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All questions of Classification of Elements and Periodicity in Properties for JEE Exam
The valence of sodium with atomic number 11 is:- a)4
- b)1
- c)3
- d)2
Correct answer is option 'B'. Can you explain this answer?
The valence of sodium with atomic number 11 is:
a)
4
b)
1
c)
3
d)
2
|
Rohan Singh answered |
For Sodium Na - 2,8,1 and chlorine Cl-2,8,7. Both Na and Cl require 1 electron either to loose or to gain ,so they can attain stable configuration. Therefore Na has +1 and Cl -1 valency. Valence electrons are the outermost electrons, and are the ones involved in bonding.
In Na2O oxidation state of oxygen is:- a)+2
- b)-1
- c)0
- d)+1
Correct answer is option 'D'. Can you explain this answer?
In Na2O oxidation state of oxygen is:
a)
+2
b)
-1
c)
0
d)
+1
|
Geetika Shah answered |
In Na2O oxidation state of Na is +1.
It gains 2 electrons so, the oxidation state is +1 which is equal to one oxygen atom (2 electrons)
It gains 2 electrons so, the oxidation state is +1 which is equal to one oxygen atom (2 electrons)
Lothar Meyer proposed that on arranging the elements in order of increasing atomic weights; similarities appear in which type of properties?- a)Only physical properties
- b)Only chemical properties
- c)In both physical and chemical properties
- d)thermodynamic properties
Correct answer is option 'C'. Can you explain this answer?
Lothar Meyer proposed that on arranging the elements in order of increasing atomic weights; similarities appear in which type of properties?
a)
Only physical properties
b)
Only chemical properties
c)
In both physical and chemical properties
d)
thermodynamic properties
|
Anoushka Yadav answered |
Lothar Meyer proposed the periodic table in 1864. He arranged the elements in order of increasing atomic weights. He noticed that similarities appeared in both physical and chemical properties of the elements. The correct answer is option 'C' which means similarities appear in both physical and chemical properties.
Explanation:
The periodic table arranges the elements in a way that helps in understanding their properties. The modern periodic table is based on the electronic configuration of the elements. But the original periodic table was based on the atomic weight of the elements. Lothar Meyer was the first to realize that there is a periodicity in the properties of the elements when they are arranged in order of increasing atomic weights.
Physical properties are those that can be observed or measured without changing the chemical composition of the substance. Some examples of physical properties are:
- Melting point
- Boiling point
- Density
- Electrical conductivity
- Thermal conductivity
- Atomic radius
- Ionic radius
- Electronegativity
Chemical properties are those that can be observed during a chemical reaction. Some examples of chemical properties are:
- Reactivity with acids
- Reactivity with oxygen
- Reactivity with water
- Reduction potential
- Oxidation potential
Meyer observed that when the elements are arranged in order of increasing atomic weights, there is a periodicity in their physical and chemical properties. This means that elements with similar atomic weights have similar physical and chemical properties. For example, lithium, sodium, and potassium have similar physical and chemical properties because they all belong to the same group and have similar atomic weights.
Conclusion:
Lothar Meyer proposed the periodic table in 1864. He arranged the elements in order of increasing atomic weights. He noticed that similarities appeared in both physical and chemical properties of the elements. When the elements are arranged in order of increasing atomic weights, there is a periodicity in their physical and chemical properties.
Explanation:
The periodic table arranges the elements in a way that helps in understanding their properties. The modern periodic table is based on the electronic configuration of the elements. But the original periodic table was based on the atomic weight of the elements. Lothar Meyer was the first to realize that there is a periodicity in the properties of the elements when they are arranged in order of increasing atomic weights.
Physical properties are those that can be observed or measured without changing the chemical composition of the substance. Some examples of physical properties are:
- Melting point
- Boiling point
- Density
- Electrical conductivity
- Thermal conductivity
- Atomic radius
- Ionic radius
- Electronegativity
Chemical properties are those that can be observed during a chemical reaction. Some examples of chemical properties are:
- Reactivity with acids
- Reactivity with oxygen
- Reactivity with water
- Reduction potential
- Oxidation potential
Meyer observed that when the elements are arranged in order of increasing atomic weights, there is a periodicity in their physical and chemical properties. This means that elements with similar atomic weights have similar physical and chemical properties. For example, lithium, sodium, and potassium have similar physical and chemical properties because they all belong to the same group and have similar atomic weights.
