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• Discovery of Proton

An Introduction

An atom consists of three subatomic particles which are – Protons, Neutrons and Electrons. Protons and neutrons are found in the nucleus of the atom while electrons are found in the orbits around the nucleus. In this article, we will discuss the discovery of protons in detail but before that you need to know what protons and their fundamental properties are. 

What are Protons? 

Protons are positively charged fundamental subatomic particles of atoms. Its symbol is p or p + . As we know that a hydrogen atom consists of one proton and one electron, so on removing the electron from the hydrogen atom a proton is produced. That is why protons are also denoted as H + . It possesses +1e (or 1.60 x 10 -19 coulomb) positive electric charge. Thus, protons have equal and opposite charge of electrons. 

The word Proton is a Greek word which means ‘First’. It was 1 st used by Ernest Rutherford in 1920. The subatomic particles protons and neutrons are together known as nucleons. Nucleons form the nucleus of an atom.

What is The Mass of Proton? 

The mass of the proton is 1.67 x 10 -24 gram or 1.67 x 10 -27 kg. As we know the mass of an electron is 9.1 x 10 -28 so the mass of a proton is 1836 times the mass of an electron. Although the mass of a proton is almost equal to the mass of a neutron. 

Discovery of a Proton 

Proton was found at the early stages of the investigations of atomic structure. English chemist William Prout gave Prout’s hypothesis in 1815 in which he proposed that all atoms are composed of hydrogen atoms. He called these hydrogen atoms ‘protyles’. Although it was disproved by various other discoveries and experiments later but set a fundamental base for discovery of various subatomic particles. Then in 1886, German physicist Eugen Goldstein carried out a modified cathode ray tube experiment in which he used electric discharge in a modified discharge tube with perforated cathode. In this experiment he discovered positively charged rays which he named ‘canal rays’. Canal rays are also known as anode rays.

Let us investigate the discovery of protons through a detailed explanation of the Canal Ray Experiment performed by Goldstein. 

Canal Ray Experiment: Discovery of Protons 

Goldstein used almost the same discharge tube as the cathode ray discharge tube used for discovery of electrons. The point of difference was the perforated cathode used in Goldstein’s canal ray experiment.  

Apparatus - Canal ray experiment apparatus consists of a tube (known as anode rays discharge tube) which is made of glass containing two thin pieces of metal, called electrodes, sealed in it. Out of these two electrodes one electrode (or one metal piece) has many holes in it which acts as a cathode while another electrode acts as anode. Both the electrodes are connected to the high voltage generator. The electrical discharge through the gasses could be observed only at very low pressures and at very high voltages. So, the tube was evacuated so that pressure of different gasses could be adjusted. When sufficiently high voltage is applied across the electrodes, current starts flowing through a stream of particles in the tube. 

Procedure and Observation – Electric current was passed through both the electrodes which creates an electric field in the tube and ionizes the gaseous atoms in the tube. At this point anode starts emitting positively charged rays which move towards the negatively charged cathode and pass the holes of the cathode and strike the glass walls of the tube at the end near the cathode. These rays produced a faint red glow. These rays were passing in the opposite direction of the cathode rays so it was concluded that the charge they carry must be opposite of cathode rays. As these rays were moving from anode to cathode so called anode rays as well. Due to the same reason the glass tube used in this experiment was called anode ray discharge tube. 

The characteristics of positively charged particles of canal rays are listed below –

Unlike cathode rays, mass of positively charged particles depends upon the nature of gas present in the anode ray tube. These are simply positively charged gaseous ions. 

The charge to mass ratio of the particles depends on the gas from which these originate.

Some of the positively charged particles carry a multiple of the fundamental unit of electric charge.

The behavior of these particles in the magnetic or electrical field is opposite to that observed for electron or cathode rays in cathode ray’s experiment. 

Thus, Eugen Goldstein 1 st observed the protons although it was named and identified in other nuclei by British physicist Ernest Rutherford in 1919. 

Properties of Protons

Physical properties of protons are as follows –

Charge of a Proton – Protons are positively charged particles. A proton has 1.60 x 10 -19 coulomb positive charge which is equal and opposite to that of an electron.

