CHEM UNIT 1 AND 2

Group

Columns in the periodic table, Their valency is the same.

Period

The rows in the periodic table, the number of shells are the same

Valence Electrons

The number of electrons on the outermost shell

Oxidation Number

Valency with charge

Isotopes

Same element, same atomic number, but different mass number, and different neutrons

Ions

Electrically charges particles, either has gained electrons or lost electrons

Ionization Energy

The energy required to remove an electron from the outermost shell, from a gaseous atom, because it is easies to remove electrons in a gas state

Increases up the group, and right across the period (Upper right corner)

Electronic Affinity

It is the energy change that occurs when a neutral atom in the gaseous state gains an electron to form a negative ion. It is a measure of how strongly an atom attracts an extra electron and is typically expressed in units like kilojoules per mole (kJ/mol)

Electronegativity

The tendency to attract a shared pair of electrons

Increases from left to right across a period, increases up the group (Upper right-hand corner)

Metals

Substances that can lose electrons (electropositive)

Non-Metals

Substances that can gain electrons (electronegative)

Alkali Metal Physical Properties

Soft, Silvery Metals

Low melting and boiling points

Low density

All properties of metals

Alkali Metals Chemical Properties

Highly Reactive

Form 1+ Ions

Reacts with oxygen and water

Transition Metal, Physical Properties

High Density

High melting and boiling points

Metallic Properties

Halogens, Physical Properties

Non-metals

Colored Gases

They are all soluble in organic solvents

Halogens, Chemical Properties

Highly Reactive

Strong oxidizing agents

In nature, they exist as diatomic particles

Bromine - Orange

Chlorine - Yellow-Green

Noble Gases

Colorless, Odorless, Tasteless

Under standard conditions, they are gases

Low solubility

Low melting/boiling points

Highly stable

Inert

Monatomic

Metal and Non-Metal Bonding

Ionic Bonding - transfer of an electron from a metal to a non-metal

They are non actually bonded but, have a very strong electrostatic force of attraction

Properties: Crystalline Solids, High melting and boiling points, Molten/Solution conducts electricity

Non-Metal and Metal

Covalent Bonds - no electrons are lost, both non-metals share them

Properties: Are liquids/gases at RTP, Low melting/boiling points, Don’t conduct electricity

Metal and Metal

Metallic Bonding - attraction between the negatively charged, mobile electons

Electrons are free-roaming in the sea of electrons

Always the same element

Ammonium

NH4 Valency: +1

Hydroxide

OH Valency:-1

Sulfate

SO4 Valency: -2

Sulfite

SO3 Valency: -2

Carbonate

CO3 Valency:-2

Phosphate

PO4 Valency:-3

Nitrate

NO3 Valency:-1

Matter

Anything that has mass and takes up space

Pure Substances

Made up of only one type of particle

Impure Substances

Made up of multiple types of particles

Element

Anything that is made up of a single type of atoms

Element

Made up of one type of atom

Compound

Made of two or more elements that are chemically bonded in a fixed ratio

Mixture

Made of more than one element that is not in a fixed ratio

Homogenous Mixtures

Have a uniform composition

Heterogenous Mixture

Have a non-uniform composition

Solids

Solids have the highest intermolecular force of attraction, they have a fixed volume, vibrate in place, and they keep their form

Liquid

Liquids have the second highest intermolecular force, have a fixed volume, take the shape of their container, move semi-fast

Gas

Gases have the lowest intermolecular force, they move freely and quickly, with no fixed volume

Solid to Liquid

Melting

Liquid to Solid

Freezing

Liquid to Gas

Boiling/Evaporation

Differences between Evaporation and Boiling
Evaporation	Boiling
Evaporation is a normal process that occurs when the liquid form changes into the gaseous form; while causing an increase in the pressure or temperature.	Boiling is an unnatural process where the liquid gets heated up and vaporized due to continuous heating of the liquid.
Evaporation usually occurs on the heated liquid’s surface.	Boiling usually occurs on the entire mass of the liquid that gets heated up.
Bubbling effect is not visible in evaporation.	Bubbling effect is visible during the process of boiling.
The process of evaporation is slow.	The process of boiling is much quicker.

Gas to Liquid

Condensation

Gas to Solid

Sublimation

Solid to Gas

Deposition

Crystallization

The process of boiling, removes soluble impurities from a liquid

Magnetic Separation

Separates magnetic materials from non-magnetic materials

Filtration

Separates insoluble solids from a liquid or solution

Tripod, Filter Paper, Filter Funnel, Beaker, Funnel

Chromatography

A separation process that is used to separate two solids is used to create the same ink. 

Chromatography paper, Solvent, Beaker, Lid

Distillation

The action of purifying a liquid by the process of heating and cooling. It can be used to separate two liquids that have different boiling points by heating them to evaporate one of them and then cooling to condense it while the other remains a liquid.

Round-bottom beaker, Cork, Temperature, Condenser, Bunsen Burner

Fractional Distillation

Fractional distillation is a more advanced type of distillation that uses a fractionating column to separate liquids with closely related boiling points. The main difference lies in the apparatus: fractional distillation's column, often filled with packing material, allows for repeated vaporization and condensation cycles to achieve a more precise separation, which is necessary when the boiling point differences are small

Solubility

When two substances are combined within a solution, they can either be soluble and insoluble. A substance that is soluble, will ocmplet

Solvent

Substance that dissolves a solute (Greater Quantity)

Solute

A substance that dissolves in a solvent (Lesser Quantity)

Saturated Solution

Maximum amount of solute possible in the solvent possible at room temperature

Unsaturated Solution

An unsaturated solution contains less than the maximum amount of solute possible

Supersaturated Solution

Holds more solute than normally possible. This happens when the solution is heated to a high temperature, more solute is added, and then the solution is cooled quickly.

Colloid

A homogeneous solution is made up of larger particles, but the substance remains evenly distributed throughout. It is a combination of two substances, where the molecules of one substance are much larger than those of the other substance, but they are still evenly distributed throughout

Sol

Colloidal Suspension with solid particles in a liquid

Emulsion

Colloidal Suspension with liquid particles in liquid. 

Foam

Colloidal Suspension with gas in liquid or gas in solid

Aerosol

Colloidal Suspension with solid or liquid particles in gas

Gel

Colloidal Suspension with liquid paritcles in solid

Solid Sol

Colloidal Suspension with solid in solid

Colloidal Suspension

A colloidal suspension is a mixture where tiny, insoluble particles are dispersed throughout a continuous medium, and they do not settle out over time.

Diffusion

Diffusion is the movement of particles from higher concentration to lower concentration

Factors that affect diffusion

• Temperature

• Pressure

When a substance is unevenly distributed, there’s a concentration gradient. The particles will undergo the process of diffusion until they reach a state of equilibrium.