Conclusion:
Lothar Meyer proposed the periodic table in 1864. He arranged the elements in order of increasing atomic weights. He noticed that similarities appeared in both physical and chemical properties of the elements. When the elements are arranged in order of increasing atomic weights, there is a periodicity in their physical and chemical properties.
Sodium forms which types of oxides?- a)Acidic
- b)Basic
- c)Neutral
- d)Amphoteric
Correct answer is option 'B'. Can you explain this answer?
Sodium forms which types of oxides?
a)
Acidic
b)
Basic
c)
Neutral
d)
Amphoteric
|
Pooja Mehta answered |
Basic oxides are always oxides of metals. They combine with water to form bases which are usually called metal hydroxides. Na2O, MgO, CaO, FeO and CuO are examples of basic oxides. Acidic oxides are mostly oxides of non-metals, and they dissolve in water to form acids.
Horizontal rows in the periodic table are called:- a)Cell
- b)Table
- c)Groups
- d)Periods
Correct answer is option 'D'. Can you explain this answer?
Horizontal rows in the periodic table are called:
a)
Cell
b)
Table
c)
Groups
d)
Periods
|
|
Rohan Singh answered |
The Periodic Table: Families and Periods. In the periodic table of elements, there are seven horizontal rows of elements called periods. The vertical columns of elements are called groups, or families.
Can you explain the answer of this question below:In the modern periodic table, which period contains 32 elements?
- A:
Sixth
- B:
First
- C:
Seventh
- D:
Second
The answer is a.
In the modern periodic table, which period contains 32 elements?
Sixth
First
Seventh
Second
|
|
Preeti Iyer answered |
The answer is c.
The total number of electrons that can be accommodated in seventh period are 2 ( in 7s) + 14(in 5f) + 10(in 6d )+ 6(in 7p) = 32. The maximum number of elements present in it is 32.
Among the following statements the one that is not true about Mendeleev’s Periodic Table is:- a)Elements of group 7 and 8 were arranged on the basis of equivalent weights
- b)Some elements in the same group differ in their properties
- c)Elements were arranged on the basis of atomic weights
- d)The position of hydrogen was not justified
Correct answer is option 'A'. Can you explain this answer?
Among the following statements the one that is not true about Mendeleev’s Periodic Table is:
a)
Elements of group 7 and 8 were arranged on the basis of equivalent weights
b)
Some elements in the same group differ in their properties
c)
Elements were arranged on the basis of atomic weights
d)
The position of hydrogen was not justified
|
Om Desai answered |
In Mendeleev’s periodic table, elements were arranged on the basis of atomic weights.
An element with atomic number will form a basic oxide________ - a)7
- b)17
- c)14
- d)11
Correct answer is option 'D'. Can you explain this answer?
An element with atomic number will form a basic oxide________
a)
7
b)
17
c)
14
d)
11
|
EduRev NEET answered |
Sodium forms a basic oxide because it is a metal. Metals generally form basic oxides because they tend to donate electrons to oxygen atoms. In the case of sodium, when it reacts with oxygen, it forms sodium oxide, in which each sodium atom donates one electron to oxygen. This results in the formation of sodium ions (Na+) and oxide ions (O2-), which can combine to form the ionic compound sodium oxide. Sodium oxide is basic because it can react with water to form a solution of sodium hydroxide, a strong base.
Which block of the periodic table contains the man made elements?- a)p block
- b)s block
- c)f block
- d)d block
Correct answer is option 'C'. Can you explain this answer?
Which block of the periodic table contains the man made elements?
a)
p block
b)
s block
c)
f block
d)
d block
|
|
Raghav Bansal answered |
Most of the f block elements, lanthanoids and actinoids are man made/synthetic/prepared in the lab. Especially actinoids.
Where would you find the smallest atoms of elements in the periodic table?
- a)top and right hand side
- b)top and left hand side
- c)bottom and left hand side
- d)bottom and right hand side
Correct answer is option 'A'. Can you explain this answer?
Where would you find the smallest atoms of elements in the periodic table?
a)
top and right hand side
b)
top and left hand side
c)
bottom and left hand side
d)
bottom and right hand side
|
Nandini Chakraborty answered |
The smallest atom is the one with the smallest number of protons. This is hydrogen, located in the top left side of the periodic table. Hydrogen is particularly small because the most common isotope doesn't have a neutron, plus it readily loses its electron.
