Subatomic Particles
•Download as PPT, PDF•
3 likes•3,023 views
This document summarizes key information about subatomic particles including protons, neutrons, electrons, isotopes, and ions. Protons have a positive charge and are found in the nucleus. Neutrons have no charge and are also found in the nucleus. Electrons have a negative charge and are found outside the nucleus. The number of protons determines the element. The number of neutrons can vary between isotopes of the same element. Isotopes are identified using hyphen or nuclear notation. To find the number of neutrons in an isotope, subtract the atomic number from the atomic mass. The number of electrons in a neutral atom equals the number of protons. Ions have a different number of electrons than
Report
Share
Report
Share
![Protons ,[object Object],[object Object],[object Object],[object Object]](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
Recommended
subatomic particles
Protons, neutrons, and electrons are the three main subatomic particles. Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The atomic number identifies the number of protons in an atom's nucleus, while atomic mass refers to the total number of protons and neutrons.
Atoms And Subatomic Particles
An atom is incredibly small, with its diameter needing to be increased 200 million times to equal the diameter of a penny. Atoms are made up of subatomic particles, including protons and neutrons in the central nucleus and electrons orbiting the nucleus. Most of an atom's mass comes from its nucleus. The number of protons determines the element and is called the atomic number. Isotopes are atoms of the same element that differ in their number of neutrons.
Atomicsstructure
- Atoms are the building blocks of matter and are made up of protons, neutrons, and electrons. The nucleus contains protons and neutrons and accounts for nearly all an atom's mass, while electrons orbit the nucleus.
- The number of protons determines the element and cannot be changed. Neutrons can vary between atoms of the same element, creating isotopes of that element.
- An atom's mass number is the total number of protons and neutrons, while its atomic mass refers to the average mass of all isotopes of that element as found in nature.
Atomic Structure Part 2
1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
2) Electrons are arranged in shells around the nucleus numbered 1, 2, 3, etc. The first shell can hold up to 2 electrons and subsequent shells can hold up to 8 electrons.
3) To find an element's electronic configuration, electrons are filled into the lowest available energy shell first.
Grade 9, U1-L9-Atomic structure
This document discusses the structure of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons surround the nucleus in energy levels. The number of protons determines the element and is known as the atomic number. The total number of protons and neutrons is the mass number. Standard atomic notation uses the mass number as a superscript on the left of the element symbol and the atomic number as a subscript.
Atomic structure
The document discusses the structure of atoms. It describes the historical understanding of atoms from Dalton's theory that atoms cannot be created or destroyed to Rutherford's discovery of the nucleus and Bohr's model of the atom. The key parts of an atom are protons, neutrons, and electrons. Protons are positively charged and located in the nucleus, electrons are negatively charged and orbit the nucleus, and neutrons have no charge and are also located in the nucleus. The number of protons defines the element. The total number of protons and neutrons is the nucleon number. Examples are provided to demonstrate how to calculate nucleon number from proton and neutron numbers.
The three subatomic particles
1) Michael Faraday discovered cathode rays (now known as electrons) in 1838 through experiments with glass tubes containing rarefied air and electrodes.
2) The experiment showed a strange luminous arc near the anode and a dark space near the cathode, marking the beginning of research into cathode rays.
3) Other scientists like J.J. Thomson, R.A. Millikan, and J. Chadwick later discovered the subatomic particles proton, electron, and neutron through discharge tube and oil drop experiments.
Inside the Atom~Notes
The document discusses the structure and composition of atoms. It can be summarized as follows:
1) Atoms have a small, dense nucleus containing protons and neutrons, surrounded by an electron cloud where electrons are found.
2) The number of protons determines the element, and protons plus neutrons equals the mass number. Electrons equal protons for neutral atoms.
3) Atoms can gain or lose electrons to become ions with a positive or negative charge.
4) Isotopes of the same element have different numbers of neutrons but the same number of protons.
Recommended
subatomic particles
Protons, neutrons, and electrons are the three main subatomic particles. Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The atomic number identifies the number of protons in an atom's nucleus, while atomic mass refers to the total number of protons and neutrons.
Atoms And Subatomic Particles
An atom is incredibly small, with its diameter needing to be increased 200 million times to equal the diameter of a penny. Atoms are made up of subatomic particles, including protons and neutrons in the central nucleus and electrons orbiting the nucleus. Most of an atom's mass comes from its nucleus. The number of protons determines the element and is called the atomic number. Isotopes are atoms of the same element that differ in their number of neutrons.
Atomicsstructure
- Atoms are the building blocks of matter and are made up of protons, neutrons, and electrons. The nucleus contains protons and neutrons and accounts for nearly all an atom's mass, while electrons orbit the nucleus.
- The number of protons determines the element and cannot be changed. Neutrons can vary between atoms of the same element, creating isotopes of that element.
- An atom's mass number is the total number of protons and neutrons, while its atomic mass refers to the average mass of all isotopes of that element as found in nature.
Atomic Structure Part 2
1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
2) Electrons are arranged in shells around the nucleus numbered 1, 2, 3, etc. The first shell can hold up to 2 electrons and subsequent shells can hold up to 8 electrons.
3) To find an element's electronic configuration, electrons are filled into the lowest available energy shell first.
