www.sakshieducation.com ATOMIC STRUCTURE.
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The proton and neutron together called as _______________
Charge on proton is_____, electron is ______and neutron is____________.
Electron was discovered by _________________
First model of atom was proposed by _______________
According to Thomson electrons are present in _______________
Thomson’s model of atom failed to explain _____________
Rutherford proposed the model of atom based on his _________experiment.
Rutherford’s model of atom is also known as ___________
According to Rutherford, atoms are ________in shape.
Most of the mass of the atom is present in its ____________
According to Rutherford, the two forces acting on the electron are ______and ______forces.
Quantum theory of radiation is proposed by _________________
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According to Quantum theory electromagnetic radiation is in the form of packets called______________.
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Quantum principle is _____________
In the formula E = hν ‘h’ is ________________________
Planck based on his theory explained the radiation of _____________
Value of Planck’s constant is _____________
Bohr proposed a model of atom based on __________________
According to Bohr’s model, electrons revolve in ________________
The energy of a stationary orbit which is near to the nucleus is ___________
Electron jumps from _______energy level to _________energy level.
When electron jumps form higher energy level to lower energy level the difference in the energy
levels is radiated as _________________
Angular momentum of electron is equal to _____________
In the formula mvr = nh /2π ‘n’ is known as __________________
Splitting of spectral lines in the presence of magnetic field is known as _____________
Bohr’s model is applicable only for the atoms of ___________________
Elliptical orbits are introduced by __________________
The angular momentum of an electron revolving in elliptical orbit is ____________
According to Sommerfeld stationary orbits are further divided into______________.
Dual nature of electron was explained by_________________.
De broglie explained __________________based on the dual nature of electron.
Wave equation of electron was proposed by ________________
Derivations of wave equation lead to ______________
Stationary orbits are denoted by _______________
Sub stationary orbits are also known as __________
The number of sub stationary orbits present in a stationary orbit depends on ____value.
Number of sub stationary orbits in M orbit are ___________
Principle quantum number was proposed by ________________
‘n’ value of N shell is _______
The quantum number which gives the size and energy of an orbit is _________
No. of sub stationary orbit in a stationary orbit is __________
Azimuthal quantum number was proposed by __________________
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Azimuthal quantum number is also known as ___________________
For a given value of n, the maximum value of l is __________
Shape of sub stationary shell can be determined by using ________
When l = 0, the shape of the orbit is ____________
Magnetic quantum number was proposed by__________.
‘m’ value depends on ________
For a given ‘l’ value, ‘m’ can have __________values.
The boundaries of ‘m’ values for a given ‘l’ value are __________
Orbitals having same energy are called _____________
The orientation of orbitals in the presence of magnetic field can be determined by ____
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The shell having least energy is -__________.
Sub shells present in L- shell are ___________
Maximum value of l when n=5 is__________
f- orbital is present in _________shell.
No. of sub shells present in L shell are -----------Spin quantum number was proposed by ______________
Spin of electrons takes the values as _____________
No. of electrons present in a sub shell are _______
The region in space where there is finite probability of finding electron is called ________
Shape of s- orbital is _______________
Type of orbital present in K- shell is _________
Type of orbital present in L- shell are ______________
Type of orbital present in M-shell are ______________
Type of orbital present in N- shell are ‘_____________
The n+l value of 3s orbital is__________.
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The region in space where the probability of finding electron is zero is called ______________
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P-orbitals will start in _______shell.
Shape of P-orbital is ___________
‘d’-orbital will start from __________
The number of d- orbitals present in n = 3 is________.
The orbital with least energy is _________
Among 3s, 3p the orbital having least energy is ______.
________has given a diagram to know the order of energy levels of orbitals.
A systematic representation of the occupation of electrons in the orbitals is known as ___
According to __________principle electron occupies the orbital having lowest energy.
Aufbau principle in terms of quantum numbers, the incoming electron occupies an orbital whose
n+l value is ___________
The ‘l’ value of s-orbital is _______
The ‘l’ value of p-orbital is________.
The ‘l’ value of d-orbital is ________
The ‘l’ value of f-orbital is ______
____________rule states that electron pairing takes place only after al the available degenerate
orbitals are occupied by one electron each.
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_________________principle states that no two electrons will have all four quantum numbers same.
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Electronic configuration of Si (Z = 14 ) is ______________
Electronic configuration of Zn (Z=30) is ______________
Electronic configuration of K (Z=19) is _____________
Electronic configuration of Cr (Z=24) is ______
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The distance between nucleus and valency orbital is known as __________
Units of atomic radius A0.
1 A0 = _______cm.
Atomic radius depends on ______________________
The minimum energy required to remove an electron from the outer most orbital of an atom in
gaseous state is known as _______________
Units of Ionization Energy are ____________
As nuclear charge increases the I.E. __________
As the ion charge increases the I.E.__________.
I.E. ____________with increase in atomic size.
The energy released when an electron is added to a neutral gaseous atom in its lowest nergy state
is known as ___________________
Electron affinity is measured in ________
Among 3p, 4s, 3d and 4p the orbital having least energy is _____
After filling the 3d orbital electron enters into _____orbital.
Valence electronic configuration of Cu is __________
www.sakshieducation.com www.sakshieducation.com MATCHING
GROUP : A
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GROUP : B
Neils Bohr.
Sommerfeld
Uhlenbeck & Goudsmith
Lande
Louis De – Broglie
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D
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B
E
C
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B)
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D)
E)
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G)
GROUP : A
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GROUP : B
Principle Quantum number
Wave equation
Quantum theory of radiation
Planetary model of atom
Azimuthal quantum number
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D
E
C
B
A
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B)
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D)
E)
F)
G)
GROUP : A
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Sommerfeld
Rutherford.
