1. Snapshot
The ____ model was designed in _____ and has a solid positive nucleus surrounded by electrons.
The _____ model is the current model of the atom.
____ model says the electrons were in fixed orbitals.
Protons & neutrons are made of smaller parts called _______.
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

2. PS.4 Investigating Bonding & the Periodic Table
PS.4 The student will understand & investigate the organization and use of the periodic table of elements
to obtain information.

3. Periodic Table Table showing known elements (~115)
Arranged several ways:
Atomic number (1-118)
Groups/ Families (1-18)
Vertical columns
Periods (1-7)
Horizontal rows
Properties
Bonding
Metallic or nonmetallic
Designed by Dmitri Mendeleev in late 1800’s
Organized elements by similar properties.
Left room for unknown elements.
Table was updated by Henry Moseley in 1913 to organize by atomic number
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

4. Mendeleev’s 1st Periodic Table
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

5. Groups/ Families = columns
Elements in same group:
Have same # of valence electrons
e- in outer shell = valence e-
Group number = # of valence e-
Ex. Nitrogen is in group 5A or 15 (for use 2nd digit)
It has 5 e- in its outer energy level
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

6. Ex. Na is in period 3 so it has 3 energy levels in its electron cloud
The period number tells you the number of energy levels (orbital/shells) in the e- cloud
Ex. Na is in period 3 so it has 3 energy levels in its electron cloud
Periods = rows
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

7. Group 1A are the alkali metals (but NOT H)
Group 2A are the alkaline earth metals
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

8. These are called the Inner Transition Elements, and they belong here
Groups 3-12 are called the Transition Elements
These are called the Inner Transition Elements, and they belong here
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

9. Group 8A are the Noble Gases Group 7A are the Halogens
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

10. As move from left to right elements b/c more nonmetallic
Metalloids
Nonmetals
Metals
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

11. Info Found in Periodic Table
Atomic Number
Symbol (1-3 letter abbreviation)
Name
Atomic Mass
State of Matter at Room Temp.
protons
Atomic number always equals the number of ____________ and may equal ________________ in a neutral atom.
electrons
protons
neutrons
Atomic mass equals the number of ______________ + _____________.
Number of neutrons = atomic mass – atomic number
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

12. PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

13. Snapshot Calcium Symbol Atomic Number Atomic Mass # of protons
#of electrons
# of neutrons
Group #
Period #
State of Matter at Room Temperature
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

14. Snapshot The vertical columns in the periodic table are called _____.
The horizontal rows are called _____.
From left to right the atomic _____ increases.
The group number tells you the number of _____.
Which elements are liquids at room temperature?
Provide the name of elements 57-71
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

15. Metals, Metalloids, & Nonmetals
Property
Metals
Metalloids
Nonmetals
Luster
Shiny
Not Shiny
Hardness
Hard
Malleable/
Ductile
Yes No
Conductor (Heat & Electricity)
Semi
room temp
Solid (1 liquid)
High density
Solid
Varies
Low density
Reactivity
Most reactive
elements
Least reactive
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

16. Properties of Metals
Metals have luster. This means they are shiny 16

17. Properties of Nonmetals
Nonmetals do not have luster; they are dull. 17

18. Properties of Metals
Ductile
metals can be drawn into wire. 18

19. Properties of Metals
Malleable
metals can be hammered into sheets 19

20. Properties of Nonmetals
Brittle
Nonmetals are brittle so they break easily. This means nonmetals ARE NOT ductile or malleable. 20

21. Properties of Metals
Metals have a high melting point. They are also very dense. 21

22. Properties of Metals
A chemical property of metal is its reaction with water and oxygen. This results in corrosion and rust. 22

23. What are these elements?23

24. What are these elements?24

25. What are these elements?25

26. Isotopes
An element that has a different number of neutrons (higher or lower than periodic table)
B/c mass number equals # of n0 + # of p+, the mass number will now be different
Most elements have isotopes
Isotope notation looks like this:
1-Hydrogen-3
H H 3 1 1 3
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

27. Ions
An ion is a positively or negatively charged atom {cations (+) & anions(-)}
Gaining or losing electrons makes an atom an ion
Positive ions have lost an electron
Negative ions have gained an election
Looks like this
Ca2+ or Ca2-

28. Helium Ions— p+, n0, e-
# of protons
# of electrons
Charge
Notation

29. Your turn! p+, n0, e-
# of protons
# of electrons
Charge
Notation

30. Chemical Bonding Atoms bond to become more stable
They desire 8 valence e-
Atoms bond together by gaining, losing, or sharing valence electrons
The number of valence electrons determines how an atom will bond
Two or more elements bonded = a compound
2 elements = binary compound
3 elements = trinary compound
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

31. Ionic Bonds Ionic bonds occur when atoms gain or lose electrons
Form when a metal and nonmetal react
the metal will give up its valence electrons
the nonmetal will take the valence electrons

32. How many valence electrons does each atom have before they bond?
How many valence electrons does each atom have after they bond?
Both now have full shells and are stable

33. Covalent Bonds Occur when atoms share e-
Formed with a Nonmetal and a Nonmetal
e- are shared
They have full outer shells
Both are stable
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

35. Polyatomic Ions Poly = many Covalently bonded atoms Have a charge
Considered to be ionic and covalent
Often bond with metals
Ex. OH- or ClO3-1
Ex. With Metal sodium make:
NaOH & NaClO3
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

36. Parts of a Chemical Formula
2 Main Parts
Symbols
letters representing elements
First letter always capitalized
Ex. C6
Subscripts
Numbers found behind symbols
Sub= below
Script= writing
Tell number of atoms of each element
PS.4 The student will understand & investigate the organization and use of the periodic table of elements to obtain information.

37. Subscripts N H How many atoms of each element are in the formula: NH3
1 Nitrogen
3 Hydrogen

38. Subscripts
How many atoms of each element are in the formula:
C3H8 C H

39. Putting it Together
Use the chemical formulas and periodic table to determine if the atoms in each formula formed an ionic or covalent bond
Remember:
Metal + Nonmetal = Ionic
Nonmetal + Nonmetal = Covalent
Metal + Nonmetal + Nonmetal = Both