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Atomic model of Bohr in section third

Three dimensional teaching objective

1, knowledge and skills

(1) understanding the main content of Bohr' s atomic theory;

(2) understanding the concepts of energy levels, energyquantization, ground state and excited state.

2, process and method: through the study of Bohr theory, tofurther understand the hydrogen spectrum.

3, emotion, attitude and values: cultivate our spirit ofinquiry into science, and develop the spirit of independenceand innovation.

Teaching emphasis: the basic hypothesis of Bohr' s atomictheory.

Teaching difficulties: explanation of hydrogen spectrum byBohr theory.

Teaching methods: teacher elicitation, guidance, studentdiscussion and communication.

(1) introducing new courses

Put questions to

(1) what is the phenomenon of alpha particle scatteringexperiment?

(2) what is the content of the nuclear structure theory?

(3) the contradiction between Lu Sefu' s nuclear structuretheory and classical electromagnetic theory

In order to solve these contradictions, Bohr, a Danishphysicist, proposed his own atomic structure hypothesis in

1913.

(two) take a new course

1. Bohr' s atomic theory

(1) energy level (steady state) hypothesis: the atom can onlyexist in a series of discontinuous energy states. In theseStates, the atom is stable, although electrons move around thenucleus, but do not radiate energy outwards. These states arecalled stationary states. (this hypothesis is proposed foratomic stability)

(2) transition hypothesis: atoms from a steady state (energyEn) transition to another steady state (energy Em) , itsradiation (or absorption) photon frequency, the photon energyis determined by the deviation of the two kinds of stationaryenergy, namely the MERGEFORMAT (EMBED Equation.3 h Planck

(constant) the assumptions for the linear spectrum method)

(3) orbital quantization hypothesis: the different energystates of the atom correspond to the motion of electrons aroundthe nucleus in different circular orbits. The stationary stateof atoms is discontinuous, so the distribution of the possibleorbits of electrons is also discontinuous. (for the nuclearmodel, it is a supplement to the energy level hypothesis)

2. According to the classical electromagnetic theory andNewtonian mechanics, Bohr calculated the possible orbitalradii of hydrogen atoms and the energy (including kineticenergy and potential energy) of electrons moving in variousorbits:

The MERGEFORMAT Equation. 3 orbit radius: EMBED n=1, 2, 3. . . . . .The MERGEFORMAT Equation. 3 energy: EMBED n=1, 2, 3. . . . . .Type R1, E1, representing the first (i. e. from the recentnuclear) movement may orbit radius and electron in the orbitof energy, RN and En respectively represent the article n maytrack radius and electron in the N orbit and the energy of nis a positive integer, called quantum number.

3. Energy level diagram of hydrogen atom

Starting from Bohr' s basic hypothesis, using the classicalelectromagnetism and classical mechanics theory, we cancalculate the possible orbit radius and the correspondingenergy of electrons in hydrogen atom.

(1) the size of the hydrogen atom: the radius of each possibleorbit of the electron of hydrogen atom rn:rn=n2r1,

R1 represents the first line (nearest to the nucleus) . Theradius of the possible orbit is r1=0.53 x 10-10 M

For example: n=2, r2=2. 12 x 10-10 M

(2) energy levels of hydrogen atom:

The energy value En of an atom in its steady state is calledthe energy level of an atom. It can track the correspondingelectron kinetic energy En (including En=E1/n2 n=1 kinetic andpotential energy) , 2, 3,

E1 represents the energy that electrons move on the firstpossible orbit, E1=-13.6eV

Note: when calculating the energy, the electric potentialenergy is zero, the electron is negatively charged, theelectron is negative in the positive charge field, the kineticenergy of the electrons is half of the absolute value of theelectric potential energy, and the total energy is negative.For example: n=2, E2=-3.4eV, n=3, E3=-1.51eV, n=4,

E4=-0.85eV, . . . . . .

The energy level diagram of hydrogen atom is shown:

Explanation of hydrogen spectrum by 4 and Bohr' s Theory

(1) ground state and excited state

Ground state: in the normal state, the atom is in the lowestenergy level, when the electron moves in the nearest orbit fromthe nucleus, which is called the ground state.

Excited state: when the atom is in the higher energy level, theelectron moves in the orbit far away from the nucleus. Thissteady state is called excited state.

Class practice

(1) in the following statements of Bohr' s theory, what iscorrect is (ACD)

A. inherits Rutherford' s atomic model, but introduces quantumhypothesis to atomic energy and electronic orbit

B. agrees with the point of view that the electromagnetic chargeof accelerating motion should be radiated in the classicalelectromagnetic theory

The quantitative relation between the atomic luminescencefrequency and the atomic energy change is established by theenergy transformation and conservation of C.

The two formula of D. Bohr is based on his theory, usingclassical electromagnetic theory and Newtonian mechanics

(2) in the following explanation of Bohr' s theory, the

incorrect statement is (C)

A. atoms can only exist in a series of discontinuous States,each state corresponding to a certain energy

In the B. atom, although the electrons outside the nucleuscontinue to accelerate, they do not radiate energy as long asthe energy state does not change

When the C. atom transitions from one stationary state toanother, it is necessary to radiate a certain frequency ofphotons

Each energy state of the D. atom corresponds to an electronicorbit, and these orbits are discontinuous

(3) according to Bohr' s theory, the greater the quantum numberN in hydrogen atom, the correct in the following statement is(ACD)

The larger the electron orbit radius of A. is, the higher therate of electrons outside the B. nucleus is

The greater the energy level of the C. hydrogen atom, thegreater the potential energy of the outer electrons of the D.nucleus

(4) according to Bohr' s atomic theory, the radius of electronmotion around an atom (D)

A. can take any value, B. can take any value in a certain range

C. can take a series of discontinuous arbitrary values, D. isa series of discontinuous specific values

(5) according to Bohr' s theory, the electrons in ahydrogen atomspontaneously transition from a circular orbit with a radiusof RA to a circular orbit with a radius of Rb, and the knownra>rb is in this process (C)

The A. atom emits a series of photons, and the B. atom absorbsa series of photons

C. atoms emit photons of a certain frequency, and D. atomsabsorb photons of a certain frequency

The center of http://www. zgjhjy.com/.

The motion of electrons around nuclei (with acceleration)The frequency of the radiation electromagnetic wave is equalto the frequency of the operation around the nucleus

Energy reduction, orbital radius reduction, frequencyvari ati on

The electronfalls into theatomicnucleus alongthe spiral line,and the spectrum of the atom should be continuous

(contradiction: actually a discontinuous bright line)The atom is unstable

(contradiction: in fact, atoms are stable)

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