COVID-19 Awareness and Atomic Structure

Flashcards covering key vocabulary and concepts related to COVID-19 awareness and atomic structure, helping in exam preparation.

COVID-19

Caused by a virus known as Severe Acute Respiratory Syndrome Coronavirus-2 (SARS-CoV-2).

Symptoms of COVID-19

Fever or chills, cough, difficulty in breathing, cold, headache, diarrhea, loss of taste/smell, and other non-specific symptoms.

Transmission of COVID-19

Spread through respiratory droplets, airborne, and contaminated surfaces.

Prevention of COVID-19

Adhere to safety protocols including respiratory hygiene, hand hygiene, physical distancing, and avoiding crowds.

Democritus

First proposed the particulate nature of matter, calling it atoms around 500 BC.

Aristotle

Proposed that matter was continuous and had no smaller particles and named it 'Hyle'.

What two laws were Dalton's theory based on

Law of mass destruction

Law of indefinite proportion

John Dalton

First put forward a scientific theory about the physical and chemical properties of atoms.

The Law of Definite Proportions

States that a chemical compound always contains exactly the same proportion of elements by mass.

The Law of Conservation of Mass

States that mass cannot be created or destroyed in a chemical reaction.

Dalton's Atomic Theory Postulates

1. Elements are made of indivisible atoms. 2. Atoms cannot be created or destroyed. 3. Atoms of the same element are identical. 4. Atoms combine in simple ratios to form compounds.

Indivisibility of Atoms

Incorrect aspect of Dalton's theory; atoms are made of sub-atomic particles (protons, neutrons, electrons).

Sub-atomic Particles

Particles that make up atoms, including protons, neutrons, and electrons.

Quarks

Elementary particles that make up protons and neutrons.

Isotopes

Atoms of the same element that have different masses.

Hydrogen Isotopes

Protium (1H), Deuterium (2H), Tritium (3H).

Dalton's Atomic Model

A small indivisible hard ball model of atoms.

J.J. Thompson's Model

Plum pudding model, representing a solid sphere with electrons embedded in it.

Ernest Rutherford's Model

Nuclear atom model with a massive central nucleus and electrons in orbit.

Planetary Model

Model by Neil Bohr depicting electrons moving in orbits around the nucleus.

Wave Mechanical Model

Model posited by Schrödinger incorporating wave-particle duality of electrons.

Wave-Particle Duality

Concept that electrons exhibit both wave-like and particle-like properties.

Uncertainty Principle

States it is impossible to know both the position and momentum of an electron simultaneously.

Schrödinger Equation

An equation derived to describe the behavior of electrons in atoms.

Wave Function (Ψ)

Mathematical representation of an electron's probability distribution.

Orbital

Volume of space around the nucleus where there is a high probability of finding an electron.

Quantum Numbers

Set of numbers that describe the properties of atomic orbitals and electrons.

Principal Quantum Number (n)

Indicates the energy level and proximity of an electron to the nucleus.

Orbital Quantum Number (l)

Defines the shape of an orbital, ranging from 0 to n-1.

Magnetic Quantum Number (mₗ)

Describes the orientation of orbitals in space.

Spin Quantum Number (mₛ)

Represents the direction of an electron's spin, with possible values of +1/2 or -1/2.

Aufbau's Principle

Electrons fill the lowest energy orbitals first.

Hund's Rule

Electrons occupy degenerate orbitals singly before pairing up.

Pauli's Exclusion Principle

No two electrons in an atom can have the same set of four quantum numbers.

Electron Configuration

The arrangement of electrons in an atom's orbitals.

1s orbital

The spherical orbital closest to the nucleus.

2s orbital

The spherical orbital in the second energy level.

2p orbital

The dumbbell-shaped orbital which can hold a maximum of six electrons.

3s orbital

Spherical orbital in the third energy level.

3p orbital

Dumbbell-shaped orbital in the third energy level.

3d orbital

Complex-shaped orbital found in the third energy level and can hold a maximum of 10 electrons.

4s orbital

Spherical orbital in the fourth energy level.

4p orbital

Dumbbell-shaped orbital in the fourth energy level.

4d orbital

Complex-shaped orbital in the fourth energy level.

4f orbital

Complex-shaped orbital in the fourth energy level.

Electron Orbital Diagram

A visual representation of electron configurations in subshells.

Quantum Number Sequence for Transition Metals

Describes the filling of d orbitals in transition metals.

Stability in Electron Configuration

Occurs when 3d and 4s orbitals are half-filled or fully filled.

Periodic Table Arrangement

Elements arranged by increasing atomic number and filling of orbitals.

Atomic Mass

Total number of protons and neutrons in the nucleus of an atom.

Noble Gas Configuration

Using noble gases to simplify electron configuration notation.

Core Electrons

Electrons in the inner shells of an atom, not involved in bonding.

Valence Electrons

Electrons in the outermost shell that are involved in chemical bonding.

Chemical Bonding

The joining of atoms to form new chemical substances.

Ionic Bonding

Bond formed when electrons are transferred from one atom to another.

Covalent Bonding

Bond formed when atoms share electrons.

Metallic Bonding

Bond formed between metal atoms where electrons are shared collectively.

Electronegativity

A measure of an atom's ability to attract and hold onto electrons.

Mole Concept

A method of quantifying atoms and molecules based on moles.

Avogadro's Number

6.022 x 10²³, the number of particles in one mole of a substance.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Chemical Reaction

A process that leads to the transformation of one set of chemical substances to another.

Reactants

The starting materials in a chemical reaction.

Products

The substances formed as a result of a chemical reaction.

Balanced Chemical Equation

An equation representing a chemical reaction with equal numbers of atoms for each element on both sides.

Concentration

The amount of solute in a given volume of solution.

pH Scale

A logarithmic scale used to measure the acidity or basicity of a solution.

Catalyst

A substance that increases the rate of a chemical reaction without being consumed.

Equilibrium

The state in a reversible chemical reaction when the concentrations of reactants and products remain constant over time.

Le Chatelier's Principle

When a system at equilibrium is disturbed, it will shift in a direction to counteract the disturbance.

Thermodynamics

The study of heat, energy, and work in chemical processes.

Exothermic Reaction

A reaction that releases energy in the form of heat.

Endothermic Reaction

A reaction that absorbs energy from its surroundings.

Kinetic Molecular Theory

Explains states of matter based on particle motion.

Gas Laws

Laws that describe the behavior of gases in relation to pressure, volume, and temperature.

Ideal Gas

A hypothetical gas whose particles occupy negligible space and have no interactions.