1. Unit 3: Periodic Table Have your Periodic Table out everyday for this unit

2. Herriman High Chemistry
Essential Questions
What is the periodic table and why do we use it?
How did the periodic table come into being?
How is the periodic table arranged?
What is periodic law and what are the different trends?
What are ions and what are the types?
Herriman High Chemistry

3. I. Historical Development of the Table
A. Dmitri Mendeleev (__________)
Arranged elements into table based on…
similarities in the physical and chemical properties
thought similarities were function of atomic mass
Noticed that some elements seemed out of order (Iodine and Tellurium)
Mendeleev Video Clip

4. I. Historical Development of the Table
1913
B. Henry Mosely (__________)
Established that properties of elements were functions of ____________
Atomic Number
1. Present table based on ________________
Atomic Number
2. Elements’ properties depend on ________________
Structure of atom
3. Properties of elements vary ________________
Systematically throughout the table

5. I. Historical Development of the Table
C. Periodic Law: When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

6. II. Period (or Rows)
Horizontal rows
Number at the beginning of the period indicates the number of energy levels 1 2 3
Periods 

7. II. Period (or Rows) 4 Properties change as you move across a period
Example:
A) What period is potassium and bromine in? ____
____________________________________________ 4
Properties change as you move across a period

8. III. Groups(or Families)
Vertical Columns
Each group has similar chemical properties
For representative elements (A) the group number tells you the number of valance electrons
Group 1A has 1 valance electron
Group 3A has 3 valance electrons

9. Valance electrons are electrons found in the outermost energy level of an atom

10. II. Period (or Rows) 2 Similar (both have 2 valence e-) Example:
A) What group is magnesium and calcium in? ____
B) Based on the group, how do the properties of magnesium and calcium compare? _______________ 2
Similar (both have 2 valence e-)

11. III. Groups(or Families)
Sample Questions:
Which sequence of atomic numbers represents elements which have similar chemical properties?
A) 19, 23, 30, 36 C) 9, 16, 33, 50
B) 3, 12, 21, 40 D) 4, 12, 38, 88
Which two elements have the most similar chemical properties?
A) Aluminum and Barium C) Nickel and Phosphorous
B) Chlorine and Sulfur D) Sodium and Potassium

12. Forming Cations & Anions
IONS are atoms or groups of atoms with a positive or negative charge.
A CATION is positively charged and forms when an atom loses one or more electrons
An ANION is negatively charged and forms when an atom gains one or more electrons
Mg --> Mg e-
F + e- --> F-

13. PREDICTING ION CHARGES
In general
metals lose electrons and form cations
nonmetals gain electrons and form anions

14. VI. Ions
An atom that has lost or gained electrons (# of protons does NOT EQUAL # of electrons)
2311 Na +1
# of p =
# of n =
# of e- = 11
Mass # =
Atomic # =
Ion Charge = 23
23 – 11 = 12 11
Atomic # - Ion
Charge +1
# of e- = 11- (+1) = 10

15. VI. Ions Examples: 3 15 16 18 Mass # - Atomic # Atomic # - Charge
Lost e- (cation) 3
7 – 3 = 4
3 – (+1) = 2
7 Li ______ p ________ n ____________ e ________
31 P – 3 ______ p ________ n ________ e ___________
79 Se – 2 ______ p ________ n ________ e ___________
39 K ______ p ________ n ________ e ___________
Gained e- (anion) 15 16 18
gained e (anion)
lost e (cation)

18. IV. Metals- Outline green
Atoms that lose e- and form positive ions (cations) when bonding
Alloy:
Mixture of metals by melting them together
(can use pg 158 or back of book to see elements better)

19. IV. Metals 1. Low ionization energy and electronegativity
Properties of Metals:
1. Low ionization energy and electronegativity
2. Good conductors of heat and electricity
3. Exhibit metallic luster (shine)
4. Malleability (can be pounded into thin sheets)
5. Ductility (can be pulled into thin wires)
6. More than 2/3 of the elements are metals
7. High densities
8. Mercury (Hg) is a metal which a liquid at room temperature.