Mass of a Proton – Mass of one proton is equal to that of the mass of one hydrogen atom. As a hydrogen atom contains only one proton in its nucleus and mass of an atom depends on its nucleus. Protons can be produced by removing an electron from a hydrogen atom. The mass of a proton is 1836 times the mass of an electron. Mass of a proton is 1.676 x 10 -27 kg or 1.676 x 10 -24 g.

Number of protons in an atom possesses its atomic number. For example, hydrogen contains one proton, so its atomic number is 1 while helium contains two protons, so its atomic number is 2.

Protons are spin -½  fermions. This property of protons is used in Proton NMR. 

Fun Facts About Proton

Protons live up to 10 34 years 

Every element or material made in the lab will have at least one proton

Protons help bind nuclei together 

Characteristics of Proton

How to Determine the Number of Protons in any Element?

If you want to determine the number of protons, then it is equal to the atomic number of that element. For eg, hydrogen has an atomic number1 hence the number of protons in hydrogen will be 1

Similarly, below is the list of elements with the number of protons in it:

Different Type of Elements and Their Proton Number

Questions that can be asked in the Exam

What is the mass of a proton? 

How was the proton discovered?

Give some properties of proton

How many protons do the following elements have?

Explain in detail the gold foil experiment with a properly labeled diagram.

What color is produced by protons in the cathode ray tube?

What is the composition of the proton?

Explain some main functions of the proton.

This ends our coverage on the topic “Discovery of a Proton”. We hope you enjoyed learning and were able to grasp the concepts. We hope after reading this article you will be able to solve problems based on the topic. If you are looking for solutions to NCERT Textbook problems based on this topic, then log on to Vedantu website or download Vedantu Learning App. By doing so, you will be able to access free PDFs of NCERT Solutions as well as Revision notes, Mock Tests and much more. 

FAQs on Discovery of Proton

1. How was the proton discovered?

Proton is an atomic particle with a positive charge and having a mass slightly less than that of a neutron. Proton was discovered by Rutherford in the year 1909, through his famous gold foil experiment. Rutherford bombarded on gold foil and thought that hydrogen might be the fundamental building block of the nuclei. And then in 1920, he postulated the hydrogen nucleus as a new particle and named it a proton. You can study more about the discovery of a proton from the link available in this article.

2. What happens if an electron comes near a proton?

Proton is a positively charged particle whereas electron is a negatively charged particle. Any atom has the same number of protons and electrons making the atom neutrally charged and stable in nature. But if protons and electrons collide with each other it is called electron capture. However, it strongly depends on the energy of these collisions happening. If collided at high energy, the proton gets converted into a neutron with the emission of neutrinos. But protons and electrons cannot collide so easily in normal conditions due to the presence of strong nuclear force between them. 

3. Are there any online resources available to study this topic?

There are various books and online materials available to study atomic properties and revolving concepts. Students can read more about these, then they can log onto the Vedantu website . There you will get all solutions for NCERT textbook problems. It also has some revision notes, mock tests and all the study material needed for preparing any topic related to Science. Below given is the link to access all the study materials for free. 

4. Can protons leave an atom?

Atoms are the fundamental building blocks for building matters. All the atoms have the same number of protons as electrons. And the mass of an atom is determined by the number of protons in it. A proton is a leaving atom in a couple of ways. One is radioactive decay, the second can be alpha decay and the third is nuclear fission. Whenever an atom has an unstable nucleus, through radioactive decay, protons can leave the atom. The stability of the nucleus depends upon the ratio of protons to neutrons. There are three types of radioactive decay, which are alpha, beta, and gamma. A second way known as alpha decay is the only spontaneous process by which an atom will lose protons. And by performing nuclear fission, neutrons accelerate towards the nucleus and it causes the nucleus to break into fragments. 

5. Can we split protons? 

Yes, protons can be split. As they are not any fundamental particle. Protons are made of 2 quarks 2 up and 1 down. It is important to note that these protons cannot be simply taken apart and analyzed. Due to high energy bombarding them spontaneously at extremely high velocities, protons can be split. They can also be split using accelerators such as Large Hadron colliders. However, many other studies contradict the same. 

6. Is a proton bigger than an electron?

Protons are positively charged while electrons are negatively charged. A proton is 1835 times more massive than electrons. However protons and electrons both have approximately the same size. But a neutron is slightly heavier than a proton. The nucleus of an atom, which consists of protons and neutrons, occupies a space about 100,000 times smaller than the entire atom. Proton measures 1/50th of the diameter of an atom. So electrons are much smaller than protons and neutrons. But being small, the change of the electron is as strong as a proton. And one proton and one electron balance each other out. 

