Podcast
Questions and Answers
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?
Orbitals in the same sublevel must be filled before any orbital in a higher sublevel is occupied.
Orbitals in the same sublevel must be filled before any orbital in a higher sublevel is occupied.
True
What principle states that electrons fill orbitals from the lowest energy level to the highest?
What principle states that electrons fill orbitals from the lowest energy level to the highest?
Aufbau Principle
The ________ rule states that two electrons in the same orbital must have opposite spins.
The ________ rule states that two electrons in the same orbital must have opposite spins.
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Match the following energy levels with their corresponding sublevels and number of orbitals:
Match the following energy levels with their corresponding sublevels and number of orbitals:
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What is the condensed electron configuration for lithium?
What is the condensed electron configuration for lithium?
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The first ionization energy is generally higher for elements with fewer protons.
The first ionization energy is generally higher for elements with fewer protons.
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What is the full electron configuration for an oxygen atom?
What is the full electron configuration for an oxygen atom?
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The maximum number of electrons in a main energy level is given by the formula _____, where n is the principal quantum number.
The maximum number of electrons in a main energy level is given by the formula _____, where n is the principal quantum number.
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Match the following elements with their full electron configurations:
Match the following elements with their full electron configurations:
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Which factor affects the difficulty of removing an electron from an atom?
Which factor affects the difficulty of removing an electron from an atom?
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Inner electrons have no effect on the effective nuclear charge felt by outer electrons.
Inner electrons have no effect on the effective nuclear charge felt by outer electrons.
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What is the full electron configuration for a magnesium ion (Mg2+)?
What is the full electron configuration for a magnesium ion (Mg2+)?
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Which sublevel has the highest energy in the n=3 main energy level?
Which sublevel has the highest energy in the n=3 main energy level?
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The maximum number of electrons in the s sublevel is 2.
The maximum number of electrons in the s sublevel is 2.
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How many total electrons can the p sublevel hold?
How many total electrons can the p sublevel hold?
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In the __ sublevel, there are three orbitals that can hold a maximum of six electrons.
In the __ sublevel, there are three orbitals that can hold a maximum of six electrons.
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Match the following main energy levels with their maximum number of electrons:
Match the following main energy levels with their maximum number of electrons:
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What is the order in which the sublevels are filled as electrons increase?
What is the order in which the sublevels are filled as electrons increase?
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Electrons can occupy the same orbital if they have the same spin.
Electrons can occupy the same orbital if they have the same spin.
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What electron configuration is given for Lithium?
What electron configuration is given for Lithium?
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The __ shape of orbitals corresponds to the 's' sublevel.
The __ shape of orbitals corresponds to the 's' sublevel.
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Match the orbitals with their respective shapes:
Match the orbitals with their respective shapes:
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Which of the following elements has an electron configuration ending in 4s² 3d¹⁰?
Which of the following elements has an electron configuration ending in 4s² 3d¹⁰?
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The maximum number of electrons that can occupy a single orbital is 2.
The maximum number of electrons that can occupy a single orbital is 2.
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What is the electron configuration for Argon?
What is the electron configuration for Argon?
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Each electron in an atom experiences a property called __, which describes its intrinsic angular momentum.
Each electron in an atom experiences a property called __, which describes its intrinsic angular momentum.
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Match the following elements with their number of valence electrons:
Match the following elements with their number of valence electrons:
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Study Notes
Electron Configurations (Structure 1.3)
- Guiding Question: How can we model the energy states of electrons in atoms?
- Time Allocation: Standard Level (SL) and Higher Level (HL) - 3 hours; Advanced Higher Level (AHL) - 3 hours.
Prior Knowledge
- Students should know the different types of electromagnetic radiation (e.g., microwaves, X-rays, UV)
- Important to consider differences between types of electromagnetic radiation.
SL and HL Content
- Content related to SL and HL is included.
Part A: The Electromagnetic Spectrum (S1.3.1)
- Includes a diagram of the electromagnetic spectrum showing the different types of radiation.
- Students need to understand the relationship between wavelength and energy of electromagnetic radiation: shorter wavelengths correspond to higher energy.
