Chapter Fundamental concept of Chemistry
Q: How many significant figures are in the number 0.00450?
a) 2
b) 3
c) 4
d) 5
Answer: c) 4
Q: In the measurement 8.75 cm, how many significant figures are there?
a) 2
b) 3
c) 4
d) 5
Answer: b) 3
Q: If you round the number 6.725 to two decimal places, what is the result?
a) 6.73
b) 6.72
c) 6.7
d) 7
Answer: a) 6.73
Q: If a thermometer consistently reads temperatures 2 degrees higher than the actual temperature, what type of error is this?
a) Random error
b) Systematic error
c) Gross error
d) Absolute error
Answer: b) Systematic error
Q: In the formula Δx = xᵢ - x̄, what does Δx represent ?
a) Absolute error
b) Relative error
c) Deviation
d) Percentage error
Answer: c) Deviation
Q: What does the atomic mass of an element represent ?
a) The mass of one mole of atoms of the element
b) The mass of one atom of the element
c) The total mass of electrons in the element
d) The mass of one molecule of the element
Answer: a) The mass of one mole of atoms of the element
Q: The mass number of an atom is equal to the sum of its ?
a) Protons and electrons
b) Protons and neutrons
c) Electrons and neutrons
d) Valence electrons and protons
Answer: b) Protons and neutrons
Q: Which unit is used to express atomic mass ?
a) Atomic mass unit (amu)
b) Gram
c) Kilogram
d) Pound
Answer: a) Atomic mass unit (amu)
Q: If you have 1 mole of carbon atoms, what is the mass in grams ?
a) 12 g
b) 24 g
c) 6 g
d) 18 g
Answer: a) 12 g
Q: What is the total number of protons in the nucleus of an atom?
a) Mass number
b) Atomic number
c) Isotope number
d) Valence number
Answer: b) Atomic number
Q: What is the molecular mass of water (H₂O) ?
a) 16 amu
b) 18 amu
c) 20 amu
d) 22 amu
Answer: b) 18 amu
Q: What is the empirical formula of a compound ?
a) The simplest whole-number ratio of atoms in the compound
b) The total number of atoms in the compound
c) The molecular formula of the compound
d) The mass of one mole of the compound
Answer: a) The simplest whole-number ratio of atoms in the compound
Q: Which of the following is true about the molar mass of a substance ?
a) It is equal to the molecular mass for all substances
b) It is expressed in grams per mole (g/mol)
c) It is always a whole number
d) It is the mass of one mole of electrons
Answer: b) It is expressed in grams per mole (g/mol)
Q: What is Avogadro's number ?
a) 6.02 x 10^23
b) 3.14 x 10^6
c) 1.00 x 10^8
d) 2.18 x 10^12
Answer: a) 6.02 x 10^23
Q: Avogadro's number represents the number of ?
a) Atoms in one mole of a substance
b) Moles in one gram of a substance
c) Molecules in one liter of a gas
d) Ions in one formula unit of an ionic compound
Answer: a) Atoms in one mole of a substance
Q: In a chemical reaction, the mole ratio between reactants and products is determined by ?
a) The temperature
b) The concentration
c) The coefficients in the balanced chemical equation
d) The color of the reactants
Answer: c) The coefficients in the balanced chemical equation
Q: What is stoichiometry?
a) The study of atomic structure
b) The study of chemical bonding
c) The calculation of quantities in chemical reactions
d) The study of gas laws
Answer: c) The calculation of quantities in chemical reactions
Q: In the balanced chemical equation: 2H₂ + O₂ → 2H₂O, what is the mole ratio of hydrogen to oxygen ?
a) 1:1
b) 2:1
c) 1:2
d) 2:2
Answer:b) 2:1
Q : In the reaction 2H2+O2→2H2O, if you have 4 moles of hydrogen gas (H₂), how many moles of water (H₂O) can be produced ?
a) 2 moles
b) 4 moles
c) 8 moles
d) 16 moles
Answer: c) 8 moles
Q: In the reaction 2H2+O2→2H2O, if 5 liters of hydrogen gas (H₂) react, how many liters of water vapor (H₂O) will be produced at the same temperature and pressure?
a) 2.5 liters
b) 5 liters
c) 10 liters
d) 20 liters
Answer: c) 10 liters
Q: If 50 grams of sodium hydroxide (NaOH) are dissolved in water, how many liters of a 2 M (molar) NaOH solution are formed? (Assume the density of water is 1 g/mL) ?
a) 25 liters
b) 50 liters
c) 75 liters
d) 100 liters
Answer: a) 25 liters
NTS BSN Entry Test Preparation
Chapter : Three States of Matter
Q: In which state of matter do particles have the least energy and are closely packed together?
a. Solid
b. Liquid
c. Gas
d. Plasma
Answer: a. Solid
Q: Which of the following is a characteristic of liquids?
a. Definite shape and volume
b. Indefinite shape and definite volume
c. Indefinite shape and indefinite volume
d. Definite shape but indefinite volume
Answer: b. Indefinite shape and definite volume
Q: If you round the number 6.725 to two decimal places, what is the result?
a) 6.73
b) 6.72
c) 6.7
d) 7
Answer: a) 6.73
Q: What is the term for the process of a substance changing directly from a solid to a gas without passing through the liquid phase?
a. Sublimation
b. Condensation
c. Evaporation
d. Melting
Answer: a. Sublimation
Q: Which of the following is an example of a physical change in matter?
a. Burning wood
b. Rusting of iron
c. Melting ice
d. Digesting food
Answer:c. Melting ice
Q: Which of the following is a characteristic of gases?
a. Definite shape and volume
b. Indefinite shape and definite volume
c. Indefinite shape and indefinite volume
d. Definite shape but indefinite volume
Answer: c. Indefinite shape and indefinite volume
Q: The process of a gas changing into a liquid is known as ?
a. Sublimation
b. Vaporization
c. Condensation
d. Evaporation
Answer: c. Condensation
Q: At what temperature does water boil at standard atmospheric pressure?
a. 0°C
b. 100°C
c. -273°C
d. 373°C
Answer: b. 100°C
Q: At what temperature does absolute zero occur on the Celsius scale?
a. -273.15°C
b. 0°C
c. 100°C
d. 273.15°C
Answer: a. -273.15°C
Q: Which law states that the pressure of a gas is inversely proportional to its volume when the temperature is constant?
a. Boyle's Law
b. Charles's Law
c. Avogadro's Law
d. Gay-Lussac's Law
Answer: a. Boyle's Law
Q: Which law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of individual gases?
a. Boyle's Law
b. Charles's Law
c. Dalton's Law
d. Avogadro's Law
Answer: c. Dalton's Law
Q: In the kinetic theory of gases, what is the relationship between the temperature and the average kinetic energy of gas molecules?
a. Directly proportional
b. Inversely proportional
c. No relationship
d. Quadratically proportional
Answer: a. Directly proportional
Q: The ideal gas law is expressed as ?
a. PV = nRT
b. PV = k
c. P = V/nRT
d. P = nRT
Answer: a. PV = nRT
Q: Which law states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass?
a. Boyle's Law
b. Graham's Law
c. Charles's Law
d. Avogadro's Law
Answer: b. Graham's Law
Q: According to Charles's Law, if the volume of a gas is kept constant, what happens to the pressure if the temperature increases?
a. Increases
b. Decreases
c. Remains the same
d. Depends on the gas
Answer: a. Increases
Q: The Van der Waals equation corrects the ideal gas law by considering ?
a. Volume of gas particles
b. The pressure of gas particles
c. Attraction between gas particles d. Temperature of gas particles
Answer: b) It is expressed in grams per mole (g/mol)
Q: What is surface tension?
a. The resistance of a liquid to flow
b. The tendency of a liquid to vaporize
c. The force that acts to minimize the surface area of a liquid
d. The ability of a liquid to conduct electricity
Answer: c. The force that acts to minimize the surface area of a liquid
Q: What is effusion?
a. The process of a gas escaping through a small hole into a vacuum
b. The process of a liquid turning into a gas
c. The process of a gas condensing into a liquid
d. The process of a solid turning into a liq
Answer: a. The process of a gas escaping through a small hole into a vacuum
Q: In a chemical reaction, the mole ratio between reactants and products is determined by ?
