Skip to main content
Chemistry LibreTexts

Sub-Atomic Particles

  • Page ID
  • \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

    \( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)

    ( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)

    \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

    \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)

    \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

    \( \newcommand{\Span}{\mathrm{span}}\)

    \( \newcommand{\id}{\mathrm{id}}\)

    \( \newcommand{\Span}{\mathrm{span}}\)

    \( \newcommand{\kernel}{\mathrm{null}\,}\)

    \( \newcommand{\range}{\mathrm{range}\,}\)

    \( \newcommand{\RealPart}{\mathrm{Re}}\)

    \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

    \( \newcommand{\Argument}{\mathrm{Arg}}\)

    \( \newcommand{\norm}[1]{\| #1 \|}\)

    \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

    \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)

    \( \newcommand{\vectorA}[1]{\vec{#1}}      % arrow\)

    \( \newcommand{\vectorAt}[1]{\vec{\text{#1}}}      % arrow\)

    \( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vectorC}[1]{\textbf{#1}} \)

    \( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)

    \( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)

    \( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)

    \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

    A typical atom consists of three subatomic particles: protons, neutrons, and electrons (as seen in the helium atom below). Other particles exist as well, such as alpha and beta particles (which are discussed below). The Bohr model shows the three basic subatomic particles in a simple manner. Most of an atom's mass is in the nucleus—a small, dense area at the center of every atom, composed of nucleons. Nucleons include protons and neutrons. All the positive charge of an atom is contained in the nucleus, and originates from the protons. Neutrons are neutrally-charged. Electrons, which are negatively-charged, are located outside of the nucleus.


    The Bohr model is outdated, but it depicts the three basic subatomic particles in a comprehensible way. Electron clouds are more accurate representations of where electrons are found. Darker areas represent where the electrons are more likely to be found, and lighter areas represent where they are less likely to be found.

    Beryllium Atom

    Particle Electric Charge (C) Atomic Charge Mass (g) Atomic Mass (Au) Spin
    Protons +1.6022 x 10-19 +1 1.6726 x 10-24 1.0073 1/2
    Neutrons 0 0 1.6740 x 10-24 1.0078 1/2
    Electrons -1.6022 x 10-19 -1 9.1094 x 10-28 0.00054858 1/2
    • Au is the SI symbol for atomic mass unit.
    • The positive charge of protons cancels the negative charge of the electrons. Neutrons have no charge.
    • With regard to mass, protons and neutrons are very similar, and have a much greater mass than electrons. Compared with neutrons and protons, the mass of an electron is usually negligible.
    • Spin is associated with the rotation of a particle. Protons, neutrons, and electrons each have a total spin of 1/2.


    Protons were discovered by Ernest Rutherford in the year 1919, when he performed his gold foil experiment. He projected alpha particles (helium nuclei) at gold foil, and the positive alpha particles were deflected. He concluded that protons exist in a nucleus and have a positive nuclear charge. The atomic number or proton number is the number of protons present in an atom. The atomic number determines an element (e.g., the element of atomic number 6 is carbon).


    Electrons were discovered by Sir John Joseph Thomson in 1897. After many experiments involving cathode rays, J.J. Thomson demonstrated the ratio of mass to electric charge of cathode rays. He confirmed that cathode rays are fundamental particles that are negatively-charged; these cathode rays became known as electrons. Robert Millikan, through oil drop experiments, found the value of the electronic charge.

    Electrons are located in an electron cloud, which is the area surrounding the nucleus of the atom. There is usually a higher probability of finding an electron closer to to the nucleus of an atom. Electrons can abbreviated as e-. Electrons have a negative charge that is equal in magnitude to the positive charge of the protons. However, their mass is considerably less than that of a proton or neutron (and as such is usually considered insignificant). Unequal amounts of protons and electrons create ions: positive cations or negative anions.


    Neutrons were discovered by James Chadwick in 1932, when he demonstrated that penetrating radiation incorporated beams of neutral particles. Neutrons are located in the nucleus with the protons. Along with protons, they make up almost all of the mass of the atom. The number of neutrons is called the neutron number and can be found by subtracting the proton number from the atomic mass number. The neutrons in an element determine the isotope of an atom, and often its stability. The number of neutrons is not necessarily equal to the number of protons.


    Both of the following are appropriate ways of representing the composition of a particular atom:


    Often the proton number is not indicated because the elemental symbol conveys the same information.

    Consider a neutral atom of carbon: \(\ce{^{12}_{6}C}\). The atomic mass number of Carbon is 12 amu, the proton number is 6, and it has no charge. In neutral atoms, the charge is omitted.

    He Atom.png

    Above is the atomic symbol for helium from the periodic table, with the atomic number, elemental symbol, and mass indicated.

    Every element has a specific number of protons, so the proton number is not always written (as in the second method above).

