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15 Cards in this Set

  • Front
  • Back

Write an equation that shows HCL is a strong acid

HCL (aq) ---> H+ (aq) + Cl-(aq)

Suggest why a solution of pH8 is not suitable for use in eye drops

Alkali/OH- ions damage/harmful to/irritate the eye

Describe the colour changes of potassium diicrhomate if oxidises alcohols or aldehyde

- Potassium dichromate (if oxidises alcohol or aldehyde) Orange to green



Describe the colour change in bromine water when testing for c=c bonds in alkene

Bromine water - yellow/orange/brown to colourless

Describe the colour change in iron(III) chloride in the presence of phenol group

Iron(III) chloride in presence of phenol group ) yellow brown to purple

Dot and cross structure cannot account for the bonding in some molecules such as B2H6 so why chemists continue to use dot and cross structures?

- it works effectively/ well for the majority of molecules /substances

Describe the properties ionic structures

Ionic structures - properties


High melting point - strong electrostatic attractions between ions need much energy to overcome


- Soluble in water - ions can be hydrated/from strong ion-dipole bonds to water molecules


- conduct when molten ( or aqueous solution if soluble)- ions free to move in liquid/solution and carry charge and create a current

Explain why salts containing large cations and large anions are likely to have low melting points

- Weak ionic bonds or weak electrostatics forces between ions


- Small amount of energy needed to separate the ions

Explain why calcium oxide has a high melting point

Calcium oxide has a high melting point


- reference to ions or ionic structure


- strong electrostatic forces or strong attraction between forces between ions or strong ionic bonds or a lot of energy needed to break ionic bonds



How does adding -SO3H, or -SO3- Na+ change properties of organic substances

- Make more soluble in water, -ionic -SO3- groups are strongly hydrated (form strong ion-dipole bonds) in water

Carbon dioxide vs. silicon dioxide

- CO2 gas at room temp, SiO2 = solid with very high melting point


- CO2 = simple molecules, only weak instantaneous dipole-induced dipole bonds between CO2 molecules - need little energy to overcome


- SiO2 = covalent network, vast amount of energy needed to break network of strong covalent bonds


- SiO2 insoluble in water, water can't break down network of covalent bonds


- CO2 slightly soluble in water as lone pair onO atoms in CO2 can form (limited ) H- bonds to H on water molecules

Why is it goo d to bury CO2 in deep oceans/ why is it not being done?

- CO2 responsible for greenhouse effect - melts polar icecap or sea level rise, climate change harming agriculture/ecosystems


- adding CO2 to sea water reduce water pH/increase acidity - harms marine life, technology not yet developed or technology very expensive.

Give 2 ways of removing carbon dioxide from the atmosphere

- Increasing photosynthesis /planting more trees


- capture and storage by pumping to the ocean floor or sea bed/ pump deep under the sea


- capture and storage in (former) oil/gas wells/ porous rock

Why is the shape of molecule x important in a biological context ?

- to be effective x must fit the receptor/active site of the bacteria = molecular recognition


- enzyme active site( receptor sites) have specific shapes so only molecules that fit this will react ( produce response), - x bonds or forms intermolecular bonds to the active site

Write an equation corresponding to the third ionisation enthalpy of zinc

- Zn2+ (g) ---> Zn3+ (g) + e-