a) The temperature
b) The concentration
c) The coefficients in the balanced chemical equation
d) The color of the reactants
Answer: c) The coefficients in the balanced chemical equation
Q: What is the critical temperature of a substance?
a. The temperature at which it freezes
b. The temperature at which it boils
c. The highest temperature at which it can exist as a liquid
d. The lowest temperature at which it can exist as a gas
Answer: c. The highest temperature at which it can exist as a liquid
Q: According to Avogadro's Law, at constant temperature and pressure, equal volumes of different gases contain an equal number of?
a. Atoms
b. Molecules
c. Ions
d.Electrons
Answer: b. Molecules
Q : What is the SI unit for viscosity ?
a. Pascal-second (Pa·s)
b. Newton-meter (N·m)
c. Joule-second (J·s)
d. Watt-per-meter squared (W/(m²)
Answer: a. Pascal-second (Pa·s)
Q: What is viscosity?
a. The tendency of a liquid to vaporize
b. The resistance of a liquid to flow
c. The ability of a liquid to conduct electricity
d. The temperature at which a liquid turns into a gas
Answer: b. The resistance of a liquid to flow
Q: Which factor is most likely to increase the viscosity of a liquid?
a. Higher temperature
b. Smaller molecular size
c. Stronger intermolecular forces
d. Lower density
Answer: c. Stronger intermolecular forces
Chapter Chemical Bonding
Q: What is the term for the relative
attraction of the nucleus for the electrons in a chemical bond?
A. Electron Affinity
B. Ionization Energy
C. Electronegativity
D. Atomic Radius
Answer: C. Electronegativity
Q: What is the main factor
responsible for the paramagnetic behavior of a substance?
A. Type of Bonds
B. Presence of Unpaired Electrons
C. Molecular Shape
D. Electronegativity
Answer: B. Presence of Unpaired Electrons
Q: What is the molecular geometry of
a simple molecule with sp3 hybrid orbitals?
A. Linear
B. Trigonal Planar
C. Tetrahedral
D. Octahedral
Answer: C. Tetrahedral
Q: In the molecule CH4, what is the
hybridization of the carbon atom?
A. sp
B. sp2
C sp3
D. sp3d
Answer: C sp3
Q: What type of orbital overlap is
involved in the formation of bonds in methane (CH₄)?
A. s-s overlap
B. p-p overlap
C. s-p overlap
D. d-d overlap
Answer: C. s-p overlap
Q: What is the unit of dipole moment?
A. Paschal
B. Joule
C. Tesla
D. Debye
Answer: D. Debye
Q: In Nitrogen molecule, the very first bond is generally formed by ?
A. s - s overlap
B. s - p overlap
C. p - p head-on overlap
D. p - p parallel overlap
Answer: C. p - p head-on overlap
Q: How does ionization energy change
across a period ?
A. It decreases from left to right.
B. It increases from right to left.
C. There is no specific trend.
D. It remains constant.
Answer: B. It increases from right to left.
A. Linear
B. Trigonal Planar
C. Tetrahedral
D. Trigonal Bipyramidal
Answer: D. Trigonal Bipyramidal
Q: The product of charge and distance is called ?
A. Ionization Energy
B. Bond Length
C. Coulombic Potential
D. Dipole Moment
Answer: D. Dipole Moment
Q: Which hybridization state is
associated with a molecule having a pyramidal geometry?
A. sp
B. sp2
C. sp3
D. dsp3
Answer: C.sp3
Q: Which of the following molecules
has no dipole moment?
A. H2O
B. CO2
C. H-Br
D. None
Answer: B. CO2
Q: In a molecule with a triple bond between two carbon atoms, what is the likely hybridization of each carbon atom?
A. sp
B. sp2
C. sp3
D. dsp3
Answer: A. sp
Q : Which of the following pairs is an example of an ionic bond?
A. HCl
B. KCL
C. C2H4
D. O2
Answer: B. KCL
Q: In which molecule is p-p orbital
overlapping present, leading to the formation of pi (π) bonds?
