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Questions and Answers
What is the maximum number of electrons that can occupy the third shell?
What is the maximum number of electrons that can occupy the third shell?
Which quantum number indicates the main energy level occupied by the electron?
Which quantum number indicates the main energy level occupied by the electron?
How many orbitals does the f subshell contain?
How many orbitals does the f subshell contain?
Which statement about the Angular Momentum Quantum Number is true?
Which statement about the Angular Momentum Quantum Number is true?
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What is the maximum number of electrons the p sublevel can hold?
What is the maximum number of electrons the p sublevel can hold?
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How many sublevels are present in the third energy level?
How many sublevels are present in the third energy level?
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What is the range of values for the Angular Momentum Quantum Number when n = 3?
What is the range of values for the Angular Momentum Quantum Number when n = 3?
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According to the Aufbau principle, which atomic orbital is filled first?
According to the Aufbau principle, which atomic orbital is filled first?
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What is the total number of orbitals in the d sublevel?
What is the total number of orbitals in the d sublevel?
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What number of electrons can the f sublevel accommodate?
What number of electrons can the f sublevel accommodate?
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What is the total number of electrons that can be present in the s sublevel?
What is the total number of electrons that can be present in the s sublevel?
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What is the maximum number of electrons that can occupy a single orbital?
What is the maximum number of electrons that can occupy a single orbital?
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What does the Magnetic Quantum Number (m1) indicate?
What does the Magnetic Quantum Number (m1) indicate?
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Which rule states that electrons fill each orbital singly before pairing up?
Which rule states that electrons fill each orbital singly before pairing up?
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For the p subshell, which values can the Magnetic Quantum Number (m1) take?
For the p subshell, which values can the Magnetic Quantum Number (m1) take?
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What symbol represents a spin-up electron?
What symbol represents a spin-up electron?
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What is the value of the azimuthal quantum number (l) for a p subshell?
What is the value of the azimuthal quantum number (l) for a p subshell?
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According to the Pauli Exclusion Principle, what is true about electrons in the same orbital?
According to the Pauli Exclusion Principle, what is true about electrons in the same orbital?
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What is the maximum number of electrons that can be housed in the second energy level?
What is the maximum number of electrons that can be housed in the second energy level?
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Which subshell can hold the highest number of electrons?
Which subshell can hold the highest number of electrons?
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How is the number of orbitals in a subshell calculated?
How is the number of orbitals in a subshell calculated?
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How many orbitals are present in the d subshell?
How many orbitals are present in the d subshell?
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What does the angular momentum quantum number (l) represent?
What does the angular momentum quantum number (l) represent?
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Which of the following electron configurations represents the element Neon (Ne)?
Which of the following electron configurations represents the element Neon (Ne)?
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What is the role of the magnetic quantum number (m1)?
What is the role of the magnetic quantum number (m1)?
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What is the maximum number of electrons allowed in a p subshell?
What is the maximum number of electrons allowed in a p subshell?
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What is the total number of electrons in the third energy level?
What is the total number of electrons in the third energy level?
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What is the angular momentum quantum number (l) for the n=4 energy level?
What is the angular momentum quantum number (l) for the n=4 energy level?
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Which subshells are present in the n=2 energy level?
Which subshells are present in the n=2 energy level?
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What is the maximum value of the angular momentum quantum number (l) for n=3?
What is the maximum value of the angular momentum quantum number (l) for n=3?
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Which orbital represents the angular momentum quantum number (l) of 1?
Which orbital represents the angular momentum quantum number (l) of 1?
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Where is the valence electron of carbon likely located?
Where is the valence electron of carbon likely located?
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For the n=1 energy level, what subshell(s) can be found?
For the n=1 energy level, what subshell(s) can be found?
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If n=3, which of the following describes the subshells available?
If n=3, which of the following describes the subshells available?
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What shapes are represented by the s and p orbitals, respectively?
What shapes are represented by the s and p orbitals, respectively?
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Study Notes
Electron Configuration
- The arrangement of electrons in orbitals around the atomic nucleus
-
Sublevels can only hold a specific number of electrons:
- s = 2 electrons
- p = 6 electrons
- d = 10 electrons
- f = 14 electrons
Electron Distribution Mnemonics
- Level 1 has 1 sublevel (s)
- Level 2 has 2 sub levels (s,p)
- Level 3 has 3 sub levels (s,p,d)
- Level 4 has 4 sub levels (s,p,d,f)
Sublevels
- Can only hold 2 electrons per orbital
- s = 1 orbital, 2 electrons
- p = 3 orbitals, 6 electrons
- d = 5 orbitals, 10 electrons
- f = 7 orbitals, 14 electrons
Aufbau Principle
- Electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels
Orbitals Filling Order
- 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
Mnemonic for Orbital Filling Order
- Si Susan Pumasok Sa Pinto
- Si Daddy Pumasok Sa Door
- Paano Si Frank, Daddy? Paano Si Frank, Daddy? Paano?
Quantum Numbers
- Describe the location of an electron in a three-dimensional atom
-
Principal Quantum Number (n):
- Specifies the main energy level occupied by the electron
- Also called as shell
- Represented by a whole number, starting at 1 for the closest energy level to the nucleus
- Higher numbers indicate farther away from the nucleus (e.g., n=2, n=3)
-
Angular Momentum Quantum Number (l):
- Describes the general region occupied by the electron, called subshell or orbital
- Every energy level has at least one subshell
- Denoted by an integer starting from 0 up to the value equal to n-1
- Also called as Azimuthal Quantum Number
- Values for l correlate to the types of orbitals:
- l = 0 : s orbital
- l = 1 : p orbitals
- l = 2 : d orbitals
- l = 3 : f orbitals
-
Magnetic Quantum Number (m1):
- Used to identify each electron within a subshell
- Values range from -l to +l, including 0
- Number of orbitals in a subshell is given by (2l + 1)
-
Spin Quantum Number (ms):
- Describes the spin of a given electron
- Electron spin can only take two orientations with respect to a specified axis
- Two possible values: +1/2 (spin up, denoted as ↑) and -1/2 (spin down, denoted as ↓)
Hund's Rule
- Electrons fill orbitals singly with the same spin before pairing up
Pauli Exclusion Principle
- No two electrons in an atom can have the same four quantum numbers
- An orbital can hold a maximum of two electrons, but they must have opposite spins (↑↓)
Important Concepts
- Valence Electrons: These are the electrons in the outermost energy level of an atom, and they are responsible for the atom's chemical behavior.
- Electron Configuration : Describes how electrons are arranged in an atom's orbitals, usually written with a shorthand notation (e.g., 1s2 2s2 2p6).
Summary
- Atoms are made up of subatomic particles: protons, neutrons, and electrons.
- Electrons occupy specific regions called orbitals around the nucleus.
- The electron configuration provides a map for understanding the arrangement and behavior of electrons in an atom.
- Quantum numbers provide a framework for describing the state of an electron in an atom.
- Hund's Rule and the Pauli Exclusion Principle are important rules to follow when assigning electrons to orbitals.
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Description
This quiz explores the fundamentals of electron configuration, including the arrangement of electrons in orbitals and the specific capacities of sublevels. Test your knowledge of the Aufbau principle and the order in which orbitals are filled. Additionally, you'll learn useful mnemonics to remember these concepts.
