Atom structure
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This document discusses atomic structure and properties. It defines: - Atoms consist of a nucleus with protons and neutrons, and electrons orbiting the nucleus. - The atomic number is the number of protons, which identifies an element and its position on the periodic table. - Neutrons have no charge and contribute to an atom's mass. - The mass number is the total number of protons and neutrons, and provides an indication of an atom's mass.
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Structure of atom
This document discusses the particulate nature of matter. It explains that matter is made up of particles including atoms, molecules, and ions. Atoms are the smallest particle of an element, molecules contain two or more bonded atoms, and ions are charged particles formed in liquids or molten states. The document then discusses the kinetic theory of matter and how particle behavior differs between solids, liquids, and gases. It also summarizes the early models of the atomic structure proposed by scientists like Dalton, Thomson, Rutherford, and Bohr. Finally, it defines key atomic concepts like protons, neutrons, isotopes, and their uses.
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.
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.
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- Dalton's model proposed that all matter is made of tiny particles called atoms, all atoms of the same element are alike but different from other elements, and compounds form from atoms combining in fixed proportions. Thomson's model pictured the atom as a positively charged sphere with electrons embedded within it. Rutherford's model showed that the atom's positive charge and most of its mass are concentrated in a tiny, dense nucleus at the center with electrons orbiting outside. The parts of an atom include the nucleus containing protons and neutrons at its center, surrounded by electrons. Protons have a positive charge while neutrons have no charge. Electrons have a negative charge and much less mass than protons or neutrons.
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Atoms are the basic building blocks of all matter and are made up of a nucleus containing protons and neutrons surrounded by electrons. John Dalton's atomic theory established that atoms are indivisible and that different elements are composed of different types of atoms. Rutherford discovered that the nucleus contains a concentrated positive charge and most of an atom's volume is empty space. Niels Bohr's model represented electrons orbiting the nucleus in fixed energy levels like planets around the sun, explaining atoms' distinct properties and how they form bonds.
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The document discusses the atomic structure including protons, neutrons, and electrons. Protons and neutrons are found in the nucleus which contains over 99% of the atom's mass. Protons are positively charged while neutrons are neutral. Electrons are negatively charged and orbit the nucleus, balancing out the positive charge of the protons to give atoms a net neutral charge.
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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.
Atomic structure.ppt 1
Atoms are composed of a nucleus containing protons and neutrons surrounded by an electron cloud. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons reside outside the nucleus in the electron cloud. The number of protons defines the identity of an element and is equal to its atomic number. The total number of protons and neutrons is the mass number. The number of electrons equals the number of protons to maintain electroneutrality. Models such as the Bohr model depict electron arrangement in shells surrounding the nucleus.
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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.
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Atomic structure.ppt 1
Atoms are composed of a nucleus containing protons and neutrons surrounded by an electron cloud. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons reside outside the nucleus in the electron cloud. The number of protons defines the identity of an element and is equal to its atomic number. The total number of protons and neutrons is the mass number. The number of electrons equals the number of protons to maintain electroneutrality. Models such as the Bohr model depict electron arrangement in shells surrounding the nucleus.
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2. Different atomic species like isotopes, isobars, and isotones.
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Democritus first proposed the idea of atoms in 460 BC, suggesting that all matter was made up of tiny spheres called atoms. An atom is the smallest particle of a chemical element that retains the properties of that element, and consists of a nucleus surrounded by a cloud of electrons. Atoms themselves are made up of even smaller subatomic particles - electrons, protons, and neutrons. The nucleus contains nearly all of an atom's mass and is very small compared to the size of the entire atom. Isotopes are variants of the same chemical element that differ in their number of neutrons.
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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
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3) It explains how atoms are distinguished based on their number of protons (atomic number) and total nuclear particles (mass number), including definitions of isotopes.
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Structure of atom
Ashish Raj presented on atomic structure. The presentation included:
1. Definitions of an atom, atomic number, and mass number.
2. Different atomic species like isotopes, isobars, and isotones.
3. Subatomic particles like electrons, protons, and neutrons.
4. Early atomic models including Thomson's plum pudding model, Rutherford's nuclear model, and Bohr's planetary model.
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Democritus first proposed the idea of atoms in 460 BC, suggesting that all matter was made up of tiny spheres called atoms. An atom is the smallest particle of a chemical element that retains the properties of that element, and consists of a nucleus surrounded by a cloud of electrons. Atoms themselves are made up of even smaller subatomic particles - electrons, protons, and neutrons. The nucleus contains nearly all of an atom's mass and is very small compared to the size of the entire atom. Isotopes are variants of the same chemical element that differ in their number of neutrons.