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Class Notes

Free Class Notes & Study Material

Discovery of Proton

Last Updated on July 3, 2023 By Mrs Shilpi Nagpal

​Since the atom as a whole is electrically neutral and the presence of negatively charged particles in it was established ,therefore, it was thought that some positively charged particles must also be present in the atom.

Goldstein in 1886  performed discharge tube experiment in which he took perforated cathode and a gas at low pressure was kept inside the tube, as before.

1)On passing high voltage between the electrodes ,it was found that some rays were coming from the side of the anode which passed through the holes in the cathode and produced green fluorescence on the opposite glass wall coated with zinc sulphide. These rays were called anode rays or canal rays or positive rays.

Properties of anode rays

1)They travel in straight line.

2)They are made up of material particles.

3)They are positively charged.

4)The value of e/m depend upon the nature of gas taken inside the discharge tube.

5)The value of the charge on the particles constituent the anode rays is also found to depend upon the nature of the gas taken inside the discharge tube.

6)The mass of the particle constituting the anode rays is also found to be different for different gases taken in discharge tube.

The charge on these particles is found to be same as that on the electron i.e. 1.6 × 10 -19  coulombs per gram.

The ratio, charge/mass, for each of the particle is found to be 9.58 × 10 -24 g.

These particles were termed as protons.

A proton may be defined as that fundamental particle which carries 1 unit positive charge and has a mass nearly equal to that of hydrogen atom.

Discovery of neutron

Chadwick in 1932  ,performed some scattering experiment in which he bombarded some light elements like beryllium and boron with fast moving Alpha particles. He found that some new particles were emitted which carried no charge ie. were neutral but had a mass nearly equal to that of proton. This particle was termed neutrons.

A neutron may be defined as that fundamental particles which carries no charge but has a mass nearly equal to that of hydrogen atom or proton.

About Mrs Shilpi Nagpal

Author of this website, Mrs. Shilpi Nagpal is MSc (Hons, Chemistry) and BSc (Hons, Chemistry) from Delhi University, B.Ed. (I. P. University) and has many years of experience in teaching. She has started this educational website with the mindset of spreading free education to everyone.

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CBSE Class 11 Chemistry Notes: Structure of Atom (Part - I)

This article provides you the revision notes on class 11 chemistry: chapter- structure of atom. some of the important topics covered in this part are: atom and its subatomic particles, rutherford’s nuclear model of atom, thomson’s model of atom, electromagnetic radiations and electromagnetic spectrum. these quick notes are prepared strictly according to the latest cbse syllabus for class 11..

• Atom and its subatomic particles
• Thomson model of atom
• Rutherford’s Nuclear Model of Atom

Electromagnetic radiations:

• Properties of electromagnetic radiations
• Characteristics of electromagnetic radiations
• Particle nature of electromagnetic radiation
• Photoelectric effect
• Dual behavior of electromagnetic radiation

CBSE Class 11 Chemistry Syllabus 2017 – 2018

Key notes of the chapter are:

• Atom is the smallest particle of matter that can take part in a chemical reaction. 
• Atom is made of electron, proton and neutrons.
• Atom is not capable of independent existence. 
• Two or more atoms combine together to form molecules.
• Negatively charged particle discovered on the basis of ‘cathode ray discharge tube’ experiments.
• Cathode rays start from cathode and move toward anode.
• These rays are not visible but their behaviour can be observed with fluorescent or phosphorus sent material.
• In the absence of electric or magnetic field these travels in strait lines.
• In the presence of electric or magnetic field the behaviour of cathode rays is similar to negatively charged particles which suggest that these rays contain negatively charge particles called electron.
• Positively charged particle discovered on the basis of anode ray experiment.
• These travel in straight line and posses mass many times the mass of an electron.
• These are not originated from anode.
• These are deflected by electric and magnetic field.
• Unlike cathode rays, the positively charged particles depend upon the nature of the gas from which these originate.
• Neutral particles discovered by bombarding a thin sheet of beryllium by α- particles.
• Most of the α-particles passed through foil undeflected, indicating most of the  space in atom is empty.
• Some of the α-particles are deflected to certain angles, which means that there is positively mass present in atom.
• Only some of the α-particles suffered large deflections, which means that the positively charged mass must be occupying very small space.
• Strong deflections or even bouncing back of α-particles from metal foil indicate the direct collision with positively charged mass in atom.

