Year 11 Triple Chemistry Review

A comprehensive set of vocabulary flashcards covering key concepts in Year 11 Triple Chemistry.

Ionic Bonding

Occurs between metals and non-metals where electrons are transferred, resulting in 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.

Melting and Boiling Points of Ionic Compounds

Ionic compounds have high melting and boiling points due to strong forces between ions that require a lot of energy to break.

Reasons for High Melting Points in Giant Covalent Compounds

Giant covalent compounds have strong bonds between atoms that require a lot of energy to break.

Melting and Boiling Points of Simple Covalent Molecules

Simple covalent molecules have low melting and boiling points due to weak forces between molecules that don’t require much energy to break.

Electrical Conductivity of Ionic Compounds

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

Electrical Conductivity of Metallic Substances

Metallic substances conduct electricity because they have free electrons that can move throughout the structure.

Covalent Compounds and Electrical Conductivity

Covalent compounds do not conduct electricity because there are no free electrons.

Why MgO has a Higher Melting Point than NaCl

MgO has greater charges (2+ and 2-) leading to a stronger attraction compared to NaCl.

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 between layers.

Graphite's Ability to Conduct Electricity

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

Fullerenes Uses

Fullerenes can be used for drug delivery, lubricants, and catalysts.

Nanometre

A unit of measurement equal to one billionth of a meter (1 nm); a nanoparticle consists of 1-100 atoms.

Properties of Silver Nanoparticles

Silver nanoparticles have antibacterial, antiviral, and antifungal properties.

Uses of Silver Nanoparticles

Silver nanoparticles are used in plasters, antiseptic sprays, socks, and deodorant sprays.

Properties of Titanium Dioxide Nanoparticles

Titanium dioxide nanoparticles absorb and reflect UV light and are transparent.

Uses of Titanium Dioxide Nanoparticles

Titanium dioxide nanoparticles are used in sunscreen and self-cleaning windows.

Smart Materials

Materials that have properties that change reversibly when a change occurs in their environment.

Thermochromic Pigments

Pigments that change color with temperature.

Photochromic Pigments

Pigments that change color with changing light intensity.

Polymer Gels

Gels that absorb water and swell or release water and shrink due to changes in pH or temperature.

Shape Memory Alloys and Polymers

Materials that regain their original shape when heated.

pH of Strong Acid with Universal Indicator

A strong acid appears red with a pH of 1-2.

pH of Strong Alkali with Universal Indicator

A strong alkali appears purple with a pH of 13-14.

pH of Neutral Substance with Universal Indicator

A neutral substance appears green with a pH of 7.

Ions in Acids and Alkalis

Acids contain H+ ions (hydrogen ions) and alkalis contain OH- ions (hydroxide ions).

Products of Acid Reaction with Metal

When an acid reacts with a metal, it produces a salt and hydrogen.

Observation of Acid Reaction with Carbonate

Fizzy reaction occurs due to the production of carbon dioxide.

Neutralisation Products

When an acid reacts with a base, a salt and water are produced.

Ionic Equation for Neutralisation

The ionic equation for neutralisation involves H+ and OH- ions forming H2O.

Testing for Sulfate Ions

To identify sulfate ions, add barium chloride, and a white precipitate should appear.

Ore Definition

An ore is a mineral found in the Earth's crust that contains enough metal to make it worthwhile extracting.

Native State Metals

Gold and silver are two metals that can be found in the ground in their native state.

Oxidation and Reduction in Terms of Oxygen

Oxidation is gaining oxygen, and reduction is losing oxygen.

Displacement Reaction Definition

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

Raw Materials of Blast Furnace

The four raw materials added to the blast furnace are iron ore, coke, limestone, and hot air.

Function of Coke in Blast Furnace

Coke is used as fuel and produces carbon monoxide for reduction.

Limestone's Role in Blast Furnace

Limestone is added to remove impurities as slag.

Purpose of Hot Air in Blast Furnace

Hot air provides oxygen so that the coke can burn.

Electrolysis Definition

The process of splitting up a compound using electricity.

Oxidation and Reduction in Terms of Electrons

Oxidation is the loss of electrons, and reduction is the gain of electrons.

Positive Ions at the Negative Electrode

When positive ions move to the negative electrode, they gain electrons and are reduced.

Negative Ions at the Positive Electrode

When negative ions move to the positive electrode, they lose electrons and are oxidised.

Aluminium Ore and Cryolite

Aluminium ore is dissolved in molten cryolite to lower the energy needed for electrolysis.

