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reactivity Trends Flashcards

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1
Q

why are group 2 elements defined as ‘s’ block elements

A

the highest energy electron is found in an ‘s’ subshell

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2
Q

why does electronegativity decrease down the group

A

atomic radii increases, bonding electrons further from the nucleus , sheilding the nucleus is less able to attract these electrons

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3
Q

why does reactivity increase down the group

A

increased atomic radius , increased sheilding , which leads to decreased attraction between nucleus and outer shell electrons which means it can lose electrons easier

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4
Q

group 2 metal with water forms

A

Metal hydroxide + hydrogen

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5
Q

group 2 metal with oxygen

A

metal oxide

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6
Q

group 2 metal with dilute acid

A

metal acid and hydrogen

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7
Q

group 2 metals react ….. with oxygen

A

vigorously

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8
Q

what is the type of reaction that takes place when group 2 metal reacts with oxygen

A

redox reaction

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9
Q

what is produced when oxides react with water

A

metal hydroxide ( alkaline)

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10
Q

what are oxides and hydroxides of group 2 metals

A

bases

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11
Q

are the solid oxides and hydroxides soluble in acid

A

yes

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12
Q

what is the typical PH for a metal hydroxide

A

10-12

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13
Q

the group 2 hydroxides are only slightly ………… in water . when it becomes saturated any further metal and hydroxide ions will form a solid precipitate

A

soluble

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14
Q

solubility of the group 2 hydroxides

A

increases down the group

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15
Q

what happens to the ph as you go down group 2 and why

A

ph increases ( becomes more alkaline ) as conc of OH- ions increases as higher solubility so more alkaline

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16
Q

what is calcium hydroxide used for

A

used by farmers to neutralise acidic soils

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17
Q

what is magnesium hydroxide used for

A

indigestion remedies to neutralise excess stomach acid

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18
Q

what is calcium carbonate used for

A

neutralise stomach acid

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19
Q

how reactive are the halogens

A

the halogens are highly reactive

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20
Q

what do the halogens exist as

A

diatomic molecules

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21
Q

what melting points do the halogens have

A

they have low melting and boiling points

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22
Q

what happens to boiling points down the group and why

A

boiling points increase down the group because number of electrons increases which makes the london forces (induced dipole - dipole interactions ) between molecules stronger so more energy is needed to overcome them

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23
Q

what happens to the physical states down the group

A

gas - liquid - solid

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24
Q

what is the configuration of the halogens

A

(noble gas ) s2 p5

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25
Q

where is the highest energy electron

A

p sub shell

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26
Q

what happens to reactivity down the group and why

A

reactivity decreases down the group and oxidising power decreases because atomic radius increases as number of shells increases. electron sheilding increases , decrease nuclear attraction down the group and ability to gain an electron decreases.

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27
Q

why are the halogens strong oxidising agents

A

they gain electrons . oxidising power decreases down the group . therefore less reactive down the group

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28
Q

what happens to the halogens

A

the more reactive halogen will oxidise and displace a halide of the less reactive halogen . this is a displacement reaction

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29
Q

what is the defenition of a displacement reaction

A

is a reaction in which a more reactive element displaces a less reactive element from an aqueous solution of the latters ions

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30
Q

what colour is chlorine in water

A

pale green

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31
Q

what colour is chlorine in chlorohexane

A

pale green

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32
Q

what colour is bromine in water

A

orange

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33
Q

what colour is bromine with cyclohexane

A

orange

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34
Q

what colour is iodine with water

A

brown

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35
Q

what colour is iodine with cyclohexane

A

violet

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36
Q

why has asatine never been observed

A

because it is highly reactive

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37
Q

why are small amounts of chlorine added to drinking water

A

to kill bacteria. a mixture of two acids hydrochloric and chloric(I) is formed

38
Q

what is the formula for chloric(I)

A

HCLO(aq)

39
Q

what is the defenition for disproportionation

A

disproportionation is the oxidation and reduction of the same element in a redox reaction

40
Q

How is household bleach formed

A

If you mix chlorine gas with cold , dilute aqueous sodium hydroxide you get sodium chlorate(1) solution , sodium chloride and water

