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9 | 2339-2342 | These are
called the stationary states of the atom (ii) Bohr’s second postulate defines these stable orbits This postulate
states that the electron revolves around the nucleus only in those
orbits for which the angular momentum is some integral multiple of
h/2p where h is the Planck’s constant (= 6 6 ´ 10–34 J s) |
9 | 2340-2343 | (ii) Bohr’s second postulate defines these stable orbits This postulate
states that the electron revolves around the nucleus only in those
orbits for which the angular momentum is some integral multiple of
h/2p where h is the Planck’s constant (= 6 6 ´ 10–34 J s) Thus the
angular momentum (L) of the orbiting electron is quantised |
9 | 2341-2344 | This postulate
states that the electron revolves around the nucleus only in those
orbits for which the angular momentum is some integral multiple of
h/2p where h is the Planck’s constant (= 6 6 ´ 10–34 J s) Thus the
angular momentum (L) of the orbiting electron is quantised That is
L = nh/2p
(12 |
9 | 2342-2345 | 6 ´ 10–34 J s) Thus the
angular momentum (L) of the orbiting electron is quantised That is
L = nh/2p
(12 5)
(iii) Bohr’s third postulate incorporated into atomic theory the early
quantum concepts that had been developed by Planck and Einstein |
9 | 2343-2346 | Thus the
angular momentum (L) of the orbiting electron is quantised That is
L = nh/2p
(12 5)
(iii) Bohr’s third postulate incorporated into atomic theory the early
quantum concepts that had been developed by Planck and Einstein It states that an electron might make a transition from one of its
specified non-radiating orbits to another of lower energy |
9 | 2344-2347 | That is
L = nh/2p
(12 5)
(iii) Bohr’s third postulate incorporated into atomic theory the early
quantum concepts that had been developed by Planck and Einstein It states that an electron might make a transition from one of its
specified non-radiating orbits to another of lower energy When it
does so, a photon is emitted having energy equal to the energy
difference between the initial and final states |
9 | 2345-2348 | 5)
(iii) Bohr’s third postulate incorporated into atomic theory the early
quantum concepts that had been developed by Planck and Einstein It states that an electron might make a transition from one of its
specified non-radiating orbits to another of lower energy When it
does so, a photon is emitted having energy equal to the energy
difference between the initial and final states The frequency of the
emitted photon is then given by
hn = Ei – Ef
(12 |
9 | 2346-2349 | It states that an electron might make a transition from one of its
specified non-radiating orbits to another of lower energy When it
does so, a photon is emitted having energy equal to the energy
difference between the initial and final states The frequency of the
emitted photon is then given by
hn = Ei – Ef
(12 6)
where Ei and Ef are the energies of the initial and final states and Ei > Ef |
9 | 2347-2350 | When it
does so, a photon is emitted having energy equal to the energy
difference between the initial and final states The frequency of the
emitted photon is then given by
hn = Ei – Ef
(12 6)
where Ei and Ef are the energies of the initial and final states and Ei > Ef For a hydrogen atom, Eq |
9 | 2348-2351 | The frequency of the
emitted photon is then given by
hn = Ei – Ef
(12 6)
where Ei and Ef are the energies of the initial and final states and Ei > Ef For a hydrogen atom, Eq (12 |
9 | 2349-2352 | 6)
where Ei and Ef are the energies of the initial and final states and Ei > Ef For a hydrogen atom, Eq (12 4) gives the expression to determine
the energies of different energy states |
9 | 2350-2353 | For a hydrogen atom, Eq (12 4) gives the expression to determine
the energies of different energy states But then this equation requires
the radius r of the electron orbit |
9 | 2351-2354 | (12 4) gives the expression to determine
the energies of different energy states But then this equation requires
the radius r of the electron orbit To calculate r, Bohr’s second postulate
about the angular momentum of the electron–the quantisation
condition – is used |
