1. http://www.youtube.com/watch?v=x Tx_DWboEVs http://www.youtube.com/watch?v=5 IJqPU11ngY

2.  Valence electrons › electrons in the highest occupied energy level › always in the s and p orbitals  normally just a draw a circle to represent these two orbitals › determines the chemical properties of an element › usually the only electrons used in chemical bonds

4. http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_09/FG09_27-06un.JPG IB may group levels together and therefore you would see the 3d 10 before the 4s 2

7. IB uses this one

8.  electron dot structures/diagrams are used to show valence electrons › each dot around the element symbol represents a valence electron

10.  B is 1s 2 2s 2 2p 1 ; › 2 is the outermost energy level › it contains 3 valence electrons, 2 in the s and 1 in the p  Br is [Ar] 4s 2 3d 10 4p 5 How many valence electrons are present?

13. http://images.google.com/imgres?imgurl=http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/imgper/econfig.gif&imgrefurl=http://hyperphysics.phy- astr.gsu.edu/hbase/pertab/perlewis.html&h=267&w=512&sz=22&tbnid=__EXctBwlG0J:&tbnh=66&tbnw=128&hl=en&start=1&prev=/images%3Fq %3DElectron%2BDot%2BDiagrams%26svnum%3D10%26hl%3Den%26lr%3D

14.  when forming compounds, atoms tend to achieve the electron configuration of a noble gas (ns 2 np 6 ) › this means their highest energy level will be filled with 8 electrons that requires the least amount of energy › cations  atoms of metallic elements (groups 1-14) lose electrons producing cations (positive ions)  the term oxidized (O.I.L – Oxidized Is Losing) is used to say it lost an electron  example- Ca becomes Ca 2+

15. › anions  atoms of nonmetallic elements (groups 15, 16, 17) gain electrons producing anions (negative ions)  the term reduced (R.I.G.) – Reduction Is Gaining) is used to say it gained an electron  example- Cl becomes Cl 1-

16. NeN Na F Na Na + O O O 2- Mg Mg Mg 2+ CationsAnions N N 3- F F 1-

17. ...etc. As it turns out, atoms bond together for a very simple reason: atoms that have full valence shells are more chemically stable than those that don’t‘. 1+2+ 3-3+4+2-1-0

18. › some transitional metals can often form more than one cation and therefore charges may vary  some orbitals get filled but might not get a noble gas electron configuration  iron can be Fe 2+ or Fe 3+ (you don’t have to memorize this)  these always have the same charge  Al 3+, Sc 3+, Zn 2+, Cd 2+, Ag 1+ (you do have to memorize these)

19. 3+ 2+ 1+ 2+ 3+ = charge will vary except “x”

20.  usually composed of oppositely charged metallic cations and nonmetallic anions › because of the electrostatic attraction between oppositely charged particles  electro- electricity/electrons  static- non-moving (vs. current which is moving charges) + cations - anions

21.  forms a compound with overall zero charge › (+ and -) need to cancel out  referred to as formula units, not a molecule, that is a term used only for covalently bonds which is something different

22.  ions must have a difference in electronegativity of 1.7 or greater to form an ionic bond

23. 0.1 – 1.0 1.1 – 1.7 >1.7 0.0covalent, nonpolar covalent, slightly polar covalent, very polar ionic electronegativty difference probable type of bond

25. Na Cl e–e– 1) 2) 3) Na + Cl –

26.  shows number of each element in the lowest whole-number ratio of ions in the ionic compound › Na 1+ + Cl 1-  NaCl › Ca 2+ + Cl 1-  CaCl 2 › Mg 2+ + O 2-  MgO

27. Mg and N?  Mg 2+, N 3-  it takes two nitrogens to combine with three magnesiums › Mg 3 N 2 › magnesium nitride

28. Na 1+ + F 1-  NaF

31.  cations  transition metals form more than one cation with different ionic charges › charge is determined from the # of electrons lost  Fe 2+ lost two electrons (the 2 in the 4s)  Fe 3+ lost three electrons (the 2 in the 4s and 1 in the 3d) › naming  Stock system  a Roman numeral is used to show the charge of the transition metal  Fe 2+ is iron(II) and Fe +3 is iron(III)

