p.5
Electron Configurations
What should we understand to determine electron configurations in multi-electron atoms?
The energies of the atomic orbitals.
p.19
Electron Configurations
What are the four types of electron blocks in the periodic table?
f block, d block, s block, p block.
p.7
Pauli Exclusion Principle
What does the Pauli Exclusion Principle state?
No two electrons in an atom can have the same four quantum numbers; a maximum of two electrons can occupy the same orbital with opposite spins.
What does Hund's Rule state about electron pairing in degenerate orbitals?
Electrons will not pair in degenerate orbitals if an empty orbital is available.
What happens to the energies of atomic orbitals in multielectron atoms?
The energies of the atomic orbitals are split.
p.3
Development of the Periodic Table
What is the basis of the Modern Periodic Table?
Atomic number (Z) and properties.
What does the Aufbau principle state?
Electrons will fill up the lowest energy orbitals first before filling higher energy orbitals.
p.21
Anomalies in Electron Configurations
What are the exceptions to the order of electron filling in?
Some transition metals in the d block and f block.
p.4
Electron Configurations
What is an example of an excited state for hydrogen?
H: 1e- with n = 1, l = 0, m_l = 0, m_s = +1/2.
p.14
Electron Configurations
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.12
Paramagnetic and Diamagnetic Properties
What does it mean for an atom to be paramagnetic?
It has one unpaired electron or multiple unpaired same-spin electrons, making it attracted to a magnetic field.
p.15
Noble Gas Core Configurations
What is the significance of noble gas core configurations?
They simplify the representation of electron configurations by using the nearest noble gas.
What happens once all the p orbitals are singly occupied?
Additional electrons will have to pair with those already in the orbitals.
p.20
Electron Configurations
What are electron configurations?
The distribution of electrons in an atom's orbitals.
What does the magnetic quantum number (mℓ) represent?
The orientation of the orbital, with values ranging from -ℓ to +ℓ.
What is the range of values for the spin quantum number (ms)?
+1/2 or -1/2, indicating the direction of electron spin.
p.16
Electron Configurations
What are valence electrons?
Electrons in the outermost shell involved in bond formation and determining chemical properties.
p.23
Electron Configurations
What is the electron configuration for Group 2A elements?
ns² (Alkaline earth metals).
p.23
Electron Configurations
What is the electron configuration for Group 4A elements?
ns² np² (no specific name).
p.2
Development of the Periodic Table
How did Mendeleev group the elements in his periodic table?
By atomic mass and properties.
p.2
Development of the Periodic Table
What was one of Mendeleev's significant contributions to the periodic table?
He predicted the properties of undiscovered elements.
p.2
Development of the Periodic Table
What limitation did Mendeleev face with his periodic table?
He could not explain inconsistencies.
What is the procedure for filling the 2p orbitals according to Hund's rule?
Put 1 electron in each 2p orbital before pairing.
p.3
Electron Configurations
How are elements arranged in the Modern Periodic Table?
According to electron configuration.
p.3
Development of the Periodic Table
How does electron configuration aid in understanding the periodic table?
It helps understand the structure of the periodic table.
What does Hund's rule state about the arrangement of electrons in degenerate orbitals?
The most stable arrangement maximizes the number of electrons with the same spin by placing one electron in each empty orbital before pairing.
p.16
Electron Configurations
What are core electrons?
Inner electrons that are not involved in bonding.
p.24
d block and f block metals
What is unique about Group 12 elements regarding their d subshells?
They have filled d subshells and are not transition metals.
p.5
Electron Configurations
What is important to know about electron configurations?
The ground state electronic configuration, which shows how electrons are distributed in different atomic orbitals.
p.24
d block and f block metals
What are the transition metals characterized by?
Having unfilled d subshells.
p.24
d block and f block metals
What elements make up the f-block?
The lanthanides and actinides.
p.5
Electron Configurations
Why are there more lines in the He line spectra compared to the H line spectra?
Because of the more complex electron configurations in helium due to its additional electrons.
p.4
Electron Configurations
What does the electron configuration describe?