9 | 2352-2355 | 4) gives the expression to determine
the energies of different energy states But then this equation requires
the radius r of the electron orbit To calculate r, Bohr’s second postulate
about the angular momentum of the electron–the quantisation
condition – is used The radius of nth possible orbit thus found is
2
2
0
42
2
n
n
h
r
m
e
ε
π
=
π
(12 |
9 | 2353-2356 | But then this equation requires
the radius r of the electron orbit To calculate r, Bohr’s second postulate
about the angular momentum of the electron–the quantisation
condition – is used The radius of nth possible orbit thus found is
2
2
0
42
2
n
n
h
r
m
e
ε
π
=
π
(12 7)
The total energy of the electron in the stationary states of the hydrogen
atom can be obtained by substituting the value of orbital radius in
Eq |
9 | 2354-2357 | To calculate r, Bohr’s second postulate
about the angular momentum of the electron–the quantisation
condition – is used The radius of nth possible orbit thus found is
2
2
0
42
2
n
n
h
r
m
e
ε
π
=
π
(12 7)
The total energy of the electron in the stationary states of the hydrogen
atom can be obtained by substituting the value of orbital radius in
Eq (12 |
9 | 2355-2358 | The radius of nth possible orbit thus found is
2
2
0
42
2
n
n
h
r
m
e
ε
π
=
π
(12 7)
The total energy of the electron in the stationary states of the hydrogen
atom can be obtained by substituting the value of orbital radius in
Eq (12 4) as
2
2
2
2
0
0
2
8
4
n
e
m
e
E
h
n
ε
ε
π
= −
π
π
or
4
2
2
2
0
8
n
me
E
n
εh
= −
(12 |
9 | 2356-2359 | 7)
The total energy of the electron in the stationary states of the hydrogen
atom can be obtained by substituting the value of orbital radius in
Eq (12 4) as
2
2
2
2
0
0
2
8
4
n
e
m
e
E
h
n
ε
ε
π
= −
π
π
or
4
2
2
2
0
8
n
me
E
n
εh
= −
(12 8)
Substituting values, Eq |
9 | 2357-2360 | (12 4) as
2
2
2
2
0
0
2
8
4
n
e
m
e
E
h
n
ε
ε
π
= −
π
π
or
4
2
2
2
0
8
n
me
E
n
εh
= −
(12 8)
Substituting values, Eq (12 |
9 | 2358-2361 | 4) as
2
2
2
2
0
0
2
8
4
n
e
m
e
E
h
n
ε
ε
π
= −
π
π
or
4
2
2
2
0
8
n
me
E
n
εh
= −
(12 8)
Substituting values, Eq (12 8) yields
18
2 |
9 | 2359-2362 | 8)
Substituting values, Eq (12 8) yields
18
2 182
10
J
En
n
−
×
= −
(12 |
9 | 2360-2363 | (12 8) yields
18
2 182
10
J
En
n
−
×
= −
(12 9)
Atomic energies are often expressed in electron volts (eV) rather than
joules |
9 | 2361-2364 | 8) yields
18
2 182
10
J
En
n
−
×
= −
(12 9)
Atomic energies are often expressed in electron volts (eV) rather than
joules Since 1 eV = 1 |
9 | 2362-2365 | 182
10
J
En
n
−
×
= −
(12 9)
Atomic energies are often expressed in electron volts (eV) rather than
joules Since 1 eV = 1 6 ´ 10–19 J, Eq |
9 | 2363-2366 | 9)
Atomic energies are often expressed in electron volts (eV) rather than
joules Since 1 eV = 1 6 ´ 10–19 J, Eq (12 |
9 | 2364-2367 | Since 1 eV = 1 6 ´ 10–19 J, Eq (12 9) can be rewritten as
2
13 |
9 | 2365-2368 | 6 ´ 10–19 J, Eq (12 9) can be rewritten as
2
13 6 eV
En
= −n
(12 |
9 | 2366-2369 | (12 9) can be rewritten as
2
13 6 eV
En
= −n
(12 10)
The negative sign of the total energy of an electron moving in an orbit
means that the electron is bound with the nucleus |
9 | 2367-2370 | 9) can be rewritten as
2
13 6 eV
En
= −n
(12 10)
The negative sign of the total energy of an electron moving in an orbit
means that the electron is bound with the nucleus Energy will thus be
required to remove the electron from the hydrogen atom to a distance
infinitely far away from its nucleus (or proton in hydrogen atom) |
9 | 2368-2371 | 6 eV
En
= −n
(12 10)
The negative sign of the total energy of an electron moving in an orbit
means that the electron is bound with the nucleus Energy will thus be
required to remove the electron from the hydrogen atom to a distance
infinitely far away from its nucleus (or proton in hydrogen atom) Rationalised 2023-24
Physics
300
12 |
9 | 2369-2372 | 10)
The negative sign of the total energy of an electron moving in an orbit
means that the electron is bound with the nucleus Energy will thus be
required to remove the electron from the hydrogen atom to a distance
infinitely far away from its nucleus (or proton in hydrogen atom) Rationalised 2023-24
Physics
300
12 4 |
9 | 2370-2373 | Energy will thus be