Grade 9, U1-L9-Atomic structure
This document discusses the structure of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons surround the nucleus in energy levels. The number of protons determines the element and is known as the atomic number. The total number of protons and neutrons is the mass number. Standard atomic notation uses the mass number as a superscript on the left of the element symbol and the atomic number as a subscript.
Atomic structure
The document discusses the structure of atoms. It describes the historical understanding of atoms from Dalton's theory that atoms cannot be created or destroyed to Rutherford's discovery of the nucleus and Bohr's model of the atom. The key parts of an atom are protons, neutrons, and electrons. Protons are positively charged and located in the nucleus, electrons are negatively charged and orbit the nucleus, and neutrons have no charge and are also located in the nucleus. The number of protons defines the element. The total number of protons and neutrons is the nucleon number. Examples are provided to demonstrate how to calculate nucleon number from proton and neutron numbers.
The three subatomic particles
1) Michael Faraday discovered cathode rays (now known as electrons) in 1838 through experiments with glass tubes containing rarefied air and electrodes.
2) The experiment showed a strange luminous arc near the anode and a dark space near the cathode, marking the beginning of research into cathode rays.
3) Other scientists like J.J. Thomson, R.A. Millikan, and J. Chadwick later discovered the subatomic particles proton, electron, and neutron through discharge tube and oil drop experiments.
Inside the Atom~Notes
The document discusses the structure and composition of atoms. It can be summarized as follows:
1) Atoms have a small, dense nucleus containing protons and neutrons, surrounded by an electron cloud where electrons are found.
2) The number of protons determines the element, and protons plus neutrons equals the mass number. Electrons equal protons for neutral atoms.
3) Atoms can gain or lose electrons to become ions with a positive or negative charge.
4) Isotopes of the same element have different numbers of neutrons but the same number of protons.
Struture of an atom
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
Atomic Structure
All substances are made of atoms, which contain a nucleus of protons and neutrons surrounded by electrons. The periodic table organizes the over 100 known elements based on their atomic structure, including the number of protons (atomic number) and total protons and neutrons (mass number). Atoms of the same element can differ in number of neutrons, making them isotopes with the same atomic number but different mass numbers. Electrons occupy specific energy levels around the nucleus according to rules.
Elements, compounds, molecules and subatomic particles
This document defines and describes the basic concepts of elements, compounds, molecules, and subatomic particles. It states that elements are substances made of atoms with the same number of protons, while compounds contain atoms of different elements chemically combined in fixed ratios. Molecules are the smallest units that retain a compound's characteristics. The three main subatomic particles are protons, neutrons, and electrons, which make up atoms. The document also provides examples and properties of these scientific terms.
Atomic structure part 1 fundamental particles
Atoms are composed of protons, neutrons, and electrons. Protons and neutrons have mass while electrons have negligible mass. The number of protons is the atomic number and the total number of protons and neutrons is the mass number. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same atomic number and chemical properties. Examples provided are the isotopes of carbon, chlorine, and their atomic and mass numbers.
Structure Of Atoms Part 3
The document discusses atomic structure and ions. It defines isotopes as atoms of the same element with different numbers of neutrons. The outermost electrons of an atom are involved in chemical reactions. The periodic table arranges elements by their number of outermost electrons. Noble gases have full outermost shells with 2 or 8 electrons. Atoms form ions by gaining or losing electrons to achieve stable configurations. Positively charged ions are formed when electrons are lost, and negatively charged ions are formed when electrons are gained.
Isotopes
This document discusses isotopes and atomic structure. It defines isotopes as atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes have the same chemical properties but slightly different physical properties. The document also discusses nucleon number, which is the total number of protons and neutrons in an atom's nucleus. The mass number equals the nucleon number. Radioactive isotopes are unstable and undergo nuclear decay over time into stable daughter isotopes.
Atom Structure Notes
An atom is the smallest particle of an element that retains the properties of that element. Atoms consist of protons and neutrons in the nucleus, and electrons orbiting the nucleus. The number of protons determines the element, while the total number of protons and neutrons determines the isotope. Atoms bond by sharing or transferring electrons to fill their outer electron shells and become stable.
What is atom
What is Atom in Chemistry ?
Atom is basic building block of all matter.
Atom Have
1. Nucleus
Nucleus is very small and heavy part of the atom.
2. An Surrounding Electron Cloud
Surrounding electron cloud is large and lightweight part of the atom.
Nucleus of an Atom
Nucleus Contains
Protons
Protons have a positive charge.
All atoms are distinguished by the number of protons it has (atomic number).
Neutrons
Neutrons have no charge.
Neutrons have same mass as protons.
Electron Cloud of an Atom
An Electron Cloud of an Atom Contains
Electrons
Electron have a negative charge.
Electrons are contained within the shells of electron cloud.
Electrons have very small mass as compared to neutrons and protons.
Electron move in orbital motion around nucleus.
Electrons decides how bonds formed.
Atomic Structure
Atom is made up of Nucleus (Protons and Neutrons) and Electrons.