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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.
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The document outlines the history of the atomic model from ancient Greek philosophers to modern atomic theory. It describes early atomic theories from Democritus and Dalton who proposed atoms as indivisible and spherical particles. It then discusses the discoveries of J.J. Thompson, Rutherford, and Bohr that led to developments in atomic structure. Key developments included the discovery of the electron by Thompson, Rutherford's nuclear model from alpha scattering experiments, and Bohr's refinement incorporating electron orbits around the nucleus. The document concludes with explanations of atomic structure including electronic configurations and dot and cross diagrams.
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This science lesson covers subatomic particles like protons, neutrons, and electrons and their locations and charges in atoms. It discusses isotopes which have the same number of protons but different neutrons. Students are asked to draw shell diagrams for boron and phosphorus atoms and use an online simulation to build atoms and form cations and anions by gaining or losing electrons. The goal is for students to gain knowledge and understanding of the relationship between atoms and ions.
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1. Elements are the basic building blocks of all matter and are made up of atoms, which are the smallest particles of an element that retain its chemical properties.
2. Atoms consist of a tiny, dense nucleus surrounded by electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. The number of protons determines the element.
3. Modern atomic theory developed through the works of scientists like Dalton, Thomson, Rutherford, and Bohr, who discovered the subatomic particles and proposed models of atomic structure.
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J.J. Thomson discovered the electron in 1897 through his cathode ray experiment and proposed the "plum pudding" model of the atom in 1904. Later experiments provided evidence that atoms are made of even smaller subatomic particles. In the 1910s, Rutherford discovered the nucleus through his gold foil experiment and proposed a nuclear model of the atom. In 1932, Chadwick discovered the neutron through experiments bombarding beryllium with alpha particles. Atoms are now understood to have a small, dense nucleus containing protons and neutrons, surrounded by electrons in orbit.
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An atom consists of a dense nucleus containing protons and neutrons surrounded by a cloud of electrons. The nucleus contains protons which have a positive charge and neutrons which have a neutral charge. Electrons orbit the nucleus and have a negative charge. The atomic number represents the number of protons in an atom's nucleus, while the mass number is the total number of protons and neutrons.
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The document discusses the basic building blocks of matter at the atomic level. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and found in the atom's nucleus along with neutrons, which have no charge. Electrons are negatively charged and orbit the nucleus. It provides examples of hydrogen, oxygen, and sodium atoms, showing their proton, neutron, and electron composition. The atomic number is the number of protons, while the mass number includes protons and neutrons. Atoms can gain or lose electrons to become ions that are electrically charged.
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
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Matter is made up of atoms, which contain a nucleus of protons and neutrons surrounded by an electron cloud. Atoms are electrically neutral and bond with other atoms by sharing, losing, or gaining electrons in their outer valence shell. There are two main types of bonds: covalent bonds form when atoms share electrons, and ionic bonds form when one atom transfers an electron to another. Understanding the basic building blocks of matter and how atoms bond is fundamental to chemistry.
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The document discusses the history and structure of the atomic model. It describes how ancient Greek philosophers like Democritus first proposed that all matter is made up of indivisible particles called atoms. In the early 1900s, scientists like Thomson and Rutherford began experimentally determining the internal structure of atoms. Atoms are now understood to have a small, dense nucleus containing protons and neutrons, surrounded by electrons in energy levels.
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This document summarizes key concepts from Chapter 4 on atomic structure:
1) It describes early atomic theories from Democritus and Dalton, including defining atoms as indivisible particles and Dalton's atomic theory.
2) It outlines the discovery of subatomic particles like electrons, protons, and neutrons through experiments by Thomson, Rutherford, and Chadwick.
3) It explains how atoms are distinguished based on their number of protons (atomic number) and total nuclear particles (mass number), including definitions of isotopes.
4) It provides an overview of how Mendeleev organized the periodic table and how this has been refined, including the organization of groups and periods.
Structure of atom
The document summarizes key concepts about the structure of the atom:
1) Atoms contain positively charged protons, neutral neutrons, and negatively charged electrons. Rutherford discovered the nucleus and that atoms are mostly empty space.
2) Bohr's model improved on Rutherford's by proposing electrons orbit in discrete energy levels.
3) Elements are defined by their atomic number, or number of protons. Isotopes are atoms of the same element with different numbers of neutrons.