A. H₂
B. O₂
C. Cl₂
D. NH₃
Answer: C. Cl₂
A. Lithium (Li)
B. Neon (Ne)
C. Chlorine (Cl)
D. Aluminum (Al)
Answer: C. Chlorine (Cl)
Q: Which compound is characterized by
a polar covalent bond among the following options?
A. HF
B. CH4
C. H2
D. N2
Answer: A. HF
Q: What is another name for a
coordinative covalent bond?
A. Polar bond
B. Dative bond
C. Ionic bond
D. Metallic bond
Answer: B. Dative bond
A. Copper
B. Ice
C. Diamond
D. Graphite
Answer: A. Copper
Q: What is the molecular geometry of
ammonia (NH₃) ?
A. Linear
B. Trigonal Planar
C. Tetrahedral
D. Trigonal Pyramidal
Answer: D. Trigonal Pyramidal
Chapter Periodic Classification
Q: In 1913, Henry Moseley Found that the fundamental property of elements is ?
A. Atomic Mass
B. Electron Configuration
C. Atomic Size
D. Atomic Number
Answer: D. Atomic Number
Q: The element with the highest electronegativity is ?
A. Fluorine
B. Oxygen
C. Hydrogen
D. Nitrogen
Answer: A. Fluorine
Q: What is the outermost electron configuration of the most electronegative elements (halogens) in the periodic table?
A. ns²np²
B. ns²np³
C. ns²np⁴
D. ns²np⁵
Answer: D. ns²np⁵
Q: The concept of Triads was proposed by?
A. Dmitri Mendeleev
B. John Dalton
C. Dobereiner
D. J.J. Thomson
Answer: C. Dobereine.
Q: What is the common oxidation state of alkali metals in their compounds?
A. +1
B. -1
C. 0
D. +2
Answer: A. +1
Q: Atoms of the same element, with the same atomic number but different mass number, are called ?
A. Isomers
B. Isotopes
C. Isobars
D. Isotones
Answer: B. Isotopes
Q:Which one of the following is not an alkali metal?
A. Francium
B. Caesium
C. Rubidium
D. Radium
Answer: D. Radium
Q: How many valence electrons do elements in Group II A of the periodic table have?
A. 1
B. 2
C. 6
D. 8
Answer: B. 2
Q: Among the following groups in the periodic table, which one contains elements with the largest atomic radii?
A. Group I A
B. Group II A
C. Group VII A
D. None
Answer: A. Group I A
Q: Which noble gas does not follow the octet rule?
A. Helium (He)
B. Neon (Ne)
C. Argon (Ar)
D. Krypton (Kr)
Answer: A. Helium (He)
Q: Elements in the same group of the periodic table have similar properties because they have the same number of?
A. Protons
B. Neutrons
C. Valence Electrons
D. Isotopes
Answer: C. Valence Electrons
Q: Which of the following elements is a metalloid?
A. Silicon (Si)
B. Chlorine (Cl)
C. Sodium (Na)
D. Iron (Fe)
Answer: A. Silicon (Si)
Q: Which of the following elements has the least density?
A. Na (Sodium)
B. Li (Lithium)
C. Mg (Magnesium)
D. K (Potassium)
Answer: B. Li (Lithium)
Q: In the long form of the periodic table, all nonmetals are placed under which block?
A. s-block
B. p-block
C. d-block
D. f-block
Answer: B. p-block
Q: Which subshell is filled after 4s in the electronic configuration of elements?
A. 3p
B. 4p
C. 3d
D. 5s
Answer: C. 3d
Q: The addition of a second electron to a uninegative ion is ?
A. Exothermic
B. Endothermic
C. Isothermic
D. No change in energy
Answer: B. Endothermic
Q: When deuterium reacts with oxygen, what is the formed?
A. Heavy hydrogen
B. Water ( H2O)
C. Heavy water ( D2O)
D. Hydrogen peroxide ( H2O2)
Answer: C. Heavy water ( D2O)
Q: Diagonal relationship exists between which pair of elements?
