Thursday, November 21, 2024

MCQ Chemistry Unit 3: Classification of Elements and Periodicity in Properties, HS 1st year

1. Who is credited with the development of the Modern Periodic Table?

A. Johann Dobereiner
B. Dmitri Mendeleev
C. Henry Moseley
D. Lothar Meyer

Answer: B. Dmitri Mendeleev

2. What is the Modern Periodic Law?
A. The properties of elements are a periodic function of their atomic weights.
B. The properties of elements are a periodic function of their atomic numbers.
C. Elements are arranged by increasing mass.
D. Elements are arranged alphabetically.

Answer: B. The properties of elements are a periodic function of their atomic numbers.

3. What are elements in Groups 1 and 2 known as?
A. Transition elements
B. Halogens
C. Alkali and alkaline earth metals
D. Noble gases

Answer: C. Alkali and alkaline earth metals

4. Which element has the highest electronegativity according to the Pauling scale?
A. Oxygen
B. Fluorine
C. Chlorine
D. Nitrogen

Answer: B. Fluorine

5. How many periods are present in the Modern Periodic Table?
A. 7
B. 8
C. 18
D. 10

Answer: A. 7

6. Which element is classified as a metalloid?
A. Boron
B. Sodium
C. Helium
D. Iron

Answer: A. Boron

7. What is the IUPAC name for the element with atomic number 120?
A. Unbinilium
B. Ununseptium
C. Rutherfordium
D. Livermorium

Answer: A. Unbinilium

8. Which group in the periodic table contains noble gases?
A. Group 1
B. Group 2
C. Group 17
D. Group 18

Answer: D. Group 18

9. What type of bond is typically formed by elements in Group 1?
A. Covalent bonds
B. Ionic bonds
C. Metallic bonds
D. Hydrogen bonds

Answer: B. Ionic bonds

10. Which periodic property decreases across a period and increases down a group?
A. Atomic radius
B. Ionization energy
C. Electronegativity
D. Electron affinity

Answer: A. Atomic radius

11. What type of elements are found in the "d-block" of the periodic table?
A. Alkali metals
B. Transition metals
C. Noble gases
D. Non-metals

Answer: B. Transition metals

12. Which scientist proposed the "Law of Triads"?
A. Dmitri Mendeleev
B. Johann Dobereiner
C. Lothar Meyer
D. John Newlands

Answer: B. Johann Dobereiner

13. What is the oxidation state of aluminum in $[AlCl(H_2O)_5]^{2+}$ ?
A. +2
B. +3
C. +4
D. +6

Answer: B. +3

14. Which group contains elements with ns² outermost electronic configuration?
A. Group 1
B. Group 2
C. Group 17
D. Group 18

Answer: B. Group 2

15. The atomic radius increases as you move down a group because of:
A. Increasing nuclear charge
B. Shielding effect
C. Decreasing nuclear charge
D. Greater ionization energy

Answer: B. Shielding effect

16. What is the electron configuration of an element with atomic number 19?
A. $1s^2 2s^2 2p^6 3s^2$
B. $1s^2 2s^2 2p^6 3s^2 3p^6 4s^1$
C. $1s^2 2s^2 2p^6 3s^2 3p^6$
D. $1s^2 2s^2 2p^6 3s^1$

Answer: B. $1s^2 2s^2 2p^6 3s^2 3p^6 4s^1$

17. Which of the following elements has the largest atomic radius?
A. Lithium
B. Sodium
C. Potassium
D. Cesium

Answer: D. Cesium

18. What is the IUPAC name for element with atomic number 114?
A. Livermorium
B. Flerovium
C. Rutherfordium
D. Nihonium

Answer: B. Flerovium

19. Which of the following blocks in the periodic table contains the lanthanoids?
A. s-block
B. p-block
C. d-block
D. f-block

Answer: D. f-block

20. Which type of elements exhibit properties of both metals and non-metals?
A. Metalloids
B. Transition metals
C. Alkali metals
D. Noble gases

Answer: A. Metalloids

21. What is the main characteristic of noble gases?
A. High reactivity
B. Low melting points
C. Completely filled valence shells
D. Metallic properties

Answer: C. Completely filled valence shells

22. What does the "octet rule" refer to?
A. All elements in a group have similar properties
B. Elements prefer having 8 electrons in their valence shell
C. Atomic masses are multiples of eight
D. Elements occur in triads of three

Answer: B. Elements prefer having 8 electrons in their valence shell

23. Which scientist observed that every eighth element had similar properties?
A. John Newlands
B. Johann Dobereiner
C. Dmitri Mendeleev
D. Lothar Meyer

Answer: A. John Newlands

24. What is the formula of a compound formed between silicon and bromine?
A. SiBr
B. SiBr₂
C. SiBr₄
D. Si₂Br₃

Answer: C. SiBr₄

25. What is the oxidation state of oxygen in $H_2O_2$ ?
A. -1
B. -2
C. 0
D. +2

Answer: A. -1

26. Which element is a member of Group 17?
A. Helium
B. Fluorine
C. Sodium
D. Magnesium

Answer: B. Fluorine

27. How many elements are there in the second period of the periodic table?
A. 2
B. 8
C. 18
D. 32

Answer: B. 8

28. The noble gas with the smallest atomic radius is:
A. Helium
B. Neon
C. Argon
D. Krypton

Answer: A. Helium

29. Which group is known as the "halogen family"?
A. Group 16
B. Group 17
C. Group 18
D. Group 2

Answer: B. Group 17

30. What is the electron gain enthalpy of chlorine?
A. Positive
B. Highly negative
C. Neutral
D. Zero

Answer: B. Highly negative

31. Why does ionization energy decrease down a group?
A. Increased nuclear charge
B. Increased atomic size
C. Decreased shielding
D. Increased electronegativity