required to remove the electron from the hydrogen atom to a distance
infinitely far away from its nucleus (or proton in hydrogen atom) Rationalised 2023-24
Physics
300
12 4 1 Energy levels
The energy of an atom is the least (largest negative value)
when its electron is revolving in an orbit closest to the
nucleus i |
9 | 2371-2374 | Rationalised 2023-24
Physics
300
12 4 1 Energy levels
The energy of an atom is the least (largest negative value)
when its electron is revolving in an orbit closest to the
nucleus i e |
9 | 2372-2375 | 4 1 Energy levels
The energy of an atom is the least (largest negative value)
when its electron is revolving in an orbit closest to the
nucleus i e , the one for which n = 1 |
9 | 2373-2376 | 1 Energy levels
The energy of an atom is the least (largest negative value)
when its electron is revolving in an orbit closest to the
nucleus i e , the one for which n = 1 For n = 2, 3, |
9 | 2374-2377 | e , the one for which n = 1 For n = 2, 3, the
absolute value of the energy E is smaller, hence the energy
is progressively larger in the outer orbits |
9 | 2375-2378 | , the one for which n = 1 For n = 2, 3, the
absolute value of the energy E is smaller, hence the energy
is progressively larger in the outer orbits The lowest state
of the atom, called the ground state, is that of the lowest
energy, with the electron revolving in the orbit of smallest
radius, the Bohr radius, a 0 |
9 | 2376-2379 | For n = 2, 3, the
absolute value of the energy E is smaller, hence the energy
is progressively larger in the outer orbits The lowest state
of the atom, called the ground state, is that of the lowest
energy, with the electron revolving in the orbit of smallest
radius, the Bohr radius, a 0 The energy of this state (n = 1),
E1 is –13 |
9 | 2377-2380 | the
absolute value of the energy E is smaller, hence the energy
is progressively larger in the outer orbits The lowest state
of the atom, called the ground state, is that of the lowest
energy, with the electron revolving in the orbit of smallest
radius, the Bohr radius, a 0 The energy of this state (n = 1),
E1 is –13 6 eV |
9 | 2378-2381 | The lowest state
of the atom, called the ground state, is that of the lowest
energy, with the electron revolving in the orbit of smallest
radius, the Bohr radius, a 0 The energy of this state (n = 1),
E1 is –13 6 eV Therefore, the minimum energy required to
free the electron from the ground state of the hydrogen atom
is 13 |
9 | 2379-2382 | The energy of this state (n = 1),
E1 is –13 6 eV Therefore, the minimum energy required to
free the electron from the ground state of the hydrogen atom
is 13 6 eV |
9 | 2380-2383 | 6 eV Therefore, the minimum energy required to
free the electron from the ground state of the hydrogen atom
is 13 6 eV It is called the ionisation energy of the hydrogen
atom |
9 | 2381-2384 | Therefore, the minimum energy required to
free the electron from the ground state of the hydrogen atom
is 13 6 eV It is called the ionisation energy of the hydrogen
atom This prediction of the Bohr’s model is in excellent
agreement with the experimental value of ionisation energy |
9 | 2382-2385 | 6 eV It is called the ionisation energy of the hydrogen
atom This prediction of the Bohr’s model is in excellent
agreement with the experimental value of ionisation energy At room temperature, most of the hydrogen atoms are
in ground state |
9 | 2383-2386 | It is called the ionisation energy of the hydrogen
atom This prediction of the Bohr’s model is in excellent
agreement with the experimental value of ionisation energy At room temperature, most of the hydrogen atoms are
in ground state When a hydrogen atom receives energy
by processes such as electron collisions, the atom may
acquire sufficient energy to raise the electron to higher
energy states |
9 | 2384-2387 | This prediction of the Bohr’s model is in excellent
agreement with the experimental value of ionisation energy At room temperature, most of the hydrogen atoms are
in ground state When a hydrogen atom receives energy
by processes such as electron collisions, the atom may
acquire sufficient energy to raise the electron to higher
