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describe chemical equations by showing only the reacting ions in solutions while leaving out the spectator ions

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Ionic equations

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Ions which are present but not involved in the reaction

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Spectator ions

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a reaction in which produces a solid precipitate on mixing 2 solutions containing ions

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Ionic precipitation reaction

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When a compound decomposes on heating

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Thermal decomposition

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green copper(II) carbonate breaks up into black copper(II) oxide and CO2. Most carbonates other than the group 1 metals decompose on heating. Hydrated compounds also decompose on heating

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Thermal decomposition example and details

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salt + hydrogen salt + water salt + water salt + water + carbon dioxide

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Acid + metal > Acid + metal oxide > Acid + metal hydroxide > Acid + metal carbonate >

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All are soluble

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Which acids are soluble/insoluble in water

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Soluble: Alkalis, Na/K CO3 and OH. CaOH is slightly soluble.

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Which metal hydroxides/carbonates are soluble/insoluble?

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Soluble: all nitrates, chlorides (except silver and lead ones), sulphates (Ca and Ag slightly)(except barium and lead aren't)

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Which Salts are soluble/insoluble?

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Li2CO3 is used in drugs for treating mental illness, some of its compounds are vital for organic synthesis

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(Group 1) uses of lithium

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Sodium is a powerful reducing agent used to extract titanium, sodium vapour is used in streetlights and NaOH is the most important industrial alkali

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(Group 1) uses of Sodium

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Potassium ions are an essential nutrient in plants and an ingredient of some fertilisers

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(Group 1) uses of Potassium

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describes the way in which a property increases or decreases along a series of elements or compounds

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Trend

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Charge of the nucleus increases, and number of filled inner shells increases, thus the atomic radius increases down the group

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How does atomic radius change down the group

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The no. of electrons in the inner shells is always 1 less than the number of protons in the nucleus, the shielding affect increases down the group meaning that, with a constant effective nuclear charge, and the outer electrons getting further away, the outer electron is less attracted down the group.

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(Group 1) Why does reactivity increase down the group?

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metal hydroxide + hydrogen

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Alkali metal + water >

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All G1 metals react vigorously with chlorine to for colourless ionic salts (2M + Cl2 > 2MCl) which are soluble in water

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Group 1 plus chlorine...

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anti-acids, acids give up H+ ions, whilst bases accept H+ ions

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Bases

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all white solids, soluble in water forming alkaline solutions, solubility increases down the group. These are strong bases because they are fully ionised in water

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Hydroxides of G1

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white with general formula M2CO3. They are soluble unusually and solutions of these are alkaline because the carbonate ions remove H+ ions. CO32-(aq) + H2O(l) > HCO3-(aq)+ OH-(aq). Most of these don't decompose when heated, except for Li2CO3

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Carbonates of G1

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White crystalline solids (MNO3(s)) and highly soluble. These are much harder to decompose than most nitrates, first melting before decomposing, releasing O2 and becoming nitrites: 2KNO3(s) > 2KNO2(s) + O2(g). LiNO3 however behaves like other nitrates, decomposing to form an oxide, NO2 and O

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Nitrates of G1

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the ions are unreactive and are thus spectators. Additionally their compounds are soluble in water and they are colourless so they don't hide or interfere with colour changes

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Why are Na and K compounds are used as chemical reagents

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lithium: bright red, sodium: bright yellow, potassium: lilac

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Flame colours of G1

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Flame excites outer electrons of sodium ions, raising them to higher energy levels. The atoms emit the light as the electrons drop back to lower energy levels

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Why do flame colours happen?

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Alkaline earth metals

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Group 2 are

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Harder and denser than group 1, with higher melting temperatures

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Difference between G1 and G2

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Be is a strong metal with a high MT, but less dense than transition metals. Mg is low density, making light alloys used in aircraft and car manufacture. Ba is soft, and highly reactive with air and moisure so is kept under oil.

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Uses of beryllium, magnesium and barium

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The increasing no. of shells down the group means the atomic radii increase down the group hence the reactivity increases down the group as the pull on outer electrons decreases

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(G2) why does reactivity increase down the group?

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The 1st and 2nd decrease down the group, the shielding means the greater effective nuclear charge attracting the outer electron is 2+. Down the group the outer electrons get further away from the same nuclear charge so they are attracted less

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G2 ionisation energy trends

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Mg burns with a white flame, which is why it is used in fireworks and flares. It produces MgO

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(Group 2) Mg reacting with oxygen

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Ca burns with a red flame forming CaO, strontium reacts similarly

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(Group 2) Ca reacting with oxygen

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Ba burns with a green flame to form Barium peroxide, BaO2

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(Group 2) Ba reacting with oxygen

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Mg reacts very slowly with cold water producing Mg(OH)2 and H2. It reacts better with steam

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(Group 2) Mg reacting with water

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Ca reacts to produce H2 and Ca(OH)2, initially the Ca(OH)2 dissolves but the solubility is low so as more forms the solution becomes saturated and a precipitate appears

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(Group 2) Ca reacting with water

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Ba reacts even faster than Ca and its hydroxide is more soluble

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(Group 2) Ba reacting with water

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all G2 metals react with Cl on heating to form white chlorides, MCl2

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How does group 2 react with chlorine?

