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Questions and Answers
What is the main difference between an energy level and an atomic orbital?
What is the electron configuration (s, p) of an atom of silicon in its ground state?
How many main energy levels are occupied in the ground state of a silicon atom?
How many atomic orbitals are occupied by a silicon atom in its ground state?
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What was the purpose of Millikan’s 'oil drop' experiments from 1908 to 1913?
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Which term refers to a fixed energy value of an electron in an atom?
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How many electrons are present in the 3d subshell of an iron atom?
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Which subshell is filled after the 4s subshell in an iron atom's electron configuration?
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In which subshell does the last electron reside in an iron atom's ground state configuration?
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'To measure the magnitude of the charge on an electron' describes the purpose of which experiment?
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How many electrons are present in each p orbital when all three p orbitals are half-filled?
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Study Notes
Bohr's Contribution to Atomic Theory
- Niels Bohr provided insights into electron arrangement in atoms through his study of atomic spectra.
- When white light passes through a prism, it produces a continuous spectrum; Bohr focused on hydrogen's emission spectrum, which consists of narrow colored lines.
- Each element has a unique emission spectrum, important for element identification.
Spectroscopy Tools
- A spectrometer measures light wavelength; a spectroscope observes spectra without measuring wavelengths.
- Flame tests can identify metals based on the color they produce when burned:
- Lithium: Crimson
- Potassium: Lilac
- Barium: Green
- Strontium: Red
- Copper: Blue-green
- Sodium: Yellow
Bohr's Theory of Electron Energy Levels
- Electrons possess fixed energy values called quanta, moving in defined paths or orbits (energy levels).
- Energy levels are labeled with 'n', starting with n=1 as the lowest.
- Atoms in the ground state have electrons at the lowest energy levels; they absorb energy to jump to excited states.
Ground and Excited States
- Ground state: Electrons occupy the lowest energy levels available.
- Excited state: Electrons occupy higher energy levels, becoming unstable and eventually returning to the ground state while emitting energy as light.
- Energy difference between levels corresponds to emitted light frequency, defined by the equation E2 – E1 = hf, where 'h' is Planck's constant, and 'f' is frequency.
Emission Spectra and the Balmer Series
- Electrons falling to the n=2 energy level produce visible light, called the Balmer Series, identifiable by specific colored lines in the emission spectrum.
Atomic Absorption Spectrometry (AAS)
- Atoms also absorb specific wavelengths of light, creating an Atomic Absorption Spectrum where certain wavelengths are missing.
- Ground state atoms absorb the same wavelengths they emit when excited.
- AAS is utilized for analyzing metals in water, blood samples, and forensic applications, reflecting the absorbed light's correlation with the element's concentration.
Energy Sublevels
- Energy levels above n=1 include sublevels, subdivisions containing orbitals of identical energy.
- The number of sublevels matches the energy level’s principal quantum number (n), e.g., n=2 has 2 sublevels.
Wave-Particle Duality
- Louis de Broglie proposed that all moving particles, including electrons, have associated wave motion.
- Werner Heisenberg formalized this with the Uncertainty Principle, stating simultaneous measurement of an electron's velocity and position is impossible, challenging Bohr's model.
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Description
Test your knowledge on the Balmer Series of emission lines, where electrons transition from n=2 energy level, and the principles of Atomic Absorption Spectrometry (AAS) in analyzing samples. Explore the relationship between energy levels, frequency of emitted light, and Planck's constant.