Prepared and Published by-
http://www.ChemistryNotesInfo.com
http://www.ChemistryNotesInfo.Blogspot.com
Read full article on what is Atom in chemistry at
https://chemistrynotesinfo.com/what-is-an-atom/
and view video of Atom at https://youtu.be/5Sdo7VKJ1uk
Ps ch 3_presentation
This document provides an overview of atomic structure and the periodic table. It defines protons, neutrons, and electrons, and describes early atomic models including the Bohr model. It introduces electron orbitals and explains how they relate to an element's valence electrons and position on the periodic table. The document then explores periodic trends in atomic properties, including metals, nonmetals, and noble gases. It defines ions, isotopes, and molar mass, and discusses using moles as a unit for counting particles.
Atoms
PowerPoint describing the basic structure of atoms. Geared toward Middle School science and technology classes.
08 inside the atom
1) Atoms are the smallest particle of an element that retains the properties of that element.
2) Atoms consist of electrons that orbit a nucleus, which contains protons and neutrons.
3) Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons defines the element.
4) Atoms are electrically neutral when they contain an equal number of protons and electrons. Ions are formed when atoms gain or lose electrons.
Inside the atom presentation by loida
The document provides information about the structure of atoms, including:
1) The three main subatomic particles that make up atoms are protons, neutrons, and electrons.
2) Isotopes are atoms of the same element that differ in their number of neutrons.
3) The atomic number identifies the number of protons in an atom, while the mass number provides the total number of protons and neutrons.
Atomic Structure Review
This document provides a review of key concepts in atomic structure:
1) Protons have a positive charge and determine the atomic number, neutrons have no charge and determine isotope variations, electrons have a negative charge and determine ion charge state.
2) Atomic mass is the total number of protons and neutrons, while the atomic number indicates just the number of protons. Neutrons can be calculated by subtracting the atomic number from atomic mass.
3) Elements are arranged on the periodic table by atomic number, which identifies each unique atom, while isotopes of an element can vary in neutron number.
The Atom
The document defines key atomic terms like atom, nucleus, protons, neutrons, and electrons. It describes how atoms are made up of a tiny nucleus surrounded by an electron cloud. Atoms of the same element have the same number of protons. The number of neutrons and electrons can vary. The periodic table arranges elements in periods and groups based on their atomic structure and number of valence electrons.
Atomic number and mass number
This document provides information about atomic structure, including the three main subatomic particles - protons, neutrons, and electrons. It discusses the key properties of each particle, including their location within the atom, mass, and electrical charge. Protons determine the element and have a positive charge. Neutrons are neutral and have a similar mass to protons. The number of protons and neutrons gives an atom its identity and mass number.
Structure of atoms10
Scientists have been studying atoms since the 1800s using models to understand their structure and behavior. Early philosophers proposed the idea of atoms, while scientists like Dalton, Thomson, Rutherford, and Bohr developed atomic models through experiments. They discovered that atoms are mostly empty space with a small, dense nucleus at the center containing protons and neutrons, and electrons orbiting the nucleus. The number of protons determines the element, while isotopes of an element have different numbers of neutrons.
Atoms and the periodic table
The document discusses atoms and the periodic table. It describes atoms as being made up of protons, neutrons, and electrons. Elements are organized on the periodic table based on their atomic structure. Atoms are designated a symbol and atomic mass, which is the average mass of its isotopes. Isotopes are variants of the same element that have a different number of neutrons. The mass number of an isotope is the total protons and neutrons. Ions are formed when atoms gain or lose electrons, becoming positively or negatively charged.
Atom inside out
This document provides an overview of the history and development of the atomic theory. It discusses early Greek philosophers like Democritus who proposed that all matter is composed of indivisible atoms. Later, scientists like John Dalton developed atomic theory further by proposing that atoms are tiny, indivisible particles that combine to form all substances. The document then outlines evidence for subatomic particles like J.J. Thomson's discovery of electrons and Rutherford's discovery of the nucleus. It defines key subatomic particles like protons, neutrons, and electrons and how they combine to form different atoms and isotopes.
3.2 structure of atoms
- Thompson discovered electrons using cathode ray tubes. Rutherford discovered the nucleus and that it is positively charged through gold foil experiments.
- Chadwick discovered neutrons by observing particles in a beam that were not deflected by a magnetic field.
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit the nucleus. The number of protons defines the element.
4.2 Notes
The document discusses the structure of atoms and properties of subatomic particles. It defines protons, neutrons, and electrons, noting their charges and locations. It explains that the atomic number is the number of protons and determines the element, while the mass number is the total of protons and neutrons. Isotopes are defined as atoms of the same element that have different numbers of neutrons and mass numbers.
Naresh
The periodic table arranges elements in order of increasing atomic number and groups elements with similar chemical properties together. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties. Atoms are made up of protons and neutrons in the nucleus and electrons in energy levels outside the nucleus. Atoms are neutral when they have an equal number of protons and electrons. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different atomic masses. An element's relative atomic mass takes into account the abundance of each isotope.
Naresh Periodic Table
The periodic table arranges elements in order of increasing atomic number and groups elements with similar chemical properties together. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties. Atoms are made up of protons and neutrons in the nucleus and electrons in energy levels outside the nucleus. Atoms are neutral when they have an equal number of protons and electrons. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different atomic masses. An element's relative atomic mass is averaged from the masses of its naturally occurring isotopes.
