TOPIC 1 - ATOMIC STRUC AND PERIODIC TABLE

. only show show substances that are involved in the reaction basically formation of ionic compounds from ions(aq). . First split main eq into ions composed of and identify the ionic compound formed and write ionic eq. The rest is spectator ions (do not change and not involved in reaction.)

. made of subatomic particles - protons and neutrons in the nucleus and electrons in the electronic shells surrounding the nucleus. . protons relative mass = 1 and charge +1 . neutron r.m = 1 and charge = 0 . electrons r.m= 1/1840 and charge = -1 . Same e- config= same chemical reactions/ properties 1800’s John Dalton’s atomic theory: - all atoms of an element are identical and atoms can not be divided. JJ Thompsons’s theory: - Atoms contain electrons and overall charge of an atom is neutral due to Plum pudding model _ e- scattered throughout + charge Ernest Rutherford Nuclear model - gold foil experiment charged + alpha particles at gold foil some deflected back shows + charge of atom and most of its mass is concentrated in nucleus at center and e- orbit around. Most of atoms volume is the space. Proved balance of charge. Niels Bohr Planetary Model Orbiting e- attracted to opposite charged nucleus and occupy in fixed energy levels. James Chadwick - Neutrons

Number of protons in the nucleus of an atom of that element = no. of e-

Sum of the protons and number of neutrons in the nucleus of that atom

Atoms of the same element with the same amount of protons and electrons but different amount of neutrons

The weighted mean mass of an atom of an element compared to 1/12 the mass of an atom of carbon-12 Calc by %abundance times by relative mass of isotope and add all isotopes divide by 100. Make sure all abundance adds up to 100

The mass of an isotope compared to 1/12th of the mass of an atom of the isotope Carbon-12

mass of molecules and compounds and relative abundances of diff. isotopes and predict struc of more complex molecules.

Peak with the HIGHEST m/z ratio in the mass spectrum. Determines an exact Relative Molecular Mass. The strongest peak furthest to the right

For compounds with giant structures Calc by the elements Mr times by no of atoms and add all together

coz struc is infinitive and there are number atoms of an element - too many to count.

The number of isotopes

Ionisation - vaporizes sample and high volt applied/high energy e- and e= lost and ion formations. Acceleration - + ions accelerated by electric field in uniform speed and smaller ions ( low m/z) have a greater speed than larger ones Deflection - In magnetic field the lighter they are, the more they are deflected. greater charge more deflected, shorter time to hit detector. Detection - ions create a current and time taken is recorded. Greater abundance of isotopes = larger current. Greater no. particles landing at a single point, greater e- current and larger the peak. The amount of deflection, therefore the mass of the atom.

• It means no interference from atoms or molecules in air - Molecular fragments could not exist otherwise

a region within an atom that can hold up to two electrons with opposite spins

energy levels of an electron - lowest inside.

e- always fll the lowest energy orbital first.

electrons will occupy the orbits singly before pairing up

Two electrons cannot occupy the same orbital unless they have opposite spins (↑↓)

s orbital - spherical hold 2e- p orbital - dumbbell/hourglass shape, all axis/oreinatations smaller x,y,z energy level symbols. hold 6 e- d hold 10e-. 4s goes FIRST then 3d as it has a lower energy than 3d.

Regular repeating pattern of atomic, physical and chemical properties with increasing atomic number

Lost e- to the right X(g)➝X+(g) + e- The energy required to remove an electron from each atom in ONE MOLE of atoms in the GASEOUS state to form ONE MOLE of Gaseous 1+ IONS

X+(g)➝X2+(g) + e- The energy required to remove an electron from each +1 charged positive ion in ONE MOLE of positive ions in the GASEOUS state

• proton number/ nuclear charge • electron shielding • electron orbitals (subshells) DOWN THE GP - FRIST IE DECRESEASES nuclear charge, e- shielding, atomic radius increases so nuclear attraction btw outershell e- DECREASES. ACROSS THE PERIOD, IE INCREASES: nuclear charge increases, atomic radius decreases as the e- shielding stays the same so the nuclear attraction on outershell e- INCREASES. THEREFORE MORE ENERGY IS NEEDED to remove it.