Question

use each of the terms below to complete the statements.

atomic emission spectrum electron frequencies ground state higher energy levels lower

1. the lowest allowable energy state of an atom is called its
2. bohrs model of the atom predicted the of the lines in hydrogens atomic emission spectrum.
3. according to bohrs atomic model, the smaller an electrons orbit, the the atoms energy level.
4. according to bohrs atomic model, the larger an electrons orbit, the the atoms energy level.
5. bohr proposed that when energy is added to a hydrogen atom, its moves to a higher - energy orbit.
6. according to bohrs atomic model, the hydrogen atom emits a photon corresponding to the difference between the associated with the two orbits it transitions between.
7. bohrs atomic model failed to explain the of elements other than hydrogen.

circle the term in parentheses that correctly completes the statement.

1. atomic orbitals (do, do not) have an exactly defined size.
2. each orbital may contain at most (two, four) electrons.
3. all s orbitals are (spherically shaped, dumbbell shaped).
4. a principal energy has (n, n²) energy sublevels.
5. the maximum number of (electrons, orbitals) related to each principal energy level equals 2n²
6. there are (three, five) equal energy p orbitals.
7. sulfurs principal energy level 3 consists of (four, three) orbitals.

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Explanation:

1. The ground state is defined as the lowest - energy state of an atom.
2. Bohr's model used energy level transitions to predict the frequencies of lines in hydrogen's atomic emission spectrum.
3. In Bohr's model, smaller electron orbits correspond to lower energy levels.
4. Larger electron orbits in Bohr's model correspond to higher energy levels.
5. When energy is added to a hydrogen atom (in Bohr's model), the electron moves to a higher - energy orbit.
6. The hydrogen atom emits a photon corresponding to the energy difference between the energy levels of the two orbits it transitions between.
7. Bohr's model was mainly successful for hydrogen and failed for the atomic emission spectra of other elements.
8. Atomic orbitals do not have an exactly defined size as they represent probability regions for electrons.
9. Each orbital can hold a maximum of two electrons (Pauli exclusion principle).
10. All s orbitals are spherically shaped.
11. A principal energy level \(n\) has \(n\) energy sublevels (e.g., \(n = 2\) has \(s\) and \(p\) sublevels).
12. The formula for the maximum number of electrons in a principal energy level is \(2n^{2}\).
13. There are three equal - energy p orbitals (\(p_{x}\), \(p_{y}\), \(p_{z}\)).
14. Sulfur's principal energy level 3 (\(n=3\)) has \(s\), \(p\), and \(d\) sublevels. The number of orbitals in \(n = 3\) is \(n^{2}=9\) (1 \(s\) orbital, 3 \(p\) orbitals, 5 \(d\) orbitals). But if we consider the sum of \(s\), \(p\) orbitals (\(l = 0\) and \(l=1\)), there are \(1 + 3=4\) orbitals (the \(d\) orbitals are also part of \(n = 3\), but if we assume a basic consideration of filling order where \(3s\) and \(3p\) are filled before \(3d\) in some simple models, the number of orbitals from \(s\) and \(p\) sublevels in \(n = 3\) is \(4\)).

Answer:

1. ground state
2. frequencies
3. lower
4. higher
5. electron
6. energy levels
7. atomic emission spectrum
8. do not
9. two
10. spherically shaped
11. \(n\)
12. electrons
13. three
14. four