More Related Content
What's hot
Struture of an atom
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
Atomic Structure
All substances are made of atoms, which contain a nucleus of protons and neutrons surrounded by electrons. The periodic table organizes the over 100 known elements based on their atomic structure, including the number of protons (atomic number) and total protons and neutrons (mass number). Atoms of the same element can differ in number of neutrons, making them isotopes with the same atomic number but different mass numbers. Electrons occupy specific energy levels around the nucleus according to rules.
Elements, compounds, molecules and subatomic particles
This document defines and describes the basic concepts of elements, compounds, molecules, and subatomic particles. It states that elements are substances made of atoms with the same number of protons, while compounds contain atoms of different elements chemically combined in fixed ratios. Molecules are the smallest units that retain a compound's characteristics. The three main subatomic particles are protons, neutrons, and electrons, which make up atoms. The document also provides examples and properties of these scientific terms.
Atomic structure part 1 fundamental particles
Atoms are composed of protons, neutrons, and electrons. Protons and neutrons have mass while electrons have negligible mass. The number of protons is the atomic number and the total number of protons and neutrons is the mass number. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same atomic number and chemical properties. Examples provided are the isotopes of carbon, chlorine, and their atomic and mass numbers.
Structure Of Atoms Part 3
The document discusses atomic structure and ions. It defines isotopes as atoms of the same element with different numbers of neutrons. The outermost electrons of an atom are involved in chemical reactions. The periodic table arranges elements by their number of outermost electrons. Noble gases have full outermost shells with 2 or 8 electrons. Atoms form ions by gaining or losing electrons to achieve stable configurations. Positively charged ions are formed when electrons are lost, and negatively charged ions are formed when electrons are gained.
Isotopes
This document discusses isotopes and atomic structure. It defines isotopes as atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes have the same chemical properties but slightly different physical properties. The document also discusses nucleon number, which is the total number of protons and neutrons in an atom's nucleus. The mass number equals the nucleon number. Radioactive isotopes are unstable and undergo nuclear decay over time into stable daughter isotopes.
Atom Structure Notes
An atom is the smallest particle of an element that retains the properties of that element. Atoms consist of protons and neutrons in the nucleus, and electrons orbiting the nucleus. The number of protons determines the element, while the total number of protons and neutrons determines the isotope. Atoms bond by sharing or transferring electrons to fill their outer electron shells and become stable.
What is atom
What is Atom in Chemistry ?
Atom is basic building block of all matter.
Atom Have
1. Nucleus
Nucleus is very small and heavy part of the atom.
2. An Surrounding Electron Cloud
Surrounding electron cloud is large and lightweight part of the atom.
Nucleus of an Atom
Nucleus Contains
Protons
Protons have a positive charge.
All atoms are distinguished by the number of protons it has (atomic number).
Neutrons
Neutrons have no charge.
Neutrons have same mass as protons.
Electron Cloud of an Atom
An Electron Cloud of an Atom Contains
Electrons
Electron have a negative charge.
Electrons are contained within the shells of electron cloud.
Electrons have very small mass as compared to neutrons and protons.
Electron move in orbital motion around nucleus.
Electrons decides how bonds formed.
Atomic Structure
Atom is made up of Nucleus (Protons and Neutrons) and Electrons.
Prepared and Published by-
http://www.ChemistryNotesInfo.com
http://www.ChemistryNotesInfo.Blogspot.com
Read full article on what is Atom in chemistry at
https://chemistrynotesinfo.com/what-is-an-atom/
and view video of Atom at https://youtu.be/5Sdo7VKJ1uk
Ps ch 3_presentation
This document provides an overview of atomic structure and the periodic table. It defines protons, neutrons, and electrons, and describes early atomic models including the Bohr model. It introduces electron orbitals and explains how they relate to an element's valence electrons and position on the periodic table. The document then explores periodic trends in atomic properties, including metals, nonmetals, and noble gases. It defines ions, isotopes, and molar mass, and discusses using moles as a unit for counting particles.
Atoms
PowerPoint describing the basic structure of atoms. Geared toward Middle School science and technology classes.
08 inside the atom
1) Atoms are the smallest particle of an element that retains the properties of that element.
2) Atoms consist of electrons that orbit a nucleus, which contains protons and neutrons.
3) Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons defines the element.
4) Atoms are electrically neutral when they contain an equal number of protons and electrons. Ions are formed when atoms gain or lose electrons.
Inside the atom presentation by loida
The document provides information about the structure of atoms, including:
1) The three main subatomic particles that make up atoms are protons, neutrons, and electrons.
2) Isotopes are atoms of the same element that differ in their number of neutrons.
3) The atomic number identifies the number of protons in an atom, while the mass number provides the total number of protons and neutrons.
Atomic Structure Review
This document provides a review of key concepts in atomic structure:
1) Protons have a positive charge and determine the atomic number, neutrons have no charge and determine isotope variations, electrons have a negative charge and determine ion charge state.
2) Atomic mass is the total number of protons and neutrons, while the atomic number indicates just the number of protons. Neutrons can be calculated by subtracting the atomic number from atomic mass.
3) Elements are arranged on the periodic table by atomic number, which identifies each unique atom, while isotopes of an element can vary in neutron number.
