Midterm review 2014
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Models of atom and where electrons are found
Masses of subatomic particles
How is spectra produced
Energy amounts of electron shells – further from nucleus more energy
Counting subatomic particles, definition of isotopes
Properties related to structure – O3 vs O2
Determe element from proton number
Picking elements with similar chemical properties
Electronegativity meaning and application
Definition of temperature
Sublimation as solid to gas
Identifying a homogeneous mixture
Identifying Hydrogen bonding – FON
Physical properties – MP, BP, solubility, density, magnetism
Properties of organic compounds relate to functional groups
Names of nuclear reactions – nat trans, art trans, fission, fusion
Using table N
Matching lines in a bright line spectrum mixture
Determing the charge of a particle given the amounts of subatomic particles
Periodic trends in a group or period
Excited state electron configuration vs ground state configuration
Counting electrons in a bond – 1 bond = 1 pair of electrons = 2 electrons total
Identifying ionic and molecular compounds from formulas
Converting C to Kelvin and Kelvin to C
Using q=mCΔT, q=mHf, q=mHv
Definition of element and compound
Unsaturated vs Saturated hydrocarbons
Definition of a radioisotope
Half life problems, fractions with the number of half lifes
Expaining sizes of ions compared to atoms
Addition and substitution reactions
Identifying a homologous series of hydrocarbons
Identifying bond type given a formula
Explaining stability of bonded atoms and ions compared to unbounded atoms
Distillation, evaporation, filtration as means of separating mixtures
Relating Boiling points to imf strength
Identifying a compound with ionic and covalent bonds
Explaining polarity in terms of electronegativity differences
Lewis diagrams for common molecules – water, ammonia, methane, oxygen, nitrogen
Reactant location vs product location in a chemical reaction
41. Homogeneous vs Heterogeneous mixtures
42. Using a the density formula (triangle) to solve for mass or volume
43. Writing a decay equation for alpha decay or beta decay
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Honors extension
s and p electron configurations
orbital diagrams
properties of metals vs non metals
Van der Waals forces identification
Molecular geometries of common molecules – water, carbon dioxide, ammonia, methane
Lewis dot structures
Molecular polarity
Transition metals are colorful