Comparison between the subatomic particles of an atom

• atom is considered asa uniform positively charged sphere with radius about 10 -10  m, in which electrons are is uniformly distributed.
• Electrons are embedded in such a manner to give most stable electrostatic arrangement.
• Mass of atom is assumed to be uniformly distributed in atom.
• Also known as plum pudding raisin pudding orwatermelon model.
• Based upon α-particles scattering experiment.
• Most part of the atom is empty.
• Atom possesses a highly dense, positively charged centre, called nucleus of the order 10 -13  cm.
• Entire mass of the atom is concentrated inside the nucleus.
• Electrons revolve around the nucleus in circular orbits.
• Electrons and the nucleus are held together by electrostatic forces of attraction.
• It doesn’t explain the stability of atom.
• It doesn’t say anything about the electronic distribution of electrons around nucleus.

Answer the following questions to check your preparedness:

Q. What information is obtained from the cathode rays experiment about the structure of atom?  

Q. How was the presence of proton detected and what are their characteristic?

Q. Give the characteristic properties of alpha (a) rays.

Q. Discuss the weakness of Rutherford atomic model.

Q. Calculate the mass and charge of one mole of electrons.

• Equal to the total number protons present in the nucleus or total number of electrons present the neutral atom.
• Represented by Z.
• Mass number of an element = number of protons + number of neutrons
• Denoted by A.
• These are the atoms of the same element having the same atomic number but different mass number.
• For example: 1 H 1 , 1 H 2 , 1 H 3
• These are the atoms of different elements having the same mass number but different atomic number.
• For example:  18 Ar 40  ,  20 Ca 40

• Radiations associated with electrical and magnetic fields.
• When an electrically charged particle moves under acceleration, alternating electrical and magnetic fields are produced and transmitted in the form of waves called electromagnetic waves or electromagnetic radiations.
• Oscillating electric and magnetic field are produced by oscillating charged particles. These fields are perpendicular to each other and both are perpendicular to the direction of propagation of the wave.
• These waves do not require medium i.e. electromagnetic wave can travel in vacuum.
• Wavelength:  It may be defined as the distance between two neighbouring crests or troughs of wave. It is denoted by λ.

• Frequency (ν):  It may be defined as the number of waves which pass through a particular point in one second.
• Velocity (v):  It is defined as the distance travelled by a wave in one second. In vacuum all types of electromagnetic radiations travel with thesame velocity which is 3 ×10  8 m/sec. It is denoted by v.

•   Amplitude (a): It is the height of the crest or depth of the trough of a wave.
• The radiant energy is emitted or absorbed not continuously but discontinuously in the form of small discrete packets of energy called ‘quantum’. In case of light, the quantum of energy is called a ‘photon’
• The energy of each quantum is directly proportional to the frequency of the radiation, i.e. E α υ

Or        E = hυ     

• Energy is always emitted or absorbed as integral multiple of this quantum, i.e,

           E = nhυ

           Where n =1,2,3,4,.....

• An ideal body, which emits and absorbs all frequencies, is calleda black body.
• The radiation emitted by such a body is called black body radiation.
• The phenomenon of ejection of electrons from the surface of metal when light of suitable frequency strikes it is calledphotoelectric effect. The ejected electrons are called photoelectrons.
•   Number of electron ejected is directly proportional to intensity (or brightness) of light.
• There is characteristic minimum frequency (ν 0  threshold frequency) below which photoelectric effect is not observed.
•  If ν > ν 0  then electrons comes out with kinetic energy which increases with increase in frequency of light.
• Kinetic energy of ejected electrons is given by-

                                    h ν = h ν 0 + ½(m e V 2 )

CBSE Class 11 Physics Syllabus 2017 - 2018

• The light possesses both particle and wave like properties.
• whenever radiation interacts with matter, it displays particle like properties (Black body radiation and photoelectric effect).
• When it propagates, it shows wave like properties (interference and diffraction).

When a white light is passed through a prism, it splits into a series of coloured bands known as spectrum.

Types of spectrum:

It is of two types:

(a) Continuous and line spectrum: The spectrum which consists of all the wavelengths is called continuous spectrum.