Answer: B. Increased atomic size

32. What is the outer electronic configuration of group 1 elements?
A. $ns^2$
B. $ns^1$
C. $np^6$
D. $nd^10$

Answer: B. $ns^1$

33. Which of the following is a transition element?
A. Potassium
B. Zinc
C. Copper
D. Neon

Answer: C. Copper

34. The element with the highest ionization energy in Period 2 is:
A. Lithium
B. Carbon
C. Oxygen
D. Neon

Answer: D. Neon

35. Elements of Group 2 are also known as:
A. Alkali metals
B. Alkaline earth metals
C. Transition metals
D. Halogens

Answer: B. Alkaline earth metals

36. What type of oxide is formed by Group 14 elements?
A. Acidic
B. Basic
C. Amphoteric
D. Neutral

Answer: C. Amphoteric

37. What does "f-block" stand for?
A. Metals with f-orbitals filled
B. Noble gases
C. Reactive non-metals
D. Alkali metals

Answer: A. Metals with f-orbitals filled

38. What is the covalency of nitrogen in $NH_3$ ?
A. 1
B. 3
C. 5
D. 7

Answer: B. 3

39. The group 18 elements are referred to as:
A. Halogens
B. Noble gases
C. Alkaline earth metals
D. Transition metals

Answer: B. Noble gases

40. Which period of the periodic table contains lanthanoids?
A. Third
B. Fourth
C. Sixth
D. Seventh

Answer: C. Sixth

১. মৌলসমূহের শ্রেণীবিন্যাস ও পর্যায়বৃত্ত গুণাবলী

প্রয়োজনীয়তা: মৌলসমূহের সংখ্যা বাড়ার সাথে সাথে তাদের বৈশিষ্ট্যগুলি বিশ্লেষণ ও সংরক্ষণ করা কঠিন হয়ে পড়েছিল। বৈজ্ঞানিকরা শ্রেণীবিন্যাসের মাধ্যমে এটি সহজ করতে চেয়েছিলেন।
শ্রেণীবিন্যাসের সূচনা:
- দোবেরাইনারের ত্রয়ী: মৌলগুলিকে গুণাবলীর মিল অনুযায়ী ত্রয়ীতে বিভক্ত করা।
- নিউল্যান্ডসের অক্টাভ: প্রতি অষ্টম মৌল পূর্ববর্তীটির সাথে মিল রাখে।
- মেন্ডেলিফের পর্যায় সারণি: পারমাণবিক ভরের উপর ভিত্তি করে মৌলসমূহকে শ্রেণীবদ্ধ করেন এবং অজানা মৌলগুলির জন্য ফাঁকা স্থান রাখেন।

২. আধুনিক পর্যায় সারণি ও পর্যায়বৃত্ত আইন

আধুনিক পর্যায়বৃত্ত আইন: মৌলগুলির ভৌত ও রাসায়নিক গুণাবলী তাদের পারমাণবিক সংখ্যার পর্যায়বৃত্ত ফাংশন।
সারণির বিন্যাস:
- পর্যায়: অনুভূমিক সারি।
- গোষ্ঠী: উল্লম্ব কলাম।
- ব্লকসমূহ: মৌলসমূহকে s, p, d এবং f ব্লকে বিভক্ত করা হয়েছে।

৩. মৌলসমূহের ইলেকট্রনিক কনফিগারেশন এবং পর্যায় সারণি

প্রতিটি মৌলের অবস্থান তার ইলেকট্রনিক কনফিগারেশন অনুযায়ী নির্ধারিত।
ইলেকট্রন পূরণ:
- s-ব্লক: গ্রুপ ১ ও ২।
- p-ব্লক: গ্রুপ ১৩ থেকে ১৮।
- d-ব্লক: গ্রুপ ৩ থেকে ১২।
- f-ব্লক: ল্যানথানাইডস ও অ্যাক্টিনাইডস।

৪. মৌলসমূহের ধাতব, অধাতব ও উপধাতব বৈশিষ্ট্য

ধাতু: বিদ্যুৎ ও তাপ পরিবাহী, নমনীয়।
অধাতু: ভঙ্গুর, নিম্ন তাপ ও বিদ্যুৎ পরিবাহী।
উপধাতু: ধাতু ও অধাতুর মিশ্র বৈশিষ্ট্য প্রদর্শন করে।

৫. পর্যায়বৃত্ত প্রবণতাসমূহ

পারমাণবিক ও আয়নিক ব্যাসার্ধ:
- পর্যায়ে ডানে গেলে কমে, গোষ্ঠীতে উপরে গেলে বাড়ে।
আয়নায়ন শক্তি:
- পর্যায়ে ডানে বাড়ে, গোষ্ঠীতে উপরে কমে।
ইলেকট্রন গ্রহণ এন্টালপি:
- গ্রুপ ১৭-এ সর্বোচ্চ ঋণাত্মক, গ্রুপ ১৮-এ সর্বাধিক ধনাত্মক।
ইলেকট্রনেগেটিভিটি:
- ডানে বাড়ে, গোষ্ঠীতে উপরে কমে।

৬. রাসায়নিক বিক্রিয়া ও মৌলসমূহের বৈশিষ্ট্য

ডান দিকের মৌলগুলি অক্সিডাইজিং চরিত্র প্রদর্শন করে।
বাম দিকের মৌলগুলি রিডিউসিং চরিত্র প্রদর্শন করে।
মাঝামাঝি মৌলগুলির রাসায়নিক বিক্রিয়া তুলনামূলক কম।

