% of that of hydrogen. Helium has the lowest melting and boiling point of any element which makes liquid helium an ideal coolant for many extremely low temperature application such as super conducting magnet and cryogenic research where temperature close to absolute zero are needed.
- a)
- b)
- c)
- d)
Correct answer is option 'A'. Can you explain this answer?
a)
b)
c)
d)
|
|
Priyanka Sharma answered |
(i) Nitrogen is a non-metal.
(ii) Phosphorus is a non-metal.
(iii) Arsenic is a metalloid and shows Sublimation.
(iv) Bismuth is metal and shows the Inert pair effect.
(ii) Phosphorus is a non-metal.
(iii) Arsenic is a metalloid and shows Sublimation.
(iv) Bismuth is metal and shows the Inert pair effect.
Hence, option A is correct.
The valency of inert gas is:- a)Zero
- b)1
- c)2
- d)3
Correct answer is option 'A'. Can you explain this answer?
The valency of inert gas is:
a)
Zero
b)
1
c)
2
d)
3
|
|
Sushil Kumar answered |
The correct answer is Option A.
Valency of an element is defined as its tendency to accept valence electrons.
Since noble gas has completely filled valence (outer) shells, they have the least reactivity.
Hence noble gases are already stable in its elemental form. So its valency is zero.
Since noble gas has completely filled valence (outer) shells, they have the least reactivity.
Hence noble gases are already stable in its elemental form. So its valency is zero.
Dry ice is- a)Solid N2
- b)Solid CO2
- c)Solid SO2
- d)Solid NH3
Correct answer is option 'B'. Can you explain this answer?
Dry ice is
a)
Solid N2
b)
Solid CO2
c)
Solid SO2
d)
Solid NH3
|
Krish Ghoshal answered |
Dry ice is solid CO2
Inert pair effect of p-block elements is due to the- a)the most unstable valence number of p-block elements
- b)the most stable valence number of p-block elements
- c)the group oxidation state of p-block elements
- d)the oxidation state two unit less than the group oxidation state
Correct answer is option 'D'. Can you explain this answer?
Inert pair effect of p-block elements is due to the
a)
the most unstable valence number of p-block elements
b)
the most stable valence number of p-block elements
c)
the group oxidation state of p-block elements
d)
the oxidation state two unit less than the group oxidation state
|
Infinity Academy answered |
Due to the presence of inner lying d and f electrons oxidation state which is 2 unit less than the group oxidation state become popular.
Find the sum of bond pairs and non-bonding electron pairs in ICI molecule.
Correct answer is '4'. Can you explain this answer?
Find the sum of bond pairs and non-bonding electron pairs in ICI molecule.
|
Tarun Chakraborty answered |
3 lone pairs and 1 bond pair.
In XeF2, state the total number of electron pairs in its Lewis dot structure.
Correct answer is '3'. Can you explain this answer?
In XeF2, state the total number of electron pairs in its Lewis dot structure.
|
|
Suresh Iyer answered |
Electron dot structure of XeF2 is
The number of hydrogen atoms (s) attached to phosphorus atom in hypophosphorous acid is – [AIEEE-2005]- a) Two
- b)Zero
- c) Three
- d) One
Correct answer is option 'A'. Can you explain this answer?
The number of hydrogen atoms (s) attached to phosphorus atom in hypophosphorous acid is – [AIEEE-2005]
a)
Two
b)
Zero
c)
Three
d)
One
|
|
Anjali Iyer answered |
Molecular formula of Hypophosphorous Acid is H3PO2. In this, two hydrogen atoms are attached to phosphorus atom with single bond, one -OH group is attached to phosphorus atom with single bond and one oxygen atom is attached to phosphorus atom with double bond.
Among the following compounds, the number of compounds which have oxidation states of S is +4 ?PbS, SO2, SF6, Na2S2O3, H2SO3
Correct answer is '2'. Can you explain this answer?
Among the following compounds, the number of compounds which have oxidation states of S is +4 ?
PbS, SO2, SF6, Na2S2O3, H2SO3
|
|
Shreya Singh answered |
SO2...x+2(-2)=0.x=4..H2SO3.2(1)+x+3(-2)=0.2+x-6=0.-4+x=0.x=4...
The elements of group 14 are slightly more electronegative than group 13 elements because of- a)small size
- b)their being liquids
- c)high melting point
- d)high boiling point
Correct answer is option 'A'. Can you explain this answer?
The elements of group 14 are slightly more electronegative than group 13 elements because of
a)
small size
b)
their being liquids
c)
high melting point
d)
high boiling point
|
Pankaj Sengupta answered |
As we move along the period electronegativity increases due to increase in nuclear charge.
- a)
- b)
- c)
- d)
Correct answer is option 'B'. Can you explain this answer?
a)
b)
c)
d)
|
|
Gauri Datta answered |
Oxidation of ammonia with CuO produces nitrogen gas and water vapor. This reaction is represented as:
2NH3 + 3CuO → 3Cu + N2 + 3H2O
The gaseous chemical produced in this reaction is nitrogen gas (N2), which is also obtained by reacting excess ammonia with chlorine. This reaction is represented as:
2NH3 + Cl2 → N2 + 2HCl
Explanation:
- Ammonium nitrate: Heating ammonium nitrate results in the decomposition of ammonium nitrate into nitrogen gas, water vapor, and oxygen gas. The reaction is represented as:
NH4NO3 → N2 + 2H2O + O2
- Potassium dichromate: Heating potassium dichromate results in the production of oxygen gas and potassium chromate. The reaction is represented as:
4K2Cr2O7 → 4K2CrO4 + 3O2
- Catalytic oxidation of ammonia: Catalytic oxidation of ammonia involves the use of a catalyst (such as platinum or palladium) to oxidize ammonia to nitrogen gas and water vapor. The reaction is represented as:
4NH3 + 5O2 → 4NO + 6H2O
2NO + O2 → 2NO2
4NO2 + O2 → 2N2O5
N2O5 → N2 + 2.5O2
- Reacting excess ammonia with chlorine: This reaction involves the reaction of excess ammonia with chlorine gas to produce nitrogen gas and hydrochloric acid. The reaction is represented as:
2NH3 + Cl2 → N2 + 2HCl
Therefore, option B, reacting excess ammonia with chlorine, is the correct answer.
2NH3 + 3CuO → 3Cu + N2 + 3H2O
The gaseous chemical produced in this reaction is nitrogen gas (N2), which is also obtained by reacting excess ammonia with chlorine. This reaction is represented as:
2NH3 + Cl2 → N2 + 2HCl
Explanation:
- Ammonium nitrate: Heating ammonium nitrate results in the decomposition of ammonium nitrate into nitrogen gas, water vapor, and oxygen gas. The reaction is represented as:
NH4NO3 → N2 + 2H2O + O2
- Potassium dichromate: Heating potassium dichromate results in the production of oxygen gas and potassium chromate. The reaction is represented as:
4K2Cr2O7 → 4K2CrO4 + 3O2
- Catalytic oxidation of ammonia: Catalytic oxidation of ammonia involves the use of a catalyst (such as platinum or palladium) to oxidize ammonia to nitrogen gas and water vapor. The reaction is represented as:
4NH3 + 5O2 → 4NO + 6H2O
2NO + O2 → 2NO2
4NO2 + O2 → 2N2O5
N2O5 → N2 + 2.5O2
- Reacting excess ammonia with chlorine: This reaction involves the reaction of excess ammonia with chlorine gas to produce nitrogen gas and hydrochloric acid. The reaction is represented as:
2NH3 + Cl2 → N2 + 2HCl
Therefore, option B, reacting excess ammonia with chlorine, is the correct answer.
Which one of the following reactions of Xenon compounds is not feasible ? [AIEEE-2009]- a) 3 XeF4 + 6 H2O → 2 Xe + XeO3 + 12 HF + 1.5 O2
- b)2 XeF2 + 2H2O → 2 Xe + 4 HF + O2
- c)XeF6 + RbF → Rb [XeF7]
- d)XeO3 + 6 HF → XeF6 + 3 H2O
Correct answer is option 'D'. Can you explain this answer?