(b) Line spectrum: A spectrum in which only specific wavelengths are present is known as a line spectrum.

• It is a continuous spectrum.
• It consists of a range of electromagnetic radiations arranged in the order of increasing wavelengths or decreasing frequencies.
• Emission spectrum: The spectrum of radiation emitted by a substance that has absorbed energy is called an emission spectrum.
• Absorption spectrum: It is the spectrum of radiation transmitted through a substance, showing dark lines or bands due to absorption at specific wavelengths.

Try following questions to check your preparedness:

Q. Define spectrum and discuss line spectrum.

Q. Calculate the wavelength, frequency and wavenumber of a light wave whose period is 2.0 × 10–10 s.

Q. Mass of an electron is 9.1 × 10 -31 kg. if its K.E. is 3.0 × 10 -25 J, calculate its wavelength.

Q. Calculate the wave number of lines having the frequency of 5 x10 16 cycles per second.

CBSE Class 11 Biology Syllabus 2017 - 2018

CBSE Class 11 Mathematics Syllabus 2017 – 2018

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Structure of Atom Class 11 Chemistry Notes

Structure of atom class 11 chemistry notes chapter 2, atomic   theory of matter :-.

• Cathode rays start from cathode and move toward anode.
• These rays are not visible but there behavior can be observed with fluorescent or phosphorescent material.
• In the absence of magnetic or electric field these rays travels in straight lines. 
• In the presence of magnetic or electric field, the behavior of cathode rays is similar to Negatively   charged   particles. Which suggest that these rays contain negatively charge particles called electron.
• Cathode rays (or electrons) do not depend on  the material of the electrode and   nature of the gas in the tube so electrons are basic constituent of all atoms.

Charge (e) to mass (me) ratio of electron  

Measured by   j. j. thomson (1897). by using cathode ray tube. by applying electrical & magnetic field perpendicular to each other & also perpendicular to path of electrons. he proposed   deviation of particles from their path in presence of magnetic or electrical field depend upon the following-, charge of electron, mass of electron.

Discovery of protons

Discovery of neutrons, thomson model of atom, rutherford’s nuclear model of atom.

           Rutherford observed that-

• 1)     Most of the α-   practical   passed   through gold foil un-deflected.
• 2)     A small fraction of α- particles was deflected by small angles.
• 3)     A very few α- particles (about 1 in 20,000) bounced back means deflected by nearly 180 0

                     From above observations he concludes the structure of atom .

        on the basis of observation &   conclusion rutherford proposed model of atom as -, isobars :-  .

Wave nature of electromagnetic radiations: -

Particle nature of electromagnetic radiation :-    , photo electric effect :-, spectroscopy :- , bohr’s model for hydrogen atom:-.

Limitation of Bohr’s model:-

Dual behaviour of matter :-.

Heisenberg’s uncertainty principle:-

Quantum mechanical model of atom:-

• Branches of science which explain duel behavior of Metter is called quantum mechanics. 
• Quantum mechanics independently developed by Werner Heisenberg and Erwin Schrodinger (1926).
• Fundamental equation developed by Schrodinger. (He won Nobel Prize in 1933).
• Equation for a system (atom or molecules was, energy does not change with time)

Principle quantum number ‘n’ :-

             azimuthal quantum no.‘l’   :-.

  Magnetic orbital quantum no ‘m i ’ :-   

Electron spin quantum (m s )   :-  

Aufbau principle    :- , pauli exclusion principle   :-, hund’s   rule of maximum multiplicity :-..

Structure of Atom Class 11 MCQ

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Show Answer

2. Neutron was discovered by :

3.   radioactive isotope of hydrogen has ________ number of neutrons  :, 4.   cathode rays are deflected by  :.

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Canal Ray Experiment: Experimental Procedure, Explanation, Observations

Collegedunia Team

Content Curator

Canal Ray Experiment led to the discovery of protons . The discovery of protons after the electron strengthened the area of atomic structure . During his experiment, he applied a high voltage across the discharge tube containing a perforated cathode. The discharge tube was called Crookes tubes. Canal rays can also be called anode or positive rays as it’s a beam of positive ions . 