Eka silicon predicted by Mendeleev is which element:- a)Germanium
- b)Aluminium
- c)Gallium
- d)Sodium
Correct answer is option 'A'. Can you explain this answer?
Eka silicon predicted by Mendeleev is which element:
a)
Germanium
b)
Aluminium
c)
Gallium
d)
Sodium
|
Suresh Iyer answered |
Mendeleev predicted the existence of 'eka-silicon', which would fit into a gap next to silicon. The element germanium was discovered later. Its properties were found to be similar to the predicted ones and confirmed Mendeleev's periodic table.
Which of the following pairs have both the members from the same group of periodic table?- a)Mg, Cl
- b)Mg, Cu
- c)Mg, Be
- d)Mg, Na
Correct answer is option 'C'. Can you explain this answer?
Which of the following pairs have both the members from the same group of periodic table?
a)
Mg, Cl
b)
Mg, Cu
c)
Mg, Be
d)
Mg, Na
|
|
Neha Joshi answered |
The elements in the group include beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
Which scientist proposed that atomic number is more fundamental property of an element than its atomic mass?- a)Newlands
- b)Lothar Meyer
- c)Henry Moseley
- d)Meyer
Correct answer is option 'C'. Can you explain this answer?
Which scientist proposed that atomic number is more fundamental property of an element than its atomic mass?
a)
Newlands
b)
Lothar Meyer
c)
Henry Moseley
d)
Meyer
|
|
Pooja Shah answered |
The scientist who first of all showed that the atomic number is more fundamental property of an element than its atomic mass was Henry Moseley.
Which of the following is the most non-metallic element?- a)F
- b)Si
- c)N
- d)B
Correct answer is option 'A'. Can you explain this answer?
Which of the following is the most non-metallic element?
a)
F
b)
Si
c)
N
d)
B
|
|
Nandini Patel answered |
The non-metallic character increases as we go from left to right across the periodic table. Hence, fluorine (F) is most non-metallic. Further F has maximum tendency to accept an electron characteristic of non-metal.
Na+ is smaller than Na atom because:- a)The effective nuclear charge is greater in case of sodium ion.
- b)Nucleus in each case contains different nucleons.
- c)Na+ is more stable than in Na atom.
- d)Sodium atom has one electron lesser than sodium ion.
Correct answer is option 'A'. Can you explain this answer?
Na+ is smaller than Na atom because:
a)
The effective nuclear charge is greater in case of sodium ion.
b)
Nucleus in each case contains different nucleons.
c)
Na+ is more stable than in Na atom.
d)
Sodium atom has one electron lesser than sodium ion.
|
|
Geetika Shah answered |
According to the electronic configuration of sodium(Na),it has 1 valence electron(2,8,1).So it loses one electron to form a cation and becomes sodium cation (Na+).As it loses one electron ,the outermost shell has 0 electrons (i.e it gets eliminated ) and Na+ has only 2 shells. Hence, it lost one of its shell, the sodium ion is smaller than the sodium atom.
The lanthanide series starts with:
- a)Thorium
- b)Lutetium
- c)Lawrencium
- d)cerium
Correct answer is option 'D'. Can you explain this answer?
The lanthanide series starts with:
a)
Thorium
b)
Lutetium
c)
Lawrencium
d)
cerium
|
|
Suresh Reddy answered |
The lanthanide series starts from cerium and ends in lutetium
What is the relationship between the number of elements in each period and the number of atomic orbitals available in the energy level that is being filled?- a)Number of elements is twice the number of atomic orbitals.
- b)Number of elements is three times the number of atomic orbitals.
- c)Number of elements is half the number of atomic orbitals.
- d)Number of elements is same as the number of atomic orbitals.
Correct answer is 'A'. Can you explain this answer?
What is the relationship between the number of elements in each period and the number of atomic orbitals available in the energy level that is being filled?
a)
Number of elements is twice the number of atomic orbitals.
b)
Number of elements is three times the number of atomic orbitals.
c)
Number of elements is half the number of atomic orbitals.
d)
Number of elements is same as the number of atomic orbitals.
|
Krishna Iyer answered |
The number of elements in each period is twice the number of atomic orbitals available in the energy level that is being filled.
Let's understand it by taking the elements of the 4th period.
In the fourth period, there are 18 elements. The types of subshells used in the 4th period are s, p, and d.
Number of orbitals of s subshell = 1
Number of orbitals of p subshell = 3
Number of orbitals of d subshell = 5
Total number of orbitals = 9
The total number of elements is 18 i.e. twice the total number of orbitals.
