🔋college physics i – introduction review

key term - Atoms

Definition

Atoms are the fundamental building blocks of all matter in the universe. They are the smallest units of an element that retain its chemical properties, consisting of a nucleus containing protons and neutrons, surrounded by a cloud of orbiting electrons.

5 Must Know Facts For Your Next Test

  1. Atoms were first proposed by the ancient Greek philosopher Democritus, who theorized that matter was composed of indivisible particles called 'atomos'.
  2. In the early 20th century, Ernest Rutherford's gold foil experiment led to the discovery of the atomic nucleus, challenging the previously accepted 'plum pudding' model of the atom.
  3. The modern model of the atom, developed by Niels Bohr, describes electrons orbiting the nucleus in specific energy levels or shells.
  4. The number of protons in the nucleus determines the element's atomic number, while the number of protons and neutrons together determine the atom's mass number.
  5. Atoms can form bonds with other atoms through the sharing or transfer of electrons, leading to the formation of molecules and compounds.

Review Questions

  • Explain the key features of the Rutherford's gold foil experiment and how it led to the discovery of the atomic nucleus.
    • Rutherford's gold foil experiment involved firing a beam of alpha particles (helium nuclei) at a thin sheet of gold foil. Most of the alpha particles passed straight through the foil, as expected, but a small number were unexpectedly deflected at large angles. This observation led Rutherford to conclude that the atom must have a dense, positively charged core (the nucleus) surrounded by a largely empty space, rather than the previously accepted 'plum pudding' model. The discovery of the atomic nucleus was a crucial step in the development of the modern understanding of atomic structure.
  • Describe the Bohr model of the atom and how it explains the behavior of electrons within an atom.
    • The Bohr model of the atom, proposed by Niels Bohr, depicts electrons orbiting the nucleus in specific, discrete energy levels or shells. According to this model, electrons can only occupy certain allowed energy levels and cannot exist in the space between these levels. When an electron absorbs or emits energy, it transitions between these fixed energy levels, leading to the emission or absorption of photons with specific wavelengths. This model helped explain the observed line spectra of atoms and laid the foundation for the quantum mechanical understanding of atomic structure.
  • Analyze the relationship between the number of protons, neutrons, and electrons in an atom, and how this determines the element's properties.
    • The number of protons in the nucleus of an atom is the defining characteristic of an element, as it determines the element's atomic number and chemical properties. The number of neutrons, on the other hand, can vary for a given element, resulting in different isotopes with the same atomic number but different mass numbers. The number of electrons orbiting the nucleus is typically equal to the number of protons, giving the atom a neutral charge. However, atoms can gain or lose electrons, becoming positively or negatively charged ions, which can significantly impact their chemical reactivity and bonding behavior. The interplay between protons, neutrons, and electrons is crucial in understanding the diverse properties and behaviors of atoms and the elements they constitute.