AWES TGT Chemistry Mock Test - 3 - AWES TGT/PGT MCQ

NEP 2020 aims to achieve a Gross Enrollment Ratio (GER) of 50% in higher education by 2035.

Inclusive Education means education for all children in school as It refers to the inclusion of all children in the education system, regardless of their differences and disabilities.

• It values the diversity, each child brings to the classroom and facilitates all with equal opportunities to learn and grow.
• Inclusive education improves the quality and making provisions of education for all. >Inclusive education welcomes and celebrates diversity.
• It provides a provision to include disabled children along with normal children in a regular classroom environment.
• It refers to an education system that accommodates all children regardless of their physical, intellectual, social, emotional, linguistic, or other conditions.

Key Points

Basic Principles of Inclusive Education:

• Equity and equal opportunities for all.
• Well constructed educational plan.
• Use of multilingualism as a resource.
• Use of specific pedagogical strategies.
• Sensitization towards individual differences.

Important Points

Institutional initiative for inclusive education can be evidenced when :

• Time is provided for teams of teachers and paraprofessionals to plan together
• A differentiated curriculum is designed
• School provides students to explore different co-curricular activities as per their interests.

Additional Information

• Entry-level tests to enroll students should not be supported according to NCF
• School should have differentiated material for all students
• Instead of common assessments, assessments as per the need of learners should be conducted.

Hence, we can say that institutional initiative for inclusive education can be evidenced when time is provided for teams of teachers and paraprofessionals to plan together.

(V) form s m ost stable, tertiary allylic, carbocation. (II) is vinylic halide, least reactive.

Coordination No. in NaCl is 6.

Dehydration of alcohol to alkene in presence of concentrated H₂SO₄ involves the –OH group in the alcohol that donates two electrons to H⁺ from the acid reagent, forming an alkyloxonium ion. The deprotonated acid (the nucleophile) then attacks the hydrogen adjacent to the carbocation and form a double bond.

Thus, the initiation step is protonation of alcohol.

The correct option is C.

• This yellow colour is due to metal excess defect of anionic valency.
• Na+ion deposited on the surface of crystal of NaCl . The Cl-ion diffused to form NaCl. This happens by loss of electron from Na to Na+.
• The released electro diffused into the crystal and occupy anionic site called F center which imparts yellow colour to NaCl.

Br-atom has configuration

To get pentavalency, two of the p-orbitals are unpaired and electrons are shifted to 4d-orbitals. 

In this excited state, sp³d²-hybridisation occurs giving octahedral structure. Five positions are occupied by F atoms forming sigma bonds with hybrid bonds and one position occupied by lone pair, i.e., the molecule as a square pyramidal shape. 

 

• There are a total of 7 periods in the periodic table.
• The sixth period of the periodic table contains 32 elements.
• It is beginning with cesium and ends with radon.
• Lead (Pb) is currently the last stable element whereas all subsequent elements are radioactive.

Answer:

Given

Density of water (ρ) = 1g/cm³

Molar mass of water (M) = 18 g/mol

∴ Molar volume (Vm) = M/ρ

Vm = 18 cm³/mol

∴ Volume of 1 molecule of water = V_m/N_A

Where N_A is Avogadro number

Volume of 1 molecule of water = 18/(6.022 × 10²³)

Volume of 1 molecule of water = 2.989 × 10^-23 ≈ 3 × 10^-23.

Ksp = S²
⇒ 6.4 × 10^–5 = S²
⇒ S = 8 × 10^–3 mole/L
S = 8 × 10^–3 × 10³ mole/m³
⇒ S = 8 mole/m³

KCI is an ionic compound. Force of attraction (F) between K+


Greater the value of D, smaller the value of F, hence larger the solubility.
Note D for CH₃OCH₃ is least out of given solvents, thus solubility is minimum.

Atomic and ionic radii increase down the group due to increasing number of quantum shells.

Atomic size decreases across the period.
Cl has a smaller size than Ar due to the inert nature atoms exist as single atoms.

The metallic character of group 14 elements increases from top to bottom because removal of electron becomes easier on moving down the group. Metallic character increases as you move down an element group in the periodic table. This is because electrons become easier to lose as the atomic radius increases, where there is less attraction between the nucleus and the valence electrons because of the increased distance between them.

The correct answer is Option B.
The optically active hydrocarbon X is 3-methyl-1-pentene CH₂=CH−CH(CH₃)CH₂CH_3​. On catalytic hydrogenation, it forms 3-methyl pentane CH₃CH₂CH(CH₃)CH₂CH₃, which is optically inactive.

Δ_rH=Δ_rH_(product)-ΔrH_(reactant)
=3×-393+81+3×110-9.7
=-777.7kJ
ΔH = ΔU+Δn_gRT
AS Δn_g = 0, ΔH = ΔU
So, ΔU = -777.7 kJ

Correct Answer :- b

Explanation : The 2o hydrogens are 20 times more reactive than the 1o ones.

Number of chiral centers = 2

Ford-block elements, group number is equal to the number of electrons in (n - 1)d subshell + number of electrons in valence shell (nth shell).

In non-polar molecular solids, molecules are held by weak dispersion forces or London forces.

Additional Information:

• Non-polar molecules are composed of atoms that have a similar value of electronegativity.
• H₂, Cl₂ and I₂ are some of the typical examples.
• In non-polar Molecular solids, the comprised atoms or molecules are held together by weak dispersion forces or London forces.
• They are soft and non-conductors of electricity.
• They have low melting points and usually exist in a liquid or gaseous state at room temperature and pressure.

• Amorphous solids are isotropic in nature.
• The structure of amorphous solids is similar to that of liquids.
• Hence, these are also called pseudo solids or supercooled liquids.
• Isotropy of amorphous solids is due to the same irregular arrangement of constituent particles along with all the directions.
• Cotton candy is a classic example of amorphous solids. 

1/2X₂  + 3/2Y₂ ⟶XY₃,
ΔH= −30 kJ
ΔS_reaction = ∑ΔS_product−∑ΔS_reactant 
X₂ + 3Y₂ → 2XY₃
​ΔH=−60 kJ
ΔS_reaction = 2×50−3×40−1×60 =100−120−60=−80 JK⁻¹mol⁻¹
 ΔG=ΔH−TΔS=0
ΔH=TΔS
1000×(−60)=−80×T
T=750 K

H₂O₂ behaves as a bleaching agent because it breaks the chemical bonds of the chromophores

sp² hybridisation gives three sp² hybrid orbitals which are planar triangular forming an angle of 120° with each other.
The electronic configurations of three elements A, B and C are given below.
Answer the questions from 14 to 17 on the basis of these configurations.
A ls²2s²2p⁶
B ls²2s²2p⁶3s²3p³
C ls²2s²2p⁶3s²3p^s 

The hardness increases with increasing atomic number.

Isobar means when pressure is constant.

In frame test thermal excitation deexcitation takes place in cation with low Ionisation potential

For option a
12 = [Ne]3s2 , 20 = [Ar]4s2 , 4 = [He]2s2 , 88 = [Ra]7s2.
For option b
8 = [He]2s22p4 , 16 = [Ne]3s23p4 , 34 = [Ar]4s23d104p4 , 2 = 1s2
We can see that only in option a, the last electrons enter in similar group. So, option a is correct.
Similarly we can check for option c and d as done above. However they won't fall in the same group.