NATURE OF MATTER & CHEMICAL PRINCIPLES

Flashcards covering the nature of matter, states of matter, atomic structure, periodic table trends, chemical bonding, separation techniques, reaction types, reactivity series, redox, qualitative analysis and gas tests.

Matter

Anything that has mass and occupies space.

Particle Theory of Matter

A theory stating that: 1. Matter is made of tiny particles. 2. Particles are constantly moving. 3. There are spaces between particles. 4. Particles attract each other. 5. Heating increases particle movement.

Properties of Solids

Fixed shape, fixed volume, and particles closely packed.

Properties of Liquids

Fixed volume, no fixed shape, and takes the shape of the container.

Properties of Gases

No fixed shape, no fixed volume, and easily compressed.

Melting

The change of state from solid to liquid.

Freezing

The change of state from liquid to solid.

Evaporation

The change of state from liquid to gas.

Condensation

The change of state from gas to liquid.

Sublimation

The direct change of state from solid to gas.

Atom

The smallest particle of an element that retains its chemical properties.

Proton

A positively charged particle found in the nucleus.

Neutron

A neutral particle found in the nucleus.

Electron

A negatively charged particle found outside the nucleus.

Atomic number

The number of protons in an atom.

Mass number

The sum of the number of protons and the number of neutrons.

Calculation for Neutrons

$$\text{Mass number} - \text{Atomic number}$$

Periodic Table

An arrangement of elements according to increasing atomic number.

Groups

Vertical columns in the Periodic Table.

Commonalities of Group Elements

Elements in the same group have the same number of outer-shell electrons and similar properties.

Periods

Horizontal rows in the Periodic Table.

Period Number

Indicates the number of electron shells in an atom.

Noble Gases

Elements found in Group 18 (also known as Group VIII or 0).

Properties of Metals

Conduct heat, conduct electricity, malleable, and ductile.

Properties of Non-metals

Poor conductors, brittle, dull, and usually have low melting points.

Malleable

The property of a material that allows it to be hammered into sheets.

Ductile

The property of a material that allows it to be drawn into wires.

Filtration

A technique used to separate sand from water.

Residue

The substance that remains on the filter paper after filtration.

Filtrate

The liquid that passes through the filter paper during filtration.

Evaporation (Technique)

A technique used to separate salt from seawater.

Crystallisation

A technique used for obtaining pure crystals.

Simple Distillation

A technique used to obtain a pure solvent from a solution.

Fractional Distillation

A technique used for separating miscible liquids with different boiling points.

Chromatography

A technique used for separating coloured substances.

Separating Funnel

An apparatus used to separate oil and water.

Ionic Bonding

The transfer of electrons between a metal and a non-metal, forming positive and negative ions.

Covalent Bonding

The sharing of electrons between non-metals.

Metallic Bonding

Positive metal ions surrounded by delocalized electrons.

Sodium Chloride Bonding

Ionic bond.

Oxygen Gas ($O_2$) Bonding

Covalent bond.

Sodium ion

$$Na^+$$

Potassium ion

$$K^+$$

Ammonium ion

$$NH_4^+$$

Magnesium ion

$$Mg^{2+}$$

Calcium ion

$$Ca^{2+}$$

Zinc ion

$$Zn^{2+}$$

Aluminium ion

$$Al^{3+}$$

Chloride ion

$$Cl^-$$

Hydroxide ion

$$OH^-$$

Nitrate ion

$$NO_3^-$$

Sulfate ion

$$SO_4^{2-}$$

Carbonate ion

$$CO_3^{2-}$$

Magnesium chloride

$$MgCl_2$$

Aluminium oxide

$$Al_2O_3$$

Calcium nitrate

$$Ca(NO_3)_2$$

Ammonium sulfate

$$(NH_4)_2SO_4$$

Law of Conservation of Matter

Matter cannot be created or destroyed during a chemical reaction.

Balanced Equation

An equation with equal numbers of each atom on both sides.

Molecular Equation

An equation that shows compounds as whole substances.

Ionic Equation

An equation that shows only the ions actually involved in the reaction.

Spectator Ions

Ions that do not take part in the reaction.

Acid

A substance that produces $H^+$ ions in water.

Base

A substance that neutralizes an acid.

Alkali

A soluble base.

Salt

A compound formed when the hydrogen in an acid is replaced by a metal or ammonium ion.

pH of Acids

Below $7$.

pH of Alkalis

Above $7$.

pH of Neutral Substances

$7$.

Acid on Blue Litmus

Turns red.

Alkali on Red Litmus

Turns blue.

Neutralisation

$$\text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water}$$

Acid + Metal Reaction

$$\text{Salt} + \text{Hydrogen}$$

Acid + Carbonate Reaction

$$\text{Salt} + \text{Water} + \text{Carbon dioxide}$$

Acid + Hydrogen Carbonate Reaction

$$\text{Salt} + \text{Water} + \text{Carbon dioxide}$$

Combination Reaction

A reaction where two or more substances form one product.

Decomposition Reaction

A reaction where one compound breaks into simpler substances.

Displacement Reaction

A reaction where a more reactive element replaces a less reactive one.

Precipitation Reaction

The formation of an insoluble solid from two solutions.

Reactivity Series

$$K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Ag > Au$$

Potassium (Reactivity)

The most reactive metal in the series.

Gold (Reactivity)

The least reactive metal in the series.

Electrolysis Extraction

Used for extracting potassium, sodium, calcium, magnesium, and aluminium.

Carbon Reduction Extraction

Used for extracting zinc, iron, and lead.

Oxidation

Loss of electrons, gain of oxygen, or increase in oxidation number.

Reduction

Gain of electrons, loss of oxygen, or decrease in oxidation number.

Redox Reaction

A reaction where oxidation and reduction occur simultaneously.

Oxidizing Agent

A substance that causes oxidation and is itself reduced.

Reducing Agent

A substance that causes reduction and is itself oxidized.

$Cu^{2+} + NaOH$ precipitate

Blue precipitate.

$Fe^{2+} + NaOH$ precipitate

Green precipitate.

$Fe^{3+} + NaOH$ precipitate

Reddish-brown precipitate.

$Zn^{2+} + NaOH$ precipitate

White precipitate soluble in excess.

$Al^{3+} + NaOH$ precipitate

White precipitate soluble in excess.

$Ca^{2+} + NaOH$ precipitate

White precipitate insoluble in excess.

$NH_4^+$ warmed with $NaOH$ result

Produces ammonia gas.

Test for Carbonate Ions

Add acid; produced $CO_2$ turns limewater milky.

Test for Sulfate Ions

Add barium chloride; a white precipitate forms.

Test for Chloride Ions

Add silver nitrate; a white precipitate forms.

Test for Bromide Ions

Add silver nitrate; a cream precipitate forms.