EL1 (Nuclear Fusion, Moles/Mr + Atomic Models) Flashcards
What are isotopes and relative atomic mass?
Isotopes are different forms of the same element with a different number of neutrons so a different mass number.
Relative Atomic Mass is the large number next to the chemical symbol in the periodic table, it takes into account all isotope abundances to form an average mass.
How do you calculate RAM from an intensity spectrum data table?
Add all relative intensities to find the total, divide the specific intensity by the total then multiply by 100 to find the relative abundance. Multiple the abundance with the mass number and repeat this in a sum with all the others and divide by 100.
What is the equation for moles?
Mass = Moles * Mr
Mass = Grams
Moles = Mol
Mr = gmol-1
What is the conversion of tonnes to grams?
Multiply by 10 to the power of 6 or multiply tonnes by 1000 to get Kg then repeat to find the grams.
What happens in a nuclear fusion?
2 smaller nuclei fuse to make a single larger nucleus, releasing a lot of energy. The nuclei must come close which takes a lot of energy.
What happens in a ★?
There is enough energy that 2 nuclei can collide and overcome the repulsion then fuse.
what is the empirical and molecular formula
the empirical is the simple whole number ratio of atoms present and the molecule is the actual number of atoms of each element in a molecule of the compound
describe dalton’s atomic model
atoms are indestructible and indivisible particles, all atoms of the same element are identical, compounds were formed when atoms of different elements are combined in simple ratios. 1808.
describe thomson’s plum pudding model
the atom is a positively charged ball with negatively charged particles randomly embedded into it.
explained the findings of his cathode ray experiment as the cathode ray was deflected away from negatively charged electric plate which indicates the presence of electrons. 1904.
describe rutherford’s nuclear model
most of an atom’s mass and its positive charge are concentrated in the nucleus. electrons orbit at a distance from the nucleus.
this was due to alpha particles going mostly through the gold foil which suggested a concentrated positive nucleus and the rest empty space. 1911.
describe bohr’s quantum model
electors occupy fixed energy levels around the nucleus and they can jump between these levels when emitting/absorbing energy. he was the first to introduce quantised energy levels. 1913.
describe the modern atomic model
there is a dense nucleus surrounded by clouds of electrons and orbitals which are regions of space where an electron is most likely to be found. the uncertainty principle is pivotal. 1926-present
describe the difference between the emission and absorption spectra
the emission is presented by coloured lines on a black background whereas absorption is black lines on colour. emission shows radiation emitted while absorption shows wavelengths absorbed
what is the half equation for nuclear fusion
1
1 H + 2
1 H = 3
2He + a photon
