An element X which occurs in the first short period has an outer electronic structure \[{{s}^{2}}{{p}^{1}}\]. What are the formula and acid-base character of its oxides [DCE 1999]

\[{{X}_{2}}{{O}_{3}},\] amphoteric

Which of the following sequence correctly represents the decreasing acid nature of oxides [AMU 2000]

\[C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\]

\[L{{i}_{2}}O>BeO>{{B}_{2}}{{O}_{3}}>C{{O}_{2}}>{{N}_{2}}{{O}_{3}}\]

\[{{N}_{2}}{{O}_{3}}>C{{O}_{2}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\]

\[C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\]

\[{{B}_{2}}{{O}_{3}}>C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>L{{i}_{2}}O>BeO\]

Fluorine, chlorine, bromine and iodine are placed in the same group (17) of the periodic table, because [KCET (Med.) 1999]

Their atoms are generally univalent

They have 7 electrons in the outermost shell of their atom

Elements A and B with their respective electronic configurations \[3{{d}^{10}}\,4{{s}^{1}}\] and \[4{{d}^{10}}\,5{{s}^{1}}\] in their outermost shell are

A is a non-metal and B is coinage metal

A is a coinage metal and B is non-metal

The correct order of reactivity of halogen is [BHU 2000]

Iodine > bromine > chlorine > flourine

Flourine > bromine > chlorine > iodine

Flourine > chlorine > bromine > iodine

Iodine > bromine > chlorine > flourine

Bromine > chlorine > flourine > iodine

Pentavalency in phosphorus is more stable when compared to that of nitrogen even through they belong to same group is due to [KCET 2002]

Dissimilar electronic configuration

Which is correct in the following?

Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\]while that of \[C{{l}^{-}}\] ion is \[0.81\,\overset{\text{o}}{\mathop{\text{A}}}\,\]

Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\] while that of \[C{{l}^{+}}\] ion is \[1.54\,\overset{\text{o}}{\mathop{\text{A}}}\,\]

Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\] while that of Na atom is \[1.54\,\overset{\text{o}}{\mathop{\text{A}}}\,\]

Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\]while that of \[C{{l}^{-}}\] ion is \[0.81\,\overset{\text{o}}{\mathop{\text{A}}}\,\]

Radius of Na atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\] while that of \[N{{a}^{+}}\] ion is \[1.54\,\overset{\text{o}}{\mathop{\text{A}}}\,\]

Why is the \[{{E}^{o}}\] value of \[M{{n}^{+3}}\text{/}M{{n}^{+2}}\] couple much more positive than \[C{{r}^{+3}}/C{{r}^{+2}}\]

Due larger third ionization enthalpy of Cr

Due to larger third ionization enthalpy of Mn

Due larger third ionization enthalpy of Cr

Due to smaller third ionization enthalpy of Mn

Due to lesser hydration enthalpy of Cr

The first ionisation enthalpies for two isotopes of the same elements are

\[|{{E}_{1}}=2|{{E}_{(II\text{ isotope)}}}\] (n isotope)

The statement that is not correct for periodic classification of elements is

the first ionisation enthalpies of elements generally increase with increase in atomic number as we go along a period.

the properties of elements are periodic functions of their atomic numbers

non - metallic elements are less in number than metallic elements

for transition elements, the 3d-orbitals are filled with electrons after 3p-orbitals and before 4s-orbitals.

the first ionisation enthalpies of elements generally increase with increase in atomic number as we go along a period.

Consider the following ionization enthalpies of two elements 'A' and 'B'. Elements 1st Lionization 2nd Enthalpy (KJ/mol) A 899 1757 14847 B 737 1450 7731 Which of the following statements is correct?

Both 'A' and 'B' belong to group-2 where 'A' comes below 'B'.

Both 'A' and 'B' belong to group-1 where 'B' comes below 'A'.

Both 'A' and 'B' belong to group-1 where 'A' comes below 'B.

Both 'A' and 'B' belong to group-2 where 'B' comes below 'A'.