The Atom
The document defines key atomic terms like atom, nucleus, protons, neutrons, and electrons. It describes how atoms are made up of a tiny nucleus surrounded by an electron cloud. Atoms of the same element have the same number of protons. The number of neutrons and electrons can vary. The periodic table arranges elements in periods and groups based on their atomic structure and number of valence electrons.
Atomic number and mass number
This document provides information about atomic structure, including the three main subatomic particles - protons, neutrons, and electrons. It discusses the key properties of each particle, including their location within the atom, mass, and electrical charge. Protons determine the element and have a positive charge. Neutrons are neutral and have a similar mass to protons. The number of protons and neutrons gives an atom its identity and mass number.
Structure of atoms10
Scientists have been studying atoms since the 1800s using models to understand their structure and behavior. Early philosophers proposed the idea of atoms, while scientists like Dalton, Thomson, Rutherford, and Bohr developed atomic models through experiments. They discovered that atoms are mostly empty space with a small, dense nucleus at the center containing protons and neutrons, and electrons orbiting the nucleus. The number of protons determines the element, while isotopes of an element have different numbers of neutrons.
Atoms and the periodic table
The document discusses atoms and the periodic table. It describes atoms as being made up of protons, neutrons, and electrons. Elements are organized on the periodic table based on their atomic structure. Atoms are designated a symbol and atomic mass, which is the average mass of its isotopes. Isotopes are variants of the same element that have a different number of neutrons. The mass number of an isotope is the total protons and neutrons. Ions are formed when atoms gain or lose electrons, becoming positively or negatively charged.
Atom inside out
This document provides an overview of the history and development of the atomic theory. It discusses early Greek philosophers like Democritus who proposed that all matter is composed of indivisible atoms. Later, scientists like John Dalton developed atomic theory further by proposing that atoms are tiny, indivisible particles that combine to form all substances. The document then outlines evidence for subatomic particles like J.J. Thomson's discovery of electrons and Rutherford's discovery of the nucleus. It defines key subatomic particles like protons, neutrons, and electrons and how they combine to form different atoms and isotopes.
3.2 structure of atoms
- Thompson discovered electrons using cathode ray tubes. Rutherford discovered the nucleus and that it is positively charged through gold foil experiments.
- Chadwick discovered neutrons by observing particles in a beam that were not deflected by a magnetic field.
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit the nucleus. The number of protons defines the element.
4.2 Notes
The document discusses the structure of atoms and properties of subatomic particles. It defines protons, neutrons, and electrons, noting their charges and locations. It explains that the atomic number is the number of protons and determines the element, while the mass number is the total of protons and neutrons. Isotopes are defined as atoms of the same element that have different numbers of neutrons and mass numbers.
What's hot (20)
Elements, compounds, molecules and subatomic particles
Elements, compounds, molecules and subatomic particles
Similar to Subatomic Particles
Naresh
The periodic table arranges elements in order of increasing atomic number and groups elements with similar chemical properties together. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties. Atoms are made up of protons and neutrons in the nucleus and electrons in energy levels outside the nucleus. Atoms are neutral when they have an equal number of protons and electrons. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different atomic masses. An element's relative atomic mass takes into account the abundance of each isotope.
Naresh Periodic Table
The periodic table arranges elements in order of increasing atomic number and groups elements with similar chemical properties together. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties. Atoms are made up of protons and neutrons in the nucleus and electrons in energy levels outside the nucleus. Atoms are neutral when they have an equal number of protons and electrons. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different atomic masses. An element's relative atomic mass is averaged from the masses of its naturally occurring isotopes.
Atomic Theory
The document discusses atomic theory and the structure of atoms. It explains that all matter is made up of atoms, which are the smallest particles of elements that can exist. Atoms consist of a nucleus containing protons and neutrons, surrounded by electrons. The number of protons determines the element, while the number of neutrons can vary between isotopes of the same element. Chemical bonds form when atoms share or transfer electrons to fill their valence shells. This allows the formation of compounds with properties different from their constituent elements.
Mod+13,+Atomic+Structure+Part+B
Each element is unique due to its atomic structure. Atoms consist of protons and neutrons located in the nucleus, and electrons outside the nucleus. The number of protons determines the element, while the total of protons and neutrons is the mass number. Isotopes are atoms of the same element with different numbers of neutrons.
Ch 4 l 3 how atoms differ
The document discusses the differences between elements, isotopes, and ions at the atomic level. Elements are defined by their atomic number, or number of protons. Isotopes are atoms of the same element that have different numbers of neutrons. Ions are atoms that have gained or lost electrons, giving them a positive or negative charge. The periodic table organizes elements by their atomic number and provides other atomic information. Atoms of the same element can have different isotopes depending on their number of neutrons. Atoms can also form ions by gaining or losing electrons.
Topic 1.2 atoms
The document discusses atoms and their structure. It explains that atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons orbit around the nucleus in energy levels. The document also notes that atoms are very small, around 0.00000001mm in diameter, and discusses how scientists have worked to discover the structure of atoms over time.
Ch 5 Notes
This document provides an overview of elements, atoms, ions, isotopes, and the periodic table. It defines elements as pure substances that cannot be broken down further. Atoms are the smallest particles that retain an element's chemical properties and consist of protons, neutrons, and electrons. Ions are atoms or groups of atoms with a positive or negative charge formed by gaining or losing electrons. Isotopes are atoms of the same element with different numbers of neutrons. The periodic table organizes the elements and provides their properties based on their atomic structure.