MCQ Chemistry Unit 2: Structure of Atom, HS 1st year (with Chapter Summery in Bengali)

1. What is the charge of an electron?

a) +1.602 × 10⁻¹⁹ C
b) -1.602 × 10⁻¹⁹ C
c) 0
d) +1

Answer: b) -1.602 × 10⁻¹⁹ C

2. Who proposed the atomic theory that laid the foundation for understanding chemical behavior?

a) J.J. Thomson
b) Ernest Rutherford
c) John Dalton
d) Niels Bohr

Answer: c) John Dalton

3. In the cathode ray experiment, which observation indicates that cathode rays are negatively charged?

a) They travel in straight lines in the absence of an electric field.
b) They are deflected towards the positive plate in an electric field.
c) They produce fluorescence on striking certain materials.
d) They depend on the gas in the tube.

Answer: b) They are deflected towards the positive plate in an electric field.

4. What is the mass of a neutron relative to a proton?

a) Equal to the mass of a proton
b) Slightly greater than the mass of a proton
c) Slightly less than the mass of a proton
d) Half the mass of a proton

Answer: b) Slightly greater than the mass of a proton

5. What does the term "isotopes" refer to?

a) Atoms with the same number of electrons but different chemical properties.
b) Atoms with the same atomic number but different mass numbers.
c) Atoms with different atomic numbers but the same number of neutrons.
d) Atoms that behave identically in all reactions.

Answer: b) Atoms with the same atomic number but different mass numbers.

6. According to Rutherford’s nuclear model, where is the mass of the atom concentrated?

a) Distributed throughout the atom.
b) In the electrons orbiting the nucleus.
c) In the nucleus.
d) In the orbital paths of electrons.

Answer: c) In the nucleus.

7. What is the energy of a photon whose frequency is $5 \times 10^{14} \, \text{Hz}$ ? (Planck’s constant $h = 6.626 \times 10^{-34} \, \text{J·s}$ )

a) $3.313 \times 10^{-19} \, \text{J}$
b) $1.986 \times 10^{-19} \, \text{J}$
c) $6.626 \times 10^{-14} \, \text{J}$
d) $2.312 \times 10^{-12} \, \text{J}$

Answer: a) $3.313 \times 10^{-19} \, \text{J}$

8. Which postulate is part of Bohr’s model of the hydrogen atom?

a) Electrons move around the nucleus in elliptical orbits.
b) Electrons emit radiation continuously as they orbit the nucleus.
c) The angular momentum of an electron is quantized.
d) Electrons are stationary around the nucleus.

Answer: c) The angular momentum of an electron is quantized.

9. What did Millikan's oil drop experiment determine?

a) Mass of the electron
b) Charge on the electron
c) Charge-to-mass ratio of the electron
d) Size of the electron

Answer: b) Charge on the electron

10. The smallest and lightest positive ion is called:

a) Neutron
b) Proton
c) Electron
d) Photon

Answer: b) Proton

11. What is the value of the Rydberg constant ( $R_H$ )?

a) $1.097 \times 10^{5} \, \text{cm}^{-1}$
b) $2.18 \times 10^{-18} \, \text{J}$
c) $6.626 \times 10^{-34} \, \text{J·s}$
d) $3.0 \times 10^{8} \, \text{m/s}$

Answer: a) $1.097 \times 10^{5} \, \text{cm}^{-1}$

12. What is the wavelength range of visible light?

a) 200–400 nm
b) 400–750 nm
c) 750–1000 nm
d) 10–400 nm

Answer: b) 400–750 nm

13. Who discovered neutrons?

a) James Chadwick
b) Ernest Rutherford
c) J.J. Thomson
d) Niels Bohr

Answer: a) James Chadwick

14. What does Planck's quantum theory state?

a) Energy can be emitted or absorbed in continuous amounts.
b) Energy is quantized and emitted in discrete packets called quanta.
c) Energy of radiation is independent of its frequency.
d) Energy depends only on the wavelength of radiation.

Answer: b) Energy is quantized and emitted in discrete packets called quanta.

15. Which phenomenon demonstrates the dual nature of light?

a) Photoelectric effect
b) Diffraction
c) Interference
d) Both a and b

Answer: d) Both a and b

16. In the hydrogen spectrum, the series of lines in the visible region is called:

a) Lyman series
b) Balmer series
c) Paschen series
d) Brackett series

Answer: b) Balmer series

17. According to Bohr’s model, what happens when an electron jumps from a higher energy orbit to a lower one?

a) Energy is absorbed.
b) Energy is emitted.
c) Energy remains constant.
d) The atom becomes unstable.

Answer: b) Energy is emitted.

18. What is the angular momentum of an electron in the $n$ -th orbit as per Bohr’s theory?

a) $nh/4\pi$
b) $nh/2\pi$
c) $2nh/\pi$
d) $nh^2/2\pi$

Answer: b) $nh/2\pi$

19. Which particle has a relative charge of +1?

a) Electron
b) Proton
c) Neutron
d) Positron

Answer: b) Proton

20. The dual behavior of matter was proposed by:

a) Max Planck
b) Louis de Broglie
c) Albert Einstein
d) Ernest Rutherford

Answer: b) Louis de Broglie

21. What is the speed of electromagnetic radiation in a vacuum?

a) $3.0 \times 10^{6} \, \text{m/s}$
b) $3.0 \times 10^{8} \, \text{m/s}$
c) $3.0 \times 10^{10} \, \text{m/s}$
d) $3.0 \times 10^{12} \, \text{m/s}$

Answer: b) $3.0 \times 10^{8} \, \text{m/s}$

22. Which of the following series belongs to the ultraviolet region of the hydrogen spectrum?

a) Lyman series
b) Balmer series
c) Paschen series
d) Pfund series

Answer: a) Lyman series

23. What did Rutherford’s alpha-particle scattering experiment conclude?

a) Atoms are indivisible.
b) Atoms have a positively charged nucleus.
c) Electrons revolve in elliptical orbits.
d) All mass is concentrated in electrons.

