Atomic Structure and Isotopes of Hydrogen
This page covers the fundamental concepts of atomic structure, focusing on the isotopes of hydrogen and the calculation of relative atomic mass. It also provides a historical overview of atomic models and details about subatomic particles.
What are the 3 isotopes of hydrogen? The page begins by listing the three isotopes of hydrogen:
Definition:
- Hydrogen-1 (Hโ)
- Hydrogen-2 (Hยฒ)
- Hydrogen-3 (Hยณ)
These isotopes differ in their number of neutrons while maintaining the same number of protons, which is characteristic of isotopes.
The document then explains the concept of relative atomic mass and provides examples of its calculation:
Example: Calculating Relative Atomic Mass for Chlorine
Chlorine-35 75 and Chlorine-37 (25% abundance)
Calculation: (75ร35 + 25ร37) / 75+25 = 35.5
Example: Calculating Relative Atomic Mass for Copper
Copper-63 69 and Copper-65 (31% abundance)
Calculation: (63ร69 + 65ร31) / 69+31 = 63.62
The page also covers key concepts in atomic structure:
Highlight:
- Mass number = neutrons + protons
- Atomic number = number of protons
- The number of protons determines the element
- Atoms of the same element can have different numbers of neutrons (isotopes)
The document provides information on the components of an atom:
Definition: An atom is made up of:
- Neutrons and protons in the nucleus
- Electrons orbiting the nucleus
It also introduces the concept of ions:
Vocabulary: Ion - an atom that loses or gains electrons, becoming either positively or negatively charged.
The page includes a table of subatomic particles and their properties:
Highlight: Subatomic Particles:
- Electrons: Charge -1, Mass almost 0
- Neutrons: Charge 0, Mass 1
- Protons: Charge +1, Mass 1
The document then presents a historical overview of atomic models:
- John Dalton (1803): All matter made of indivisible tiny spheres called atoms
- J.J. Thomson (1897): Discovered the electron, created the plum pudding model
- Ernest Rutherford (1909): Conducted the gold foil experiment, concluded atoms have a positively charged nucleus with negative electrons encasing it
- Niels Bohr (1913): Adapted Rutherford's model to include fixed energy shells
- James Chadwick (1932): Discovered the neutron
Finally, the page describes the modern-day atomic model:
Highlight: Modern Atomic Model Characteristics:
- Most of the atom is empty space
- Number of electrons equals number of protons
- Most mass is concentrated in the positively charged nucleus
- Electrons are arranged in shells around the nucleus
This comprehensive overview provides students with a solid foundation for understanding isotopes of hydrogen in atomic structure class and beyond.