Chemistry Flashcards

Flashcards from lecture notes

Ionic Compound

Metal + Non-metal. Give / Take electrons.

Cation

positively charged ion (loses electron)

Anion

negatively charged ion (gains electron).

Covalent Compound

Non - metal + Non-metal. Share elections.

Ion

Atoms of the same element with a different number of protons and neutrons.

Isotopes

Atoms of the same element with a different number of neutrons.

Electron Shell

The area around the nucleus where electrons are found. Can be calculated using the formula: 2n²

Hydrogen

Gas that explodes when ignited in a 'Pop Test'.

Oxygen

Gas that is essential for combustion and identified using a Glowing Splint Test.

Carbon Dioxide

Gas that reacts with limewater to turn it milky, identified using a Limewater Test.

Water

Turns dry blue cobalt copper paper pink, identified using Cobalt copper Paper Test.

Ammonium

Polyatomic ion with the formula NH₄⁺

Acetate

Polyatomic ion with the formula C₂H₃O₂⁻

Carbonate

Polyatomic ion with the formula CO₃²⁻

Hydroxide

Polyatomic ion with the formula OH⁻

Nitrate

Polyatomic ion with the formula NO₃⁻

Hydrogen Carbonate

Polyatomic ion with the formula HCO₃⁻

Phosphate

Polyatomic ion with the formula PO₄³⁻

Phosphite

Polyatomic ion with the formula PO₃³⁻

Sulfate

Polyatomic ion with the formula SO₄²⁻

Sulfite

Polyatomic ion with the formula SO₃²⁻

Nitrite

Polyatomic ion with the formula NO₂⁻

Acetic acid

Common acid with the formula CH₃COOH

Carbonic acid

Common acid with the formula H₂CO₃

Hydrochloric acid

Common acid with the formula HCl

Nitric acid

Common acid with the formula HNO₃

Sulfuric acid

Common acid with the formula H₂SO₄

Sodium Hydroxide

Common base with the formula NaOH

Potassium Hydroxide

Common base with the formula KOH

Calcium Hydroxide

Common base with the formula Ca(OH)₂

Ammonium Hydroxide

Common base with the formula NH₄OH

Neutralisation

Acid + base → salt + water

Decomposition

Chemical reaction where: AX → A + X

Combination

Chemical reaction where: A + X → AX

Combustion

Fuel + Oxygen → carbon dioxide + water

Corrosion

Iron + oxygen → Iron oxide (rust).

Combustion

A chemical reaction between a fuel and an oxidant, typically oxygen, that produces heat and sometimes light or a flame (exothermic).

Corrosion

Gradual destruction of a metal due to reactions with other chemicals in its environment.

Rusting

iron + oxygen +water —> hydrated iron oxide

Exothermic

Giving out energy in the form of light/heat. Chemical bonds are formed.

Endothermic

Taking in energy in the form of light/heat. Chemical bonds are broken.

Soluble

All compounds of Group 1 metal ions/ammonium ion and All nitrates.

Insoluble

All carbonates (ammonium, Group 1 metal ions) and All hydroxides (ammonium, calcium, barium, Group 1 metal ions).

Evidence of Chemical Reaction

Temperature change, Precipitate, Change in odour, Emission of gas, Emission of light.

Acid and Metal Reaction

Acid + metal → salt + hydrogen.

Acid and Carbonate Reaction

Acid + carbonate → Salt + carbon dioxide + water.

Endothermic

When heat is taken in as chemical bonds are broken; temperature decreases.

Exothermic

Heat is produced as chemical bonds are formed; temperature increases.

Factors affect Reaction Rate

Concentration, Temperature, Agitation, Pressure, Catalyst.

Independant Variable

The one being changed

Dependant Variable

The one being changed

Controlled Variable

The ones that remain the same/constant

Validity

A scientific investigation that fairly tests the hypothesis

• Variables are kept constant

Reliability

How repeatable the results are

• Reptition of tests for consistent results

Accuracy

How close the value calculated from the experiment is to the known value

• Appropriate Units and Measurements Techniques

Groups

Number of electrons in valence shell

Periods

Number of electron shells

Solute

The substance being dissolved

Solvent

The one being dissolved

All compounds of Group metal 1 ions

Soluble

All nitrates are

soluble

All chlorides

soluble except (silver, lead, mercury)

All bromides

soluble except (silver, lead, mercury)

All iodides

soluble except (silver, lead, mercury)

All sulfates

soluble except barium, calcium, and lead

All carbonates are

insoluble except ammonium, Group 1 metal ions

All hydroxides are

insoluble except ammonium, calcium, barium, Group 1 metal ions