Answer: b) Atoms have a positively charged nucleus.

24. What type of wave is light?

a) Sound wave
b) Mechanical wave
c) Electromagnetic wave
d) Pressure wave

Answer: c) Electromagnetic wave

25. Which quantum number determines the size of an orbital?

a) Principal quantum number (n)
b) Angular momentum quantum number (l)
c) Magnetic quantum number (m)
d) Spin quantum number (s)

Answer: a) Principal quantum number (n)

26. What is the energy of an electron in the first orbit of hydrogen?

a) $0 \, \text{J}$
b) $-2.18 \times 10^{-18} \, \text{J}$
c) $2.18 \times 10^{-18} \, \text{J}$
d) $-1.09 \times 10^{-18} \, \text{J}$

Answer: b) $-2.18 \times 10^{-18} \, \text{J}$

27. Which principle explains the distribution of electrons in an atom?

a) Aufbau principle
b) Heisenberg uncertainty principle
c) Hund’s rule
d) Pauli exclusion principle

Answer: a) Aufbau principle

28. Who developed the quantum mechanical model of the atom?

a) Niels Bohr
b) Max Planck
c) Erwin Schrödinger
d) Werner Heisenberg

Answer: c) Erwin Schrödinger

29. Which phenomenon could not be explained by classical physics?

a) Diffraction of light
b) Photoelectric effect
c) Reflection of light
d) Refraction of light

Answer: b) Photoelectric effect

30. What is the unit of frequency in the SI system?

a) Meter (m)
b) Joule (J)
c) Hertz (Hz)
d) Second (s)

Answer: c) Hertz (Hz)

31. Which rule is used to fill orbitals of the same energy before pairing electrons?

a) Aufbau principle
b) Pauli exclusion principle
c) Hund’s rule of maximum multiplicity
d) Uncertainty principle

Answer: c) Hund’s rule of maximum multiplicity

32. The wavelength ( $\lambda$ ) and frequency ( $\nu$ ) of light are related by the equation:

a) $c = \nu \lambda$
b) $c = \nu / \lambda$
c) $\lambda = c / \nu^2$
d) $\nu = c / \lambda^2$

Answer: a) $c = \nu \lambda$

33. What does the Pauli exclusion principle state?

a) No two electrons in an atom can have the same set of all four quantum numbers.
b) No two electrons can occupy the same orbital.
c) Orbitals are filled in order of increasing energy.
d) Electrons pair up only after each orbital is singly occupied.

Answer: a) No two electrons in an atom can have the same set of all four quantum numbers.

34. What is the maximum number of electrons in a shell with $n = 3$ ?

a) 18
b) 8
c) 10
d) 32

Answer: a) 18

35. Which particle was discovered by J.J. Thomson?

a) Neutron
b) Proton
c) Electron
d) Photon

Answer: c) Electron

36. The charge-to-mass ratio of the electron was determined by:

a) Rutherford
b) Millikan
c) J.J. Thomson
d) Chadwick

Answer: c) J.J. Thomson

37. Which experiment showed that electrons have particle-like properties?

a) Double-slit experiment
b) Oil drop experiment
c) Photoelectric effect
d) Alpha-particle scattering

Answer: c) Photoelectric effect

38. What happens when an electron is in its ground state?

a) It has maximum energy.
b) It is closest to the nucleus.
c) It is at an infinite distance from the nucleus.
d) It emits energy continuously.

Answer: b) It is closest to the nucleus.

39. What is the shape of an s-orbital?

a) Spherical
b) Dumbbell-shaped
c) Cloverleaf
d) Linear

Answer: a) Spherical

40. What is the principle quantum number ( $n$ ) for the second orbit of an atom?

a) 0
b) 1
c) 2
d) 3

Answer: c) 2

41. In the hydrogen atom, which series lies in the infrared region?

a) Balmer
b) Lyman
c) Paschen
d) Pfund

Answer: c) Paschen

42. Which fundamental particle has no charge?

a) Electron
b) Proton
c) Neutron
d) Positron

Answer: c) Neutron

43. What does the Heisenberg uncertainty principle state?

a) Electrons have both wave and particle properties.
b) It is impossible to know the exact position and momentum of an electron simultaneously.
c) Energy is quantized in discrete levels.
d) Electrons occupy the lowest energy orbital available.

Answer: b) It is impossible to know the exact position and momentum of an electron simultaneously.

44. What does the Aufbau principle dictate?

a) Electrons enter the orbital with the lowest energy first.
b) No two electrons can have the same quantum numbers.
c) Electrons pair up after single occupancy of orbitals.
d) The probability of finding an electron is highest near the nucleus.

Answer: a) Electrons enter the orbital with the lowest energy first.

