1. Atoms, Elements and How They Behave
Basic Chemistry
Atoms, Elements and How They Behave

2. _______ ___________  ____________ ______  ________  _______ 
Start Small End Big
_______ ___________ 
____________ ______ 
________  _______ 
_______________ 
___________

3. ATOM:
______________ of an element that still has the __________ of that element. Made up of:
- ____________________, p+, Charge of __
- _________, e-, charge of __
- _________, n, charge of ___

4. Structure of an Atom e
Orbit: N P
Nucleus: P N e

5. Orbits spin and rotate in three dimensions.
Structure of an Atom P N e
Orbits spin and rotate in three dimensions.

6. Orbits spin and rotate in three dimensions.
Structure of an Atom
Orbits spin and rotate in three dimensions.

7. Each Orbit is a ______ _______from the nucleus.
Structure of an Atom P N e
Each Orbit is a ______ _______from the nucleus.

8. Structure of an Atom P N e

9. Structure of an Atom

11. Each type of atom has its own number of ________
Structure of an Atom - e
Each type of atom has its own number of ________ N + P + P N - - e

12. The different combination of p+, n and e- make each element _______
Structure of an Atom - e
The different combination of p+, n and e- make each element _______ N + P + P N - - e

13. Structure of an Atom
Normally, all the “+” of the protons and the “-” from the electrons balance out and the overall charge of the atom is zero. We call this a ________ atom.

14. What if an atom loses an electron?
Structure of an Atom -
What if an atom loses an electron? e e N N + P P + P P N N - e -

15. Structure of an Atom What if an atom gains an electron? - + + - - e NP + P N - e - - - e

16. Any charged atom is called an ___
Structure of an Atom
Any charged atom is called an ___
- Positive ions are called _______
- Negative ions are called ______

17. The Periodic Chart Atomic number _____ __________________
Atomic Mass _______
__________________
Assume _______= ________
(except ions)

18. Atomic Mass = Protons + Neutrons
Why don’t the electrons figure in?

19. Drawing Atoms: Each orbit can hold a maximum number of electrons.
You must fill the inner orbits before adding electrons to the outer orbits.

20. Examples e e 12 Mg 24 e P N

21. Examples
Sodium: 11 Na 23 29 Cu 63

22. Valence electrons Electrons in __________ orbit
Atoms want a ________ outer orbit
They will bond with atoms that fill the orbit

23. Examples
Look at the column number on periodic table to figure out Valence electrons
Na __________ Cl ____________

24. Examples
Look at the column number on periodic table to figure out Valence electrons
C __________ N____________

25. Main Elements in Human Body
Oxygen
Carbon
Hydrogen
Nitrogen

26. Compounds Two or more atoms ______ together in a _________________
H20 vs. H2O2
what is different?

27. Compounds Parts are _____________ together
___________ proportions required
Properties of a compound are __________ from the properties of the elements that make up that compound.

28. Mixtures
Mixtures have “ingredients” that do _______ chemically with each other
Each ingredient keeps its ____
____________________
Definite proportions ___________
3 Types: ________, __________, __________

29. Mixtures Solution: _______________ (even throughout)
_______ (dissolved substance) completely dissolves in __________ (liquid)
________________
Doesn’t _________
Example - ___________________

30. Mixtures Suspension: _______________
May look homogeneous if shaken but particles will __________
____________ (murky)
Can be ______________
Example: _________________

31. Mixtures Colloid: _____________ BUT does not settle
Sort of ____________the other two.
Appears ____________ (let light through but image is not sharp)
Does not filter out.
Example -

32. What are three big differences between Mixtures and Compounds?
Mixtures vs. Compounds
Look at your notes:
What are three big differences between Mixtures and Compounds?

33. Types of bonds that form Compounds
Ionic Bond- ____________
_______________________

34. Creates ____________ that holds atoms together
IONIC:
Creates ____________ that holds atoms together

35. Types of bonds that form Compounds
Covalent- each atom ______ ___________ with the other

36. Change in the arrangement of atoms that creates a different substance
Chemical Reactions
Change in the arrangement of atoms that creates a different substance
A + B  C synthesis reaction
A  B + C decomposition
A + B  C + D Displacement

37. Chemical Reactions
Reactants:
Products:
A + B  C
_________
________

38. Al + O2  Al2O3 C2H6 + O2  CO2 + H2O H20  H+ + OH-
Chemical Reactions
Al + O2  Al2O3
C2H6 + O2  CO2 + H2O
H20  H+ + OH-

39. Properties of Water
Water is held together with special covalent bond called _____ covalent bond - Means water has poles, or ends. - O is the __________ end - H’s are the ________ ends

40. Properties of Water

41. Properties of Water
Cohesion: __________________ ___________________________

42. Cohesion
Creates __________________ - allows stickbugs to walk on water!

43. Adhesion
Glass stirring rod

44. Water is the Universal Solvent
Anything with a charge will attract water molecules and dissolve
Ionic and polar molecules have __________
______________(like fat) do not have charge and will not dissolve

45. Acids and Bases
Acids:
HX (in water)  H+ + X-

46. Properties of Acids
Taste sour – think of lemon
Turn litmus paper from blue to red
Corrodes Metal
Examples:_____________
_______________________

47. Acids and Bases
Base:
XOH (in water)  OH- + X+

48. Properties of Bases
Taste bitter – cough meds.
Turn litmus paper back to blue after acid turns it red
Can cause serious burns
Examples:

49. Acids and Bases - Examples
NaOH + H2O  Na+ + ___ + H2O
HCl + H2O  ___ + Cl- + H2O

50. Acids and Bases will “cancel” each other out
When an Acid and a Base are mixed together they will ___________each other and create ______ and a _____
This is a ___________ Reaction

51. Neutralization Reaction
HCl + NaOH  NaCl + H2O
_____ ____
HNO3 + KOH  KNO3 +H2O
_____ _____

52. pH = ___________________
Concept of pH
pH = ___________________
A way of measuring how many Hydrogen ions, H+, there are in a solution
Determines whether a solution is an __________________

53. pH Scale – a measure of the concentration of Hydrogen Ions
Acid
Neutral
(water)
Base 1 2 3 4 5 6 7 8 9 10 11 12 13 14
High H+
Low OH-
High OH-
Low H+
H+ = OH-

54. pH must stay between _____ in the human body
Concept of pH
Where is the “safe” pH?
pH must stay between _____ in the human body
Another factor that must maintain homeostasis

55. Intestines are _______ ________ are necessary
Concept of pH
Are there exceptions?
Stomach is _______
Intestines are _______
________ are necessary
weak acids or bases that react with strong acids or bases to prevent sudden changes in pH

56. What is the pH of Rain water??
Usually between _________
- Water reacts with CO2 in air to form Carbonic Acid (H2CO3)

57. What is the pH of Rain water??
Acid Rain:
- Rain water reacts with pollutants such as Sulphur dioxide and Nitrogen oxides in air
- Forms Sulphuric Acid, Nitric Acid, Ammonium Sulphate
- ______________________