Atomic Structure and Electron Arrangement

Basics of Atomic Structure

• The higher the coefficient or shell, the higher the energy of an atom.
• The arrangement of electrons in an atom determines how it interacts with other atoms.
• The arrangement of electrons in each atom determines its physical properties.
• All orbitals in the same sublevel (e.g. 2s, 1s, 3p) have the same amount of energy.
• Mass Number = Protons + Neutrons, not shown on the periodic table.
• Atomic Number = Protons, shown as the large number on the periodic table.
• Average Atomic Mass = average mass of all isotopes of an element.

Principal Quantum Number

• Principal Quantum Number (N) describes the energy level and size of an orbital.
• As N increases, the energy and distance from the nucleus also increase.
• N can be any positive integer (1, 2, 3, 4, ...).
• Orbitals do not exist unless an electron is occupying it.
• Orbitals are the last shell level.

Periodic Table

• The periodic table is split into blocks, with rows corresponding to the coefficient in electron configuration.
• For the d block, the coefficient is one less than the row it is in.
• The exponent is the number of columns from the left of the start of the specific letter block.
• Students can explain the reasoning behind the organization of the periodic table.

Electron Configuration and Orbitals

• Students can construct the appropriate electron configuration and orbital diagram for a given element.
• Students can identify the alkali metals, alkaline earth metals, transitional metals, halogens, noble gases, metals, non-metals, and metalloids on the periodic table.

Vocabulary

• Isotope: a different version of an element with a different number of neutrons.
• Ground State: the lowest energy state of an atom or other particle.
• Electron Configuration: the distribution of electrons in an atom.
• Orbital: a region around the nucleus that can hold a specific number of electrons (s: 2, p: 6, d: 10, f: 14).
• Valence Electrons: electrons that are furthest from the nucleus and have the most energy.
• Protons: positively charged particles found in the nucleus.
• Neutrons: neutrally charged particles found in the nucleus.
• Electrons: negatively charged particles found around the nucleus.
• Nucleus: the center of the atom, positively charged, containing protons and neutrons.
• Electron Cloud: the area around the nucleus where there is a negative charge.

Principles/Laws

• Pauli Exclusion Principle: electrons in the same orbital must have a different spin.
• Hund's Rule: in a sublevel, all orbitals get one electron before pairing up.
• Aufbau Principle: fill orbitals from low energy to high energy (s → p).

Unit 7: Wave Types

• Radio Waves: much longer wavelength than visible light, used for communication.
• Microwave: used for cooking, heat application, and communication, similar to radio waves.
• Infrared: used for thermal imaging and remote controls.
• Ultraviolet: used for killing bacteria and creating fluorescent effects, but can damage cells.
• X-Ray: used for imaging, but can damage molecular structure and cause harm.
• Gamma Rays: used to treat cancer, but can damage the entire body.

Emissions Spectra

• Each element has a unique emission spectra.
• Emission spectra shows the colors of light emitted when an element is hit with the right wavelength needed to make a jump to a higher energy level.

This quiz covers the basics of atomic structure, including the arrangement of electrons and their impact on atomic interactions. It explores the relationship between energy and electron shells, and the role of orbitals in determining atomic behavior.