2024 Exam! AQA Foundation Chemistry Paper 1

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The text outlines essential concepts and calculations in chemistry for foundation pupils following the AQA specification, including key equations, practical experiments, and the characteristics of various materials and reactions. Important topics include the principles of electrolysis, relative atomic mass calculations, the organization of the periodic table, and the physical properties of covalent structures, all critical for success in related examinations.

Insights

  • The Chemistry Paper 1 for foundation pupils studying the AQA specification includes various question types such as evaluate, compare, and explain, each requiring specific approaches to demonstrate understanding, highlighting the need for students to be well-prepared with clear reasoning and detailed scientific knowledge.
  • Important practical skills are emphasized, with required experiments like making salts and performing electrolysis accounting for 15% of the exam marks, indicating that hands-on experience is crucial for success in the course and students must be familiar with the procedures and underlying principles of these experiments.
  • The development of the atomic model illustrates the progression of scientific understanding, moving from the plum pudding model to the nuclear model through experiments like alpha particle scattering, which revealed that atoms have a dense nucleus and mostly empty space, fundamentally changing how we perceive atomic structure and influencing the organization of the periodic table.

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Recent questions

  • What is a covalent bond?

    A covalent bond is a type of chemical bond formed when two non-metal atoms share pairs of electrons. This sharing allows each atom to attain a stable electron configuration, similar to that of noble gases. Covalent bonds can vary in strength, with single bonds involving one shared pair of electrons, double bonds involving two pairs, and triple bonds involving three pairs. The resulting molecules can exhibit different properties based on the number of shared electrons and the types of atoms involved. For example, in a molecule of oxygen (O2), each oxygen atom shares two pairs of electrons, resulting in a strong double bond. Covalent bonding is fundamental in the formation of many organic compounds and is characterized by strong intramolecular forces, although the intermolecular forces between covalent molecules are generally weaker.

  • How do you calculate relative atomic mass?

    Relative atomic mass is calculated by taking into account the different isotopes of an element and their respective abundances. To find the relative atomic mass, you multiply the mass of each isotope by its natural abundance (expressed as a fraction), then sum these values. For instance, chlorine has two stable isotopes: chlorine-35, which makes up about 75% of natural chlorine, and chlorine-37, which accounts for about 25%. The calculation would be: (0.75 x 35) + (0.25 x 37) = 26.25 + 9.25 = 35.5. This average gives the relative atomic mass of chlorine as 35.5. This concept is crucial in chemistry as it helps in understanding the mass relationships in chemical reactions and the behavior of elements in the periodic table.

  • What is the conservation of mass?

    The conservation of mass is a fundamental principle in chemistry stating that the total mass of reactants in a chemical reaction must equal the total mass of products. This means that matter cannot be created or destroyed in an isolated system. For example, if 73 grams of hydrochloric acid react with 100 grams of calcium carbonate, the total mass of the reactants is 173 grams. If the reaction produces water and other products, the combined mass of these products must also equal 173 grams. This principle is essential for balancing chemical equations, as it ensures that the number of atoms of each element remains constant throughout the reaction. Understanding the conservation of mass is crucial for accurately predicting the outcomes of chemical reactions and for conducting quantitative analyses in chemistry.

  • What are giant covalent structures?

    Giant covalent structures are large networks of atoms bonded together by strong covalent bonds, resulting in materials with high melting and boiling points. These structures do not consist of individual molecules but rather a continuous lattice of atoms. Examples include diamond, graphite, and silicon dioxide. In diamond, each carbon atom is tetrahedrally bonded to four other carbon atoms, creating a very hard material. Graphite, on the other hand, consists of layers of carbon atoms arranged in hexagonal patterns, with weak forces between the layers allowing them to slide over one another, making graphite useful as a lubricant. Silicon dioxide, commonly found in sand, forms a three-dimensional network that gives it high stability and strength. The properties of giant covalent structures make them significant in various applications, from industrial materials to electronics.

  • What is an endothermic reaction?

    An endothermic reaction is a type of chemical reaction that absorbs heat from its surroundings, resulting in a decrease in temperature of the environment. During an endothermic reaction, the energy required to break the bonds of the reactants is greater than the energy released when new bonds are formed in the products. A common example of an endothermic reaction is the process of photosynthesis, where plants absorb sunlight to convert carbon dioxide and water into glucose and oxygen. In a laboratory setting, endothermic reactions can be observed using a thermometer; as the reaction occurs, the thermometer reading will drop, indicating that heat is being absorbed. Understanding endothermic reactions is important in various fields, including chemistry, biology, and environmental science, as they play a crucial role in energy transfer and transformation processes.

