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ELECTRON CONFIGURATIONS

ELECTRON CONFIGURATIONS. Sulfur 1s 2 2s 2 sp 6 3s 2 3p 4 Chromium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 Lead (give the noble gas configuration) [Xe]6s 2 4f 14 5d 10 6p 2 Barium [Xe]6s 2. Name the element…. 2p 3 nitrogen 4s 2 calcium 4d 6 rhodium 5 p 6 xenon.

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ELECTRON CONFIGURATIONS

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  1. ELECTRON CONFIGURATIONS • Sulfur • 1s22s2sp63s23p4 • Chromium • 1s22s22p63s23p64s23d4 • Lead (give the noble gas configuration) • [Xe]6s24f145d106p2 • Barium • [Xe]6s2

  2. Name the element… • 2p3 • nitrogen • 4s2 • calcium • 4d6 • rhodium • 5 p6 • xenon

  3. Identify As Either Ionic Or Covalent • potassium hydroxide • ionic • Pb3S2 • ionic • Nitrogen dioxide • Covalent • Carbon tetrachloride • covalent • ammonium sulfate • ionic • Carbon monoxide • covalent • Magnesium chloride • ionic • Sulfur dioxide • covalent • Dihydrogen dioxide • covalent

  4. Give the oxidation numbers So, how many protons and electrons? Oxygen 8 p, 10 e Calcium 12 p, 10 e Aluminum 13 p, 10 e Chlorine 17p 18 e • Oxygen • -2 • Calcium • +2 • Aluminum • +3 • Chlorine • -1

  5. Writing Formulas And Naming Ionic Bonds • KOH  potassium hydroxide • (NH4)2S ammonium sulfide • KCl  potassium chloride Li2S • Lithium sulfide • Calcium iodide • CaI2 • Ammonium hydroxide • NH4OH • Aluminum chlorate • Al(ClO3)3 • Lead(II) sulfide • Pb3S2 • Magnesium hydroxide • Mg(OH)2

  6. Writing formulas andnaming covalent bonds • CO2 • Carbon dioxide • CH4 • Carbon tetrahydride • S3O • Trisulfur monoxide • Sulfur trioxide • SiO3 • Dinitrogen trisulfide • N2S3 • P3N2 • Triphosphorus dinitride

  7. Complete The Blanks • In an ionic bond, electrons are ____. • Transferred • An ionic bond is always between a__ and a ___. • Metal, nonmetal • In a covalent bond, electrons are ____. • Shared • A covalent bond is always between 2 ____. • Nonmetals • When you name a covalently bonded molecule, you use ____. • prefixes

  8. Given the two chemical equations, circle the one that is balanced. a. 2Na + Cl2 → 2NaCl b. 2Na + 2Cl2 → 2NaCl (a is balanced) a. C3H8 + 5O2 →3CO2 + 4H2O b. 2C3H8 + 5O2 → 3CO2+ 8H2O (a is balanced) a. 2NH3 + 5O2 → 2NO + 3H2O b. 4NH3 + 5O2 →4NO + 6H2O (b is balanced)

  9. Balance the equations ____ Al + ____Fe3N2 → ___ AlN + ____ F 2,1,2,3 ____Ag2S →____Ag + ____ S8 8, 16,1 ____ ZnS + ____AlP → ____Zn3P2 + ____Al2S3 3, 2,1,1 ____ Cu2O + ____ C → ____ Cu + ____ CO2 2,1,4,1

  10. The oxidation number of calcium is _____. • +2 • Is calcium a metal or nonmetal? • Metal • Because it forms a positive ion, it is called a __. • cation • The oxidation number for chlorine is ____. • -1 • Is it a metal or nonmetal? • Nonmetal • Because it forms a negative ion, it is called an ____. • anion

  11. Definitions… • The amount of matter in a substance? • Matter • The amount of space an object takes up is • Volume • A ratio that compares the mass of an object to its volume? • Density • If you cut a piece of gold in half, it’s volume and mass change. Does it’s density? • No- density is an intrinsic property

  12. Another half-life problem • What is the half-life of an isotope if 125 g of a 1000 g sample of the isotope remains after 3.0 years? • To go from 1000 g to 125 g means that 3 half lives have passed. The half life must be 1 year. 1 year (1 half-life= 500 g) 2 year (2 half-lives = 250 g) 3 years (3 half-lives = 125 g left)

  13. Identify The Reactant(s) In The Equation • SnO2 + 2 H2 → Sn + 2 H2O • SnO2 + 2 H2 • What are Sn + 2 H2O? • The products

  14. SOLID, LIQUID OR GAS? • Fastest moving particles • Gas • Particles are tightly packed together • Solid • The state of matter with an indefinite shape and definite volume • Liquid • Particles are in constant motion • gas

  15. The state of matter with an indefinite shape and indefinite volume • gas • The state of matter with a definite shape and definite volume • Solid • List the 3 types of nuclear radiation in order from most massive to least massive. • Alpha, beta, gamma

  16. What type of nuclear reaction occurs in the sun? • Fusion • What type of nuclear reaction produces electricity? • Fission • When a chemical reaction occurs, the mass of the reactants ___ the mass of the products. • Equals • If the mass of the reactants is 10 g, then the mass of the products is ___ g. • 10 • Which law explains why these must be equal? • Law of Conservation of Mass

  17. SCIENTISTS… • Bohr Bohr Model • Mendeleev Organized Periodic Table by atomic number • Rutherford The atom is mostly empty space • JJ Thompson Plum pudding model Democritus First came up with the idea that all matter is made of atoms, but that it cannot be broken down any further

  18. Review all the worksheets!!! • Good luck!

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