A. Magnesium (Mg) and Potassium (K)
B. Lithium (Li) and Magnesium (Mg)
C. Chlorine (Cl) and Bromine (Br)
D. Carbon (C) and Silicon (Si)
Answer:B. Lithium (Li) and Magnesium (Mg)
Q: The "zero group" in the periodic table is also known as?
A. Halogens
B. Alkaline Earth Metals
C. Inert Gases
D. Transition Metals
Answer: C. Inert Gases
Chapter Solution and Electroytes
Q: If 5.85 grams of sodium chloride (NaCl) with a molecular weight of 58.5 g/mol is dissolved in water and the solution is made up to 0.5 liters, what is the molarity of the solution?
A. 0.1 M
B. 0.2 M
C. 0.5 M
D. 1.0 M
Answer: B. 0.2 M
Q:What is the term for the number of moles in 1 kg of solvent in a solution?
A. Molarity
B. Molality
C. Mass fraction
D. Volume percent
Answer: B. Molality
Q: If 60 grams of acetic acid is dissolved in one liter of water, what is the normality of the solution?
A. 0.5 N
B. 0.75 N
C. 1 N
D. 1.25 N
Answer: C. 1 N
Q: What is the nature of the solution formed when Na2SO4 is dissolved in water?
A. Acidic
B. Basic
C. Neutral
D. Amphoteric
Answer: C. Neutral
Q: If an acid is added to an aqueous solution, what will happen to the pH of the solution?
A. Increase
B. Decrease
C. Remain unchanged
D. Become neutral
Answer: B. Decrease
Q: What is a homogeneous mixture of two or more substances called?
A. Compound
B. Heterogeneous mixture
C. Solution
D. Suspension
Answer: C. Solution
Q:What is the weight of glucose in a 1 molar solution in water?
A. 18.01 grams
B. 90.08 grams
C. 180.16 grams
D. 360.32 grams
Answer: C. 180.16 grams
Q: Solution with the maximum concentration of solute at a given temperatureis known as?
A. Concentrated
B. Dilute
C. Saturated solution
D. All of the above
Answer: C. Saturated solution
Q: What is the concentration of alcohol in a solution where 10 ml of alcohol is dissolved in 90 ml of water?
A. 5%v/v
B. 10%v/v
C. 15%v/v
D. 20%v/v
Answer: B. 10%v/v
Q: The relative lowering of vapor pressure is?
A. Equal to the mole fraction of solvent
B. Equal to the vapor pressure of the solute
C. independent of the mole fraction of solute
D. Directly proportional to the mole fraction of solute
Answer: D. Directly proportional to the mole fraction of solute
Q: What is the nature of a solution with a pH of 4?
A. Neutral
B. Acidic
C. Basic
D. Alkaline
Answer: B. Acidic
Q: What is the term for a solution that distills over with a change in composition?
A. Isotonic solution
B. Azeotropic solution
C. Homogeneous solution
D. Heterogeneous solution
Answer: B. Azeotropic solution
Q: Which of the following are the conditions of colligative properties?
A. Non-electrolyte solute
B. Non-volatile solute
C. Dilute solution
D. All of the above
Answer: D. All of the above
Q: What is the result of adding a proton to a base in an acid-base reaction?
A. Formation of a conjugate base
B. Formation of a conjugate acid
C. Formation of a neutral molecule
D. No change in the base
Answer: B. Formation of a conjugate acid
Q: To prepare 1 liter of a 0.5 M HCl solution, what volume of a 4M HCl solution is needed?
A. 0.25 L
B. 0.5 L
C. 0.125 L
D. 1.5 L
Answer: C. 0.125 L
Q: What does normality (N) represent?
A. The number of moles of solute per liter of solution
B. The concentration of a solution in grams per liter
C. The number of equivalent weights of solute per liter of solution
D. The ratio of solute particles to solvent particles
Answer: C. The number of equivalent weights of solute per liter of solution
Q: Which of the following compounds is a strong base?
A. NH4
B. KOH
C.HCL
D.NH 4 OH
Answer: B. KOH
Q: What is the term for the concentration of solute molecules when they are in equilibrium with a solid substance at a particular temperature?
