Lecture Notes: Understanding Atoms

Introduction

Presenter: Pharoah Ed
Focus: Understanding atoms, their structure, and calculating subatomic particles.
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Atoms are the smallest particles of a chemical element.
Size: Approximately 0.0000001 cm wide.
Comparison: 7 million atoms needed to equal the thickness of a crisp or the height of Mount Everest.

Atoms are composed of three smaller particles:
- Neutrons
- Protons
- Electrons

Electron Shells:
- White lines surrounding the nucleus where electrons orbit.
Nucleus:
- Dense core at the atom's center.
- Contains protons and neutrons.

Each particle has mass and charge:
- Protons:
  - Mass = 1
  - Charge = Positive
- Neutrons:
  - Mass = 1
  - Charge = Neutral
- Electrons:
  - Mass ≈ 0
  - Charge = Negative
Mnemonic to remember charges:
- "Pro for positive" (Proton = Positive)
- "Nu for neutral" (Neutron = Neutral)
- Electron is negative by elimination.

Example: Carbon (C)
- Symbol: C
- Atomic Number: 6 (number of protons and electrons)
- Atomic Weight: 12 (sum of protons and neutrons)

Atoms consist of neutrons, protons, and electrons forming the structure.
Nuclear composition: Nucleus contains protons and neutrons; electrons orbit the nucleus.
Particle properties: Mass and charge differ across protons, neutrons, and electrons.
Chemical symbols:
- Letter represents the element.
- Top number = Atomic weight.
- Bottom number = Atomic number.
Mathematical Equations:
- Mass number = Protons + Neutrons
- Neutrons = Mass number - Atomic number
- Protons = Atomic number
Protons and electrons are equal in number in an atom.