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CBSE Questions for Class 11 Medical Chemistry Structure Of Atom Quiz 3 - MCQExams.com
CBSE
Class 11 Medical Chemistry
Structure Of Atom
Quiz 3
What is the nucleon number of an atom?
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The number of neutrons
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The number of protons
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The total number of protons and neutrons
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The total number of protons and electrons
Explanation
Solution:- (C) The total number of protons and neutrons
The nucleon number or mass number of an atom, is the total number of protons and neutrons in an atomic nucleus.
The number of neutrons in the dispositive zinc ion is: (mass number of Zn=65)
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35
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33
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65
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67
How many electrons can fit in the orbital for which:
$$n=3$$ and $$l=1$$?
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10
0%
14
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2
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6
The electronic configuration of an element is $$1s^{2} 2s^{2} 2p^{3}$$. The number of unpaired electron in this atom are
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$$3$$
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$$5$$
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$$7$$
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$$1$$
Which of the following is the correct electronic configuration of scandium (atomic number = $$21$$) ?
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$$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{3} $$
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$$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{1} 4s^{2} $$
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$$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{2} 4s^{1} $$
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$$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 4p^{1} $$
Charge of one mole of alpha particle is:
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+ 2 units
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+ 1 units
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+ 2 faraday
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+ 2 coulombs
Explanation
Hint:
An alpha particle is a helium atom with $$(+2)$$ charge in it.
Formula:
$$1 $$ Coulomb $$=\frac{1}{96500}$$ Faraday
Step 1: To find the charge on a one-mole alpha pacticle.
We know that,
One mole of alpha particles has $$2$$ moles of protons.
We already know that charge of one proton $$=1.6 \times 10^{-19} C$$.
Therefore,
Charge in one mole of protons $$=1.6 \times 10^{-19} C \times 6.02 \times 10^{23}=96500 C$$
Therefore,
Charge on two moles of protons will be given as $$=(2 \times$$ charge on one mole of the proton)
$$=2 \times 96500$$
$$=193000 C$$
As,
$$1 $$ Coulomb $$=\frac{1}{96500}$$ Faraday
Therefore,
$$193000 \mathrm{C}=\frac{193000}{96500}=2$$ faraday
Final answer:
Hence, option $$C$$ is the correct option.
Which of the following is/are true as per Thomson's model of atom?
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An atom is not electrically neutral.
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An atom is a positively charged sphere with electrons embedded in it.
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Negative and positive charges in the atom are equal in magnitude.
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None of the above
Explanation
Thomson's model of atom states that:
1. An atom consists of a positively charged sphere with electrons embedded in it.
2. Total positive and negative charges in the atom are equal in magnitude. So, atom is electrically neutral.
If Aufbau rule is violated, then $$Ca^{20} $$ will be in:
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s-block
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p-block
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d-block
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f-block
Explanation
According to the Aufbau principle, electron enters into the lowest energy level (orbital), before entering into a higher energy level. Hence, according to this principle, the electronic configuration of $$Ca^{20}$$ is $$1s^22s^22p^63s^23p^64s^2$$, as differentiating electron enters into the s-orbital, $$Ca$$ belongs to s-block.
If we don't follow the Aufbau rule, the electronic configuration of $$Ca^{20}$$ would be $$1s^22s^22p^63s^23p^63d^2$$.
Here, the differentiating electron is entering in the d orbital, so it would belong to the d-block element.
To which of the following is Bohr's theory applicable:
I) $$He^{+}$$
II) $$Li^{2+}$$
III) Tritium
IV) $$Be^{2+}$$
The correct combination is:
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III, IV
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I, II, III, IV
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I, II
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I, II, III
Explanation
Bohr's atomic model explains the spectra of single-electron atoms like $$H$$-atom. It does not explain the spectra of multi-electron atoms.
So the atoms which are isoelectronic and have the same electronic configuration are well explained by this atomic model.
$$He^+$$, $$Li^{2+}$$ and tritium $$_{ 1 }{ H }^{ 3 }$$ have same number of electrons as that of hydrogen atom i.e. $$1$$ while $$Be^{2+}$$ is formed by losing $$2e$$. So, it is a two-electron system.