Presentation for Radioactivity
Atoms are made up of protons, neutrons, and electrons, with the number of protons defining the element. Different isotopes of an element have the same number of protons but different numbers of neutrons. Radioactive decay occurs spontaneously as nuclei emit alpha, beta, or gamma radiation to become more stable, conserving nuclear particles but decreasing mass.
Atom Presentation With Narration
This document provides an overview of atoms and atomic structure through a self-guided computer activity. It discusses the atomic-molecular theory of matter and how scientists have gathered indirect evidence to develop models of atoms. It describes the subatomic particles that make up atoms, including protons, neutrons, and electrons. Atoms are electrically neutral due to having equal numbers of protons and electrons. The activity guides students to learn about atomic structure by visiting websites and completing a study guide.
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The document summarizes the history and development of atomic theory from ancient Greek philosophers to modern atomic structure. It discusses early atomic models proposed by philosophers like Democritus and scientists like Dalton, Thomson, and Rutherford. It then explains atomic structure including subatomic particles like protons, neutrons, and electrons. The periodic table is introduced as a way to organize the elements based on their atomic structure and properties. Key aspects of the periodic table like atomic number, mass number, groups and periods are defined.
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The periodic table is a chart that arranges the elements by atomic number in rows and columns according to their chemical and physical properties. It provides important information about each element such as the number of protons, neutrons, and electrons. The position of an element on the periodic table can reveal whether it is a metal or nonmetal based on location relative to the zigzag line. Metals are generally found on the left side and have properties of being shiny, malleable, ductile, good conductors of heat and electricity, and high melting points.
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.
Atomic structure
An atom is composed of a nucleus containing protons and neutrons surrounded by electrons. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons exist outside the nucleus in the electron cloud. The number of protons defines the element and is equal to the atomic number. The total number of protons and neutrons is the mass number. For neutral atoms, the number of electrons equals the number of protons. Isotopes are atoms of the same element with different numbers of neutrons.
How do elements and compounds combine to form all types of matter
The document summarizes key concepts in atomic theory:
- Ancient Greek philosophers proposed that matter is made of indivisible particles called atoms. Democritus further hypothesized that atoms were tiny, indivisible spheres.
- J.J. Thomson's experiments showed atoms contain negatively charged electrons distributed in a sphere of positive charge. Rutherford proposed a nuclear model with electrons orbiting a tiny, dense nucleus.
- Atoms are composed of protons, neutrons, and electrons. Protons and neutrons are in the nucleus, electrons orbit the nucleus. The number of protons defines an element. Neutral atoms have equal numbers of protons and electrons.
Atoms and the periodic table
This document discusses the structure of atoms and the periodic table. It explains that atoms are made up of protons, neutrons, and electrons. Elements are organized on the periodic table based on their atomic number. Each element has an atomic symbol. The document also describes isotopes, which are variants of an element with different numbers of neutrons. It defines key terms like atomic mass, mass number, and ions.
1 atomic theory (site)
1. Atoms are the smallest units of matter and consist of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus in electron orbitals.
2. The periodic table organizes elements based on their physical and chemical properties. It lists the atomic number and mass of each element.
3. Atoms are electrically neutral when they have the same number of protons and electrons. Valence electrons are in the outermost shell and determine how atoms bond together.
Atoms and the periodic table
This document discusses the structure of atoms and the periodic table. It describes atoms as being made up of protons, neutrons, and electrons. Elements are organized on the periodic table according to their atomic structure. The periodic table lists the atomic number and average atomic mass of each element. Isotopes are variants of elements that have different numbers of neutrons but the same number of protons. Ions are formed when atoms gain or lose electrons, becoming positively or negatively charged.
ATOMS ppt.pptx
Atoms are the smallest particle into which an element can be divided and still be the same element. Atoms are made up of subatomic particles, including protons and neutrons located in the nucleus, and electrons that orbit around the nucleus. Elements are substances composed of only one type of atom, with each element identified by its atomic number which is equal to the number of protons. The periodic table arranges the elements and displays important information about each element like atomic number, atomic mass, and number of protons, neutrons, and electrons.
