The energy required to remove one electron from each atom in one mole of gaseous atoms of an element
1 of 16
Why does atomic radius effect the first ionisation energy?
The greater the distance between the nucleus and outer electrons, the less the nuclear attraction
2 of 16
The shielding effect/Atomic shielding
The inner shell electrons repel the outer shell electrons, reducing the attraction between the nucleus and outer electrons
3 of 16
What happens with successive ionisation?
The electrons get pulled closer to the nucleus as nuclear attraction increases. More energy is needed to remove each electron
4 of 16
Second Ionisation Energy
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element
5 of 16
What do large increases ionisation energy show?
They show when an electron has been removed from a different shell, closer to the nucleus and with less shielding
6 of 16
What predictions can be made from successive ionisation energies?
The number of electrons in the outer shell, the group element and the identity of the element
7 of 16
Why does the first ionisation energy decrease down a group?
The atomic radius and shielding increases and nuclear attraction decreases.
8 of 16
Why does the first ionisation energy increase across a period?
The nuclear change and nuclear attraction increases and atomic radius decreases. They have similar shielding.
9 of 16
Metallic bonding
The strong electrostatic attraction between positive metal ions and delocalised electrons
10 of 16
Giant metallic lattice
Metal atoms held together by metallic bonding
11 of 16
Properties of metals
Most metals have strong metallic bonds, high electrical conductivity and high melting and boiling points. They're insoluble as any interaction would lead to a reaction
12 of 16
Simple covalent lattice
Held together by weak intermolecular forces. They have low melting and boiling points.
13 of 16
Giant covalent lattice
Non-metal atoms held together by strong covalent bonds. They have high melting and boiling points. They're insoluble. They do not conduct electricity
14 of 16
Graphite
Composed of parallel layers of graphene bonded by weak London forces. Conducts electricity because one electron from each carbon is delocalised
15 of 16
What marks the the change from giant to simple molecular structures?
The increase of melting point from group 1 to 14 followed by the decrease in melting point from group 14 to 18
16 of 16
Other cards in this set
Card 2
Front
The greater the distance between the nucleus and outer electrons, the less the nuclear attraction
Back
Why does atomic radius effect the first ionisation energy?
Card 3
Front
The inner shell electrons repel the outer shell electrons, reducing the attraction between the nucleus and outer electrons
Back
Card 4
Front
The electrons get pulled closer to the nucleus as nuclear attraction increases. More energy is needed to remove each electron
Back
Card 5
Front
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element
Comments
No comments have yet been made