Oxygen Production During Electrolysis of Aluminium Oxide

Oxygen produced reacts with carbon electrodes to form carbon dioxide.

Five Properties of Metals

Metals typically have high melting points, are malleable, ductile, and are good conductors of heat and electricity.

Location of Transition Metals on Periodic Table

Transition metals are located between groups 2 and 3 on the periodic table.

Distinct Properties of Transition Metals

Transition metals can form more than one type of ion and produce colored compounds.

Solution Colors of Fe2+, Fe3+, and Cu2+ Ions

Fe2+ is pale green, Fe3+ is brown, and Cu2+ is blue.

Definition of Alloy

An alloy is a mixture made by mixing molten metals.

Factors Influencing Metal Extraction Plant Locations

Transport links, electricity supply, and proximity to towns or cities influence plant locations.

Activation Energy Definition

The minimum amount of energy needed to start a chemical reaction.

Exothermic Reaction Description

Exothermic reactions release energy to the surroundings, increasing temperature.

Endothermic Reaction Description

Endothermic reactions absorb energy from the surroundings, decreasing temperature.

Crude Oil Definition

Crude oil is a mixture of hydrocarbons.

Hydrocarbon Definition

A hydrocarbon is a compound made of hydrogen and carbon only.

Separation of Crude Oil

Crude oil is separated by fractional distillation, where it is vaporized and condensed at different points in a column.

Effect of Carbon Chain Length on Viscosity and Color

Longer carbon chains result in more viscous compounds and darker colors.

Effect of Carbon Chain Length on Boiling Point

Longer carbon chains have higher boiling points due to stronger forces between molecules.

Effect of Carbon Chain Length on Ignition

Shorter carbon chains are easier to ignite.

Fuels Combustion Description

The combustion of fuels involves burning in oxygen to produce carbon dioxide and water.

Advantages of Hydrogen as Fuel

Water is the only product of combustion, making it non-contributory to global warming and renewable.

Disadvantages of Hydrogen as Fuel

Producing hydrogen requires a lot of energy, and storage needs bulky pressurized containers.

Fire Triangle Components

The three components that make up the fire triangle are fuel, oxygen, and heat.

Cracking Process

Cracking is the heating of hydrocarbons at high temperatures with a catalyst to break them into smaller molecules.

General Formula for Alkenes

The general formula for alkenes is CnH2n.

Preparing Crystals of Salt

To prepare crystals of salt, add excess base to use up all the acid, filter to remove excess base, and evaporate water.

First Five Alkanes

The first five alkanes are methane, ethane, propane, butane, and pentane.

Testing for Alkenes

To test for alkenes, add bromine water, which will change from orange-brown to colorless.

Monomer Definition

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

Uses of Polythene and Poly(propene)

Polythene is used for bags and plastic bottles, while poly(propene) is used for ropes and crates.

Uses of PVC and PTFE

PVC is used for drain pipes and window frames, while PTFE is used for non-stick pans.

Environmental Issues with Plastics

Plastics take up space in landfills, do not biodegrade, and are made from crude oil, which is a non-renewable resource.

Equation for Calculating Moles in a Solution

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

Difference Between Strong and Weak Acids

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

Difference Between Dilute and Concentrated Acids

Concentrated acids contain less water, while dilute acids contain more water.

Identifying Iron Ions with Sodium Hydroxide

Fe2+ produces a green precipitate, Fe3+ produces a brown precipitate, and Cu2+ produces a blue precipitate with sodium hydroxide.

Products of Electrolysis of Water

The products of electrolysis of water are hydrogen and oxygen.

Competing Ions During Electrolysis

If there are more than one positive and negative ion, the least reactive ion will form at the electrode.

Products of Electrolysis of Salt Water

The products of electrolysis of salt water are chlorine gas, hydrogen gas, and sodium hydroxide solution.

Other Uses of Electrolysis

Electrolysis is used for electroplating and purification of copper.

Production of Ethanol from Sugar

Ethanol is made by fermenting sugar using an enzyme from yeast, with carbon dioxide as a waste product.

Testing for Alcohols

Alcohols can be tested using acidified potassium dichromate; a color change from orange to green indicates the presence of alcohol.

Issues with Ethanol in Drinks

The use of ethanol in alcoholic drinks can lead to anti-social behavior and health issues like liver damage.

Other Uses of Ethanol

Ethanol can also be used as a solvent and a fuel.

Benefits of Bioethanol as Fuel

Bioethanol is renewable and carbon neutral.

Oxidation of Ethanol

During the oxidation of ethanol, ethanoic acid is formed, which leads to beer and wine going 'off.'