Part 5- Chemistry Paper 1 Atomic Structure Knowledge Questions 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 TRILOGY Chemistry (8464) from 2016 Topics T5.1 Atomic structure and the periodic table Topic Student Checklist R A G State that everything is made of atoms and recall what they are Describe what elements and compounds are State that elements and compounds are represented by symbols; and use chemical symbols and formulae to represent elements and compounds Write word equations and balanced symbol equations for chemical reactions, including using appropriate state symbols HT ONLY: Write balanced half equations and ionic equations Describe what a mixture is Name and describe the physical processes used to separate mixtures and suggest suitable separation techniques Describe how the atomic model has changed over time due to new experimental evidence, inc discovery of the atom and scattering experiments (inc the work of James Chadwick) Describe the difference between the plum pudding model of the atom and the nuclear model of the atom State the relative charge of protons, neutrons and electrons and describe the overall charge of an atom State the relative masses of protons, neutrons and electrons and describe the distribution of mass in an atom Calculate the number of protons, neutrons and electrons in an atom when given its atomic number and mass number Describe isotopes as atoms of the same element with different numbers of neutrons Define the term relative atomic mass and why it takes into account the abundance of isotopes of the element Calculate the relative atomic mass of an element given the percentage abundance of its isotopes Describe how electrons fill energy levels in atoms, and represent the electron structure of elements using diagrams and numbers 5.1.1 A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes 5.1.2 The periodic table Recall how the elements in the periodic table are arranged Describe how elements with similar properties are placed in the periodic table Explain why elements in the same group have similar properties and how to use the periodic table to predict the reactivity of elements Describe the early attempts to classify elements Explain the creation and attributes of Mendeleev's periodic table Identify metals and non-metals on the periodic table, compare and contrast their properties Explain how the atomic structure of metals and non-metals relates to their position in the periodic table Describe nobel gases (group 0) and explain their lack of reactivity Describe the properties of noble gases, including boiling points, predict trends down the group and describe how their properties depend on the outer shell of electrons Describe the reactivity and properties of group 1 alkali metals with reference to their electron arrangement and predict their reactions Describe the properties of group 7 halogens and how their properties relate to their electron arrangement, including trends in molecular mass, melting and boiling points and reactivity Describe the reactions of group 7 halogens with metals and non-metals
A. Atoms, Elements, Compounds and Mixtures part 1 Atoms, Elements, Compounds, Word and Symbol Equations 1. How many different types of atoms are there? 2. What does it mean if a compound ends in ide? 3. What does it mean if a compound ends in ate? 4. What does a chemical reaction involve? 5. Name the following substances: NaCl NaSO 4 6. Why is it useful to have symbols for atoms of different elements? 7. What is the difference between an element and a compound? 8. Why is it difficult to separate a compound? 9. Solid sodium reacts with water to form a sodium hydroxide (NaOH) solution and hydrogen gas. a) Write a word equation to represent this reaction. b) Give the balance symbol equation for the reaction.
B. Atoms, Elements, Compounds and Mixtures part 2 Separating Techniques 1. What is the difference between a compound and a mixture? 2. Describe the method used to collect the salt from a mixture of sand and salt. 3. What process is used to purify seawater to obtain usable water? 4. Describe how the following equipment is used to separate water and ethanol. 5. A mixture and six colours are tested using chromatography. The following chromatogram was produced:
a) What can you conclude about the mixture? b) Why do the inks separate? C. Atomic Model part 1 History of the Atom 1. What was the earliest model of the atom? 2. Which subatomic particle did JJ. Thomson discover? 3. Which early atomic model does the following diagram show: 4. Name Rutherford s experiment. 5. State two ways in which Rutherford changed Thomson s model of the atom. 6. How did Bohr adapt the nuclear model? 7. Explain why Bohr revised Rutherford s model of the atom.
D. Atomic Model part 2 Size and Mass of Atoms and Atomic Structure 1. Name three subatomic particles and their charges. 2. Complete the sentence All atoms of one type of element have the same number of 3. What does the atomic number tell us about an atom? 4. What does the mass number tell us about an atom? 5. How is an isotope different to an atom? 6. What is the electron configuration for sodium? 7. Why is the overall charge of an atom zero? 8. Draw the electron configuration for a chlorine atom. 9. Write the electron configuration for potassium. 10. How many electrons does potassium have on its highest energy level?
11. Calculate how many protons, electrons and neutrons there are in: a) A silver atom with atomic number 47 and mass number 108 b) 12. The atomic radius of a bromine atom is 9 x 10-11 m. a) Give its atomic radius in nanometres. b) Calculate the radius of the nucleus (in nm), given that it will be about 1/10,000 the radius of the atom. Give your answer in standard form. E. Periodic Table part 1 History of the Periodic Table 1. How are elements arranged in the periodic table? 2. What are the columns of the periodic table called? 3. What are the rows of a periodic table called? 4. What does the column an element is in tell you about the atoms? 5. What does the row an element is in tell you about the atoms?
6. Which side of the periodic table are the non-metals found? 7. How were elements classified before the discovery of subatomic particles? 8. What was the problem with early periodic tables? 9. How did Mendeleev overcome these problems? 10. Why is the order based on atomic masses not always correct? 11. What do we call elements that tend to form positive ions? F. Periodic Table part 2 Group 0, group 1 and group 7 1. What are the elements in Group 0 called? 2. What are the elements in Group 1 called? 3. What are the elements in Group 7 called? 4. What happens to the boiling point of elements in Group 0 as you go down the group? 5. Why are the elements in Group 0 so unreactive?
6. Why do all elements in Group 1 react in a similar way to each other? 7. What happens to the reactivity of the elements as you go down Group 1? 8. Write a word equation for the reaction between sodium and oxygen. 9. Why do all the elements in Group 7 react in a similar way to each other? 10. Halogens are diatomic. What does the word diatomic mean? 11. What happens to the reactivity as you go down Group 7? 12. What happens to the melting point and boiling point as you go down Group 7? 13. Write a word equation for the reaction between lithium and chlorine. 14. Write a balanced chemical equation for the reaction between lithium and chlorine gas.