Structure 1.2 The nuclear atom

Any particle in the nucleus

92

Not much. Similar b/c same electron configuration

Slightly different physical properties. Lighter isotope will have lower density, greater diffusion + lower melting/boiling points

An unstable isotope that breaks down spontaneously via radioactive decay (emitting nuclear radiation)

Positively charged ion (atom that has lost electrons)

Negatively charged ion (atom that has gained electrons)

The mass of an isotope relative to 1/12 the mass of a carbon-12 atom (ie. ~ 1 carbon-12 nucleon)

analytical technique that is used to measure the mass-to-charge ratio of ions

A sample of an element is injected into the mass spectrometer. Several electron streams hit the element, causing ioinsation. Result is isotopes with a charge (usually of 1+). These isotopes are accelerated by an electric field, until they reach an applied magnetic field. The magnetic field separates ions by weight and charge, with the lower mass-to-charge ratio being deflect more. The detection area measures the proportion of each isotope that hits the detection (seeing abundance)

Number of isotopes in a given sample of an element Relative isotopic mass of each isotope Relative abundance of each isotope

Usually more stable

weighted average of isotopic mass, according to relative abundances, relative to 1/12 of carbon-12

(Ir(1) x %abundance + Ir(2) x %abundance + …) / 100

Suitable acid mix