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Questions and Answers
What determines an element's chemical behavior?
What is the energy required to remove an electron from an atom known as?
What is the arrangement of electrons in an atom's energy levels known as?
What determines the size and energy of an energy level in an atom?
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What is the distance from the nucleus to the outermost electron known as?
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As you move left to right across a period, what happens to the atomic radius?
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What is the format used to write the electron configuration?
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As you move down a group, what happens to the ionization energy?
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What is the number of valence electrons in an atom's outermost energy level?
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Which of the following is a trend for ionization energy across a period?
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What is the arrangement of electrons in an atom's energy levels known as?
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What is the relationship between the number of energy levels and the distance from the nucleus?
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What is the effect of moving down a group on the atomic radius?
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Study Notes
Bohr Diagrams
Valence Electrons
- Valence electrons: outermost energy level electrons participating in chemical bonding
- Number of valence electrons determines an element's chemical behavior
- Typically, atoms tend to gain, lose, or share electrons to achieve a full outer energy level (octet)
Ionization Energy
- Ionization energy: energy required to remove an electron from an atom
- Measures the energy required to overcome the electron-nucleus attraction
- Increases as you move:
- Left to right across a period (due to increasing nuclear charge)
- Top to bottom within a group (due to increasing distance from the nucleus)
Electron Configuration
- Electron configuration: arrangement of electrons in an atom's energy levels
- Described using the Aufbau principle, Pauli's Exclusion principle, and Hund's rule
- Written in the format: 1s² 2s² 2p⁶ 3s² 3p⁶ ...
Energy Levels
- Energy levels: specific energy states occupied by electrons in an atom
- Represented by the principal quantum number (n), which determines the energy level's size and energy
- Sublevels: s, p, d, and f orbitals, which have different shapes and orientations
Atomic Radius
- Atomic radius: distance from the nucleus to the outermost electron
- Decreases as you move:
- Left to right across a period (due to increasing nuclear charge)
- Increases as you move down a group (due to increasing energy levels)
Valence Electrons
- Valence electrons are the outermost energy level electrons that participate in chemical bonding
- The number of valence electrons determines an element's chemical behavior
- Atoms tend to gain, lose, or share electrons to achieve a full outer energy level, which is known as an octet
Ionization Energy
- Ionization energy is the energy required to remove an electron from an atom
- It measures the energy required to overcome the electron-nucleus attraction
- Ionization energy increases:
- Left to right across a period due to increasing nuclear charge
- Top to bottom within a group due to increasing distance from the nucleus
Electron Configuration
- Electron configuration is the arrangement of electrons in an atom's energy levels
- It is described using the Aufbau principle, Pauli's Exclusion principle, and Hund's rule
- Electron configuration is written in a specific format, such as 1s² 2s² 2p⁶ 3s² 3p⁶...
Energy Levels
- Energy levels are specific energy states occupied by electrons in an atom
- They are represented by the principal quantum number (n), which determines the energy level's size and energy
- Energy levels have sublevels, including:
- s orbitals, which are spherical in shape
- p orbitals, which are dumbbell-shaped
- d orbitals, which have a complex shape
- f orbitals, which have a complex shape
Atomic Radius
- Atomic radius is the distance from the nucleus to the outermost electron
- Atomic radius decreases:
- Left to right across a period due to increasing nuclear charge
- It increases as you move down a group due to increasing energy levels
Atomic Structure and Bonding
- A Bohr diagram is a visual representation of an atom's energy levels, showing the electron configuration of an atom.
- It consists of concentric circles representing energy levels, with electrons placed in specific energy levels.
Naming Compounds
- Compounds are named using a set of rules based on the type of bond (ionic or covalent) and the type of atoms involved.
- Ionic compounds are named using the name of the cation, followed by the name of the anion.
- Covalent compounds are named using prefixes to indicate the number of atoms of each element.
WHMIS Symbols
- WHMIS (Workplace Hazardous Materials Information System) symbols are used to identify hazardous substances.
- There are several WHMIS symbols, each representing a specific type of hazard, such as flammability, toxicity, or corrosivity.
Ionic and Covalent Compounds
- Ionic compounds are formed when a metal element loses electrons to become a cation, and a non-metal element gains electrons to become an anion.
- Covalent compounds are formed when two or more non-metal elements share electrons to form a molecule.
- The type of bond formed depends on the electronegativity of the atoms involved.
Elements
- Elements are the building blocks of matter, consisting of atoms with the same proton number (atomic number).
- Elements are represented by a one- or two-letter symbol, and are organized on the periodic table based on their properties.
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Description
Test your understanding of Bohr diagrams, valence electrons, and ionization energy in chemistry. Learn how to determine an element's chemical behavior and the energy required to remove an electron from an atom.