In the fourth period, there are 18 elements. The types of subshells used in the 4th period are s, p, and d.
Number of orbitals of s subshell = 1
Number of orbitals of p subshell = 3
Number of orbitals of d subshell = 5
Total number of orbitals = 9
The total number of elements is 18 i.e. twice the total number of orbitals.
Which of the following is an ionic hydride?- a)PH3
- b)H2S
- c)HI
- d)KH
Correct answer is option 'D'. Can you explain this answer?
Which of the following is an ionic hydride?
a)
PH3
b)
H2S
c)
HI
d)
KH
|
Mohit Rajpoot answered |
Ionic hydrides are commonly known as saline hydrides or pseudohalides. These compounds form between hydrogen and the most active metals, especially with the alkali and alkaline-earth metals of group one and two elements.
In this group, the hydrogen acts as the hydride ion (H−). They bond with more electropositive metal atoms. Ionic hydrides are usually binary compounds (i.e., only two elements in the compound) and are also insoluble in solutions. Now I hope you can form your own examples, but common examples are Sodium Hydride (NaH), Lithium hydride (LiH), Potassium hydride (KH) etc.
Elements in the same group have same:- a)Number of valence electrons
- b)Density
- c)Atomic radius
- d)Nuclear charge
Correct answer is option 'A'. Can you explain this answer?
Elements in the same group have same:
a)
Number of valence electrons
b)
Density
c)
Atomic radius
d)
Nuclear charge
|
Lavanya Menon answered |
- Elements in the same group have the same number of valence electrons in their outermost shell, hence, have similar properties.
- Elements in the same period don't have same number of valence electrons, hence, have different properties. But, elements in the same period have same number of shells.
Among Al2O3, SiO2, P2O3 and SO2 the correct order of acid strength is : [AIEEE-2004]- a)Al2O3 < SiO2 < SO2 < P2O3
- b)SiO2 < SO2 < Al2O3 < P2O3
- c)SO2 < P2O3 < SiO2 < Al2O3
- d)Al2O3 < SiO2 < P2O3 < SO2
Correct answer is option 'D'. Can you explain this answer?
Among Al2O3, SiO2, P2O3 and SO2 the correct order of acid strength is : [AIEEE-2004]
a)
Al2O3 < SiO2 < SO2 < P2O3
b)
SiO2 < SO2 < Al2O3 < P2O3
c)
SO2 < P2O3 < SiO2 < Al2O3
d)
Al2O3 < SiO2 < P2O3 < SO2
|
|
Lavanya Menon answered |
While moving along a group from top to bottom acidic nature of oxides decreases and along a period left to right, acidic nature increases.
Al, Si, P, S
Al, Si, P, S
The symbol for element with atomic number 111 and name Unununnium is- a)Uun
- b)Uuu
- c)UUU
- d)None of the above
Correct answer is option 'B'. Can you explain this answer?
The symbol for element with atomic number 111 and name Unununnium is
a)
Uun
b)
Uuu
c)
UUU
d)
None of the above
|
|
Gaurav Kumar answered |
- The element was to be called unununium (with the corresponding symbol of Uuu),a systematic element name as a placeholder, until the element was discovered (and the discovery then confirmed) and a permanent name was decided on.
- Although widely used in the chemical community on all levels, from chemistry classrooms to advanced textbooks, the recommendations were mostly ignored among scientists in the field, who called it element 111, with the symbol of E111, (111) or even simply 111.
Eka aluminium predicted by Mendeleev is which element?- a)Germanium
- b)Magnesium
- c)Gallium
- d)Sodium
Correct answer is option 'C'. Can you explain this answer?
Eka aluminium predicted by Mendeleev is which element?
a)
Germanium
b)
Magnesium
c)
Gallium
d)
Sodium
|
|
Gaurav Kumar answered |
Eka aluminium predicted by Mendeleev is Gallium. Eka-aluminium and gallium are the two names of the same element as Eka -Aluminum has almost exactly the same properties as the actual properties of the gallium element.
According to Dobereiner’s law of triads the number of elements present in each group is:
- a)2
- b)4
- c)5
- d)3
Correct answer is option 'D'. Can you explain this answer?
According to Dobereiner’s law of triads the number of elements present in each group is:
a)
2
b)
4
c)
5
d)
3
|
|
Geetika Shah answered |
- According to Dobereiner's law of triads each triad contains three elements.
