the nuclear atom

nucleus

positively charged, highly dense structure that contains virtually all the mass of the atom

protons + neutrons

relative mass (number of neutrons)

the difference between the atomic number and mass number is the number of neutrons in the element

nuclear symbol notation

A = mass number

Z = atomic number

ionic bonds

opposite charges on two ions result in a force of attraction between the two

isotopes

different atoms of the same element with a different number of neutrons

- different mass numbers (A)

- same atomic number (Z)

properties of isotopes

similar chemical properties because they are the same element

different physical properties such as density

relative atomic mass (Ar)

average masses, taking into account the proportion of each isotope in a naturally occurring sample → weighed average mass

natural abundance (Na)

the percentage of its atoms among all atoms of the given element found on our planet

know how to calculate relative atomic mass and natural abundance

...

mass spectrometer

an instrument used to detect the relative abundance of isotopes in a sample

- results in cations (+)