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Questions and Answers
What does a huge increase in ionisation energy between the first and second ionisation of sodium indicate about its electron configuration?
What does a huge increase in ionisation energy between the first and second ionisation of sodium indicate about its electron configuration?
Which of the following statements is correct regarding magnesium's ionisation energy?
Which of the following statements is correct regarding magnesium's ionisation energy?
What can be inferred about aluminium based on its third to fourth ionisation energy jump?
What can be inferred about aluminium based on its third to fourth ionisation energy jump?
Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p1?
Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p1?
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What is the group classification of sodium based on its electron configuration?
What is the group classification of sodium based on its electron configuration?
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Why is the third ionisation energy of magnesium significantly higher than the second?
Why is the third ionisation energy of magnesium significantly higher than the second?
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What characteristic of ionisation energy is reflected in the trends observed for aluminium?
What characteristic of ionisation energy is reflected in the trends observed for aluminium?
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How does the electron configuration influence the ionisation energies of the elements listed?
How does the electron configuration influence the ionisation energies of the elements listed?
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What principle states that electrons occupy the lowest energy subshells first?
What principle states that electrons occupy the lowest energy subshells first?
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Which of the following correctly describes the maximum occupancy of an atomic orbital?
Which of the following correctly describes the maximum occupancy of an atomic orbital?
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The energy levels of orbitals in an atom do not follow a regular pattern beyond which principal quantum number?
The energy levels of orbitals in an atom do not follow a regular pattern beyond which principal quantum number?
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Which of the following shapes corresponds to the p orbitals?
Which of the following shapes corresponds to the p orbitals?
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Which statement about the ground state of an atom is true?
Which statement about the ground state of an atom is true?
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What characterizes the d orbitals in relation to the IB Chemistry curriculum?
What characterizes the d orbitals in relation to the IB Chemistry curriculum?
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Which of the following correctly describes the role of subshells in ionization energies?
Which of the following correctly describes the role of subshells in ionization energies?
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Identifying electron configuration helps predict which atomic property?
Identifying electron configuration helps predict which atomic property?
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What does the principal quantum number (n) indicate about an atom’s electron configuration?
What does the principal quantum number (n) indicate about an atom’s electron configuration?
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Which principal quantum number can hold a maximum of 8 electrons?
Which principal quantum number can hold a maximum of 8 electrons?
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What is the maximum number of electrons that can be held in the subshell represented by 'd'?
What is the maximum number of electrons that can be held in the subshell represented by 'd'?
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Which of the following correctly describes the order of energy levels in subshells?
Which of the following correctly describes the order of energy levels in subshells?
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How many total electrons can be held in the principal quantum shell with n = 4?
How many total electrons can be held in the principal quantum shell with n = 4?
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Which of the following statements about subshells is true?
Which of the following statements about subshells is true?
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What mathematical relationship defines the maximum number of electrons in a principal quantum shell?
What mathematical relationship defines the maximum number of electrons in a principal quantum shell?
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Which of the following correctly identifies the pattern of subshell filling across principal quantum shells?
Which of the following correctly identifies the pattern of subshell filling across principal quantum shells?
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Study Notes
HL IB Chemistry - Electronic Configurations
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Electromagnetic Spectrum:
- A range of frequencies covering all electromagnetic radiation, with related wavelengths and energy.
- Divided into bands, important in analytical chemistry.
- Shows the relationship between frequency, wavelength, and energy.
- Frequency is the number of waves passing per second; wavelength is the distance between consecutive peaks.
- Gamma rays, X-rays, and UV radiation are high-energy, high-frequency, and dangerous.
- All light waves travel at the same speed, differing only in frequency.
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Emission Spectra:
- Electrons orbit the nucleus in energy shells.
- Increased energy allows electrons to jump to higher energy levels.
- Electrons return to original energy levels emitting energy.
- Emitted energy frequency is the same as absorbed energy, just emitted instead of absorbed.
- Emitted energy in the visible region can be analyzed using a diffraction grating.
- Resulting pattern is a line emission spectrum.
- The spectrum of hydrogen shows specific frequencies of light (ie., quantized).
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Continuous vs. Line Spectra:
- Continuous spectrum displays all frequencies of light (like a rainbow).
- Line spectrum displays only specific frequencies of light, indicating quantized energy levels.
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Speed of Light:
- Constant (3.00 x 10⁸ ms⁻¹).
- Inverse relationship between frequency and wavelength (c = fλ).
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Energy Levels, Sublevels & Orbitals:
- Electrons arranged in principal energy levels (shells, numbered by principal quantum numbers, n).
- Lower n value, closer to nucleus and lower energy.
- Higher n value, farther from nucleus, and higher energy.
- Each shell has a fixed capacity of electrons.
- (n = 1, up to 2 electrons; n = 2, up to 8 electrons; n = 3, up to 18 electrons; n = 4, up to 32 electrons).
- Shells split further into subshells (s, p, d, f).
- Subshells contain atomic orbitals.
- s orbitals are spherical; p orbitals are dumbbell-shaped.
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Electron Configuration:
- Describes the arrangement of electrons in shells, subshells, and orbitals.
- Filled in order of increasing energy.
- Each orbital can hold two electrons with opposite spins (Pauli Exclusion Principle).
- Hund's Rule states that orbitals in a subshell are singly occupied before any one orbital is doubly occupied.
- Electron configurations can be represented in full form or shorthand (using noble gas notation).
- Different blocks in the periodic table correspond to different subshells (s, p, d, f).
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Ionisation Energy from an Emission Spectrum (HL):
- Electrons move between shells, absorbing or emitting energy.
- When an electron falls back to the ground state, it emits a photon corresponding to the energy difference between levels (n = 1 to n = ∞).
- Measuring the wavelength/frequency of emitted photons reveals the differences in energy levels in the atom.
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Successive Ionisation Energies (HL):
- Successive Ionisation Energies (IEs) of elements increase as electrons are removed.
- IEs increase as fewer electrons remain and the net positive charge of the ion increases.
- There are notable jumps in IE corresponding to changes in electron shells or subshells.
- IEs provide information about electronic configurations and shell structure.
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Description
Explore the intricacies of electronic configurations and the electromagnetic spectrum in this HL IB Chemistry quiz. Understand the relationship between frequency, wavelength, energy, and emission spectra. This quiz will enhance your grasp of analytical chemistry concepts and the behavior of electrons within atom energy shells.