45. What are the orbitals in the second energy level?

a) s
b) s and p
c) s, p, and d
d) s, p, d, and f

Answer: b) s and p

১. পরমাণুর গঠন

পরমাণুর ধারণা: প্রাচীন ভারতীয় ও গ্রিক দার্শনিকরা (খ্রিষ্টপূর্ব ৪০০) প্রথম পরমাণুর ধারণা দেন। ১৮০৮ সালে জন ডালটন বৈজ্ঞানিক ভিত্তিতে পরমাণু তত্ত্ব উপস্থাপন করেন।
পরমাণুর উপাংশিক কণা: ইলেকট্রন, প্রোটন ও নিউট্রনের আবিষ্কার এবং এদের বৈশিষ্ট্য ব্যাখ্যা।

২. পরমাণু মডেল

থমসনের মডেল: পরমাণু একটি গোলাকার গঠন, যেখানে ধনাত্মক চার্জ সমভাবে বিতরণ থাকে এবং ঋণাত্মক ইলেকট্রন এতে স্থাপিত।
রাদারফোর্ড মডেল: আলফা কণা বিচ্ছুরণের পরীক্ষার মাধ্যমে দেখানো হয় যে পরমাণুর অধিকাংশ স্থান শূন্য, এবং একটি কেন্দ্রীয় নিউক্লিয়াস ধনাত্মক চার্জ বহন করে।
বোর মডেল: পরমাণুর ইলেকট্রন নির্দিষ্ট কক্ষপথে ঘোরে, এবং ইলেকট্রন নির্দিষ্ট শক্তি শোষণ বা বিকিরণ করে কক্ষপথ পরিবর্তন করে।

৩. পরমাণু শক্তি স্তর

ইলেকট্রনের শক্তি স্তর: বোর মডেল অনুযায়ী, পরমাণুতে ইলেকট্রনের শক্তি স্তর স্থির এবং পরিমাণগত।
হাইড্রোজেনের বর্ণালীর ব্যাখ্যা: হাইড্রোজেন পরমাণুর নির্দিষ্ট বর্ণরেখা বোরের তত্ত্বের মাধ্যমে ব্যাখ্যা করা হয়েছে।

৪. ইলেকট্রোম্যাগনেটিক তত্ত্ব

ব্ল্যাক বডি রেডিয়েশন: ম্যাক্স প্ল্যাঙ্ক এর কোয়ান্টাম তত্ত্ব।
ফটোইলেকট্রিক প্রভাব: আলবার্ট আইনস্টাইনের ব্যাখ্যা অনুযায়ী আলো কণা আকারে (ফোটন) শক্তি বহন করে।
দ্বৈত প্রকৃতি: আলো এবং ইলেকট্রনের তরঙ্গ ও কণার প্রকৃতি উভয়ই থাকতে পারে।

৫. কোয়ান্টাম মেকানিক্যাল মডেল

ডি-ব্রগ্লি এবং হাইজেনবার্গ তত্ত্ব: ইলেকট্রন তরঙ্গ প্রকৃতি এবং অবস্থান-গতি সম্পর্কিত অনিশ্চয়তার নীতি।
অরবিটাল ধারণা: পরমাণুতে ইলেকট্রনের অবস্থান সম্ভাব্যতাভিত্তিক।

৬. পরমাণুর ইলেকট্রনিক কনফিগারেশন

আউফবাও নীতি, পাউলি বর্জন নীতি এবং হান্ডের নীতি: ইলেকট্রন কিভাবে অরবিটালে স্থাপিত হয় তা ব্যাখ্যা করা হয়েছে।

MCQs for NEET, JEE, IIT, NIT, CUET, CTET, and SSC Entrance Exams: Your Ultimate Preparation Guide

Are you preparing for competitive exams like NEET, JEE, IIT, NIT, CUET, CTET, or SSC? Multiple Choice Questions (MCQs) are a proven way to enhance your preparation strategy. These MCQs are designed to strengthen your concepts, boost problem-solving skills, and improve time management—key elements to ace any entrance exam.

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MCQ Chemistry Unit 1: Some Basic Concepts of Chemistry, HS 1st year (with Chapter Summery in Bengali)

MCQs from "Some Basic Concepts of Chemistry"

Which of the following is the definition of chemistry?
- A. The study of planets and celestial bodies
- B. The science of molecules and their transformations
- C. The analysis of cultural history
- D. The science of plant growth
- Answer: B
What was the primary focus of early alchemical traditions?
- A. Developing new metals
- B. Discovering the Philosopher's Stone and Elixir of Life
- C. Understanding atomic structure
- D. Creating advanced technologies
- Answer: B
Which of these statements about the states of matter is correct?
- A. Solids have a definite shape and volume.
- B. Liquids have neither definite shape nor volume.
- C. Gases have definite shape and volume.
- D. Liquids have a fixed shape.
- Answer: A
The law of conservation of mass was proposed by:
- A. John Dalton
- B. Joseph Proust
- C. Antoine Lavoisier
- D. Gay Lussac
- Answer: C
According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain:
- A. Different numbers of molecules
- B. Equal numbers of molecules
- C. Different types of molecules
- D. Equal masses of molecules
- Answer: B
The SI unit of luminous intensity is:
- A. Ampere
- B. Mole
- C. Candela
- D. Kelvin
- Answer: C
Which substance is considered a pure compound?
- A. Air
- B. Sugar solution
- C. Glucose
- D. Sand
- Answer: C
Who was the first to propose the atomic theory in India?
- A. Nagarjuna
- B. Charaka
- C. Acharya Kanda
- D. Varāhamihira
- Answer: C
What is the mass of one mole of a substance called?
- A. Atomic mass
- B. Molecular mass
- C. Formula mass
- D. Molar mass
- Answer: D
What is the empirical formula for a compound with 4.07% hydrogen, 24.27% carbon, and 71.65% chlorine by mass?

