Questions and Answers
What is the term for the set of frequencies of the electromagnetic waves emitted by the atoms of an element?
What is the minimum amount of energy that can be lost or gained by an atom called?
quantum
What is the form of energy that exhibits wavelike behavior as it travels through space?
electromagnetic radiation
What is a three-dimensional region around the nucleus of an atom that describes an electron's probable location?
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What is the shortest distance between equivalent points on a continuous wave?
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What is the lowest allowable energy state of an atom called?
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What is a particle of electromagnetic radiation with no mass that carries a quantum of energy?
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What is the emission of electrons from a metal's surface when light of a certain frequency shines on it called?
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What does the principal quantum number indicate?
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The relationship defined by the equation $c = \lambda v$ connects the speed of light, wavelength, and frequency.
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What is the orbital diagram and complete electron configuration for nitrogen?
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What is the orbital diagram and complete electron configuration for fluorine?
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What is the orbital diagram and complete electron configuration for sodium?
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Calculate the wavelength of the radiation emitted by a radio station with a frequency of 103.7 MHz.
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Microwaves are higher in frequency than radio waves.
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The atomic emission spectrum for each element would change if the same procedure is repeated.
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What does each line in an atomic emission spectrum represent?
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What conclusion can you draw if you compare the atomic emission spectrum of hydrogen to other samples?
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According to Bohr's model, how many times are photons emitted from the excited atoms in each sample?
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Explain how hydrogen's emission spectrum demonstrates that the difference between successive energy levels becomes smaller as n becomes larger.
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What would the absorption spectra look like if the chemist measured the photons absorbed instead of emitted?
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Study Notes
Atomic Emission Spectrum
- Describes frequencies of electromagnetic waves emitted by atomic elements.
- Each element has a unique atomic emission spectrum.
Quantum
- Represents the smallest amount of energy that can be lost or gained by an atom.
Electromagnetic Radiation
- Energy that exhibits wave-like properties as it travels through space.
Atomic Orbital
- A three-dimensional region around an atom's nucleus, indicating the probable location of electrons.
Wavelength
- Defined as the shortest distance between equivalent points on a continuous wave.
Ground State
- Refers to the lowest energy state of an atom.
Photon
- A massless particle of electromagnetic radiation carrying a quantum of energy.
Photoelectric Effect
- Occurs when electrons are emitted from a metal surface upon exposure to light with a certain frequency.
Principal Quantum Number
- Indicates the relative sizes and energies of atomic orbitals, representing major energy levels.
Frequency and Amplitude
- Frequency is the count of waves passing a point per second; Amplitude measures the wave height from origin to crest/trough.
Valence Electrons and Electron-Dot Structure
- Valence electrons are in an atom's outermost orbitals; Electron-dot structures depict valence electrons using dots.
Principal Energy Levels and Energy Sublevels
- Major energy levels (1 to 7) within an atom; Energy sublevels increase with the principal energy level's value.
Wave Equation
- c = λv relates the speed (c), wavelength (λ), and frequency (v) of electromagnetic waves.
Electron Configuration
- Nitrogen: 1s², 2s², 2p³
- Fluorine: 1s², 2s², 2p⁵
- Sodium: 1s², 2s², 2p⁶, 3s¹
- Aluminum: 1s², 2s², 2p⁶, 3s², 3p¹ and Noble-gas notation: [Ne]3s², 3p¹
- Iodine: Noble-gas notation [Kr]5s², 4d¹⁰, 5p⁵
Wavelength Calculation
- Wavelength of a radio station with frequency 103.7 MHz calculated as λ ≈ 2.892 m, falling between 10¹ m and 1 m in the electromagnetic spectrum.
Microwaves vs. Radio Waves
- Microwaves have higher frequency and shorter wavelength compared to radio waves.
Atomic Emission Spectra Observations
- Spectra indicate the identity of elements; identical spectra suggest the same element, differing spectra indicate different elements.
- Atomic emission spectra are unique for each element.
Absorption vs. Emission Spectra
- Dark lines in absorption spectra correspond to bright lines in emission spectra, reflecting energy absorption.
Bohr Model
- Only explains the emission spectrum of hydrogen and similar single-electron atoms.
- Indicates that the difference between successive energy levels diminishes as energy levels increase, demonstrated by closely spaced emission lines in hydrogen's spectrum.
Photon Emission
- Each line in an atomic emission spectrum corresponds to a photon of specific energy being emitted or absorbed, highlighting energy changes of electrons.
Spectral Repeatability
- Atomic emission spectra remain consistent across multiple measurements due to characteristic patterns unique to each element.
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Description
Test your knowledge on key concepts related to electrons in atoms with this flashcard quiz. Dive into topics such as atomic emission spectra, quantum energy levels, and electromagnetic radiation. Perfect for students studying chemistry at any level.
