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Year 10 Revision Booklet Chemistry Easter Holidays Revision Instructions: Use the Knowledge Organizer to Help You Answer the Questions on the Revision Sheets

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Year 10 Revision Booklet Chemistry Easter Holidays Revision Instructions: Use the Knowledge Organizer to Help You Answer the Questions on the Revision Sheets Year 10 Revision booklet Chemistry Easter holidays Revision Instructions: Use the knowledge organizer to help you answer the questions on the revision sheets. Atomic Structure Periodic Table Atoms are the basic building Periods in the periodic table. In each period (horizontal blocks of ordinary matter. row), the atomic numbers increase from left to right. Atoms can join together to The periods are numbered 1 through 7 on the left-hand form molecules, which in side of the table. Elements that are in the same period turn form most of the objects have chemical properties that are not all that similar. around you. Atoms are composed of particles called protons, electrons and neutrons. Mixtures, Elements & Compounds Discovery of the nucleus An element is a substance made from only one type of atom. For example. Carbon is made In 1909 Ernest Rutherford designed an experiment to test the plum entirely from carbon atoms. pudding model. In the experiment, positively charged alpha particles were fired at thin gold foil. Most alpha particles went straight through the foil. But a few were scattered in different directions. Group 0 Elements A compound is a molecule made of atoms from This evidence led Rutherford to suggest a new model for the atom, called different elements. All compounds are the nuclear model. In the nuclear model: The group 0 elements, the noble gases, are all molecules, but not all molecules are • the mass of an atom is concentrated at its centre, the nucleus unreactive non-metal gases. They show trends in their compounds. Hydrogen gas (H2) is a molecule, • the nucleus is positively charged physical properties. Their uses depend on their but not a compound because it is made of only inertness, low density and non-flammability. one element. Atomic Structure Group 1 Elements A mixture contains two or more substances. Electrons in shells. Electrons in atoms that have not reacted chemically with each occupy energy levels, also called The Group 1 elements in the periodic table are known as the alkali other. A mixture is made of little bits of each electron shells, outside the nucleus . substance mixed together. A mixture can be metals. They include lithium, sodium and potassium, which all react Different shells can hold different vigorously with water to produce an alkaline solution. separated by physical methods, a compound maximum numbers of electrons. The can not. electrons in an atom occupy the lowest Plumb Pudding Model available energy level first Group 7 Elements The Plum Pudding Model is a The Group 7 elements are called the halogens. They are placed in the model of atomic structure Mendeleev vertical column, second from the right, in the periodic table . proposed by J.J. Thomson in the Chlorine, bromine and iodine are the three common Group 7 late 19th century. Thomson had Mendeleev left gaps in his table for elements not known at the elements. Group 7 elements form salts when they react with metals. discovered that atoms are time. By looking at the properties of the elements next to a gap, composite objects, made of pieces he could also predict the properties of these undiscovered elements. For example, Mendeleev predicted the existence of with positive and negative charge, Properties of Metals and that the negatively charged 'eka-silicon', which would fit into a gap below silicon. Another electrons within the atom were scientist later discovered the missing element, germanium. Its very small compared to the entire properties were found to be similar to the predicted ones and atom. confirmed Mendeleev's periodic table. Atomic Theory Niels Bohr adapted Ernest Rutherford's nuclear model. Bohr did calculations that led him to suggest that electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus. Further experiments led to the idea that the nucleus contained small particles, called protons. James Chadwick found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutrons. This led to another development of the atomic model, which is still used today. Write the word equation for: Explain crystallisation as a separation Burning magnesium in air technique C1 Atomic Structure and the Periodic Table Can you write the balanced symbol AQA Trilogy equation? Define the following terms: Balance the symbol equations below: Draw a diagram to illustrate chromatography Atom as a separation technique H2SO4 + NaOH Na2SO4 + H2O Element Zn + O ZnO Number of protons = Compound 2 Number of neutrons = Mixture CH4 + O2 CO2 + H2O Number of electrons = Write the symbols for the following Simple distillation Explain simple distillation as a separation Describe the difference between the elements: technique, shown in the diagram plum pudding and the nuclear model of Oxygen an atom Carbon Sodium Magnesium Chlorine Copper Write the name of the compound: fractional distillation Explain fractional distillation as a separation Where in an atom are the neutrons and technique CO2 proton? The number of protons = the number H2O of_________ Atomic number is the number of NaCl _________ Mass number is the number of CuSO4 ________ + the number of _________ Isotopes have a different number of ____________ In the periodic table, the elements are When developing the periodic table, Properties of metals arranged in order of their ___________ Why did Medeleev leave gaps? • number C1 Atomic Structure • Elements in the same group, have the and the Periodic Table same number of ______________ • AQA Trilogy Groups go ____________ • Approximately how may elements are in Periods go ___________ the periodic table? • Draw the electron structure for sodium What is group 1 also known as? Delete as appropriate: Properties of non-metals • As you go down group 1, what If you remove electrons from an atom is happens to the reactivity? becomes positive/ negative • If you add electrons to an atom it • How many electrons are in the becomes positive/negative outer shell of a group 1 metal? • • Draw the electron structure for chlorine What is group 7 also known as? What is an isotope? To work out the relative atomic mass using the abundance of isotopes we can As you go down group 7, what use the following calculation: happens to the reactivity? What happens to melting point and (% of isotope 1 × mass of isotope 1) boiling point as you go down the group? + (% of isotope 2 × mass of isotope 2) How many electrons are in the ÷ 100 outer shell of a group 7 element? Draw the electron structure for chlorine What is group 0 also know as? Copper has two stable isotopes Cu-63 which In any sample of Chlorine 25% will has an abundance of 69.2% and Cu-65 which be 37Cl and 75% 35Cl. Calculate the In group 0, how many electrons has an abundance of 30.8% relative atomic mass to 1dp. are in the outer shell? Calculate relative atomic mass to 1dp. How is boiling point affected as you go down the group? Ionic Bonding Diamond Graphite In diamond, each carbon atom Positive and negative ions form when a metal reacts with a In graphite, each carbon atom forms three forms four covalent bonds covalent bonds with three other carbon atoms, non-metal, by transferring electrons. The oppositely with other carbon atoms in a charged ions are strongly attracted to each other, forming forming layers of hexagonal rings which have giant covalent structure, so ionic no covalent bonds between the layers. In diamond is very hard, has a graphite, one electron from each carbon atom A dot and cross diagram models the transfer of electrons very high melting point and is delocalised. from metal atoms to non-metal atoms. The electrons from does not conduct electricity. one atom are shown as dots, and the electrons from the Diamond is a giant covalent Graphite is a giant covalent substance in other atom are shown as crosses. substance in which: which: Giant Ionic Compounds • each carbon atom is • each carbon atom is joined to three joined to four other other carbon atoms by covalent bonds carbon atoms by An ionic compound is a giant structure of ions. The ions have a • the carbon atoms form a hexagonal covalent bonds regular, repeating arrangement called an ionic lattice. The lattice is layered network structure • the carbon atoms form formed because the ions attract each other and form a regular • the layers have weak forces between a regular tetrahedral pattern with oppositely charged ions next to each other. them and can slide over each other network structure The ions in an ionic compound held together in a giant ionic lattice. • each carbon atom has one un-bonded • there are no free Ionic compounds have high melting points and boiling points. Ionic outer electron electrons compounds form crystals (which can be cleaved along certain • these un-bonded electrons are planes). Ionic compounds do not conduct electricity when solid. delocalised, and are free to move Fullerene Covalent Bonding Fullerenes are molecules of carbon atoms with hollow shapes. The structure of fullerenes is based on hexagonal rings of carbon atoms but they may also contain A covalent bond is formed when two atoms share a pair of rings with five or seven carbon atoms. The first fullerene to be discovered was electrons. Covalent bonding occurs in most non-metal Buckminsterfullerene (C60) which has a spherical shape. elements, and in compounds formed between non-metals These shared electrons are found in the outer shells of the atoms. Usually each atom contributes one electron to the Metallic Bonding shared pair of electrons. Metals consist of giant structures of atoms arranged in a regular pattern. The electrons from the outer shells of the metal atoms are delocalised, and are Simple Covalent Molecules free to move through the whole structure.
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