C 2.1.1 Atomic structure & Isotopes

2.1.1a Define Isotope

Atoms of the same element with the same number of protons and different number of neutrons, resulting in a different mass number

2.1.1a State the properties/reactivity of isotopes

Isotopes have the same electron configurations, react chemically the same and share e- the same but have different physical properties

2.1.1a The maximum number of e- a single shell can hold is determined by?

The number of that specific shell (n) put into the equation 2n²

2.1.1b How is an ion formed?

When an atom gains or loses an electron giving it a positive or negative charge

2.1.1b Atomic/proton number shows?

The protons/electron number

2.1.1b Mass number shows?

The number of protons AND neutrons together

2.1.1c Define relative molecular mass Mr

The weighted mean mass of a molecule of a compound, relative to one twelfthof the mean mass of an atom of the carbon-12 isotope.

2.1.1c Define relative atomic mass Ar

The weighted mean mass of an atom of an element, relative to one twelfthof the mean mass of an atom of the carbon-12 isotope.

2.1.1d What is mass spectrometry used for and how?

Identifies different isotopes and relative atomic masses

ToF (Time of Flight) How long is takes an ion of an isotope to reach a detector

2.1.1di Define relative isotopic mass

The isotopic mass of an isotope relative to one twelfth of themean mass of an atom of the carbon-12 isotope.

2.1.1di What is relative abundance?

The percentage of an atom which is made up of a specific isotope

2.1.1dii Equation of relative atomic mass Ar

2.1.1e What is relative formula mass used for?

Used for compounds with giant structures

2.1.1e What is relative molecular mass used for and how is it found?

Used for simple molecules

Adding the Ar of each element together