1. Elements and Periodic Table
Bonding, Compounds, Periodic Table

2. What does the periodic table tell me?
Element symbol
Atomic number: number of protons (and usually electrons, neutrons)
Atomic mass: the average of all the isotopes’ mass
What type of element it is (metal, nonmetal, etc)
What elements can bond together (valence #)
In what ratio elements bond (oxidation #)

3. Reading the Periodic Table: Elements
Atomic number 16
Element symbol
32.06
Atomic mass

4. Types of Elements
Metals: usually shiny, conductors, malleable, ductile, solids at room temperature. On left side of periodic table
Non-metals: gas or brittle solid at room temperature, insulators. On right side of periodic table.
Metalloids: have properties of both metals and non-metals. Between metals and non-metals.

5. Three types of Elements

6. Things to remember with symbols
They are either one or two letters.
Only the first letter is capitalized!
Some symbols are based on the Latin name
Some of the newest symbols use three letters until they are renamed (the atomic number in Latin)

7. Element symbols you need to know
Gold Au
Chlorine Cl
Silver Ag
Sodium Na
Iron Fe
Hydrogen H
Lead Pb
Helium He
Copper Cu
Carbon C

8. More element symbols Potassium K Neon Ne Mercury Hg Zinc Zn Iodine I
Titanium Ti
Oxygen O
Aluminum Al Ca
Calcium
Sulfur S

9. Atomic Masses The mass comes from:
the average mass of the isotopes
protons and neutrons each weigh one atomic unit
Remember Isotopes - different number of neutrons.
Identified by name and mass number.
Boron-10, Boron-11
Try It! 5 atoms of Boron, four are Boron-10, one is Boron-11. What is the average atomic mass?
( ) / 5 = 10.2 u

10. What’s the diff?
Atomic Weight: Is an AVERAGE – usually in decimal form. On the periodic table
Mass number: The weight of that specific atom. Is a whole number. Often listed in the name (Boron-10, Carbon-14, Uranium-235)
We will be more concerned with mass number because it is how we find the number of neutrons! (mass number-atomic number = neutron number)

11. Periodic Table Non-metals Noble Gas Metalloids Halogen Metals
Transition Metals

12. Types of Elements
Noble Gas: Chemically stable. Has outer valence level full. “Happy” AKA: Inert elements. Don’t bond with others.
Halogens: Are non-metals. Bond VERY easily. Have 7 electrons in outer shell.
Non-metals: Do not easily conduct electricity or heat.
Metalloids: Have traits of both metals and non-metals.
Metals: Good conductor of heat and electricity, shiny, ductile (pulled into a wire), and malleable (pounded into flat sheets)
Transition metals: Metals that can have two different valence numbers. Is shown in the formula. Example: Fe (II)

13. Periodic Table
Alkali metals
Alkaline Earth metals
Transition metals

14. Hindenburg (5 minutes)

15. Reasons for the crash (7 minutes)

16. Element symbols you need to know
Gold Au
Chlorine Cl
Silver Ag
Sodium Na
Iron Fe
Hydrogen H
Lead Pb
Helium He
Copper Cu
Carbon C

17. More element symbols Potassium K Neon Ne Mercury Hg Zinc Zn Iodine I
Titanium Ti
Oxygen O
Aluminum Al Ca
Calcium
Sulfur S

18. Periodic Table Video Clip1

19. Periodic Table video clip2

20. Word Wizard vocabulary

21. Word wizard: Ionic Bond
Your definition
Important Points
Bond that is formed by the “stealing” of electrons.
One atom is now + and one is now -. This makes them attract to each other. Most are solid at room temp.
Ionic Bond
Examples
Non-Examples
Sodium Chloride: NaCl
Sugar: C6H12O6
Water: H2O
Diatomic molecules: Cl2, H2, N2 (gasses)

22. Word wizard: Covalent Bond
Your definition
Important Points
Bond that is formed by the “sharing” of electrons.
A stronger bond than ionic. Atoms can share more than one electron. Most are liquid or gas at room temp.
Covalent Bond
Examples
Non-Examples
Water: H2O
Diatomic molecules: Cl2, H2, N2 (gasses)
Sodium Chloride: NaCl
Sugar: C6H12O6

23. Word wizard: Polar Molecule
Your definition
Important Points
A molecule that has a positive end and a negative end
Polar will mix with polar.
Polar will not mix with non-polar
Polar Molecule
Examples
Non-Examples
Water: H2O
Sugar: C6H12O6
Salt: NaCl
Oil
Grease
Gasoline

24. Word wizard: Non-Polar Molecule
Your definition
Important Points
Non-polar will mix with non-polar.
Non-polar will not mix with polar
A molecule that has an equal charge all over.
Non-polar
Molecule
Examples
Non-Examples
Cooking Oil
Grease
Car oil
(things that don’t mix with water)
Water: H2O
Sugar: C6H12O6
Salt: NaCl

