Grade 12 University Preparation Chemistry - SCH4U1 Course Overview

These flashcards cover key vocabulary and concepts from the Grade 12 University Preparation Chemistry course, including terminology related to chemical bonding, molecular properties, and foundational principles in chemistry.

Organic Chemistry

The study of the structure, properties, composition, reactions, and preparation of carbon-containing compounds.

Electrochemistry

The branch of chemistry that deals with the relationship between electricity and chemical reactions.

Chemical Equilibrium

A state in which the concentrations of reactants and products remain constant over time.

Scientific Investigation Skills

Skills required to conduct research, including initiating and planning, performing and recording, analyzing and interpreting, and communicating results.

Covalent Bonds

Chemical bonds formed between two non-metal atoms through the sharing of electrons.

Ionic Bonds

Bonds formed between a metal and a non-metal, resulting from the transfer of electrons.

Electronegativity

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

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule, determined by the bonds and lone pairs around the central atom.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

A model used to predict the shape of molecules based on the repulsion between electron pairs.

Hydrogen Bonds

Strong intermolecular forces occurring between hydrogen and highly electronegative atoms such as fluorine, oxygen, or nitrogen.

Surface Tension

The cohesive force at the surface of a liquid that causes it to behave as if it were covered with a stretched elastic membrane.

Intermolecular Forces

Forces of attraction or repulsion between molecules, which influence properties such as boiling point and melting point.

Aufbau Principle

A rule stating that electrons occupy the lowest energy orbitals available before filling higher energy levels.

Lewis Diagrams

Diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons.

Isoelectronic Particles

Particles that have the same electron configuration.

Quantum Mechanical Model of the Atom

A model where electrons are described as wave functions, giving a probability distribution for their positions.

Molecular Polarity

A property that describes the unequal sharing of electrons in a molecule, resulting in partial positive and negative charges.

Chemical Bonds

Forces that hold atoms together in molecules or compounds, including ionic, covalent, and metallic bonds.

Organic Chemistry

The study of the structure, properties, composition, reactions, and preparation of carbon-containing compounds.

Electrochemistry

The branch of chemistry that deals with the relationship between electricity and chemical reactions.

Chemical Equilibrium

A state in which the concentrations of reactants and products remain constant over time.

Scientific Investigation Skills

Skills required to conduct research, including initiating and planning, performing and recording, analyzing and interpreting, and communicating results.

Covalent Bonds

Chemical bonds formed between two non-metal atoms through the sharing of electrons.

Ionic Bonds

Bonds formed between a metal and a non-metal, resulting from the transfer of electrons.

Electronegativity

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

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule, determined by the bonds and lone pairs around the central atom.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

A model used to predict the shape of molecules based on the repulsion between electron pairs.

Hydrogen Bonds

Strong intermolecular forces occurring between hydrogen and highly electronegative atoms such as fluorine, oxygen, or nitrogen.

Surface Tension

The cohesive force at the surface of a liquid that causes it to behave as if it were covered with a stretched elastic membrane.

Intermolecular Forces

Forces of attraction or repulsion between molecules, which influence properties such as boiling point and melting point.

Aufbau Principle

A rule stating that electrons occupy the lowest energy orbitals available before filling higher energy levels.

Lewis Diagrams

Diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons.

Isoelectronic Particles

Particles that have the same electron configuration.

Quantum Mechanical Model of the Atom

A model where electrons are described as wave functions, giving a probability distribution for their positions.

Molecular Polarity

A property that describes the unequal sharing of electrons in a molecule, resulting in partial positive and negative charges.

Chemical Bonds

Forces that hold atoms together in molecules or compounds, including ionic, covalent, and metallic bonds.

Acid

A substance that produces H^+ ions when dissolved in water.

Base

A substance that produces OH^- ions when dissolved in water.

pH Scale

A logarithmic scale used to specify the acidity or basicity of an aqueous solution, ranging from 0 (very acidic) to 14 (very basic), with 7 being neutral.

Stoichiometry

The calculation of quantities of reactants and products in chemical reactions.

Chemical Reaction

A process that involves rearrangement of the molecular or ionic structure of a substance, as opposed to a change in physical form or a nuclear reaction.

Redox Reaction

A chemical reaction in which the oxidation states of atoms are changed; involves both reduction and oxidation processes.

Catalyst

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

Activation Energy

The minimum amount of energy required to initiate a chemical reaction.

Exothermic Reaction