A. CH2Cl
B. C2H5Cl
C. CHCl
D. C2HCl3
Answer: A

Which branch of science studies the properties, structure, and reactions of material substances?
- A. Biology
- B. Chemistry
- C. Physics
- D. Geology
- Answer: B
In which period did modern chemistry take shape in Europe?
- A. 13th Century
- B. 16th Century
- C. 18th Century
- D. 20th Century
- Answer: C
What is the oldest Ayurvedic epic of India?
- A. Charaka Samhita
- B. Brihat Samhita
- C. Arthashastra
- D. Sushruta Samhita
- Answer: A
Which metal was used by Harappans to improve the hardness of copper?
- A. Zinc
- B. Tin
- C. Lead
- D. Arsenic
- Answer: B
What is the SI base unit of electric current?
- A. Volt
- B. Ampere
- C. Coulomb
- D. Ohm
- Answer: B
Which law states that matter can neither be created nor destroyed?
- A. Law of Definite Proportions
- B. Law of Conservation of Mass
- C. Law of Multiple Proportions
- D. Avogadro’s Law
- Answer: B
Who proposed the Law of Definite Proportions?
- A. Dalton
- B. Joseph Proust
- C. Avogadro
- D. Gay Lussac
- Answer: B
What is the fixed numerical value of Avogadro’s constant?
- A. $6.022 \times 10^{23}$
- B. $3.14 \times 10^3$
- C. $9.81 \times 10^{-1}$
- D. $1.38 \times 10^{-23}$
- Answer: A
Which of the following is an example of a homogeneous mixture?
- A. Oil and water
- B. Sugar solution
- C. Sand and iron filings
- D. Mud
- Answer: B
What is the base SI unit for temperature?
- A. Celsius
- B. Fahrenheit
- C. Kelvin
- D. Joule
- Answer: C

What is the physical state of water at 100°C and 1 atm pressure?
- A. Solid
- B. Liquid
- C. Gas
- D. Plasma
- Answer: C
Who introduced the mole as the SI unit for the amount of substance?
- A. Lavoisier
- B. Dalton
- C. Avogadro
- D. Cannizzaro
- Answer: C
What is the molecular mass of water?
- A. 16.00 u
- B. 18.02 u
- C. 12.01 u
- D. 28.02 u
- Answer: B
What does the term "Rasayan Shastra" refer to in ancient India?
- A. Chemistry
- B. Medicine
- C. Metallurgy
- D. Astronomy
- Answer: A
What is the SI base unit of luminous intensity?
- A. Mole
- B. Kelvin
- C. Candela
- D. Lumen
- Answer: C
What does 1 mole of a substance contain?
- A. $6.022 \times 10^{23}$ atoms
- B. $6.022 \times 10^{23}$ molecules
- C. Both A and B
- D. None of the above
- Answer: C
What is the empirical formula of glucose (C6H12O6)?
- A. CHO
- B. CH2O
- C. C2H4O2
- D. C3H6O3
- Answer: B
Which element is the basis of the modern system of atomic masses?
- A. Hydrogen
- B. Oxygen
- C. Carbon-12
- D. Nitrogen
- Answer: C
Which scientist proposed the atomic theory in 1808?
- A. Democritus
- B. Lavoisier
- C. Dalton
- D. Rutherford
- Answer: C
What is the primary unit used to measure the volume of a liquid in a laboratory?
- A. Litre
- B. Gram
- C. Kelvin
- D. Newton
- Answer: A

Which of the following is not a physical property of a substance?
- A. Colour
- B. Boiling point
- C. Combustibility
- D. Melting point
- Answer: C
The atomic mass unit (amu) is now replaced by which term?
- A. Dalton
- B. Unified mass (u)
- C. Mole
- D. Kilogram
- Answer: B
Which device is commonly used to measure the mass of a substance in a laboratory?
- A. Volumetric flask
- B. Analytical balance
- C. Burette
- D. Thermometer
- Answer: B
What is the molecular mass of methane (CH4)?
- A. 14.00 u
- B. 16.04 u
- C. 12.01 u
- D. 18.02 u
- Answer: B
Which law explains the whole-number ratios in volumes of gases?
- A. Law of Definite Proportions
- B. Gay-Lussac’s Law
- C. Dalton’s Law
- D. Avogadro’s Law
- Answer: B

Which gas law is explained using Avogadro's hypothesis?
- A. Boyle’s Law
- B. Charles’s Law
- C. Gay-Lussac’s Law
- D. Ideal Gas Law
- Answer: D
Who is credited with discovering mercury sulphide?
- A. Nagarjuna
- B. Chakrapani
- C. Varāhamihira
- D. Charaka
- Answer: B
What was the first element discovered as a part of atomic theory in India?
- A. Oxygen
- B. Paramāṇu (atom)
- C. Hydrogen
- D. Nitrogen
- Answer: B
Which of the following elements was used to prepare firecrackers in ancient India?
- A. Potassium nitrate
- B. Sodium chloride
- C. Calcium carbonate
- D. Sulfuric acid
- Answer: A
The law of multiple proportions is credited to which scientist?
- A. Dalton
- B. Proust
- C. Lavoisier
- D. Avogadro
- Answer: A

