1.3 Flashcards
define atomic mass
the amount of protons and neutrons in an element
define relative atomic mass
the average mass of an element taking into consideration the presence of isotopes which have different atomic masses relative to carbon 12
define isotope
different form of the same element which share the same number of protons but a different atomic mass
what does the relative atomic mass depend on
the number of isotopes present and the percentage abundance of it
what makes an element neutral
an equal number of protons and neutrons
what happens if an ion has more protons that electrons
it has a positive charge
what happens if an ion has more electrons than protons
it has a negative charge
what is the equation for working out relative atomic mass
(mass of isotope x percentage abundance) + (mass of isotope x percentage abundance) / total abundance
what is the molecular/formula mass
the average sum of the relative atomic masses of the elements present in a chemical formula
when is it called the molecular mass
what the elements involved were bonded covalently
define covalent
bonding between two non-metals
when is it called the formula mass
when the elements involved were bonded ionically
define ionic bonding
bonding between a metal and a non-metal
how to calculate empirical formula
mass
ar
mass/ar to get moles
divide all by smallest number
round up if necessary
define empirical formula
a chemical compound of a formula in its simplest form
