The energy levels, emission spectra and atomic orbitals of an anti-hydrogen atom which is compared with a hydrogen atom and the colliding of an anti-atom with a hydrogen atom should be explained. Concept Introduction: For a quantum mechanical system or a particle that is bound can only take on certain discrete values of energy. This contrasts with classical particles, which can have any energy. These discrete values are called energy levels . Electrons in an atom can shift between the different energy levels corresponding to orbitals in different shells. An energy level is the measurement of discrete energy a subatomic particle, such as an electron, can absorb. When light or other energy strikes an atom, it can transfer some of that energy to its particles, raising their energy level. The arrangements of atomic orbitals are based upon energy levels of hydrogen atom. When electromagnetic radiation interacts with matter, atoms and molecules may absorb energy and reach to a higher energy state. With higher energy, these are in an unstable state. For returning to their normal (more stable, lower energy) energy state, the atoms and molecules emit radiations in various regions of the electromagnetic spectrum. The spectrum of radiation emitted by a substance that has absorbed energy is called an emission spectrum . The word, an atomic orbital is used rather than an orbit to differentiate the quantum mechanical description of an atom from Bohr’s model . An atomic orbital is the region of three-dimensional space defined by the square of the wave function of an electron in an atom where the probability of finding an electron is high. Therefore, an atomic orbital has a characteristic energy as well as a characteristic distribution of electron density. They have different shapes.
The energy levels, emission spectra and atomic orbitals of an anti-hydrogen atom which is compared with a hydrogen atom and the colliding of an anti-atom with a hydrogen atom should be explained. Concept Introduction: For a quantum mechanical system or a particle that is bound can only take on certain discrete values of energy. This contrasts with classical particles, which can have any energy. These discrete values are called energy levels . Electrons in an atom can shift between the different energy levels corresponding to orbitals in different shells. An energy level is the measurement of discrete energy a subatomic particle, such as an electron, can absorb. When light or other energy strikes an atom, it can transfer some of that energy to its particles, raising their energy level. The arrangements of atomic orbitals are based upon energy levels of hydrogen atom. When electromagnetic radiation interacts with matter, atoms and molecules may absorb energy and reach to a higher energy state. With higher energy, these are in an unstable state. For returning to their normal (more stable, lower energy) energy state, the atoms and molecules emit radiations in various regions of the electromagnetic spectrum. The spectrum of radiation emitted by a substance that has absorbed energy is called an emission spectrum . The word, an atomic orbital is used rather than an orbit to differentiate the quantum mechanical description of an atom from Bohr’s model . An atomic orbital is the region of three-dimensional space defined by the square of the wave function of an electron in an atom where the probability of finding an electron is high. Therefore, an atomic orbital has a characteristic energy as well as a characteristic distribution of electron density. They have different shapes.
Solution Summary: The author explains the energy levels, emission spectra, and atomic orbitals of an anti-hydrogen atom which is compared with a hydrogen
The energy levels, emission spectra and atomic orbitals of an anti-hydrogen atom which is compared with a hydrogen atom and the colliding of an anti-atom with a hydrogen atom should be explained.
Concept Introduction:
For a quantum mechanical system or a particle that is bound can only take on certain discrete values of energy. This contrasts with classical particles, which can have any energy. These discrete values are called energy levels. Electrons in an atom can shift between the different energy levels corresponding to orbitals in different shells. An energy level is the measurement of discrete energy a subatomic particle, such as an electron, can absorb. When light or other energy strikes an atom, it can transfer some of that energy to its particles, raising their energy level. The arrangements of atomic orbitals are based upon energy levels of hydrogen atom.
When electromagnetic radiation interacts with matter, atoms and molecules may absorb energy and reach to a higher energy state. With higher energy, these are in an unstable state. For returning to their normal (more stable, lower energy) energy state, the atoms and molecules emit radiations in various regions of the electromagnetic spectrum. The spectrum of radiation emitted by a substance that has absorbed energy is called an emission spectrum.
The word, an atomic orbital is used rather than an orbit to differentiate the quantum mechanical description of an atom from Bohr’s model. An atomic orbital is the region of three-dimensional space defined by the square of the wave function of an electron in an atom where the probability of finding an electron is high. Therefore, an atomic orbital has a characteristic energy as well as a characteristic distribution of electron density. They have different shapes.
What are the IUPAC Names of all the compounds in the picture?
1) a) Give the dominant Intermolecular Force (IMF) in a sample of each of the following
compounds. Please show your work. (8) SF2, CH,OH, C₂H₂
b) Based on your answers given above, list the compounds in order of their Boiling Point
from low to high. (8)
19.78 Write the products of the following sequences of reactions. Refer to your reaction road-
maps to see how the combined reactions allow you to "navigate" between the different
functional groups. Note that you will need your old Chapters 6-11 and Chapters 15-18
roadmaps along with your new Chapter 19 roadmap for these.
(a)
1. BHS
2. H₂O₂
3. H₂CrO4
4. SOCI₂
(b)
1. Cl₂/hv
2. KOLBU
3. H₂O, catalytic H₂SO4
4. H₂CrO4
Reaction
Roadmap
An alkene 5. EtOH
6.0.5 Equiv. NaOEt/EtOH
7. Mild H₂O
An alkane
1.0
2. (CH3)₂S
3. H₂CrO
(d)
(c)
4. Excess EtOH, catalytic H₂SO
OH
4. Mild H₂O*
5.0.5 Equiv. NaOEt/EtOH
An alkene 6. Mild H₂O*
A carboxylic
acid
7. Mild H₂O*
1. SOC₁₂
2. EtOH
3.0.5 Equiv. NaOEt/E:OH
5.1.0 Equiv. NaOEt
6.
NH₂
(e)
1. 0.5 Equiv. NaOEt/EtOH
2. Mild H₂O*
Br
(f)
i
H
An aldehyde
1. Catalytic NaOE/EtOH
2. H₂O*, heat
3. (CH,CH₂)₂Culi
4. Mild H₂O*
5.1.0 Equiv. LDA
Br
An ester
4. NaOH, H₂O
5. Mild H₂O*
6. Heat
7.
MgBr
8. Mild H₂O*
7. Mild H₂O+
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell