1. 2/23
On your PT on page 31, find and underline symbol for the non-metal Sulfur. Identify and underline 2 other elements that are in its family.

2. Periodic – means regular, repeated pattern.
Modern Periodic table vs. Mendeleev’s
Brainpop

3. Reading the Periodic Table
- atomic #= #of protons & electrons
- element symbol
-element’s name
Atomic mass/weight: protons + neutrons (nucleus)
Round off for mass#. Mass # of Fe=______ 26 Fe
Iron
55.847

4. What’s the difference between Mass # & atomic #?
Atomic # is equal to the number of protons or electrons (unless charged)
Mass # is the # of protons PLUS the # of neutrons (each equals 1 AMU)

7. Drawing an atom Draw atomic structure of H & He as a class.
Draw atomic structure O on your own.
Determine valence e-s for each one.
Building an atom

8. Lewis Dot structure
Uses the elements symbol and dots for # of val. e-s.
Ex. H
Complete Lewis Dot structure page on PT Basics Packet.

9. Ca H Cl Ar P

10. Groups: Columns
The vertical columns of the periodic table (there are 18) are
called groups (18) or families (I- VIII)
Family # gives # of valence e-s.
Metallic character increases from top to bottom.
Share similar chemical and physical properties/looks as long as in the same column/family.
Ex. Li, Na, and K have similar properties, all in 1 family.
Write the val e-s for families I thru VIII on your PT

11. Periods: Rows (7)
The horizontal rows of the periodic table are called periods
‘periodic’ means repeating pattern.
Per. # tells us how many energy levels the elements have.
Elements in a period are not alike in properties.
3 repeated PATTERNS left to right:
1. METAL TO NONMETAL
2. REACTIVE TO NONREACTIVE
3. Val. E-s go up.
Draw the number of shells for Periods 1 thru 7 on your PT

12. Rows (cont’d) Atomic # (# of protons) from L to R across a period. &
Atomic mass (# of protons & neutrons) increases from left to right across a period.
Groups and columns review

13. Locate the element Chlorine on your PT
Locate the element Chlorine on your PT. Decide which 2 elements will have properties similar to those of Cl.
S and Ar
Br and I
Br and F
O and F
PT Videos

14. 2/24 Periodic table notes cont’d
IQ: Circle the element Ca on your PT. Determine and circle the 2 elements that have properties most similar to Ca.

15. Rows & Columns Combined OVERALL (back of PT)
Metals are on the left.
Non-metals are on the right.
Metalloids are in between metals & non-metals, on ‘staircase’ or the “zig-zag.”
Brainpop

16. Metals and non-metals

17. * Metalloids are combined properties of both metals and nonmetals.
Conductive (heat/electricity)
Nonmetals
silver or white in color, lustrous (shiny)
dull in appearance
malleable and ductile
brittle if solid
Dense
poor conductor of heat and electricity
high melting and boiling points
low mps and bps
low densities
many react with acids
does not react with acids
all solids except, mercury (Hg)
exist in all three states of matter  * Metalloids are combined properties of both metals and nonmetals.
 * Metalloids are combined properties of both metals and nonmetals.

18. Each color represents a different group,
or family.

19. Some properties of metals to look at (in notebook)
Malleability- Ability to be flattened into thin sheets. Ex. Aluminum
Ductility- Ability to be drawn into wires. Ex. Copper.
Heat and electrical conductivity- Ability to allow heat and electricity to pass through. Ex. Copper (p. 306)

20. 2/25 p. 30 Atomic Bonding
IQ: Draw the Bohr model for Sodium (Na). Then, predict what would a Na +1 ion be like.

21. Bonding (back of PT)
The # of outer/“valence” e-s in an atom affects the way an atom bonds.
The ‘magic #’ is 8 “octet”…e- want to have 8 friends total! Makes a complete outer shell.
Noble gases have a complete outer shell (2 or 8e-s) so they don’t bond with anything.
The way an atom bonds determines many properties of the element.
Group 1 elements will readily bond with Group 17 elements to form salts. Can you tell why?

22. For example, during the reaction of sodium with chlorine:
                            sodium (on the left) loses its one valence electron to chlorine (on the right),
   resulting in
                            a positively charged sodium ion (left) and a negatively charged chlorine ion (right).
The reaction of sodium with chlorine
Concept simulation - Reenacts the reaction of sodium with chlorine.
(Flash required)

23. Bonding cont’d :
“Valence/Outermost” e- effects the way an atom reacts.
The ‘magic number’ is 8 e-s want to have 8 friends total.
Makes complete outermost shell, called a complete octet. 4) Ex. Group 1 elements will readily bond with Group 7 elements. 5) Two types of bonds: a) Covalent bond: means to share electrons. Usually between two non-metals.
b) Ionic means to gain or lose valence e-s, metals & non-metals usually metal with non metal.