1. Chapter 20
Chemical Bonds

2. Stability In Bonding
Roughly 110 elements on the periodic table can form a nearly infinite number of compounds
Elements bond with each other, seeking stability
Only one group of elements (Noble Gases) are stable without bonding
All others must bond with either another atom of the same element or a different element to be stable

3. Combined Elements Elemental copper is a shiny metal
The Statue of Liberty is copper, why is she a pale green color?
The copper that the statue is made of reacted with oxygen and sulfur to form a compound called copper sulfate, that has its own properties

4. Combined Elements
Sodium (Na) is a soft, silvery metal that is highly reactive– it actually catches fire in the presence of oxygen
Chlorine (Cl) is a green poisonous gas.
Together, they make a compound that you can put on your food, table salt, NaCl
Table salt’s compound name is Sodium Chloride

5. Chemical Formulas
A chemical formula tells what elements are in a compound, and in what numbers
Subscripts (a number written below) show how many atoms are in each compound.
If there is no subscript, you can assume it is 1
Example, H2O, water, has two atoms of Hydrogen and one atom of oxygen

6. Some Familiar Compounds

7. Atomic Stability
An atom is considered stable if its outer shell electrons are full
This is considered an “Octet”, because 8 electrons fill the outer shell of some atoms
Outer shell electrons are called “valence” electrons and are the electrons that are involved in bonding

9. Dot Diagrams
Uses dots around the chemical symbol to show number of valence electrons

10. Dot Diagrams, Cont Write the symbol of the element
Look at the periodic table and determine the number of outer shell, or valence electrons
Start on the top, put one dot on each side as you move clockwise
Exceptions: He (helium) has a full shell at two electrons, so put those dots on top
Group 1: Alkali metals (including H) put the one dot to the right

11. Stability is Reached
Atoms form chemical bonds with each other to reach chemical stability– to fill up their outer shells
They will either give away, take, or share electrons to do this

12. Types of Bonds When atoms gain or lose an electron, they become an ion
A positive ion, such as Ca +2, gives away 2 electrons
A negative ion, such as Chlorine -1, gains one electron
A bond where electrons are transferred, (given or taken) is called an IONIC bond

13. Ionic Bonds
Ionic bond is the force of attraction between opposite charges in an ionic compound
For the most part, ionic bonds are formed by elements that are far apart on the periodic table
A metal and a non-metal
Metals tend to lose electrons
Non-metals tend to gain electrons
Once ionic bonds are formed, the resulting compound has a net charge of zero

14. Sharing Electons
Non metals, when bonding with other non metals, are unlikely to gain or lose electrons
The attraction that forms between atoms when they share electrons is called a covalent bond
A neutral particle that forms due to a covalent bond is called a molecule

15. Types of Covalent Bonds
Single covalent bonds share one pair of electrons, example is water H2O this is called a single bond
A multiple covalent bond shares two or three pairs of electrons, called a double or a triple bond, example N2
Covalent bonds form between non-metals
Many covalent compounds are liquids or gases at room temperature

16. Bond Types

17. Polar vs Non-Polar
Polar covalent compounds are molecules that have ends that have partial opposite charges
This means that the electrons are shared unevenly
One atom has a greater “pull” on the shared electrons than another
A non-polar compound mean that the electrons are shared evenly with no partial charges

18. Polar vs. Non Polar
Carbon Tetrachloride is non-polar
Water is Polar

19. Diatomic Atoms
Some atoms are so reactant that they can’t exist as only one atom
They must bond with themselves in order to reach stability
They are called “diatomic” which literally means “two atoms”
The diatomic atoms are: Nitrogen, Oxygen, Fluorine, Chlorine, Iodine, Hydrogen, Bromine
Magic 7- they make a 7 and then add hydrogen
They are all written with a subscript: Cl2

20. Diatomic Atoms

21. Binary Ionic Compound
A binary ionic compound is one that consists of two elements bonded together where electrons are transferred
You need to know what elements are involved and how many electrons are gained or lost
The element’s OXIDATION NUMBER tells how many electrons are transferred when ions are formed
Oxidation numbers are often referred to as “charge”

22. Oxidation Numbers

23. Special Ions- have more than one oxidation number

24. Compounds are Neutral
When compounds are formed, their net charge must be zero
Therefore, when you are putting compounds together and writing their formulas, their oxidation numbers must equal zero
Sodium (Na +1) and Chlorine (Cl -1) together are NaCl
Magnesium (Mg +2) and Chlorine (Cl -1) together are MgCl2
It takes two chlorine atoms to cancel out the +2 charge of Mg to zero
Criss-Cross method

25. Naming Ionic Compounds
Step 1: Write the name of the positive ion
Step 2: Determine if the positive ion has a special oxidation number (refer to table 2.) If it does, you’ll have to determine its oxidation number and write roman numerals after the name
Step 3: Write the root of the negative ion (chlor-, ox-, phosph-)
Add –ide to the end of the root of the negative ion

26. Naming Ionic Compounds
NaCl
Step one: Sodium
Step two: not needed, it only has one possible oxidation number
Step three: Sodium Chlor-
Step four: Sodium Chloride
Now, you do MgI

27. Naming Compounds with polyatomic ions
A polyatomic ion is a special ion that is made of many atoms
Look at the chart to the right
To write the names of a special compound with polyatomic ion, you write the name of the positive ion and then the name of the polyatomic ion
Ex K2SO4 is potassium sulfate

28. Naming Covalent Compounds
Naming covalent compounds uses prefixes that tell how many of the atoms are present in the molecule
Often the prefix for one, mono is omitted but is used for emphasis in some cases

29. Naming Covalent Compounds
CO is Carbon Monoxide
CCl4 is Carbon Tetrachloride
H2O is Dihydrogen Monoxide
Your Turn
NO2
N2O5