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1. Probably not, its water (H2O)2. SATP (standard ambient temperature & pressure: 25C, 100 kPa), STP (standard T&P: 0C, 101.325 kPa)Element: cannot be broken down by chemical means (all same type of atom). Compound: broken down by chemical means (two or more different types of atoms)Group: vertical column on periodic tablePeriod: horizontal (Ieft/right) rowMetal: element to the left of the staircase line. They tend to be solids at SATP, and conduct.Nonmetals: to the right of staricase line. Tend to be gases, non-conductors, and brittle as solid3. I - Alkali metals, II - Alkaline earth metals, VII - halogens, VIII - noble gasses, middle - transition elements/metals, bottom - inner transition elements (lanthanides, actinides)4. Democritus: first to propose atom and the void based purely on logicAristotle: his ideas were also based on thought. He was way off, but his ideas persisted for 2000 yearsDalton: 1st to investigate structure of matter by experiment. His five postulates included the idea that all matter is made of atoms, each element has its own type of atoms, and atoms are rearranged in chemical reactionsThompson: with the identification of electrons he proposed that negative electrons existed in a positive dough.Rutherford: famous gold foil experiment proved that an atom was mostly empty, with a dense positive nucleus orbited by electronsBohr: added to Rutherfords model the idea of “shells”. Evidence includes line spectra.5. Mendeleev ordered table according to atomic mass (today its done by atomic number)6. Atomic number = # of protonsMass number = # or protons + # of neutronsThey are averages (of different isotopes)7. 20, 37, 17, 178. Size increases down a group (more shells), it decreases left to right as the # of protons increases, pulling outer electrons closer9. Ionization energy: energy required to remove outer electron. It is high when atoms are small (high in group) with lots of protons (right in period). Electron affinity: the energy change when an electron adds to an atom. It is also high when atoms are small (high in group) with lots of protons (right in period).Electronegativity: ability of atoms, when bonded, to attract electrons (essentially a numerical value for electron affinity). It follows the same trend as electron affinity for the same reason10. Ions: O2 Al3+ Na+ I no ionValence: 2 3 1 1 n/a11.Covalent = a, d Ionic = b, c, e12.Lewis:OAlNaIXe3Mg + 2P Mg32+P23 P 23Mg32+PMgPMgMg1e-2e-15p+16n05e- 8e- 2e-12p+12n0 2e- 8e-2e-1e-12p+12n0 2e- 8e-2e-15p+16n05e- 8e- 2e-12p+12n0 2e- 8e-2e-2e-15p+16n08e- 8e- 2e-15p+16n08e- 8e- 2e-12p+12n02e- 8e-12p+12n02e- 8e-12p+12n02e- 8e-13. ClCl Cl 2 Ca2+OHPHHHPHHCl O ClNNNN14. Ionic: high melting/boiling points, soluble in polar solvents, conducts when dissolved in water but not as solid, brittle.Covalent: low melting/boiling points, soluble in non-polar solvents, doesnt conduct, soft.These differences are caused by the different strength of intermolecular forces in ionic versus covalent molecules.15.In order from low to high boiling points: H2: covalent (EN=0), CH4: covalent (0.4), H2O: polar covalent (1.4), LiF: ionic (3.0)16.HCl, Na2O, PCl3, Al2O3, MgO17.A) copper(I) iodide, b) HI(aq), c) dinitrogen tetroxide, d) phosphorous acid, e) PBr5, f) Fe2O3, g) K3N, h) H2C2O4, i) dichlorine heptoxide, j) hydrofluoric acid, k) nickel (II) sulfate hexahydrate, l) hydrogen bustion: AB + oxygen oxides of A & Bsynthesis: A+BC, decomposition: AB A + Bsingle displacement: A + BC AC + Bdouble displacement: AB + CD AD + CBa) S, b) DD, c) S, d) D, e) SD, f) DD, g) S, h) SD19. a) Ca + CuSO4 Cu + CaSO4b) FeCl2 + Ag NRc) H2O + Ca H2 + Ca(OH)2d) Al + H2SO4 H2 + Al2(SO4)3e) Na + Ni3(PO4)2 Ni + Na3PO4f) Au + HCl NRFor more lessons, visit
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