What does "molar mass" represent?
- A. Mass of one atom
- B. Mass of one molecule
- C. Mass of one mole of a substance
- D. Mass of one ion
- Answer: C
What is the SI unit for mass?
- A. Kilogram
- B. Gram
- C. Mole
- D. Newton
- Answer: A
Which process was well-known in ancient India for making alcohol?
- A. Distillation
- B. Fermentation
- C. Sublimation
- D. Electrolysis
- Answer: B
The golden gloss of black-polished ware in northern India is an example of:
- A. Advanced metallurgy
- B. Controlled kiln temperatures
- C. Alchemy
- D. Dyeing techniques
- Answer: B
The "Charaka Samhita" describes which concept related to metals?
- A. Synthesis of acids
- B. Atomic theory
- C. Reduction of particle size
- D. Properties of alloys
- Answer: C
What is the molecular mass of glucose (C6H12O6)?
- A. 120.0 u
- B. 180.2 u
- C. 100.2 u
- D. 160.0 u
- Answer: B
Who suggested that matter is made up of indivisible particles called atoms?
- A. Kanda
- B. Dalton
- C. Democritus
- D. Lavoisier
- Answer: C
What type of chemical bonding occurs in sodium chloride?
- A. Metallic
- B. Ionic
- C. Covalent
- D. Hydrogen bonding
- Answer: B
The molecular formula is always a multiple of the:
- A. Isotope mass
- B. Average atomic mass
- C. Empirical formula
- D. Ionic formula
- Answer: C
What is the significance of Avogadro’s constant?

A. Number of molecules in 1 liter of gas
B. Number of atoms in 1 mole of substance
C. Number of molecules in 1 gram of substance
D. Volume of gas at STP
Answer: B

Some Basic Concepts of Chemistry

১. রসায়নের বিকাশ

প্রাচীন ভারতীয় রসায়ন:
- রসায়নের ইতিহাস প্রাচীন এবং এটি প্রাথমিকভাবে ধাতু প্রস্তুতি, ওষুধ, প্রসাধনী এবং কাচ তৈরিতে ব্যবহৃত হত।
- মোহেঞ্জোদারো ও হরপ্পার আবিষ্কারে পোড়ামাটির তৈজস, ধাতুর নানান আকৃতির বস্তু এবং ফায়েন্স (গ্লাসের এক প্রকার) প্রাপ্তি ঘটেছে।

২. রসায়নের গুরুত্ব

কৃষি, খাদ্য, স্বাস্থ্যসেবা, শিল্প ও পরিবেশ সংরক্ষণে রসায়নের অবদান অপরিসীম।
পরিবেশের ক্ষতিকর উপাদান, যেমন সিএফসি, পরিবর্তে নিরাপদ উপাদান উদ্ভাবন করা হয়েছে।

৩. পদার্থের প্রকৃতি

পদার্থ স্থান দখল করে ও ভরযুক্ত। এটি কঠিন, তরল ও গ্যাসীয় অবস্থায় পাওয়া যায়।
মিশ্রণকে দুটি ভাগে ভাগ করা যায়: সমসত্ত্ব ও অসমসত্ত্ব।

৪. রাসায়নিক সংযোজনের নিয়ম

ভরের সংরক্ষণ আইন: রাসায়নিক বিক্রিয়ায় ভর ধ্রুবক থাকে।
নির্দিষ্ট অনুপাতের আইন: যৌগে প্রতিটি উপাদান নির্দিষ্ট ভর অনুপাতে থাকে।
গ্যাসীয় আয়তনের আইন: গ্যাসের আয়তনগুলো সরল পূর্ণসংখ্যার অনুপাতে যুক্ত হয়।

৫. পরমাণু ও অণুর ভর

পরমাণুর ভর: এটি কার্বন-১২ কে ভিত্তি ধরে নির্ধারিত।
অণুর ভর: অণুর মধ্যে থাকা পরমাণুর ভর যোগফল।

৬. স্টয়কিওমেট্রি এবং গণনা

রাসায়নিক বিক্রিয়ার মাধ্যমে প্রতিক্রিয়ক ও উৎপন্ন পদার্থের পরিমাণ নির্ণয়।
সীমাবদ্ধ বিকারক: যে উপাদানটি প্রথম শেষ হয়, তা বিক্রিয়াকে সীমাবদ্ধ করে।

৭. গণনাগুলি

গণনা পদ্ধতি: গাণিতিক প্রক্রিয়ার মাধ্যমে রাসায়নিক উপাদানগুলির গুণগত ও পরিমাণগত বিশ্লেষণ।

যদি কোনো নির্দিষ্ট বিষয় নিয়ে বিস্তারিত জানতে চান, আমাকে জানান।

MCQs for NEET, JEE, IIT, NIT, CUET, CTET, and SSC Entrance Exams: Your Ultimate Preparation Guide

Why MCQs Are Essential for Competitive Exams?

Concept Clarity: MCQs cover important topics, ensuring a deep understanding of fundamental concepts.
Time Management: Practicing MCQs improves speed and accuracy, essential for high-stakes exams.
Exam Pattern Familiarity: MCQs simulate the real exam pattern, helping you feel confident on the big day.

Benefits of Using These MCQs for NEET, JEE, IIT, and More

Targeted Preparation: Specially curated MCQs focus on the specific syllabus of exams like NEET, JEE, and CUET, making your study focused and efficient.
Wide Subject Coverage: Includes questions from Physics, Chemistry, Mathematics, Biology, and more.
Boosts Competitive Edge: High-quality MCQs ensure you're ready to tackle even the trickiest questions.

Exams These MCQs Help With:

NEET: For aspiring medical students.
JEE & IIT: For engineering and technical aspirants.
NIT Admissions: A stepping stone to prestigious National Institutes of Technology.
CUET: Common University Entrance Test for undergraduate programs.
CTET: A mandatory test for teachers.
SSC: Government job aspirants preparing for SSC exams.

Pro Tips to Use MCQs Effectively:

Regular Practice: Dedicate time daily to solve topic-wise MCQs.
Review and Revise: Go through solutions and explanations to understand your mistakes.
Mock Tests: Attempt full-length MCQ tests to build exam stamina.

Get Started Now!