Key Terms: Canal rays, cathode rays, ionization, charged particle, electrodes, Crookes tube, cathode ray tube

Read More:   Number of Moles Formula

Apparatus Required

[Click Here for Sample Questions]

• A Cathode ray tube made of glass with two metal electrodes ( anode and cathode ) on each differentiated side.
• A high voltage source (external) is connected to the metal electrodes.
• The glass tube pressure is minimized through vacuum pumps or evacuating the air.
• To maintain a low pressure inside the glass tube , evacuate the air through the vacuum pump.
• Connect the two electrodes (anode and cathode) to a high external voltage source.
• High voltage passing through the electrode ionizes the air and makes it conduct the electricity like a conductor. This leads to the completion of the circuit and apparatus setup.
• Increase the external voltage source to several thousand volts, which results in the emission of faint luminous rays emerging from the cathode electrode holes.
• The rays which were moving in opposite to the cathode rays were called canal rays.

Explanation

Fig 1 Canal Ray Experiment

When a high external voltage source is applied to the glass tube via electrodes, it ionizes the gas present inside the tube where the positive ions constitute the origin of the canal ray. In addition, the canal rays are considered to be the nucleus of the gas which has differentiated properties compared to cathode rays. 

The canal rays depend on the nature or type of gas present inside the glass tube and are different from cathode rays. It is because the canal rays consist of positive ions formed as a result of gas ionization. In addition, the charge to mass ratio of ionized particles was found to be different and depended on the type of gasses.

Further, the particle behavior of canal rays is quite opposite to cathode rays when exposed to electric and magnetic fields. They also carry multiples of fundamental charges during emission. Finally, from the experiment of E.Goldstein, he concluded that the canal rays that move from the positive electrode to the negative electrode led to the discovery of “Proton ''.

Things to Remember

• Canal rays are ionized particles emerging from the ionization of gas and moving from positive to negative electrodes when external high voltage sources are applied.
• Canal rays are beams of positive ions discovered in 1886 by E.Goldstein.
• Canal ray experiment led to the discovery of subatomic particle called “Proton”
• The charge to mass ratio of canal rays varies in accordance with the type of gasses used within glass-tube or Crookes tubes .
• The particle behavior of canal rays, when exposed to electric and magnetic fields, was opposite compared to cathode rays.

Read More:  Gay-Lussac’s Law

Sample Questions

Ques. Who discovered the canal rays? (2 Marks)

Ans. E.Goldstein

Scientist Dempster was the one who used a spectrometer with ion sources but failed to achieve it in the magnetic field. But during later years, E.Goldstein discovered the canal rays through his glass-tube experiment using fluorescent patches.

Ques. Why are canal rays referred to as anode rays? (2 Marks)

Ans. Both anode rays and canal rays travel in opposite directions compared to cathode rays.

We know that the canal rays move from the positive electrode to the negative electrode similar to the anode rays. But, the cathode rays travel from the negative electrode to the positive electrode. Therefore, canal rays can also be called anode rays.

Ques. Write the difference between Cathode and Canal rays. (2 Marks)

• Cathode rays are negatively charged and emerge from negative electrodes whereas canal rays are positively charged and do not emerge from positive electrodes.
• In an electric field, cathode rays are attracted towards positive electrodes whereas canal rays are attracted toward negative electrodes.
• The charge to mass ratio of canal rays varies with respect to the type of gasses used within glass tubes whereas the charge to mass ratio of cathode rays does not change.

Ques. How are canal rays produced? (2 Marks)

Ans. When a high source of electric charges is applied to the electrodes of a glass tube containing low-pressure gasses, the gas gets ionized. The electrons emerging from the cathode collide with ionized particles to produce particles of positive charge which we call canal rays. 

Ques. State the characteristics of canal rays. (2 Marks)

• Canal rays are positively charged particles or ions that travel from positive to negative electrodes along with the gas.
• Canal rays are deflected in opposite direction compared to cathode rays when exposed to an electric and magnetic field
• Canal rays travel in unidirectional and at lower velocity compared to cathode rays
• It affects the photographic plate and produces fluorescence through gas ionization .

Ques. Does the charge of mass ratio vary for canal rays? (1 Mark)

Ans. Yes. We know that the charge to mass ratio of canal rays varies and is different for different types of gasses present within the glass tube. It is because canal rays are produced from the ionized gasses and each gas has different properties. So, the answer is “Yes''.

Ques. Explain the condition under which the canal rays are produced. (1 Mark)

• A glass-tube (Crookes tube) with low pressured air achieved through vacuum pump or air evacuation and two metal electrodes (anode and cathode)
• A high external voltage source is applied to the two metal electrodes.

