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Questions and Answers
What property of electrons is overlooked by the Bohr theory?
According to the Heisenberg Uncertainty Principle, what cannot be precisely determined simultaneously?
What is the term for the spatial region where an electron is likely to be found around the nucleus?
Which principle explains the order in which electrons fill energy sublevels?
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What is referred to as a group of orbitals that share the same energy?
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What does an emission spectrum display?
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How is the presence of an element typically measured using atomic absorption spectrometry?
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What happens to energy when an electron transitions from a higher to a lower energy level?
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What is the distinction between a continuous spectrum and an emission spectrum?
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What two methods are commonly used to energize atoms?
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Study Notes
Limitations of Bohr Theory
- Did not account for the dual wave-particle nature of electrons.
- Failed to recognize the existence of atomic orbitals.
Heisenberg Uncertainty Principle
- It is impossible to simultaneously determine the exact position and velocity of an electron.
Atomic Orbital
- Represents the region around the nucleus where the probability of finding an electron is relatively high.
Aufbau Principle
- Governs the arrangement of electrons in energy sublevels, indicating they fill from lowest to highest energy.
Energy Sublevel
- Refers to a group of atomic orbitals that have the same energy.
Energy Level
- Defined as a region of specific energy that electrons can occupy within an atom.
Methods to Energise Atoms
- Atoms can be energised by supplying heat or electricity.
Spectrum
- A spectrum is a range of colors produced when light is dispersed into different wavelengths, used for identifying gases or elements.
Balmer Series
- The visible series of light produced by transitions in hydrogen's electron energy levels.
Continuous vs Emission Spectrum
- Continuous spectrum displays a full range of colors without gaps.
- Emission spectrum features distinct lines that correspond to specific wavelengths of light emitted by atoms.
Atomic Absorption Spectrometer
- Instrument used to measure the presence and concentration of an element in a sample.
Electron Energy Transition
- According to Bohr's theory, an electron emits a definite amount of energy as light when moving from a higher to a lower energy level.
Energy Level Difference Formula
- The energy difference can be calculated using the equation E - E = hf, where h is Planck's constant and f represents the frequency of the emitted light.
Hund’s Rule
- Electrons will occupy available orbitals singly before pairing up in any orbital.
Pauli’s Exclusion Principle
- When two electrons occupy the same orbital, they must have opposite spins.
Electron Capacity of Orbitals
- Each orbital can hold a maximum of 2 electrons.
Orbital Shapes
- The s orbital has a spherical shape; the p orbital is characterized by a dumbbell shape.
Evidence Supporting Bohr Theory
- Line emission spectrums serve as evidence for the existence of quantized energy levels in atoms.
Electron States
- An electron can exist in two states: Ground state (n=1) or Excited state (n>1).
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Description
This quiz explores key concepts in quantum mechanics, including limitations of the Bohr theory, the Heisenberg Uncertainty Principle, and atomic orbitals. Test your understanding of how these fundamental principles shape our knowledge of electrons and their behavior. Perfect for students of physics!
