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Chapter 05 – Text Questions
Electrons in Atoms
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Directions: Answer each of the following questions using the text or other sources.
Section 5.1
1) Why did scientists consider Rutherford’s nuclear model of the atom incomplete?
2) List the four characteristic properties of all waves. At what speed do electromagnetic waves travel in a vacuum?
3) Compare the wave and particle models of light. What phenomena can only be explained by the particle model?
4) What is a quantum of energy? Explain Planck’s quantum concept as it relates to energy lost or gained by matter.
5) Explain the difference between the continuous spectrum of white light and the atomic emission spectrum of an element.
6) Explain how the gaseous neon atoms in a neon sign emit light.
7) List the seven regions of the EM spectrum in order of the increasing wavelength.
Section 5.2
1) According to the Bohr atomic model, why do atomic emission spectra contain only certain frequencies of light?
2) Why is the wavelength of a moving soccer ball not detectable to the naked eye?
3) What sublevels are contained in the hydrogen atom’s first four energy levels? What orbitals are related to each s
sublevel and each p sublevel?
4) Thinking critically, use deBroglie’s wave-particle duality and the Heisenberg uncertainty principle to explain why the
location of an electron in an atom is uncertain.
5) What is the difference between an atom’s ground state and an excited state?
6) According to the Bohr model, how do electrons move in atoms?
Chapter 05 – Text Questions
Electrons in Atoms
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Hour:
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7) What does n designate in Bohr’s atomic model? What does n represent in the quantum mechanical model of the atom?
8) What is the name of the atomic model in which electrons are treated as waves?
9) What is the maximum number of electrons an orbital may contain?
10) What is the probability that an electron will be found within an atomic orbital?
11) How many energy sublevels are contained in each of the hydrogen atom’s first three energy levels?
12) What do the sublevel designations s, p, d, and f specify with respect to the atom’s orbitals?
13) Why is it impossible to know precisely the velocity and position of an electron at the same time?
Section 5.3
1) State the Aufbau principle in your own words.
2) Explain the meaning of the Aufbau principle as it applies to atoms with many electrons.
3) In what sequence do electrons fill the atomic orbital related to a sublevel?
4) Why must two arrows within a single block of an orbital diagram be written in opposite (up and down) directions?
5) How does noble-gas notation shorten the process of writing an element’s electrons configuration?
6) Light is said to have a dual wave-particle nature. What does this statement mean?
7) Describe the difference between a quantum and photons.
Chapter 05 – Text Questions
Electrons in Atoms
Name:
Hour:
Date:
Directions: Define each of the following terms. For some of the terms, you may need to consult sources other than your
textbook, such as a dictionary or encyclopedia.
Vocabulary Word
amplitude
atomic emission
spectrum
atomic orbital
Aufbau principle
electromagnetic
radiation
electromagnetic
spectrum
electron configuration
electron-dot structure
energy sublevel
frequency
ground state
Heisenberg uncertainty
principle
Hund’s rule
Pauli exclusion
principle
photoelectric effect
photon
principal energy level
Definition
Example/Diagram
Chapter 05 – Text Questions
Electrons in Atoms
principal quantum
number
quantum
quantum mechanical
model of the atom
valence electron
wavelength
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