energy states The atom is then said to be in an excited
state |
9 | 2385-2388 | At room temperature, most of the hydrogen atoms are
in ground state When a hydrogen atom receives energy
by processes such as electron collisions, the atom may
acquire sufficient energy to raise the electron to higher
energy states The atom is then said to be in an excited
state From Eq |
9 | 2386-2389 | When a hydrogen atom receives energy
by processes such as electron collisions, the atom may
acquire sufficient energy to raise the electron to higher
energy states The atom is then said to be in an excited
state From Eq (12 |
9 | 2387-2390 | The atom is then said to be in an excited
state From Eq (12 10), for n = 2; the energy E2 is
–3 |
9 | 2388-2391 | From Eq (12 10), for n = 2; the energy E2 is
–3 40 eV |
9 | 2389-2392 | (12 10), for n = 2; the energy E2 is
–3 40 eV It means that the energy required to excite an
electron in hydrogen atom to its first excited state, is an
energy equal to E2 – E1 = –3 |
9 | 2390-2393 | 10), for n = 2; the energy E2 is
–3 40 eV It means that the energy required to excite an
electron in hydrogen atom to its first excited state, is an
energy equal to E2 – E1 = –3 40 eV – (–13 |
9 | 2391-2394 | 40 eV It means that the energy required to excite an
electron in hydrogen atom to its first excited state, is an
energy equal to E2 – E1 = –3 40 eV – (–13 6) eV = 10 |
9 | 2392-2395 | It means that the energy required to excite an
electron in hydrogen atom to its first excited state, is an
energy equal to E2 – E1 = –3 40 eV – (–13 6) eV = 10 2 eV |
9 | 2393-2396 | 40 eV – (–13 6) eV = 10 2 eV Similarly, E3 = –1 |
9 | 2394-2397 | 6) eV = 10 2 eV Similarly, E3 = –1 51 eV and E3 – E1 = 12 |
9 | 2395-2398 | 2 eV Similarly, E3 = –1 51 eV and E3 – E1 = 12 09 eV, or to excite
the hydrogen atom from its ground state (n = 1) to second
excited state (n = 3), 12 |
9 | 2396-2399 | Similarly, E3 = –1 51 eV and E3 – E1 = 12 09 eV, or to excite
the hydrogen atom from its ground state (n = 1) to second
excited state (n = 3), 12 09 eV energy is required, and so
on |
9 | 2397-2400 | 51 eV and E3 – E1 = 12 09 eV, or to excite
the hydrogen atom from its ground state (n = 1) to second
excited state (n = 3), 12 09 eV energy is required, and so
on From these excited states the electron can then fall back
to a state of lower energy, emitting a photon in the process |
9 | 2398-2401 | 09 eV, or to excite
the hydrogen atom from its ground state (n = 1) to second
excited state (n = 3), 12 09 eV energy is required, and so
on From these excited states the electron can then fall back
to a state of lower energy, emitting a photon in the process Thus, as the excitation of hydrogen atom increases (that is
as n increases) the value of minimum energy required to
free the electron from the excited atom decreases |
9 | 2399-2402 | 09 eV energy is required, and so
on From these excited states the electron can then fall back
to a state of lower energy, emitting a photon in the process Thus, as the excitation of hydrogen atom increases (that is
as n increases) the value of minimum energy required to
free the electron from the excited atom decreases The energy level diagram* for the stationary states of a
hydrogen atom, computed from Eq |
9 | 2400-2403 | From these excited states the electron can then fall back
to a state of lower energy, emitting a photon in the process Thus, as the excitation of hydrogen atom increases (that is
as n increases) the value of minimum energy required to
free the electron from the excited atom decreases The energy level diagram* for the stationary states of a
hydrogen atom, computed from Eq (12 |
9 | 2401-2404 | Thus, as the excitation of hydrogen atom increases (that is
as n increases) the value of minimum energy required to
free the electron from the excited atom decreases The energy level diagram* for the stationary states of a
hydrogen atom, computed from Eq (12 10), is given in
Fig |
9 | 2402-2405 | The energy level diagram* for the stationary states of a
hydrogen atom, computed from Eq (12 10), is given in
Fig 12 |
9 | 2403-2406 | (12 10), is given in
Fig 12 7 |
9 | 2404-2407 | 10), is given in
Fig 12 7 The principal quantum number n labels the stationary
states in the ascending order of energy |
9 | 2405-2408 | 12 7 The principal quantum number n labels the stationary
states in the ascending order of energy In this diagram, the highest
energy state corresponds to n =¥ in Eq, (12 |
9 | 2406-2409 | 7 The principal quantum number n labels the stationary
states in the ascending order of energy In this diagram, the highest
energy state corresponds to n =¥ in Eq, (12 10) and has an energy
of 0 eV |
9 | 2407-2410 | The principal quantum number n labels the stationary
states in the ascending order of energy In this diagram, the highest
energy state corresponds to n =¥ in Eq, (12 10) and has an energy
of 0 eV This is the energy of the atom when the electron is
completely removed (r = ¥) from the nucleus and is at rest |
9 | 2408-2411 | In this diagram, the highest
energy state corresponds to n =¥ in Eq, (12 10) and has an energy
of 0 eV This is the energy of the atom when the electron is
completely removed (r = ¥) from the nucleus and is at rest Observe how
the energies of the excited states come closer and closer together as
n increases |
9 | 2409-2412 | 10) and has an energy
of 0 eV This is the energy of the atom when the electron is
completely removed (r = ¥) from the nucleus and is at rest Observe how
the energies of the excited states come closer and closer together as
n increases 12 |
9 | 2410-2413 | This is the energy of the atom when the electron is
completely removed (r = ¥) from the nucleus and is at rest Observe how
the energies of the excited states come closer and closer together as
n increases 12 5 THE LINE SPECTRA OF THE HYDROGEN ATOM
According to the third postulate of Bohr’s model, when an atom makes a
transition from the higher energy state with quantum number ni to the
lower energy state with quantum number nf (nf < ni), the difference of
energy is carried away by a photon of frequency nif such that
FIGURE 12 |
9 | 2411-2414 | Observe how
the energies of the excited states come closer and closer together as
n increases 12 5 THE LINE SPECTRA OF THE HYDROGEN ATOM
According to the third postulate of Bohr’s model, when an atom makes a
transition from the higher energy state with quantum number ni to the
lower energy state with quantum number nf (nf < ni), the difference of
energy is carried away by a photon of frequency nif such that
FIGURE 12 7 The energy level
diagram for the hydrogen atom |
9 | 2412-2415 | 12 5 THE LINE SPECTRA OF THE HYDROGEN ATOM
According to the third postulate of Bohr’s model, when an atom makes a
transition from the higher energy state with quantum number ni to the
lower energy state with quantum number nf (nf < ni), the difference of
energy is carried away by a photon of frequency nif such that
FIGURE 12 7 The energy level
diagram for the hydrogen atom The electron in a hydrogen atom
at room temperature spends
most of its time in the ground
state |
9 | 2413-2416 | 5 THE LINE SPECTRA OF THE HYDROGEN ATOM
According to the third postulate of Bohr’s model, when an atom makes a
transition from the higher energy state with quantum number ni to the
lower energy state with quantum number nf (nf < ni), the difference of
energy is carried away by a photon of frequency nif such that
FIGURE 12 7 The energy level
diagram for the hydrogen atom The electron in a hydrogen atom
at room temperature spends
most of its time in the ground
state To ionise a hydrogen
atom an electron from the
ground state, 13 |
9 | 2414-2417 | 7 The energy level
diagram for the hydrogen atom The electron in a hydrogen atom
at room temperature spends
most of its time in the ground
state To ionise a hydrogen
atom an electron from the
ground state, 13 6 eV of energy
must be supplied |
9 | 2415-2418 | The electron in a hydrogen atom
at room temperature spends
most of its time in the ground
state To ionise a hydrogen
atom an electron from the
ground state, 13 6 eV of energy
must be supplied (The horizontal
lines specify the presence of
allowed energy states |
9 | 2416-2419 | To ionise a hydrogen
atom an electron from the
ground state, 13 6 eV of energy
must be supplied (The horizontal
lines specify the presence of
