1. Chemistry
MYP 1 Advanced

2. Modern Atomic Theory All matter is composed of atoms.
Atoms can’t be subdivided, created or destroyed in ORDINARY chemical reactions.
It is possible with nuclear reactions.
Atoms of an element have a mass that is unique to that specific element.
Atoms of any one element have properties that differ from other elements.

3. What’s in an atom? Atoms are neutral
There are protons, which have a positive charge.
Electrons which have a negative charge.
Neutrons that have no charge.
These are found in the nucleus of the atom.
The mass of an atom is made up of the protons and the neutrons.
The nucleus is small and dense.

4. Atomic Number
The number of protons in the nucleus of an element

5. Atomic Mass
The number of protons and neutrons in the nucleus of the element.

6. The Bohr Model of the Atom
Neils Bohr imagined that electrons orbited the nucleus like planets orbited the sun.

7. Electron Energy Level

8. Electron Orbitals
An orbital is a region within an energy level where there is a probability of finding an electron.
Orbital shapes are defined as the surface that contains 90% of the total electron possibility.
The S orbital has a spherical shape
The P orbitals are dumbbell shaped
The D orbitals are double dumbbell shaped

9. Electron Orbitals and Energy Levels

11. Periodic Table of the Elements

12. Periodic Table of the Elements
The groups are arranged in columns and the periods are arranged in rows

13. Alkali Metals They are in group 1 They all have one valence electron
They are never found pure in nature because they are too reactive.
As you go down the group the reactivity increases.

14. Alkaline Earth Metals They have 2 valence electrons
Less reactive than alkali metals
They are the 2nd group in the periodic table
They are not found pure in nature because they are too reactive

15. Properties of Metals Good conductors of heat and electricity Malleable
Ductile
High Tensile Strength
Luster

16. Transition Metals
All of the metals in the middle section of the periodic table
Includes gold and silver

17. Properties of Metalloids
Properties of metals and non metals
More brittle than metals but less brittle than non metals
Semiconductors of electricity

18. Nonmetals Poor conductors of electricity Brittle
Gases at room temperature
Ex: Carbon

19. Halogens The group before last They have 7 valence electrons
Never found pure in nature because they are too reactive
They must be diatomic molecules to be found pure
Ex. Cholorine

20. Noble Gases 8 valence electrons; except helium it has 2
Only found pure in nature and are not reactive
Colorless and odorless
They were the last of the elements to be found.

21. Valence Electrons
The electrons that sit in the last energy level that are available for bonding.

22. The Periodic Table and Valence Electrons
Group 1 has one valence electron
Group 2 has 2 valence electrons available for bonding
Group 13 has 3 Valence electrons available for bonding
Group 14 has 4 valence electrons available
Group 15 has 5 valence electrons
Group 16 has 6 valence electrons
Group 17 has 7 valence electrons
Group 18 has 8 valence electrons that are not available to share.
Transition Elements have 1-2 valence electrons
Lanthanides (f block) also have 1-2 valence electrons

23. Bonds
Forces that hold groups of atoms together and make them function as a unit.
Ionic bonds give up electrons
Covalent bonds share electrons

24. Ionic Bonds Cation is a positively charged ion
Anions are negatively charged ions
This happens because in Ionic Bonds atoms give up or gain electrons in order to fill their outer energy shell
Metals tend to lose electrons to become positively charged
Nonmetals tend to gain electrons to become negatively charged.
When writing ionic formulas you need to write them with the charges and make sure that they are a balanced.
When you name ionic compounds the cation goes first and then the anion.
The anion normally will end in the suffix -ide

25. Covalent Bond One of the strongest bonds. Electrons are shared.
Only involved in nonmetals
The term molecule is exclusively used for covalent bonding
They follow the same rules about satisfying the need to fill the last electron shell.
Fluorine will give it up to anyone.
When writing or representing them bonds can be represented by dots : or with dashes –
Hydrogens and Halogens form one covalent bond
Oxygen and Sulfur form 2 covalent bonds ( either 1 double bond or 2 single bonds)
Nitrogen and Phosphorus form 3 covalent bonds (either 1 triple, 2 double and 1 single, or 3 single bonds)
Carbon and silicon form 4 covalent bonds

26. Lewis Structures for Covalent Bonds

27. Forming Covalent Bonds