p.8
Electron Capacity of Orbitals
What does the simple model of electron configuration explain?
It explains valency, the octet rule, and the 18-electron rule.
p.18
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What influences the bonding angle in the VSEPR model?
The repulsion between electron pairs.
p.17
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What does the VSEPR model stand for?
Valence-Shell Electron-Pair Repulsion model.
p.6
Electron Shells and Principal Quantum Number (n)
How many subshells are in Shell 2?
Two subshells (2s and 2p)
p.8
Electron Capacity of Orbitals
How many electrons can each orbital hold?
Each orbital can hold 2 electrons.
p.15
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What is the main principle of the VSEPR model?
Electron pairs around a central atom repel each other, determining the geometry of the molecule.
p.4
Orbitals and Magnetic Quantum Number (m_l)
How many orbitals does the f subshell have?
The f subshell has 7 orbitals (calculated as 2 x 4 - 1).
p.9
Electron Capacity of Orbitals
How many electrons can n = 3 hold?
18 electrons (2 from s, 6 from p, and 10 from d).
p.14
Electronic Configuration Examples
What is the electronic configuration of titanium (22 electrons)?
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d².
p.3
Orbitals and Magnetic Quantum Number (m_l)
How many orbitals are associated with each subshell?
Each subshell has (2n - 1) orbitals.
p.1
Atomic Structure Overview
What are the three main subatomic particles?
Protons, neutrons, and electrons.
p.18
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What does VSEPR stand for?
Valence-Shell Electron-Pair Repulsion.
p.18
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
How does the repulsion between free electron pairs affect bonding angles?
It results in a reduced bonding angle between bonding electron pairs.
What is energetically favorable in a subshell according to Hund's Rule?
To have half-filled orbitals with electrons that have parallel spins.
p.4
Orbitals and Magnetic Quantum Number (m_l)
How many orbitals are associated with each subshell?
Each subshell has (2n - 1) orbitals.
p.4
Subshells and Azimuthal Quantum Number (l)
At what principal quantum number does the f subshell start?
The f subshell starts at n = 4.
p.14
Electron Capacity of Orbitals
How do electrons fit into orbitals?
Electrons occupy orbitals according to specific rules such as the Aufbau principle, Pauli exclusion principle, and Hund's rule.
p.5
Electron Capacity of Orbitals
How many p orbitals are there and how many electrons can they hold in total?
3 p orbitals hold a total of 6 electrons (2 x 3).
p.15
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What types of electron pairs are considered in VSEPR theory?
Both bonding pairs and lone pairs of electrons.
p.2
Electron Shells and Principal Quantum Number (n)
What identifies each electron shell?
The principal quantum number, n.
p.10
Pauli Exclusion Principle
What does the Pauli Exclusion Principle state about electrons in an orbital?
Every electron must have a unique spin.
p.9
Subshells and Azimuthal Quantum Number (l)
What subshells are present in n = 3?
s, 3 x p, and 5 x d subshells.
p.9
Subshells and Azimuthal Quantum Number (l)
What subshells are present in n = 4?
s, 3 x p, 5 x d, and 7 x f subshells.
p.8
Electron Shells and Principal Quantum Number (n)
How many subshells does each shell have?
Each shell has n subshells.
p.15
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What does VSEPR stand for?
Valence-Shell Electron-Pair Repulsion.
p.9
Electron Capacity of Orbitals
What is the 18-electron rule?
A guideline for transition elements indicating stability with 18 electrons.
p.5
Electron Capacity of Orbitals
How many d orbitals are there and how many electrons can they hold in total?
5 d orbitals hold a total of 10 electrons (2 x 5).
p.10
Orbitals and Magnetic Quantum Number (m_l)
How are orbitals labeled?
Based on their principal quantum number and subshell type (e.g., 1s, 3p, 4d, 6f).
p.10
Aufbau Principle and Order of Filling
What are the tricky areas/rules to be aware of when filling orbitals?
Aufbau principle, Pauli Exclusion Principle, and Hund's Rule.
p.16
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What does the VSEPR model state about valence electrons in hybrid orbitals?
They will arrange themselves as far apart from each other as possible in space.
p.18
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What is the relationship between bonding electron pairs and free electron pairs in terms of repulsion?
Free electron pairs exert greater repulsion compared to bonding electron pairs.
p.4
Subshells and Azimuthal Quantum Number (l)
At what principal quantum number does the d subshell start?
The d subshell starts at n = 3.
p.5
Electron Capacity of Orbitals
How many f orbitals are there and how many electrons can they hold in total?
7 f orbitals hold a total of 14 electrons (2 x 7).
p.2
Electron Shells and Principal Quantum Number (n)
How are electrons organized in atoms?
Electrons are divided into shells.
p.13
Electron Capacity of Orbitals
How do electrons fit into orbitals?
Electrons occupy orbitals based on the order of filling and the capacity of each subshell.
p.4
Orbitals and Magnetic Quantum Number (m_l)
How many orbitals does the d subshell have?
The d subshell has 5 orbitals (calculated as 2 x 3 - 1).
p.9
Electron Capacity of Orbitals
What is the octet rule?
Atoms tend to have eight electrons in their valence shell.
p.15
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
How does VSEPR predict molecular shapes?
By considering the repulsion between electron pairs in the valence shell.
p.1
Atomic Structure Overview
What is the mass number of an atom?
The total number of protons and neutrons.
p.6
Electron Capacity of Orbitals
How many orbitals are in the 3d subshell?
Five orbitals (3d_xy, 3d_yz, 3d_xz, 3d_x^2-y^2, 3d_z^2)
p.13
Aufbau Principle and Order of Filling
What is the order of filling for electron orbitals?
1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d → 7p.
p.9
Electron Capacity of Orbitals
How many electrons can n = 4 hold?
32 electrons (2 from s, 6 from p, 10 from d, and 14 from f).
p.1
Atomic Structure Overview
What determines the atomic number of an element?
The number of protons in the nucleus.
p.15
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What are some common molecular shapes predicted by VSEPR?
Linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.
p.9
Electron Capacity of Orbitals
How many electrons can n = 2 hold?
8 electrons (2 from s and 6 from p).
p.8
Subshells and Azimuthal Quantum Number (l)
What is the subshell for n = 1?
It has only an s subshell, which holds 2 electrons.
p.1
Atomic Structure Overview
Where are electrons located in an atom?
In electron shells surrounding the nucleus.
p.15
Valence-Shell Electron-Pair Repulsion (VSEPR) Model
What is the effect of lone pairs on molecular geometry according to VSEPR?
Lone pairs occupy more space and can distort the bond angles between bonding pairs.
p.2
Subshells and Azimuthal Quantum Number (l)
How many subshells does the third shell have?
3 subshells, labeled s, p, and d.
p.9
Electron Capacity of Orbitals
What does the simple model of electron configuration explain?
Valency and the octet rule for first row elements.
p.11
Aufbau Principle and Order of Filling
What is the order of filling for orbitals?
1s → 2s → 2p → 3s → 3p → 3d → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d → 7p.
p.10
Aufbau Principle and Order of Filling
In what order are electrons added to orbitals?
In order of increasing energy.
p.2
Subshells and Azimuthal Quantum Number (l)
How is the number of subshells in a shell determined?
Each shell has n subshells, where n is the principal quantum number.
p.14
Aufbau Principle and Order of Filling
What is the order of filling for electron subshells?
1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d → 7p.
