2022-01-12T00:01:19+03:00[Europe/Moscow] en true <p>definition of enthalpy change</p>, <p>definition of the standard enthalpy change of atomisation </p>, <p>standard temperature conditions</p>, <p>standard pressure conditions</p>, <p>what is Δ<em>H<sub>at</sub></em><sup>ꝋ</sup></p>, <p>is Δ<em>H<sub>at</sub></em><sup>ꝋ</sup> endothermic or exothermic</p>, <p>why is Δ<em>H<sub>at</sub></em><sup>ꝋ</sup> endothermic</p>, <p>the standard enthalpy of atomisation can be shown by</p>, <p>what is an example of a typical element that has a standard enthalpy of atomisation </p>, <p>definition of lattice energy</p>, <p>what is the symbol for lattice energy?</p>, <p>is Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> endothermic or exothermic?</p>, <p>why is Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> always exothermic?</p>, <p>what does the large negative value of Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> suggest? (1)</p>, <p>what does the large negative value of Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> suggest? (2)</p>, <p> the more exothermic the value is, the</p>, <p>true or false</p><p>the Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> can be determined directly by one single experiments</p>, <p>why are gaseous ions less stable than a solid ionic lattice</p>, <p>to find the Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> of ionic compounds, what methods can be used?</p>, <p>what can the lattice energy also be expressed as ?</p>, <p>an example of an ionic compound with a Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup></p>, <p>an equation to express an examplary equation for Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup></p>, <p>remember to always include **** in Δ<em>H<sub>latt</sub></em><sup>ꝋ</sup> equations</p> flashcards

A2 Level Lattice Energy & Enthalpy Change Of Atomisation

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  • definition of enthalpy change

    the amount of heat energy transferred during a chemical reaction at a constant pressure

  • definition of the standard enthalpy change of atomisation

    the enthalpy change when 1 mole of gaseous atoms is formed from its element under standard conditions

  • standard temperature conditions

    298K

  • standard pressure conditions

    101KPa

  • what is ΔHatꝋ

    standard enthalpy change of atomisation

  • is ΔHatꝋ endothermic or exothermic

    always endothermic, always positive

  • why is ΔHatꝋ endothermic

    energy is required to break bonds

  • the standard enthalpy of atomisation can be shown by

    equations

  • what is an example of a typical element that has a standard enthalpy of atomisation

    sodium

  • definition of lattice energy

    the enthalpy change when 1 mole of an ionic compound is formed from its gaseous ions under standard conditions

  • what is the symbol for lattice energy?

    ΔHlattꝋ

  • is ΔHlattꝋ endothermic or exothermic?

    always exothermic, always negative

  • why is ΔHlattꝋ always exothermic?

    when ions combine to form a lattice, there is an extremely large release of energy (large negative)

  • what does the large negative value of ΔHlattꝋ suggest? (1)

    the ionic compound formed is more stable than the gaseous ions

  • what does the large negative value of ΔHlattꝋ suggest? (2)

    strong electrostatic forces of attraction between oppositely charged ions in the solid lattice

  • the more exothermic the value is, the

    stronger the ionic bonds within the lattice are

  • true or false

    the ΔHlattꝋ can be determined directly by one single experiments

    false

    it cannot

  • why are gaseous ions less stable than a solid ionic lattice

    there are no electrostatic forces of attraction between the gaseous ions

  • to find the ΔHlattꝋ of ionic compounds, what methods can be used?

    multiple experimental values

    an energy cycle

  • what can the lattice energy also be expressed as ?

    an equation

  • an example of an ionic compound with a ΔHlattꝋ

    magnesium chloride

  • an equation to express an examplary equation for ΔHlattꝋ

    Mg2+(g) + 2Cl–(g) → MgCl2(s)

  • remember to always include **** in ΔHlattꝋ equations

    state symbols