Year 11 Triple Chemistry

A collection of vocabulary flashcards based on chemistry concepts from Year 11 lecture notes.

Ionic Bonding

Occurs between metals and non-metals where electrons are transferred, creating an electrostatic force of attraction between oppositely charged ions.

Covalent Bonding

Occurs between non-metals where electrons are shared in pairs.

Metallic Bonding

Occurs between metals, involving a regular arrangement of positive ions surrounded by a 'sea' of delocalised electrons.

High Melting and Boiling Points in Ionic Compounds

Due to strong forces between ions that require a lot of energy to break.

High Melting and Boiling Points in Giant Covalent Compounds

Due to strong bonds between atoms that require significant energy to break.

Low Melting and Boiling Points in Simple Covalent Molecules

Due to weak forces between molecules that do not need much energy to break.

Conductivity in Ionic Compounds

They only conduct electricity when molten or in solution because the ions are free to move.

Conductivity in Metallic Substances

They conduct electricity due to free electrons able to move throughout the structure.

Lack of Conductivity in Covalent Compounds

They do not conduct electricity because there are no free electrons.

MgO versus NaCl Melting Point

MgO has a higher melting point than NaCl because magnesium and oxide ions have greater charges, resulting in a stronger attraction.

Hardness of Diamond

Diamond is hard because each carbon atom is strongly bonded to four others through covalent bonds.

Softness of Graphite

Graphite is soft because each carbon is covalently bonded to three others in hexagonal layers, with weak forces allowing layers to slide over each other.

Electrical Conductivity of Graphite

Graphite can conduct electricity because the fourth electron of each carbon atom is free to move throughout its structure.

Fullerenes

Used for drug delivery, lubricants, and catalysts.

Nanometre

A unit of measurement equal to 1 billionth of a meter; a nanoparticle typically consists of 1-100 atoms.

Properties of Silver Nanoparticles

Antibacterial, antiviral, antifungal.

Uses of Silver Nanoparticles

Used in plasters, antiseptic sprays, socks, and deodorant sprays.

Properties of Titanium Dioxide Nanoparticles

Absorb and reflect UV light, transparent.

Uses of Titanium Dioxide Nanoparticles

Used in sunscreen and self-cleaning windows.

Risks of Nanoscience

Unknown long-term effects and potential for easy absorption into the body or environment.

Smart Material

Materials with properties that change reversibly in response to environmental changes.

Thermochromic Pigments

Change color with temperature.

Photochromic Pigments

Change color with changing light intensity.

Polymer Gels

Absorb water and swell or release water and shrink due to changes in pH or temperature.

Shape Memory Alloys and Polymers

Regain their original shape when heated.

Strong Acid with Universal Indicator

Appears red with a pH of 1-2.

Strong Alkali with Universal Indicator

Appears purple with a pH of 13-14.

Neutral Substance with Universal Indicator

Appears green with a pH of 7.

Ions in Acids

Contain H+ (Hydrogen ions).

Ions in Alkalis

Contain OH- (Hydroxide ions).

Acid and Metal Reaction Products

Produces a salt and hydrogen.

Acid and Carbonate Reaction Observation

Fizzy reaction due to carbon dioxide production.

Acid and Base Reaction Products

Produces a salt and water.

Neutralisation Ionic Equation

𝑯⁺ + 𝑶𝑯⁻ → 𝑯₂𝑶.

Sulfate Ion Test

Add barium chloride to observe a white precipitate.

Ore Definition

A mineral found in the Earth's crust that contains enough metal to make extraction worthwhile.

Native State Metals

Gold and silver are found in the ground in their native state.

Oxidation

Gaining oxygen.

Reduction

Losing oxygen.

Displacement Reaction

A chemical reaction where a more reactive element displaces a less reactive element from its compound.

Blast Furnace Raw Materials

Iron ore, coke, limestone, hot air.

Coke in Blast Furnace

Used as fuel and produces carbon monoxide for reduction.

Limestone in Blast Furnace

Removes impurities as slag.

Hot Air in Blast Furnace

Provides oxygen for coke combustion.

Electrolysis Definition

Splitting up of a compound using electricity.

Oxidation (Electrons)

Loss of electrons.

Reduction (Electrons)

Gain of electrons.

Positive Ions at Negative Electrode

Gain electrons and are reduced.

Negative Ions at Positive Electrode

Lose electrons and are oxidized.

Aluminium Ore and Cryolite

Dissolved in molten cryolite to save energy during electrolysis.