- He also noticed that the middle element of each of the triads had an atomic weight about halfway between the atomic weights of the other two.
The oxygen family is also known as:- a)halogen family
- b)oxo family
- c)chalcogen family
- d)peroxo family
Correct answer is option 'C'. Can you explain this answer?
The oxygen family is also known as:
a)
halogen family
b)
oxo family
c)
chalcogen family
d)
peroxo family
|
|
Rajat Kapoor answered |
The Oxygen family, sometimes also known as chalcogens, is group 16 on the periodic table and consisted of oxygen, sulfur, selenium, tellurium, polonium and ununhexium.
Moseley performed experiments and studied the frequencies of which radiations emitted from the elements?- a)Gamma rays
- b)X-rays
- c)UV rays
- d)Infra red rays
Correct answer is option 'B'. Can you explain this answer?
Moseley performed experiments and studied the frequencies of which radiations emitted from the elements?
a)
Gamma rays
b)
X-rays
c)
UV rays
d)
Infra red rays
|
|
Naina Bansal answered |
Moseley performed experiments and studied the frequencies of the X-rays emitted from the elements.
Which of the following set of elements obeyes Newland’s octave rule -- a)Na, K, Rb
- b)F, Cl, Br
- c)Be, Mg, Ca
- d)B, Al, Ga
Correct answer is option 'C'. Can you explain this answer?
Which of the following set of elements obeyes Newland’s octave rule -
a)
Na, K, Rb
b)
F, Cl, Br
c)
Be, Mg, Ca
d)
B, Al, Ga
|
|
Gaurav Kumar answered |
Because Be Mg and Ca have same chemical properties.
The electronegativity of following elements increases in the order of?- a)Si, P, C, N
- b)P, Si, N, C
- c)C, N, Si, P
- d)N, Si, C, P
Correct answer is option 'A'. Can you explain this answer?
The electronegativity of following elements increases in the order of?
a)
Si, P, C, N
b)
P, Si, N, C
c)
C, N, Si, P
d)
N, Si, C, P
|
|
Pooja Shah answered |
Si,P,C,N
Electronegativity increases along a period and decreases down the group.Nitrogen is expected to have maximum electronegativity.
The first period has how many orbitals?- a)1
- b)3
- c)2
- d)4
Correct answer is option 'A'. Can you explain this answer?
The first period has how many orbitals?
a)
1
b)
3
c)
2
d)
4
|
|
Raghav Bansal answered |
1st period contains only 2 elements hydrogen and helium having atomic no. 1 and 2 respectively.
The electronic configuration of hydrogen is 1s1 while that of helium is 1s2. Both contain only s subshell. S subshell that only contains 1 orbital i.e. z.
Thus, 1st period has 1 orbital.
Johann Dobereiner classified elements in group of three elements called as- a)Trinity
- b)Trials
- c)Triads
- d)Diads
Correct answer is option 'C'. Can you explain this answer?
Johann Dobereiner classified elements in group of three elements called as
a)
Trinity
b)
Trials
c)
Triads
d)
Diads
|
|
Om Desai answered |
In 1829, Johann Dobereiner, a German scientist made some groups of three elements each and called them triads.
He observed that the atomic mass of the middle element of a triad was nearly equal to the arithmetic mean of the atomic masses of the other two elements. All three elements of a triad were similar in their properties.
Which of the following elements will have the largest atomic radii?- a)Sr
- b)Al
- c)Li
- d)Ca
Correct answer is option 'A'. Can you explain this answer?
Which of the following elements will have the largest atomic radii?
a)
Sr
b)
Al
c)
Li
d)
Ca
|
|
Pooja Shah answered |
Strontium has the highest atomic radii because it on the group atomic radius increases also it belongs to 4D so if there is doubt of Lanthanide contraction then the size of 4D is largest followed by 3D and 5D has the smallest size.
Pick out the isoelectronic structure from the following : [AIEEE-2005]I. +CH3 II. H3O+ III. NH3 IV. CH3-- a)I and II
- b)III and IV
- c)I and III
- d)II, III and IV
Correct answer is option 'D'. Can you explain this answer?
Pick out the isoelectronic structure from the following : [AIEEE-2005]
I. +CH3
II. H3O+
III. NH3
IV. CH3-
a)
I and II
b)
III and IV
c)
I and III
d)
II, III and IV
|
|
Lavanya Menon answered |
H3O+, NH3 and CH3- are not only isoelectronic but are also iso-structural with pyramidal shape.
