Chemistry Unit 1 - Chapter 3 (Edexcel)

Atomic Structure and the periodic table, Hunds rule, Afbau principle etc. 

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Atomic number, relative atomic mass and isotopes.

atomic number: the number of protons in the nucleus of an atom of an element. 

r.a.m.: the weighted average mass compared to the mass of a carbon-12 atom.

isotopes --> identical chemical properties (same electron configuration.)

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How a mass spectrometer works

Bombardment  Acceleration      Deflection          Detection 

  1. sample is vaporised 
  2. vaporised sample is bombarded w/ high energy electrons
  3. accelerated by an electric field
  4. deflected by a magnetic field
  5. ions are detected and m/e ratio recorded on computer.

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Uses of mass spectrometers

1. Determining r.a.m
e.g. two isotopes of Lithium  6Li and 7Li
(m/e 6Li x % 6Li) + (m/e 7Li x % 7Li) / 100 

2. Detecting drugs in urine samples 
steroids = certain mass/charge ratio
low energy mass spectrometer detects steroid molecules

3. Pharmaceutical industry
low-energy mass spectrometer prevents decomposition of molecule ion. 
laser needle @ high electric potential
fog charged particles produced --> analyzed in mass spectrometer for m/e values 

4.Carbon-14 dating 
radioactive decay of carbon and other isotopes depending on m/e values can tell us how old an item is

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Orbits and Orbitals

*when H+ atoms are heated, electrons are promoted from ground state to excited state.

1st orbit 
1-s orbital is undivided.
 
2nd orbit
2-s orbital and 2-p orbitals (b/c of penetrating towards the nucleus the 2s is lower than 2p).

4th orbit
4-s x 1, 4-p x 3, 4-d x 5, 4-f x 7

*if there is more than 18 protons 4s becomes lower than 3d (elements beyond Ar).  

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Electron configuration rules

rule one:  one orbital can contain a maximum of two electrons with opposite spin 

rule two: Afbau principle -  electrons build succesively upwards from the lowest energy level.

rule three: Hund's rule- (seats on a bus) if there is more than one orbital in a subshell electrons are initially added so the electrons have parallel spins.

rule four: Pauli's exclusion principle -   all electrons in an atom must be in different orbitals or have different spins (minimize repulsion). 

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Trends in periodic table

Li --> Ne 
Na --> Ar

melting points increase steadily up to the 4th element; from the 5th onwards they fall dramatically.

Valency: number of electrons used by an element in bonding.

Li --> Fl, Na --> Cl (1,2,3,4,3,2,1)  

* all elements in the same period have the same number of orbitals containing electrons (quantum shells). 

 

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Blocks of the periodic table

s-block group one and two elements 
in an s-block element the last electron added goes into an s-orbital.

p-block elements in groups 3-7 and in group 0
in a p-block element the last electron added goes to a p-orbital

d-block Sc -> Zn in period 4 and elements below 
*cannot be defined in terms of energy b/c the energy level of the d-orbitals is altered by the presence of electrons in the outer s orbital. (only defined x afbau terms).
last electron added goes to a d-orbital.

f-block 14+14 elements 
14 rare earth metals (Ce --> Lu)
14 actinide elements (after actinium)
last electron added goes to an f-orbital

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Metals and their properties

across a period elements become less metallic. 
down a group elements become more metallic.

typical properties of a metal
more reactive metal + acid --> salt + H(g)
conducts electricity
malleable and ductile
forms cations in compounds (looses e- itself)
reacts with oxygen to form oxides that are bases

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Forces on the nucleus of an atom

inside nucleus - strong & weak nuclear forces ( hold the nucleus together) 
*change in nuclear structure involves LARGE amounts of energy.

Radioactivity; the longer the half life - the more dangerous

Types of radiation
 
alpha rays - 2 protons & 2 neutrons, fast moving He nuclei, stopped by few cm air or a sheet of paper.
beta rays -  fast moving electrons; stopped by a thin sheet of metal.  
gamma rays-  similar to X rays but higher frequency, therefore higher energy; stopped by a thick layer of concrete.  

breathe in/ eat material w/ a/B emitters = v. dangerous
b/c radiation will destroy cells that absorb chemical w/ isotope.
Thyroid cancer is treated with iodine-131 isotope.
gamma rays are absorbed by human tissue (causes changes to cells) cancer cells are more likley to die than normal cells so radiotherapy (controlled cobalt-60)

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Nuclei, fission and fusion

heavy nuclei are fissile (when the nucleus absorbs a neutron they become so unstable tehy break into much smaller pieces). - when this happens huge amounts of energy are released. 

U-235 --> chain reaction

Nuclear fission is environmentally friendly!
 + no greenhouse gases 
 + b/c so little uranium is used there is an unlimited supply
 + can answer threat to climate change
 - nuclear fission makes reactors and materials used to build the reactor very radioactive
 - ^ must be safely stored for 1000's of years
 - nuclear energy = nuclear weapons?
 
Fusion
nuclei of light isotopes fuse together realeasing LARGE amounts of energy 

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Forces on electrons in an atom are magnetic

Couloumb's Law

  • opposites attract; like repel 
  • the bigger the charge the stronger the force
  • the larger the sum of the radii the weaker the force

electrons are attracted to the nucleus!
*the > the atomic number the higher the form of attraction & the further away from the nucleus, the less attraction. 

nuclear charge in a group hardly varies b/c nuclear charge and the number of inner sheilding electrons increase by the same amount.

*the nuclear charge of d-block elements in the same period hardly varies.

Atomic radii decreases across a period (greater nuclear charge --> greater force of attraction on the electrons therefore they are drawn closer together).

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Size of cations and anions

Cations 
always smaller  than its neutral atom. Smaller atomic radius because:
there is one less electron shell.
fewer electrions in ion than atom so there is less electron-electron repulsion --> further decrease in radius.

*for electrons with the same electron configuration the ion w/ the greatest charge will have the smallest radius.

Anions
a negative ion is always LARGER than a neutral atom 
must gain e- to form negative ion so the forces of attraction are the same BUT there is extra repulsion due to the increased number of e- in same shell. the ion expands to balance forces of attraction and repulsion.

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Ionization energies

ionization energy: the energy needed to remove an electron from an atom, ion or molecule. 

jumps in ionization energies = evidence for existence of quantum shells.
*find group of an element looking at the first big jump in ionization energies

1st ionization energies increase across a period
why? b/c... more energy is required to remove an electron across the group b/c atomic radii decreases so electrons are packed closer to the nucleus of an atom. also nuclear charge increases so increase in attraction for highest energy electron.

Group one elements after noble gases have lower first ionization energies (than prev. elements).
b/c they are well shielded
they hae a nuclear charge close to +1
atomic radius has a greater p.p.

In period 2 the energy level of 2-p is higher than 2-s so less energy is required to remove a 2-p electron.  

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Electron Affinitiy

1st electron affinity: energy change when one electron is added to each atom in a mole of neutral gas atoms. 
  A(g) + e- --> A- (g)

Second electron affinity =  same as first electron affinity BUT applied when added to singly charged gaseous negative ions. 

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