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Structure of Atom Class 11 MCQ

Structure of Atom MCQ

Structure of Atom Chemistry Question Answers
These are some of the random multiple question answers from Structure of Atom... 

1. Who discovered anode rays :

 Goldstein
 Rutherford
 J. Stanley
 J. J. Thomson


2. Neutron was discovered by :

 Rutherford
 Chadwick
 Austin
 Langmuir


3. Radioactive isotope of hydrogen has ________ number of neutrons :

 0
 1
 2
 3


4. Cathode rays are deflected by :

 A magnetic field only
 An electric field only
 By Both
 By None


5. Cathode rays have :

 Mass Only
 Charge Only
 Mass and Charge Both
 No Charge and No Mass


6. Mass of atom is mainly constituted by :

 Neutrons and neutrino
 Neutrons and electrons
 Neutrons and protons
 Protons and electrons


7. Ratio of mass of proton and electron is :

 1.8
 1.8x103
 Infinite
 None of these


8. Atomic number of an element is equal to the number of  :

 Proton
 Electron
 Neutron
 Electron and Proton


9. Size of nucleus is :

 10-8 m
 10-10 m
 10-12 m
10-15 m


10. Who modifies Bohr’s model :

 Dalton
 Pauli
 Rutherford
 Sommerfeld




Also read Chemistry Notes of this chapter at below link...
11 Class Chapter 2- Structure of Atom

Some Basic Concepts of Chemistry Class 11 MCQ

Some Basic Concepts of Chemistry Class 11 MCQ

some basic concepts of chemistry mcq

These are some of the random multiple question answers from Some Basic Concept of Chemistry...

1. If a matter has definite volume and definite shape, then it is :

Solid
Liquid
Gas
All of the Above


2. Mole is SI unit of :

Current
Temperature
Amount of Substance
Luminous intensity



3. A measured temperature is 100 0F on Fahrenheit scale, then what is this reading be on Celsius scale :

11.2 0C

78 0C

102.7 0C

37.8 0C



4. What amount of H­2O produced by combustion of 32 g of CH4 :

36 g
18 g
72 g
90 g


5. How many moles of CH4 is needed to get 44 gram CO2 after combustion :

0.5 mol of Methane
1 mol of Methane
2 mol of Methane
4 mol of Methane


6. Calculate the mass per cent of the solute, when a solution is prepared by adding 4 gram of substance A to 36 gram of water :

10%
20%
30%
40%


7. What is molarity of  NaOH in the Solution, that is prepared by adding 2 gram NaOH in water to get 500 mL of the solution :

0.4 M
1.0 M
0.1 M
4.0 M


8. A measured temperature is 44 0C on Celsius scale, then what is this reading be on Fahrenheit scale :

111.2 0F

88.8 0F

32 0F

199.8 0F



9. Dalton in 1803, gives :

Law of conservation of mass

Law of definite proportion

Law of multiple proportion

Gay Lussac’s law of gaseous volume



10. The prefix 10-15 is :

Atto
Femto
Peta
Tera




Also read Chemistry Notes of this chapter at below link...

11 Class Chapter 1- Some Basic Concept of Chemistry Notes


Science Quiz : Acids and Bases Chemistry MCQs Part 18

Science Quiz : Acids and Bases Chemistry MCQs


Science Quiz by www.ChemistryNotesInfo.com

These are some of the random multiple question answers from Acids and Bases Chemistry...

1. OH- ion is called as:

Hydronium Ion
Hydroxide Ion
Hydrate Ion
Hydrogen Ion


2. Taste of acidic food is:

Sweet
Salty
Sour
Bitter


3. H+ Ion (Hydrogen Ion) is simply a:

Proton
Neutron
Electron
Hydroxide Ion


4. Bases increases concentration of what in water:

H+ Ion
OH- Ion
Both
None


5. Which of the acid from given below choice of acids is more dangerous:

Citric Acid
Carbonic Acid
Hydrochloric Acid
None of the above


6. Which of the given below statement about Alkalis is true:

They cannot neutralise acids
They are all insoluble
They are all acids
They are all bases


7. What happens to litmus paper in basic solutions:

Red litmus paper turns blue
Blue litmus paper turns red
Pink litmus paper turns Black
Black litmus paper turns blue


8. A liquid has a pH of 6.5, so this liquid is:

Weakly acidic
Weakly alkaline
Strongly acidic
Neutral


9. A liquid has a pH of 14, so this liquid is:

Weakly acidic
Weakly alkaline
Strongly acidic
Strongly basic


10. If a solution have pH of 9, then its H+ concentration is:

1 x 10-9 moles/liter
1 x 10-18 moles/liter
1 x 109 moles/liter
1 x 1018 moles/liter