Max planck
Neils Bohr.
Erwin schrodinger
Louis De-broglie
J.J.Thomson
GROUP : B
K – Shell
L – Shell
M – Shell
N – Shell
O – Shell
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(
(
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A
D
B
C
E
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A)
B)
C)
D)
E)
n=1
n = 3.
f – orbital.
n = 2.
s,p,d,f,and g orbitals.
GROUP : B
GROUP : A
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Elliptical orbits.
Spin Quantum number.
Dual nature of electron.
Stationary orbits
Magnetic Quantum Number.
Wave Equation.
Planetary model.
Ar
Al
Mg
Ca
Ne
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E
B
F
A
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1s2 2s2 2p6
1s2 2s2 2p63s2
1s2 2s2 2p63s2 3p6
1s2 2s2 2p63s2 3p2
1s2 2s2 2p63s2 3p1
1s2 2s2 2p63s2 3p64s2
1s2 2s2 2p63s2 3p4
ELECTRONIC CONFIGURATION OF SOME ELEMENTS
Element
Name of the
symbol
element
Hydrogen
H
Atomic
number
1
1s1
Electronic configuration
Long form
Valence
configuration
1s1
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Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorin
He
Li
Be
B
C
N
O
F
2
3
4
5
6
7
8
9
Neon
Sodium
Magnesium
Aluminium
Silicon
Phosphorous
Sulphur
Chlorine
Argon
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
1s2
1s22s1
1s22s2
1s2 2s 2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s22s22p5
1s22s22p6
1s22s22p63s1
1s22s22p63s2
1s22s22p63s2 3p1
1s22s22p63s2 3p2
1s22s22p63s2 3p3
1s22s22p63s2 3p4
1s22s22p63s2 3p5
1s22s22p63s2 3p6
1s22s22p63s2 3p64s1
1s22s22p63s2 3p64s2
1s22s22p63s2 3p64s23d1
1s22s22p63s2 3p64s23d2
1s22s22p63s2 3p64s23d3
1s22s22p63s2 3p64s13d5
1s22s22p63s2 3p64s23d5
1s22s22p63s2 3p64s23d6
1s22s22p63s2 3p64s23d7
1s22s22p63s2 3p64s23d8
1s22s22p63s2 3p64s13d10
1s22s22p63s2 3p64s23d10
1s2
(He) 2s1
(He) 2s2
(He) 2s2 2p1
(He) 2s22p2
(He) 2s22p3
(He) 2s22p4
(He) 2s22p5
(He) 2s22p6
(Ne)3s1
(Ne)3s2
(Ne)3s23p1
(Ne)3s23p2
(Ne)3s23p3
(Ne)3s23p4
(Ne)3s23p5
(Ne)3s23p6
(Ar) 4s1
(Ar) 4s2
(Ar)4s23d1
(Ar)4s23d2
(Ar)4s23d3
(Ar)4s13d5
(Ar)4s23d5
(Ar)4s23d6
(Ar)4s23d7
(Ar)4s23d8
(Ar)4s13d10
(Ar)4s23d10
ANSWERS
1) Nucleons 2) Positive, Negative, No charge 3) J.J.Thomson 4) J.J. Thomson 5) Nucleus
6) Atomic spectra 7) α – ray scattering experiment 8) Planetary model or Nuclear model
9) Spherical 10) Nucleus 11) Centripetal, Centrifugal 12) Max planck 13) Quanta 14) E = hν
15) Planck’s Constant 16) Black body 17) 6.625 x 10-27 erg sec or 6.625 x 10-34 joule.sec
18) Planck’s Quantum theory 19) Stationary orbit 20) Less 21) Higher, Lower
22) E2 - E1 = hν 23) mvr = nh /2π. 24) Principle quantum number 25) Zeeman effect
26) Single electron 27) Sommerfield 28) mvr = kh/ 2π 29) Sub stationary orbits 30) Louis De Broglie
31) Quantizationof angular momentum 32) Erwin Schordinger 33) Atomic orbitals 34) Principle
quantum number 35) Atomic orbitals 36) n 37) 3 38) Neils bohr 39) 4 40) Principle quantum number
41) n2 42) Somerfield 43) Angular momentum quantum number 44) n – 1 45) l 46) Circular 47)
Lande 48) l 49) (2l + 1) 50) -l to +l 51) Degenerate orbitals
52) Magnetic quantum number 53) K 54) s and p 55) 4 56) N 57) 2
58) Uhlenbeck and Goudsmith 59) +1/2 or -1/2 60) 2 61) Orbital 62) Spherical 63) s 64) s and p 65)
s, p, and d 66) s,p,d, and f 67) 3 68) Nodal region 69) L 70) Dumbell 71) M 72) 5 73) 1s
74) 3S 75) Moeller 76) Electronic configuration 77) Aufbau 78) n + l 79) 0 80) 1 81) 2 82) 3
83) Hund’s 84) Pauli’s exclusion 85) 1s22s2 2p6 3s2 3p2 (or) (Ne) 3s2 3p2.
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86) 1s 2s 2p 3s 3p 4s 3d (or) (Ar) 4s2 3d10. 87) 1s22s2 2p6 3s2 3p6 4s1 (or) (Ar) 4s1.
88) 1s22s2 2p6 3s2 3p6 4s1 3d5(or) (Ar) 4s1 3d5 89) Atomic radius 90) A0 91) 10-8 Cm
92) Principle quantum number 93) Ionization energy 94) e.v or K. Cal/mole or K. Joule/mole
95) increases 96) increases 97) Decreases 98) Electron Affinity 99) ev 100) 3p 101) 4p
102) 4s13d10.
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