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a metal oxide which reacts to form salts and water. Soluble basic oxides are alkalis as the oxide acts as a base taking the H+ ions from the acid. All G2 metals apart from Be form these.

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Basic oxide

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MgO is a white solid, which turns into a hydroxide when added to water. This is slightly soluble. MgO has a high melting point so is often used as a heat resistant ceramic to line furnaces

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Magnesium oxide

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CaO is a white solid made by heating CaCO3, it reacts vigorously with cold water, hence the traditional name 'quicklime', and this reaction produces calcium hydroxide.

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Calcium oxide

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Mg(OH)2 is the active ingredient in milk of magnesia, used as an antacid and a laxative

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Magnesium hydroxide

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Ca(OH)2 is slightly soluble in water forming an alkaline solution, limewater. The CO2 test works because a solution of Ca(OH)2 reacts with the gas forming a white insoluble calcium carbonate precipitate

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Calcium hydroxide

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Ba(OH)2 is soluble, sometimes used as an alkali in chemical analysis. It is better than sodium and potassium for this as it can't be contaminated by its carbonate, because barium carbonate is insoluble in water

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Barium hydroxide

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All have the formula M (OH)2 and are to varying degrees soluble in water, forming alkaline solutions, however their solubility increases down the group

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G2 hydroxides

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They all have the formula MCO3 and are insoluble in water, they all react with dilute acids and decompose on heating to give the oxide and CO2. However they are more difficult to decompose down the group - they become more thermally stable

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G2 carbonates

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They all have the formula M(NO3)2, are colourless, crystalline solids, very soluble in water and decompose to the oxide on heating. They become more difficult to decompose down the group

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G2 nitrates

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All colourless solid with the formula MSO4 but are less soluble down the group

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G2 sulphates

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beryllium and magnesium - no colour, calcium - brick red, strontium - bright red, barium - pale green

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Flame colours for G2

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an indication as to the ease with which compounds decompose on heating. Compounds are stable if they do not tend to decompose into their elements or into other compounds. A compound, which is stable at RTP may become more or less stable as conditions change

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Thermal stability

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an indication of the extent to which a + ion is able to distort the electron cloud around a - ion. The larger the charge of the + ion and the smaller its size, the greater its polarising power

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Polarising power

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...that the larger the charge on the metal ion, and the smaller the metal ion, the less stable the compounds

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G2 carbonates and nitrates are generally less stable than the corresponding G1 compounds. This suggests...

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The carbonates become more stable down group 1 and 2, this helps confirm that the larger the metal ion, the more stable the compound

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Trend in stability in carbonates..?

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The larger the charge and the smaller the ionic radius, the greater the charge density and thus the greater the polarising power of the ion. Higher polarising power means the ions pulls at the electrons more, distorting the bonding and making it easier to break up the - ion into an oxide ion and CO2

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thermal stability explained in terms of polarising power

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Although the charge remains constant down the group the size increases, decreasing the charge density, and thus the polarising power. Thus the thermal stability of the nitrates and carbonates increases down the group

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why does thermal stability increase down the group?

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They are used as ingredients in plastics, pharmaceuticals, anaesthetics and dyestuffs

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Uses of the halogens

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At RTP, chlorine is a yellow-green gas, bromine is a dark red liquid and iodine is a dark grey solid. They exist as diatomic molecules linked by a single covalent bond.

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Appearance of halogens

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Intermolecular forces increase down the group as the numbers of electrons in the molecules increase, the larger molecules are therefore more polarisable so M and B temps increase down the group.

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Halogens and intermolecular forces

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most electronegative element, oxidation state -1

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Fluorine

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1 oxidation state, but can be oxidised to positive states by F and O. Chlorine is used in the product of polymers (PVC). It is also used to 'chlorinate' drinking water.

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Chlorine

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Reactive but a less powerful oxidising agent than fluorine, it is used to make medicines, dyes and flame-retardants.

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Bromine

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Used to make medicines, dyes and catalysts. Iodine is important in the diet so that the thyroid gland can make the hormone thyroxine, which regulates growth and metabolism.

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Iodine

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Dissolve in hydrocarbon solvents (cyclohexane), when dissolved, the solution will appear a similar colour to the free halogen vapours (iodine - violet...)

