Unit 4 The Bohr Model Revisited OW
Select the correct electron configuration for Boron. (Atomic Number 5) *1s²2s³ *1s²2s¹2p² *1s³2s¹2p¹ *1s²2s²2p¹
*1s²2s²2p¹
Select the correct electron configuration for Vanadium. (Atomic Number 23) *1s²2s⁶2p³3s ²3p⁴4s²3d⁵ *1s²2s²2p⁶3s ²3p⁸4s²3d¹ *1s²2s²2p⁶3s ²3p⁶4s²3d³ *1s²2s²2p⁵3s ²3p⁷4s¹3d⁴
*1s²2s²2p⁶3s ²3p⁶4s²3d³
If an atom has 3 energy levels, how many sublevels should it have? *1 *2 *3 *4
*3
The maximum number of energy sublevels found in any energy level is: *2 *3 *4 *6
*4
What is meant by "the energy of an electron is quantized"? *The quantity of electron energy can be measured. *Each electron around an atom has a discrete amount of energy. *The quantity of electron energy changes as it moves around the nucleus. *all of the above
*Each electron around an atom has a discrete amount of energy.
Why do the elements of period 4 start a new cycle of properties after the element argon? Select all that apply. *The electrons in the outermost energy level are primarily responsible for the properties of an element. *The n = 3 energy level of argon is complete. *Additional electrons after argon begin to fill a sublevel of the n = 4 energy level. *All the energy levels of period 4 elements are less than period 3 because the amount of energy between energy levels decrease with distance from the nucleus.
*The electrons in the outermost energy level are primarily responsible for the properties of an element. *Additional electrons after argon begin to fill a sublevel of the n = 4 energy level.
Choose the correct abbreviation of potassium (K) written in its noble gas configuration *[Ar]4s¹ *[Ar]3p⁶4s¹ *[Ar]3p⁶ *[Kr]5s¹
*[Ar]4s1
The light emitted by an incandescent element produces: *a unique continuous spectrum *a line emission spectrum *a spectrum identical to the hydrogen atom *a spectrum of one unique wavelength
*a line emission spectrum
Complete the sentence. Select all that apply. The use of the term "energy levels" in the text implies: *s, p, d, f *a quantized amount of energy found at the dfferent levels *n = 1, 2, 3, ... *orbitals *groups
*a quantized amount of energy found at the different levels *n = 1, 2, 3, ...
What causes the lines in the emission spectrum for elements? *a continuous release of energy from the heated element *a quantum absorption of energy as various electrons are *excited to a higher energy level *a quantum release of energy as electrons drop back to their *ground state *none of the above
*a quantum release of energy as electrons drop back to their ground state
The quantum theory of energy levels within atoms was aided by: *study of the sun's light spectrum *emission line spectra of various elements *alpha particles *gamma rays
*emission line spectra of various elements
Which statement applies to the energy change illustrated in the quantized energy emission diagram? *energy added > energy released *energy added < energy released *energy added = energy released
*energy added = energy released
Which requires more energy to move an electron? *from n = 3 to n = 4 *from n = 2 to n = 3 *from n = 1 to n = 2
*from n = 1 to n = 2
Which condition will release more energy when an electron changes levels? *from n = 4 to n = 3 *from n = 3 to n = 2 *from n = 2 to n = 1
*from n = 2 to n = 1
Where would electrons in the d sublevel be found? *only in the n = 3 energy level *in energy levels >= 3 *possibly in any energy level
*in energy levels >= 3
What are energy sublevels? *multiple energy levels of any magnitude within an energy level *multiple orbitals of specific magnitude within an energy level *only those energy levels that overlap others *electrons whose energy has dropped to a lower state
*multiple orbitals of specific magnitude within an energy level
Where would the electrons in the 3d sublevel be found? *only in the n = 3 energy level *in energy levels > 3 *possibly in any shell
*only in the n = 3 energy level
A principal quantum number refers to: *the numbered energy levels starting from the nucleus outward *the total energy of an electron *the maximum number of electrons at a given level *the s, p, d, f levels
*the numbered energy levels starting from the nucleus outward
What is the maximum number of electrons in the following energy level? n = 3
18
What is the maximum number of electrons in the following energy level? n = 1
2
What is the atomic number of the first element to start filling a d sublevel?
21
What is the maximum number of electrons found in any energy level of the known elements? (Refer to the periodic table.)
32
What is the maximum number of electrons in the following energy level? n = 4
32
What is the theoretical maximum number of electrons in the n = 5 energy level?
50
What is the maximum number of electrons in the following energy level? n = 2
8
Research has shown that the electrons orbit the nucleus in circular motions exactly as shown on the classic Bohr model. True False
False
The broad bands or regions located around the nucleus where the electrons are found are called energy rings. True False
False
The light reflected off an element produces unique identifying spectrum. True False
False
The sequence of filling the electron configuration of the elements is not indicated in the periodic table. True False
False
Scientists have not yet determined exactly why electrons do not collapse into the nucleus. True False
True
maximum number of electrons = 10
d
The distribution of light when passed through a prism or other device that breaks the light into its individual components.
emission spectrum
The broad bands or regions located around the nucleus where the electrons are found.
energy level
maximum number of electrons = 14
f
maximum number of electrons = 6
p
Energy available or given off in specific, predictable quantities.
quantum
maximum number of electrons = 2
s
