SCH3U0

Periodic Table

This table was arranged through atomic number and remains this way till now.

Arranged the elements in increasing atomic mass

97 years later a chemist named Henry Moseley rearranged the periodic table

This table was arranged through atomic number and remains this way till now.

Electronegativity

The tendency of an atom to gain more electrons, this varies with atomic number

The direction of the arrow shows increasing
electronegativity.

Ionization Energy

Simply put, the ionization energy of an atom is the minimum energy required to lose a valence electron.

Francium has the lowest ionization energy as it has more shells in comparison to Helium which has just one shell.

The more shells an atom has the easier it gets to lose a valence electron as it gets further away from the nucleus and isn't held on as strongly.

Atomic Radius

Atomic radius is a measurement found by measuring the size of the atoms from the nucleus to the outermost electron.

Francium has the largest atomic radius as it has the most shells and doesn't hold onto the electrons on the outer shells as tight as Helium does.

Reactivity

Reactivity can be explained as how strongly an atom might react with another atom. It's basically an expenditure of energy.

Highly electropositve and electronegative atoms have a high tendancy to react. This may also depend upon temperature.

Electron Arrangement

Atomic Number

This is how the periodic table is determined today.

This number is determined by the number of protons in the nucleus of any certain atom.

Diagrams

Bohr-Rutherford diagram

This is a Bohr Rutherford diagram of hydrogen

The Bohr=Rutherford diagram is used to show the orbiting
electrons of an atoms nucleus.

Lewis Dot Diagram

This is a Lewis dot diagram of H20. This is an example of a covalent bond between hydrogen and oxygen.

A Lewis dot diagram is used to show the bond between the atoms of a molecule.

Valence Electrons

Chemical Bonds

Ionic Bonds

The result of bonding by 2 oppositely charged ions.

The atom with the valence electron furthest from it's shell gets its electron permantley transfered to the other atom.

The atom losing the electron becomes a positively charged ion and the gaining one becomes negatively charged.

Ions

Polyatomic

A polyatomic ion is an ion which consists of more than 3 atoms.

Example: Sulfate Ion

Diatomic

Diatomic elements can be classified as molecules with only 2 atoms.

There are 7 total diatominc elements and can be easily memorized using HOFBrINCl

Hydrogen, Oxygen, Flourine, Bromine, Iodine, Nitrogen and Chlorine.

A covalent bond is the result of 2 non metal atoms sharing electron pairs hence connecting and making a bond.

The distribution of electron charge throughout the whole molecule joined at the bonds.

An H2O molecule would be a polar molecule because of the unequal electron charge throughout the bonds. The molecule itself has an unsymmetrical shape.

This can be either negative or positive (polar or nonpolar)

This reaction occurs when reactants (2 or more) react together to form a singular product, hence synthesizing themselves.

Decomposition is the complete opposite of synthesis. The synthesized reactants now break up into their original reactant forms.

A single displacement occurs when in the reaction an element needs to be swapped out with another product in the element compound.

A double displacement is when the positive and negative ions of a compound are swapped out with the other negative and positive counter parts of the other compound.

A combustion reaction can only occur in the presence of oxygen. This reaction when completed is often accompanied by light, heat and sound.

Gas Laws

Gay-Lussac's Law

Pressure and temperature are directly proportional. The temperature much remain constant

Boyle's Law

In this, pressure and volume are inversly proportional. The temperature must remain constant.

Charle's Law

I this, volume and temperature are directly proportional to each other. The pressure must remain constant.

Combined Gas Law

The pressure and the volume are proportional as long as the gas temperature is equal to a constant.

Ideal Gas Law

Stays constant

Molar Volume In Gas Units

STP

Standard Temperature Pressure

STAP

Characteristics

A homogenous solution, transparent, aqueous, may be coloured.

Solute particles can be filtered out. Also, precipitate formed when the mixing occurs is created due to the mixture of positive and negatively charged ions.

Components

The Measurement of how much of a substance is mixed into another substance.

Dilution

Making a concentrated substance weaker by diluting it with excess solvent.

Formula: C1V1= C2V2

Standards

Mass/mass%

Mass/Volume%

Volume/Volume%

PPM Concentration

Used to measure miniscule substance concentrations. (PPM= Parts Per Million)

Can also be calculate further using PPB and PPT (Parts Per Billion and Parts Per Trillion). These can be used to trace contaminants in water sources.

Can be used for quality testing in air quality, metal, plastic parts in food and pollutants in water supplies.

6-9 PPM is considered polluted, First Nations in Canada are now suffering from polluted water sources.

Molar Concentration

Calculated by c= n/V or M= n/V

Acids And Bases

Properties

Acid: Forms electrolytes Produces hydronium ions and they taste sour.

Base: Also forms electrolytes, produces hydroxide ions in water and tastes bitter.

pH Scale

A logarithmic scale is used to determine the acidic or basic levels or a solution.

Acids are solutions with a pH of under 7 and bases are above 7

Quantities in Chemical Reactions

Limiting Reactant

The reactant in the equation which will run out first. This is limiting because without this the reaction cannot advance.

Excess Reactant

Simply the other reactant which still remains after the completion of the reaction.

Stoichiometric Ratio's

Example= 2H2O= 2NO3
The mol:mol ration for O is 2 because they each have 2 moles in front.

Empirical Formula

Simplified formula with minimal rations

Molecular Formula

Finding the number of individual atoms in the equation.