What are subatomic particles definition types and charges
Subatomic particles is essential in chemistry and helps students understand various practical and theoretical applications related to this topic.
What is Subatomic Particles in Chemistry?
A subatomic particle refers to a particle smaller than an atom, including protons, neutrons, and electrons. This concept appears in chapters related to Atomic Structure, Discovery of Proton, and Structure of Atom, making it a foundational part of your chemistry syllabus.
Molecular Formula and Composition
The molecular formula concept does not apply to subatomic particles, as they are the building blocks of atoms—not molecules themselves. Atoms are made of a nucleus (containing protons and neutrons) and electrons orbiting outside.
Preparation and Synthesis Methods
Subatomic particles are not synthesized in the lab like compounds. Instead, their existence was revealed through experiments such as cathode ray tubes for electrons, gold foil experiments for protons, and nuclear bombardment for neutrons. Today, advanced particle accelerators can create or observe more exotic particles.
Physical Properties of Subatomic Particles
Subatomic particles differ by mass, charge, and location in the atom:
- Proton: Mass = 1 amu, Charge = +1, Location = Nucleus
- Neutron: Mass ≈ 1 amu, Charge = 0, Location = Nucleus
- Electron: Mass ≈ 1/1837 amu, Charge = –1, Location = Electron shells/cloud
| Particle | Symbol | Charge | Relative Mass | Location in Atom |
|---|---|---|---|---|
| Proton | p+ | +1 | 1 amu | Nucleus |
| Neutron | n | 0 | 1 amu | Nucleus |
| Electron | e- | –1 | 1/1837 amu | Outside nucleus (shells) |
Chemical Properties and Reactions
Subatomic particles participate in chemical properties through interactions like:
- Electrons drive chemical bonding and reactions.
- Protons define the element’s identity (atomic number).
- Neutrons influence isotopes and nuclear stability.
Frequent Related Errors
- Confusing the charge of protons and electrons.
- Thinking only electrons can move; protons and neutrons stay fixed in chemistry.
- Assuming all subatomic particles have significant mass—electrons are much lighter.
- Believing electrons orbit in flat circles; they actually exist in clouds/orbitals.
Uses of Subatomic Particles in Real Life
Subatomic particles are used in several areas:
- Protons are used in proton therapy to treat cancers.
- Neutrons are used in nuclear reactors and medical imaging.
- Electrons flow in electric currents and play a key part in electronics.
Relation with Other Chemistry Concepts
Subatomic particles are closely related to concepts like isotopes (varying neutrons), ion formation (loss or gain of electrons), and differences in atomic number/mass. They also help explain periodic table trends and how atoms bond together.
Step-by-Step Reaction Example
1. Consider sodium (Na) reacting with chlorine (Cl).2. Sodium atom loses 1 electron (subatomic particle) → forms Na+ ion.
3. Chlorine atom gains that 1 electron → forms Cl- ion.
4. Opposite charges attract, creating ionic NaCl.
Lab or Experimental Tips
Remember: Protons and neutrons are always found inside the nucleus, while electrons orbit outside. A simple tip Vedantu educators share is to picture the atom like a mini solar system—nucleus (sun) in the center, electrons (planets) moving around.
Try This Yourself
- Draw a labelled diagram of an atom and mark locations of proton, neutron, and electron.
- Fill out a table for mass and charge of each subatomic particle.
- Find out how ions form from atoms using electron gain/loss.
- Give an example of a medical use of subatomic particles.
Final Wrap-Up
We explored subatomic particles—their discovery, types, mass, charge, and importance for chemistry and real life. Use the summaries and examples above to strengthen your concepts. For more help, join live doubt-solving and exam-prep sessions on Vedantu or explore related topics like structure of atom any time.
FAQs on Subatomic Particles in Atomic Structure
1. What are subatomic particles?
Subatomic particles are the smaller particles that make up an atom, mainly protons, neutrons, and electrons. These particles determine the structure and properties of all elements in chemistry.
- Protons: Positively charged particles located in the nucleus.
- Neutrons: Neutral particles located in the nucleus.
- Electrons: Negatively charged particles found in energy levels around the nucleus.
2. What is the charge and mass of protons, neutrons, and electrons?
Protons have a charge of +1, neutrons have 0 charge, and electrons have a charge of −1, with relative masses of about 1, 1, and 1/1836 respectively. These values are essential in atomic structure calculations.
- Proton: Charge = +1, Relative mass ≈ 1 amu
- Neutron: Charge = 0, Relative mass ≈ 1 amu
- Electron: Charge = −1, Relative mass ≈ 1/1836 amu
3. Where are subatomic particles located in an atom?
Protons and neutrons are located in the nucleus, while electrons occupy the electron cloud or energy levels surrounding the nucleus. This arrangement forms the basis of the modern atomic model.
- The nucleus is dense and contains protons and neutrons.
- Electrons move in specific energy levels (shells and orbitals).
- Most of the atom’s volume is empty space occupied by electron probability regions.
4. What is the difference between protons, neutrons, and electrons?
The main difference between protons, neutrons, and electrons is their charge, mass, and location in the atom. These differences determine atomic identity and chemical behavior.
- Protons: +1 charge, mass ≈ 1 amu, located in nucleus, determine atomic number.
- Neutrons: 0 charge, mass ≈ 1 amu, located in nucleus, determine isotopes.
- Electrons: −1 charge, very small mass, located in energy levels, responsible for bonding.
5. How do you calculate the number of protons, neutrons, and electrons in an atom?
You calculate subatomic particles using the atomic number (Z) and mass number (A). These values are found in the periodic table or isotope notation.
- Protons = Atomic number (Z)
- Electrons (neutral atom) = Atomic number (Z)
- Neutrons = Mass number (A) − Atomic number (Z)
- Protons = 11
- Electrons = 11
- Neutrons = 23 − 11 = 12
6. What are isotopes and how are they related to subatomic particles?
Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This means they have the same atomic number but different mass numbers.
- Same protons → same element
- Different neutrons → different mass
7. What are ions and how do electrons form them?
An ion is a charged atom formed when it gains or loses electrons. The number of protons remains unchanged, but the electron count changes.
- Cation: Formed by loss of electrons (positive charge), e.g., Na → Na+ + e−
- Anion: Formed by gain of electrons (negative charge), e.g., Cl + e− → Cl−
8. Who discovered protons, neutrons, and electrons?
The electron was discovered by J.J. Thomson, the proton is credited to Ernest Rutherford, and the neutron was discovered by James Chadwick. These discoveries shaped modern atomic theory.
- 1897: Thomson discovered the electron using cathode rays.
- 1917: Rutherford identified the proton through nuclear experiments.
- 1932: Chadwick discovered the neutron.
9. What is the mass number and how is it related to subatomic particles?
The mass number (A) is the total number of protons + neutrons in an atom’s nucleus. It represents the approximate atomic mass in atomic mass units (amu).
- Mass number (A) = Protons + Neutrons
- Electrons are not included because their mass is negligible.
10. Why are subatomic particles important in chemistry?
Subatomic particles are important because they determine an element’s identity, mass, charge, and chemical reactivity. Without understanding protons, neutrons, and electrons, atomic structure cannot be explained.
- Protons define the element (atomic number).
- Neutrons affect stability and isotopes.
- Electrons control bonding and chemical reactions.