Option D is correct.
Which of the following properties are similar for isotopes?
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Physical properties
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Chemical properties
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Both physical and chemical properties
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Neither physical nor chemical properties
The atomic number at which filling of a g-orbital is likely to begin is:
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$$121$$
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$$116$$
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$$106$$
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$$124$$
Explanation
The above question can be answered on the basis of reasoning from analogy. We note that two periods have to pass before d-orbitals begin to fill. This is also true of the spot where f-orbitals commence filling. The second row where f-orbitals fill happens to be row #7 (the one starting with Fr). The first element where 5f-orbitals enter in is actinium (Ac, Z = 89). Adding 32 to this would give element #121 termed as Unbiunium, the first Super-Actinide.
The ratio of $$\dfrac{e}{m}$$ of proton and $$\alpha$$ - particle is:
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$$ 2:1 $$
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$$ 1:2$$
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$$ 1:1 $$
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$$ 1:3$$
Explanation
Alpha particle is $$He^{2+}$$ where as proton is $$H^+$$ and mass of alpha is $$4$$ times the mass of proton.
Thus, $$\dfrac{e}{m_{proton}}= \dfrac{1}{m}$$ and $$\dfrac{e}{m_{\alpha}}= \dfrac{2}{4m}$$.
Therefore, the ratio is $$2:1$$
The best evidence that electrons are arranged in definite orbits or energy levels is based on the observation that:
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atomic spectra consist of discrete lines and not continuous bands
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electrons in the beta ray have high kinetic energy
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the penetrating power of cathode ray electrons depends upon the voltage used to produce them
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electrons revolve around the nucleus
Explanation
The best evidence that electrons are arranged in definite orbits or energy levels is based on the observation that the spectral lines of hydrogen atom consist of discrete lines and not continuous bands.
The band spectrum is caused by:
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molecules
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atoms
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any substance in solid state
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any substance in liquid state
Explanation
Hint: Band spectrum arises because of electron transition between the valence band and conduction band.
Explanation:
The band spectrum is caused by molecules. The energy levels of molecules are so close to each other that they combine to form a band. The valence band and conduction band are two types of bands. Electron transition between these two bands forms band spectrum.
For example a spectrum of air. The bright bands are due to molecular oxygen (O$$_2$$), molecular nitrogen (N$$_2$$), and other molecules.
So from the above example, it is clear that Option A is the answer.
The number of neutrons present in the deuterium
isotope of hydrogen is:
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2
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3
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5
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1
Explanation
The mass number of deuterium is 2. Therefore. deuterium nuclide will have 1 neutron as its atomic number is equal to one.
In the lowest energy level of hydrogen atom, electron has an angular momentum equal to:
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$$\dfrac{\pi }{h}$$
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$$\dfrac{h}{\pi }$$
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$$\dfrac{h}{2\pi }$$
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$$\dfrac{2\pi }{h}$$
Explanation
The angular momentum$$ L$$ $$=m_{e}vr$$ is on integer multiple of $$\dfrac{h}{2\pi }$$
$$mvr=\dfrac{nh}{2\pi}$$
For, $$n=1$$
$$mvr=\dfrac{h}{2\pi}$$
In the phenomenon of electric discharge through
gases at low pressure, the coloured glow in the
tube appears as a result of:
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collisions between the charged particles emitted from the cathode and the atoms of the gas
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collision between different electrons of the atoms of the gas
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excitation of electrons in the atoms
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collision between the atoms of the gas
Explanation
Collisions between charged particles emitted from cathode and atoms of gas.
The discharge of electricity through liquefied gases is an interesting phenomenon which can be systematically studied with the help of a discharge tube.In discharge tube collision between charged particles emitted from cathode and atoms of the gas results to colorless glow in tube.
