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Unit 3 Atomic Structure and the Periodic Table Vocabulary to know proton neutron electron nucleus atom atomic mass mass number atomic number isotope ion charge element period group alkali metal alkaline earth metal transition metal representative metal nonmetal halogen noble gas atomic radii ionic radii isoelectronic series ionization energy electronegativity s orbital p orbital d orbital f orbital s block p block d block f block quantum numbers principle quantum number angular momentum quantum number magnetic quantum number spin quantum number orbital energy Aufbau Principle Hund’s rule Pauli Exclusion Principle Electron configuration People: Democritis Boyle Lavoisier Dalton Thomson Millikan Rutherford Bohr - Chadwick Schrӧdinger Heisenberg deBroglie Mendeleev - first person to propose the existence of atoms Started scientific revolution with his Skeptical Chemist publication Demonstrated Law of Conservation of Mass, Discovered Oxygen First atomic theory based on experimental evidence, 5 parts, atoms are spheres. Discovered electron using the Cathode Ray Tube; Plum Pudding model of atom, measured charge to mass ratio of electron Oil drop experiment allowed accurate measure of electron mass and charge Used gold foil experiment to discover nucleus of the atom; Discovered protons; Nuclear model of atom Explained optical spectra using the planetary Bohr Model of atom; First quantized model Uses orbits. Discovered neutrons Provided mathematical description of quantum mechanical orbitals Proposed the Uncertainty principle – the electron is only probably located in orbital Proposed electrons and other particles have wavelengths Developed the first periodic table; Predicted the discovery of Gallium Atomic models Atomic theory - Know 4 parts Plum Pudding model - Be able to describe parts of atom including what parts are +/Nuclear atom first model that is still relevant; we use the nuclear model; know 3 parts; know features of subatomic particles, know where subatomic particles are located, their charges, relative masses, and symbols Bohr model Basically the nuclear model + electrons organized into quantized circular orbits Quantum mechanics Currently accepted atomic theory; Basically the nuclear model + electrons organized into quantized regions of space where you are likely to find an electron called orbitals, HIGHLY confirmed theory. 100 yrs old, and still best Experiments: Cathode Ray Tube - Millikan Oil Drop- Gold Foil Experiment Optical Spectra - Vacuum tube with an electrical charge creates a stream of negatively charged particles that respond to an applied magnetic field. – used by Thomson to discover electron, first subatomic particle and measure its charge/mass ratio, led to Plum pudding model – used in CRT televisions Tiny oil drop exposed to radiation to give it a charge. Size of charge measured by balancing oil drop in an electric field. Determines charge on an electron, and therefore mass of electron. Radioactive source of heavy positively charged alpha particles shot at very thin gold foil. Most go through, but some are highly deflected. When neon light is passed through a prism, you get lines. Explained by electrons being excited from one orbit to a higher orbit by absorbing a photon of a certain wavelength, and then emitting that same wavelength when the electron drops back down. Explained by quantized orbits of the Bohr model. Memory items Particle Symbol Location Charge Relative Mass 1 Actual Mass (amu) Electron e Outside nucleus -1 Proton p nucleus +1 1 1.0073 Neutron n nucleus 0 1 1.0087 Common labels 1840 ~0 0.00055 Quantum Number Name Allowed Values Determines Specifies n Principle 1, 2, 3, 4….. Size and Energy Shell 1, 2, 3,… (Period #) Angular Momentum 0, 1, 2… (only up to n-1) Shape Subshell s, p, d, f ml Magnetic ml Orientation Orbital subscripts: x, y, z, xz, yz, z2… ms Spin +½ or -½ Spin Electron Up ↑, Down ↓ States of the elements ( 2 liquid, 11 gas, all others solid) Molecular elements (9, including 7 diatomic elements) Filling order of atomic subshells and the maximum number of electrons for each subshell Skills Calculate using percent composition: % = part/whole x 100 Calculate using conservation of mass Determine average atomic mass from natural isotopic abundances and masses Determine group #, period #, group name for an element Rank elements based on atomic size, ionic size, ionization energy or electronegativity State orbitals described by a given set of quantum numbers Count electrons within shells, subshells or orbital Write an electron configuration Other Review Resources Class powerpoints (posted online) Homework worksheets Personal Class notes Review worksheet (Hint: The test will look VERY much like the Review worksheet) After school and/or lunch meeting with teacher 20 pt Vocab quiz on Friday. Test on Monday Unit 3 Test Description: 20 x 1 pts 10 x 2 pts 9 pts 10 x 1 pt 6 x 2 pts 3 x 4 pts 1 x 5 pts 1 x 5 pts 1 x 7 pts People, Experiments, Theories, Vocabulary (like quiz) Quantum numbers, shell, shapes, electron counting, etc… Subatomic particle memory items Element designations from periodic table Periodic trend decision with justification Electron configurations Percent composition calculation Conservation of Mass problem Atomic mass calculation There will be two parallel versions of the test. You will not be allowed to sit next to someone with the same version. Testing folder crosses will be positioned around the center of each table to block view of same version on opposite side of table. BEWARE: YOU WILL NOT BE ALLOWED TO USE YOUR PHONE AS A CALCULATOR AND THERE ARE LIMITED CALCULATORS AVAILABLE TO BORROW. BRING YOUR OWN CALCULATOR. You will be asked to place your phone in your backpack at your feet or in a box on the front bench. There shall be nothing on the tables beside the test, your calculator, the vocabulary word bank, a periodic table, and a writing implement.