Part B: Emission Spectra and the Bohr Model of the Atom (S1.3.2)
- Discusses emission spectra and the Bohr model of the atom.
What is White Light?
- An image shows white light separated into its component colors (spectrum) by a prism.
- White light is composed of all colors of visible light.
Practical: Continuous and Line Emission Spectra
- Students should observe the difference between continuous and line emission spectra using diffraction grating.
- Students should observe the visible spectrum produced from white light, and also from a hydrogen gas lamp.
Continuous and Line Emission Spectra
- A continuous spectrum shows all frequencies of light.
- A line spectrum, shows only specific frequencies of light.
The Bohr Model
- Electrons in hydrogen atoms can absorb energy and move to a higher energy level.
- When the electron returns to a lower energy level, energy is released.
- This released energy is in the form of electromagnetic radiation.
Hydrogen Emission Spectrum
- Transitions between different energy levels produce specific wavelengths of light.
- Transitions to the n=1 level produce UV light.
- Transitions to the n=2 level produce visible light.
- Transitions to the n=3 level produce infrared light.
The Bohr Model and the Hydrogen Emission Spectrum
- The different colored lines in the emission spectrum represent the specific energy amounts released during the electron transitions.
Quick Check (MCQ)
- Questions concerning the hydrogen emission spectrum.
Practical: Flame Tests
- Students perform a practical activity using a Bunsen burner.
- The practical involves holding wooden splints soaked in metal ion solutions in a burner flame.
- Observation and identification of likely metal ions in the unknown solutions is also part of the experiment.
Hydrogen Emission Spectrum: Excitation to n=∞
- Energy levels converge as we get further out.
- The edge of the atom is known as n=∞.
- Electrons can leave the atom if they absorb enough energy to reach n=∞, forming an ion.
Practice Questions
- Includes questions about sketching energy level diagrams, explaining why certain lines aren't visible in the hydrogen emission spectrum, and other related topics.
Part C: Energy Levels, Sublevels and Orbitals (S1.3.3 & S1.3.4)
- This section describes sublevels and orbitals in greater detail.
When is an Electron No Longer an Electron?
- Electrons are probabilistic.
- Heisenberg's Uncertainty Principle explains the probabilistic nature of electrons.
- Schrödinger's Wave Equation describes the probability of finding an electron.
Maximum Number of Electrons for Each Energy Level
- Mathematical formula to determine maximum number of electrons for different energy levels.
Main Energy Levels → Sublevels
- The relationship between main energy levels and sublevels.
Sublevels → s Orbitals
- Describes the spherical shape of s orbitals.
Sublevels → p Orbitals
- Describes the dumbbell-shaped p orbitals.
Sublevels → d Orbitals
- Describes the different shapes of d orbitals.
Sublevels → f Orbitals
- Discusses the shapes of f orbitals.
Summary
- Table summarizing the relationship between energy level, sublevel, number of orbitals, and maximum number of electrons.
Practice Questions (Page 35)
- Questions covering the definitions of sublevels and orbitals, sketching orbitals.
- Questions explain the maximum number of electrons and why n=4 can hold 32 electrons.
Part D: Orbital Box Diagrams and Electron Configurations (S1.3.5)
- Discusses orbital box diagrams and electron configurations.
How do We Represent Orbitals More Simply?
- Orbital box diagrams are a simpler way to represent orbitals.
Orbital Box Diagram for n=1, n=2, and n=3 Energy Levels
- Diagrams illustrating orbital box diagrams for different energy levels.
How do We Tell the Difference Between a 1s and 2s Orbital?
- Illustrates the difference between 1s and 2s orbitals using graphs and diagrams showing nodes.
Orbital Box Diagram Rules
- Aufbau Principle, Pauli Exclusion Principle, and Hund's Rule—the rules for filling orbital box diagrams.
Orbital Filling Order
- Diagram showing the order of filling orbitals with electrons.
Relative Energy Levels—First Twenty Atoms
- Diagram showing the arrangement of orbitals for first 20 atoms.
