CH4 +2O2 → CO2 + 2H2O

Chemical compound

bond polarity(Intramolecular forces)

Molecular

Valence shell electron pair repulsion theory

Vsepr shape allows us to predict the individual molecule structure and it's polarity based on the number of electron pairs that surround the center atom.

Polarity

Polar

Non-polar

Intermolecular forces(molecule polarity)

London dispersion

Electrons are always moving, sometimes they bunch up on one side of an atom, causing them to be slightly negative.

If this happens to a neighbouring molecule at the same time there would be a temporary attraction called London dispersion.

Dipole-Dipole

This intermolecular force forms between a slightly negative end of one Polar molecule and a slightly positive end of a neighbouring molecule causing them to pull towards each other

Hydrogen bonding

A special type of dipole-dipole which occurs between hydrogen and either oxygen, nitrogen and fluorine. This intermolecular has a strong attraction because of big difference in electronegativities.

This type of forces is between the molecules(weak)

sharing electrons

Ionic

Transfer of electrons

The type of bond will be determined by the difference in electronegativity of two atoms.

This type of force is within the molecules(strong)

atoms

Proton

Neutron

Electron

Atomic theory

Atomic mass

Multivalent

Isotopes

Average weight

Non-metals

Anion

Metals

Cation

Diagram

Properties

Physical

Chemical

Trends

Solution and gases

Titration

Is the process to measure the concentration or volume of a substance by adding a certain amount of another substance

Solubility curves

The relationship between solubility and temperature can be expressed by a solubility curve.

Reading solubility curves

Unsaturated

Below the line

Saturated

Directly at the line

Super Saturated

Above the line

Solubility curves shows the maximum amount of solute that can be dissolved in a given amount of water over a range of temperatures.

Acids

Binary

hydrochloric acid (HCl)

contains a hydrogen and another nonmetal

Oxyacids

''Ous''acids

Nitrous acid(HNO2)

''ic'' acids

Nitric acid(HN3)

It contains hydrogen and a polyatomic that has hydrogen.

Substances that produce hydrogen ions in solution and donate proton to another compund.

Bases

Substances that produce hydroxide ions and take a proton from another compound.

Most of the bases contain a metal and a hydroxide polyatomic group.

Potassium hydroxide(KOH)

Bronsted-Lowry Acid and Bases

When an acid and base are mixed together, the acid will transfer a proton to the base.

HCL + H2O = H3O + CL

hydrochloric acid (The Bronsted Lowry acid)

Water (The Bronsted Lowry base)

Hydronium (The conjugate Acid)

Chlorine gas ( The conjugate base)

Indicators

indicators are chemicals that when it is dissolved in acid or bases it would change the colour so it would make it easier for us to recognize them.

Most acid and bases are colourless and clear it's hard to distinguish them so it's better to use indicators

Quantities in chemistry

Factor label formula

Units

Kg

L

What you can find=what you know X the fraction(s)you need to get to the answer

We use this formula to switch back and forth between different units and muasurments

Avogadro

Avogadro discovered in exactly 12g of carbon there were 6.02 x 10*23 carbon atmos. this number is called ''Mole''

1 Mole=6.02 x 10*23 things

Concentration

n

C

V

Dilution

Initial

Stock solution

Final

Stoichiometry

The study of quantitative relationships in chemical reactions

limiting and excess reactants

In chemistry we use stoichiometry to determine which reactant yields the smaller mass of product in a chemical reaction.

Molar mass

Mass

Yield

How much of a product we expect to get based on calculations

Percent Yield=Actual Yield/Theoretical Yield x 100%

Chemical reaction

Types

Decomposition

When one reactant breaks to form multiple products

Combustion

When a fuel (especially hydrocarbons) burns with oxygen to form carbon dioxide and water.

Synthesis

When two or more reactants combine and form a new product

Neutralization

This type of reaction happens when an acid and a base combine to form water and salt.

Displacement

Double

Double displacement will not happen unless either water or a precipitate is being formed.

To predict if the double displacement reaction can occur or not we should use solubility rules chart.

Single

When a free element replaces with a less active element that is in a chemical compound. (based on reactivity charts of metals and non-metals)

word equation

Methane reacts with Oxygen gas to produce Carbon dioxide and water.

Solution

Solute

Solubility

Soluble

Insoluble

Percipitate

a solid formed in a chemical reaction

ability of a solute to dissolve

The measurement of how well a solute will dissolve in a solvent at a given pressure and temperature

The pure substance being dissolved

Solvent

The pure substance that will dissolve the solute.

Chemical equation

Balancing

Law of conservation of mass (Lavoisier)

In chemical reactions, no mass is lost or gained.

Reaction/No reaction

First ionization energy

How easy it is for an atom to lose electron. Easier to lose= lower ionization energy

PH scale

Between 0-6.9

Between 7.1-14

Neutral(7)

If all electron density regions are the same which they should be all bonded electrons then the molecule is non-polar because of the symmetry

If there are any lone pairs (it means nonbonding) on the central atom, then the molecule is polar. but there are exceptions: linear and square planer

Difference in electronegativity

equals to zero

more than zero bigger or equal to 1.7

more than 1.7

The further it gets from neutral the stronger acid or base is