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Halogens and hydrocarbon solvents

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Halogens are less soluble in water, Cl and Br(aq) are useful reagents, colours are similar to those of vapours. These also react with water. I doesn't dissolve in water but is does dissolve in KI(aq), I2 reacts with the iodide ions to form triiodide ions (yellow-brown colour)

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Halogens and water

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react with G1 and 2 to form ionic halides

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(G7) Cl and Br + metals

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reacts to form iodides but because of the polarisability of the iodide ion, iodides formed with small cations (Li+) or highly charged ones (Al3+) are essentially covalent

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(G7) I + metals

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Halogens do react with most d block metals - when they react with hot iron, they form Iron (III) chloride, Iron(III) bromide and iron(II) iodide as iodine reduces the iron (III) ions

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(G7) Halogens + d block metals

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Cl reacts with most non metals to form molecular chlorides, e.g. SiCl4(l). However chlorine will not react directly with C, O or F. H burns in Cl to produce colourless HCl(g)

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(G7) Chlorine + non metals

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Bromine oxidises non-metals such as S and H when heated forming molecular bromides. Bromine vapour and hydrogen gas react smoothly with a pale bluish flame

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(G7) Bromine + non metals

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Iodine oxidises H on heating to form HI, which is a reversible reaction

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(G7) Iodine + non metals

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Cl and Br can oxidise iron (II) ions(aq) but iodine cannot

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Halogens + Fe2+ ions (aq)

question

1) White precipitate turns purple-grey in sunlight 2)Dissolves in dilute ammonia, forming a colourless solution

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AgCl: 1) obs when AgNO3 is added, 2) obs when ammonia is added

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1) Creamy precipitate 2)Dissolves in concentrated ammonia forming a colourless solution.

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AgBr: 1) obs when AgNO3 is added, 2) obs when ammonia is added

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1)Yellow precipitate 2)Does not dissolve.

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AgI: 1) obs when AgNO3 is added, 2) obs when ammonia is added

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Silver fluoride is soluble so there is no precipitate to start with.

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AgF: 1) obs when AgNO3 is added, 2) obs when ammonia is added

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NaCl + NaSO4 -> HCl (g). The gas fumes in moist air. This doesn't work with Br as bromide ions are oxidised to bromine by sulphuric acid. Iodide ions as such strong reducing agents that they reduce sulphur from +6 to 0 and -2

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Halogens reacting with concentrated sulphuric acid overview..

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> HCl + NaHSO4. Product: HCl, observation: gas which fumes in moist air, reaction type: acid -base.

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NaCl reacting with concentrated H2SO4 (Halide Cl-).

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Observation: orange vapour, reaction type: oxidation, equation: 2Br- > Br2 + 2e-

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Bromide reacting with H2SO4. Product: Br2

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Observation: Colourless acidic gas, Reaction type: Reduction, Equation: H2SO4 + 2H+ + 2e- > SO2 + 2H2O

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Bromide reacting with H2SO4. Product: SO2

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Observation: Steamy fumes, Reaction type: Acid-base, Equation: 2NaBr + H2SO4 > HBr + NaHSO4

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Bromide reacting with H2SO4. Product: HBr

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Observation: Steamy fumes, Reaction type: Acid-base Equation: NaI + H2SO4 > HI + NaHSO4

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Iodide reacting with H2SO4. Product: HI

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Observation: Purple solid, Reaction type: Oxidation, Equation: H2SO4 + 8H+ + 8I- > 4I2 + H2S + 4H2O

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Iodide reacting with H2SO4. Product: I2

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Observation: - Reaction type: Reduction, Equation: H2SO4 + 8H+ + 8I- > 4I2 + H2S + 4H2O

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Iodide reacting with H2SO4. Product: H2S

question

Observation: Gas with bad egg smell, Reaction type: Reduction, Equation: H2SO4 + 2H+ + 2I- > I2 + SO2 + H2O

answer

Iodide reacting with H2SO4. Product: SO2

question

Observation: Yellow solid, Reaction type: Reduction, Equation: H2SO4 + 6H+ + 6I- > 3I2 + S + 4H2O

answer

Iodide reacting with H2SO4. Product: S

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The power of halides as reducing agents increases down the group, and for oxidising agents increases up the group.

answer

Halide reducing and oxidising trends

question

They are colourless polar, molecular compounds at RT that fume in moist air, with formula HX. They are soluble in water, forming acidic solutions, which ionise completely in water.

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Hydrogen halides

question

Mixing the hydrogen halides with ammonia produces a white smoke of an ammonium salt. Ammonia molecules become ammonium ions in this reaction

answer

hydrogen halide + ammonia

question

an ion with the general formula XxOyz- (where X is any element and O is oxygen)

answer

Oxoanion

question

Oxoanions form. Cl dissolves in water to form a mix of weak chloric and strong hydrochloric acid. This is a disprop reaction. Cl2 + H2O > HCl + HClO Br reacts similarly but to a lesser extent and I is insoluble in water and barely reacts

answer

What happens when halogens react with water and alkalis

question

chlorate (I) and chloride ions: The active ingredient in bleach is sodium chlorate, made by using NaOH in this reaction. When heated the chlorate (I) ions disproportionate to chlorate (V) and chloride ions. Cl2 + 2OH- > ClO + Cl + H2O

answer

(G7 in +1 and +5 states) When chlorine dissolves in KOH at RT, it produces

question

Br and I react in a similar way to Cl with alkalis, though the BrO- and IO- are less stable, so they disproportionate at a lower temperature.

answer

(G7 in +1 and +5 states) When Br and I react with alkalis

Chapter 4 – Inorganic chemistry and the periodic table – Flashcards

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