41
Q

What is the formula for household bleach

A

NACLO

42
Q

What is the equation for household bleach forming

A

2NAOH + CL2 -> NACLO + NACL + H20

43
Q

What are some uses of sodium chlorate(I) solution

A

Water treatment, bleach paper and textiles , cleaning

44
Q

What are the benefits of chlorine use

A

-Typhoid and cholera might break out if chlorine is not used
-chlorine prevents the growth of algae eliminating bad smells and tastes and removes discolouration caused by organic compounds
-it kills disease causing microorganisms
-some chlorine remains in the water and prevents reinfection further down the supply

45
Q

What are the risks of chlorine use

A

It is an extremely toxic gas and it is a respiratory irritant in small concentrations and large concentrations can be fatal .
Chlorine in drinking water can react with organic hydrocarbons eg methane and these chlorinated hydrocarbons are suspected of causing cancer
Additionally liquid chlorine on skin or eyes can cause chemical burns p

46
Q

What are the risks of chlorine use

A

It is an extremely toxic gas and is a respiratory irritant in small concentrations and large concentrations can be fatal . Chlorine in drinking water can react with organic hydrocarbons eg methane and these chlorinated hydrocarbons are suspected of causing cancer additionally liquid chlorine on skin or eyes can cause chemical burns

47
Q

What else can we use to treat water

A

Ozone (03) - a strong oxidising agent which makes it great at killing microorganisms. However it’s expensive to produce and it’s half life in water means that treatment isn’t permanent
Ultraviolet light - it kills microorganisms by damaging their DNA but it is ineffective in cloudy water and like ozone it won’t stop water being contaminated down the line

48
Q

How do we tell apart the colours of the displaced halogens

A

To tell them apart we add organic , non polar solvent eg cyclohexane and shake the mixture. The non polar halogen molecules dissolve more readily in organic solvents than in water .

49
Q

What are the phases in the tubes

A

The lower phase is the aqueos phase (water) and the upper the organic phase (hexane)

50
Q

What colour is chlorine water and potassium chloride before and after cyclohexane

A

Pale Green and pale Green

51
Q

What colour is chlorine water and potassium bromide before and after cyclohexane

A

Yellow and orange

52
Q

What colour is chlorine water and potassium iodide before and after cyclohexane

A

Orange/brown and purple

53
Q

What colour is bromine water and potassium chloride before and after cyclohexane

A

Yellow and orange

54
Q

What Is the colour of bromine water and potassium bromide before and after cyclohexane

A

Yellow and orange

55
Q

What is the colour of potassium iodide and bromine water Before and after cyclohexane

A

Orange/brown and purple

56
Q

What is the colour of iodine water and potassium chloride before and after cyclohexane

A

Orange/ brown and purple

57
Q

What is the colour of iodine water and potassium bromide before and after cyclohexane

A

Orange/ brown and purple

58
Q

What is the colour of iodine water and potassium iodide before and after cyclohexane

A

Orange/brown and purple

59
Q

what substance is used to test for halide ions

A

silver nitrate solution is used to test for halides

60
Q

describe the test for halide ions

A

first you add dilute nitric acid to remove ions that might interfere with the test, the colour of the precipitate identifies the halide then we add ammonia as each halide has a different solubility in ammonia. ( the larger the ion the more difficult to dissolve)

60
Q

what is the general ionic equation for silver nitrate and halide ion

A

Ag+ + X- -> AgX

61
Q

what colour is chloride

A

white precipitate

62
Q

what colour is bromide

A

cream precipitate

63
Q

what colour is iodide

A

yellow precipitate

64
Q

what does chloride dissolve in

A

dilute ammonia ( NH3)

65
Q

what does bromide dissolve in

A

concentrated NH3

66
Q

what does iodide dissolve in

A

insoluble in conc or dilute nh3

67
Q

What are qualitative tests for ions

A

They rely on observations , not measurements .

68
Q

What do we look for in qualitative tests for ions

A

Gas bubbles , precipitate appearance , colour changes or identification of gases

69
Q

How do you test for carbonate ions ( co3 2-)

A

Add dilute acid ( eg HCl) and if carbonate ions are present fizzing will occur and co2 is produced. If the evolved gas is co2 it will form a milky / cloudy precipitate when bubbled through limewater .