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Chemistry Formulas for Nuclear Chemistry (Radioactivity)

Chemistry Formulas for Nuclear Chemistry (Radioactivity)

Empirical relationship between size of nucleus and its mass number is
            R = R0A1/3
Where,                       
            R = radius of nucleus,
            A = mass number,
            R0 = contestant = 1.4x10-13cm

Rate of Decayof radioactive substance

Where,
            K = decay constant,
            N = No. of atoms,
            t = time of decay,
            dN = small fraction of N,
            dt = small fraction of t

Value of Decay Constant

            
Where,
            N0 = No. of atoms originally present,
            N = No. of atoms present after time t

Half Life Time (t1/2)

            t1/2 = 0.693/K
Where,
            K = decay constant

Average Life Time (T)

            Average life time (T) =Sum of the lives of the nuclei/ Total number of nuclei
            T = 1/K 
Also,
            Average life time (T) = 1.44 x Half-life (T1/2)
Where,
            K = decay constant
            T = Average Life Time
            T1/2 = Half Life

Specific Activity

            Specific Activity = Rate of decay/m
                                      = KN/m
                                      = K x Avogadro Number/ Atomic Mass in gram
Where,
            N = Number of Radioactive nuclei that undergoes disintegration

Units of Radioactivity

            Standard unit of radioactivity is curie (c).
            1c = Activity of 1gram Ra226 = 3.7 x 1010dps
Where,
            dps = disintegrations per second
millicurie (mc) = 3.7 x 107dps
microcurie (µc) = 3.7 x 104dps
Other units of radioactivity are Rutherford (rd) and Becquerel (Bq).

Rutherford (rd)

1rd = 106dps

Becquerel (Bq)

            Becquerel (Bq) is the SI unit of radioactivity.
                        1Bq = 1 disintegrations per second
                        1 Bq = 1 dps

Radioactive Equilibrium

            A ----à B ----à C
            At steady state,
                        NA/NB = KB/KA = TA/TB
Where,
            KA = radioactivity constant for the process A---àB
            KB = radioactivity constant for the process B---àC
            TA = average life period of A
            TB = average life period of B
Radioactive Equilibrium in terms of half-life periods,
            NA/NB = (T1/2)A/ (T1/2)B

Famous Scientists and their Inventions

Scientists and Their Important Research in the Field of Chemistry

chemist, chemistry, chemistry experiments, chemistry scientists, famous chemists, famous scientists, great scientists, list of scientists, names of scientists, scientific name, scientist names,
Given below is the list of scientists and their important research and inventions. These famous scientists or chemists perform many science and chemistry experiments which help in the development of Chemistry and Science. 

 List of Famous Scientists and their Inventions

List of Scientists
Research and Inventions
Ernest Rutherford
Bombardment of Atoms by alpha-particles
J. J. Thompson
Discovery of Electron, e/m of Electron
Eugen Goldstein
Discovery of Proton
James Chadwick
Discovery of Neutron
Louis De-Broglie
Wave Equation
Niels Henrik David Bohr
Atomic Model, Long Form of Periodic Table
Albert Einstein
Photoelectric Effect
Niels Bohr, Wolfgang Pauli and Friedrich Hund
Distribution of electrons
Heisenberg Principle
Uncertainty Principle
Becquerel
Radioactivity
Marie Curie
Radium
Francis William Aston
Mass Spectrograph
Dmitri Ivanovich Mendeleev
Periodic Law, Periodic Table
Sidwick and Powell
Theory of Hybridisation
Louis Allred and Eugene George Rochow
Electronegativity
Robert Sanderson Mulliken
Electronegativity
Robert Boyle
Boyle’s Law, Relation Between P and V
Jacques Alexandre César Charles
Charle’s Law, Relation Between T and V
Lorenzo Romano Amedeo Carlo Avogadro
Avogadro’s Law, Relation Between V and number of molecules (n)
John Dalton
Dalton’s Law, Relation Between the Total Pressure and Partial Pressure of Individual Gases
Thomas Graham
Graham’s Law, Relation Between the Rate of Diffusion and Density (or Molecular Weight) of Gases
François Marie Raoult
Raoult’s Law, Relation Between Partial Vapour Pressure and Mole Fraction
Harold Clayton Urey
Heavy Water
Henry Louis Le Chatelier
Le Chatelier Principle, Effect of P, T and Concentration of Reactants on the System in Equilibrium


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