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The Structure of the Atom
The Structure of the Atom
This lesson covers the fundamental structure of the atom as required by the AQA GCSE Physics specification (4.4.1). You need to understand the basic model of the atom, the sub-atomic particles it contains, and how they are arranged. This knowledge is the foundation for understanding radioactivity, nuclear reactions, and the behaviour of matter at the smallest scales.
The Nuclear Model of the Atom
The atom consists of a tiny, dense nucleus at the centre, surrounded by electrons that orbit the nucleus at different energy levels (sometimes called shells). The nucleus contains two types of sub-atomic particle: protons and neutrons. Together, protons and neutrons are called nucleons.
Key features of the nuclear model:
- The nucleus is extremely small compared to the overall size of the atom. The radius of the nucleus is about 1 x 10^-14 m, while the radius of the atom is about 1 x 10^-10 m. This means the nucleus is roughly 10,000 times smaller than the atom itself.
- Most of the mass of the atom is concentrated in the nucleus, because protons and neutrons are much heavier than electrons.
- The electrons orbit the nucleus at relatively large distances. Most of the atom is empty space.
- The electrons are held in orbit by the electrostatic force of attraction between the negatively charged electrons and the positively charged protons in the nucleus.
Exam Tip: If asked to describe the nuclear model, always mention three things: (1) a small, dense, positively charged nucleus, (2) electrons orbiting at a distance, and (3) most of the atom is empty space. These three points will secure full marks.
Sub-Atomic Particles
There are three sub-atomic particles you need to know. Each has a different charge and relative mass.
| Particle | Location | Relative Mass | Relative Charge |
|---|---|---|---|
| Proton | Nucleus | 1 | +1 |
| Neutron | Nucleus | 1 | 0 |
| Electron | Orbiting nucleus | Very small (approx. 1/1836) | -1 |
Key Points
- Protons and neutrons have approximately the same mass. For GCSE purposes, we say they each have a relative mass of 1.
- Electrons have a mass that is negligible compared to protons and neutrons. This is why the mass of an atom is almost entirely due to its nucleus.
- A proton has a charge of +1 and an electron has a charge of -1. These charges are equal in magnitude but opposite in sign.
- A neutron has no charge (it is electrically neutral).
Exam Tip: The relative mass of an electron is sometimes given as 0.0005 or 1/1836. For most GCSE questions, you can simply say the mass of an electron is "negligible" or "very small" compared to a proton or neutron. Do not say it is zero — it does have mass, just a very small amount.
Atoms Are Electrically Neutral
In a neutral atom, the number of protons equals the number of electrons. Because each proton has a +1 charge and each electron has a -1 charge, the charges cancel out, making the atom electrically neutral overall.
- A hydrogen atom has 1 proton and 1 electron: total charge = +1 + (-1) = 0.
- A carbon atom has 6 protons and 6 electrons: total charge = +6 + (-6) = 0.
- A uranium atom has 92 protons and 92 electrons: total charge = +92 + (-92) = 0.
The Size of Atoms
Atoms are incredibly small. The radius of a typical atom is about 1 x 10^-10 m (0.1 nanometres). To put this in perspective:
- A human hair is about 0.1 mm (1 x 10^-4 m) thick, so roughly one million atoms could fit across the width of a human hair.
- The nucleus is even smaller — about 1 x 10^-14 m in radius, which is about 1/10,000th the radius of the atom.
If the atom were scaled up to the size of a football stadium, the nucleus would be about the size of a marble on the centre spot. Everything else would be empty space with tiny electrons orbiting far from the centre.
graph TD
A["Atom (radius ~ 1 x 10^-10 m)"] --> B["Nucleus (radius ~ 1 x 10^-14 m)"]
A --> C["Electron Cloud"]
B --> D["Protons (+1 charge, mass 1)"]
B --> E["Neutrons (0 charge, mass 1)"]
C --> F["Electrons (-1 charge, negligible mass)"]
style A fill:#2c3e50,color:#fff
style B fill:#e74c3c,color:#fff
style C fill:#3498db,color:#fff
style D fill:#e74c3c,color:#fff
style E fill:#95a5a6,color:#fff
style F fill:#3498db,color:#fff
Electron Configuration
Electrons orbit the nucleus in energy levels (shells). Each energy level can hold a certain maximum number of electrons:
| Energy Level (Shell) | Maximum Electrons |
|---|---|
| 1st (closest to nucleus) | 2 |
| 2nd | 8 |
| 3rd | 8 |
Electrons always fill the lowest available energy level first before moving to the next shell outward. This is because electrons in lower energy levels are closer to the nucleus and experience a stronger electrostatic attraction.
Examples
| Element | Atomic Number | Electron Configuration |
|---|---|---|
| Hydrogen | 1 | 1 |
| Helium | 2 | 2 |
| Lithium | 3 | 2, 1 |
| Carbon | 6 | 2, 4 |
| Oxygen | 8 | 2, 6 |
| Sodium | 11 | 2, 8, 1 |
| Chlorine | 17 | 2, 8, 7 |
| Calcium | 20 | 2, 8, 8, 2 |
Exam Tip: You can work out the electron configuration from the atomic number (which equals the number of protons, which equals the number of electrons in a neutral atom). Fill the first shell with up to 2, the second with up to 8, the third with up to 8, and so on.
Ions
When an atom gains or loses electrons, it becomes an ion. Ions are charged particles:
- If an atom loses one or more electrons, it becomes a positive ion (cation) because it now has more protons than electrons.
- If an atom gains one or more electrons, it becomes a negative ion (anion) because it now has more electrons than protons.
| Atom | Protons | Electrons in Atom | Change | Electrons in Ion | Ion Charge |
|---|---|---|---|---|---|
| Sodium (Na) | 11 | 11 | Loses 1 | 10 | +1 (Na+) |
| Chlorine (Cl) | 17 | 17 | Gains 1 | 18 | -1 (Cl-) |
| Magnesium (Mg) | 12 | 12 | Loses 2 | 10 | +2 (Mg2+) |
| Oxygen (O) | 8 | 8 | Gains 2 | 10 | -2 (O2-) |
Important: When an atom becomes an ion, only the number of electrons changes. The number of protons and neutrons stays the same. This means the element does not change — a sodium ion is still sodium.
Common Exam Mistakes
- Saying the nucleus contains electrons — electrons orbit outside the nucleus.
- Saying electrons have no mass — they have a very small mass, not zero.
- Confusing atoms and ions — an atom is neutral; an ion has gained or lost electrons.
- Saying the atom is "solid" or "full" — most of the atom is empty space.
- Giving the wrong relative charges — protons are +1, electrons are -1, neutrons are 0.
Summary
- The atom has a small, dense nucleus containing protons (+1 charge, mass 1) and neutrons (0 charge, mass 1).
- Electrons (-1 charge, negligible mass) orbit the nucleus at different energy levels.
- The radius of an atom is about 1 x 10^-10 m; the radius of the nucleus is about 1 x 10^-14 m.
- In a neutral atom, the number of protons equals the number of electrons.
- Electrons fill the lowest energy levels first (2, 8, 8 pattern).
- Ions are formed when atoms gain or lose electrons, becoming electrically charged.
- Most of the atom is empty space.
Exam Tip: A common 4-mark question asks you to describe the structure of the atom. Structure your answer logically: start with the nucleus (protons and neutrons), then describe the electrons orbiting in shells, then state that the atom is mostly empty space and that the nucleus is very small compared to the overall atom. Include the relative charges and masses for full marks.