Chapter 13 Section 1 – Electrons and Chemical Bonding
Chemical Bonding:
the ________________________ of atoms to form ________________________
substances.
Chemical Bond: a force of ________________________ that holds ________________________ atoms
together
**** Involves the electrons! *****
Theory of Chemical Bonding

The number of _____________________ an atom has is the key

The ___________________ energy level ________________________ determine the chemical bonds
formed

How many electrons in each level: 1st ______, 2nd ______, 3rd(1st time)_____, 4th (1st time)_____, 3rd(2nd
time)_____, 4th (2nd time)_______
Valence Electrons: ________________________ in the ________________________ energy level of an
atom
Examples:
Oxygen
Sodium
Atomic Number: ______
Atomic Number: ______
Number of Electrons: ______
Number of Electrons: ______
First level: ______
First level: ______
Second level: ______
Second level: ______
Valence Electrons: ______
Third level: _____
Valence Electrons: ______
Chapter 13 Section 2 Notes: Types of Chemical Bonds
Electron Dot Diagrams or Lewis Dot Structure:
Shows only the _________________ _____________ in an atom.
Examples:
Hydrogen:
Neon:
H
Practice:
1. Calcium
Carbon:
Ne
C
4. Aluminum
7. Helium
2. Potassium
5. Bromine
8. Oxygen
3. Argon
6. Nitrogen
9. Phosphorous
Ionic Bond: Force of attraction between _________________ charged ions; formed when
atoms _____________ or ______________ electrons.
Ions: ________________ particles that form during chemical changes when one or more
_______________ electrons ____________ from one atom to another.
Transfer of Electrons: When an ______________ leaves or comes to an atom, the charge
____________, for the atom; thus becoming an ______________.
• Atoms that ______________ electrons form _______________ ions (have
____________ charge).
• Atoms that ____________ electrons form ________________ ions (have a ___________
charge).
Element
# of
Protons
# of
Electrons
Charge
Type of Ion
(+/-)
H
1
0
+1
+
C
6
4
O
8
-2
-
Na
11
+1
+
___________ is needed to remove electrons from metal atoms to form ___________ ions.
Energy is released when most _______________ gain electrons to form negative ions.
Charged ions bond with each other to form compounds with a _______________ charge!
Examples:
1. Sodium (Na) and Chlorine (Cl)
Electron Dot Diagram
Criss Cross Method
2. Calcium (Ca) and Bromine (Br)
Electron Dot Diagram
Criss Cross Method
3. Magnesium + Iodine
Electron Dot Diagram
4.
Potassium + Fluorine
Electron Dot Diagram
5.
Criss Cross Method
Criss Cross Method
Sodium + Oxygen
Electron Dot Diagram
Criss Cross Method
Covalent Bonds: force of _________________ between the ________________ of atoms
and the ______________ shared by the atom;
• The _______________ are _______________ between the atoms.
• Covalent bonds are formed between a _________________ and a
__________________.
Examples:
Hydrogen + Oxygen
Element
Hydrogen
# of
Protons
# of
Electrons
# of
Valence
Electrons
# of
Electrons
to fill
Outer shell
# of
Covalent
Bonds
made
Carbon
Chlorine
Hydrogen
Phosphorus
Oxygen
Sulfur
Nitrogen
Practice:
1. Nitrogen and Oxygen
3. Phosphorus and Bromine
2. Carbon and Hydrogen
4. Carbon and Oxygen
Molecule: a ________________ group of atoms held together by ________________ bonds.
A __________________ is the ________________ particle into which a ________________
bonded compound can be ___________________ and still be the same compound.
Diatomic Molecule:
Consists of ______________ of the atom bonded together
Simplest _______________ covalently bonded together
Examples: O2, H2, Cl2, N2
Metallic Bond: the force of _____________ between a _________________ charged metal ion
and the _______________ in a metal.
• __________________ move throughout the metal
• The metallic bonds extend _____________________ the metal in all
_______________.
This is what allows the metal to be _____________, _______________ ect.
Practice:
Classify each of the following compounds as ionic (metal + nonmetal) or as covalent (nonmetal
+ nonmetal).
1. CaCl2 ___________________
2. CO2 ___________________
3. H2O ___________________
4. K2O ___________________
5. NaF ___________________
6. CH4 ___________________
7. SO3 ___________________
8. LiBr ___________________
9. MgO ___________________
10.HCl ___________________
11.KI ___________________
12.NO2 ___________________
13.FeCl3 ___________________
14.P2O5 ___________________
15.N2O3 ___________________
16.CaBr2 ___________________
17.SO2 ___________________
18.NaCl ___________________
19.K2S ___________________
20.PCl3 ___________________
Counting the Number of Atoms
For the following compounds count how many atoms of element are in the compound and how many total
atoms are in the compound.
Compound
Number of each atom
Total number of atoms
in the compound
KClO3
C6H12O6
MgBr2
Mg(NO3)2
Al2(SO4)3
Extra Practice:
1. An ionic bond is between a ________________ and a ______________.
2. A covalent bond is between a ______________________ and a _________________.
3. Give the oxidation number for the following elements:
a. Sodium ______
e. Nitrogen ______
b. Calcium ______
f. Sulfur ______
c. Aluminum ______
g. Fluorine ______
d. Lead ______
4. Show the ionic bond that will occur using both methods:
Magnesium and Phosphorus
Electron Dot Diagram:
Criss Cross
5. Show the covalent bond that will occur.
Phosphorus and Hydrogen