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Questions and Answers
What happens to energy as wavelength increases?
What happens to energy as wavelength increases?
Which type of radiation has the shortest wavelengths?
Which type of radiation has the shortest wavelengths?
What defines a line spectrum?
What defines a line spectrum?
Which of the following statements about frequency is true?
Which of the following statements about frequency is true?
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What portion of the electromagnetic spectrum does visible light occupy?
What portion of the electromagnetic spectrum does visible light occupy?
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How is the electromagnetic spectrum generally arranged?
How is the electromagnetic spectrum generally arranged?
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Which statement correctly describes the relationship between wavelength and frequency?
Which statement correctly describes the relationship between wavelength and frequency?
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What role do emission spectra play in atomic models?
What role do emission spectra play in atomic models?
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Which orbital designation is NOT considered legitimate?
Which orbital designation is NOT considered legitimate?
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What does an electron configuration denote?
What does an electron configuration denote?
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What is indicated by the superscript in an electron configuration?
What is indicated by the superscript in an electron configuration?
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In an orbital diagram, how are paired electrons represented?
In an orbital diagram, how are paired electrons represented?
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What is the primary purpose of quantum mechanics (QM) in relation to atomic orbitals?
What is the primary purpose of quantum mechanics (QM) in relation to atomic orbitals?
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Which of the following shapes is correctly associated with the f orbitals?
Which of the following shapes is correctly associated with the f orbitals?
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How many sublevels are present in the principal energy level when n = 3?
How many sublevels are present in the principal energy level when n = 3?
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Which of the following statements about electron spin is accurate?
Which of the following statements about electron spin is accurate?
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Which of the following statements about atomic orbitals is true?
Which of the following statements about atomic orbitals is true?
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Which of the following best describes orbital energy levels?
Which of the following best describes orbital energy levels?
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Which sublevel can be occupied at the principal quantum number n=3?
Which sublevel can be occupied at the principal quantum number n=3?
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Which sublevel corresponds to the principal quantum number n = 2?
Which sublevel corresponds to the principal quantum number n = 2?
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What does an electron density map represent?
What does an electron density map represent?
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What did Niels Bohr utilize to conceive his atomic model?
What did Niels Bohr utilize to conceive his atomic model?
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What is the lowest energy level of an electron in a hydrogen atom according to the Bohr model?
What is the lowest energy level of an electron in a hydrogen atom according to the Bohr model?
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What occurs when a hydrogen atom absorbs energy?
What occurs when a hydrogen atom absorbs energy?
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What is the main limitation of the Bohr model when it comes to multiple electron atoms?
What is the main limitation of the Bohr model when it comes to multiple electron atoms?
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What does the quantum mechanical model define instead of specific electron locations?
What does the quantum mechanical model define instead of specific electron locations?
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Which characteristic of orbitals differentiates the quantum mechanical model from the Bohr model?
Which characteristic of orbitals differentiates the quantum mechanical model from the Bohr model?
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What happens when an electron relaxes back to a lower-energy orbit?
What happens when an electron relaxes back to a lower-energy orbit?
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What quantum mechanical concept conflicts with the idea of fixed electron orbits?
What quantum mechanical concept conflicts with the idea of fixed electron orbits?
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What type of ion is formed when an atom loses one or more electrons?
What type of ion is formed when an atom loses one or more electrons?
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Which trend is observed for an atom regarding electron loss and gain across a period in the periodic table?
Which trend is observed for an atom regarding electron loss and gain across a period in the periodic table?
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What is the term used for atoms that achieve a noble gas electron configuration?
What is the term used for atoms that achieve a noble gas electron configuration?
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What charge does an atom acquire when it gains one or more electrons?
What charge does an atom acquire when it gains one or more electrons?
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Which of the following correctly identifies an atom maintaining equal numbers of protons and electrons?
Which of the following correctly identifies an atom maintaining equal numbers of protons and electrons?
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In terms of charge, how does an atom become a cation?
In terms of charge, how does an atom become a cation?
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Which process is primarily involved in an atom achieving isoelectronic status?
Which process is primarily involved in an atom achieving isoelectronic status?
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What can be predicted about the ions formed by main-group elements according to the content?
What can be predicted about the ions formed by main-group elements according to the content?
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Study Notes
Atomic Orbitals
- The shapes of f orbitals are highly complex.
- Atomic orbital energy levels are more complex for multi-electron atoms.
- The sub-level designation 1p is not a legitimate designation because the principal quantum number, n, cannot be equal to 1 for a p sub-level.
- Sub-Level Designation 2s, 3f, and 4p are legitimate.
Electron Configurations
- The behavior of an atom depends on its electron configuration, which describes the specific arrangement of electrons within the atom's orbitals.
- Electron configurations are written as a series of numbers and letters indicating occupied energy sublevels, with the superscript indicating the number of electrons in the sublevel.
Orbital Diagrams
- An orbital diagram uses a square box to represent each orbital, which is labelled with the n value and s, p, d, or f designation.
- Orbital diagrams also use arrows to represent each electron.
- The first electron in an orbital is usually represented with an arrow pointing upward. The second electron in an orbital must point downward.
Nature of Light
- Wavelength (λ) is the distance between identical points on consecutive waves, such as the distance between two crests.
- Frequency (ν) is the number of waves that pass through a particular point in one second.
- As wavelength increases, energy decreases, and as frequency increases, energy increases.
- The electromagnetic spectrum arranges all types of electromagnetic radiation (light), from gamma rays, which have the shortest wavelengths, to radio waves, which have the longest wavelengths.
- Line Spectra are emission spectra that are not continuous, but contain only discrete lines.
- The line spectra of elements are critical to developing our understanding of atomic models.
The Bohr Atom
- Photons, tiny discrete packets of light, were used by Danish physicist Niels Bohr to create a model of the atom, which is now known as the Bohr atom, in conjunction with the line spectrum of hydrogen.
- The concentric circular paths around the nucleus in Bohr's model are called orbits, and each orbit is at a specific energy level designated by a quantum number, n.
- The electron in the hydrogen atom resides at the lowest possible energy level (n = 1), called the ground state.
- The Bohr model explained the observed line spectra of hydrogen but failed to explain the spectra of any other elements.
Quantum Mechanical Model
- The quantum mechanical (QM) model replaced the Bohr model.
- The QM model does not define the location of an electron, instead, it defines a region of space called an orbital where an electron is most likely to be found.
- QM orbitals vary in shape, as opposed to Bohr's orbits, which were all circular and only varied in size.
Electron Density Map
- Probability density maps for electrons can be calculated using the mathematics of QM, creating a visual representation called an atomic orbital.
Electron Configuration and Periodic Trends
- The number of energy sublevels in each principal energy level, n, is equal to the principal quantum number.
- The number of orbitals contained in each sublevel is equal to 2l + 1.
- Each orbital can contain a maximum of two electrons.
- Elements in the same group (column) of the periodic table have the same number of valence electrons.
- Valence electrons are the electrons in the outermost shell of an atom.
Ions
- An ion is an atom in which the number of electrons is not equal to the number of protons.
- Cations are atoms that have lost one or more electrons and become positively charged.
- Anions are atoms that have gained one or more electrons and become negatively charged.
- Atoms of main-group elements will lose or gain electrons to achieve a noble gas electron configuration - This is referred to as being isoelectronic.
- The loss or gain of electrons allows predictions of the ion's charge.
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Description
This quiz explores the concepts of atomic orbitals, electron configurations, and orbital diagrams. You will learn about the legitimacy of sub-level designations and how to interpret electron arrangements within atoms. Test your understanding of these fundamental principles in atomic structure.