Part 6- Chemistry Paper 1 Bonding Application Questions Triple Science How bonding and structure are related to the properties of substances A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes Chemical bonds, ionic, covalent and metallic Bonding Structure, and the Properties of Matter Use of amount of substance in relation to masses of pure substances Quantitative Chemistry Yield and atom economy of chemical reactions (Triple) Using concentrations of solutions in mol/dm3 (Triple) Chemical measurements, conservation of mass and the quantitative interpretation The periodic table Atomic Structure and the Periodic Table Paper 1 Chemical Changes Reactions of acids Reactivity of metals Reversible reactions and dynamic equilibrium The Rate and Extent of Chemical Change Chemistry Paper 2 Energy Changes Chemical cells and fuel cells (Triple) Exothermic and endothermic reactions Electrolysis Rate of reaction Reactions of alkenes and alcohols (Triple) Carbon compounds as fuels and feedstock Organic Chemistry Synthetic and naturally occurring polymers (Triple) Purity, formulations and chromatograph & 4.8.2 ID of gases Chemical Analysis Identification of ions by chemical and spectroscopic means (Triple) Chemistry of the Atmosphere Common atmospheric pollutants and their sources The composition and evolution of the Earth's atmosphere Carbon dioxide and methane as greenhouse gases Using Resources Life cycle assessment and recycling Using materials (Triple) Using the Earth's resources and obtaining potable water The Haber process and the use of NPK fertilisers (Triple)
AQA Chemistry (8462) from 2016 Topics C4.2 Bonding, structure, and the properties of matter Topic Student Checklist R A G Describe the three main types of bonds: ionic bonds, covalent bonds and metallic bonds in terms of electrostatic forces and the transfer or sharing of electrons Describe how the ions produced by elements in some groups have the electronic structure of a noble gas and explain how the charge of an ion relates to its group number Describe the structure of ionic compounds, including the electrostatic forces of attraction, and represent ionic compounds using dot and cross diagrams Describe the limitations of using dot and cross, ball and stick, two and three-dimensional diagrams to represent a giant ionic structure Work out the empirical formula of an ionic compound from a given model or diagram that shows the ions in the structure Describe covalent bonds and identify different types of covalently bonded substances, such as small molecules, large molecules and substances with giant covalent structures Represent covalent bonds between small molecules, repeating units of polymers and parts of giant covalent structures using diagrams Draw dot and cross diagrams for the molecules of hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia and methane Deduce the molecular formula of a substance from a given model or diagram in these forms showing the atoms and bonds in the molecule Describe the arrangement of atoms and electrons in metallic bonds and draw diagrams the bonding in metals Name the three States of matter, identify them from a simple model and state which changes of state happen at melting and boiling points Explain changes of state using particle theory and describe factors that affect the melting and boiling point of a substance HT ONLY: Discuss the limitations of particle theory Recall what (s), (l), (g) and (aq) mean when used in chemical equations and be able to use them appropriately Explain how the structure of ionic compounds affects their properties, including melting and boiling points and conduction of electricity (sodium chloride structure only) Explain how the structure of small molecules affects their properties Explain how the structure of polymers affects their properties Explain how the structure of giant covalent structures affects their properties Explain how the structure of metals and alloys affects their properties, including explaining why they are good conductors Explain why alloys are harder than pure metals in terms of the layers of atoms Explain the properties of graphite, diamond and graphene in terms of their structure and bonding Describe the structure of fullerenes, and their uses, including Buckminsterfullerene and carbon nanotubes Chem ONLY: Compare the dimensions of nanoparticles to other particles and explain the effect of their surface area to volume ratio on their properties Chem ONLY: Discuss the applications of nanoparticles and their advantages and disadvantages, including uses in medicine, cosmetics, fabrics and the development of catalysts 4.2.1 Chemical bonds, ionic, covalent and metallic 4.2.2 How bonding and structure are related to the properties of substances
A. Changes of State States of matter 1. Explain why different substances have different melting points. (2). 2. Describe the general properties of solids, liquids and gases, including the arrangement and movement of particles. (4).. 3. Extended response question: Describe what happens to particles during changes of state as a gas is cooled down to a temperature below its freezing point. (6)..
4. Evaporation is the change of state that occurs when some liquid changes into a gas. Many factors can affect the rate of evaporation. Plan an investigation into one factor that might affect the rate of evaporation using wet cotton wool and a high resolution digital balance. (5)... B. Ionic Bonding part 1 Joining of atoms and Ionic compounds 1. Explain the charges on the following ions: a) Na + b) O 2-. 2. Sodium chloride NaCl and sodium oxide has ionic bonds. a) Draw dot and cross diagrams to show what happens to sodium and chlorine atoms when they react to form sodium chloride. You only need to show the outer electrons in your diagrams. (3)
b) Draw dot and cross diagrams to show what happens to sodium and oxygen atoms when they react to form sodium oxide. (3) 3. What is the chemical formula for: a) Calcium oxide (1) b) Magnesium fluoride (1) c) Aluminum oxide (1) C. Ionic Bonding part 2 Properties of ionic compounds 1. Explain why ionic compounds have high melting points and boiling points. (2). 2. Why can ionic compounds conduct electricity when they are molten or dissolved in water? (1). 3. Why is seawater a better conductor of electricity than freshwater? (1) D. Covalent Bonding part 1 Joining of atoms and small molecules 1. Draw a diagram to represent the covalent bonding between two chlorine atoms. (2)
2. The melting point of ammonia, NH3 is -78 C and its boiling point is 33 C. What state is ammonia at 20 C? (1) 3. Why don t simple molecular substances conduct electricity? (1) 4. Nitrogen gas has a very strong triple covalent bond holding the atoms together. Explain why nitrogen has a boiling point of -196 C. (2). 5. Describe what is meant by intermolecular forces. (1) E. Covalent Bonding part 2 Giant structures 1. Graphite is sometimes used to reduce the friction between two surfaces that rub together. Explain how it does this. (2). 2. Extended response question: Describe how the structures of diamond and graphite are similar and explain why graphite can conduct electricity, but diamond cannot. (6)..
3. State which properties of graphene make it useful in the manufacture of bullet-proof vests. (2). 4. Explain why Graphene is such a good conductor of electricity (5).. 5. Ethene C 2H 4 can be polymerised to Poly(ethene). a) Explain in terms of its structure why ethene is a gas at room temperature. (2). b) Explain in terms of its structure why poly(ethene) is a polymer. (2). a) Explain why poly(ethene) has a high melting point. (1)
F. Metallic Bonding part 1 Joining of atoms 1. This diagram shows a model of metallic bonding: a) Why are the particles that makeup a metal described as positively charged ions? (3).. b) What are delocalised electrons? (2). 2. Explain the bonding in a metal using the theory of metallic bonding (4).. G. Metallic Bonding part 2 Properties of metals and alloys 1. Copper can be hammered into shape. The structure of copper metal can be represented by the following diagram:
a) Explain why copper can be hammered into shape. (1) b) Copper can be mixed with zinc to make the alloy brass. Brass is much harder than copper. Explain why. (2). c) Extended response question: Copper is a good metal for making a kettle because it has a high melting point. Explain why copper has a high melting point. You should describe the structure and bonding of a metal in your answer. (6).. 2. Explain why magnesium sulfide has melting point of 2000 C, whereas sodium chloride has one of 801 C. (3).
H. Nanoparticles Chemistry only 1. How many nanometres make up 1 millimetre? (1) 2. What is a nanoparticle (1). 3. Explain why nanoparticles would make very efficient catalysts. (2). 4. Describe one social and one economic benefit of nanoscience. (2)....