20. CHECKS FOR UNDERSTANDING
IV. Metals
CHECKS FOR UNDERSTANDING
Which element is malleable and can conduct electricity in the solid phase? A) Iodine B) Phosphorous C) Sulfur D) Tin

21. V. Nonmetals- Outline red
atoms gain e- and form negative ions (anions) when bonding
(can use pg 158 or back of book to see elements better)

22. V. Nonmetals 1. High ionization energy and electronegativity
Properties of Nonmetals:
1. High ionization energy and electronegativity
2. Poor conductors of heat and electricity
3. Brittle and hard
4. Low densities
5. Many are gases
Graphite is an allotrope of carbon. It is used in pencils (brittle, soft, and low density)

23. CHECKS FOR UNDERSTANDING
V. Nonmetals
CHECKS FOR UNDERSTANDING
Which element is brittle and not a conductor of electricity? A) Sulfur B) Sodium C) Potassium D) Argon

24. Herriman High Chemistry
Essential Questions
What are the types of elements and how can you tell what type an element is?
What are the different groups on the periodic table and what properties do they have?
Herriman High Chemistry

25. VI. Metalloids – Outline purple
Atoms that gain or lose e- and form ions when bonding
Have properties of both metals and nonmetals
Can be located using the “staircase” (see periodic table)
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Astatine
(can use pg 158 or back of book to see elements better)

26. CHECKS FOR UNDERSTANDING
VI. Metalloids
CHECKS FOR UNDERSTANDING
Which element has both metallic and nonmetallic properties? A) Rb B) Rn C) Si D) Sr
Which list of elements contains 2 metalloids?
Si, Ge, Po, Pb C) As, Bi, Br, Kr
Si, P, S, Cl D) Po, Sb, I, Xe

27. VIII. Groups within Groups
A. Group 1A/1: ________________
Alkali Metals- Color green
All soluble (dissolves) in water and strongly basic
Hydrogen is the exception on the periodic table – it belongs nowhere : (
ALKALI METALS- clip

28. VIII. Groups within Groups
Alkaline Earth Metals-
color light green
B. Group 2A/2: ______________________
Reactive with water and air, but less reactive than group 1A
In General for Groups 1 and 2:
As you move down, they become more reactive

29. VIII. Groups within Groups
Transition Metals
color blue
C. Groups B’s/3-12: ________________
Dense Metals and high melting points
Form multiple ions and less reactive than Groups 1 and 2
Form ions that have color
Copper (II) Sulfate Solution (Cu2+ ions)
Cobalt (II) Chloride Solution (Co2+ ions)

30. VIII. Groups within Groups
CHECKS FOR UNDERSTANDING
4. Identify the metal that has multiple oxidation states.
A) K B) Ba C) Be D) Pd
5. Which compound forms a green aqueous solution?
A) RbCl B) CaCl2 C) NiCl2 D) BeCl2
6. Which set of properties is most characteristic of transition elements?
Colorless ions in solutions, multiple positive oxidation states
Colorless ions in solutions, multiple negative oxidation states
Colored ions in solutions, multiple negative oxidation states
Colored ions in solutions, multiple positive oxidation states

31. VIII. Groups within Groups
Halogens- color orange
D. Group 7A/17: ________________
Most reactive nonmetals, especially with group 1A
Mostly nonmetallic elements

32. VIII. Groups within Groups
E. Group 8A/18: ________________
Noble Gases- color red
Have 8 valence electrons (or 2 for He)
Have a full outer energy level
Do not react because their outer shell is completely full (8)
They are stable (do not react easily because their out shell is full
ALL OTHER ELEMENTS WANT TO BE LIKE THEM