Tro3 lecture 04
The document summarizes key concepts from Chapter 4 of Nivaldo Tro's "Introductory Chemistry" textbook, including:
1) John Dalton proposed atoms as tiny, indivisible particles that combine in whole number ratios to form compounds.
2) Atoms are composed of protons, neutrons, and electrons, with protons and electrons determining an element's identity and charge.
3) Elements are arranged on the periodic table based on their atomic number, which is the number of protons in the nucleus.
Physics 22 - The Nuclear Atom.pptx
1) Atoms consist of a small, dense nucleus surrounded by electrons. The nucleus contains positively charged protons and neutral neutrons, while electrons are negatively charged and orbit the nucleus.
2) The number of protons determines the element and is known as the atomic number. The total number of protons and neutrons is the mass number. Isotopes are atoms of the same element with different numbers of neutrons.
3) Evidence for the nuclear model includes Rutherford's gold foil experiment, which showed that most alpha particles passed through but some were deflected at large angles, indicating a small, dense nucleus.
Atomic structure
The document discusses the history and development of atomic structure and models. It describes J.J. Thomson's discovery of the electron using cathode ray tubes in 1897. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense, positively charged nucleus. The key parts of an atom - protons, neutrons, electrons - and their roles are defined. Atomic number identifies the number of protons in an element, and mass number identifies the total protons and neutrons in an isotope.
11/16/11
The charge of the ion is indicated
by the superscript number after the element
symbol. A positive number means the atom
lost electrons and is positively charged. A
negative number means the atom gained
electrons and is negatively charged.
Model: Na+ Ion
Sodium ion (Na) that lost 1 electron
Charge: +1
Protons: 11
Electrons: 10
Neutrons: 12
Mass: 22.9898
Model this ion in your notebook!
Model: Cl- Ion
Chlorine ion (Cl) that gained 1 electron
Charge: -1
Protons: 17
Electrons: 18
Neutrons: 18
Review questions: atoms, periodic table, chemical bonds
The document provides an overview of key concepts in atomic structure and chemical bonding. It defines the electron cloud model and notes electrons are found in energy levels around the nucleus. The nucleus contains protons and neutrons, which are similar in size. An element is defined by its atomic number, while isotopes have different numbers of neutrons. Atoms form ionic bonds by gaining or losing electrons or covalent bonds by sharing electrons. Metals bond through metallic bonds and are found on the left side of the periodic table, while nonmetals are on the right and form ionic or covalent bonds.
Chemistry
1) There are 118 known chemical elements, of which 94 occur naturally on Earth. Elements are distinguished by their atomic number, which is the number of protons in the nucleus. Elements can have different isotopes that vary in the number of neutrons.
2) Elements up to iron are formed through nuclear fusion in stars, while heavier elements are formed in supernova explosions. Elements are categorized based on their general physical and chemical properties, states of matter, melting/boiling points, and densities.
3) The periodic table organizes the elements based on their atomic structure and recurring trends in chemical properties. Elements can exist in multiple structural forms known as allotropes.
Chapter 6.1
The document discusses the fundamental particles and forces that make up atoms. It describes how atoms were discovered to be made up of even smaller particles, including electrons discovered by J.J. Thomson and the nuclear model developed by Rutherford based on experiments by Rutherford, Geiger, and Marsden. The document also discusses the three main subatomic particles (protons, neutrons, and electrons), isotopes, radioactive decay, and the four main forces (electromagnetic, strong nuclear, weak, and gravity) that act inside atoms.
How many electrons?
The document discusses isotopes, ions, atomic numbers, and atomic masses. It defines isotopes as atoms of the same element that have varying numbers of neutrons. It notes that ions are atoms with unequal numbers of protons and electrons, making them positively or negatively charged. For neutral atoms, the number of protons equals the number of electrons and is equal to the atomic number. The document also provides examples of calculating the number of protons, neutrons, and electrons for different atoms and ions.
Chapter 4 atomic structure
This document summarizes key concepts from Chapter 4 on atomic structure:
1) It describes early atomic theories from Democritus and Dalton, including Dalton's postulates that atoms are indivisible and atoms of different elements have different properties.
2) Modern research has shown atoms are composed of subatomic particles like electrons, protons, and neutrons. Experiments by Thomson, Millikan, Rutherford and others led to discoveries about these particles and the nuclear model of the atom.
3) Isotopes are atoms of the same element that differ in number of neutrons. Atomic mass is an average that takes isotopic abundance into account. The periodic table organizes elements based on repeating atomic properties.
Structure of Atom CBSE Class 9 PPT-2.pptx
This document provides information about the structure of atoms, including:
1. Neutrons are subatomic particles found in atomic nuclei except hydrogen.
2. Electrons fill atomic shells in a step-wise manner according to the 2n^2 rule.
3. An atom's valency is determined by the number of electrons it gains, loses, or shares to achieve an octet in its outer shell.
