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Chemistry Module 3 > The periodic table and energy part 2 > Flashcards

The periodic table and energy part 2 Flashcards

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1
Q

A more reactive halogen…..

A

A more reactive halogen will oxidise and displace a less reactive halogen this is called a displacement reaction

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2
Q

What is the colour of …. in water
A, chlorine
B, Iodine
C, Bromine

A

A, Pale Green
B, Brown
C, Orange

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3
Q

What is the colour of …. in cyclohexane (organic compound)
A, Chlorine
B, Iodine
C, Bromine

A

A, pale green
B, Violet
C, Orange

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4
Q

Displacement reaction ionic equations

A

Cl2(aq) + 2Br-(aq) = 2Cl-(aq) + Br2(aq)
Cl2(aq)+2I-(aq)=2Cl-(aq)+I2(aq)
Br2(aq)+2I-(aq)= 2Br-(aq)+ I2(aq)

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5
Q

What is a disproportionate reaction

A

this is a reaction in which the same element is both reduced and oxidised

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6
Q

What does chlorine do in water

A

chlorine kills bacteria and makes the water safer the drink

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7
Q

What is done to chlorine when it reacts with water

A

both oxidised and reduced

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8
Q

Write out the equation of the reaction of chlorine and water

A

Cl2(aq)+H20(l)= HClO(aq)+ HCl(aq)

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9
Q

write out the equation of the reaction of chlorine with cold dilute aqueous NaOH

A

Cl2(aq)+2NaOH(aq)=NaCl(aq)+NaClO(aq)+H20(l)

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10
Q

what are the benefits and cons of adding chlorine to water

A 
\+Kills bacteria 
\+ gets rid of waterborne diseases 
- chlorine is a toxic gas
- chlorine reacts with organic matter to form chlorinated hydrocarbons these can cause cancer 
- ethical as people not given choice
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11
Q

What holds the metal together

A
  • BETWEEN CATIONS (positive ions in a fixed position in the lattice) AND DELOCALISED ELECTRONS (in the outer shells)
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12
Q

in a giant metallic lattice…..

A

delocalised electrons are spread throughout
electrons can move within the structure
charge must balance over the whole structure
- ARE ALL METALS

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13
Q

what is the difference between covalent and metallic structure

A

covalent - electrons are localised

metallic - electrons are delocalised

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14
Q

What are the properties of giant metallic lattices

A
  • high melting and boiling points
    this means that the electrons are free to move but positive ions are fixed, the attraction between positive ions and negative delocalised electrons are strong, high temperatures are needed to overcome the bonds
  • good electrical conductivity
    this is because the delocalised electrons can move freely within the metallic lattice this allows the electrical charge to flow
  • malleability and ductability
    malleable - can be hammered into different shapes
    ductile - can be drawn out or stretched
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15
Q

Describe the trend in melting point across the period

A

between group 1-14 melting points increase steadily, elements have giant structures and it increases each successive group as its nuclear charge increases as does the number of electrons in the outer shell causing a stronger attraction each successive element group has more electrons to form more covalent bonds
between groups 14-15 there is a sharp decrease in its melting point, elements have simple molecular structure so have weak London forces
between elements group 15-18 the melting points are low as elements have a simple molecular structure

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16
Q

LOOK AT THE TABLE ON PAGE 118

A

NO LIKE SERIOUSLY LOOK AT IT, SCAR IT IN TO YOUR MIND NOW

17
Q

Structure and bonding of diamond

A

form giant covalent
each carbon atoms form 4 other carbon atoms around it
high melting and boiling points

18
Q

structure and bonding of graphite

A

for giant covalent
layers of carbon atoms
delocalised electrons
strong and light

19
Q

structure and bonding of silicon dioxide

A

giant covalent

20
Q

What is a qualitative test

A

tells you which ions are present but not how much of each ion

21
Q

what does a qualitative test involve

A

involved a precipitation reaction from 2 aqueous solutions in which an insoluble solid forms, it is carried out on a small scale

22
Q

Describe the test for carbonate ions (negative ions)

A

add a dilute strong acid (H+) to the suspected carbonate solution
collect any gas that is formed and pass it through lime water
If the colourless gas is formed shown by fizzing and bubbles and it turns limewater cloudy then a carbonate is present in the solution

23
Q

test for carbonate ions equation

A

CO32-(aq)+2H+=H20(L) + CO2(g)

24
Q

Describe the test for sulfate ions (negative ions)

A

add dilute hydrochloric acid and barium chloride to the suspected sulfate ion. then a white precipitate of barium sulfate is produced

25
Q

write the equation for sulfate ions

A

Ba2+(aq)+SO42-(aq)= BaSO4(aq)

26
Q

What doe sulfate ions and barium sulfate ions react to form

A

sulfate ions react with barium ions to form an insoluble salt called barium sulfate

27
Q

Describe the test for halide ions (negative ions)

A

dissolve suspected halide in to water then add aqueous silver nitrate, note the colour of any precipitate formed, if colour is hard to distinguish then add dilute aqueous ammonia then concentrated, note the colour and solubility of the precipitate in the aqueous ammonia

silver chloride - white precipitate and soluble dilute ammonia
silver bromide - cream precipitate soluble in concentrated ammonia
silver iodide - yellow precipitate and insoluble in concentrated and dilute ammonia

28
Q

write the ionic equations for halide reactions

A

Ag+(aq) + Cl-(aq) = AgCl(s)
Ag+(aq) + Br-(aq) = AgBr(s)
Ag+(aq) + I-(aq) = AgI(s)

29
Q

describe the test for ammonium ions

A

add sodium hydroxide solution to the suspected ammonium compound and warm, test for any gas with red litmus paper
ammonia gas will turn red litmus paper blue, ammonia gas has a very distinct smell
bubbles will form

30
Q

write the equation for ammonium ion test

A

NH4+(aq) + OH-(aq) = NH3(aq) + H2O(aq)

31
Q

Describe Graphene

A
  • Giant covalent lattice
  • interlocking hexagonal rings
  • strong and light
  • can conduct electricity
  • used in nanotechnology as its one atom thick
32
Q

How do trends in ionisation energy support the Bohr model of the atom

A
  • Bohr model describes a positive nucleus with negatively charged electrons orbiting it
  • supported by successive ionisation energies
  • the jumps in ionisation energies tell us the electrons and the electronic structure
33
Q

Group 2 reacting with oxygen equation

A

2Mg(gas) + O2(gas) = 2MgO

34
Q

Group 2 reacting with water equation

A

Mg(s) + 2H2O(l) = Mg(OH)2(aq) + H2(g)

35
Q

Group 2 reacting with dilute acids equation

A

Mg(s) + 2HCl (aq) = MgCl2 + H2

36
Q

2nd ionisation energy of group 2

A

Be+(g) = Be2+(g) + e-

37
Q

what is the correct order to carry out tests

A
  1. carbonates
    - this is addition of acid so will no affect the sulfate or halides tests
  2. sulfate
    - must come after carbonates because BaCO3 can form which can confuse results
  3. halides
    - last test as this forms AgNO3 which will form a precipitate with carbonates and sulfates so needs to be carried out last

Chemistry Module 3 (6 decks)

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