1. SPS4. Students will investigate the arrangement of the Periodic Table.

2. Chapter 3: Atoms & The Periodic Table
Why do coins shine?
Their chemical properties determine their physical properties.
Example: Gold vs. Silver

3. Atoms are the building blocks of ___________.
Atomic Structure
Atoms are the building blocks of ___________.
In 1808, John Dalton proposed the Atomic Theory

4. The Atomic Theory
Every element is made of tiny, unique particles called _________ that cannot be subdivided.
Atoms of the same element are exactly alike
Atoms of different elements can join to form __________.

5. Atoms have no overall charge ________ Atomic # =_________
3 parts to an atom
Protons
Neutrons
Electrons
Atoms have no overall charge ________
Atomic # =_________
Atomic Mass =__________
Nucleus

6. Bohr’s Model Compares electrons to planets that orbit.
Stated that electrons in an atom move in set paths around the nucleus.
The path defines the electron’s ________ ________.

7. Energy Levels (Orbitals)
Electrons can only be in certain energy levels
Electrons must________ energy to move to higher energy level & _________ energy to move to a lower energy level.
Ex. Elevator

8. Modern Model Electrons move more like _________ instead of orbits.
It is impossible to determine the exact location of an electron or its speed & direction.
Ex. Blades of a Fan

9. Electrons are found in orbitals within energy levels
The region where electrons are found are called Orbitals.
Electrons can occupy 4 kinds of orbitals
The simplest orbital is the ____ orbital.
The s orbital can have only ______ possible orientation in space. Shaped like a _________

10. Orbitals Continued
The p orbital is dumbell-shaped and can be oriented 3 different ways in space.
There are also d & f orbitals.
There are 5 possible d orbitals
There are 7 possible f orbitals
Each orbital can only hold ____electrons.

11. Electrons usually occupy the ________energy levels available in an atom
In any level, the _____ orbital has the lowest energy.
The p orbital has slightly more energy
The _____ orbital has slightly more than the p
The ______ has the greatest energy.

12. Valence Electrons
An electron in the outmost energy level is a __________ electron.
Valence electrons determine the atom’s reactivity with other atoms.

13. Energy Levels First Energy Level Second Energy Level
closest to nucleus
contains one sublevel (s)
contains only 2 electrons
Second Energy Level
Contains 2 sublevels (s & p)
1 s orbital & 3 p orbitals
8 total electrons

14. Third Energy Level Fourth Energy Level 3 sublevels (s, p, d)
1 s orbital, 3 p orbitals, & 5 d orbitals
______total electrons
Fourth Energy Level
4 sublevels (s, p, d, f)
1 s orbital, 3 p orbitals, 5 d orbitals, & 7 f orbitals

15. Chapter 3 Section 2: The Periodic Table
The periodic table groups __________ elements together.
Makes it easier to predict the properties of an element based on its location on the table.
The order is based on the # of protons in atom of that element has in it nucleus.

16. The Periodic Law
States that when elements are arranged this way similarities in their properties will occur in a regular pattern

17. Atomic # Protons Neutrons Electrons Atomic Mass8 16 18 26 17 31 23 10

18. Organization of the Periodic Table
Horizontal Rows in the periodic table are called _________.
The number of protons increases by 1 as you move from left to right.
Vertical Columns are called ________.
Elements in the same group have the same number of ___________ electrons
Valence electrons determine the chemical properties of elements

19. Reactivity & Ionization
Elements in Group 1 are reactive because their outermost levels are ________filled by electrons.
Example: Hydrogen (only 1 electron)
Atoms that don’t have their outermost energy levels filled may undergo Ionization
They may gain or lose valence electrons
Atoms are called __________.

20. When an atom loses an electron it becomes a __________. (positive ion)
Ex. Li+
When an atom gains an electron it becomes an __________. (negative ion)
Ex. Fl-
Isotopes vary in the number of neutrons
Example: Carbon 14

21. The Mass of an Atom
An atomic mass unit (amu) is equal to 1/12th the mass of a carbon-12 atom
An element’s average atomic mass is a weighted average of the masses of its naturally occurring isotopes.

22. Chapter 3 Section 3: Groups of Elements
Members of the same “Group” have many similar chemical & physical properties because they have the same # of _______________ electrons
Elements are classified in 2 main categories:
_________________

23. Nonmetals & their compounds are plentiful on Earth.
Elements with properties similar to metals & nonmetals are called _________________or Semiconductors.
Nonmetals & their compounds are plentiful on Earth.
Ex. Oxygen, Nitrogen, & Sulfur

24. Halogens & Noble Gases Halogens (Group 17) Noble Gases (Group 18)
Example: Chlorine
Noble Gases (Group 18)
Examples: Neon & Helium
Exist as single atoms instead of molecules
Inert (Unreactive)
Outer level is filled with electrons
Do not gain or lose electrons
Do not join to create compounds under normal conditions

25. Chp. 3 Sec 4: Moles
The Mole is useful for counting _________ particles.
Large counting unit
Abbreviate mol =
6.022 X 1023

26. 6.022 X 1023 = 1 mol of a pure substance
Avogadro’s Constant
6.022 X 1023 = 1 mol of a pure substance
Molar Mass = The mass in grams of 1 mol of a substance

27. Conversion Factors
A ratio equal to one that expresses the same quantity in 2 ways.