Atomic Structure Unit 6

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What is an isotope of an element?

A version of an element with a different number of orbitals

A version of an element with a different number of neutrons (correct)

A version of an element with a different number of protons

A version of an element with a different number of electrons

What is the electron configuration of an atom?

The distribution of protons in an atom

The distribution of atoms in an atom

The distribution of electrons in an atom (correct)

The distribution of neutrons in an atom

What is the maximum number of electrons that an 'f' orbital can hold?

10 electrons

2 electrons

14 electrons (correct)

6 electrons

What are valence electrons?

Electrons that are furthest from the nucleus and have the most energy Signup and view all the answers

What is the Pauli Exclusion Principle?

Electrons in the same orbital must have a different spin Signup and view all the answers

What type of wave is used for thermal imaging and remote controls?

Infrared Signup and view all the answers

What is an emission spectrum?

The colors of light that are emitted by an element Signup and view all the answers

What is the purpose of X-rays?

To treat cancer Signup and view all the answers

What determines how atoms interact with each other?

The arrangement of electrons in each atom Signup and view all the answers

What do all the orbitals in the same sublevel have in common?

The same amount of energy Signup and view all the answers

What is the principal quantum number (N) in electron configuration?

The energy level and size of the orbital Signup and view all the answers

What happens to the energy and distance from the nucleus as the principal quantum number (N) increases?

The energy increases and the distance from the nucleus increases Signup and view all the answers

What is the relationship between the row of the periodic table and the coefficient in electron configuration?

The coefficient is one less than the row Signup and view all the answers

What determines an atom's reactivity with other elements?

The number of valence electrons Signup and view all the answers

What can students do with the knowledge of electron configuration and orbital diagrams?

Construct the appropriate electron configuration and orbital diagram for a given element Signup and view all the answers

What can students identify on the periodic table?

The alkali metals, alkaline earth metals, transitional metals, halogens, noble gases, metals, non-metals, and metalloids Signup and view all the answers

Study Notes

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.