Tags:

MCQs for NEET, JEE MCQs, IIT preparation, CUET questions, CTET practice, SSC MCQs, competitive exam tips, entrance exam success.

Make your preparation smarter, not harder. Let these MCQs guide your way to success!

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Thursday, November 21, 2024

MCQ Chemistry Unit 3: Classification of Elements and Periodicity in Properties, HS 1st year

১. মৌলসমূহের শ্রেণীবিন্যাস ও পর্যায়বৃত্ত গুণাবলী

২. আধুনিক পর্যায় সারণি ও পর্যায়বৃত্ত আইন

৩. মৌলসমূহের ইলেকট্রনিক কনফিগারেশন এবং পর্যায় সারণি

৪. মৌলসমূহের ধাতব, অধাতব ও উপধাতব বৈশিষ্ট্য

৫. পর্যায়বৃত্ত প্রবণতাসমূহ

৬. রাসায়নিক বিক্রিয়া ও মৌলসমূহের বৈশিষ্ট্য

MCQ Chemistry Unit 2: Structure of Atom, HS 1st year (with Chapter Summery in Bengali)

1. What is the charge of an electron?

2. Who proposed the atomic theory that laid the foundation for understanding chemical behavior?

3. In the cathode ray experiment, which observation indicates that cathode rays are negatively charged?

4. What is the mass of a neutron relative to a proton?

5. What does the term "isotopes" refer to?

6. According to Rutherford’s nuclear model, where is the mass of the atom concentrated?

7. What is the energy of a photon whose frequency is 5×1014 Hz5 \times 10^{14} \, \text{Hz}5×1014Hz? (Planck’s constant h=6.626×10−34 J\cdotpsh = 6.626 \times 10^{-34} \, \text{J·s}h=6.626×10−34J\cdotps)

8. Which postulate is part of Bohr’s model of the hydrogen atom?

9. What did Millikan's oil drop experiment determine?

10. The smallest and lightest positive ion is called:

11. What is the value of the Rydberg constant (RHR_HRH​)?

12. What is the wavelength range of visible light?

13. Who discovered neutrons?

14. What does Planck's quantum theory state?

15. Which phenomenon demonstrates the dual nature of light?

16. In the hydrogen spectrum, the series of lines in the visible region is called:

17. According to Bohr’s model, what happens when an electron jumps from a higher energy orbit to a lower one?

18. What is the angular momentum of an electron in the nnn-th orbit as per Bohr’s theory?

19. Which particle has a relative charge of +1?

20. The dual behavior of matter was proposed by:

21. What is the speed of electromagnetic radiation in a vacuum?

22. Which of the following series belongs to the ultraviolet region of the hydrogen spectrum?

23. What did Rutherford’s alpha-particle scattering experiment conclude?

24. What type of wave is light?

25. Which quantum number determines the size of an orbital?

26. What is the energy of an electron in the first orbit of hydrogen?

27. Which principle explains the distribution of electrons in an atom?

28. Who developed the quantum mechanical model of the atom?

29. Which phenomenon could not be explained by classical physics?

30. What is the unit of frequency in the SI system?

31. Which rule is used to fill orbitals of the same energy before pairing electrons?

32. The wavelength (λ\lambdaλ) and frequency (ν\nuν) of light are related by the equation:

33. What does the Pauli exclusion principle state?

34. What is the maximum number of electrons in a shell with n=3n = 3n=3?

35. Which particle was discovered by J.J. Thomson?

36. The charge-to-mass ratio of the electron was determined by:

37. Which experiment showed that electrons have particle-like properties?

38. What happens when an electron is in its ground state?

39. What is the shape of an s-orbital?

40. What is the principle quantum number (nnn) for the second orbit of an atom?

41. In the hydrogen atom, which series lies in the infrared region?

42. Which fundamental particle has no charge?

43. What does the Heisenberg uncertainty principle state?

44. What does the Aufbau principle dictate?

45. What are the orbitals in the second energy level?

১. পরমাণুর গঠন

২. পরমাণু মডেল

৩. পরমাণু শক্তি স্তর

৪. ইলেকট্রোম্যাগনেটিক তত্ত্ব

৫. কোয়ান্টাম মেকানিক্যাল মডেল

৬. পরমাণুর ইলেকট্রনিক কনফিগারেশন

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MCQ Chemistry Unit 1: Some Basic Concepts of Chemistry, HS 1st year (with Chapter Summery in Bengali)

MCQs from "Some Basic Concepts of Chemistry"

১. রসায়নের বিকাশ

২. রসায়নের গুরুত্ব

৩. পদার্থের প্রকৃতি

৪. রাসায়নিক সংযোজনের নিয়ম

৫. পরমাণু ও অণুর ভর

৬. স্টয়কিওমেট্রি এবং গণনা

৭. গণনাগুলি

MCQs for NEET, JEE, IIT, NIT, CUET, CTET, and SSC Entrance Exams: Your Ultimate Preparation Guide

Why MCQs Are Essential for Competitive Exams?

Benefits of Using These MCQs for NEET, JEE, IIT, and More

7. What is the energy of a photon whose frequency is $5 \times 10^{14} \, \text{Hz}$ ? (Planck’s constant $h = 6.626 \times 10^{-34} \, \text{J·s}$ )

11. What is the value of the Rydberg constant ( $R_H$ )?

18. What is the angular momentum of an electron in the $n$ -th orbit as per Bohr’s theory?

32. The wavelength ( $\lambda$ ) and frequency ( $\nu$ ) of light are related by the equation:

34. What is the maximum number of electrons in a shell with $n = 3$ ?

40. What is the principle quantum number ( $n$ ) for the second orbit of an atom?