Topic 1:

Periodic table elements:

1. H - Hydrogen

2. He - Helium

3. Li - Lithium

4. Be - Beryllium

5. B - Boron

6. C - Carbon

7. N - Nitrogen

8. O - Oxygen

9. F - Fluorine

10. Ne - Neon

11. Na - Sodium

12. Mg - Magnesium

13. Al - Aluminum, Aluminium

14. Si - Silicon

15. P - Phosphorus

16. S - Sulfur

17. Cl - Chlorine

18. Ar - Argon

19. K - Potassium

20. Ca - Calcium

21. Sc - Scandium

22. Ti - Titanium

23. V - Vanadium

24. Cr - Chromium

25. Mn - Manganese

26. Fe - Iron

27. Co - Cobalt

28. Ni - Nickel

29. Cu - Copper

30. Zn - Zinc

31. Ga - Gallium

32. Ge - Germanium

33. As - Arsenic

34. Se - Selenium

35. Br - Bromine

36. Kr - Krypton

37. Rb - Rubidium

38. Sr - Strontium

39. Y - Yttrium

40. Zr - Zirconium

41. Nb - Niobium

42. Mo - Molybdenum

43. Tc - Technetium

44. Ru - Ruthenium

45. Rh - Rhodium

46. Pd - Palladium

47. Ag - Silver

48. Cd - Cadmium

49. In - Indium

50. Sn - Tin

51. Sb - Antimony

52. Te - Tellurium

53. I - Iodine

54. Xe - Xenon

Units:

1in= 2.54 cm

1cm= 10^{-2 meters}

^1mg= 10^{-3 gram}

^{1kg= 1,000 grams}

Topic 2:

• Atomic #=#of protons

• #of protons=#of electrons

• Charged Atom=Ion

• Ionic= metal+nonmetal

  → TRANSFER of electrons between the atoms(IONS)

• Covalent= nonmetal+ nonmetal

  → SHARING of electrons between nonmetal and nonmetal atoms

• Isotopes: elements w/diff # of neutrons

• d4 atoms: Cr & Mo have s1d5 electron configuration

• All of the d9 atoms have an s1d10 electron configuration

Topic 3:

• ALL bonding is based on electrostatic interactions between the negatively charged electrons of one atom & the positively charged nucleus of the other

Compounds can be divided into 2 groups: Binary vs. non binary

Binary: Composed of 2 and ONLY 2 different types of atoms

Not Binary: Composed of more than 2 types of atoms

Ions: when atoms gain or lose electrons they form ions

→lose electrons= cations(positive)

• usually on the left side of the periodic table

→gain electrons=anions (negative)

• usually on the right side of the periodic table

Naming Compounds:

Prefixes for COVALENT compounds:

• Mono-1

• di-2

• tri-3

• tetra-4

• penta-5

• hexa-6

• hepta-7

• octa-8

• nona-9

• deca-10

  prefix→ name of 1st element→ prefix→ name of 2nd element + -ide

  Naming IONIC compounds:

  IF the cation is a single metal + nonmetal that forms only one type of ion (like sodium Na+ or Ca² +) you use: Example: NaCl → NaCl is named sodium chloride.

  IF the cation can form multiple charges (like iron, copper, etc.), specify the charge using Roman numerals.Example: FeCl2

• FeCl2​ is named iron(II) chloride (since iron has a +2 charge).

• For single nonmetals: name of metal + name of nonmetal & change the ending to -ide

• For polyatomic ions, use the name of the ion as is.

Topic 4:

• Electronegativity increases as you go up and across the periodic table

• Non-polar= similar electronegativities

  → ex: F-F

  Since both atoms have the same electronegativity, there is no difference in electron density.

• Polar=large electronegativity difference

  → ex: Ge-F

Bonding:

• Carbon will always want to make 4 bonds

• Nitrogen will always want to make 3 bonds

• Oxygen will always want to make 2 bonds

• Halogens and Hydrogen will always want to make 1 bond

7 diatomic molecules: H2, N2, 02, F2, CI2, Br2, I2

→start w/ H, find element 7 on the P.T. to find the other 6

-draw a 7 to find the other 6 elements aside from H

Topic 5:

Kinetic energy: due to MOTION (KE= ½ mv²)

Potential energy: due to POSITION (PE=mgh)

Combustion reactions are exothermic: Combustion→ surroundings get hot→ heat is absorbed

ΔE=ΔH

Δ E= change in internal energy of the system

ΔH= change in enthalpy of the system

Exothermic: Δ H= — (negative)

→ heat is being released because it’s coming down

ΔH< 0

Endothermic:

ΔH= + (positive)

→ heat is higher because it’s coming in

heat is abosrbed

ΔH >0