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What property describes how much energy must be added to an atom to remove an outermost electron?
The process is absorption of a photon. When energy like this is added to the system, if enough is added, then an electron can be ejected from the atom. The relevant theory involved with this is called 'band-gap' theory. Electrons are Fermions and as such obey the Pauli exclusion principle. This demands that no two electrons can occupy the same quantum state. Energy is quantised and therefore electrons can only take distinct energy levels at each orbital around an atom. The orbitals close to the nucleus are most tightly bound which means they must be given a tremendous energy to leave the atom. But if all the available slots in a particular orbital are filled, then an electron bound to the atom must occupy the next orbital further out. When all but the outer shell is filled, the only place for an electron attached to the atom is in this outer shell. In some atoms these electrons can be given enough energy by a photon to leave the atom and they do so because there are no further orbitals to occupy. In Silicon, this band-gap is 1.1 electron-volts. The figure varies by material.
What two characteristics of liquid oxygen contradict predictions from the valence bond theory but are explained by the molecular orbital theory?
Liquid oxygen exhibits paramagnetism and a relatively low boiling point, characteristics that contradict predictions from the valence bond theory. Valence bond theory suggests that all electrons in O2 should be paired, leading to diamagnetism; however, molecular orbital theory accounts for the presence of unpaired electrons in the antibonding π* orbitals, resulting in paramagnetism. Additionally, the molecular orbital theory explains the lower boiling point of liquid oxygen compared to other diatomic molecules by considering the weaker intermolecular forces due to its electronic configuration.
What is the bond order of F2 according to the molecular orbital theory?
According to molecular orbital theory, the bond order of F2 can be calculated by using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2. In F2, there are 10 bonding electrons in the molecular orbitals and 4 antibonding electrons. Thus, the bond order is (10 - 4) / 2 = 3. Therefore, the bond order of F2 is 3, indicating a strong bond between the two fluorine atoms.
Why oxyzen is paramagnetic explain it forrm mo theory?
Oxygen is paramagnetic due to the presence of two unpaired electrons in its molecular orbital configuration. In molecular orbital theory, oxygen molecule (O2) consists of two oxygen atoms, each contributing one unpaired electron to form pi* anti-bonding molecular orbitals. These unpaired electrons make oxygen molecule paramagnetic, which means it is attracted to a magnetic field.
What is the first energy level in helium called?
The first energy level in the quantum (current) theory of the atom is the 1s electron orbital, which can hold two electrons.The following energy levels go like this:1s22s22p63s23p64s24p63d105s25p64d106s2...And so on. (The first number being the energy level, the letter being the shape of the electron orbital, and the superscript being the number of electrons the orbital can hold.)
What is the difference between the homo and lumo energy levels in molecular orbital theory?
In molecular orbital theory, the HOMO (highest occupied molecular orbital) is the highest energy level that contains electrons, while the LUMO (lowest unoccupied molecular orbital) is the lowest energy level that does not contain electrons. The difference between the HOMO and LUMO energy levels determines the reactivity and stability of a molecule.
How many electrons are present in an orbital formed from the overlap of two different atomic orbitals?
2 electrons. Each orbital can only have a maximum of 2 electrons according to quantum mechanics and more specifically Paulis theory... The over lap is occurring because each orbital only has 1 electron so the over lap when finished will have 2.
What are paired electrons?
Pi electron pairs are electron pairs residing in the p orbital (as in s, p, d, f). This is the electron orbital responsible for double bonds and conjugated molecules according to molecular orbital theory.
What is covalent bond theory?
A covalent bond forms when the orbitals of two atoms overlap and a pair of electrons occupy the overlap region is called covalent bond theory
What property describes how much energy must be added to an atom to remove an outermost electron?
The process is absorption of a photon. When energy like this is added to the system, if enough is added, then an electron can be ejected from the atom. The relevant theory involved with this is called 'band-gap' theory. Electrons are Fermions and as such obey the Pauli exclusion principle. This demands that no two electrons can occupy the same quantum state. Energy is quantised and therefore electrons can only take distinct energy levels at each orbital around an atom. The orbitals close to the nucleus are most tightly bound which means they must be given a tremendous energy to leave the atom. But if all the available slots in a particular orbital are filled, then an electron bound to the atom must occupy the next orbital further out. When all but the outer shell is filled, the only place for an electron attached to the atom is in this outer shell. In some atoms these electrons can be given enough energy by a photon to leave the atom and they do so because there are no further orbitals to occupy. In Silicon, this band-gap is 1.1 electron-volts. The figure varies by material.
Why is oxygen molecule paramagnetic?
Answer 1) O2 molecule has two unpaired electrons which is only proved by Molecular orbitals theory (M.O.T). the M.O.T may be checked in any standard book of Inorganic chemistry.Answer 2) If you examine the orbital diagram for dioxygen, it contains a SOMO (Singly-Occupied Molecular Orbital) with 2 unpaired electrons. Dinitrogen does not have this. These unpaired electrons contribute to magnetism.
What two characteristics of liquid oxygen contradict predictions from the valence bond theory but are explained by the molecular orbital theory?
Liquid oxygen exhibits paramagnetism and a relatively low boiling point, characteristics that contradict predictions from the valence bond theory. Valence bond theory suggests that all electrons in O2 should be paired, leading to diamagnetism; however, molecular orbital theory accounts for the presence of unpaired electrons in the antibonding π* orbitals, resulting in paramagnetism. Additionally, the molecular orbital theory explains the lower boiling point of liquid oxygen compared to other diatomic molecules by considering the weaker intermolecular forces due to its electronic configuration.
What are the key differences between valence bond theory and molecular orbital theory in explaining chemical bonding?
Valence bond theory focuses on the overlap of atomic orbitals to form bonds between atoms, emphasizing the localized nature of bonding. Molecular orbital theory considers the entire molecule as a whole, with electrons delocalized over the entire molecule, leading to the formation of molecular orbitals.
Molecular orbital theory is based upon which model of the atom?
Molecular orbital theory determines molecular structure that the electrons are not assigned as individual bonds between atoms, however, are treated as moving under the influence of the nuclei in the whole molecule.
What is the bond order of F2 according to the molecular orbital theory?
According to molecular orbital theory, the bond order of F2 can be calculated by using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2. In F2, there are 10 bonding electrons in the molecular orbitals and 4 antibonding electrons. Thus, the bond order is (10 - 4) / 2 = 3. Therefore, the bond order of F2 is 3, indicating a strong bond between the two fluorine atoms.
Why oxyzen is paramagnetic explain it forrm mo theory?
Oxygen is paramagnetic due to the presence of two unpaired electrons in its molecular orbital configuration. In molecular orbital theory, oxygen molecule (O2) consists of two oxygen atoms, each contributing one unpaired electron to form pi* anti-bonding molecular orbitals. These unpaired electrons make oxygen molecule paramagnetic, which means it is attracted to a magnetic field.
What are the main three parts of an electrons used in the current atomic theory that describe an electrons location?
An electron configuration shows the distribution of electrons among the subshells. Each number shows the principal quantum number, or shell, the subshell and finally the orbital of the electron.