However CH3+ is trigonal planar with one empty orbital perpendicular to this plane.
Among the following oxides, neutral oxide is:- a)ZnO2
- b)SiO2
- c)CO
- d)SnO2
Correct answer is option 'C'. Can you explain this answer?
Among the following oxides, neutral oxide is:
a)
ZnO2
b)
SiO2
c)
CO
d)
SnO2
|
|
Shreya Gupta answered |
Neutral oxide. Neutral oxides are oxides which are neither acidic nor basic. In other words, oxides which neither react with acids or with bases are called neutral oxides. Some examples of neutral oxides are nitrous oxide (N2O), and carbon monoxide (CO).
The transition elements have characteristic electronic configuration which can be represented as:- a)(n-1) d1-10 ns0-2
- b)(n-2) d1-10 (n-1) p6 ns2
- c)(n-1)s2 p6 d 10 ns2 np6 nd1-10
- d)(n-2) d1-10 (n-1) s2 p6 d1 or 2 ns1
Correct answer is option 'A'. Can you explain this answer?
The transition elements have characteristic electronic configuration which can be represented as:
a)
(n-1) d1-10 ns0-2
b)
(n-2) d1-10 (n-1) p6 ns2
c)
(n-1)s2 p6 d 10 ns2 np6 nd1-10
d)
(n-2) d1-10 (n-1) s2 p6 d1 or 2 ns1
|
|
Om Desai answered |
Transition elements are d-block elements and the characteristic electronic configuration of d block element is in option A
Which of the following elements has the largest ionisation enthalpy?- a)O
- b)F
- c)C
- d)N
Correct answer is option 'B'. Can you explain this answer?
Which of the following elements has the largest ionisation enthalpy?
a)
O
b)
F
c)
C
d)
N
|
|
Gaurav Kumar answered |
Ionisation energy increases along a period. The very next elements C,N,O,F results F with higher ionisation energy.
Mendeleev predicted the existence of which element/elements in the periodic table?- a)Gallium
- b)Sodium and germanium
- c)Gallium and germanium
- d)Germanium and Gold
Correct answer is option 'C'. Can you explain this answer?
Mendeleev predicted the existence of which element/elements in the periodic table?
a)
Gallium
b)
Sodium and germanium
c)
Gallium and germanium
d)
Germanium and Gold
|
|
Neha Joshi answered |
Gallium and Germanium were the elements not discovered at that time and Mendeleev put gaps in the periodic table.
Gallium was called as Eka aluminium
Germanium was called as Eka silicon
Gallium was called as Eka aluminium
Germanium was called as Eka silicon
For alkali metals, which one of the following trends is INCORRECT?
- a)Hydration energy: Li > Na > K > Rb
- b)Ionization energy: Li > Na > K > Rb
- c)Atomic size: Li < Na < K < Rb
- d)Density: Li < Na < K < Rb
Correct answer is option 'D'. Can you explain this answer?
For alkali metals, which one of the following trends is INCORRECT?
a)
Hydration energy: Li > Na > K > Rb
b)
Ionization energy: Li > Na > K > Rb
c)
Atomic size: Li < Na < K < Rb
d)
Density: Li < Na < K < Rb
|
|
Om Desai answered |
Density: Li < Na < K < Rb.
The density of K is lower than that of Na. Thus, option D is incorrect. The correct trend is
Li < K < Na < Rb
The density of K is lower than that of Na. Thus, option D is incorrect. The correct trend is
Li < K < Na < Rb
The element which shows only negative oxidation state/s among following elements is:- a)Iodine
- b)Fluorine
- c)Bromine
- d)Chlorine
Correct answer is option 'B'. Can you explain this answer?
The element which shows only negative oxidation state/s among following elements is:
a)
Iodine
b)
Fluorine
c)
Bromine
d)
Chlorine
|
|
Geetika Shah answered |
Fluorine has highest electronegativity among all known elements, so it shows only negative oxidation states.
Can you explain the answer of this question below:The atomic numbers of vanadium (V). Chromium (Cr), manganese (Mn) and iron (Fe) respectively 23, 24, 25 and 26. Which one of these may be expected to have the higher second ionization enthalpy ? [AIEEE-2003]
- A:
Cr
- B:
Mn
- C:
Fe
- D:
V
The answer is A.
The atomic numbers of vanadium (V). Chromium (Cr), manganese (Mn) and iron (Fe) respectively 23, 24, 25 and 26. Which one of these may be expected to have the higher second ionization enthalpy ? [AIEEE-2003]
Cr
Mn
Fe
V
|
Infinity Academy answered |
The electronic configurations are as follows;
V:(Ar)3d34s2
Cr:(Ar)3d54s1
Mn:(Ar)3d54s2
Fe:(Ar)3d64s2
The second ionization of Cr means removal of electron from the stable configuration of 3d5.
The highest second ionization enthalpy is Cr
Hence a is the correct answer.
Which one of the following ions has the highest value of ionic radius ? [AIEEE-2004]- a)O2-
- b)B3+
- c)Li+
- d)F-
Correct answer is option 'A'. Can you explain this answer?
Which one of the following ions has the highest value of ionic radius ? [AIEEE-2004]
a)
O2-
b)
B3+
c)
Li+
d)
F-
|
Hansa Sharma answered |
This can be explained on the basis of z/e, where as z/e ratio increases, the size decreases and when z/e ratio decreases the size increases.
z is atomic number and e is number of electrons.
For Li+, z/e = 3/2 = 1.5
For F-, z/e = 9/10 = 0.9
For O2-, z/e = 8/10 = 0.8
For B3+, z/e = 5/2 = 2.5
The correct option is A.
The basis of long form of periodic table is:- a)Mass number
- b)Atomic weight
- c)Atomic number
- d)Ionic radius
Correct answer is option 'C'. Can you explain this answer?
The basis of long form of periodic table is:
a)
Mass number
b)
Atomic weight
c)
Atomic number
d)
Ionic radius
|
|
Nandini Patel answered |
In long form of periodic table elements are arranged in increasing order of their Atomic number.
The maximum number of elements present in seventh period of the modern periodic table is:- a)32
- b)8
- c)2
- d)18
Correct answer is option 'A'. Can you explain this answer?
The maximum number of elements present in seventh period of the modern periodic table is:
a)
32
b)
8
c)
2
d)
18
|
Anjali Iyer answered |
The total number of electrons that can be accommodated in seventh period are 2 ( in 7s) + 14(in 5f) + 10(in 6d )+ 6(in 7p) = 32. The maximum number of elements present in it is 32.
What is the maximum number of electrons that can be filled in 3d subshell?- a)2
- b)14
- c)6
- d)10
Correct answer is option 'D'. Can you explain this answer?
What is the maximum number of electrons that can be filled in 3d subshell?
a)
2
b)
14
c)
6
d)
10
|
|
Shreya Gupta answered |
There are 5 orbitals in d subshell and each orbital can accommodate 2 electrons. Hence maximum number of electrons that can be filled in 3d subshell is 10.
Among the following elements element with highest ionisation enthalpy is:- a)N
- b)C
- c)O
- d)B
Correct answer is option 'A'. Can you explain this answer?
Among the following elements element with highest ionisation enthalpy is:
a)
N
b)
C
c)
O
d)
B
|
|
Pooja Shah answered |
Among the given molecules, N2 has highest ionization enthalpy.The reason behind is the stability of half-filled orbitals which makes it more stable than other elements in the given option list.
In which of the following arrangements, the sequence is not strictly according to the property written against it ? [AIEEE-2009]- a)CO2<SiO2 <SnO2 <PbO2 : increasing oxidising power
- b)HF< HCl < HBr < HI : increasing acid strength
- c)NH3 <PH3 <AsH3 <SbH3 : increasing basic strength
- d)B < C < O < N : increasing first ionization enthalpy.
Correct answer is option 'C'. Can you explain this answer?
In which of the following arrangements, the sequence is not strictly according to the property written against it ?
[AIEEE-2009]
a)
CO2<SiO2 <SnO2 <PbO2 : increasing oxidising power
b)
HF< HCl < HBr < HI : increasing acid strength
c)
NH3 <PH3 <AsH3 <SbH3 : increasing basic strength
d)
B < C < O < N : increasing first ionization enthalpy.
|
Mira Sharma answered |
As the size of the central non-metal increasing appreciably, the basicity of hydride decreases.
NH3< PH3< AsH3< SbH3
Which of the following elements are called representative elements?- a)p block elements only
- b)s and p block elements only
- c)d block elements only
- d)s block elements only
Correct answer is option 'B'. Can you explain this answer?