DIGITAL LP 1.pptx
This digital lesson plan introduces the structure of atoms. It defines atoms as the smallest particle of matter, composed of subatomic particles including protons, neutrons, and electrons. It explains that protons and neutrons are located in the nucleus, while electrons orbit the nucleus. The document also defines atomic number as the number of protons and mass number as the total number of protons and neutrons. It provides examples of how to calculate atomic number and mass number for different elements. Students are assigned problems to calculate atomic number and mass number.
identify proton, neutrons and electrons.pptx
An atom is composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons move around the nucleus. The number of protons determines the element, while the number of neutrons can vary, creating isotopes of that element. Isotopes are identified by their isotope notation, which includes the element symbol, mass number (protons + neutrons), and atomic number (protons).
Atoms and the periodic table
- The document discusses atoms and the periodic table. It provides information on the structure of atoms including electrons, protons, and neutrons.
- Key points from the periodic table are that elements are organized on it and each has an atomic symbol. The periodic table can provide atomic mass and other information about elements.
- Atoms consist of electrons in an electron cloud surrounding the nucleus of protons and neutrons. Protons have a positive charge while electrons have a negative charge, making the overall atom neutral. Isotopes are variants of elements with different numbers of neutrons.
Unit iii the atom and the prediodic table (2)
This document discusses the structure of atoms and the periodic table. It begins by introducing atomic theories proposed by scientists like Dalton, Thomson, Rutherford, Bohr and Schrodinger. It then discusses subatomic particles like protons, neutrons and electrons. The document explains how elements are organized on the periodic table based on their atomic number and electronic configuration. It provides examples of writing out electronic configurations and identifying protons, neutrons and electrons in different isotopes.
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How do elements and compounds combine to form all types of matter
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Atom structure
- 1. Atom Structure Atomic Number, Mass Number and Ion Charge
- 2. Lesson Outcomes • By the end of this lesson you should be able to: – Illustrate the structure of an atom. – Accurately explain the terms “atomic number” and “mass number” and identify each value on the periodic table. – Calculate the number of neutrons in an atom/ the mass of an atom when given specific variables. – Calculate the charge on an atom.
- 3. Atomic Structure • An atom is composed of: – A nucleus with: - Protons that are positively charged - Neutrons that are neutral – A space around the nucleus with: - Energy levels surrounding the nucleus - Electrons that are negatively charged
- 4. Atomic Number • The atomic number of an element is the number of protons (+) in the nucleus. It also indicates the position of the element on the periodic table.
- 5. Neutral Atoms • Atoms are capable of having positive and negative charges. • In a neutral atom the amount of protons (+ charge) is equal to the amount of electrons (- charge).
- 6. Can you determine whether this atom is positively/negatively charged?
- 7. Neutrons • Neutrons are particles in atoms that contribute to approximately half of an atom’s mass. This is because protons and neutrons are roughly the same size. • Neutrons do not possess any charge, unlike positive protons and negative electrons.
- 8. Calculating the number of Neutrons in an Atom. • Number of Neutrons = Mass Number - Number of Protons (atomic number).
- 9. Calculating the Number of Neutrons • Can you calculate the amount of neutrons in the following mercury atom?
- 10. Relative Atomic Mass • Carbon has an atomic mass of exactly 12 amu. The masses of other elements are calculated by comparison to this. • Thus, the hydrogen atom’s mass is one twelfth of this and so its relative atomic mass is one. • The relative atomic mass can be read straight off the periodic table. • Most elements occur in nature as a mixture of isotopes, so the atomic mass of the element will be a weighted average of all of these masses.
- 11. Mass Number • The mass number is the total number of nucleons, that is the number of protons and neutrons in the nucleus, in an element. • The mass number gives only an indication of the mass of an atom. • The mass of an atom is determined by its nucleons (protons and neutrons). • Electrons have a relatively small mass and simply impart volume to the atom instead of mass.
- 12. Notation on the Periodic Table • Elements are portrayed by the nuclear notation: (mass number is always larger than the atomic number)
- 13. • In the example above it means that: – The element is Helium. – There are 4 protons and neutrons in the nucleus. – There are 2 protons. – There are 3 electrons. – Helium is element number 2 on the periodic table.
- 14. Ions • An ion is a charged particle • When a neutral atom looses an electron it becomes a positive ion known as a cation. • When a neutral atom gains an electron it becomes a negatively charged ion known as an anion. • The number of protons and neutrons DOES NOT CHANGE.
- 15. Determining Ion Charge • What is the charge on a Li atom if it loses an electron? - is it +/-? - what is the charge value? • What is the charge on an F atom if it gains 2 electrons? - is it +/-? - what is the charge value?
- 16. Activity • Complete the activity sheets in pairs or groups of three.
Editor's Notes
- do extra calculations to show how to calculate mass, proton number (atomic number), mass due to protons.