32. › anions gain valence electrons and therefore are negatively charged  change ending to –ide for the name

33.  composed of more than one atom that form a single unit/ion with a charge › most end with -ite or –ate  the –ite ending indicates one less oxygen than the –ate ending

34. Memorize these! NO 3 1- nitrate NO 2 1- nitrite OH 1- hydroxide ClO 2 1- chlorite ClO 3 1- chlorate HCO 3 1- hydrogencarbonate (bicarbonate) SO 4 2- sulfate SO 3 2- sulfite CO 3 2- carbonate PO 4 3- phosphate NH 4 1+ ammonium

36.  Binary Compounds › cation is written first, followed by the anion with and –ide ending  Cs 2 O  cesium oxide  SrF 2  strontium fluoride  transitional metals are more difficult  CuO  copper(II) oxide  oxygen is always 2- and therefore copper will be 2+  Cu 2 O  copper(I) oxide  oxygen is 2- and therefore needed two copper atoms with 1+ charge

37. › SnF 2  ?  fluorine is always 1- and therefore tin will be 2+  tin(II) fluoride › SnS 2  ?  sulfur is always 2- and therefore tin will be 4+  tin(IV) sulfide

38.  write symbol of cation and then anion  add subscripts to balance the charges › calcium bromide  Ca 2+ and Br 1- is CaBr 2 › potassium sulfide  K +1 and S 2- is K 2 S › iron(III) oxide  Fe +3 and O 2- is Fe 2 O 3

39.  the ionic charge number of each ion is crossed over and becomes the subscript for the other ion

40.  Compounds with polyatomic ions › do same as binary compounds  use the name of the polyatomic ion with the mono atomic ion  calcium nitrate  ?  Ca is 2+ and nitrate is 1-  Ca(NO 3 ) 2  Li 2 CO 3  ?  lithium carbonate

41. aluminum chloride Al Cl 3 2. Determine number of ions 1. Write symbols of elements Final Formula x(+3) + y(-1) = 0 1 For aluminum, a 1 is multiplied times the +3 to give a +3 charge If there is only one atom the “1” is not shown If there is no Roman Numeral, you must know the oxidation number of the positive ion. +3 If there is no Roman Numeral, you must know the oxidation number of the positive ion. What is the Lowest Common Multiple “LCM” of 3 and 1. Do not worry about the sign(+/-) (Al ) x (Cl -1 ) y What is the Lowest Common Multiple “LCM” of 3 and 1. Do not worry about the sign(+/-) For chloride, a 3 is multiplied times the -1 to give a -3 charge 1(+3) + 3(-1) = 0 Remember all compounds are neutral, thus the total positive charge must equal the total negative charge Next This formula says that the +3 charge of one Al atom will cancel the-3 charge from 3 Cl atoms

42. Fe(NO 3 ) 3 Choose the correct name for the compound 1. Iron trinitrate 2. iron(I) nitrate 3. iron(III) nitrite 4. iron(III) nitrate 5. none of the above next problem Polyatomic Ions Periodic Chart

43. sodium chlorite Choose the correct formula for the compound 1. NaCl 2. NaClO 3. NaClO 2 4. Na(ClO) 2 5. none of the above next problem Prefixes Periodic Chart

44.  high melting and boiling points › takes a lot of energy to break apart the electrostatic forces between cations and anions  crystalline structure › repeating arrays of cations and ions › an ionic lattice

45.  volatility- how easily a substance turns into a gas › very low as electrostatic forces between cations and anions is very strong  electrical conductivity › can conduct electric currents when melted or dissolved in water because cations and anions are free moving instead in a lattice  solubility › will dissolve in other polar solvents such as water