1. Language of Chemistry

2. Molecules
Monatomic = 1 atom

3. Molecules
Molecule =
2 or more nonmetal
atoms acting as a unit

4. Diatomic = molecules of 2 of the same atoms

5. Triatomic = 3 of the same atoms (O3)
Molecules
Triatomic = 3 of the same atoms (O3)

6. Molecular Compounds Composed of molecules
Low melting and boiling points
Do not conduct electricity in H2O
Gases or liquids at room temp
2 or more different nonmetals

7. Ions
Atoms or groups of atoms with a positive or negative charge
Form when atoms lose or gain electrons

9. Cations
Any atom or group of atoms with a positive charge
It has lost electrons
Metals

10. Cations

11. Cations
Written with a symbol and charge; Na+
Named by element; sodium ion

12. Atoms or groups of atoms with a negative charge Gained electrons
Anion
Atoms or groups of atoms with a negative charge
Gained electrons
Nonmetals

13. Anion

14. Written with symbol and charge; Cl-
Anion
Written with symbol and charge; Cl-
Named by elements name plus –ide; chloride ion

15. Ionic Compounds
Composed of ions; cations and anions; metal and nonmetal
Solid crystals at room temperature
High mp/ bp
Neutral
Na+ + Cl-  NaCl
Conduct electricity
In H2O

16. Chemical Formulas
Shows the kinds and numbers of atoms in the smallest representative unit of a substance
Symbols show the
type of atom
Subscripts show
how many atoms

17. Summary What does it mean to say an atom is neutral?
What happens to the charge of an atom if an electron is removed? Gained?
What is a molecule?
What is the difference between molecular and ionic compounds?

18. Dalton’s Laws

19. Law of Conservation of Mass
Atoms are neither created nor destroyed

20. Law of Definite Proportions
In any sample size of a compound, the mass of the elements are always in the same proportions

21. Law of Definite Proportions
If you take 100g of MgS, you always obtain a ratio of 43.13g Mg / 56.87g S or :1.

22. Law of Multiple Proportions
When any two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in small whole number ratios

23. Law of Multiple Proportions
A + B  C
A + B  D
A in C/ A in D = 5/10 = 1/2

24. Dalton’s Laws
Which law is illustrated below?
“In every sample of carbon monoxide, the mass ratio of C:O is 3:4”

25. Dalton’s Laws
Which law is illustrated below?
“When C and O form CO and CO2, the different masses of C that combine with the same mass of O is in a ratio of 2:1”

26. Monatomic ions
ions made of one type of atom

27. Monatomic ions
Metallic elements tend to lose electrons to form cations
For group A metals, the charge equals the group #

28. Monatomic ions
Nonmetallic elements tend to gain electrons to form anions
For group A nonmetals, the charge equals the group # - 8

29. Monatomic ions Hydrogen is + or - Carbon makes +/- 4
group 8 usually do not make ions

30. Monatomic ions

31. Monatomic ions
For all other metals (group B metals, others) there is often more than one possible charge

32. Monatomic ions
For group B and other metals, the classical system used to be used for naming

33. Monatomic ions
Now the stock system is used and a roman numeral is used to represent the charge or the charge can be determined by the formula

34. Monatomic ions
Exceptions:
Zn2+ ,Cd2+, and Ag+

35. Monatomic ions

36. Polyatomic ions
tightly bound groups of atoms that act as a unit and carry a charge

37. Summary What type of ions form from metals? Nonmetals?
What is the difference between Cu ,Cu+, and Cu2+?
What is an ionic compound?

38. Formulas for Binary Ionic Compounds
The cation and anion must balance each other out by lowest whole number ratios
Ex: magnesium nitride

39. Names for Binary Ionic Compounds
Name the cation and the anion
If it is a metal with more than one charge, don’t forget the roman numeral

40. Ternary Ionic Compounds
Same rules as binary ionic compounds except you have a polyatomic ion

41. Molecular Compounds
Prefix system used

42. Molecular Compounds
Prefix system used

43. Molecular Compounds Prefix1element1 prefix2element2 + -ide
Except mono is never used on element1

44. Acids

45. Acids
6 common acids names and formulas to know

46. Acids HCl hydrochloric acid HNO3 nitric acid H2SO4 sulfuric acid
H2CO3 carbonic acid
H3PO4 phosphoric acid
HC2H3O2 acetic acid