Which of the following elements are called representative elements?
a)
p block elements only
b)
s and p block elements only
c)
d block elements only
d)
s block elements only
|
|
Gaurav Kumar answered |
The elements of "s" and "p" blocks except "d" group elements are called as representative elements. Their outer shells are not completely filled with electrons. The elements get the nearest inert gas configuration by losing or gaining or sharing of electrons.
Inert gases belong to which block of the periodic table?- a)s-block
- b)d-block
- c)p-block
- d)f-block
Correct answer is 'A'. Can you explain this answer?
Inert gases belong to which block of the periodic table?
a)
s-block
b)
d-block
c)
p-block
d)
f-block
|
|
Rajeev Saxena answered |
The six noble gases are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn). Their atomic numbers are, respectively, 2, 10, 18, 36, 54, and 86.
In which of the following arrangements, the sequence is not strictly according to the property written against it? [2008]- a)HF < HCl < HBr , HI : increasing acid strength
- b)NH3 < PH3 < AsH3 <SbH3 : increasing basic strength
- c)B < C < O < N : increasing first ionization enthalpy
- d)CO2 < SiO2 < SnO2 < PbO2 : increasing oxidising power
Correct answer is option 'B'. Can you explain this answer?
In which of the following arrangements, the sequence is not strictly according to the property written against it? [2008]
a)
HF < HCl < HBr , HI : increasing acid strength
b)
NH3 < PH3 < AsH3 <SbH3 : increasing basic strength
c)
B < C < O < N : increasing first ionization enthalpy
d)
CO2 < SiO2 < SnO2 < PbO2 : increasing oxidising power
|
|
Lavanya Menon answered |
(a,c) As we move from top to bottom in a group, the acidic strength of hydrides increases. Therefore, order of acidic strength of hydrides of VA and VII A group elements is
NH3 < PH3 < AsH3< SbH3
HF<HCl < HBr <HI
NH3 < PH3 < AsH3< SbH3
HF<HCl < HBr <HI
b) As we move from top to bottom in a group acidic nature (Ka) increases. Therefore, pKa decreases. Thus, order of pKa value of hydrides of VI A group elements is
H2O > H2S >H2Se > H2Te
d) On moving from top to bottom, oxidising power of oxides increases. Thus, order of oxidising power of oxides of IVA group elements is
CO2 < SiO2 < SnO2 < PbO2
H2O > H2S >H2Se > H2Te
d) On moving from top to bottom, oxidising power of oxides increases. Thus, order of oxidising power of oxides of IVA group elements is
CO2 < SiO2 < SnO2 < PbO2
(a,c) As we move from top to bottom in a group, the acidic strength of hydrides increases. Therefore, order of acidic strength of hydrides of VA and VII A group elements is
NH3 < PH3 < AsH3< SbH3
HF<HCl < HBr <HI
NH3 < PH3 < AsH3< SbH3
HF<HCl < HBr <HI
b) As we move from top to bottom in a group acidic nature (Ka) increases. Therefore, pKa decreases. Thus, order of pKa value of hydrides of VI A group elements is
H2O > H2S >H2Se > H2Te
d) On moving from top to bottom, oxidising power of oxides increases. Thus, order of oxidising power of oxides of IVA group elements is
CO2 < SiO2 < SnO2 < PbO2
H2O > H2S >H2Se > H2Te
d) On moving from top to bottom, oxidising power of oxides increases. Thus, order of oxidising power of oxides of IVA group elements is
CO2 < SiO2 < SnO2 < PbO2
The nature of bonds in the compounds of carbon is mostly:- a)Electrovalent
- b)Covalent as well as electrovalent
- c)Covalent
- d)Metallic
Correct answer is option 'C'. Can you explain this answer?
The nature of bonds in the compounds of carbon is mostly:
a)
Electrovalent
b)
Covalent as well as electrovalent
c)
Covalent
d)
Metallic
|
|
Rajat Kapoor answered |
The atomic no. of carbon is 6 which means that a nutral atom of carbon contains 6 electrons .so, the electronic confugration of carbon is 2 and 4. Since a corbon atom has 4 electrons in tis outermost cell ,so it should either lose 4 electrons or gain 4 electrons to achieve the inert gas electron configuration and become stable,its not possible to remove 4 electrons from a carbon atom,its not possible to add as many as 4 electrons to a carbon atom,,therefore carbon atoms can achieve the inert gas electron arrangment only by the sharing of electrons,tthere fore ,carbon alwayz forms covalent bonds.
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