allowed energy states )
*
An electron can have any total energy above E = 0 eV |
9 | 2417-2420 | 6 eV of energy
must be supplied (The horizontal
lines specify the presence of
allowed energy states )
*
An electron can have any total energy above E = 0 eV In such situations the
electron is free |
9 | 2418-2421 | (The horizontal
lines specify the presence of
allowed energy states )
*
An electron can have any total energy above E = 0 eV In such situations the
electron is free Thus there is a continuum of energy states above E = 0 eV, as
shown in Fig |
9 | 2419-2422 | )
*
An electron can have any total energy above E = 0 eV In such situations the
electron is free Thus there is a continuum of energy states above E = 0 eV, as
shown in Fig 12 |
9 | 2420-2423 | In such situations the
electron is free Thus there is a continuum of energy states above E = 0 eV, as
shown in Fig 12 7 |
9 | 2421-2424 | Thus there is a continuum of energy states above E = 0 eV, as
shown in Fig 12 7 Rationalised 2023-24
301
Atoms
hvif = Eni – Enf
(12 |
9 | 2422-2425 | 12 7 Rationalised 2023-24
301
Atoms
hvif = Eni – Enf
(12 11)
Since both nf and ni are integers, this immediately shows that in
transitions between different atomic levels, light is radiated in various
discrete frequencies |
9 | 2423-2426 | 7 Rationalised 2023-24
301
Atoms
hvif = Eni – Enf
(12 11)
Since both nf and ni are integers, this immediately shows that in
transitions between different atomic levels, light is radiated in various
discrete frequencies The various lines in the atomic spectra are produced when electrons
jump from higher energy state to a lower energy state and photons are
emitted |
9 | 2424-2427 | Rationalised 2023-24
301
Atoms
hvif = Eni – Enf
(12 11)
Since both nf and ni are integers, this immediately shows that in
transitions between different atomic levels, light is radiated in various
discrete frequencies The various lines in the atomic spectra are produced when electrons
jump from higher energy state to a lower energy state and photons are
emitted These spectral lines are called emission lines |
9 | 2425-2428 | 11)
Since both nf and ni are integers, this immediately shows that in
transitions between different atomic levels, light is radiated in various
discrete frequencies The various lines in the atomic spectra are produced when electrons
jump from higher energy state to a lower energy state and photons are
emitted These spectral lines are called emission lines But when an atom
absorbs a photon that has precisely the same energy needed by the
electron in a lower energy state to make transitions to a higher energy
state, the process is called absorption |
9 | 2426-2429 | The various lines in the atomic spectra are produced when electrons
jump from higher energy state to a lower energy state and photons are
emitted These spectral lines are called emission lines But when an atom
absorbs a photon that has precisely the same energy needed by the
electron in a lower energy state to make transitions to a higher energy
state, the process is called absorption Thus if photons with a continuous
range of frequencies pass through a rarefied gas and then are analysed
with a spectrometer, a series of dark spectral absorption lines appear in
the continuous spectrum |
9 | 2427-2430 | These spectral lines are called emission lines But when an atom
absorbs a photon that has precisely the same energy needed by the
electron in a lower energy state to make transitions to a higher energy
state, the process is called absorption Thus if photons with a continuous
range of frequencies pass through a rarefied gas and then are analysed
with a spectrometer, a series of dark spectral absorption lines appear in
the continuous spectrum The dark lines indicate the frequencies that
have been absorbed by the atoms of the gas |
9 | 2428-2431 | But when an atom
absorbs a photon that has precisely the same energy needed by the
electron in a lower energy state to make transitions to a higher energy
state, the process is called absorption Thus if photons with a continuous
range of frequencies pass through a rarefied gas and then are analysed
with a spectrometer, a series of dark spectral absorption lines appear in
