1. Chapters 5 sections 1, 2 & 3 6 sections 2, 3
Chemical Reactions
Chapters
5 sections 1, 2 & 3
6 sections 2, 3

2. Valence Electrons
Only electrons involved in bonding. The number of valence electrons affects whether atoms bond or not.

3. Electron Dot Diagram or Lewis Dot Structures
Just the symbol and the # of valence electrons. Li Br

6. Bonding
Chemical bonds form when a chemical reaction occurs. The bonds form when either valence electrons are transferred, taken away or shared between atoms.

7. When bonds form the atoms become more stable.
Reactivity
When bonds form the atoms become more stable.

8. Ionic Bonds
Electron Transfer: Atoms with fewer than 4 valence electrons will transfer them to an atom with four or more, causing the atoms to become stable.

10. Ions If an atoms loses an electron it becomes a positive Ion.
If it gains an electron it becomes negative.

11. Ions and Ionic Bonds
Ionic bonds form as a result of the attraction between positive and negative ions.

15. Covalent Bonds When compounds are held together by sharing electrons.
Common covalent compounds are Fat, proteins, carbs, cotton and wool.

16. Covalent Bonds cont… They have low melting points and boiling points.
Poor conductors of electricity.
Elements from same side of the table bonded together.

17. How Covalent Bonds Form
The force that holds atoms together in a covalent bond is the attraction of each atom’s nucleus for the shared pair of electrons.

20. Bonds cancel each other out  Typically covalent bonds.
Nonpolar Bonds
Bonds cancel each other out  Typically covalent bonds.

22. Polar Compounds
When electrons are shared unequally, it causes one atom to be slightly positive and the other will be slightly negative.

23. Electrons are pulled closer to Oxygen giving it a slight negative charge.
Hydrogen gets a slight positive charge because the electrons are pulled further away from hydrogen.

24. Chemical Reactions
Production of new materials that are chemically different from the beginning materials.

25. Properties and Changes in Matter
Matter can undergo both physical change and chemical change.

26. Evidence for Chemical Reactions
Color change
Precipitate
Gas production
Changes in temperature
Changes in properties
A solid that forms after a rxn.

27. Chemical Equations
A shorter, easier way of showing chemical reactions using symbols instead of words.
Chemical Formula – shows the ratio of elements in a compound
H2O
NaCl
CO2

28. Structure of an Equation
Reactants – materials you start with
Products – materials you end with

30. Reactant + Reactant  Product
H2 + O2  H2O2

31. Conservation of Mass
The amount of matter in a chemical reaction does not change, so the total mass of the reactants must equal the total mass of the products.

32. Conservation of Matter

33. Classifying Chemical Reactions
Synthesis
Decomposition
Single Replacement
Double Replacement

34. Synthesis
Two or more elements combine to form a more complex compound.
A + B  AB
Hand + kerchief  handkerchief
Example: C + 2Cl2  CCl4

35. Breaks down compounds into simpler substances. AB  A + B
Decomposition
Breaks down compounds into simpler substances.
AB  A + B
Schoolbook  school + book
Example: 2Al2O3  4Al + 3O2

36. Replacement
A reaction in which one element replaces another in a compound, or two elements in different compounds trade places
AB + C  AC + B (Single)
AB + CD  AC + BD (Double)
T.V. screen + door knob  T.V. knob + screen door
HCl + NaOH  H2O + NaCl

37. Writing and Balancing Chemical Equations
To describe a reaction accurately, a chemical equation must show the same number of each type of atom on both sides of the equation.

38. Writing and Balancing Chemical Equations
CO2
Subscript= IDENTIFIES THE NUMBER OF ATOMS IN A COMPOUND.

39. Writing and Balancing Chemical Equations cont…
Mg + O2  MgO 2 2
Coefficient is the number in front of the chemical formula that represents the # of molecules.

42. 3
H2 + N2  2
NH3 2
HgO + Cl2  2
HgCl + O2

43. Balancing Chemical Equations

44. Balancing Equations Activity
Click the Active Art button to open a browser window and access Active Art about balancing equations.

45. Balancing Chemical Equations
Magnesium (Mg) reacts with oxygen gas (O2), forming magnesium oxide (MgO). To write a balanced equation for this reaction, first write the equation using the formulas of the reactants and products, then count the number of atoms of each element.
Balancing Chemical Equations

46. Balancing Chemical Equations
Balance the equation for the reaction of sodium metal (Na) with oxygen gas (O2), forming sodium oxide (Na2O).

47. Balancing Chemical Equations:
Balance the equation for the reaction of tin (Sn) with chlorine gas (Cl2), forming tin chloride (SnCl2).

48. Controlling Rates of Reaction
Concentration: the more particles to react, the faster the reaction.

49. Controlling Rates of Reaction cont…
Surface area: the more particles that are exposed in a reaction, the faster it is.
Temperature: If temperature is increased, then the rate of reaction increases.

50. Controlling Rates of Reaction cont…
Catalyst: Helps reaction happen by lowering activation energy.
Inhibitor: Decreases rate of reaction.
Enzyme : Biological catalyst in our bodies that allow important bodily functions to occur.

51. Controlling Chemical Reactions
Every chemical reaction involves energy in one of two ways:
Exothermic: Energy is released.
Endothermic: Energy is absorbed.

52. Endothermic Reaction

53. The minimum amount of energy needed to get a reaction started.
Activation Energy
The minimum amount of energy needed to get a reaction started.

54. Acids and Bases
Acid: Tastes sour, react with metals and turns litmus paper red.
Base: Bitter, feels slippery and turns litmus paper blue.

55. pH
A scale that measures whether a chemical solution is acidic or basic.

56. pH Scale
The pH scale is from 0-14, 14 being basic, 0 being acidic and 7 being neutral.