Both 'A' and 'B' belong to group-2 where 'A' comes below 'B'.

Which transition involves maximum amount of energy?

\[{{M}^{-}}\left( g \right)\xrightarrow{{}}M\left( g \right)+{{e}^{-}}\]

\[{{M}^{-}}\left( g \right)\xrightarrow{{}}{{M}^{+}}\left( g \right)+2{{e}^{-}}\]

\[{{M}^{+}}\left( g \right)\xrightarrow{{}}{{M}^{2+}}\left( g \right)+{{e}^{-}}\]

\[{{M}^{2+}}\left( g \right)\xrightarrow{{}}{{M}^{3+}}\left( g \right)+{{e}^{-}}\]

Which of the following series correctly represents relations between the elements from X to Y?\[X\to Y\]

\[~{}_{18}Ar\to {}_{54}Xe\] Noble character increases

\[{}_{3}Li\to {}_{19}K\] Ionization enthalpy increases

\[{}_{9}F\to {}_{35}Br\] Electron gain enthalpy (negative sign) increases

\[{}_{6}C\to {}_{32}Ge\] Atomic radii increases

\[~{}_{18}Ar\to {}_{54}Xe\] Noble character increases

Choose the correct decreasing order of thermal stability of the following.

Ba\[C{{O}_{3}}\] > Ca\[C{{O}_{3}}\] > Mg\[C{{O}_{3}}\] > Be\[C{{O}_{3}}\]

Be\[C{{O}_{3}}\] > Mg\[C{{O}_{3}}\] > Ca\[C{{O}_{3}}\] > Ba\[C{{O}_{3}}\]

Ba\[C{{O}_{3}}\] > Ca\[C{{O}_{3}}\] > Mg\[C{{O}_{3}}\] > Be\[C{{O}_{3}}\]

Be\[C{{O}_{3}}\] > Ca\[C{{O}_{3}}\] > Ba\[C{{O}_{3}}\] > Mg\[C{{O}_{3}}\]

Mg\[C{{O}_{3}}\] > Ca\[C{{O}_{3}}\] > Ba\[C{{O}_{3}}\] > Be\[C{{O}_{3}}\]

As one moves along a given row in the periodic table, ionization energy [CPMT 1976, 89; NCERT 1978; EAMCET 1985]

First increases, then decreases

11242 + Mcqs in Chemistry in Joint Entrance Exam - Main (JEE Main) Page 219 McqOptions

10901.	An element X which occurs in the first short period has an outer electronic structure \[{{s}^{2}}{{p}^{1}}\]. What are the formula and acid-base character of its oxides [DCE 1999]
A.	\[X{{O}_{3}},\] basic
B.	\[{{X}_{2}}{{O}_{3}},\] basic
C.	\[{{X}_{2}}{{O}_{3}},\] amphoteric
D.	\[X{{O}_{2}},\] acidic
Answer» D. \[X{{O}_{2}},\] acidic

10902.	Which of the following set has the strongest tendency to form anions [AFMC 1999]
A.	Ga, In and Te
B.	Na, Mg and Al
C.	N, O and F
D.	V, Cr and Mn
Answer» D. V, Cr and Mn

10903.	The most basic element is [MP PET 2000; JIPMER 2000]
A.	Fluorine
B.	Iodine
C.	Chlorine
D.	Bromine
Answer» C. Chlorine

10904.	The valency shell of calcium contains [JIPMER 2000]
A.	8 electrons
B.	6 electrons
C.	4 electrons
D.	2 electrons
Answer» E.

10905.	Which of the following elements shows maximum number of different oxidation states in its compounds [CBSE PMT 1998]
A.	\[Eu\]
B.	\[La\]
C.	\[Gd\]
D.	\[Am\]
Answer» E.

10906.	Which is the weakest base [KCET 1993]
A.	NaOH
B.	KOH
C.	\[Ca{{(OH)}_{2}}\]
D.	\[Zn{{(OH)}_{2}}\]
Answer» E.

10907.	Which of the following sequence correctly represents the decreasing acid nature of oxides [AMU 2000]
A.	\[L{{i}_{2}}O>BeO>{{B}_{2}}{{O}_{3}}>C{{O}_{2}}>{{N}_{2}}{{O}_{3}}\]
B.	\[{{N}_{2}}{{O}_{3}}>C{{O}_{2}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\]
C.	\[C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\]
D.	\[{{B}_{2}}{{O}_{3}}>C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>L{{i}_{2}}O>BeO\]
Answer» C. \[C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\]

10908.	Fluorine, chlorine, bromine and iodine are placed in the same group (17) of the periodic table, because [KCET (Med.) 1999]
A.	They are non-metals
B.	They are electronegative
C.	Their atoms are generally univalent
D.	They have 7 electrons in the outermost shell of their atom
Answer» E.

10909.	Oxidising action increases in halogen in the following order [DPMT 1990]
A.	Cl < Br < I < F
B.	Cl < I < Br < F
C.	I < F < Cl < Br
D.	I < Br < Cl < F
Answer» E.

10910.	Which is the best reducing agent [MP PET 2000]
A.	\[{{F}^{-}}\]
B.	\[C{{l}^{-}}\]
C.	\[B{{r}^{-}}\]
D.	\[{{I}^{-}}\]
Answer» E.

10911.	Elements A and B with their respective electronic configurations \[3{{d}^{10}}\,4{{s}^{1}}\] and \[4{{d}^{10}}\,5{{s}^{1}}\] in their outermost shell are
A.	Both non-metals
B.	Both coinage metals
C.	A is a non-metal and B is coinage metal
D.	A is a coinage metal and B is non-metal
Answer» C. A is a non-metal and B is coinage metal

10913.	Variable valency in general, is exhibited by [CPMT 1974, 84, 89; DPMT 1981, 82; MP PET 2001]
A.	Transition elements
B.	Gaseous elements
C.	Non-metals
D.	\[s\]-block elements
Answer» B. Gaseous elements

10914.	In the ground state of cobalt atom (Z = 27) there are ....... unpaired electrons and thus the atom is.......
A.	2, diamagnetic
B.	2, paramagnetic
C.	3, diamagnetic
D.	3, paramagnetic
Answer» E.

10916.	The correct order of ionic size of \[{{N}^{3-}},N{{a}^{+}},N{{a}^{+}},{{O}^{2-}},{{F}^{-}},M{{g}^{2+}}\] will be
A.	\[{{O}^{2-}}<N{{a}^{+}}<{{F}^{-}}<{{N}^{3-}}<M{{g}^{2+}}\]
B.	\[M{{g}^{2+}}N{{a}^{+}}<{{F}^{-}}<{{O}^{2-}}<{{N}^{3-}}\]
C.	\[{{F}^{-}}<{{N}^{3-}}<{{O}^{2-}}<M{{g}^{2+}}<N{{a}^{+}}\]
D.	\[{{F}^{-}}<M{{g}^{2+}}<{{O}^{2-}}<N{{a}^{+}}<{{N}^{3-}}\]
Answer» C. \[{{F}^{-}}<{{N}^{3-}}<{{O}^{2-}}<M{{g}^{2+}}<N{{a}^{+}}\]

10918.	Atomic radii of fluorine and neon in Angstrom units are respectively given by
A.	0.72, 1.60
B.	1.60, 1.60
C.	0.72, 0.72
D.	None of these
Answer» B. 1.60, 1.60

10912.	The correct order of reactivity of halogen is [BHU 2000]
A.	Flourine > bromine > chlorine > iodine
B.	Flourine > chlorine > bromine > iodine
C.	Iodine > bromine > chlorine > flourine
D.	Bromine > chlorine > flourine > iodine
Answer» C. Iodine > bromine > chlorine > flourine

10915.	Pentavalency in phosphorus is more stable when compared to that of nitrogen even through they belong to same group is due to [KCET 2002]
A.	Reactivity of phosphorus
B.	Inert nature of nitrogen
C.	Dissimilar electronic configuration
D.	Larger size of phosphorus atom
Answer» E.