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Summary

00:00

AQA Chemistry Paper 1 Study Guide

  • Chemistry Paper 1 for foundation pupils studying the AQA specification includes evaluate questions requiring advantages, disadvantages, and a justified conclusion; compare questions need similarities and differences, while explain questions demand scientific detail on the reasoning behind answers.
  • Important equations to remember include concentration = mass/volume, conversion of cubic centimeters to cubic decimeters by dividing by 1,000, and uncertainty = range/2; these should be written down immediately at the start of the exam.
  • Required practicals for Combined Science include making salts, endothermic and exothermic reactions, and electrolysis, which collectively account for 15% of the exam marks.
  • To make copper chloride, use hydrochloric acid and copper oxide; add the solid in excess to ensure complete reaction, then filter using a conical flask, funnel, and filter paper to obtain the copper chloride solution.
  • Heat the copper chloride solution over a Bunsen burner in an evaporating dish until some water evaporates, then allow it to cool slowly to form crystals, ensuring not to evaporate all the water.
  • In endothermic reactions, the thermometer reading decreases as heat is absorbed from the surroundings, while in exothermic reactions, the reading increases due to heat being released; use a polystyrene cup and insulation to minimize heat transfer during experiments.
  • Electrolysis involves using electricity to split ionic compounds; for example, lead bromide is melted to free lead and bromide ions, which are attracted to electrodes, resulting in lead deposition and bromine gas release.
  • When performing electrolysis on sodium chloride solution, the chloride ion (from group 7) goes to the positive electrode, producing chlorine gas, while hydrogen ions (least reactive) go to the negative electrode, producing hydrogen gas.
  • Calculating relative atomic mass involves averaging isotopes based on their abundance; for chlorine with 75% chlorine-35 and 25% chlorine-37, the calculation yields a relative atomic mass of 35.5.
  • Relative formula mass is determined by counting the number of atoms in a compound and multiplying by their respective atomic masses; for example, the formula mass of calcium carbonate (CaCO3) is calculated as 40 (Ca) + 12 (C) + 48 (O) = 100, with no units since it is a relative mass.

17:39

Chemical Calculations and Atomic Models Explained

  • The total relative formula mass of magnesium nitrate is calculated as 148, derived from adding two lots of nitrogen (14 x 2 = 28) and three lots of oxygen (16 x 3 = 48) to the mass of magnesium (24).
  • To find the percentage by mass of nitrogen in magnesium nitrate, divide the mass of nitrogen (28) by the total mass (148) and multiply by 100, resulting in 18.9%.
  • For calculating the percentage by mass of carbon in calcium carbonate, use the mass of carbon (12) divided by the total mass (100) multiplied by 100, yielding 12%.
  • The key equation for concentration is concentration = mass (in grams) / volume (in decimeters cubed), with concentration measured in grams per decimeter cubed.
  • If mass is given in kilograms, convert it to grams by multiplying by 1,000; if volume is in centimeters cubed, convert it to decimeters cubed by dividing by 1,000.
  • For a sodium chloride solution made from 2 grams of sodium chloride in 200 cm³ of water, convert the volume to decimeters cubed (200 cm³ = 0.2 dm³) and calculate concentration as 2 g / 0.2 dm³ = 10 g/dm³.
  • When balancing chemical equations, count the number of atoms on each side and adjust coefficients in front of compounds to ensure the same number of each type of atom is present on both sides.
  • The development of the atomic model progressed from the plum pudding model to the nuclear model, which was established through the alpha particle scattering experiment, revealing that atoms consist mostly of empty space with a small, dense, positively charged nucleus.
  • Mendeleev's periodic table was organized by atomic mass and included gaps for undiscovered elements, while the modern periodic table is organized by atomic number, grouping elements with similar properties together.
  • Reactivity trends in the periodic table show that group one (alkaline metals) becomes more reactive down the group due to increased distance between the nucleus and outer electron, while group seven (halogens) becomes less reactive down the group as the distance makes it harder to gain an electron.

35:04

Chemical Bonds and Structures Explained

  • The formula for a reaction involving chlorine requires one magnesium (Mg) and two chlorine (Cl) atoms, indicating the need to assess the number of electrons each element can donate or require for covalent bonding.
  • Covalent bonds form between non-metals through the sharing of electrons, resulting in strong bonds and weak intermolecular forces; for example, in O2, each oxygen atom shares two pairs of electrons, leading to a double bond.
  • Small molecules, such as O2, exhibit low melting and boiling points due to weak intermolecular forces, which require minimal energy to overcome, unlike the strong covalent bonds that hold the atoms together.
  • Giant covalent structures, including diamond, graphite, and silicon dioxide, consist of strong covalent bonds and have high melting and boiling points; diamond features carbon atoms bonded in a tetrahedral structure, while graphite has layers that can slide due to weak forces between them.
  • Fullerenes, such as Buckminsterfullerene (C60), are spherical structures made of hexagons and pentagons, providing a large surface area for applications like catalysis and drug delivery, and can also act as lubricants due to their spherical shape.
  • Nanotubes, formed by rolling a single layer of graphite (graphene) into a tube, are lightweight, strong, and capable of conducting electricity due to delocalized electrons, making them useful in various applications.
  • Polymers are long chains of molecules connected by covalent bonds, typically represented by a small section in diagrams, and their properties depend on the arrangement and types of monomers used.
  • Pure metals have a regular arrangement of atoms that allows layers to slide easily, making them soft, while alloys, which consist of different-sized atoms, distort this arrangement, resulting in harder materials that resist deformation.
  • The conservation of mass principle states that the total mass of reactants must equal the total mass of products in a chemical reaction; for example, in a reaction involving 73 grams of hydrochloric acid and 100 grams of calcium carbonate, the mass of water produced can be calculated as 18 grams by ensuring the mass balance is maintained.
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