How the electrons are distributed in the various atomic orbitals.
p.15
Noble Gas Core Configurations
What is the purpose of using a noble gas core in electron configurations?
To represent the electron configurations of all elements except hydrogen and helium.
p.21
Anomalies in Electron Configurations
What contributes to the anomalies in electron configurations?
The greater stability of d subshells that are half-full (d5) or completely full (d10).
p.13
Paramagnetic and Diamagnetic Properties
What does it mean for an atom to be diamagnetic?
All electrons are paired, making the atom repelled by a magnetic field.
p.13
Electron Configurations
What is the significance of the highest energy level in Neon?
It indicates the number of electrons in the outermost shell, which is 8.
What does Hund's rule state about electron arrangement?
The most stable arrangement of electrons is the one in which the number of electrons with the same spin is maximized.
What is the energy status of the 2p orbitals?
The 2p orbitals are of equal energy (degenerate).
Which subshell has a lower energy: 2s or 2p?
2s has lower energy than 2p.
p.20
Development of the Periodic Table
How does the periodic table relate to electron configurations?
The arrangement of elements in the periodic table reflects their electron configurations.
p.22
Anomalies in Electron Configurations
What is the significance of a full d orbital in electron configurations?
A full d orbital indicates that all five d orbitals are occupied by electrons, contributing to the stability of the atom.
p.3
Paramagnetic and Diamagnetic Properties
Why is knowing electron configuration important?
It helps determine the magnetic properties of atoms.
p.17
Electron Configurations
What is the common characteristic of elements in Group 1A?
They all have 1 valence electron.
p.17
Electron Configurations
What is the common characteristic of elements in Group 7A?
They all have 7 valence electrons.
p.4
Electron Configurations
What is an orbital diagram?
A depiction of the arrangement of electrons in an atom using boxes to represent orbitals.
p.15
Noble Gas Core Configurations
What does the notation [Ar] represent in electron configurations?
The electron configuration of Argon, which is the noble gas preceding potassium.
p.11
Electron Configurations
How many electrons does nitrogen (N) have?
A total of seven electrons.
What does splitting of energy levels refer to?
The splitting of a shell into subshells of different energies.
p.3
Electron Configurations
What can electron configuration help predict?
The properties of elements.
p.7
Pauli Exclusion Principle
How many electrons can occupy the same orbital according to the Pauli Exclusion Principle?
A maximum of two electrons.
What does the principal quantum number (n) indicate?
The size of the orbital and the energy level of the electron.
What are the possible values of the angular momentum quantum number (ℓ)?
Integers from 0 to n - 1.
p.22
Anomalies in Electron Configurations
How many electrons can a full d orbital hold?
A full d orbital can hold a maximum of 10 electrons.
What analogy is used to describe the structure of an atom?
Building: atom, Floor: shell, Apartment: subshell, Room: orbital, Guests: electrons.
What are the 2p orbitals in terms of energy?
They are of equal energy (degenerate).
p.3
Development of the Periodic Table
What did Moseley's arrangement of the periodic table clear up?
Discrepancies in earlier periodic tables.
p.22
Anomalies in Electron Configurations
What does 'anomalies in electron configuration' refer to?
It refers to exceptions in the expected order of electron filling in atomic orbitals.
What does the Aufbau principle state?
Electrons will fill up the lowest energy orbitals first before filling up higher energy orbitals.
p.23
Electron Configurations
What is the electron configuration for Group 3A elements?
ns² np¹ (no specific name).
According to Hund's rule, how should electrons be placed in degenerate orbitals?
One electron should be placed in each empty orbital before starting to pair them.
p.18
Electron Configurations
Which blocks are filled in the first and second periods?
s block (period 1 and 2), p block (period 2).
p.23
Electron Configurations
What is the general electron configuration pattern for main group elements?
Highest n → valence electrons → group #A.
p.23
Electron Configurations
What is the electron configuration for Group 8A elements?
ns² np⁶ (Noble gases), with an exception for He = 1s².
p.23
Electron Configurations
What is the electron configuration for Group 5A elements?
ns² np³ (no specific name).
