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4.3 Atomic mass and diameter
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4.5 Isotopes
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As a result of the work done by previous scientists on atomic models, scientists now have a good idea of what an atom looks like. This knowledge is important because it helps us to understand why materials have different properties and why some materials bond with others. Let us now take a closer look at the microscopic structure of the atom (what the atom looks like inside).
So far, we have discussed that atoms are made up of a positively charged nucleus surrounded by one or more negatively charged electrons. These electrons orbit the nucleus.
Before we look at some useful concepts we first need to understand what electrons, protons and neutrons are.
The electron is a very tiny particle. It has a mass of \(\text{9,11} \times \text{10}^{-\text{31}}\) \(\text{kg}\). The electron carries one unit of negative electric charge (i.e. \(-\text{1,6} \times \text{10}^{-\text{19}}\) \(\text{C}\)).
Unlike the electron, the nucleus can be broken up into smaller building blocks called protons and neutrons. Together, the protons and neutrons are called nucleons.
Scientists believe that the electron can be treated as a point particle or elementary particle meaning that it cannot be broken down into anything smaller.
The electron carries one unit of negative electric charge (i.e. \(-\text{1,6} \times \text{10}^{-\text{19}}\) \(\text{C}\), C is Coulombs).
Each proton carries one unit of positive electric charge (i.e. \(\text{+1,6} \times \text{10}^{-\text{19}}\) \(\text{C}\)). Since we know that atoms are electrically neutral, i.e. do not carry any extra charge, then the number of protons in an atom has to be the same as the number of electrons to balance out the positive and negative charge to zero. The total positive charge of a nucleus is equal to the number of protons in the nucleus. The proton is much heavier than the electron (\(\text{10 000}\) times heavier!) and has a mass of \(\text{1,6726} \times \text{10}^{-\text{27}}\) \(\text{kg}\). When we talk about the atomic mass of an atom, we are mostly referring to the combined mass of the protons and neutrons, i.e. the nucleons.
The neutron is electrically neutral i.e. it carries no charge at all. Like the proton, it is much heavier than the electron and its mass is \(\text{1,6749} \times \text{10}^{-\text{27}}\) \(\text{kg}\) (slightly heavier than the proton).
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proton |
neutron |
electron |
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Mass (\(\text{kg}\)) |
\(\text{1,6726} \times \text{10}^{-\text{27}}\) |
\(\text{1,6749} \times \text{10}^{-\text{27}}\) |
\(\text{9,11} \times \text{10}^{-\text{31}}\) |
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Units of charge |
\(\text{+1}\) |
\(\text{0}\) |
\(-\text{1}\) |
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Charge (\(\text{C}\)) |
\(\text{1,6} \times \text{10}^{-\text{19}}\) |
\(\text{0}\) |
\(-\text{1,6} \times \text{10}^{-\text{19}}\) |
Table 4.2: Summary of the particles inside the atom.
The chemical properties of an element are determined by the charge of its nucleus, i.e. by the number of protons. This number is called the atomic number and is denoted by the letter Z.
The number of protons in an atom.
You can find the atomic number on the periodic table (see periodic table at front of book). The atomic number is an integer and ranges from 1 to about 118.
The mass of an atom depends on how many nucleons its nucleus contains. The number of nucleons, i.e. the total number of protons plus neutrons, is called the atomic mass number and is denoted by the letter A.
Currently element 118 is the highest atomic number for an element. Elements of high atomic numbers (from about 93 to 118) do not exist for long as they break apart within seconds of being formed. Scientists believe that after element 118 there may be an “island of stability” in which elements of higher atomic number occur that do not break apart within seconds.
A nuclide is a distinct kind of atom or nucleus characterised by the number of protons and neutrons in the atom. To be absolutely correct, when we represent atoms like we do here, then we should call them nuclides.
The number of protons and neutrons in the nucleus of an atom.