The energy of a hydrogen atom in the ground state is 13.6 eV. The energy of He+ ion in the first excited state will be
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-13.6 eV
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-27.2 eV
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-54.4 eV
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-6.8 eV
Explanation
The total number of neutrons in all isotopes of hydrogen is equal to:
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6
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2
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4
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3
Explanation
Hydrogen has 3 isotopes.
$$_{1}^{1}\textrm{H} $$
$$_{1}^{2}\textrm{H}$$
$$_{1}^{3}\textrm{H}$$
neutron 0
1
2
proton 1
1
1
The total number of neutrons in all the isotopes of Hydrogen $$=0+1+2=3$$.
The life span of atomic hydrogen is :
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fraction of one sec.
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one year
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one hour
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one day
Explanation
The life span of hydrogen is approximately 0.3 sec.
Hence option A.
A sample of rock from moon contains equal number of atoms of uranium and lead $$(\mathrm{t}_{\frac{1}{2}}$$ for $$\mathrm{U}=4.5\times 10^{9}$$ years $$)$$. The age of the rock would be
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$$4.5\times 10^{9}$$ years
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$$9\times 10^{9}$$ years
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$$13.5\times 10^{9}$$ years
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$$2.25\times 10^{9}$$ years
Explanation
$$ t_{1/2}=\frac{0.693}{k} $$
$$ \therefore k=\frac{0.693}{45x10^{g}}years^{-1} $$
It is an uranium dating technique,
$$ \therefore Age=\frac{2.303}{K}log_{10}[1+\frac{Pb^{206}}{U^{238}}] $$
$$ =\frac{2.303}{0.693}x45x10^{g}log_{10}[1+1] $$
$$ =\frac{2.303x45x10^{g}}{0.693}log_{10}(2) $$
Age = 4 x 10$$ ^{g} $$ years
Which of the following are isotone of $$_{ 32 }^{ 76 }{ Ge }$$?
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$$_{ 32 }^{ 77 }{ Ge }$$
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$$_{ 33 }^{ 77 }{ As}$$
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$$_{ 34 }^{ 77 }{ Se }$$
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$$_{ 34 }^{ 78 }{ Se }$$
Explanation
Isotones are the elements having the same number of neutrons.
$$\text{Mass number = number of protons + number of neutrons.}$$
$$\text{Atomic number = number of protons = number of electrons.}$$
$$\text{Number of neutrons} = \text{mass number - number of protons} = \text{mass number - atomic number.}$$
Number of neutrons will be the same in $$_{ 33 }^{ 77 }{As } \: (77-33 =44)$$ and $$_{ 34 }^{ 78 }{Se }\: (78-34 = 44) $$, as in $$_{ 32 }^{ 76 }{ Ge }\: (76-32 =44)$$. Hence, these are isotones.
But the number of neutrons in $$_{ 32 }^{ 77 }{Ge } \: (77-32 =45)$$ and $$_{ 34 }^{ 77 }{Se }\: (77-34 = 43)
$$, are different than the number of neutrons in $$_{ 32 }^{ 76 }{ Ge }\: (76-32 =44)$$.
The main defect of Bohr's atom model is :
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mixing of classical and quantum theories
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exclusion of nuclear motion
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failed to explain the fine structure of spectral lines
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failed to explain larger atoms
Explanation
Bohr's model can only clearly explain hydrogen or hydrogen-like atoms, it fails when applied to larger and heavier atoms like iron, gold, mercury, etc.
The $$d_{z^{2}}$$ orbital can give room only to:
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$$10$$ electrons
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$$6$$ electrons
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$$2 $$ electrons
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$$4$$ electrons
Explanation
Any orbital can give room only to 2 electrons (maximum)
The Bohr model of atoms:
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uses Einstein's photo electric equation
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predicts continuous emission spectra for atoms
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predicts the same emission spectra for all types of atoms
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assumes that the angular momentum of electrons is quantized
Explanation
Bohr model of an atom states that only those orbits are allowed where angular momentum of electron are integral multiple of $$nh/2\pi$$. These orbits have quantized energy and angular momentum associated with electron.
