Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Chemistry 3.6
A-level
| Term | Definition |
|---|---|
| Principle of conservation of energy | Energy cannot be created or destroyed but may only be converted from one form to another |
| Hess's Law | The energy change of a chemical reaction is the same, regardless of the route taken |
| Enthalpy change= | ∆Hf (products) - ∆Hf (reactants) |
| Standard conditions | 298K 1atm. 1moldm^-3 |
| Standard state | Physical state a compound is found in under standard conditions |
| Standard Enthalpy change | The enthalpy change of a reaction, between molar quantities of reactants in their standard state, under standard conditions |
| Standard enthalpy change of atomisation | The enthalpy change when one mole of atoms in the gaseous phase are formed from one mole of the element in its standard state, under standard conditions. A change of molecular structure and change of state |
| Standard enthalpy change of lattice formation | Enthalpy change when one mole of an ionic compound is formed from the ions of the elements in the gas phase, under standard conditions |
| Standard enthalpy change of lattice breaking | Enthalpy change when one mole of an ionic compound is broken into the ions of the elements in the gas phase, under standard conditions |
| Standard enthalpy change of hydration | The enthalpy change when one mole of an ionic compound in solution is formed from the ions of the elements in the gas phase, under standard conditions |
| Electron affinity | The enthalpy change when one mole of gaseous negative ions are formed from a mole of gaseous atoms gaining an electron, under standard conditions |
| Ionisation energy | The enthalpy change when one mole of gaseous positive ions are formed from a mole of gaseous atoms by losing an electron, under standard conditions |
| Exothermic reaction | Energy is given out as heat, leaving less chemical energy in the products than were in the reactants |
| Endothermic reaction | Energy is taken in as heat energy, leaving more chemical energy in the products than were in the reactants |
| Standard enthalpy change of a solution | The enthalpy change that occurs when one mole of a substance dissolves completely in a solvent, under standard condition |
| Standard enthalpy change of a solution= | - ∆Hlatt +∆H hyd |
| Standard enthalpy change of formation | Measure of enthalpy change when one mole of a gaseous substance is formed from one mole of gaseous atoms, under standard conditions |
| Standard enthalpy change of combustion | Measure of enthalpy change when one mole of a gaseous substance is completely combusted in the presence of Oxygen to form one mole of gaseous atoms, under standard conditions |
| Average bond enthalpy | The average enthalpy change when one mole of a gaseous compound bond is homolytically broken to form a mole of gaseous molecules, under standard conditions. |
| Bond enthalpy change of a reaction= | Σ∆H (reactants) - Σ∆H(products) Bonds broken - Bonds formed Exothermic if negative |
| Bond enthalpy of products are | Negative!! Energy is released when bond is formed |
Created by:
Zoe 1
Popular Chemistry sets