A. Saturation point
B. Dissociation concentration
C. Solubility
D. Equilibrium concentration
Answer: C. Solubility
Q: Which of the following salts will not undergo hydrolysis?
A. KCl (Potassium Chloride)
B. NH₄Cl (Ammonium Chloride)
C. AlCl₃ (Aluminum Chloride)
D. None of the above
Answer: A. KCl (Potassium Chloride)
Chapter S - Block Elements
Q: Which elements are found in the
S-block of the periodic table?
A. Noble Gases
B. Alkali Metals and Alkaline Earth Metals
C. Halogens
D. Transition Metals
Answer: B. Alkali Metals and Alkaline Earth Metals
Q: How can ammonia be prepared by
heating ammonium chloride?
A. With sulfuric acid
B. With hydrochloric acid
C. With sodium hydroxide
D. With nitric acid
Answer: C. With sodium hydroxide
Q: What is the primary product prepared using a Downs cell?
A. Sodium carbonate
B. Sodium metal
C. Sodium bicarbonate
D. Sodium hydroxide
Answer: B. Sodium metal
Q: Why are the first ionization
energies of alkaline earth metals higher than those of alkali metals?
A. Alkaline earth metals have more electron shells.
B. There is an increase in the nuclear charge of the alkaline earth metals.
C. Alkaline earth metals have greater atomic radii.
D. Alkaline earth metals are less reactive.
Answer: B. There is an increase in the nuclear charge of the alkaline earth metals.
Q: Why is (NaOH) named "caustic
soda"?
A. It corrodes the organic tissues
B. It is used in soda water
C. It reacts with chlorine gas
D. It reacts with fats to form soap
Answer: A. It corrodes the organic tissues
Q:How is sodium carbonate (Na2CO3)
primarily prepared?
A. Castner process
B. Haber process
C. Solvay process
D. Downs process
Answer: C. Solvay process
A. Francium
B. Caesium
C. Rubidium
D. Radium
Answer: D. Radium
Q: What happens to the nuclear charge
in S-block elements as you move down the group?
A. It decreases
B. It remains constant
C. It increases
D. It fluctuates
Answer: C. It increases
Q: Which one of the following is
least ionic in nature and decomposes on heating?
A. LiOH
B. NaOH
C. KOH
D. CsOH
Answer: A. LiOH
A. Cu (Copper)
B. Cs (Cesium)
C. Ba (Barium)
D. Cr (Chromium)
Answer: B. Cs (Cesium)
Q: Which one of the following
substances conducts electricity by the movement of ions?
A. Graphite
B. Copper
C. Molten sodium chloride
D. Mercury
Answer: C. Molten sodium chloride
Q: What is the product formed when
slaked lime reacts with chlorine?
A. Gypsum
B. Bleaching Powder
C. Brine
D. Soda Ash
Answer: B. Bleaching Powder
A. NaCl
B. KF
C. Csl
D. LiF
Answer: D. LiF
Q: During the electrolysis of brine
in Nelson's cell, what element is produced at the cathode?
A. Chlorine (Cl₂)
B. Hydrogen (H₂)
C. Sodium (Na)
D. Oxygen (O₂)
Answer: B. Hydrogen (H₂)
Q: What is the common name of sodium
hydrogen carbonate?
A. Bleaching Powder
B. Washing Soda
C. Baking Soda
D. Baking Powder
Answer: C. Baking Soda
A. Sodium sulfate
B. Potassium sulfate
C. Zinc sulfate
D. Barium sulfate
Answer: D. Barium sulfate
Q: What is sodium amalgam?
A. An alloy of sodium and mercury
B. An alloy of sodium and zinc
C. An alloy of sodium and aluminum
D. An alloy of sodium and copper
Answer: A. An alloy of sodium and mercury
Q: Which alkaline earth metal is
present in chlorophyll, essential for photosynthesis?
A. Calcium (Ca)
B. Magnesium (Mg)
C. Strontium (Sr)
D. Barium (Ba)
Answer: B. Magnesium (Mg)
A. Lithium (Li)
B. Sodium (Na)
C. Potassium (K)
D. Rubidium (Rb)
Answer: A. Lithium (Li)
Chapter Atomic Structure
Q: In Rutherford's gold foil experiment, what type of particles were bombarded at a thin gold foil?