The model can be applied to hydrogen or hydrogen-like atoms to explain their line emission spectrum.
Option D is correct.
Which of the following do not represent Bohr's model of an atom correctly?
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(i) and (ii)
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(ii) and (iii)
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(ii) and (iv)
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(i) and (iv)
Explanation
The electronic configuration of an atom of the element is derived using Bohr's formula $$2n^{2}$$, where $$n$$ is the no. of orbit.
According to this formula, the first shell can contain only 2 electrons and the second shell contain not more than 8 electrons.
The minimum angular momentum that can be possessed by an electron in hydrogen atom is:
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$$\dfrac{h}{4\pi }$$
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$$\dfrac{2h}{\pi }$$
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$$\dfrac{h}{2\pi }$$
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$$2\pi r$$
Explanation
The angular momentum that can be possessed by an electron in the hydrogen atom is given as; $$\dfrac{nh}{2\pi }$$;
where n = orbit in which electron is revolving.
So, for minimum angular momentum, $$n=1$$, therefore, the minimum angular momentum is $$\dfrac h{2 \pi}$$.
Hence, option $$C$$ is correct.
Isotopes have same____but different____.
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atomic number, mass number
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mass number, atomic number
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number of neutrons, atomic number
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None of these
Explanation
Isotopes of an element have same atomic number and different mass numbers.
Atomic models have been improved over the years. Arrange the following atomic models in the order of their chronological order.
(i) Rutherfords atomic model
(ii) Thomsons atomic model
(iii) Bohr's atomic model
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(i), (ii) and (iii)
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(ii), (iii) and (i)
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(ii), (i) and (iii)
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(iii), (ii) and (i)
Explanation
Sir J J Thomson in 1897 studied the characteristics of cathode rays and discovered protons.
Lord Rutherford in 1911 studied the atomic model and discovered the atomic nucleus.
Bohr later explained the stability of the atom which was not explained by the others in their atomic theory.
How many lines does a spectrum contain in an electronic transition from $$n =1 \:to \:n = 5$$ in hydrogen atom?
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$$10$$
0%
$$8$$
0%
$$1$$
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$$5$$
Explanation
The no. of spectral lines produced in a spectrum = $$\dfrac{{(n_{2}-n_{1})(n_{2}-n_{1}+1)}}{2}$$.
Given that $$n_{2}$$ = 5 and $$n_{1}$$ = 1; the no. of spectral lines = $$\dfrac{4\times 5}{2}$$
$$= 10.$$
The electronic configuration of element with atomic no. $$14$$ is:
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$$(2, 6, 6)$$
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$$(4, 6, 4)$$
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$$(2, 4, 8)$$
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$$(2, 8, 4)$$
Explanation
Electronic configuration of element with atomic number with $$14$$ is $$2, 8, 4$$
Select the correct statement?
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An atom has equal number of electrons and protons.
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An atom has equal number of electrons and neutrons.
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An atom has equal number of protons and neutrons.
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An atom has equal number of electrons, protons and neutrons.
Explanation
An atom is electrically neutral as it has an equal number of electrons and protons, that is, an equal number of negative and positive charges.
In order to become stable, atom loses or gains one or more electrons and forms an ion which carries a charge.
Hence the correct option is A.
Calculate the mass number of atoms $$X, Y$$ and $$Z$$?
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5, 11, 18
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10, 18, 31
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11, 18, 31
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11, 19, 30
Explanation
Atomic mass number = Total number of protons + Total number of neutrons
For $$\mathrm{X}$$, Atomic mass number = $$\mathrm{6+5=11}$$
For $$\mathrm{Y}$$, Atomic mass number= $$\mathrm{8+10=18}$$
For $$\mathrm{Z}$$, Atomic mass number= $$\mathrm{15+16=31}$$
Hence, option $$\mathrm{C}$$ is the correct answer.
The ratio of the radii of hydrogen atom and its nucleus is$$~ 10^5.$$ Assuming the atom and the nucleus to be spherical, if atom is represented by planet earth $$R_e = 6.4 \times10^6 m$$, estimate the size of the nucleus(radius).