1c. Isotopes, Ram, Qs
The document discusses isotopes and radioactive decay. It defines isotopes as atoms of the same element that have different numbers of neutrons. Three main types of nuclear radiation are described: alpha particles, beta particles, and gamma rays. Alpha particles have a +2 charge and consist of 2 protons and 2 neutrons. Beta particles are high-speed electrons. Gamma rays are highly energetic photons. Nuclear equations are provided to summarize alpha and beta decay, showing how the atom changes during radioactive decay.
Atomic structure
The document discusses atomic structure and the key parts of an atom: protons, neutrons, and electrons. It explains that protons are found in the nucleus and give an atom its atomic number. The number of protons never changes for a given element. It also defines atomic number as the number of protons and mass number as the total number of protons and neutrons in an atom's nucleus.
Chemical Reactions
Here are cutouts of magnesium and chlorine atoms:
Mg-24 atom:
Nucleus: 12 protons, 12 neutrons
Electrons: 12
Cl-35 atom:
Nucleus: 17 protons, 18 neutrons
Electrons: 17
To form an ionic bond:
- Mg loses 2 electrons to have a full outer shell of 8
- Cl gains 1 electron to have a full outer shell of 8
The ratio of Mg to Cl atoms that would result in a neutral compound is 1:1.
The name of the ionic compound is magnesium chloride.
The chemical symbol is MgCl2.
Similar to Subatomic Particles (20)
Review questions: atoms, periodic table, chemical bonds
Review questions: atoms, periodic table, chemical bonds
More from lallen
Solutions, Molarity, Molality
This document provides information on various concepts related to solutions including vocabulary terms, molarity, molality, and percent composition. For molarity, it defines the term, provides examples of how to calculate molarity given different variables, and discusses dilution problems. For molality, it notes some of the challenges in calculating molality for hydrated solutes. It also defines percent composition and provides sample problems calculating density, molality and molarity for different solutions.
Deriving the ideal gas law
This document summarizes key points from Chapter 11 of Holt Modern Chemistry regarding Avogadro's law and relating the volume and number of moles of gases. It provides an example problem of calculating the number of moles of gas in 46.5 liters at 28°C and 2.75 atm by converting to STP conditions. The document notes how the combined gas law can be used to convert volumes to moles using the definition that 1 mole of any gas at STP occupies 22.414 liters. It also suggests developing a conversion factor or "multiplier" to more directly calculate moles without intermediate steps. Finally, it directs the reader to practice problems #40-52 at the end of chapter 11.
Intro to kinetics
This document summarizes key concepts from Chapter 12 of Zumdahl's textbook on kinetics. It begins by identifying the chapter objectives, which include determining factors that influence reaction rates, writing rate laws, calculating rate constants, and determining reaction order and half-life. It then discusses specific examples to illustrate these concepts, such as using data on initial concentrations and rates to determine that the reaction 2NO2 → 2NO + O2 is first order. It also explains how to use integrated rate laws to determine concentrations over time for first and second order reactions from graphs of natural log of concentration versus time and inverse concentration versus time, respectively. The document emphasizes that reaction order must be established before applying integrated rate laws. Finally, it notes
Naming covalent compounds and acids
This document provides information on naming covalent compounds and acids. It discusses how to identify covalent compounds based on their composition and discusses prefixes used in naming them such as mono, di, and tri. Rules are provided for determining the order and modified ending of elements in covalent compound names. Examples of naming covalent compounds like CO, P2O5, and H2O are also provided. The document also discusses naming acids based on whether they contain halides, -ates, or -ites and the number of hydrogens added to match charge. It concludes with a comparison of naming conventions for ionic compounds, covalent compounds, and acids.
Acid rain pp
The document discusses acid rain, including its causes, effects, and how to simulate its effects in a lab experiment. It explains that acid rain is caused by sulfur dioxide and nitrogen oxide emissions from industrial activities and vehicles. Acid rain damages buildings, statues, and the environment by corroding materials and lowering the pH of lakes and streams. The lab experiment will test the resistance of quartz, marble, and granite to simulated acid rain using vinegar to see which material is least affected.
Solutions2010
This document provides an overview of concepts related to solutions and solubility, including:
1) Key terms like solvent, solute, concentration, and their relationships as demonstrated through examples of dissolving salt in water.
2) How temperature and concentration affect solubility, and how to read solubility curves. Exothermic and endothermic processes are discussed in relation to enthalpy of solution.
3) Molarity calculations including determining molarity from mass, calculating moles from molarity and volume, and dilution. Net ionic equations and solubility rules are also covered.
4) Colligative properties like boiling point elevation and freezing point depression are explained in terms of vapor pressure
Kinetic Molecular theory
Simple introduction to KMT, related to properties of gases, liquids, and solids. Intro to the concept of an ideal gas.
Naming Compounds
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
Attractions Between Particles
This document summarizes different types of chemical bonds: covalent bonds formed by shared electrons between similar atoms, ionic bonds formed by attractions between oppositely charged ions, and metallic bonds formed when atoms share a "sea of electrons". It also discusses polar covalent bonds that occur between atoms with some difference in electronegativity, and intermolecular forces like hydrogen bonding and London dispersion forces. Key terms like crystal lattice, formula unit, and lattice energy are defined in the context of ionic bonds.