25. Word wizard: Anion anion
Your definition
Important Points
Anions have more electrons than protons. This makes them negative overall.
An ion that has a negative charge; has extra electrons.
anion
Examples
Non-Examples
Chlorine
Oxygen
Nitrogen
Non-metals
Sodium
Potassium
Magnesium
Metals

26. Word wizard: Cation
Your definition
Important Points
Cations lose electrons. They have more protons than electrons and are positively charged.
An ion that is positively charged; has less electrons
Cation
Examples
Non-Examples
Sodium
Potassium
Magnesium
Metals
Chlorine
Oxygen
Nitrogen
Non-metals

27. Word wizard: Chemical Formula
Your definition
Important Points
Large and small letters.
Shows what elements are in a compound and how many of each.
A shorthand way of writing compounds using their symbols.
Chemical
formula
Examples
Non-Examples
Water
Sugar
Salt
H2O
C6H12O6
NaCl

28. Word wizard: Chemically Stable
Your defintion
Important Points
Elements that have the outer electron shell full.
Also called “Noble Gases” or “Inert Elements”
Will not typically bond with other elements.
Likes to be ALONE!
Chemically
Stable
Examples
Non-Examples
Helium Krypton
Neon Xenon
Argon Radon
Gold Carbon
Sodium Nickel
Potassium Oxygen

29. Valence Numbers
Valence 1 2 3 4 5 6 7 8

30. Diatomic Molecules Covalent bond between identical atoms.
Usually a gas
Examples:
H2 (hydrogen gas)
O2(oxygen gas)
N2(nitrogen gas)
Nitrogen has 5 electrons in the outer shell.
It wants 8.
Two nitrogen atoms share three electrons.
BONDED!

31. Making Compounds
Let’s bond, shall we?

32. Valence Numbers
Valence electrons: how many electrons are in the outer shell.
Chemically stable: elements having their outer shell full. The noble gases are chemically stable without bonding.
To fill the outer shell, elements can share or steal electrons (bond).
To be “Happy” atoms typically want 8 electrons in the outer shell (ionic or covalent bonds)

33. Ionic bonding Stealing electrons
This makes one negatively charged (it has an extra electron that it stole). The other is now positively charged (had an electron taken). Opposites attract!
Ionic bonds are weaker than covalent.
Compounds that are solids at room temperature are usually from ionic bonds.

34. Covalent Bonding From sharing electrons
Covalent bonds are stronger than ionic
Compounds that are liquids or gas at room temperature are typically covalent bonds.
Diatomic: Some elements will covalently bond with themselves!

35. Common Household Compounds
NaHC03
Baking Soda:
Carbon Monoxide: CO
SiO2
Sand:
Ammonia:
NH4
Carbon Dioxide:
CO2
Salt:
NaCl
Bleach:
NaClO
Propane:
C3H8
Vinegar:
HCH3O2
Stomach Acid:
Water:
H2O
HCl

36. Dihydrogen Monoxide
The dangers, uses and potential threats posed by this chemical, Dihydrogen Monoxide, are widespread, and some feel, terrifying. Here is just a small taste of what Dihydrogen Monoxide (DHMO) is:
Some call Dihydrogen Monoxide the "Invisible Killer"
In it’s gaseous form, DHMO can cause severe burns
Dihydrogen Monoxide is found in all cancerous tumors
Dihydrogen monoxide was found at every recent school shooting
Athletes use DIHYDROGEN MONOXIDE, or DHMO, to enhance performance
Dihydrogen Monoxide has been found to cause failure in automotive breaks
Dihydrogen Monoxide is a major component of acid rain
Thousands die each year after inhaling dihydrogen monoxide
Dihydrogen Monoxide can be deadly
Visit DHMO.org to find out more

37. What’s in a name? Mono = one Di = two Tri = three Tetra = four
Penta = five
Examples:
Carbon Monoxide CO
Carbon Dioxide CO2
Dihydrogen Monoxide ??
H2O

38. P Dot Diagrams What you need to know to make a dot diagram:
Chemical symbol
valence number
How to draw the dot diagram of an element: 1. Write the symbol Find the valence number Fill in dots
two together (the S ones)
one in other sides until you run out of room. P

39. More Dot Diagrams F Li Ge Mg Se Kr

40. Sr As He I’m still seeing dots! Why is this one right?
Because Helium only has two electrons in the first place!

41. Oxidation numbers +1 +3
+/-4 -2 -1 +2 -3

42. Making Compounds H Cl = HCl Criss-Cross Method:
List the Metal first, non-metal second.
Write the oxidation number above the symbol.
Criss-cross the numbers. (a 1 does not need to be written, drop the + or -)
Final answer lists only the subscripts (numbers below the line)
If they are the same number, they cancel out
Example: Combine Hydrogen and Chlorine +1 -1 H Cl
= HCl