70
Q

What is the ionic equation for carbonate ions test

A

( 2H+ + CO32- —> CO2 + H20) with acid. (CO2 + Ca2+ + 2OH- —> caco3 + h20) with limewater

71
Q

How do you test for sulphate ions (SO42-)

A

Add dilute acid followed by a solution of barium ions ( eg barium chloride solution ) and a white precipitate of barium sulphate forms . Most sulphates are soluble in water but barium sulphate is insoluble

72
Q

Why is it important that you do the carbonate test before the sulphate test

A

Barium carbonate and barium sulphite are also white precipitates so only do the sulphate test if sure not carbonate is present

73
Q

What is the issue with using barium chloride solution to test for sulphate ions

A

You cannot then use the same sample to test for halide ions (chlorine present ) therefore we should use barium nitrate

74
Q

How do we remove carbonate ions

A

Keep adding dilute acid until no more effervescence

75
Q

What is the benefit of using nitric acid

A

The benefit of using nitric acid is that we can then go on and test the same sample for sulphate ions and halide ions (after testing for carbonate ) . If we used sulfuric acid to test for carbonate we cannot then use this sample to test for sulphate ions ( sulfuric acid contains sulphate ions ) additionally hydrochloric acid cannot be used to test for halide ions ( chlorine present )

76
Q

What is the test for ammonium ions (NH4+)

A

Add sodium hydroxide solution and gently warm . A gas that has a choking smell is evolved , this gas will turn damp red litmus paper blue

77
Q

Why do you heat the solution when testing for ammonium ions

A

It will not produce fizzing as ammonia gas is highly soluble in water and immediately goes into solution . However if we warm our solution then the ammonia is released from solution back to a gas

78
Q

How does the ammonia turn the litmus paper blue

A

It is alkaline and it dissolves in the water in the damp paper

79
Q

What is the sequence we have to test in if we want to do all three tests ( carbonate , sulphate and halide)

A

Carbonate test : if bubbles obtained keep adding acid until bubbling stops . This will have removed all carbonate ions . Nitric acid is used so no chloride or sulphate ions are introduced .
Sulphate test: now add an excess of barium nitrate . Filter to remove barium sulphate
Don’t use barium chloride as has halide ions
Halide test :
Any carbonate and sulphate ions will have been removed so any precipitate must be halide .

80
Q

What is an equation to prove ammonia is an alkali

A

NH3 + H20 —> NH4+ + OH- ( alkali as OH- ions produced )

81
Q

Why do we need to test for sulphate ions before we test for halide ions

A

Sulphate ions also produce a precipitate with silver nitrate causing a false positive

82
Q

What is the reaction between calcium carbonate to form calcium oxide

A

Thermal decomposition caco3 with heat —> cao + co2

83
Q

What happens to the melting points down group 2

A

Melting points decrease down the group . The metallic bonding weakens as atomic size increases , this is because the distance between the positive ions and delocalised electrons increases , therefore the electrostatic attractive forces between the cations and delocalised electrons increases weaken

84
Q

Carbon dioxide and limewater equation

A

Ca(OH)2 + CO2 ——> CaCO3 + H20

85
Q

What happens to the reactions with group 2 metals and heat down the group

A

The solutions heat up down the group

86
Q

Magnesium and steam

A

Mg + h20 (g) —> mago + h2

87
Q

Why do you need to use emery paper before doing a reaction with mg and oxygen

A

Mg will slowly react with oxygen without a flame . Mg ribbon will often have a thin layer of magnesium oxide in it this needs to be cleaned off by emery paper before doing reactions as if we are measuring reaction rates with mg and acid for example an uncleared mg ribbon would give a false result because both the mg and mgo would react at different rates

88
Q

How come magnesium hydroxide is safe to use to neutralise stomach acid

A

Because it is very weakly alkaline

89
Q

Mg burns with oxygen to produce a what flame

A

White flame

90
Q

Why is there no reaction with sodium bromide and iodine but a reaction with chlorine and sodium bromide

A

Because iodine is a weaker oxidising agent than chlorine and therefore cannot displace sodium bromide

chemistry (21 decks)

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