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Questions and Answers
What is the net positive charge experienced by an electron in an atom?
What is the net positive charge experienced by an electron in an atom?
What is the trend in atomic radius across a period?
What is the trend in atomic radius across a period?
What is the energy required to remove an electron from an atom?
What is the energy required to remove an electron from an atom?
Which block of the periodic table includes the transition metals?
Which block of the periodic table includes the transition metals?
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What is the ability of an atom to attract electrons in a covalent bond?
What is the ability of an atom to attract electrons in a covalent bond?
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What is the result of the increase in effective nuclear charge (Zeff) across a period?
What is the result of the increase in effective nuclear charge (Zeff) across a period?
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What is the trend in ionization energy down a group?
What is the trend in ionization energy down a group?
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What is the unit of measurement for energy in chemistry?
What is the unit of measurement for energy in chemistry?
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What technique is used to measure the energy of electrons emitted from an atom?
What technique is used to measure the energy of electrons emitted from an atom?
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What is the trend in electronegativity across a period?
What is the trend in electronegativity across a period?
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Study Notes
Atomic Structure
- Atomic structure consists of protons, neutrons, and electrons
- Protons and neutrons are found in the nucleus, while electrons orbit around it
- Electrons are arranged in energy levels or shells, with each shell having a specific capacity
Effective Nuclear Charge
- Effective nuclear charge (Zeff) is the net positive charge experienced by an electron in an atom
- Zeff is the result of the attractive force between the nucleus and electrons, and the repulsive force between electrons
- Zeff increases from left to right across a period, and decreases down a group
Atomic Radius Trends
- Atomic radius decreases from left to right across a period, and increases down a group
- This is due to the increase in Zeff, which pulls electrons closer to the nucleus
- Atomic radius is measured in picometers (pm)
Ionization Energy
- Ionization energy (IE) is the energy required to remove an electron from an atom
- IE increases from left to right across a period, and decreases down a group
- This is due to the increase in Zeff, which makes it harder to remove an electron
Periodic Table Blocks
- The periodic table is divided into blocks based on the last orbital filled
- The blocks are:
- s-block (alkali metals and alkaline earth metals)
- p-block (nonmetals and metalloids)
- d-block (transition metals)
- f-block (lanthanides and actinides)
Electronegativity
- Electronegativity is the ability of an atom to attract electrons in a covalent bond
- Electronegativity increases from left to right across a period, and decreases down a group
- Electronegativity is measured using the Pauling scale, with higher values indicating greater electronegativity
Force of Energy
- Not a specific topic in AP Chemistry, but energy is a fundamental concept in chemistry
- Energy is the ability to do work, and is measured in units such as joules (J)
Photoelectron Spectroscopy
- Photoelectron spectroscopy (PES) is a technique used to measure the energy of electrons emitted from an atom
- PES involves bombarding atoms with high-energy radiation, causing electrons to be emitted
- The energy of the emitted electrons is measured, providing information about the atomic orbitals and electron binding energies
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Description
Test your knowledge of atomic structure, including effective nuclear charge, atomic radius trends, ionization energy, periodic table blocks, electronegativity, and more.