the continuous spectrum The dark lines indicate the frequencies that
have been absorbed by the atoms of the gas The explanation of the hydrogen atom spectrum provided by Bohr’s
model was a brilliant achievement, which greatly stimulated progress
towards the modern quantum theory |
9 | 2429-2432 | Thus if photons with a continuous
range of frequencies pass through a rarefied gas and then are analysed
with a spectrometer, a series of dark spectral absorption lines appear in
the continuous spectrum The dark lines indicate the frequencies that
have been absorbed by the atoms of the gas The explanation of the hydrogen atom spectrum provided by Bohr’s
model was a brilliant achievement, which greatly stimulated progress
towards the modern quantum theory In 1922, Bohr was awarded Nobel
Prize in Physics |
9 | 2430-2433 | The dark lines indicate the frequencies that
have been absorbed by the atoms of the gas The explanation of the hydrogen atom spectrum provided by Bohr’s
model was a brilliant achievement, which greatly stimulated progress
towards the modern quantum theory In 1922, Bohr was awarded Nobel
Prize in Physics 12 |
9 | 2431-2434 | The explanation of the hydrogen atom spectrum provided by Bohr’s
model was a brilliant achievement, which greatly stimulated progress
towards the modern quantum theory In 1922, Bohr was awarded Nobel
Prize in Physics 12 6 DE BROGLIE’S EXPLANATION OF BOHR’S
SECOND POSTULATE OF QUANTISATION
Of all the postulates, Bohr made in his model of the atom,
perhaps the most puzzling is his second postulate |
9 | 2432-2435 | In 1922, Bohr was awarded Nobel
Prize in Physics 12 6 DE BROGLIE’S EXPLANATION OF BOHR’S
SECOND POSTULATE OF QUANTISATION
Of all the postulates, Bohr made in his model of the atom,
perhaps the most puzzling is his second postulate It states
that the angular momentum of the electron orbiting around
the nucleus is quantised (that is, Ln = nh/2p; n = 1, 2, 3 …) |
9 | 2433-2436 | 12 6 DE BROGLIE’S EXPLANATION OF BOHR’S
SECOND POSTULATE OF QUANTISATION
Of all the postulates, Bohr made in his model of the atom,
perhaps the most puzzling is his second postulate It states
that the angular momentum of the electron orbiting around
the nucleus is quantised (that is, Ln = nh/2p; n = 1, 2, 3 …) Why should the angular momentum have only those values
that are integral multiples of h/2p |
9 | 2434-2437 | 6 DE BROGLIE’S EXPLANATION OF BOHR’S
SECOND POSTULATE OF QUANTISATION
Of all the postulates, Bohr made in his model of the atom,
perhaps the most puzzling is his second postulate It states
that the angular momentum of the electron orbiting around
the nucleus is quantised (that is, Ln = nh/2p; n = 1, 2, 3 …) Why should the angular momentum have only those values
that are integral multiples of h/2p The French physicist Louis
de Broglie explained this puzzle in 1923, ten years after Bohr
proposed his model |
9 | 2435-2438 | It states
that the angular momentum of the electron orbiting around
the nucleus is quantised (that is, Ln = nh/2p; n = 1, 2, 3 …) Why should the angular momentum have only those values
that are integral multiples of h/2p The French physicist Louis
de Broglie explained this puzzle in 1923, ten years after Bohr
proposed his model We studied, in Chapter 11, about the de Broglie’s
hypothesis that material particles, such as electrons, also
have a wave nature |
9 | 2436-2439 | Why should the angular momentum have only those values
that are integral multiples of h/2p The French physicist Louis
de Broglie explained this puzzle in 1923, ten years after Bohr
proposed his model We studied, in Chapter 11, about the de Broglie’s
hypothesis that material particles, such as electrons, also
have a wave nature C |
9 | 2437-2440 | The French physicist Louis
de Broglie explained this puzzle in 1923, ten years after Bohr
proposed his model We studied, in Chapter 11, about the de Broglie’s
hypothesis that material particles, such as electrons, also
have a wave nature C J |
9 | 2438-2441 | We studied, in Chapter 11, about the de Broglie’s
hypothesis that material particles, such as electrons, also
have a wave nature C J Davisson and L |
Subsets and Splits