33. Others Color the rest of the nonmetals yellow
Color the rare earth metals (bottom two rows) brown

34. X. Other Categories Diatomics - Molecule containing 2 identical atoms
Remember them: BrINClHOF
H, O, F, Br, I, N, Cl (7-H club)
Radioactive -
Nucleus is unstable and breaks down spontaneously (all isotopes are radioactive, but less than the ones mentioned below)
Which ones?
Atomic # greater than 84 also 43 (Technetium) and 61 (Promethium)

35. X. Other Categories Synthetic – (NOVA: How they are made)
Man-made elements (all are radioactive, as well, but disintegrate in milliseconds)
Remember them:
Atomic # greater than 93 also 43 (Technetium) and 61 (Promethium)
White on my periodic table

36. VII. Periodic Properties
A. Atomic Radius:
Distance between the center of the nucleus to the most outer electron shell (orbital)

37. VII. Periodic Properties
Periodic Trend
decreases
Atomic Radius ___________
as you move from ______________________________
Left to right across a period
Same number or energy levels, but more protons so outer e- get pulled closer to the nucleus
increases
Atomic Radius ___________
as you move ______________________________
down a group
# of energy levels increase

38. VII. Periodic Properties
B. Ionic Radius:
A loss or gain of e- causes an increase or reduction in atom’s size
Metals: __________ electrons when they form ions ( _____________ ) and ionic radius __________ than neutral atom
lose
cations
smaller
2-8-1
2-8

39. VII. Periodic Properties
B. Ionic Radius:
Nonmetals: __________ electrons when they form ions ( __________ ) and ionic radius __________ than neutral atom
anions
gain
bigger
2-8-7
2-8-8

41. IV. Periodic Properties
Sample Questions:
Which element has an atomic radius that is greater than its ionic radius?
A) S C) F
B) K D) O
In period 4, the atom with the largest covalent radius is located in group…
A) 1 C) 3
B) 13 D) 18

42. VII. Periodic Properties
C. Ionization Energy:
Amount of energy needed to remove the most loosely bound e - (valence e -)

43. VII. Periodic Properties
Periodic Trend
increases
Ionization Energy ___________
as you move from ______________________________
Left to right across a period
Number of protons and valence e- increases and size decreases, so e- are held tighter
decreases
Ionization Energy ___________
as you move ______________________________
down a group
(e- are farther away, so easier to remove e-
Electron Shielding

44. Electron Shielding

45. VII. Periodic Properties
D. Electronegativity:
Measure of atom’s attraction for electrons when bonded
Desire of an atom to gain electrons
Periodic Trend
Electronegativity ______________ as you move from ______________________________
Electronegativity ______________ as you move _____________________________
increases
Left to right across a period
decreases
down a group

46. IV. Periodic Properties
Check for Understandings
What are the electronegativity's for group 18 elements? Why do you think they have “this” electronegativity?
Which element attracts electrons the most when bonding?
A) Ca C) Br
B) Sr D) I
Which element gives off its valence electrons the easiest?
A) Ca C) Br
B) Sr D) I
They do not have electronegativity numbers. Why? Because they already have their 8 valence electrons (octet)

47. VIII. Groups within Groups
CHECKS FOR UNDERSTANDING
As you move down groups 1 and 2 elements become more reactive. Explain why this happens based on atomic size and ionization energy/electronegativity.
What will be the charge on a Ca ion when it bonds?
Based on your answer to question 2, what happens to the atomic size once it becomes an ion?
As atomic size increases, ionization energy decreases (easier to remove e-) so they become more reactive +2
Smaller (loses last energy level)

48. VIII. Groups within Groups
CHECKS FOR UNDERSTANDING
Which halogen is most reactive? Explain why, based on atomic size, electronegative/ionization energy.
Explain why noble gases don’t typically react with other elements?
F: smallest in size so attraction for electrons is very high (electronegativity)
Their outer energy level is completely full. They do not want to gain anymore e-