The Atoms And Redox Flashcards
Rules for assigning oxidation number
- Unrelated element = 0
- Group I, II, III metals become +1+2+3
- Oxygen in a compound is always -2
- Hydrogen becomes +1
- Group VII elements are usually -1
Oxidation number
The monitoring of electron movement of individual elements in compound ions and covalent compounds.
First ionisation energy
The energy required to remove one electron from each atom of 1 mole of gaseous atoms
Inner electron layers are called?
Shielding electrons
Relative atomic mass
The weighted mean average of all isotopes of an element compared to one twelfth of carbon-12
Relative isotopic mass
The mass of one atom of a specific isotope compared to one twelfth mass of one atom of the isotope carbon-12
Molar mass
The mass of one mole of the atom
Mole
The number of atoms of carbon-12 in exactly 12g of carbon-12. This number is 6.02x10^23
Salt
Compound formed when the H+ ion in an acid is replaced by a metal or ammonium ion
Isotope
Atoms with the same number of protons vut a different number of neutrons
Examples of bases (4)
- NaCl
- Any type of oxide
- CO3 ion
- Ammonia
Alkali
A soluble base that releases OH- ions in water
Acid
A proton donor
Base
A proton acceptor
Test for halides using silver nitrate (testing for halides in solution)
-If halides are present there will be either a white (chloride), cream (bromide) or yellow (iodide) precipitate
Test for halides using ammonia (2)
- In dilute ammonia solution, chloride ions are soluble while bromide and iodide ions are not
- In concentrated ammonia solution, chloride and bromide ions are soluble while iodide ions are not
Spectator ion
An ion that doesn’t undergo a chemical change
Precipitate
One or more insoluble products that form when reacting two soluble salts
Orbital
Regions of space that can be occupied by up to two electrons of the same energy and opposite spin
Electron behaviour within an orbital
According to Schroedingers equation we know that electrons are randomly moving around so orbitals are drawn as 90% orbitals as that is where we expect them to be for 90% of the time
The four types of orbital
s, p, d, f
Trends in first ionisation energy
As you go down a group the first ionisation energy decreases
As you go along a period the first ionisation energy increases
First ionisation energy dips very slightly between the transition from group 2-3, 5-6
