Structure of atom Flashcards

1
Q

No of e’s prop

A

intensity of light

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2
Q

KE of e’s increase with

A

Increase in freq of light

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3
Q

Lymann in

A

UV

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4
Q

Balmer in

A

Visible

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5
Q

Paschen, Brackett Pfund in

A

IR

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6
Q

Max wavelength n1,n2=

A

n2 = 2 and n1 = 1 in Lymann

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7
Q

Which spectral line has max wavelength?

A

1st

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8
Q

No of radiations emitted when e’ drops from nth level to ground level

A

n(n-1)/2

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9
Q

Bohr’s postulates

A

E’ revolve in circular orbits
Each orbit have fixed energy
E’ can move only in orbits with l = nh/2pi

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10
Q

Bohr merits

A

Could explain atomic spectra of H

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11
Q

Energy of nth orbit

A

En = 2.179 Z^2/(10^18 n^2) J/atom
En = -1312 Z^2/n^2 kJ/atom
-13.6 Z^2/n^2 eV/atom

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12
Q

If KE is x, PE is

A

-2x

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13
Q

Radius of nth orbit

A

rn = a(o)n^2/Z

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14
Q

Value of a(o)

A

0.529A*

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15
Q

Velocity of e’ in H

A

Vn = 2.189x10^6 Z /n

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16
Q

Energy of radiation emitted =

A

ΔE = 2.189Z^2/10^18(1/n1^2 - 1/n2^2) J
ΔE = 1312Z^2(1/n1^2 - 1/n2^2) kJ
ΔE = 13.6Z^21/n1^2 - 1/n2^2) eV

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17
Q

Bohr’s limitations

A

Failed to explain atomic spectra of multi e’ species, Zeeman & stark effect, de Broglie nature of matter

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18
Q

As mass increases, which nature increases

A

particle

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19
Q

Heisenburg uncertainty principl

A

It is impossible to determine V and position or position & momentum at the same time with accuracy
Δx.Δp = h/4pi

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20
Q

priniciple quantum no N starts from

A

1 to infinity
K, L, M, N,..

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21
Q

Max no of e’s in nth level

A

2n^2

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22
Q

Azhimuthal quantum no l =

23
Q

No of subshells in nth main shell

24
Q

Max no of e’s in sub shell

25
Magnetic quantum no m
-l to +l
26
No of orbitals in subshell
2l + 1
27
No of orbitals in nth main shell
n^2
28
Possibility of finding e's is maxm & min in
orbitals and nodes
29
No of spherical nodes
n-l-1
30
No of nodal plane
l
31
Total nodes
n-1
32
Covalent cmpds
Exist in 3 states, low MP and BP, Soluble in org solv, bad conductors
33
Formal charge FC =
Valence - Non bonding e's - 1/2 bonding e's
34
Incomplete octet eg
BCl3, AlCl3
35
Expanded octet eg
SF6, PCl5
36
Odd e' molecule
NO, NO2
37
Formation of Xe & Kr cmpds
XeO3 & XeF2
38
Factors of Ionic bond
IE - decreases for e +ve atom -ve e' gain enthalpy of e' -ve atom & lattice energy increases
39
Lattice enthalpy depends on
|Q1Q2| Size - inverse
40
Factors affecting covalent nature
Size of cation - inverse Size of anion - prop to polarisation Charge - prop
41
2 e' pair, shape
linear
42
3 e' pair, shape
trigonal planar
43
4 e' pair shape
tetrahedral
44
5 e' pair shape
trigonal bipyramidal
45
Trigonal planar eg
BF3
46
Tetrahedral eg
CH4, NH4
47
Trigonal bipyramidal eg
PCl5
48
Octahedral eg
SF6
49
Hybridisation H =
1/2[V+M+A-C] V valence, M monovalent atom, C charge of cation, A charge of anion
50
MOT
e' are present in MO MO formed are combination of at. orbitals of same energy & symmetry MO are multi centered
51
No of MO =
No of AO
52
Energy of BMO, AO and AMO
BMO
53
Bond order
1/2[Nb - Na]
54
Bond order depends on
bond len - inv bond energy - prop