3U Chemistry

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Elementary Math (MTE280)

由Cindy Ambriz

SBI 4U

由Allister Braganza

Chemistry Concept Map

由Aljdidani Jelnar

Chemistry Chemistry is ultimately the study of matter including how it behaves and . Additionally in this unit we talked about how to describe properties and changes using diagrams and nomenclature, and equations.

由Ragubavan Sathurtheha

3U Chemistry

Reactions

Writing Chemical Equations

Solubility rules

shows you which elements are insoluble

Activity series

a list of decreasing order of their reactivity

Balancing equations

To even out the amount of an element on the other side of the reaction

types of reactions

Combustion (C2H2+O2=H2O+CO2)

can also be incomplete

Double displacement ( AB+CD=AD+CB)

Single displacement (A+BC=AC+B)

Decomposition (AB=A+B)

Synthesis ( A+B=AB)

Forces and Bonds

Lewis Structures and VSEPR Diagrams

VSEPR diagrams are used to predict the geometry of a molecule from the number of atoms that are bordering the central atom

Lewis structures show which atoms are bonded together in a molecule

Chemical Bonding and Electronegativity

Electronegativity is When an atom is bonded, it has the potential to draw individual electrons to itself.

Ionic bonds

Polar covalent bonds

Non-polar covalent bonds

Intramolecular Forces

Occur within the molecule

ionic

the transfer of one or more electrons between a metal and non-metal

Covalent

sharing of electrons between two non-metals

Intermolecular forces

Occurs between molecules

Hydrogen Bonding

Polar molecules but a hydrogen has to be bonded to a F, O, N

Dipole-Dipole

Polar molecules only are held together due to their partial charges

London Dispersion

Polar and non-polar molecules form temporary bonds by the constant movement of electrons causing a short-term charge imbalance

Stoichiometry

Acids and Bases

PH scale

it tells us how basic or acidic the solution is.

Bases

A base is a substance with a PH greater than 7 that can neutralise an acid by reacting with hydrogen ions.

Bronsted-Lowry theory, Arrhenius theory

Acids

With a PH less than 7, an acid is a molecule or ion capable of contributing a proton or, alternatively, forming a covalent bond with an electron pair.

Titrations

Used to determine the concentration of a solution

The relationship between the relative quantities of the reactants in a reaction.

Limiting and access reactants

Access Reactant

A reactant that remains after the reaction is complete

Limiting Reactant

A reactant that is completely consumed during a chemical reaction

Calculated using mole to mole ratio, mass, volume, concentration, molar mass

Gases

Gas stoichiometry

Ideal Gas Law

PV=nRT

STP and SATP

Gas Law

Gay-Lussak's Law

States that temperature and pressure are directly proportional while the volume remains constant

Charle's Law

States that temperature and volume are directly proportional as long as mass and pressure remain constant

Boyle's Law

States that pressure and volume are inversely proportional as the temperature and mass remain constant

Kinetic Molecular Theory

Particles of gas are in constant motion and collide with one another

Gas is mostly empty space

Pressure is exerted when particles hit the sides of the container while causing collisions

We assume that particles do not interact with each other

Average kinetic energy is proportional to the temperature

Periodic table

Element Properties

atomic weight is the number off neutrons

Atomic number is the amount of electrons and protons

Periodic table groups

alkali metals, alkaline earth metals, transition metals, metalloids, other metals, non metals, halogens, noble gases and rare earth elements

Periodic trends

First Ionization Energy

The energy required to move one of the loosely held electrons from the gaseous atom

Electron Affinity

When an atom can attract bonded electrons

Atomic Radius

The distance from the middle of the nucleus to the outermost shell. As the energy levels increase the radius does too