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56 m
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60 m
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64 m
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68 m
Explanation
$$\frac {R_e}{r_n} = 10^5$$
If the atom is represented by the planet earth $$(R_e = 6.4 \times 10^6 m)$$ then the radius of the nucleus would be $$\displaystyle r_n = \frac {R_e}{10^5}$$
$$\displaystyle r_n = \frac {6.4 \times 10^6 m}{10^5}$$
$$r_n=6.4 \times 10 m$$
$$r_n= 64 m.$$
In an atom, the differentiating electron enters into 7s sub shell. The number of incomplete shells in the atom could be:
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$$1$$
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$$2$$
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$$3$$
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$$0$$
Explanation
According to Aufbau's Principle, when the differentiating electron enters into the 7s subshell, there will be three incomplete shells (7, 6, 5).
Energy of the electron in Bohr's orbit is equal to ?
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potential energy only
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Kinetic energy only
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Sum of potential and kinetic energy
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difference of kinetic and potential energy
Explanation
Energy of electron in Bohr orbit is equal to sum of kinetic and potential energy
$$\triangle E\quad =\quad KE\quad +\quad PE$$
Because of orbital energy is PE and electron revolving energy is kinetic energy
For manganese atom, assuming that Hund's rule is not valid for $$l=2\:sub shell,$$ predict the unpaired electrons and electron pairs in that sub shell of atom.
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$$5, 1$$
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$$5, 0$$
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$$1, 2$$
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$$1, 3$$
Identify the false statement among the following.
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Heisenberg's principle is contradictory to Bohr's theory
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Planck's quantum theory is taken as the basis for Bohr's theory
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Splitting up of spectral lines in presence of external magnetic field is due to the existence of sub shells
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Both A and C
Explanation
Option A is true. Bohr gave the theory of fixed orbits, which was contradictory to Heisenberg’s theory.
Option B is true. The electrons can only orbit stably, without radiating, in certain orbits (called by Bohr the "stationary orbits") at a certain discrete set of distances from the nucleus. These orbits are associated with definite energies and are also called energy shells or energy levels. In these orbits, the electron's acceleration does not result in radiation and energy loss as required by classical electromagnetics. The Bohr model of an atom was based upon Planck's quantum theory of radiation.
Option C is false. Bohr theory could not explain the Zeeman effect. In presence of magnetic field, each spectral line gets split up into fine lines, the phenomenon, is known as Zeeman effect.
Hence, C is the answer.
Bohr's model explains:
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the spectrum of hydrogen atom only
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the spectrum of any atom or ion having one electron only
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the spectrum of hydrogen molecule
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the solar spectrum
Explanation
Bohr's model successfully explained the spectrum of an atom or ion having one electron only.
An electron in hydrogen atom is excited to 'N' shell. What are the possible transitions it can undergo? Compare the energies of transitions.
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3 transitions, energies goes on decreasing
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2 transitions, energies goes on decreasing
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3 transitions, energies goes on increasing
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2 transitions, energies goes on increasing
Explanation
When an electron is in 'N' shell $$(n = 4)$$, it can undergo transition to $$n = 3, n = 2, n = 1\ shells$$. Therefore 3 electron transitions are possible. $$n = 4 \:to \:n = 3$$, is the least energy transition since the difference in energies of the two orbits is the least. $$n = 4 \:to \:n=1$$ corresponds to highest energy transition.
The electron is:
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$$\alpha$$-ray particle
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$$\beta$$-ray particle
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positron
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$$\gamma$$ -ray
Explanation
The electron is $$\beta $$ rays particle.
Identify the correct order of filling up of electrons in sub shells - 4p, 5s, 4d, 5p.
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4p, 5s, 4d, 5p
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4p, 4d, 5s, 5p
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5s, 5p, 4p, 4d
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4p, 5p, 5s, 5p
If a radioactive element $$_{79}{Au}$$ emits $$\beta$$-particle, what is the new group? $$_{79}{Au}$$ belongs to group I B (copper family)?
