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- https://chem.libretexts.org/Ancillary_Materials/Interactive_Applications/PhET_Simulations/PhET%3A_Rutherford_ScatteringHow did Rutherford figure out the structure of the atom without being able to see it? Simulate the famous experiment in which he disproved the Plum Pudding model of the atom by observing alpha particl...How did Rutherford figure out the structure of the atom without being able to see it? Simulate the famous experiment in which he disproved the Plum Pudding model of the atom by observing alpha particles bouncing off atoms and determining that they must have a small core.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/04%3A_Atomic_Structure/4.15%3A_Atomic_NucleusThis page likens science to a jigsaw puzzle, illustrating how researchers' discoveries enhance our understanding of complex concepts like the atomic nucleus. It traces the evolution of atomic models f...This page likens science to a jigsaw puzzle, illustrating how researchers' discoveries enhance our understanding of complex concepts like the atomic nucleus. It traces the evolution of atomic models from Thomson's to Rutherford's, highlighting how the introduction of neutrons clarified the coexistence of protons in the nucleus. This led to the recognition of the strong nuclear force, which binds protons and neutrons despite the repulsion between protons.
- https://chem.libretexts.org/Courses/University_of_California_Irvine/UCI%3A_General_Chemistry_1A_(OpenChem)/192Development_of_Atomic_Models_(OpenChem)
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_1%3A_Atomic_Structure/Chapter_1%3A_Introduction/Chapter_1.1%3A_The_AtomAlthough Rutherford could not explain why repulsion between the positive charges in nuclei that contained more than one positive charge did not cause the nucleus to disintegrate, he reasoned that repu...Although Rutherford could not explain why repulsion between the positive charges in nuclei that contained more than one positive charge did not cause the nucleus to disintegrate, he reasoned that repulsion between the positively charged nucleus and the negatively charged electrons would cause the electrons to be distributed throughout the atom’s volume.Today we know that strong nuclear forces, which are much stronger than electrostatic interactions, hold the protons and the neutrons together in…
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/04%3A_Atomic_Structure/4.14%3A_Gold_Foil_ExperimentThis page discusses Rutherford's 1911 gold foil experiment, which challenged the prevailing atomic model by demonstrating that some alpha particles were significantly deflected. This led to the propos...This page discusses Rutherford's 1911 gold foil experiment, which challenged the prevailing atomic model by demonstrating that some alpha particles were significantly deflected. This led to the proposal of a nuclear model of the atom, with a dense, positively charged nucleus made up of protons and neutrons, and electrons surrounding it in a cloud, highlighting that most of the atom is empty space. This was a pivotal advancement in atomic theory.
- https://chem.libretexts.org/Courses/Bennington_College/Chemistry_-_An_Integrated_Approach_(Bullock)/03%3A_Why_Do_Molecules_Exist/3.02%3A_Atomic_Structure[8] The radius of a “typical” atom is on the order of about 1×10 -10 m, whereas that of the nucleus is about 1×10 -15 m; using this proportion, if an atom were the size of a football field, 100 yards ...[8] The radius of a “typical” atom is on the order of about 1×10 -10 m, whereas that of the nucleus is about 1×10 -15 m; using this proportion, if an atom were the size of a football field, 100 yards across, the nucleus would be like a dime sitting on the 50-yard line; the rest of the surrounding stadium would be the electron cloud.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/05%3A_Electrons_in_Atoms/5.01%3A_Electromagnetic_SpectrumThis page discusses the nature of waves, highlighting that they represent energy beyond just water. It critiques Rutherford's atomic model for not addressing electron behavior and notes early 20th-cen...This page discusses the nature of waves, highlighting that they represent energy beyond just water. It critiques Rutherford's atomic model for not addressing electron behavior and notes early 20th-century experiments showcasing light's dual wave-particle nature. Additionally, it details visible light's wavelength (400-700 nm) and speed (3.
