Paper 1 Flashcards by Aleesha Khan

Trend in BP down halogens

More electrons

Strong LFs

More energy to break IMFs

BP increase

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Define 1st ionisation energy

Renege required to remove 1 electron form each atom in 1 mol of gaseous atoms of an element to form 1 mole of gaseous 1+ ions.

E.g. Na(g) —> Na+ (g) + e^-

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Define periodicity

Repeating trend in properties of elements across each period of periodic table

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Strongest IMFs

LFs —> permanent dipole-dipole —> HBs
—increase in strength—>

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How LFs brought about

Movement of electrons produce changing dipole

Instantaneous dipole will exist

And induce a dipole on neighbouring molecule

Which further induces dipole on neighbouring molecules and attract 1 another

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Acid + metal carbonate

Salt + H2O + CO2

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Acid + alkali

Salt + H2O

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Acid + metal oxide/hydroxide

Salt + H2O

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Ideal gas assumptions

No IMFs

Random motion

Elastic collisions

Negligible size

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Hydrated salts assumptions

All H2O lost - heat to constant mass

No further decomposition

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Define hydrated and water of crystallisation

H2O molecules are apart of crystalline structure

This water is known as water of crystallisation

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Define relative atomic mass

Weighted mean mass of an atom of an element relative to 1/12th of mass of an atom of C-12

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Define relative isotopic mass

Mass of isotope relative to 1/12th of mass of atom of C-12

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Define isotope

Atoms of same element with different numbers of neutrons and different masses

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Shape of p-orbitals

Dumb bell

Hold up to 1 or 2 electrons

3 p-orbitals

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S-orbital

Sphere

Hold 1/2 electrons

She’ll number and electrons formula

n = shell number

2n^2

Define atomic orbital

Region around nucelus that can hold up to 2 electrons with OPP spins

Acid + metal

Salt + hydrogen

Define metallic bond

Strong electrostatic attraction between positive ions and delocalised electrons

Metallic bond properties

High electrical conductivity - delocalised electrons carry charge

High MP + BP - strong MB—> strong attraction

Giant metallic lattice

Don’t dissolve

Graphene and graphite

3 of 4 outer shell e-s used in CB
remaining e- released into pool of delocalised e-s shred by all atoms in the structure
- good electrical conductors
giant covalent structures of C
planar hexagonal layers
bond angle = 120* by electron-pair repulsion

graphene =

single layer of graphite
hexagonally arranged C atoms linked by strong CBs

graphite =
- parallel layers of hexagonally arranged C atoms
- layers bonded by weak LFs
- 3 of 4 outer shell e-s used in CB
- remaining e- released into pool of delocalised e-s shred by all atoms in the structure

what is the bond angle and structure of (carbon) Diamond?

tetrahedral arrangement - bond angle = 109.5* because of electron pair repulsion

why can’t silicon and carbon (diamond) conduct electricity?

in both structures, all 4 outer shell electrons are involved in CB, so none are available for conducting electricity.

C & Si

group 14 (4) - 4 electrons in their outer shell C (in diamond form) and Si use these 4 electrons to form CBs to other C/Si atoms

what is the structure and bonding of B, C and Si?

Giant covalent lattice - many billions of atoms are held together by a network of strong covalent bonds

Define 2nd ionisation energy

He+ (g) —> He2+(g) + e- Energy required to remove 1 electron from each ion in 1 mol of gaseous 1+ ions of an element to form 1 mole of gaseous 2+ ions.

2nd ionisation energy explanation

After 1st electron lost, electron pulled closer to nucleus Nuclear attraction increases + more IE needed to remove 2nd electron

Trend in IE down group

Atomic radius increases More inner shell - increased shielding Nuclear attraction on outer electrons decreases 1st IE decreases

Trend in IE across period

Nuclear charge increases Same shell - similar shielding Nuclear attraction increases Atomic radius decreases 1st IE increases

Trend in reactivity of halogens

Atomic radius increases More inner shells so shielding increases Less nuclear attraction to capture an electron from another species Reactivity decreases

Disproportionation reaction

Redox reaction in which same element is reduced and oxidised

Enthalpy change of formation

is the enthalpy change that takes place when one mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states.

Enthalpy change of combustion

enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, with all reactants and products in their standard states.

Enthalpy change of neutralisation

is the energy change that accompanies the reaction of an acid by a base to form one mole of H.O(). under standard conditions, with all reactants and products in their standard states.

Buffer solution

Mixture of weak acid and its conjugate base which minimises changes in pH when small quantities of acid or alkali are added.

Define conjugate acid-base pair

Contains 2 species that can be interconverted by the transfer of a proton

Define a salt

The product of a reaction in which the H+ ions from the acid are replaced by metal or ammonium ions.