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Questions and Answers
What is the mass of a proton in atomic mass units (amu)?
According to the Rutherford Model, what is the charge of the nucleus?
What is the purpose of the atomic number (Z)?
What is the shape of a p-orbital?
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In the Bohr Model, what happens when an electron gains energy?
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What is the term for the regions where electrons are likely to be found?
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What determines the chemical properties of an element?
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Which of the following principles states that electrons occupy the lowest available energy level?
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What is the shape of an s-orbital?
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What is the term for the arrangement of electrons in energy levels?
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What happens to the atomic radius as you move from left to right across a period?
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Which of the following trends is observed in the periodic table?
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Study Notes
Atomic Structure
Subatomic Particles
- Proton: Positively charged, found in the nucleus, mass = 1 amu (atomic mass unit)
- Neutron: No charge, found in the nucleus, mass = 1 amu
- Electron: Negatively charged, found in energy levels, mass = 0.00055 amu
Atomic Models
-
Rutherford Model (1911): Nucleus with electrons orbiting around it
- Positively charged nucleus with negatively charged electrons
-
Bohr Model (1913): Energy levels with electrons jumping between them
- Electrons occupy specific energy levels (shells) around the nucleus
Atomic Structure Notation
- Atomic Number (Z): Number of protons in an atom's nucleus
- Mass Number (A): Sum of protons and neutrons in an atom's nucleus
-
Electron Configuration: Arrangement of electrons in energy levels
- Notation:
1s² 2s² 2p⁶(example)
- Notation:
Energy Levels (Shells)
- Principal Energy Levels (n): 1, 2, 3, ... (distance from nucleus increases)
- Subshells (l): s, p, d, f (shapes of orbitals)
-
Orbitals: Regions where electrons are likely to be found
- s-orbitals: spherical shape
- p-orbitals: dumbbell shape
- d-orbitals: four-leaf clover shape
- f-orbitals: complex shape
Atomic Structure
Subatomic Particles
- A proton has a positive charge and is found in the nucleus with a mass of 1 atomic mass unit (amu).
- A neutron has no charge and is found in the nucleus with a mass of 1 amu.
- An electron has a negative charge and is found in energy levels with a mass of 0.00055 amu.
Atomic Models
Rutherford Model (1911)
- The nucleus is positively charged, and electrons orbit around it.
- The model consists of a positively charged nucleus with negatively charged electrons.
Bohr Model (1913)
- Electrons occupy specific energy levels (shells) around the nucleus.
- Electrons jump between energy levels, and each energy level has a specific capacity.
Atomic Structure Notation
- The atomic number (Z) is the number of protons in an atom's nucleus.
- The mass number (A) is the sum of protons and neutrons in an atom's nucleus.
- Electron configuration is the arrangement of electrons in energy levels.
- Electron configuration notation is used to describe the arrangement, such as 1s² 2s² 2p⁶.
Energy Levels (Shells)
- Principal energy levels (n) are numbered from 1, 2, 3, and so on, with increasing distance from the nucleus.
- Subshells (l) are classified as s, p, d, and f, and they have different shapes of orbitals.
- Orbitals are regions where electrons are likely to be found, with different shapes:
- s-orbitals are spherical in shape.
- p-orbitals have a dumbbell shape.
- d-orbitals have a four-leaf clover shape.
- f-orbitals have a complex shape.
Atomic Structure
Subatomic Particles
- Protons have a positive charge and are found in the nucleus, determining the element through their atomic number.
- Neutrons have no charge and are found in the nucleus, contributing to the atomic mass along with protons.
- Electrons have a negative charge and are found in energy levels outside the nucleus, with their number equal to the number of protons in a neutral atom.
Energy Levels (Shells)
- Electron configuration refers to the arrangement of electrons in energy levels.
- The valence shell is the outermost energy level, determining the chemical properties of an atom.
- The Aufbau principle states that electrons occupy the lowest available energy level.
- Pauli's Exclusion Principle states that each electron has a unique set of quantum numbers.
Atomic Orbitals
- s orbitals have a spherical shape, with one orbital per energy level.
- p orbitals have a dumbbell shape, with three orbitals per energy level (x, y, z).
- d orbitals have a complex shape, with five orbitals per energy level.
- f orbitals have a complex shape, with seven orbitals per energy level.
Electron Configuration Notation
- Shorthand notation represents the number of electrons in each orbital (e.g., 1s² 2s² 2p⁶).
- Block notation groups orbitals (s, p, d, f) with the number of electrons in each.
Periodic Trends
- Atomic radius decreases from left to right across a period and increases from top to bottom in a group.
- Electronegativity increases from left to right across a period and decreases from top to bottom in a group.
- Ionization energy increases from left to right across a period and decreases from top to bottom in a group.
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Description
Learn about the basic structure of an atom, including protons, neutrons, and electrons, and explore the Rutherford and Bohr models of atomic structure.
