Atomic Structure and Electron Arrangement

Podcast Beta

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What determines how atoms interact with each other?

The atomic number of the atom

The arrangement of electrons in each atom (correct)

The mass number of the atom

The average atomic mass of the element

What is the principal quantum number (n) related to?

The average atomic mass of an element

The mass number of an atom

The energy level and size of the orbital (correct)

The atomic number of an element

What is the difference in the coefficient for the d block compared to the row in the periodic table?

It is two less than the row

It is one more than the row

It is one less than the row (correct)

It is the same as the row

Why is an atom with more valence electrons more likely to react with other elements?

Because it is more likely to gain or lose electrons Signup and view all the answers

What do the rows in the periodic table correspond to?

The coefficient in electron configuration Signup and view all the answers

What is the purpose of constructing an electron configuration and orbital diagram for a given element?

To understand how an atom will interact with other atoms Signup and view all the answers

What determines the physical properties of an atom?

The distribution of subatomic particles Signup and view all the answers

What is the term for the last shell level?

Orbital Signup and view all the answers

What is the main reason why electrons in the same orbital must have a different spin?

To obey the Pauli Exclusion Principle Signup and view all the answers

Which of the following types of waves has a wavelength similar to that of radio waves?

Microwave Signup and view all the answers

What is the primary function of the protons in the nucleus of an atom?

To attract the electrons and keep them close Signup and view all the answers

What is the term for the distribution of electrons in an atom?

Electron configuration Signup and view all the answers

Which of the following rules states that in a sublevel, all orbitals should get one electron before pairing up?

Hund's Rule Signup and view all the answers

What is the term for the different versions of an element with different numbers of neutrons?

Isotope Signup and view all the answers

What is the main purpose of using X-Ray waves?

To take medical images Signup and view all the answers

What is the term for the area around the nucleus where there is a negative charge?

Electron cloud 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.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Description

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.