chemical energetics
- Created by: studentdaniya
- Created on: 14-06-21 17:21
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- chemical energetics
- lattice energy
- energy released when 1 mole of an ionic compound is formed from it's gaseous ions under standard condtions
- only for ionic compounds
- Cl- + Na+ ----> NaCl
- Always exothermic as only bonds are being made
- H.E AND L.E are directly proportional to C.D
- Hydration energy
- always exothermic as no bond is breaking
- enthalpy change when 1 mole of gaseous ions are dissolved in excess of water under standard conditions
- L.E >H.E sol energy is +ive and the salt is insoluble
- L.E < H.E sol energy is -ive and the salt is insoluble
- Hydration energy
- energy released when 1 mole of an ionic compound is formed from it's gaseous ions under standard condtions
- Atomization energy
- energy absorbed to release 1 mole gaseous atom from its element in its standard physical state under standard conditions
- always endothermic
- FOR DIATOMIC GASES: ~BE=2AE ~1/2BE=AE
- energy absorbed to break 1 mole covalent bond in gaseous state under standard conditions
- energy absorbed to release 1 mole gaseous atom from its element in its standard physical state under standard conditions
- Bond energy
- energy absorbed to break 1 mole covalent bond in gaseous state under standard conditions
- Electron affinity
- the enthalpy change when 1 mole of electrons is added to 1 mole of gaseous atoms to form 1 mole gaseous 1- ions under standard conditions
- mostly for non-metals
- always anions are formed
- 1st EA is exothermic but second is endo
- as more e-s are added more endo it get as more energy is requiered
- the enthalpy change when 1 mole of electrons is added to 1 mole of gaseous atoms to form 1 mole gaseous 1- ions under standard conditions
- Ionization energy
- energy needed to remove 1 mole of electrons from 1 mole of atoms of an element in the gaseous state to form 1 mole gaseous ions.
- The FIRST IONIZATION ENERGY is the energy required to remove 1 mole electrons from 1 mole of atoms to form 1 mole gaseous 1+ ions.
- energy needed to remove 1 mole of electrons from 1 mole of atoms of an element in the gaseous state to form 1 mole gaseous ions.
- Charge density
- Ratio of charge to its radius
- for ions only
- C.D = charge of ion/radius
- C.D (d) Charge C.D (id)radius
- Down the group C.D decreases
- Across the period charge density increases for metals and decreases for non-metals
- Ratio of charge to its radius
- Formation energy
- enthalpy change when 1 mole compound is formed from its elements under standard conditions in standard form
- can be endo or exo as bonds are being made and break
- enthalpy change when 1 mole compound is formed from its elements under standard conditions in standard form
- Hydration energy
- always exothermic as no bond is breaking
- enthalpy change when 1 mole of gaseous ions are dissolved in excess of water under standard conditions
- Solution energy
- energy absorbed / released to dissolve 1 mole compound in excess of water under standard conditions
- soluble salt= exothermic reaction / -ive
- insoluble salt= endothermic reaction / +ive
- energy absorbed / released to dissolve 1 mole compound in excess of water under standard conditions
- Polarity
- distortion of electron cloud of anion caused by cation
- the more the polarization, the more thermally unstable the compound is
- polarization (d) charge density
- C.D (d) Charge C.D (id)radius
- polarization (d) charge density
- the more the polarization, the more thermally unstable the compound is
- distortion of electron cloud of anion caused by cation
- lattice energy
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