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Name: Date: STUDIES IN SCIENCE MATTER & ENERGY Atomic Structure Notes The Idea of the Atom Democritus (79 AD) o Greek philosopher o “All matter is made of A tomos means Democritus thought The Development of the Modern Atomic Model John Dalton (1803) o Each element has o Atoms of JJ Thompson (1897) o Atoms are Ernst Rutherford (1905) o Gold Foil Experiment o Most of the atom is o There is a tiny bunch of Niels Bohr (1911) o Negatively charged particles o The orbiting, negatively charged particles Period: The Modern Atomic Model Subatomic particles – There are three types of subatomic particles: 1. Protons (p+) – 2. Neutrons (n0) – 3. Electrons (e-) – Nucleus – Contains the Nucleus contains _____ % of the mass of the atom Electrons Comparing Subatomic Particles Particle Location Size & Mass Charge Proton (p+) Neutron (n0) Electron (e-) Atoms are Neutral Every atom has equal numbers of _______________ and _______________ Ex. Oxygen atoms The negatives cancel out the positives o 8 protons = _____ charge o 8 electrons = _____ charge o Total charge = _____ Electrons in Energy Levels Electrons surround The number of energy levels depends on How many electrons in each level? 1st energy level holds _____ e- 2nd energy level holds up to _____ e- 3rd energy level holds up to _____ e- Atoms with 2 e- or less have _____ energy level p+ n0 Atoms with 3 to 10 e- have _____ energy levels Atoms with more than 10 e- have at least _____ energy levels Valence Electrons Valence electrons – Valence electrons determine o Will it Ex. Oxygen atoms have 8 eo _____ in the 1st level o _____ in the 2nd level o How many valence e- does an oxygen atom have? _____ Oxygen Atom The periodic table gives information about 1 atom of any element Atomic Number = o Ex. 1 oxygen atom has _____ protons and _____ electrons Mass Number = o Ex. 1 oxygen atom has _____ protons + neutrons o To figure out the number of neutrons subtract the _______________ from the _______________ o 16 – 8 = 8, so an oxygen atom has _____ neutrons