Structure of Atom Class 11 MCQ

Structure of Atom MCQ

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

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

View below video on Some Basic Concept of Chemistry Quiz

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

11 Class Chapter 1- Some Basic Concept of Chemistry Notes

Chemistry Formulas for Chemical Bonding

Chemistry Formulas for Chemical Bonding

 

   1.       Necessary condition for an ionic solid to be dissolved in water

                                Hydration Energy > Lattice Energy

   2.       Order of melting and boiling points of certain compounds

NaF > NaCl > NaBr > NaI;    MgO > CaO > BaO

3.       No Bond is 100% Ionic

4.       Force of attraction between two oppositely charged ions in vacuum (air) as per Coulombs Law

F = q₁q₂/r²

5.       Order of the Lattice Energy of some compounds

·         LiX > NaX > KX > RbX > CsX    (where X = F, Cl, Br, I)

·         MgO > CaO > SrO > BaO

·         MgCO₃ > CaCO₃ > SrCO₃ > BaCO₃

·         BaSO₄ > SrSO₄ > CaSO₄ > MgSO₄  

·         Mg(OH)₂ > Ca(OH)₂ > Sr(OH)₂ > Ba(OH)₂

·         Bivalent Ions-Bivalent Ions > Univalent Ions-Bivalent Ions or Bivalent Ions-Univalent Ions > Univalent Ions- Univalent Ions

6.       Example of some compounds which contains more than one type of bond

·         NaOH, KOH, Na₂CO₃  (Ionic Bond, Covalent Bond)

·         CO, NH₃.BF₃, [Co(NH₃)₃Cl₃]  (Dative Bond, Covalent Bond)

·         NH₄Cl, CuSO₄, K₄[Fe(CN)₆], [Cu(NH₃)₄]SO₄  (Dative Bond, Ionic Bond, Covalent Bond)

·         CuSO₄.5H₂O  (Hydrogen Bond, Dative Bond, Ionic Bond, Covalent Bond)

7.       Double bond or triple bond is always shorter than corresponding single bond

8.       As S-Orbital is smaller than P-Orbital so bond length decrease with increase in S-character

SP³  C-H  =  1.093 Å (as in Alkanes)

SP²  C-H  =  1.087 Å (as in Alkenes)

SP  C-H  =  1.057 Å (as in Alkynes)

9.       Bond length increases if size of bonded atom is increases with given atom

HI > HBr > HCl > HF

10.   Bond distance is directly proportional to Atomic size

11.   Order of bond strength (or bond energy) of different hydrogen halides

H-F > H-Cl > H-Br > H-I

12.   Bond energy is directly proportional to bond order

Triple Bond > Double Bond > Single Bond

13.   Formula of Dipole Moment

Dipole moment (µ) = Electronic Charge (e) x Distance (d)

14.   Unit of Dipole Moment

Debye (D)

1D = 1 x 10^-18e.s.u. cm

SI unit of Dipole Moment is = Coulomb-Meter (C-m)

1D = 3.336 x 10^-30 C-m

15.   Dipole Moment of some substances

Substance with Formula	Dipole Moment (D)
HF	1.91
H2O	1.84
SO2	1.60
NH3	1.46
NF3	0.24
CH3Cl	1.86
HCl	1.03
H2S	1.10
HBr	0.78
HI	0.38

16.   Formula to calculate percentage ionic character of covalent bond

% Ionic Character = (Observed dipole moment x 100)/Dipole moment for 100% ionic bond

17.   Order of polarizing power of cations

Li⁺ > Na⁺ > K⁺ > Rb⁺ > Cs⁺

Be²⁺ > Mg²⁺ > Ca²⁺ > Sr²⁺ > Ba²⁺

Al³⁺ > Mg²⁺ > Na⁺

18.   Order of polarizing power of anions

N^3- > O^2- > F^-

P^3- > S^2- > Cl^-

19.   Chemistry Formula of Bond Order

Bond Order = [N_b-N_a]/2

Where,

                N_a = Number of electrons in antibonding molecular orbitals

                N_b = Number of electrons in bonding molecular orbitals

20.   Some molecules with their bond order, bond length and bond dissociation energy

Molecule	Bond Order	Bond Length (pm)	Bond Dissociation Energy (kJ/mol)
F2	1	142	158
O2	2	121	498
N2	3	110	945

21.   Bond Order in compounds which exhibits Resonance

Bond Order = (Total No. of bonds between two atoms)/(Total No. of resonating structures)

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

What are the factors which favor formation of ionic bonds?

What are the factors which favour formation of Ionic Bonds?

These are the factors which favours formation of ionic bonds...

1. One of the atoms i.e. Metal atom must have low ionization energy, so that it can easily lose its electrons.

2. Other atoms i.e. Non-Metal atoms must have high electron affinity, so that it can hold the extra electrons.

3. One of the atoms i.e. Metal atom should be large in size.

4. Other atoms i.e. Non-Metal atoms should be small in size.

5. Lattice energy of the crystal should be high, means the electrostatic attraction between charged ions in the crystal should be high.

6. Anion and cation should have inert gas electronic configuration. 

7. The combining elements should differ by at least 1.9 in electronegativity.

Chemistry Formulas for Nuclear Chemistry (Radioactivity)

Chemistry Formulas for Nuclear Chemistry (Radioactivity)

Empirical relationship between size of nucleus and its mass number is

            R = R₀A^1/3

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 (t_1/2)

            t_1/2 = 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 (T_1/2)

Where,

            K = decay constant

            T = Average Life Time

            T_1/2 = 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,

                        N_A/N_B = K_B/K_A = T_A/T_B

Where,

            K_A = radioactivity constant for the process A---àB

            K_B = radioactivity constant for the process B---àC

            T_A = average life period of A

            T_B = average life period of B

Radioactive Equilibrium in terms of half-life periods,

            N_A/N_B = (T_1/2)A/ (T_1/2)B