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Questions and Answers
What does the principle quantum number, n, indicate in the quantum mechanical model of an atom?
Which quantum number describes the shape of an orbital?
In the quantum mechanical model, what does an atomic orbital represent?
How are atomic orbitals often visualized in the quantum mechanical model?
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Which of the following statements is true regarding the four quantum numbers?
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Which quantum number has values ranging from n = 1 to n = ∞?
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What does a higher density in an electron density diagram suggest about the probability of finding an electron?
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What is true about the orbits allowed for electrons according to Bohr's model?
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What is the correct condensed electron configuration for an element with atomic number 11?
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Which atomic number corresponds to the element with the electron configuration [Ar]4s¹3d⁵?
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According to the filling order of orbital energies, which of the following orbitals is filled after 3p?
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What does the Magnetic Quantum Number, m₁, indicate?
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What is the maximum number of electrons that can be accommodated in the 3d subshell?
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What is the maximum number of electrons that can occupy an orbital according to the Pauli exclusion principle?
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Which of the following elements has the electron configuration [Ar]4s²3d¹?
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Which of the following correctly identifies the allowed values for the Orbital-shape (subshell) quantum number l?
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Which group has elements with the same number of valence electrons?
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What is the position of the 4s subshell in relation to the 3d subshell in the order of filling?
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Which orbital corresponds to l = 2?
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For which element would the filled configuration be [Ar]4s²3d⁶?
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What is the total number of orbitals in a principal energy level n = 3?
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What are the possible values of the Spin Quantum Number, m₂?
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If an electron in an orbital has a Spin Quantum Number of +1/2, what must be the Spin Quantum Number of the second electron in the same orbital?
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How many values are available for the Magnetic Quantum Number, m₁, if l = 1?
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What is the correct electron configuration for nitrogen?
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Which of the following correctly applies Hund's rule?
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What does the Pauli exclusion principle state?
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How many unpaired electrons does fluorine have?
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Electrons added to equivalent energy orbitals must have what characteristic according to spin rules?
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What is the correct orbital diagram for carbon?
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Which of the following statements about orbital energy filling is accurate?
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What is the correct orbital diagram for oxygen?
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What is the electron configuration of lithium?
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Which quantum number set is correct for the first electron in hydrogen?
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According to the aufbau principle, how should the electrons fill in lithium's electron configuration?
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What is the correct representation for the orbital diagram of helium?
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What is the second quantum number for the first electron in helium?
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Which statement is true about the electron configuration of hydrogen?
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What quantum number describes the orientation of an electron's orbital?
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Which electron configuration represents the fill order of two electrons in the first energy level?
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Study Notes
Rutherford's Model
- Negatively charged electrons orbit a positively charged nucleus
- The model is still widely used to represent the atom
Bohr's Model
- Refined Rutherford's model
- Electrons exist in specific orbits, each having a set energy level
- Higher energy levels equate to larger orbits
Quantum Mechanical Model
- Modern model that accounts for wave-like properties of electrons
- Uses wave functions to describe regions of space where electrons are likely to be found
- Atomic orbitals are these regions
- Atomic orbitals can be represented using electron density diagrams which depict the probability of finding an electron in space
Quantum Numbers
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Four quantum numbers are used to describe electron distribution
-
n (principal): Describes the energy level or shell of an orbital
- Higher values of n correspond to larger and higher energy shells
- Values range from 1 to ∞
-
l (orbital-shape): Defines the orbital's shape and subshells
- Values depend on n and range from 0 to (n-1)
- Each value is assigned a letter:
- 0 = s (spherical)
- 1 = p (dumbbell-shaped)
- 2 = d (more complex shapes)
- 3 = f (even more complex shapes)
- An energy sublevel is identified by combining n with the orbital letter (e.g., n=2, l=1: 2p sublevel)
-
m₁ (magnetic): Specifies the orbital's orientation in space
- Number of possible m₁ values depends on l: (2l+1)
- For each energy level, the total number of orbitals is n²
-
m₂ (spin): Represents the spin of an electron
- Two possible values: +1/2 or -1/2, signifying opposing spin directions
The Pauli Exclusion Principle
- States that no two electrons in an atom can have the same set of four quantum numbers
- This means a maximum of two electrons can occupy an orbital
- These two electrons must have opposite spins
Electron Configurations and Orbital Diagrams
- The aufbau principle guides us in organizing electron configurations by increasing atomic number
- Electron configuration: Represents the distribution of electrons in an atom
- Orbital diagram: Uses boxes and arrows to depict orbitals and electron spins
- Hund's rule: States that individual orbitals within a subshell are filled with one electron each, before pairing occurs
Filling Orbitals for Periods 1 and 2
- Orbital diagrams are filled in order from left to right, denoting increasing orbital energy
Filling Orbitals for Period 3
- Periods 1 and 2 follow similar filling guidelines
- Condensed electron configurations utilize noble gas symbols to represent completed inner shells
- Example: [Ne]3s¹ represents potassium (Z=19)
Filling Orbitals for Period 4
- Follow previous guidelines until Z=23
- Exceptions occur at Z=24 (Cr) and 29 (Cu), where the configurations deviate slightly
- Cr: [Ar]4s¹ 3d⁵ instead of [Ar]4s² 3d⁴
- Cu: [Ar]4s¹ 3d¹⁰ instead of [Ar]4s² 3d⁹
Using the Periodic Table to Predict Electron Configurations
- Periodic table can be divided into s, p, d, and f blocks based on orbital filling patterns
- Group and period numbers provide information:
- Group Number: The last numeral often indicates the number of valence electrons (exceptions exist, like He)
- Period Number: Represents the value of n for the highest occupied orbital
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Description
Explore the fundamental atomic models, including Rutherford's, Bohr's, and the Quantum Mechanical Model. Understand how these models describe electron behavior through quantum numbers and atomic orbitals. This quiz delves into the principles that define modern atomic theory.