10917.	Which is correct in the following?
A.	Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\] while that of \[C{{l}^{+}}\] ion is \[1.54\,\overset{\text{o}}{\mathop{\text{A}}}\,\]
B.	Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\] while that of Na atom is \[1.54\,\overset{\text{o}}{\mathop{\text{A}}}\,\]
C.	Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\]while that of \[C{{l}^{-}}\] ion is \[0.81\,\overset{\text{o}}{\mathop{\text{A}}}\,\]
D.	Radius of Na atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\] while that of \[N{{a}^{+}}\] ion is \[1.54\,\overset{\text{o}}{\mathop{\text{A}}}\,\]
Answer» C. Radius of Cl atoms is \[0.99\,\overset{\text{o}}{\mathop{\text{A}}}\,,\]while that of \[C{{l}^{-}}\] ion is \[0.81\,\overset{\text{o}}{\mathop{\text{A}}}\,\]

10919.	If the electronegativity difference between two atoms A and B is 2.0 then the percentage of covalent character in the molecule is
A.	0.54
B.	0.46
C.	0.23
D.	0.72
Answer» C. 0.23

10920.	Why is the \[{{E}^{o}}\] value of \[M{{n}^{+3}}\text{/}M{{n}^{+2}}\] couple much more positive than \[C{{r}^{+3}}/C{{r}^{+2}}\]
A.	Due to larger third ionization enthalpy of Mn
B.	Due larger third ionization enthalpy of Cr
C.	Due to smaller third ionization enthalpy of Mn
D.	Due to lesser hydration enthalpy of Cr
Answer» B. Due larger third ionization enthalpy of Cr

10921.	The first ionisation enthalpies for two isotopes of the same elements are
A.	same
B.	different
C.	some what different
D.	\[\|{{E}_{1}}=2\|{{E}_{(II\text{ isotope)}}}\] (n isotope)
Answer» B. different

10922.	The law of triads is applicable to -
A.	C, N, O
B.	H, O, N
C.	Na, K, Rb
D.	Cl, Br, I
Answer» E.

10923.	What should be the atomic number of the next halogen if discovered in future?
A.	115
B.	119
C.	117
D.	121
Answer» D. 121

10924.	The statement that is not correct for periodic classification of elements is
A.	the properties of elements are periodic functions of their atomic numbers
B.	non - metallic elements are less in number than metallic elements
C.	for transition elements, the 3d-orbitals are filled with electrons after 3p-orbitals and before 4s-orbitals.
D.	the first ionisation enthalpies of elements generally increase with increase in atomic number as we go along a period.
Answer» D. the first ionisation enthalpies of elements generally increase with increase in atomic number as we go along a period.

10925.	When an isolated gaseous cation \[{{X}^{+}}(g)\] is converted into \[{{X}^{-}}(g)\] anion, the amount of energy released is 16.8 eV. Calculate the electro negativity value of the atom X on Pauling's scale.
A.	1
B.	2
C.	4
D.	3
Answer» E.

Explore topic-wise MCQs in Joint Entrance Exam - Main (JEE Main).

An element X which occurs in the first short period has an outer electronic structure \[{{s}^{2}}{{p}^{1}}\]. What are the formula and acid-base character of its oxides [DCE 1999]

Which of the following set has the strongest tendency to form anions [AFMC 1999]

The most basic element is [MP PET 2000; JIPMER 2000]

The valency shell of calcium contains [JIPMER 2000]

Which of the following elements shows maximum number of different oxidation states in its compounds [CBSE PMT 1998]

Which is the weakest base [KCET 1993]

Which of the following sequence correctly represents the decreasing acid nature of oxides [AMU 2000]

Fluorine, chlorine, bromine and iodine are placed in the same group (17) of the periodic table, because [KCET (Med.) 1999]

Oxidising action increases in halogen in the following order [DPMT 1990]

Which is the best reducing agent [MP PET 2000]

Elements A and B with their respective electronic configurations \[3{{d}^{10}}\,4{{s}^{1}}\] and \[4{{d}^{10}}\,5{{s}^{1}}\] in their outermost shell are

The correct order of reactivity of halogen is [BHU 2000]

Variable valency in general, is exhibited by [CPMT 1974, 84, 89; DPMT 1981, 82; MP PET 2001]

In the ground state of cobalt atom (Z = 27) there are ....... unpaired electrons and thus the atom is.......