Ques. Why is fluorescent material applied to the near anode in the glass tube of the canal ray experiment? (2 Marks)

Ans. We know that fluorescence is the emission of light through the absorption of electromagnetic radiation. So, to figure out the charge to mass ratio of cathode rays during electron discovery, the fluorescent material is applied to the near anode so that it can absorb the electrons to showcase through light.

Ques. What type of gases can be used in the canal ray experiment tube? (2 Marks)

Ans. E.Goldstein took helium gas in the cathode ray tube. But to achieve better results, we can use low-pressure hydrogen gas. It is because the ionization energy of helium is higher than that of hydrogen. Since canal rays emerge from gas ionization, hydrogen would be an ideal choice for this experiment. 

Ques. Write down the difference between the canal ray experiment tube and the anode ray experiment tube. (2 Marks)

• Anode ray experiment tube has a perforated cathode in the middle of the tube
• Canal ray experiment tube has cathode and anode as two metal electrodes at each end.

CBSE CLASS XII Related Questions

1. accomplish the following conversions:  (i) nitrobenzene to benzoic acid  (ii) benzene to m-bromophenol  (iii) benzoic acid to aniline  (iv) aniline to 2,4,6-tribromofluorobenzene  (v) benzyl chloride to 2-phenylethanamine  (vi) chlorobenzene to p-chloroaniline  (vii) aniline to p-bromoaniline  (viii) benzamide to toluene  (ix) aniline to benzyl alcohol., 2. an antifreeze solution is prepared from 222.6 g of ethylene glycol c 2 h 6 o 2  and 200 g of water. calculate the molality of the solution. if the density of the solution is 1.072 g ml –1 , then what shall be the molarity of the solution, 3. the oxidation number of cobalt in  \(k[co(co)_4]\)  is, 4. name the following halides according to the iupac system and classify them as alkyl, allyl, benzyl (primary, secondary, tertiary), vinyl or aryl halides: (i)  \((ch_3)_2chch(cl)ch_3\) (ii)  \(\text{ch}_3\text{ch}_2\text{ch}(\text{ch}_3)\text{ch}(\text{c}_2\text{h}_5)\text{cl}\) (iii)  \(\text{ch}_3\text{ch}_2\text{c}(\text{ch}_3)_2\text{ch}_2\text{i}\) (iv)  \((ch_3)_3cch_2ch(br)c_6h_5\) (v)  \(\text{ch}_3\text{ch}(\text{ch}_3)\text{ch(br)ch}_3\) (vi)  \(\text{ch}_3\text{c(c}_2\text{h}_5)_2\text{ch}_2\text{br}\) (vii)  \(\text{ch}_3\text{c(cl)(c}_2\text{h}_5)\text{ch}_2\text{ch}_3\) (viii)  \(\text{ch}_3\text{ch}=c(cl)\text{ch}_2\text{ch}(\text{ch}_3)_2\) (ix)  \(\text{ch}_3\text{ch}=chc(br)(\text{ch}_3)_2\) (x)  \(\text{p-clc}_6\text{h}_4\text{ch}_2\text{ch}(\text{ch}_3)_2\) (xi)  \(\text{m-clch}_2\text{c}_6\text{h}_4\text{ch}_2\text{c(ch}_3)_3\) (xii)  \(\text{o-br-c}_6\text{h}_4\text{ch(ch}_3\text{)ch}_2\text{ch}_3\), 5. write the mechanism of the following reaction : nbubr+kcn→etoh-h 2 o nbucn  , 6. comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements., subscribe to our news letter.

Explain the main properties of anode rays.

Definition anode rays are the stream of positively charged particles produced by the discharge tube containing gas at very low pressure. since these rays were coming from an anode, so they are called anode rays. these are also known as canal rays because they passed through the holes or canals in the cathode. properties anode rays travel in a straight line. they are deflected towards the negative plate so they carry a positive charge. particles present in anode rays are positively charged. they originate from the anode. the charge on particles depends upon the number of electrons lost by atoms..

Compare and contrast cathode and anode rays with respect to properties exhibited by them.

Write the properties of anode rays.

Which of the following are properties of anode rays?

Mention the properties of Anode Ray.

Which of the following are the properties of anode rays?