Atomic Structure and Isotopes
Ever wondered why the same element can have different weights? That's where isotopes come in - they're different forms of the same element with identical protons but varying neutrons. Think of them as siblings who share the same DNA but have different weights!
The atomic structure consists of a tiny, dense nucleus containing protons positivecharge,mass=1 and neutrons nocharge,mass=1. Electrons (negative charge, practically no mass) whizz around in electron shells at fixed distances from the nucleus. The first shell holds 2 electrons maximum, whilst the second and third shells each hold up to 8.
Since elements exist as multiple isotopes, we use relative atomic mass (Ar) instead of a fixed mass. You can calculate this using: Ar = Sum of (isotope abundance × isotope mass number) ÷ sum of abundances of all isotopes.
Quick Tip: Remember that atoms are mostly empty space - if the nucleus were a marble, the whole atom would be the size of a football stadium!
History of Atomic Models
Scientists didn't always understand atoms like we do today - it took centuries of brilliant discoveries! John Dalton started things off by imagining atoms as solid spheres, like tiny snooker balls representing different elements.
J.J. Thompson (1897) developed the 'plum pudding model', picturing atoms as balls of positive charge with electrons stuck inside like raisins in a pudding. Then Ernest Rutherford (1909) conducted his famous alpha particle scattering experiment, firing positive particles at thin metal sheets. Some bounced back, proving there's a dense, positive nucleus at the centre.
Niels Bohr refined this by suggesting electrons orbit the nucleus in fixed shells, rather than floating randomly. Finally, James Chadwick discovered neutrons in 2010, completing our modern atomic model that's still used today.
Remember: Each scientist built upon previous work - that's how scientific knowledge grows!
Chemical Equations and Conservation of Mass
Chemical equations are like recipes that show exactly what happens during reactions. You can write them as word equations methane+oxygen→carbondioxide+water or symbol equations 2Mg+O2→2MgO - both tell the same story!
The golden rule is conservation of mass - no atoms are created or destroyed during chemical reactions, they just rearrange. If you're finding that mass seems to increase or decrease, don't panic! Mass might appear to change because gases from the air join the reaction, or gas products escape.
Balancing equations is crucial and easier than it looks. You can only add numbers in front of formulas (never change the formulas themselves). Check your work by adding up the relative formula mass on both sides - they should be equal.
Pro Tip: Start balancing with the most complex molecule first, then work your way to the simpler ones!