Atomic structure Flashcards
What are the subatomic particals and where are they?
proton–charge= + mass=1 found in nucleus
neutron– charge=neutral mass=1 found in nucleus
electron–charge=- mass=1/2000 orbit in shell around nucleus
what are atoms made up of?
nucleus-a very dense and small,where the protons and neutrons are
shell-where the electrons orbit the atom
most of the atom is empty space
They are also neutral so have the same number of protons and electrons
What does the number of protons tell us
The number of electeons and also what element it is
what does the atomic number tell us?
it is equal to the number protons in the nucleus of an atom of that element, also tells which element it is
what does the atomic mass number tell us?
it is equal to the mass number of protons+ the number of neutrons in the nucleus ( it tells us the mass of 1 atom of that element)
to calc no of neutrons do mass number- atomic number
Isotope definition
isotopes are atoms of the same element ( same number of protons and electrons) with different number of neutrons
differences and similarities between isotopic atoms of the same element
different masses
different numbers of neutrons
different physical properties (as this is decided by neutrons)
same number of protons and electrons
same chemical properties( as this is determined by electron)
what is a cation
A positively charged ion
what is a anion
A negatively charged ion
how are ions formed
Atoms gain or lose electrons to form ions, by transferring or sharing them
if they gain electrons they become negative ion (non metals do this)
if they lose electrons they form positive ions (metals do this and Roman numerals are used to show positive charges sometimes)
what is an ion
A charge partical
Which subshells does each shell contain?
Sub shells
shell 1 = 1s sub-shell
shell 2 = 2s sub-shell + 2p sub-shell
shell 3 = 3s sub-shell + 3p sub-shell + 3d sub-shell
shell 4 = 4s sub-shell + 4p sub-shell + 4d sub-shell + 4f sub-shell
what are subshells made up of
sub shells are made up of orbitals these are regions of space in an atom that can hold up to 2 electrons with opposite spins
there are 4 types S P D and F
What are the s subshells made up of
They are made up of 1 s orbital
s orbitals are spherical in shape and can hold 2 electrons with opposite spins
What are p sub shells made up of
3 P orbitals py pz and px
each P orbital has a dumbell shape
they each hold 2 electrons meaning a P sub shell can hold up too 6 electrons
electrons constantly move around the nucleus within this regin
What are d sub shells made up of?
5 d orbitals
each of them can hold 2 electrons with opposite spins so all together a d sub shell can hold up too 10 electrons
What are F sub shells made up of
7 F orbitals
each one can hold up to 2 electrons with opposite spins so a F sub shell can hold up too 14 electrons
how many electrons can each shell hold
Shell 1- 1s sub shell can hold 2, so shell 1 can hold 2 electrons overall
Shell 2- 2s sub shellcan hold 2 and a 2p subshell which can hold 6, so shell 2 can hold up to 8 overall
Shell 3- 3s can hold 2 3p can hold 6 3d can hold 10, so 18 overall
shell 4- 4s can hold 2 4p can hold 6 4d can hold 10 4f can hold 14, so 32 overall
how is the electron configuration of an atom shown ?
it is show by the subshells for example sodium ( atomic number of 11) is
1s² 2s² 2p⁶ 3s¹
This shows which subshells in each shell contain the electrons for example the S subshell in the 3rd shell and also how many they contain through the small
numbers for example 3s¹ means it contains 1 electron
Relative isotopic Mass defintion
The relative isotopic Mass is the Mass of an atom of an isotope compared with 1/12th of the Mass of carbon-12
Relative atomic mass definition
is the weighted mean mass of an atom of an element compared with 1/12th of an atom of carbon-12
Takes into account the percentage abundance of each isotope
and relative Mass of each isotope
what is mass spectrometry used for?
To determine info about isotopes including their mass number and relative abundance
Calc relative atomic mass
(atomic mass×percentage abundance)+( atomic mass × percentage abundance) / 100
Atomic orbital definition
A region within an atom, around the nucleus, that can hold up to two electron, with opposite spins
Shell defention+ properties
A group of atomic orbitals with the same principle quantum number
the shell closest to the nucleus has the lowest enrgy
What are sub shells
They are a group of the same type of atomic orbitals within a shell
Order of filling of the orbitals
Lowest energy fills first (closest to the nucleus)
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶…
4s² fills first as it has a lower energy than 3d¹⁰ it also loses electrons first when they become an ion
Transition elements info
A transition element is a d-block element that forms and ion with an incomplete d sub- shell
they lose their 4s electrons first when forming positive ions
Cr and Cu also only fill 4s¹ before moving onto the 3d subshell as a exception to the 4s²