Writing Electronic Configurations
- Different ways of writing electronic configurations.
Quick Check (Page 46)
- Questions on electronic configurations, examples of full and condensed configurations.
Using the Periodic Table to Write Electron Configurations
- Explains how to use the periodic table to determine electron configurations.
Writing Configurations for Ions, Quick Checks (Pages 48 & 49)
- Methods for writing electronic configurations of ions
- Questions for practice
Part E: First Ionization Energy (S1.3.6)
- Discusses the first ionization energy.
- Includes graphs and diagrams which show relationship between ionization energy and the position of an element on the periodic table.
Factors Affecting Ionization Energy
- The greater the distance between the nucleus and the outer electrons, the easier it is to remove an electron.
- The greater the number of protons in the nucleus, the harder it is to remove an electron.
Electron Shielding
- Explains how inner electrons shield valence electrons from the attractive force of the nucleus.
What is First Ionization Energy?
- Definition and general formula for calculating first ionization energy.
How Does 1st Ionization Energy Change Down a Group?
- Discusses the trend in ionization energy as you move down a group in the periodic table, and why.
Quick Checks (Pages 57 & 69)
- Questions on ionization energy and elements placement on the periodic table.
Why do Atoms Get Smaller Across a Period?
- Explains why atoms get smaller as you move across a period in the periodic table.
General Trend: 1st Ionization Energy Across a Period
- Explains how ionization energy changes across a period.
Data for 1st Ionization Energy Across a Period (Page 61)
- Shows the correlation between ionization energy and electron configuration.
Practice Questions (Page 62)
- Includes questions on trends in ionization energy across a period.
Part F: Successive Ionization Energies (S1.3.7)
- Discusses successive ionization energies.
1st Ionization Energy
- Equation, and how to write similar equations for second and third ionization energy.
Successive Ionization Energies of Na, graphs and examples (Pages 66 & 67,68)
- Provides data and graphs for successive ionization energies of sodium, showing relationships and trends.
Quick Check (Page 69)
- Questions to find an element in group 13 by its successive ionization energy.
Practice Question (Page 70)
- Includes a question asking students to sketch successive ionization energies for a nitrogen atom.
Part G: The Limit of Convergence and Ionization (S1.3.8)
- Describes the convergence limit and its relationship to ionization.
How do we Calculate Ionization Energy from Spectral Data?
- Equations explaining how ionization energy values can be calculated.
Practice Question 1
- Question about calculating ionization energy for hydrogen using spectral data.
Practice Question 2
- Questions about the calculation of frequency, wavelength and identifying radiation types.
Guiding Question and Review (Page 77)
- Questions about the models used, and link the models and concepts.
Key Terminology (Page 79)
- Includes a list of key terms and definitions from the course material.
Past-paper questions (Page 80)
- Previous past paper questions available for practice
Retrieval Practice (Pages 81, 82, 84, 85, and 86)
- Includes various retrieval practices to assess understanding of core concepts.
Extension: Doppler Shift (Page 92)
- Describes the Doppler effect in the context of emission and absorption spectra.
- Relates that to the movement of objects.
Extension: Atomic Absorption Spectra (Page 93)
- Discusses the differences between emission and absorption spectra.
Extension: Electron Configurations and Quantum Numbers (Page 94)
- Describes quantum numbers (n, l, m, ms) and their relationship to electron configurations.
Probabilities and Quantum Wavefunctions (Page 95)
- Explains the probabilistic nature of electrons and quantum wavefunctions in simple terms.
NOS: Logarithmic Scales (Page 90)
- Explains why logarithmic scales are used in scientific analysis of data, using graphs as illustrative examples.
Extension (Page 91)
Additional Notes
- The provided notes include a variety of examples and questions for practice, aiming to provide a comprehensive learning experience.
- All the information is from the images and text provided by the user.
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Description
Test your knowledge on electron configurations and principles governing the behavior of electrons in atoms. This quiz covers topics like orbital filling rules, ionization energy, and the condensed electron configurations for various elements. Challenge yourself with matching elements to their configurations and understanding key concepts in chemistry.
