Chemistry Chapter 5 Flashcards

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What are energy levels?

The fixed energies an electron can have are called energy levels.

What does quantum refer to in energy?

The amount of energy required to move an electron between energy levels (correct)

The mass of an electron

The speed of light

The size of an atom

What is the quantum mechanical model?

A modern description of electrons in atoms derived from the solutions to the Schrodinger equation.

What does an atomic orbital describe?

It describes the probability of finding an electron at various locations around the nucleus. Signup and view all the answers

What did Bohr propose about electron orbits?

He proposed that an electron is found only in specific circular paths or orbits around the nucleus. Signup and view all the answers

What does the quantum mechanical model determine?

It determines the allowed energies an electron can have and the probability of finding an electron in various locations. Signup and view all the answers

What does each energy sub level correspond to?

Each energy sub level corresponds to one or more orbitals of different shapes. Signup and view all the answers

What is electron configuration?

The arrangement of electrons in various orbitals around the nuclei of atoms. Signup and view all the answers

What does the Aufbau Principle state?

Electrons occupy the orbitals of lowest energy first. Signup and view all the answers

What does the Pauli Exclusion Principle state?

An atomic orbital may describe at most two electrons. Signup and view all the answers

What does spin refer to in quantum mechanics?

Spin is a quantum mechanical property of electrons, indicating their direction of rotation. Signup and view all the answers

What does Hund's Rule state?

Electrons occupy orbitals of the same energy to maximize the number of electrons with the same spin direction. Signup and view all the answers

What are the exponents used in electron configuration for s, p, d, and f orbitals?

s:2, p:6, d:10, f:14. Signup and view all the answers

How are electron configurations represented in order?

They are represented in a diagonal order starting from 1s to 7p. Signup and view all the answers

What is amplitude in terms of wave properties?

Amplitude is the wave's height from zero to the crest. Signup and view all the answers

What does wavelength represent, and how is it denoted?

Wavelength is represented by λ and is the distance between the crests of waves. Signup and view all the answers

What does frequency represent, and how is it denoted?

Frequency is represented by ν and is the number of wave cycles to pass a given point per unit of time. Signup and view all the answers

What are hertz?

Units of frequency equal to cycles per second. Signup and view all the answers

What is included in electromagnetic radiation?

Radio waves, microwaves, infrared waves, visible light, ultraviolet waves, x-rays, and gamma rays. Signup and view all the answers

What happens to sunlight when it passes through a prism?

It separates into a spectrum of colors. Signup and view all the answers

What does the atomic emission spectrum consist of?

The wavelengths of spectral lines characteristic of the element. Signup and view all the answers

What is Planck's constant and its value?

Planck's constant is a value of 6.626 x $10^{-34}$. Signup and view all the answers

What is the photoelectric effect?

Electrons are ejected when light shines on a metal. Signup and view all the answers

What are photons?

Light quanta. Signup and view all the answers

What is the ground state of an atom?

When the electron has the lowest possible energy. Signup and view all the answers

What does the Heisenberg Uncertainty Principle state?

It states that it is impossible to know both the velocity and the position of a particle simultaneously. Signup and view all the answers

What happens when atoms absorb energy?

Their electrons move to higher energy levels. Signup and view all the answers

How does light relate to the photoelectric effect?

Einstein proposed that light could be described as quanta of energy behaving like particles. Signup and view all the answers

What is the relationship between emitted light frequency and electron energy change?

The light emitted has a frequency directly proportional to the energy change of the electron. Signup and view all the answers

How do classical mechanics and quantum mechanics differ?

Classical mechanics describes the motion of large bodies, while quantum mechanics describes subatomic particles and atoms as waves. Signup and view all the answers

Study Notes

Energy Levels and Quantum Concepts

Energy levels refer to the distinct fixed energies an electron can possess.
Quantum denotes the minimal energy needed to relocate an electron between energy levels, indicating that electron energy is quantized.

Quantum Mechanical Model

Represents a modern understanding of electron behavior in atoms, derived from the Schrodinger equation.

Atomic Orbitals

Define the likelihood of an electron's position around the atomic nucleus, influencing electron arrangement.

Bohr Model and Quantum Mechanics

Proposed that electrons occupy specific circular orbits around the nucleus.
The quantum mechanical model establishes possible energies for electrons and predicts their spatial distribution around nuclei.

Electron Configuration Principles

Aufbau Principle: Electrons fill the lowest energy orbitals first.
Pauli Exclusion Principle: Each atomic orbital can accommodate a maximum of two electrons.
Hund's Rule: Electrons fill degenerate orbitals singly before pairing to maximize unpaired spins.

Electron Configuration and Notation

Orbital capacities: s (2), p (6), d (10), f (14).
Follows a diagonal order for filling: 1s, 2s 2p, 3s 3p 3d, etc.

Wave Properties

Amplitude: Refers to the height of a wave from the centerline to its crest.
Wavelength (λ): Distance between successive wave crests.
Frequency (ν): Number of wave cycles that pass a point per unit time, expressed in Hertz (Hz), where 1 Hz equals one cycle per second.

Electromagnetic Radiation and Spectrum

Encompasses various forms such as radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays.
Spectrum: Produced when different wavelengths from sunlight are separated through a prism.

Atomic Emission Spectrum

Characteristic wavelengths of spectral lines for each element contribute to its atomic emission spectrum.

Planck's Constant and Energy Changes

Planck's constant is valued at 6.626 × 10⁻³⁴.
The energy of a quantum can be calculated using the formula E = hv, where h represents Planck's constant and v denotes frequency.
Minor energy changes relate to low-frequency radiation; major changes pertain to high-frequency radiation.

Photoelectric Effect and Photons

Occurs when electrons are emitted from metals upon exposure to light.
Photons are defined as discrete packets of light energy.

Ground State and Energy Absorption

Ground state indicates the lowest energy state of an atom.
Absorption of energy results in electron elevation to higher energy levels; light emission occurs when electrons revert to lower levels.

Heisenberg Uncertainty Principle

States that simultaneous knowledge of a particle's position and velocity is fundamentally impossible.

Classical vs. Quantum Mechanics

Classical mechanics effectively explains motion for larger objects, while quantum mechanics describes the behavior of subatomic particles and atoms as waves.

Studying That Suits You

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

Description

Test your understanding of key concepts in Chemistry Chapter 5 with these flashcards. Focused on energy levels, quantum mechanics, and the modern model of atoms, this quiz will help reinforce your learning and comprehension of essential terms and principles.