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Atoms and Elements: Foundations

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Atoms and Elements: Foundations

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About this activity

Explore atomic structure and periodic basics.

Created by

Elsa Dowdy
Elsa Dowdy
United States

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Atoms and Elements: Foundations
 

Atoms and Elements: FoundationsOnline version

Explore atomic structure and periodic basics.

by Elsa Dowdy
1

Introduction to Atomic Theory

Atoms are the building blocks of matter. Early ideas evolved into Dalton’s theory, shaping our understanding of chemical change and conservation of mass.

2

Dalton’s Atomic Theory

Dalton proposed five postulates: matter is made of atoms; atoms are indivisible; all atoms of an element are identical; compounds are formed by combining atoms; and atoms rearrange in reactions.

3

Atoms vs. Ions

Neutral atoms have equal protons and electrons. When electrons are gained or lost, particles become ions with positive or negative charges, altering properties.

4

Atomic versus Mass Number

The atomic number (Z) counts protons, defining the element. The mass number (A) equals protons plus neutrons, indicating total nucleons.

5

Neutral Atoms and Electron Count

In neutral atoms, Z equals the number of electrons. If electrons are removed or added, the balance shifts, creating ions with charges.

6

Isotopes and Atomic Mass

Most elements exist as isotopic mixtures. The atomic mass on the periodic table is a weighted average of isotopes’ masses.

7

Subatomic Particles

Protons (mass ~1 amu, +1), neutrons (~1 amu, 0), and electrons (~0.00055 amu, −1) compose atoms and define their behavior in reactions.

8

Electron Discovery & Models

J.J. Thomson’s cathode-ray experiments revealed electrons as the first subatomic particle, leading to early atomic models and the plum pudding idea.

9

Nucleus and Rutherford

Rutherford’s gold-foil experiments showed a dense nucleus at the center, with most atom volume being empty space and electrons surrounding the nucleus.
 
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