This is a draft cheat sheet. It is a work in progress and is not finished yet.
Matter
Everything is made up of matter. |
Matter is made up of atoms. |
Classification of matter
Periodic Table
Table of all known elements arranged from left to right and top to bottom in order of increasing atomic number, or the number of protons. |
Columns: Refer to groups of the table |
Rows: Refer to as periods or the families of the table |
Structure of the Periodic Table
Elements, Compounds, and Mixtures
Element: A pure substance made from one type of atom. |
E.g. Sodium Formula: Na |
Compounds: Made from more than one type of atom bonded together. |
E.g. Sodium
Hydroxide
Formula: NaOH |
Mixtures: Made of substances which are not chemically bonded and can be separated. |
E.g. Salt Water Formula: NaCl |
Information on the Periodic Table
Atomic Number |
Atomic Mass |
| |
Number of Protons |
Number of Neutrons |
Number of Electrons |
|
|
Atoms:
Atoms consist of three subatomic particles protons, Neutrons, and Electrons. |
Electron Configurations
The shells are numbered beginning with the shell closest to the nucleus and increasing in number farther away from the nucleus. |
Electron Shell Diagrams
Electron shells are numbered from the shell closest to the nucleus outwards.
Electrons
Electrons:
Particles orbiting the nucleus
of the atom |
Properties:
Negatively charged
No mass |
Electrons orbit the nucleus in electron shells. |
| |
Maximum Number of electrons: |
The first electron shell holds |
2 atoms |
The second electron shell holds |
8 atoms |
The third electron shell holds |
8 atoms |
The Law of Conservation of Mass
The mass in an isolated system can neither be created nor be destroyed but can be transformed from one form to another |
Acid-Metal Reactions
Metals react with acids to form a salt and hydrogen. |
| |
Identification: Pop Test |
The presence of hydrogen gas can be determined by placing a lit splint near the test tube. |
Hydrogen reacts causing a squeaky pop sound. |
Acid + Metal General Formula
Exothermic and Endothermic Reactions
All chemical reactions either use energy or release energy. |
Reactions that require energy are endothermic. |
Reactions that release energy are exothermic. |
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Properties of Acids & Bases
Acids |
Bases |
pH between 0-7 |
pH between 7-14 |
Taste sour |
Taste bitter |
Neutralizes bases |
Neutralizes acids |
Reacts with metals to
form hydrogen gas |
pH Scale
pH 0 - 6 |
Acid |
pH 7 |
Neutral |
pH 8-14 |
Alkaline (Basic) |
Indicators
Name |
Colour in Acid |
Colour at neutral |
Colour in Base |
Universal Indicator (UI) |
Red |
Green |
Blue |
Blue Litmus Paper |
Red |
Purple |
Blue |
General Word Equations
Acid-Base: |
Acid + Base → Salt + water |
Acid-Metal: |
Acid + Metal → Salt + Hydrogen gas |
Acid-Carbonate: |
Acid + Carbonate → salt + water + carbon dioxide |
Combustion: |
Fuel + Oxygen → Carbon dioxide + water |
Corrosion: |
Oxygen + iron + water → iron oxide (rust) |
General Formula for Acid-Base Reactions
Acid + Base Reactions
Hydroxide ions (OH-) from the base, attach to hydroxide (H+) ions from the acid, producing water. |
The remaining atoms form a salt. |
| |
Identification: |
Neutralisation reaction using universal indicator to indicate pH of 7 |
Naming Salts
The first part of the name comes from the base, the second from the acid. |
| |
Sodium hydroxide |
+ |
Hydrochloric acid |
→ |
Sodium chloride |
Magnesium oxide |
+ |
Nitric acid |
→ |
Magnesium Nitrate |
Sodium hydroxide |
+ |
Sulfuric acid |
→ |
Sodium sulfate |
Acid-Carbonate Reactions
Acids react with metal carbonates to form a salt, water and carbon dioxide. |
| |
Identification: Limewater Test |
Limewater can be used to indicate CO2 production turning milky white when the gas is present. |
Acid + Carbonate General Equation
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