Ionic compounds and analysis. C2 Topic 2
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1 Ionic compounds and analysis C2 Topic 2
2 Why do atoms form bonds? Atoms of different elements can combine to form compounds by the formation of new chemical bonds Bonds involve the electrons in the outer shells of atoms 1 st shell holds a maximum of 2 electrons 2 nd shell holds a maximum of 8 electrons 3 rd shell holds a maximum of 8 electrons Filled electron shells are very stable
3 Why do atoms form bonds? The atoms of noble gases have completely full outer shells and so are stable This makes the noble gases very unreactive and so they do not usually form bonds The atoms of other elements have incomplete outer electron shells and so are unstable By forming bonds, the atoms of these elements are able to have filled outer shells and become stable
4 Types of bonding Different types of bonds are formed depending on the atoms involved: - Ionic bonding: between metal and non-metal atoms - Covalent bonding: between non-metal atoms only - Metallic bonding: between metal atoms only All bonds involve electrons and all bonding involves changes to the number of electrons in the outer shell
5 Ionic bonding Ionic bonds are formed by the transfer of electrons to produce cations (+) and anions (-) Atoms in group 1 form ionic bonds with atoms in group 7 Atoms in group 2 form ionic bonds with atoms in group 6
6 How do atoms form ions? An ion is an atom or group of atoms that has an electrical charge, either positive (+) or negative (-) Atoms have an equal number of protons and electrons so do not have an overall charge Atoms with incomplete outer electron shells are unstable. By either gaining or losing electrons, atoms can obtain full outer electron shells and become stable When this happens, atoms have an unequal number of protons and electrons and so have an overall charge. This is how atoms become ions
7 Positive and negative ions An atom that loses electrons has more protons than electrons and so has a positive overall charge. This is called a positive ion An atom that gains electrons has more electrons than protons and so has a negative overall charge. This is called a negative ion
8 Positive ions (+) An atom that loses one or more electrons forms a positive ion Metal atoms form positive ions Positive ions have a small + symbol to indicate how many electrons have been lost This number is usually the same as the number of electrons in the atom s outer shell (group number) lithium atom 2.1 lithium ion [ 2 ] = Li + magnesium atom magnesium ion [ 2.8 ] = Mg 2+
9 How is a sodium ion formed? Sodium atom: 11 protons = electrons = -11 Total charge = 0 Sodium ion: 11 protons = electrons = -10 Total charge = +1 + Na loses 1 electron Na [2.8]
10 How is a magnesium ion formed? Magnesium atom: 12 protons = electrons = -12 Total charge = 0 Magnesium ion: 12 protons = electrons = -10 Total charge = Mg loses 2 electrons Mg [2.8] 2+
11 Negative ions (-) An atom that gains one or more electrons forms a negative ion Non-metal atoms form negative ions Negative ions have a small - symbol to indicate how many electrons have been gained This number is usually the same as the number of electrons in the atom s outer shell (group number) chlorine atom chloride ion [ ] = Cl - oxygen atom 2.6 oxide ion [ 2.8 ] = O 2-
12 How is a fluoride ion formed? Fluorine atom: 9 protons = +9 9 electrons = -9 Total charge = 0 Fluoride ion: 9 protons = electrons = -10 Total charge = -1 - F gains 1 electron F 2.7 [2.8] -
13 How is a sulphide ion formed? Sulphur atom: 16 protons = electrons = -16 Total charge = 0 Sulphide ion: 16 protons = electrons = -18 Total charge = S gains 2 electrons S [2.8.8] 2-
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16 Compound ions An ion made up of a group of atoms is called a compound ion Ion Formula Charge Atoms present Hydroxide OH - -1 O H Sulphate SO S O O O O Nitrate NO N O O O Carbonate CO C O O O Ammonium NH N H H H H
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18 Naming ionic compounds The name of the metal is always written first Change the ending of the name of the non-metal to ide, but only when there is a single non-metal present If there are two non-metals present and one of them is oxygen, then end the name in -ate
19 What is an ionic lattice? Ionic bonds form between a positive metal ion (cation) and a negative non-metal ion (anion) Ionic bonds are the electrostatic forces of attraction between oppositely charged ions The oppositely charged ions are arranged in a regular way to form giant ionic lattices Ionic compounds often form crystals as a result
20 Ionic bonds Sodium chloride Sodium chloride is an ionic compounds formed by the reaction between the metal sodium and the non-metal chlorine Na Na + Sodium has 1 electron in its outer shell. By losing this electron, it has a filled outer shell and forms a positive ion Chlorine has 7 electrons in its outer shell. By gaining an electron from sodium, it has a filled outer shell and forms a negative ion [2.8] + Cl Cl [2.8.8] - -
21 Ionic bonds Sodium chloride The positive sodium ions and the negative chloride ions are strongly attracted to each other. It is this electrostatic attraction that forms ionic bonds in sodium chloride + - Na Cl
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23 What is the ratio of ions? In each compound, the metal needs to lose the same number of electrons that the non-metal needs to gain NaCl Na Cl Na + Cl - 1 electron MgO Mg 2 electrons O Mg 2+ O 2- Both compounds have a 1:1 ratio of metal ions to non-metal ion, which is shown by the formula of each compound
24 What is the ratio of ions? Sodium (2,8,1) needs to lose 1 electron to form a sodium ion but oxygen (2,6) must gain 2 electrons to form an ion Na Na 1 electron from each Na atom Na + O O 2- Na + Two sodium atoms are required for each oxygen atom and so the ratio of sodium ions to oxide ions is 2:1 From this ratio, the formula of sodium oxide is Na 2 O
25 What is the ratio of ions? Magnesium (2,8,2) needs to lose 2 electrons to form a magnesium ion but chlorine (2,8,7) needs to gain 1 electron to form a chloride ion Cl Mg 1 electron for each Cl atom Cl Mg 2+ Two chlorine atoms are required for each magnesium atom and so the ratio of magnesium ions to chloride ions is 1:2 From this ratio, the formula of magnesium chloride is MgCl 2 Cl - Cl -
26 Writing the formulae of ionic compounds To work out the formula of an ionic compound: 1. Write down the symbol for each element the metal is always written first. 2. Calculate the charge for each type of ion. 3. Balance the number of ions so that the positive and negative charges are balanced and equal zero. This gives the ratio of ions. 4. Use the ratio to write down the formula of the ionic compound.