Which one of the following reactions of Xenon compounds is not feasible ? [AIEEE-2009]
a)
3 XeF4 + 6 H2O → 2 Xe + XeO3 + 12 HF + 1.5 O2
b)
2 XeF2 + 2H2O → 2 Xe + 4 HF + O2
c)
XeF6 + RbF → Rb [XeF7]
d)
XeO3 + 6 HF → XeF6 + 3 H2O
|
|
Geetika Shah answered |
XeO3+6HF⟶XeF6+3H2O
This reaction is not feasible because the products again react to give reactants back. All the xenon fluorides easily undergo hydrolysis and give xenon oxides but the opposite is not possible.
Hence D
The element having highest ionisation potential is:- a)Oxygen
- b)Helium
- c)Nitrogen
- d)Hydrogen
Correct answer is option 'B'. Can you explain this answer?
The element having highest ionisation potential is:
a)
Oxygen
b)
Helium
c)
Nitrogen
d)
Hydrogen
|
|
Rajeev Saxena answered |
Thereby, the amount of energy required to remove an electron from the atom decreases. Ionization potential, thus, decreases down a group. The element with highest ionization potential in the periodic table is Helium (2372.1 kj/mol), while the element with the lowest ionization potential is Caesium (375.7 kj/mol).
As we move from B to Al in the p-block elements the sum of the first three ionisation enthalpies- a)slightly decreases
- b)remains the same
- c)considerably decreases
- d)increases
Correct answer is option 'C'. Can you explain this answer?
As we move from B to Al in the p-block elements the sum of the first three ionisation enthalpies
a)
slightly decreases
b)
remains the same
c)
considerably decreases
d)
increases
|
Om Desai answered |
On moving from B to Al size increases so sum of ionization energies also decreases.
The correct statements among the following are
- a)Bond lengths in O2 ,
are 121 , 134, 149 pm
- b)Ozone is stronger oxidising agent than dioxygen
- c)O2 acts as reducing agent when it reacts with powerful oxidising agents like PtF6
- d)Ozone is much more stable than oxygen
Correct answer is option 'A,B,C'. Can you explain this answer?
The correct statements among the following are
a)
Bond lengths in O2 , are 121 , 134, 149 pm
are 121 , 134, 149 pmb)
Ozone is stronger oxidising agent than dioxygen
c)
O2 acts as reducing agent when it reacts with powerful oxidising agents like PtF6
d)
Ozone is much more stable than oxygen
|
Srishti Kaur answered |
The correct option is Option A, B and C.
Bond length is inversely proportional to bond order. O2+ has the highest bond order among these three, so it should have the shortest bond length.
Ozone is a powerful oxidizing agent as compared to oxygen. This is due to the unstable nature of ozone and the nascent oxygen that is released during the reaction.
O2 when gas makes others like H2 gas to lose electrons, therefore, O2 gas is an oxidizing agent and H2 when gas loses electrons in redox reaction, therefore H2 gas is a reducing agent.
Oxygen is more stable than ozone. On heating, ozone readily dissociates and forms oxygen and free radicals of oxygen known as nascent oxygen which take part in reaction, thus ozone is more reactive than oxygen
In the MOT of F2 molecule, number of electrons occupying antibonding orbitals are
Correct answer is '8'. Can you explain this answer?
In the MOT of F2 molecule, number of electrons occupying antibonding orbitals are
|
|
Nandita Ahuja answered |
Fluorine atom have 2+7 electrons so an F2 molecule contain 18 electrons.
Hence, 8 electrons occupy the antibonding orbitals.
Hence, 8 electrons occupy the antibonding orbitals.
The chemical species having sp2-hybridisation for the central atom is- a)SOCI2
- b)
- c)SCI2
- d)SO3
Correct answer is option 'A,D'. Can you explain this answer?
The chemical species having sp2-hybridisation for the central atom is
a)
SOCI2
b)
c)
SCI2
d)
SO3
|
C.k Singh answered |
Only option D has sp2 hybridisation for the central atom.Rest is sp3 hybridisation.
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