The Periodic Table
The document summarizes a presentation about the periodic table given by Lisa Allen at Stonington High School. It discusses the early development of the periodic table by scientists like Cannizzaro, Mendeleev, and others. Mendeleev was able to organize the elements into the first recognizable periodic table based on their atomic masses and chemical properties. He even predicted the properties of yet-to-be discovered elements. The document then outlines assignments for students to create their own periodic tables and presentations on periodic properties.
Quantum Theory
The document discusses the early history and development of quantum theory, beginning with Max Planck's hypothesis that energy exists in discrete packets called quanta. It describes how this helped explain phenomena like the photoelectric effect. The document also summarizes Niels Bohr's early model of the hydrogen atom and its limitations, leading to developments like Louis de Broglie's proposal that electrons have wave-like properties and Werner Heisenberg's uncertainty principle.
Chapter 3 Dalton
1) In the late 1700s, new scientific ideas and improved technology allowed for better understanding of chemistry through experimentation and data collection. Laws of chemistry like conservation of mass and definite proportions were discovered.
2) In 1808, John Dalton developed an atomic theory to explain the laws of chemistry, proposing that all matter is made of tiny indivisible particles called atoms. Atoms of each element are unique and combine in simple whole number ratios to form compounds.
3) Dalton's atomic theory accounted well for the known laws of chemistry and provided a rational scientific explanation for chemical reactions and compositions. While some details were later updated, Dalton's core ideas formed the basis of modern atomic
More from lallen (13)
Recently uploaded
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective UpskillingExcellence Foundation for South Sudan
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.The Diamonds of 2023-2024 in the IGRA collection
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
বিসিএস ও ব্যাংক এর লিখিত পরীক্ষা ...+এছাড়া মাধ্যমিক ও উচ্চমাধ্যমিকের স্টুডেন্টদের জন্য অনেক কাজে আসবে ...
The History of Stoke Newington Street Names
Presented at the Stoke Newington Literary Festival on 9th June 2024
www.StokeNewingtonHistory.com
RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
RPMS Template 2023-2024 by: Irene S. Rueco
PCOS corelations and management through Ayurveda.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
Introduction to AI for Nonprofits with Tapp Network
Dive into the world of AI! Experts Jon Hill and Tareq Monaur will guide you through AI's role in enhancing nonprofit websites and basic marketing strategies, making it easy to understand and apply.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
-------------------------------------------------------------------------------
Find out more about ISO training and certification services
Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
-------------------------------------------------------------------------------
For more information about PECB:
Website: https://pecb.com/
LinkedIn: https://www.linkedin.com/company/pecb/
Facebook: https://www.facebook.com/PECBInternational/
Slideshare: http://www.slideshare.net/PECBCERTIFICATION
Hindi varnamala | hindi alphabet PPT.pdf
हिंदी वर्णमाला पीपीटी, hindi alphabet PPT presentation, hindi varnamala PPT, Hindi Varnamala pdf, हिंदी स्वर, हिंदी व्यंजन, sikhiye hindi varnmala, dr. mulla adam ali, hindi language and literature, hindi alphabet with drawing, hindi alphabet pdf, hindi varnamala for childrens, hindi language, hindi varnamala practice for kids, https://www.drmullaadamali.com
A Survey of Techniques for Maximizing LLM Performance.pptx
A Survey of Techniques for Maximizing LLM Performance
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...National Information Standards Organization (NISO)
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.Types of Herbal Cosmetics its standardization.
Physiology and chemistry of skin and pigmentation, hairs, scalp, lips and nail, Cleansing cream, Lotions, Face powders, Face packs, Lipsticks, Bath products, soaps and baby product,
Preparation and standardization of the following : Tonic, Bleaches, Dentifrices and Mouth washes & Tooth Pastes, Cosmetics for Nails.
Assessment and Planning in Educational technology.pptx
In an education system, it is understood that assessment is only for the students, but on the other hand, the Assessment of teachers is also an important aspect of the education system that ensures teachers are providing high-quality instruction to students. The assessment process can be used to provide feedback and support for professional development, to inform decisions about teacher retention or promotion, or to evaluate teacher effectiveness for accountability purposes.
Main Java[All of the Base Concepts}.docx
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
CACJapan - GROUP Presentation 1- Wk 4.pdf
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
Top five deadliest dog breeds in America
Thinking of getting a dog? Be aware that breeds like Pit Bulls, Rottweilers, and German Shepherds can be loyal and dangerous. Proper training and socialization are crucial to preventing aggressive behaviors. Ensure safety by understanding their needs and always supervising interactions. Stay safe, and enjoy your furry friends!
Recently uploaded (20)
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective Upskilling
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
Introduction to AI for Nonprofits with Tapp Network
Introduction to AI for Nonprofits with Tapp Network
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
A Survey of Techniques for Maximizing LLM Performance.pptx
A Survey of Techniques for Maximizing LLM Performance.pptx
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Assessment and Planning in Educational technology.pptx
Assessment and Planning in Educational technology.pptx
Subatomic Particles
- 1. Subatomic Particles Names, Properties, and Locations Atomic mass and isotopic mass Ions by Lisa Allen
- 8. Electrons Negative Charge Found in energy levels outside the nucleus Mass of 1/1836 AMU (almost nothing!) The number of electrons in a neutral atom is equal to the number of protons. The number of electrons in an ion is different from the number of protons .