Pentavalency in phosphorus is more stable when compared to that of nitrogen even through they belong to same group is due to [KCET 2002]

The correct order of ionic size of \[{{N}^{3-}},N{{a}^{+}},N{{a}^{+}},{{O}^{2-}},{{F}^{-}},M{{g}^{2+}}\] will be

Which is correct in the following?

Atomic radii of fluorine and neon in Angstrom units are respectively given by

If the electronegativity difference between two atoms A and B is 2.0 then the percentage of covalent character in the molecule is

Why is the \[{{E}^{o}}\] value of \[M{{n}^{+3}}\text{/}M{{n}^{+2}}\] couple much more positive than \[C{{r}^{+3}}/C{{r}^{+2}}\]

The first ionisation enthalpies for two isotopes of the same elements are

The law of triads is applicable to -

What should be the atomic number of the next halogen if discovered in future?

The statement that is not correct for periodic classification of elements is

When an isolated gaseous cation \[{{X}^{+}}(g)\] is converted into \[{{X}^{-}}(g)\] anion, the amount of energy released is 16.8 eV. Calculate the electro negativity value of the atom X on Pauling's scale.

Find the atomic number of element belonging to 4th period and 17th group in Modem periodic table:

The electronic configuration of an element is \[1{{s}^{2}},\text{ }2{{s}^{2}}2{{p}^{6}},\text{ }3{{s}^{2}}3{{p}^{4}}\]. The atomic number of the element present just below the above element in the periodic table -

The correct order of electron affinities of N, O, S and Cl are

Sodium can't exhibit + 2 oxidation state because its second ionisation potential value is

The atomic numbers of vanadium (V), chromium (Cr), manganese (Mn) and iron (Fe) are, respectively 23, 24, 25 and 26. Which one of these may be expected to have the highest second ionisation enthalpy?

I.E. of one H atom is \[2.18\times {{10}^{-18}}J\]. The I.E. of H atom is \[kJ\,\,mol{{e}^{-1}}\]is -

Covalent radius of nitrogen is 70 pm. Hence, covalent radius of boron is about:

Consider the following ionization enthalpies of two elements 'A' and 'B'. Elements 1st Lionization 2nd Enthalpy (KJ/mol) A 899 1757 14847 B 737 1450 7731 Which of the following statements is correct?

Consider the following information about element P and Q:Period numberGroup numberP215Q32

Which transition involves maximum amount of energy?

The increasing order of electron affinity of N, P and As is

Aqueous solutions of two compounds \[{{M}_{1}}-O-H\] and \[{{M}_{2}}-O-H\] are prepared in two different beakers. If, the electronegativity of \[{{M}_{1}}=3.4,\]\[{{M}_{2}}=1.2,\,\,O=3.5\] and \[H=2.1\] then the nature of two solutions will be respectively:

The elements with zero electron affinity are

First three ionisation energies (in kJ/mol) of three representative elements are given below: Element \[I{{E}_{1}}\] \[I{{E}_{2}}\] \[I{{E}_{3}}\] P 495.8 4562 6910 Q 737.7 1451 7733 R 577.5 1817 2745 Then incorrect option is:

Which of the following series correctly represents relations between the elements from X to Y?\[X\to Y\]

Choose the correct decreasing order of thermal stability of the following.

The screening effect of d-electron is

For C, N, O, and F, which of the following orders is correct for IP ?

