Podcast
Questions and Answers
What is the term used to describe the specific paths that electrons follow around the nucleus?
What is the term used to describe the specific paths that electrons follow around the nucleus?
- Energy shells
- Quantum levels
- Energy bands
- Orbits (correct)
In which state do atoms have the lowest possible amount of energy?
In which state do atoms have the lowest possible amount of energy?
- Excited state
- Ground state (correct)
- Ionized state
- Free state
What occurs when an electron absorbs energy and moves to a higher energy level?
What occurs when an electron absorbs energy and moves to a higher energy level?
- Ionization
- Photon emission
- Excitation (correct)
- Condensation
How is the energy of the electron in a particular orbit characterized according to Bohr's theory?
How is the energy of the electron in a particular orbit characterized according to Bohr's theory?
What type of spectrum is produced when light from a Hydrogen Gas Discharge Tube is passed through a prism?
What type of spectrum is produced when light from a Hydrogen Gas Discharge Tube is passed through a prism?
What device is used to measure the wavelength of the bands of light in a spectrum?
What device is used to measure the wavelength of the bands of light in a spectrum?
What happens to an electron in an atom when it is in an excited state?
What happens to an electron in an atom when it is in an excited state?
Which of the following elements would produce a crimson flame during a flame test?
Which of the following elements would produce a crimson flame during a flame test?
What occurs when energy is supplied to an atom in its ground state?
What occurs when energy is supplied to an atom in its ground state?
Which statement correctly defines the ground state of an atom?
Which statement correctly defines the ground state of an atom?
What happens to the excess energy when an electron falls back to the ground state?
What happens to the excess energy when an electron falls back to the ground state?
What is the relationship between the energy levels and the frequency of emitted light?
What is the relationship between the energy levels and the frequency of emitted light?
What is an Atomic Absorption Spectrum?
What is an Atomic Absorption Spectrum?
Which of the following is NOT a use of Atomic Absorption Spectrometry?
Which of the following is NOT a use of Atomic Absorption Spectrometry?
What principle does an Atomic Absorption Spectrometer operate on?
What principle does an Atomic Absorption Spectrometer operate on?
Which emissions line series is responsible for the emission of visible light when electrons fall to the n=2 energy level?
Which emissions line series is responsible for the emission of visible light when electrons fall to the n=2 energy level?
What defines a sublevel in an energy level?
What defines a sublevel in an energy level?
How does the number of sublevels relate to the main energy level denoted as 'n'?
How does the number of sublevels relate to the main energy level denoted as 'n'?
What is the significance of the wave-particle duality of electrons?
What is the significance of the wave-particle duality of electrons?
What limitation does Bohr’s theory have concerning multi-electron atoms?
What limitation does Bohr’s theory have concerning multi-electron atoms?
What shape is described by a 'p' orbital?
What shape is described by a 'p' orbital?
What does the Uncertainty Principle state regarding electrons?
What does the Uncertainty Principle state regarding electrons?
How many total electrons can be found in an 's' sublevel?
How many total electrons can be found in an 's' sublevel?
In atomic absorption spectrometry, what is the relationship between light absorption and element concentration?
In atomic absorption spectrometry, what is the relationship between light absorption and element concentration?
Flashcards
Excited State
Excited State
An atom's state when electrons occupy higher energy levels than in the ground state.
Ground State
Ground State
The lowest energy level an electron can occupy in an atom.
Energy Level
Energy Level
A fixed energy value that an electron in an atom can have.
Atomic Absorption Spectrometry (AAS)
Atomic Absorption Spectrometry (AAS)
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Absorption Spectrum
Absorption Spectrum
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Emission Spectrum
Emission Spectrum
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Photon
Photon
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Balmer Series
Balmer Series
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What is a continuous spectrum?
What is a continuous spectrum?
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What is an emission (line) spectrum?
What is an emission (line) spectrum?
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Flame test
Flame test
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Spectrometer
Spectrometer
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Quantized energy
Quantized energy
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What happens when an electron absorbs energy?
What happens when an electron absorbs energy?
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What's a sublevel?
What's a sublevel?
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How many sublevels are there?
How many sublevels are there?
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What are orbitals?
What are orbitals?
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Describe an 's' orbital.
Describe an 's' orbital.
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Describe a 'p' orbital.
Describe a 'p' orbital.
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De Broglie's Idea
De Broglie's Idea
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Heisenberg's Uncertainty Principle
Heisenberg's Uncertainty Principle
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Limitations of Bohr's Model
Limitations of Bohr's Model
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Study Notes
Bohr's Model of the Atom
- Bohr, a Danish scientist, explained electron arrangement in atoms.
- When white light passes through a prism, it separates into a spectrum of colors (continuous spectrum).
- Bohr observed that light from hydrogen gas produced a line spectrum (discrete colors).
- Each element has a unique emission spectrum, useful for identification.
- Spectrometers measure wavelengths of light bands in spectra.
- Spectroscopes display spectra but don't measure wavelengths.
Flame Tests
- Flame tests identify elements.
- Damp wooden splints hold samples in a Bunsen burner flame.
- Record the color of flames for each element:
- Lithium – Crimson
- Potassium – Lilac
- Barium – Green
- Strontium – Red
- Copper – Blue-green
- Sodium – Yellow
The Bohr Theory
- Electrons orbit the nucleus in fixed energy levels (orbits).
- Electrons in a given level possess a fixed amount of energy.
- Energy levels are represented by 'n' (lowest is 'n=1').
- Electrons neither gain nor lose energy, while in a single energy level.
- Atoms normally exist in the ground state (lowest energy).
- Electrons can jump to higher energy levels (excited state) when absorbing energy.
- Absorbed energy equals the difference in energy between excited state and ground state.
- Electrons fall back emitting light with specific energies and corresponding colors.
- Frequency of emitted light depends on the difference in energy between levels.
- The energy difference is 'E₂ - E₁ = hf'.
- Coloured lines in spectra represent unique emitted frequencies from atoms.
Atomic Absorption Spectrometry (AAS)
- Atoms absorb specific wavelengths of light.
- This results in missing bands in a light spectrum passed through a gas sample.
- The absorbed wavelengths match emission wavelengths of excited atoms.
- AAS measures absorption spectra and is used to measure element concentrations.
- Applications include water analysis, measuring lead in blood, forensic science.
Energy Sublevels
- Energy levels (except 'n=1') are divided into sublevels.
- Sublevels are subdivisions within an energy level, of equal energy.
- Number of sublevels equals the value of 'n'.
- Examples: 'n=2' has 's' and 'p' sublevels, 'n=3' has 's', 'p', and 'd' sublevels.
Wave Nature of Electrons
- Electrons exhibit wave-like properties (wave-particle duality).
- This means electrons have a wave motion.
- This was mathematically described by de Broglie.
Heisenberg's Uncertainty Principle
- It's impossible to precisely determine an electron's position and velocity simultaneously.
- This limitation led to refinements of the Bohr model.
Atomic Orbitals
- Orbitals are regions with high chance of finding electrons.
- 's' orbitals are spherical, 'p' are dumbbell-shaped
- Elements have a corresponding number of electrons in each orbital.
- Atomic orbitals and their shapes describe the distribution of electrons in an atom.
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Description
Explore the fascinating concepts of Bohr's model of the atom and the practical applications of flame tests in identifying elements. This quiz covers the principles of electron arrangement, emission spectra, and the unique colors produced by various elements in flame tests. Test your knowledge and understanding of these fundamental topics in chemistry.