Oxygen in Electrolysis Reaction

Reacts with carbon electrodes to produce carbon dioxide.

Metals Properties

High melting points, malleable, ductile, good conductors of heat and electricity.

Transition Metals Location

Found between groups 2 and 3 on the periodic table.

Transition Metals Properties

Form more than one type of ion and form colored compounds.

Fe2+, Fe3+, Cu2+ Ion Solutions

Fe2+ - pale green; Fe3+ - brown; Cu2+ - blue.

Alloy Definition

A mixture made by mixing molten metals.

Metal Extraction Location Factors

Transport links, electricity supply, distance from nearby towns or cities.

Activation Energy Definition

The minimum amount of energy needed to start a reaction.

Exothermic Reaction

Releases energy to the surroundings, increasing temperature.

Endothermic Reaction

Absorbs energy from the surroundings, decreasing temperature.

Crude Oil Definition

A mixture of hydrocarbons.

Hydrocarbon Definition

A compound made of hydrogen and carbon only.

Crude Oil Separation Method

Fractional distillation: vaporizing then condensing at different points in a column.

Carbon Chain Length Effects

Longer chains lead to higher viscosity, darker color, and higher boiling points.

Combustion of Fuels Description

Burning in oxygen to produce carbon dioxide and water.

Hydrogen Fuel Advantages

Water is the only product, making it non-contributive to global warming; it is renewable.

Hydrogen Fuel Disadvantages

Requires a lot of energy to produce; storage requires bulky, heavy pressurized containers.

Fire Triangle Components

Fuel, oxygen, heat.

Cracking Definition

Heating hydrocarbons at high temperatures with a catalyst to break them down into smaller molecules.

Alkene General Formula

CₙH₂ₙ.

Salt Crystals Preparation Method

Add excess base to acid, filter out excess base, evaporate water to form crystals.

First Five Alkanes

Methane, ethane, propane, butane, pentane.

Alkenes Test Method

Add bromine water, which turns from orange-brown to colorless.

Monomer Definition

A small reactive molecule that can join together to form a polymer.

Polythene Uses

Used in bags and plastic bottles.

Poly(propene) Uses

Used in ropes and crates.

PVC Uses

Used in drain pipes and window frames.

PTFE Uses

Used in non-stick pans.

Environmental Issues with Plastics

Take up landfill space, do not biodegrade, made from non-renewable resource crude oil.

Moles Calculation Equation

Moles = Volume (dm³) x Concentration (mol/dm³).

Strong vs Weak Acid Comparison

Stronger acids have lower pH (1-2); weaker acids have higher pH (3-4).

Dilute vs Concentrated Acid Comparison

Concentrated acids contain less water than dilute acids.

Fe2+, Fe3+, Cu2+ Ion Identification

Fe2+ - green precipitate; Fe3+ - brown precipitate; Cu2+ - blue precipitate.

Ionic Equation for Fe2+ Reaction with OH-

Fe²⁺ + 2OH⁻ → Fe(OH)₂ (s).

Electrolysis of Water Products

Hydrogen and oxygen.

Electrolysis with Competing Ions

The least reactive ion will form at the electrode.

Electrolysis of Salt Water Products

Chlorine gas, hydrogen gas, and sodium hydroxide solution.

Other Electrolysis Uses

Electroplating and purification of copper.

Ethanol Production Method

Fermentation of sugar using an enzyme from yeast, with carbon dioxide as a waste product.

Alcohols Test Method

Use acidified potassium dichromate, with a color change from orange to green.

Ethanol Issues in Drinks

Associated with antisocial behavior and health issues like liver damage.

Other Ethanol Uses

Used as a solvent and fuel.

Bioethanol Advantages

Renewable and carbon neutral.

Ethanol Oxidation Products

Ethanoic acid is produced; the process is slow and can spoil beverages.

Infrared Spectroscopy Use

Identifies the presence of certain bonds in organic molecules.

Reversible Reaction Definition

A reaction that can proceed in either direction.

Haber Process Conditions and Raw Materials

Conditions: 350-450⁰C, 150-200 atmospheres pressure, with an iron catalyst; Raw materials: nitrogen from air and hydrogen from methane.

Ammonia Gas Test Method

Damp red litmus paper turns blue in ammonia presence.

Contact Process for Sulfuric Acid

1. Burn sulfur in air to make sulfur dioxide; 2. React with oxygen to make sulfur trioxide; 3. React with water to produce sulfuric acid.

Sulfuric Acid Uses

Used in fertilizers, paints, dyes, fibers, plastics, and detergents.