A. Beta particles
B. Gamma particles
C. Alpha particles
D. Neutron particles
Answer: C. Alpha particles
Q: Who discovered the neutron?
A. Ernest Rutherford
B. James Clerk Maxwell
C. Niels Bohr
D. James Chadwick
Answer: D. James Chadwick
Q: In Planck's equation, what does ℎ represent?
A. Speed of light
B. Planck's constant
C. Avogadro's number
D. Boltzmann's constant
Answer: B. Planck's constant
Q: What is the maximum number of orbitals present in a subshell represented by an azimuthal quantum number (l) of 3?
A. 3
B. 6
C. 7
D. 9
Answer: C. 7
Q: Which of the following explains the shape of orbitals ?
A. Principal quantum number
B. Azimuthal quantum number
C. Magnetic quantum number
D. Spin quantum number
Answer: B. Azimuthal quantum number
Q:Question: What is the mass of an electron?
A. 1.67 x 10^-27 kg
B. 2.54 x 10^-33 kg
C. 9.109 x 10^-31 kg
D. 5.98 x 10^24 kg
Answer: C. 9.109 x 10^-31 kg
Q: The charge of the electron was mesaure by ?
A. J.J. Thomson
B. Niels Bohr
C. Millikan
D. Ernest Rutherford
Answer: C. Millikan
Q: Who was the first scientist to observe the phenomenon of radioactivity?
A. Marie Curie
B. Henri Becquerel
C. Ernest Rutherford
D. J.J. Thomson
Answer: B. Henri Becquerel
Q: The energy of an Electron can be predicted by ?
A. Magnetic qauntum number
B. Spin quantum number
C. Azimuthal quantum number
D. Quantum number
Answer: D. Quantum number
Q: What are atomic orbits having the same energy called ?
A. Conjugate orbits
B. Spherical orbits
C. Degenerate orbits
D. Orthogonal orbits
Answer: C. Degenerate orbits
Q: What is the shape of a p-orbital in an atom ?
A. Spherical
. Circular
C. Dumbbell-shaped
D. Elliptical
Answer: C. Dumbbell-shaped
Q: The wavelength of the electron was verified by?
A. J.J. Thomson
B. Niels Bohr
C. Davisson and Germer
D. Max Planck
Answer: C. Davisson and Germer
Q: When the 6d orbital is complete, the next entering electron goes into?
A. 6p
B. 7s
C. 5f
D. 7p
Answer: D. 7p
Q: What is the correct electronic configuration of nitrogen ?
A. 1s² 2s² 2p⁴
B. 1s² 2s¹ 2p⁶
C. 1s² 2s² 2p³
D. 1s² 2s² 2p⁶ 3s¹
Answer: C. 1s² 2s² 2p³
Q: What is the correct expression for Planck's equation ?
A. E=hλ
B. E=hν
C. E=hr
D. E=chf
Answer: B. E=hv
Q: Which element has the highest electronegativity ?
A. Oxygen
B. Fluorine
C. Chlorine
D. Nitrogen
Answer: B. Fluorine
Q: What is the phenomenon called when spectral lines split in the presence of a strong electric field ?
A. Bohr effect
B. Stark effect
C. Zeeman effect
D. Compton effect
Answer: B. Stark effect
Q : Energy of atomic orbitals in a particular shell is in order?
A. s<p<d<f
B. f<d<p<s
C. s<d<p<f
D. f<p<d<s
Answer: A. s<p<d<f
Q: What are neutrons moving with an energy of 1.2 MeV commonly referred to as ?
a) Thermal neutrons
b) Slow neutrons
c) Fast neutrons
d) Moderated neutrons
Answer: c) Fast neutrons
Q: An increase in atomic number is observed during ?
A. Alpha emission
B. Beta emission
C. Radioactivity
D. Both a & b
Answer: B. Beta emission
Q: An Angular momentum of an electron ?
A. n2h/2x
B. nk2/2r
C. nh/4π
D.nh/2π
Answer: D.nh/2π