Chapter 2 - Atoms, Ions and Compounds
Relative Atomic Mass
an electron has a mass of 1 7840
Atomic number proton number in the nucleus
Ions a positively or negatively charged atom or a covalently bonded group of atoms
polyatomic ion where the number of electrons and protons are different
Cation a positively charged ion with fewer electrons than protons
Anion a negatively charged ion with more electrons than protons
Isotope atoms of the same element with different numbers of neutrons and masses
Heavy water
heavy water controls in nuclear reactors
processes
all water molecules in heavy water contain the t isotope which is called deuterium and causes the
formula of heavy water to be Dao
the higher density of Dao gives heavy water its name
meltingpointto 0.00 and suggests that if all water was heavy water you
boilingpointtoo egg 10140 would see ice more often as the Dao heavy water
density gems yo 1.11 would freeze at a higher temperature
Carbon 12 is used in comparison with all other isotopes
we compare every atom to that of hacarbon 12 nu as the nuclear force holding together the protons
Relativentisostopiimesmatsthis
Ingmiasstheissan is'otopitionrelativetheijomasilainassopetitie
mass of an
atom of carbon 12
Relative atomicmass is the weighted atomic mean mass of an atom of an element relative to
1112th
of the mass of an atom of carbon 12
this weighted mean mass takesaccount of
the percentage abundance of each isotope
the relative isotopic mass of eachisotope
A mass spectrometer finds the percentage abundance of isotopes in a sample of element
1 The sample is vaporised and ionised by being bombarded with electrons
2 An electron is removed to form a positive ion which is accelerated in an electric field
3 The flight of the ion in the drift region depends on its mass ke 112mva
Light ion fast
4 The ions are detected on a mass spectrum as a mass to charge ratio mla
mass to charge ratio my relative mass of ion
relative charge on ion
Relative molecular mass is applied to chemicals that have a fixed number of atoms involved
Relative formula mass is applied to chemicals that use an empirical formula to represent them
, Chapter 2 - Atoms, Ions and Compounds
Binary compounds
contains two elements only
use the name of the first element but change the ending of the second element's name to ride
It 1 2 3
ammonium hydroxide phosphate
what on co pop
nitrate sulfate
no
n sulfite
no so
carbonate
hydrogen dichromate ri
Hoo Creo
manganate vis
ma
most elements that exist as small molecules exist as diatomic molecules
HaNaOzFaCla Braand la
the only other small molecules are so can be written as s and Pa
Ionic equations
In aqueous solutions ionic compounds dissociate into their ions
Only some of the ions in an ionic compound take part in the chemical reactions in aq solution
The ions thatdo nottake part are called spectator ions
An ionic equation only shows the ions particles taking part in a reaction
Molar mass
t Mi
Relative Atomic Mass
an electron has a mass of 1 7840
Atomic number proton number in the nucleus
Ions a positively or negatively charged atom or a covalently bonded group of atoms
polyatomic ion where the number of electrons and protons are different
Cation a positively charged ion with fewer electrons than protons
Anion a negatively charged ion with more electrons than protons
Isotope atoms of the same element with different numbers of neutrons and masses
Heavy water
heavy water controls in nuclear reactors
processes
all water molecules in heavy water contain the t isotope which is called deuterium and causes the
formula of heavy water to be Dao
the higher density of Dao gives heavy water its name
meltingpointto 0.00 and suggests that if all water was heavy water you
boilingpointtoo egg 10140 would see ice more often as the Dao heavy water
density gems yo 1.11 would freeze at a higher temperature
Carbon 12 is used in comparison with all other isotopes
we compare every atom to that of hacarbon 12 nu as the nuclear force holding together the protons
Relativentisostopiimesmatsthis
Ingmiasstheissan is'otopitionrelativetheijomasilainassopetitie
mass of an
atom of carbon 12
Relative atomicmass is the weighted atomic mean mass of an atom of an element relative to
1112th
of the mass of an atom of carbon 12
this weighted mean mass takesaccount of
the percentage abundance of each isotope
the relative isotopic mass of eachisotope
A mass spectrometer finds the percentage abundance of isotopes in a sample of element
1 The sample is vaporised and ionised by being bombarded with electrons
2 An electron is removed to form a positive ion which is accelerated in an electric field
3 The flight of the ion in the drift region depends on its mass ke 112mva
Light ion fast
4 The ions are detected on a mass spectrum as a mass to charge ratio mla
mass to charge ratio my relative mass of ion
relative charge on ion
Relative molecular mass is applied to chemicals that have a fixed number of atoms involved
Relative formula mass is applied to chemicals that use an empirical formula to represent them
, Chapter 2 - Atoms, Ions and Compounds
Binary compounds
contains two elements only
use the name of the first element but change the ending of the second element's name to ride
It 1 2 3
ammonium hydroxide phosphate
what on co pop
nitrate sulfate
no
n sulfite
no so
carbonate
hydrogen dichromate ri
Hoo Creo
manganate vis
ma
most elements that exist as small molecules exist as diatomic molecules
HaNaOzFaCla Braand la
the only other small molecules are so can be written as s and Pa
Ionic equations
In aqueous solutions ionic compounds dissociate into their ions
Only some of the ions in an ionic compound take part in the chemical reactions in aq solution
The ions thatdo nottake part are called spectator ions
An ionic equation only shows the ions particles taking part in a reaction
Molar mass
t Mi