    • # Neutrons = Atomic Mass Number - Proton Number
      • Atomic mass number is abbreviated as A.
      • Proton number(or atomic number) is abbreviated Z.
    • # Protons = Proton Number or Atomic Number
    • In neutral atoms, # Electrons = # Protons
    • In ions, # Electrons = # Protons - (Charge)
    • Charge is written with the number before the positive or negative sign
      • Example, 1+

    Note: The atomic mass number is not the same as the atomic mass seen on the periodic table. Click here for more information.

    Other Basic Atomic Particles

    Many of these particles (explained in detail below) are emitted through radioactive decay. Click here for more information. Also note that many forms of radioactive decay emit gamma rays, which are not particles.

    Alpha Particles

    Alpha particles can be denoted by He2+,α2+, or just α. They are helium nuclei, which consist of two protons and two neutrons. The net spin on an alpha particle is zero. They result from large, unstable atoms through a process called alpha decay. Alpha decay is the process by which an atom emits an alpha particle, thereby becoming a new element. This only occurs in elements with large, radioactive nuclei. The smallest noted element that emits alpha particles is element 52, tellurium. Alpha particles are generally not harmful. They can be easily stopped by a single sheet of paper or by one's skin. However, they can cause considerable damage to the insides of one's body. Alpha decay is used as a safe power source for radioisotope generators used in artificial heart pacemakers and space probes.

    Figure: Alpha Decay involves the emission of an alpha particle from the nucleus

    Beta Particles

    Beta particles (β) are either free electrons or positrons with high energy and high speed; they are emitted in a process called beta decay. Positrons have the exact same mass as an electron, but are positively-charged. There are two forms of beta decay: the emission of electrons, and the emission of positrons. Beta particles, which are 100 times more penetrating than alpha particles, can be stopped by household items like wood or an aluminum plate or sheet. Beta particles have the ability to penetrate living matter and can sometimes alter the structure of molecules they strike. The alteration usually is considered damage, and can cause cancer and death. In contrast to beta particle's harmful effects, they can also be used in radiation to treat cancer.

    Beta--) or Electron Emission

    Electron emission may result when excess neutrons make the nucleus of an atom unstable. As a result, one of the neutrons decays into a proton, an electron, and an anti-neutrino. The proton remains in the nucleus, and the electron and anti-neutrino are emitted. The electron is called a beta particle. The equation for this process is given below:

    \[ _{1}^{0}\textrm{n}\rightarrow {_{1}^{1}\textrm{p}}^+ + \textrm{e}^- + \bar{\nu_{e}} \]

    • n = Neutron
    • p+ = Proton
    • e- = Electron (beta particle)
    • νe = Anti-neutrino

    β- Decay


    Beta++) or Positron Emission

    Position emission occurs when an excess of protons makes the atom unstable. In this process, a proton is converted into a neutron, a positron, and a neutrino. While the neutron remains in the nucleus, the positron and the neutrino are emitted. The positron can be called a beta particle in this instance. The equation for this process is given below:

    \[ { _{1}^{1}\textrm{p}}^+ \rightarrow _{1}^{0}\textrm{n} + \textrm{e}^+ + \nu_{e} \]

    • n = Neutron
    • p+ = Proton
    • e+ = Positron (beta particle)
    • νe = Neutrino

    β+ Decay


    Outside Links

    • Basic Sub-Atomic Particles:
    • Alpha Particles:
    • Beta Particles:
    • What are Sub-Atomic Particles?:
    • Atomic Number and Mass Number:


    1. Petrucci, Ralph, William Harwood, Geoffrey Herring, and Jeffry Madura.General Chemistry. 9th ed. Upper Saddle River, New Jersey: Pearson Prentince Hall, 2007.
    2. Haskin, Larry A. The Atomic Nucleus and Chemistry; D. C. Heath and Company: Lexington, MA, 1972; pp. 3-4, 43-53.
    3. Petrucci, Ralph, F. Geoffrey Herring, Jeffrey D. Madura, and Carey Bissonnette. General Chemistry. 10th ed. Upper Saddle River, New Jersey: Pearson Education, Inc., 2011.


    1. Identify the number of protons, electrons, and neutrons in the following atom.

    question one.jpeg.jpg

    2. Identify the subatomic particles (protons, electrons, neutrons, and positrons) present in the following:

    • \(\ce{^{14}_6C}\)
    • \(\alpha\)
    • \(\ce{^{35}Cl^-}\)
    • \(\beta^+\)
    • \(\beta^-\)
    • \(\ce{^{24}Mg^{2+}}\)
    • \(\ce{^{60}Co}\)
    • \(\ce{^3H}\)
    • \(\ce{^{40}Ar}\)
    • \(^1_0n\)

    3. Given the following, identify the subatomic particles present. (The periodic table is required to solve these problems)

    • Charge +1, 3 protons, mass number 6.
    • Charge -2, 7 neutrons, mass number 17.
    • 26 protons, 20 neutrons.
    • 28 protons, mass number 62.
    • 5 electrons, mass number 10.
    • Charge -1, 18 electrons, mass number 36.