Which of the following alkali metal ions has lowest ionic mobility in aqueous solutions [DPMT 2004]

On going left to right in a period, in transition metals, their atomic volumes [MP PMT 2003]

As one moves along a given row in the periodic table, ionization energy [CPMT 1976, 89; NCERT 1978; EAMCET 1985]

Which of the following element has the lowest ionization potential [CPMT 1976; RPMT 2002]

Which of the following has least ionization potential [CPMT 1982, 93]

Which among the following factors is the most important in making fluorine the strongest oxidizing halogen [AIEEE 2004]

10926.	Find the atomic number of element belonging to 4th period and 17th group in Modem periodic table:
A.	17
B.	25
C.	59
D.	35
Answer» E.

10927.	The electronic configuration of an element is \[1{{s}^{2}},\text{ }2{{s}^{2}}2{{p}^{6}},\text{ }3{{s}^{2}}3{{p}^{4}}\]. The atomic number of the element present just below the above element in the periodic table -
A.	36
B.	34
C.	33
D.	32
Answer» C. 33

10928.	The correct order of electron affinities of N, O, S and Cl are
A.	\[O<N<Cl<S\]
B.	\[O<S<Cl<N\]
C.	\[O=Cl<N=S\]
D.	\[N<O<S<Cl\]
Answer» E.

10929.	Sodium can't exhibit + 2 oxidation state because its second ionisation potential value is
A.	zero
B.	equal to first
C.	less than first
D.	much higher than the first
Answer» B. equal to first

10930.	The atomic numbers of vanadium (V), chromium (Cr), manganese (Mn) and iron (Fe) are, respectively 23, 24, 25 and 26. Which one of these may be expected to have the highest second ionisation enthalpy?
A.	V
B.	Cr
C.	Mn
D.	Fe
Answer» C. Mn

10931.	I.E. of one H atom is \[2.18\times {{10}^{-18}}J\]. The I.E. of H atom is \[kJ\,\,mol{{e}^{-1}}\]is -
A.	\[1505\,kJ\,mo{{l}^{-1}}\]
B.	\[1310\,kJ\,mo{{l}^{-1}}\]
C.	\[1608\,kJ\,mo{{l}^{-1}}\]
D.	None
Answer» C. \[1608\,kJ\,mo{{l}^{-1}}\]

10932.	A, B and C are hydroxy compounds of the elements P, Q and R respectively. P, Q and R are in the same period of the periodic table. A gives an aqueous solution of \[pH>7\]. B reacts with both strong acids and strong alkalies. C gives an aqueous solution which is strongly alkaline. Which of the following statement(s) is/are true? I. All the three elements are metals. II. The atomic radius decreases in the order P, Q, R. III. The electron negativities decrease from P to Q to R. IV. P, Q and R could be \[P,Al\] and Na respectively.
A.	I, II and IV
B.	III and IV only
C.	II, III and IV
D.	All are correct
Answer» C. II, III and IV

10933.	Covalent radius of nitrogen is 70 pm. Hence, covalent radius of boron is about:
A.	60 pm
B.	110 pm
C.	50 pm
D.	40 pm
Answer» C. 50 pm

10934.	Consider the following ionization enthalpies of two elements 'A' and 'B'. Elements 1st Lionization 2nd Enthalpy (KJ/mol) A 899 1757 14847 B 737 1450 7731 Which of the following statements is correct?
A.	Both 'A' and 'B' belong to group-1 where 'B' comes below 'A'.
B.	Both 'A' and 'B' belong to group-1 where 'A' comes below 'B.
C.	Both 'A' and 'B' belong to group-2 where 'B' comes below 'A'.
D.	Both 'A' and 'B' belong to group-2 where 'A' comes below 'B'.
Answer» D. Both 'A' and 'B' belong to group-2 where 'A' comes below 'B'.

10935.	Consider the following information about element P and Q:Period numberGroup numberP215Q32
A.	QP
B.	\[{{Q}_{2}}{{P}_{3}}\]
C.	\[{{Q}_{3}}{{P}_{2}}\]
D.	\[{{Q}_{2}}P\]
Answer» D. \[{{Q}_{2}}P\]