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Chemistry > Elements From The Sea > Flashcards

Elements From The Sea Flashcards

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1
Q

Fluorine risks and benefits

A

Benefits- used to make plastics PTFE
Added to toothpaste to strengthen enamel
Used to make HFCs

Risks- highly reactive and handling must be kept to a minimum

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2
Q

Chlorine risks and benefits

A

Benefits- used in plastic industry (PVC)
Used in water treatment and to make pesticides, medicines and bleach.
Important intermediate in manufacture of HCl and chlorinated solvents

Risks- pesticides can accumulate in environment
CFCs destroy stratospheric ozone

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3
Q

Risks and benefits to bromine

A

Benefits - manufacture of flame retardants, agricultural figments and photography

Risks- organic bromine compounds can destroy ozone in stratosphere

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4
Q

Iodine benefits

A

Used in antiseptics, germicides and dyes

Iodine-131 is use to diagnose thyroid disease

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5
Q

Structure of ionic lattice (NaCl)

A

Na surrounded by 6 Cl
Simple cubic
Water in ionic lattice - water of crystallization
Crystals said to be hydrated

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6
Q

Ionic substances in solution

A

Hydrated ions are randomly arranged and behave independently
Each ion is surrounded by water molecules - known as hydration
-/+ have different shapes as H2O is bent

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7
Q

Spectator ions

A

Not involved in reaction and not in ionic equation

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8
Q

Rules to help tell if ionic precipitation reactions will take place when two solutions are mixed

A
  • all nitrates are soluble in water
  • all chloride are soluble in water except AgCl and PbCl2
  • all sulfates are soluble except BaSO4, PbSO4 & SrSO4
  • all sodium, potasium and ammonium salts are soluble
  • all carbonates are insoluble except (NH4)2CO3 and those of the group 1 elements
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9
Q

First ionization enthrall definition

A

Energy needed to remove one electron from each of one mole of isolated gaseous atoms of an element.

One mole of gaseous ions with one positive charge is formed.

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10
Q

Oxidation state of F and O

A 
O= -2 
F = -1
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11
Q

Oxyanions what are they

A

Negative ions that contain Oxygen and another element. Names end in -ate ie chlorate

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12
Q

Displacement reaction

A

More reactive halogen is passed into a solution of less reactive halogen.

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13
Q

Group 7 elements

A

Halogens

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14
Q

Fluorine physical properties

A

At rt - pale yellow gas
Volatility- gas
Solubility in water- reacts with water
Solubility in organic solvents- soluble

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15
Q

Chlorine physical properties

A

At rt - green gas
Volatility - gas
Solubility in water - slightly soluble to give pale green solution
Solubility in organic solvents - soluble to give pale green solution

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16
Q

Bromine physical properties

A

At Rt - dark red liquid
Volatility - liquid quickly forms brown gas on warming
Solubility in water - slightly soluble to give red-brown solution
Solubility in organic solvent - soluble to give red solution

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17
Q

Iodine physical properties

A

At rt - shiny black solid
Volatility - sublimes on warming to give purple vapor
Solubility in water - barely soluble gives brown solution
Solubility in organic solvent - soluble to give violet solution

18
Q

All halogen properties

A

Diatomic molecules (F2)
Intramolecular bonds - covalent
Intermolecular - I’d-I’d.

19
Q

Halogens oxidizing agents / reducing agents?

A

Oxidizing,, tend to remove electrons from other elements

20
Q

Reactions with silver ions and halide ions

A

Fluorine - none
Chlorine - white silver chloride
Bromine - cream silver bromide
Iodine - yellow silver iodide

21
Q

Anode and cathode

A

Anode =+

Cathode -

22
Q

Anion & Cation

A

Anion -

Cation +

23
Q

Storage and transport of fluorine

A

Fluorine is very reactive, too reactive to store. Made in situ when needed by electrolysing liquid hydrogen fluoride.

24
Q

Difference between being polar and being polarized

A

Polar - permanent dipole

Polarized - dipole

25
Q

Id- id

A

Electron density unevenly distributed at any one time -instantaneous dipole. Movement of electron cloud.
If another molecule is close it can become induced as its electron cloud is attracted to the positive end of the other electron cloud. = induced dipole.

26
Q

Pd-pd

A

Difference in electronegativity

27
Q

Electronegativity definition

A

Degree to which an atom of an element attracts electrons.
F> O> Cl> Br
N> I> S> C > H

28
Q

Homolytic fission of halogenoalkanes

A

Comditions - uv radiation
Or gas phase with high temp
RADICALS

29
Q

Heterolytic fission with halogenoalkanes

A

Conditions - dissolved in a polar solvent such as ethanol/water mixture

R-Hal —> R+ and Hal-
Forms carbocation

30
Q

Substitution reactions with halogenoalkanes

A

Nucleophilic substitutions. C-Hal bond breaks and is replaces by X-

31
Q

nucelophile defintnion

A

One or more lone pairs of electrons they can donate to form new bonds

32
Q

Halogenoalkanes to alcohol

A

H2O
Heat under reflux (hydrolysis)

Or with OH-
Heat under reflux with NaOH with ethanol as solvent

33
Q

Halogenoalkanes to amine

A

Ammonia (NH3)

Heated with conc. ammonia solution in a sealed tube

34
Q

Preparation of halogenoalkanes

A

Chloroalkane is immiscible in water. Forms later above aqueous products. Separating funnel.
Upper layer containing chloroalkane is run of into clean beaker
Shaken with sodium hydrgoencarbonate remove acidic impurities
Chloroalkane layer ran off again
Anhydrous sodium sulfate is added to remove water
Chloroalkane purified by distillation

35
Q

Batch and continuous process

A

Batch - placed in vessel and react. Once over, taken out machine cleaned and made ready for next batch.

Continuous - starting material regularly fed into one end of plant and product emerges at other.
KNOW ADV AND DISASDV OF BOTH

36
Q

Raw materials — >

A

Feedstock (reactants)

37
Q

Co-products

A

Produced at same time as the desired products via the same reaction

38
Q

By- products

A

Result from unwanted side reactions

39
Q

Percentage yield -

A

(Actual mass of product / theoretical max mass of product ) x 100

40
Q

Atom economy -

A

(Relative mass of useful product/ mass of reactants used) X 100

Chemistry (13 decks)

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