The atomic number (Z) and the mass number (A) are indicated using a standard notation, for example carbon will look like this: \(_{6}^{12}\text{C}\)
Standard notation shows the chemical symbol, the atomic mass number and the atomic number of an element as follows:
For example, the iron nucleus which has 26 protons and 30 neutrons, is denoted as \(_{26}^{56}\text{Fe}\) where the atomic number is \(Z = 26\) and the mass number \(A = 56\). The number of neutrons is simply the difference \(N = A - Z = 30\).
Do not confuse the notation we have used here with the way this information appears on the periodic table. On the periodic table, the atomic number usually appears in the top left-hand corner of the block or immediately above the element's symbol. The number below the element's symbol is its relative atomic mass. This is not exactly the same as the atomic mass number. This will be explained in "Isotopes". The example of iron is shown below.
For a neutral atom the number of electrons is the same as the number of protons, since the charge on the atom must balance. But what happens if an atom gains or loses electrons? Does it mean that the atom will still be part of the same element? A change in the number of electrons of an atom does not change the type of atom that it is. However, the charge of the atom will change. The neutrality of the atom has changed. If electrons are added, then the atom will become more negative. If electrons are taken away then the atom will become more positive. The atom that is formed in either of these two cases is called an ion. An ion is a charged atom. For example: a neutral sodium atom can lose one electron to become a positively charged sodium ion (\(\text{Na}^{+}\)). A neutral chlorine atom can gain one electron to become a negatively charged chlorine ion (\(\text{Cl}^{-}\)). Another example is \(\text{Li}^{+}\) which has lost one electron and now has only 2 electrons, instead of 3. Or consider \(\text{F}^{-}\) which has gained one electron and now has 10 electrons instead of 9.
Use standard notation to represent sodium and give the number of protons, neutrons and electrons in the element.
\(\text{Na}\)
Sodium has 11 protons, so we have: \(_{11}^{23}\text{Na}\)
Sodium is neutral, so it has the same number of electrons as protons. The number of electrons is \(\text{11}\).
From the periodic table we see that \(A = 23\).
We know \(A\) and \(Z\) so we can find \(N\): \(N = A - Z = 23 - 11 = 12\).
In standard notation sodium is given by: \(_{11}^{23}\text{Na}\). The number of protons is 11, the number of neutrons is 12 and the number of electrons is 11.
Explain the meaning of each of the following terms:
nucleus
electron
atomic mass
Complete the following table:
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Element |
Atomic mass units |
Atomic number |
Number of protons |
Number of electrons |
Number of neutrons |
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\(\text{Mg}\) |
\(\text{24}\) |
\(\text{12}\) |
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\(\text{O}\) |
\(\text{8}\) |
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\(\text{17}\) |
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\(\text{Ni}\) |
\(\text{28}\) |
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\(\text{40}\) |
\(\text{20}\) |
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\(\text{Zn}\) |
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\(\text{0}\) |
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\(\text{C}\) |
\(\text{12}\) |
\(\text{6}\) |
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\(\text{Al}^{3+}\) |
\(\text{13}\) |
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\(\text{O}^{2-}\) |
\(\text{10}\) |
Use standard notation to represent the following elements:
potassium
copper
chlorine
For the element \(_{17}^{35}\text{Cl}\), give the number of...
protons
neutrons
electrons
... in the atom.
Which of the following atoms has 7 electrons?
\(_{2}^{5}\text{He}\)
\(_{6}^{13}\text{C}\)
\(_{3}^{7}\text{Li}\)
\(_{7}^{15}\text{N}\)
In each of the following cases, give the number or the element symbol represented by X.
\(_{18}^{40}\text{X}\)
\(_{20}^{X}\text{Ca}\)
\(_{X}^{31}\text{P}\)
Complete the following table:
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A |
Z |
N |
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\(_{92}^{235}\text{U}\) |
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\(_{92}^{238}\text{U}\) |
In these two different forms of uranium...
What is the same?
What is different?
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4.3 Atomic mass and diameter
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4.5 Isotopes
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