43. Now try these... H O Mg N H2O Mg3N2 Hydrogen and Oxygen +1 -2
Magnesium and Nitrogen -3 +2 Mg N
Mg3N2

44. Writing Equations (again??)
Remember the “criss cross” method.
Use the oxidation number
Don’t write in 1’s or the charges
Oxidation numbers of transition elements are given in a roman numeral.
Put in “lowest terms”
Example: Combine H and O +1 -2 H O
H2O
Example: Combine Fe (III) and O +3 -2 Fe O
Fe2O3

45. Writing Equations: something new
Monoatomic Ions:
“normal”
one element
can get from the periodic table or roman numerals
what you’ve been working with
Example: H20
Example: Combine Potassium and Permanganate
Polyatomic Ions:
compounds that always work together.
Always has more than one element
Get the information off a chart
Criss cross method still works.
Keep these elements together! +1 -1 K
MnO4
KMnO4

46. More Practice: Polyatomic Ions
Combine: Iron (II) and Nitrate +2 -1 Fe
NO3
Fe(NO3)2
Combine: Calcium and Carbonate -2 +2 Ca
CO3
CaCO3

47. Word wizard
Your definition
Important Points
Real example
Analogy/memory hook
Alloy
The mixture can have new properties. (lower melt point, stronger, etc.
Two or more metals melted down and mixed together.
Not ALL metals are mixtures. (All = alloy)
Alloys are like allies (mixed but not the same)
Sterling silver, 14 karat gold, bronze, brass

48. Word wizard
Your definition
Basic equation
Real example
Analogy/memory hook
Synthesis
Reaction
Reaction where substances are combined to make a new substance.
A + B AB
Like two people going out and becoming a “couple”.
Dating is a “sin”
2Mg + O MgO

49. Word wizard
Your definition
Basic equation
Real example
Analogy/memory hook
Single replacement
Reaction
One ingredient “kicks out” the other. Leaders always stay leaders!
A + BC AC + B
D + BC BD + C
Getting “dumped” for someone else.
One ends up single
Li + FeBr LiBr + Fe

50. Word wizard
Your definition
Basic equation
Real example
Analogy/memory hook
Double replacement
Reaction
Elements will change partners in this type of reaction. Leaders are always leaders!
AB + CD AD + CB
Switching dates at the prom.
Nobody gets left alone!
AgNO3 + NaCl AgCl + NaNO3

51. Word wizard
Your definition
Basic equation
Real example
Analogy/memory hook
Decomposition
Reaction
A substance is broken down into its “parts” in this reaction
AB A + B
A couple breaking up.
Things “break down” when they decompose.
2H2O H2 + O2
elec

52. Word wizard
Your definition
Basic equation
Real example
Analogy/memory hook
Combustion
Reaction
A reaction where two of the products are water and carbon dioxide
A + B CO2 + H20
Combustion = fire
Picture a fire with smoke (CO2) and water(H20) to put it out.
HCl + Na2CO CO2 + NaCl + H2O

53. Word wizard Chemical reaction where heat is ABSORBED.
Your definition
Important Points
Real example
Analogy/memory hook
Endothermic
Reaction
Chemical reaction where heat is ABSORBED.
Heat being absorbed makes it feel COLD.
Break and shake ice pack. (Heat is absorbed by ice pack, but it feels cold)
Endo has a “d” in it. Cold has a “d” in it.
Endothermic reactions FEEL cold.

54. Word wizard Chemical reaction where heat is released.
Your definition
Important Points
Real example
Analogy/memory hook
Exothermic
Reaction
Chemical reaction where heat is released.
This reaction will feel warm/hot.
“Exo” = “exit”
Heats EXITS an exothermic reaction. (it feels warm)
“Hand warmers” BenGay, Thermocare hot wraps

55. You can’t play “God”
Law of Conservation of Mass says that we can’t create or destroy mass!
Example: the weight of a piece of paper will be the same as the weight of the ash, smoke, etc after you burn it!!
In chemical reactions, you need to have the same amount of atoms before and after the reaction!

56. It’s a balancing act Ag + H2S Ag2S + H21 Ag 2 H 2 H 2
Not Balanced! Conservation of mass says we can’t create or destroy anything!! S 1 S 1

57. It’s a balancing act 2
Ag + H2S Ag2S + H2 Ag 1 2 Ag 2 H 2 H 2 S 1 S 1

58. Try balancing this: Balanced!! 2 Mg + O2 MgO 2
Coefficient: The “big” number that is put in front to show how many units you need to have. Mg 1 2 Mg 1 2 O 2 O 1 2
Balanced!!
How to read it: 2 units of Magnesium added to oxygen gas yields 2 units of Magnesium Oxide