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I A
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I B
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II A
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II B
Explanation
$$_{79}{Au}\longrightarrow _{80}{Hg}+\beta^{-}$$. $$_{80}{Hg}$$ belongs to II B(zinc family). There is no change in the number of moles since atomic mass remains unchanged.
Atomic number of Bismuth is:
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84
0%
85
0%
83
0%
82
Explanation
The number of protons found in the nucleus of an atom of a given element is called atomic number. Elements are placed in periodic table according to their atomic number. Atomic number increases from left to right and top to bottom of periodic table. Higher the atomic number, heavier is the atom.
Example:- $$^4_2He\longrightarrow$$ Atomic number $$2$$ and mass number is $$4$$. $$[He\longrightarrow Helium]$$
$$^{208.9}_{83}Bi\longrightarrow$$ Atomic number is $$83$$ and mass number is $$208.9$$. $$[Bi\longrightarrow Bismuth]$$
Atomic number of strontium $$(Sr)$$ is equal to:
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28
0%
38
0%
42
0%
34
Explanation
The number of protons found in the nucleus of an atom of a given element is called atomic number. Elements are placed in periodic table according to their atomic number.
Example:-
(i) Atomic number of Strontium:- $$83$$
$$^{87.62}_{38}Sr$$
(ii) Atomic number of Rubidium:- $$37$$
$$^{85.4}_{37}Rb$$
The principal quantum number increases, the difference of energy between consecutive energy levels:
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decreases
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increases
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remain same
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sometimes increases and sometimes decreases
Explanation
Difference in energy is given as; $$\Delta E = -\frac{Z^{2}R}{n^{2}}.$$
Therefore, as principal quantum number(n) increases the energy of transition decreases.
A negative sign indicates the spin of electron.
The fundamental particles present in an atom are:
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Protons and electrons
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Electrons and neutrons
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Protons and neutrons
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Electrons and nucleons
Explanation
The fundamental particles present in an atom are electrons and nucleons (protons and neutrons).
Hence, (D) is the correct answer.
The ratio of the neutrons present in nitrogen atom and a silicon atom is:
(Mass number of nitrogen and silicon is 14 and 28 respectively)
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7 : 3
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3 : 7
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1 : 2
0%
2 : 1
Explanation
For nitrogen: atomic number = 7 and mass number = 14
$$\therefore$$ Number of neutrons $$= 14-7 = 7$$
For silicon: atomic number = 14 and mass number = 28
$$\therefore$$ number of neutrons $$= 28-14= 14$$
$$\therefore$$ Ratio of number of neutrons in nitrogen and silicon $$= 7:14 = 1:2$$
Atomic number of Radium is:
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84
0%
88
0%
86
0%
76
Explanation
The number of protons found in the nucleus of an tom of a given element is called atomic number. Elements that are placed in periodic table according to their atomic number.
Example:-
(1) Atomic number of Radium is $$88$$
$$^{226}_{88}Ra$$
(2) Atomic number of Barium is $$56$$
$$^{137.3}_{56}Ba$$
State whether the given statement is true or false:
Atomic mass of an element is same as the mass of a single atom of that element.
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True
0%
False
Explanation
Atomic mass of an element cannot be same as the mass of a single atom of that element because many naturally occurring elements exist in the form of two or more isotopes.
Isotopes are the atoms of the same elements having the same atomic number containing the same number of protons but different number of neutrons. So, their atomic masses vary. Average of atomic masses of different isotopes of the same element are taken and then the atomic mass of the element is decided.
For example, atomic mass of element carbon is 12 u. But we cannot say that mass of a single atom of carbon is 12 u, because there are different isotopes of carbon, like carbon-14 (atomic mass = 14 u), carbon-12 (atomic mass = 12 u), carbon-13 (atomic mass = 13 u), etc. Atomic mass of carbon element = 12u is just the average of these different atomic masses, and that's why it's more accurately called relative atomic mass.
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