Ions: formulae, charge density and tests

Question 1

name some of the common gaseous ions

Answer 1

hydrogen = H2
oxygen = O2
chlorine = Cl2
nitrogen = N2
ammonia = NH3
carbon dioxide = CO2
methane = CH4

Question 2

name some common acidic ions

Answer 2

sulphuric = H2SO4
hydrochloric = HCl
nitric = HNO3
phosphoric = H3PO4

Question 3

define ionisation enthalpy

Answer 3

the first ionisation enthalpy of an element is the energy required to remove one electron from every atom in one mole of separate, gaseous atoms of the element

Question 4

whats the equation showing ionisation enthalpy?

Answer 4

X(g) => X+ (g) + e-

Question 5

which group have the lowest ionisation enthalpy values?

Answer 5

group 1, this is why they are so reactive

Question 6

which group has the highest ionisation enthalpy values?

Answer 6

noble gases, this is why they are so unreactive

Question 7

why as you go across a period do ionisation enthalpy values generally increase?

Answer 7

across a period more protons are added to the nucleus, so the extra electrons are going into the same shell with no extra shielding meaning the outer electron is more attracted to the nucleus and it takes more energy to remove it

Question 8

why when you go down a group does the 1st ionisation enthalpy decrease?

Answer 8

there is another electron shell as you go