What Did Rutherford's Experiment Prove

The plum pudding model of J. J. Thomson could not able to explicate certain experimental results virtually the atomic structure of elements. still, there was no clear model that defines atoms, therefore in 1909, Ernest Rutherford, a British scientist conducted an experiment and based on the experiment he observed and proposed the atomic structure of elements and Rutherford Atomic Model.

Atomic model

Bones Constituents of an Atom

An atom consists of Electrons, Protons, and Neutrons are the key particles or sub-diminutive particles that build the construction of an cantlet. Permit the states understand each term.

Electron: In 1897, J. J. Thomson discovered negatively charged particles towards the anode, these rays are emitted by the cathode in a cathode ray experiment. And then these negatively charged particles are proposed as Electrons.
Protons: In 1886, Ernest Goldstein discovered that anode emitted positively charged particles with a different condition in the aforementioned tube, known as Culvert rays or as Protons.
Neutrons: A subatomic particle with no charge and a mass equivalent to protons in the nucleus of all atoms were discovered by J. Chadwick. These neutrally charged particles are termed Neutrons.

Isotopes are the elements that have the same atomic number but different mass. due east.g. Isotopes of the Hydrogen atoms are Protium (¹H_one), Deuterium (²H₁) and Tritium(ⁱⁱⁱH₁). Isotopes of the Carbon atoms are ¹²C_vi, ^xiiiC_half-dozen, ¹⁴C₆.

Isobars are the elements that have different diminutive number but have same mass number. e.k. ¹⁹K₄₀, ^eighteenAr₄₀, ^twentyCa₄₀, hither all the elements having same mass number hence the are isobars.

Rutherford'due south Alpha Scattering Experiment

fix-up of Rutherford'south experiment

He carry an experiment by bombarding alpha particles into a thin canvas of gilt and so notices their interaction with the gilt foil and trajectory or path followed by these particles.

In the experiment, Rutherford passes very loftier streams of alpha-particles from a radioactive source i.e. alpha-particle emitter, at a thin sheet of100 nm thickness of gold. In order to examine the deflection produced by the blastoff particles, he placed a screen of fluorescent zinc sulphide around the sparse golden foil. Rutherford made certain observations that oppose Thomson's atomic model.

Observations of Rutherford'due south Alpha Scattering Experiment

The observations of Rutherford'southward Alpha Scattering Experiment are:

Beginning, he observe that most of the α-particles that are bombarded towards the gilded sheet pass away the foil without whatsoever deflection, and hence it shows most of the space is empty.
Out of all, some of the α-particles were deflected through the gold sail past very modest angles, and hence it shows the positive charge in an atom is non-uniformly distributed. The positive charge is full-bodied in a very minor book in an cantlet.
Very few of the alpha-particles(1-2%) were deflected back, i.e. merely a very less amount of α-particles had virtually 180° angle of deflection. this shows that the book occupied by the positively charged particles is very small equally compared to the total book of an atom.

Rutherford Atomic Model

Rutherford proposed the atomic structure of elements, on the basis of his experiment. Co-ordinate to Rutherford's atomic model:

The positively charged particle was concentrated in an extremely small book and near of the mass of an atom was also in that book. He called this a nucleus of an cantlet.
Rutherford proposed that there is negatively charged electrons around the nucleus of an atom. the electron surrounding the nucleus revolves around it in a circular path with very high speed. He named orbits to these round paths.
Nucleus being a densely concentrated mass of positively charged particles and electrons being negatively charged are held together by a strong strength of attraction called electrostatic forces of attraction.

Observation of Rutherford's model

Limitations of Rutherford Atomic Model

The Rutherford diminutive model is failed to explicate certain things.

According to Maxwell, an electron revolving around the nucleus should emit electromagnetic radiations due to accelerated charged particles emit electromagnetic radiations. just Rutherford model says that the electrons revolve effectually the nucleus in stock-still paths called orbits. The radiation would behave free energy from the motion which led to the shrinking of orbit. Ultimately electrons would plummet within the nucleus.
As per the Rutherford model, calculations have shown that an electron would collapse in the nucleus in less than ten^-8seconds. So Rutherford model has created a loftier contradiction with Maxwell's theory and Rutherford after could not explain the stability of an atom.
Rutherford also did not describe the system of electrons in the orbit equally one of the other drawbacks of his model.

Regardless of seeing the early diminutive models were inaccurate and failed to explain certain experimental results, they were the base for future developments in the globe of quantum mechanics.

Sample Questions

Question 1: Proper name the cantlet which has i electron, one proton and no neutron.

Answer:

It is true for hydrogen atom ¹H₁.

The diminutive number of Hydrogen = No. of Proton = 1

The mass number of hydrogen = 1

No. of neutrons = 0

Therefore hydrogen cantlet has one electron, ane proton and no neutron.

Question 2: Define the term basis country of an cantlet?

Answer:

It is the country of an cantlet where all the electrons in the atom are in their everyman energy state or levels is called the ground state.

Question iii: Represent the chemical element 'Ten' which contains 15 electrons and 16 neutrons.

Answer:

Atomic number of element = no. of electron = xv

Mass number of element = no. of electrons + no. of neutrons

= 15 + 16

= 31

The correct representation of element X is ³¹X₁₅.

Question 4: Name the particle and requite its location in the cantlet which has no charge and has a mass nearly equal to that of a proton.

Answer:

The particle which has no charge and has a mass about equal to that of a proton is a neutron and it is present in the nucleus of the atom.

Question 5: An atom has both electron aspect negative charge and protons attribute positive charge but why at that place is no charge?

Reply:

The positive and negative charges of protons and electrons are equal in magnitude, they cancel the effect of each other. So, the atom as a whole is electrically neutral.

Question 6: What is the valency of the Sodium atom (Na)?

Reply: