1. Atoms, first Periodic Table, second
MT 1 Review
Atoms, first
Periodic Table, second

2. What is the central part of the atom called?
Review Questions
What is the central part of the atom called?
What is the most dense part of an atom called?
What is the biggest part of the atom?
What part of the atom contains most of its mass?
What is the smallest part of the atom that contains the atom’s properties?

3. Made of Protons (+) and Neutrons (•) Positive and Neutral
The NUCLEUS
Made of Protons (+) and Neutrons (•)
Positive and Neutral

4. What part of the atom does the electron cloud hold?
Review Questions
What part of the atom does the electron cloud hold?
What is the smallest part of an atom?
What part of the atom does not have a measurable mass?
What part of the atom is important in atomic bonding?

5. Negatively charged (-)
ELECTRONS
Negatively charged
(-)

6. Remember Protons – Positive (+) Electrons – Negative (–)
Neutrons – Neutral (•)

7. Comparison
If the nucleus of an atom was a marble at the starting line of a race track, a grain of sand 100 yards away would represent the first electron

8. Comparison
Now you make one…
2 minutes

9. Periodic Table Vocabulary
Atomic Number – # of Protons
Atomic Mass – # of Protons plus Neutrons
Atomic Number – # of Protons (also equal to Number of Electrons)
Atomic Mass – Number of Protons and Neutrons

11. Periodic Table Vocabulary
Atoms are neutral
Valence Electrons: # of electrons in outer shell ***Important for atomic bonding
Atoms are neutral
Valence Electrons: # of electrons in the outer/last shell of an atom
***Important for atomic bonding

12. Do the rows & columns have a name?

13. Columns: Known as A Group or Family

14. Rows: Known as Periods

15. What do all the colors mean?
Elements are arranged by increasing atomic number and atomic mass. The trend increases from left to right and from top to bottom.

16. What do all the colors mean?
Elements are arranged based on similar properties
Elements are arranged by increasing atomic number and atomic mass. The trend increases from left to right and from top to bottom.

17. There are 3 main groups of elements -Metals
-Nonmetals
-Semi-metals

18. Metals Shiny surface Good conductors Solids at room temperature
Malleable (bendable).
Shiny surface
Good conductors of heat and electricity.
usually solids at room temperature malleable (bendable).

19. Metals are YELLOW

20. Nonmetals
dull-colored
brittle
Do not conduct heat or electricity.

21. Nonmetals are GREEN

22. Semimetals (Metalloids)
having properties of both metals and non-metals.

23. Semimetals (Metalloids) are PURPULE

24. Groups on Periodic Table of Elements

25. Are there any subgroups?
YES!
Metals
Alkali Metals
Alkaline Earth Metals
Transition Metals
Rare Earth Metals
Non-Metals
Halogens
Noble Gases

26. Alkali Metals Group 1 highly reactive 1 Valence Electron
Low ionization energy & electronegativity
Group 1
highly reactive
1 Valence Electron
low ionization energy because they give up their 1 electron easily
Giving up electrons makes these positive ions

27. Low ionization energy & electronegativity
Alkaline Earth Metals
Group 2
very reactive
2 Valence Electrons
Low ionization energy & electronegativity
Group 2
very reactive
2 Valence Electrons
low ionization energy because they give up their 2 electrons easily
Giving up electrons makes these positive ions

28. Transition Metals 38 elements in the middle of P.T.
Metals in Group 3 to 12
Share characteristics of all metals
1 or 2 electrons in outer shell

29. Halogens Group 17 7 Valence Electrons
High ionization energy & electronegativity
Outer shell is almost full

30. Noble Gases Group 18 odorless and colorless
Gases: 8 electrons in outer shell (FULL)
No Electronegativity (don’t want additional electrons)
High Ionization Energy

31. Groups on PT of E

32. PT of E TRENDS
Ionization energy – how much energy REQUIRED to remove electrons from an atom
Electronegativity – the pull of the nucleus on electrons (attractiveness)

33. PT of E TRENDS
Ionization energy – how much energy REQUIRED to steal, take, remove electrons from an atom
Electronegativity – the pull of the nucleus on electrons (attractiveness)
Electronegativity AND Ionization Energy – top, right of periodic table
Increases moving left to right
Increases moving bottom to top

34. PT of E TRENDS Remember:
The stronger the attraction (electronegativity) electrons have to the nucleus the harder they are to remove (ionization energy)
This is why they have the same trend!

35. PT of E TRENDS
Atomic Radius/Atomic Radii– how much space an atom takes up (how big an atom is)
bottom, left of periodic table
Increases moving right to left
Increases moving top to bottom

36. Elbow Partners Turn to the person sitting next to you… Discuss…
Explain how the Periodic Table of Elements organizes the atoms by their structure.

37. The Periodic Table of Elements organizes the atoms by their structure….
Low # of protons (Atomic #), Low atomic mass
Low # of rings
High # of Valence e-
High # of protons (Atomic #), High atomic mass
Low # of Valence e-
Size increase bottom to top
High IE, High EN- hard to lose e-
High # of rings
Low IE, Low EN- easy to lose e-
Size decrease left to right-pulls atom tighter

38. Quick Write Take 5 minutes and answer this question in your notes
Explain how the location of an atom on the Periodic Table tells a lot about that atom’s characteristics.

39. Explain how the location of an atom on the Periodic Table tells a lot about that atom’s characteristics.
Metals
Non-Metals
Alkali Metals
Transition Metals
Noble Gases
-one outer e-
-very reactive
-never found alone
-soft & dense
-2 or 1 outer e-
-shiny
-good conductor of heat & electricity
-very useful in every day life
-8 outer e-
-outer ring is FULL
-never connected to another atom
-gases in our atmosphere