Atomic Structure Basics
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Atomic Structure Basics
Particle key
Use this information for Questions 1–6: proton — charge +1, relative mass 1, in the nucleus; neutron — charge 0, relative mass 1, in the nucleus; electron — charge −1, relative mass about 1/1836, in the electron cloud around the nucleus.
CARD A — J. J. Thomson’s cathode-ray experiments provided evidence for the electron. His plum pudding model pictured electrons embedded in a spread-out positive charge.
CARD B — In the gold-foil experiment, most alpha particles passed through thin gold foil, while a very small number were deflected sharply or bounced back.
CARD C — Ernest Rutherford used the surprising deflections to propose that an atom has a tiny, dense, positively charged nucleus; most of the atom is empty space.
CARD D — An atom has atomic number 11 and mass number 23. For this worksheet, mass number = protons + neutrons.
Investigate and model
- Atoms are solid throughout, with no empty space.
- Most of an atom is empty space, with a small, dense, positive nucleus.
- Electrons and positive charge are mixed evenly through the atom.
- The nucleus contains all the atom’s electrons.
3 printable pages
Page 1
Page 2
Page 3
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