    4. Arrange the following elements in order of increasing (a) number of protons; (b) number of neutrons; (c) mass.

    27Co, when A=59; 56Fe, when Z=26; 11Na, when A=23; 80Br, when Z=35; 29Cu, when A=30; 55Mn, when Z=25

    5. Fill in the rest of the table:

    Atomic Number Mass Number Number of Protons Number of Neutrons Number of Electrons
    2     2  
      23     11
        15 16  
      85 37    
    53     74  

    Solutions and Explanations

    1. There are 4 protons, 5 neutrons, and 4 electrons. This is a neutral beryllium atom.

    2. Identify the subatomic particles present in the following:

    • 146C
      • 6 protons, 8 neutrons, 6 electrons
        • There are 6 protons in accordance with the proton number in the subscript. There are 6 electrons because the atom is neutral. There are 8 neutrons because 14-6=8. 14 is the atomic mass number in the superscript.
    • α
      • 2 protons, 2 neutrons, 0 electrons
        • This is an alpha particle which can also be written as 4He2+. There are two protons because the element is helium. There are no electrons because 2-2 = 0. There are 2 neutrons because 4-2=2.
    • 35Cl-
      • 17 protons, 18 neutrons, 18 electrons
        • This is a chloride ion. According to the periodic table, there are 17 protons because the element is chlorine. There are 18 electrons due to the negative charge: 17-(-1) = 18. There are 18 neutrons because 35-17=18.
    • β+
      • 0 protons, 0 neutrons, 0 electrons, 1 positron
        • This is a beta+ particle. It can also be written as e+. "e" represents an electron, but when it has as positive charge it is a positron.
    • β-
      • 0 protons, 0 neutrons, 1 electron
        • This is a beta- particle, and can also be written as e-. This is a standard electron.
    • 24Mg2+
      • 12 protons, 12 neutrons, 10 electrons
        • This is a magnesium Ion. There are 12 protons from the magnesium atom. There are 10 electrons because 12-2 = 10. There are 12 neutrons because 24-12 = 12.
    • >60Co
      • 27 protons, 33 neutrons, 27 electrons
        • The cobalt atom has 27 protons as seen in the periodic table. There are also 27 electrons because the charge is 0. There are 33 neutrons because 60-27 = 33.
    • 3H
      • 1 protons, 2 neutrons, 1 electrons
        • There is 1 proton because the element is hydrogen. There is 1 electron because the atom is neutral. There are 2 neutrons because 3-1 = 2.
    • 40Ar
      • 18 protons, 22 neutrons, 18 electrons
        • There are 18 protons from the argon element. There 18 electrons because it is neutral, and 22 neutrons because 40 - 18 = 22.
    • n
      • 0 protons, 1 neutrons, 0 electrons
        • This is a free neutron denoted by the lower case n.

    3. Given the following, identify the subatomic particles present. (The periodic table is required to solve these problems)

    • Charge +1, 3 protons, mass number 6.
      • 3 protons, 3 neutrons, 2 electrons
    • Charge -2, 8 neutrons, mass number 17.
      • 9 protons, 8 neutrons, 7 electrons
    • 26 protons, 20 neutrons.
      • 26 protons, 20 neutrons, 26 electrons
    • 28 protons, mass number 62.
      • 28 protons, 34 neutrons, 28 electrons
    • 5 electrons, mass number 10.
      • 5 protons, 5 neutrons, 5 electrons
    • Charge -1, 18 electrons, mass number 36.
      • 17 protons, 19 neutrons, 18 electrons

    4. Arrange the following lements in order of increasing (a) number of protons; (b) number of neutrons; (c) atomic mass.

    a) Na, Mn, Fe, Co, Cu, Br

    • Z=#protons;
    • Na: z=11; Mn: Z=25, given; Fe: Z=26, given; Co: Z=27; Cu: Z=29; Br: Z=35, given

    b) Na, Cu, Fe, Mn, Co, Br

    • A=#protons+#neutrons, so #n=A-#protons(Z);
    • Na: #n=23-11=12; Cu: #n=59-29=30; Fe: #n=56-26=30; Mn: #n=55-25=30; Co: #n=59-27=32; Br: #n=80-35=45

    Note: Cu, Fe, Mn are all equal in their number of neutrons, which is 30.

    c) Na, Mn, Fe, Co, Cu, Br

    • Na: 22.9898 amu; Mn: 54.9380 amu; Fe: 55.845 amu; Co: 58.9332 amu; Cu: 63.546 amu; Br: 79.904

    Note: This is the same order as the number of protons, because as Atomic Number(Z) increases so does Atomic Mass.

    5. Fill in the rest of the table:

    Atomic Number Mass Number Number of Protons Number of Neutrons Number of Electrons
    2 4 2 2 2
    11 23 11 12 11
    15 31 15 16 15
    37 85 37 48 37
    53 127 53 74 53

    Note: Atomic Number=Number of Protons=Number of Electrons and Mass Number=Number of Protons+Number of Neutrons

    Sub-Atomic Particles is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Jiaxu Wang.

    • Was this article helpful?