Systematic Carbon Chemistry Flashcards
(18 cards)
Are compounds containing only single carbon-carbon bonds saturated or unsaturated?
Saturated
Example- alkanes and cycloalkanes
What is the molecular formula for all alkanes?
CnH2n+2
What is the molecular formula for all cycloalkanes and alkenes?
CnH2n
Are compounds contains at least one carbon-carbon double bond saturated or unsaturated?
Unsaturated
Example- alkenes
What are the intermolecular forces between hydrocarbons?
LDFs
What happens to the boiling point if the hydrocarbons as the molecules get bigger in size? Why?
They increase as the main force of attraction between the hydrocarbon molecules is LDFs. So, as the molecules get bigger the electrons increase, increasing the strength of the LDFs. So, more energy is needed to break the intermolecular forces between the bigger molecules
Are the bigger or smaller hydrocarbon molecules more volatile(evaporate more easily)?
The smaller molecules as evaporation involves molecules escaping the liquid phase and becoming free in the gas phase so if the molecules are smaller the LDFs are weaker and can be overcome more easily
Are the hydrocarbons polar or non-polar?
Non-polar so they can’t dissolve in polar compounds like water and ethanol and can’t form hydrogen bonds to water molecules
Why are the hydrocarbons useful solvents?
They’re non-polar so can dissolve other non-polar substances and as solvents they evaporate easily so they can extract compounds then be easily evaporated after
What are isomers?
Compounds with the same molecular formula but different structural formula
What are addition reactions?
When two molecules combine to form a single molecule?
What type of reaction do compounds contain double bonds take part in?
They can take part in addition reactions
How does bromine solution distinguish between saturated and unsaturated compounds?
Unsaturated compounds will de colourise in bromine solution
What different homologous series can be isomers?
Alkenes+cycloalkanes
Carboxylic acids+esters
Aldehydes+ketones
Comment on hydrogen bonding for solubility, boiling point and volatility
Increase solubility
Increases boiling point
Decreases volatility as molecules closer together
Comment on spatial arrangement of polar covalent bonds for solubility,volatility and boiling point
Polar molecules more likely to be soluble in polar solvents
PD-PD attractions bring molecules closer together raising b.p
Closer together molecules less volatile, less likely to turn into a gas
Comment on molecular size of molecules for solubility, volatility and boiling point
Solubility often decreases as molecules get bigger
Bigger molecules have stronger LDFs so increases boiling point
Bigger molecules closer together decreases volatility
Comment on polarities of solute and solvent for solubility, volatility and boiling point
If substance has polar groups more likely to be soluble in water
No effect on boiling point or volatility