27 Formula of aluminium bromide Symbol Ion charge Balance the number of ions Ratio of ions Formula Al Br bromide ions are needed for each aluminium ion 1 : 3 AlBr 3 Al 1 electron for each bromine atom Br Br Al 3+ Br - Br - Br Br -
28 Formula of aluminium oxide Symbol Ion charge Balance the number of ions Ratio of ions Formula Al O aluminium ions are needed for 3 oxide ions 2 : 3 Al 2 O 3 Al 2 electrons for each oxygen atom Al O O 2- Al 3+ O O 2- Al 3+ O O 2-
29 Formulae of aluminium oxide
30 Formulae of ionic compounds metals nonmetals F O N Br S Cl Li Ca Na Mg Al K LiF CaF 2 NaF MgF 2 AlF 3 KF Li 2 O CaO Na 2 O MgO Al 2 O 3 K 2 O Li 3 N Ca 3 N 2 Na 3 N Mg 3 N 2 AlN K 3 N LiBr CaBr 2 NaBr MgBr 2 AlBr 3 KBr Li 2 S CaS Na 2 S MgS Al 2 S 3 K 2 S LiCl CaCl 2 NaCl MgCl 2 AlCl 3 KCl
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32 Properties of ionic compounds High melting and boiling points- Ionic bonds are very strong (strong electrostatic attraction between positively and negatively charged ions)- a lot of energy is required to break them. So ionic compounds have high melting and boiling points Conductive when liquid- Ions are charged particles, but ionic compounds can only conduct electricity if their ions are free to move and act as a current. Ionic compounds do not conduct electricity when they are solid- only when dissolved in water or melted
33 How can ionic compounds conduct electricity? As solids, ionic compounds cannot conduct electricity because their ions are bonded together in the lattice ions in solid state cannot move When liquid (molten), the ions can break free of the lattice and are able to move. The ions are charged particles and so can carry an electric current ions in molten state can move and conduct electricity
34 Properties of ionic compounds Ionic compound Properties Sodium chloride, NaCl High melting point: 800 C Magnesium oxide, MgO Non-conductive in its solid state, but when dissolves in water or molten NaCl will conduct electricity Higher melting point than sodium chloride: around 2800 C. This is because its Mg 2+ and O 2- ions have a greater number of charges, so they form stronger ionic bonds than the Na + and Cl - ions in sodium chloride Because magnesium oxide stays solid at such high temperatures, it remains non-conductive. It is used for high-temperature electrical insulation
35 Solubility acid + alkali salt + water Soluble salts dissolve in water Insoluble salts do not dissolve in water
36 Solubility of salts All common sodium, potassium and ammonium salts are soluble All nitrates are soluble Common chlorides are soluble except those of silver and lead Common sulphates are soluble except those of lead, barium and calcium Common carbonates are insoluble except those of sodium, potassium and ammonium
37 Soluble and insoluble salts Soluble All nitrates Insoluble None Most sulphates Lead sulphate, barium sulphate, calcium sulphate Most chlorides, bromides and iodides Silver chloride, silver bromide, silver iodide, lead chloride, lead bromide, lead iodide Sodium carbonate, potassium carbonate, ammonium carbonate Sodium hydroxide, potassium hydroxide, ammonium hydroxide Most other carbonates Most other hydroxides
38 Insoluble salts Insoluble salts can be formed as precipitates by the reaction of suitable reagents in solution
39 Separating and purifying insoluble salts To prepare a pure, dry sample of an insoluble salt: Separate using filtration (the insoluble salt cannot pass through the filter paper) Purify the insoluble solid using deionised water Dried by leaving the excess solution to evaporate or using a warm oven
40 Uses of insoluble salts Barium sulphate is given to patients as a barium meal to x-ray patients because: - it is opaque to x-rays - It is safe to use as, although barium salts are toxic, its insolubility prevents it entering the blood
41 Identifying carbonate (CO 3 2- ) ions Carbonates react with dilute acids to produce carbon dioxide (CO 2 ) The CO 2 can be identified by testing it with limewater Limewater turns cloudy/milky if CO 2 is present
42 Identifying sulphate (SO 4 2- ) ions When hydrochloric acid and barium chloride solution are added to SO 4 2- ions, a white precipitate forms
43 Identifying chloride (Cl - ) ions When dilute nitric acid and silver nitrate solution are added to Cl - ions, a white precipitate forms
44 Flame tests Metal Sodium (Na + ) Potassium (K + ) Calcium (Ca 2+ ) Copper (Cu 2+ ) Flame test colour Orange-yellow Lilac Brick red Blue-Green
45 Flame tests
46 Spectroscopy Chemists use spectroscopy to detect the presence of very small amounts of elements This has led to the discovery of new elements, including rubidium and caesium Each metal has a distinct fingerprint
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