web Date:
___________________________
Physical
Chemical
Property
Change
1. Fill in the following table with the correct definition and two examples for each box:
2. A pure substance that cannot be broken down into simpler substances is a (n) ______________________________.
3. The electrons in the outer orbit of an atom are responsible for the elements _________________________________.
4. Atoms with a full (2 or 8 electrons) outer orbit are ________________________.
5. Electrons in an atom’s outer orbit are termed ________________________ electrons.
6. Atomic Mass = __________________________ + __________________________
7. Atomic Number = _______________________ and ___________________________
8. Fill in the table below:
Element
Sodium
# Protons
# Electrons
# Valence Electrons
Chlorine
Beryllium
Fluorine
Lithium
Oxygen
Phosphorus
9. Draw the Bohr-Rutherford and Lewis diagrams for magnesium and fluorine.
Ionic Charge
10. A (n) _____________________ is an electrically neutral particle with an equal number if protons and electrons.
11. _______________________ tend to gain electrons.
12. _______________________ tend to lose electrons.
13. An atom that gains one or more electrons will have a _________________________ charge.
14. An atom that loses one or more electrons will have a _________________________ charge.
15. An atom that gains or loses one or more electrons is called a (n) _____________________.
16. Draw a Bohr-Rutherford diagram for an atom, and an ion of each of the following elements:
Lithium
Nitrogen
Helium
Oxygen
17. A positive ion is called a _______________________.
18. A negative ion is called a (n) ________________________.
Ionic Bonding
1. An ionic bond forms between a __________________ and a ______________________.
2. Look at each of the following pairs of elements, and explain whether they would form an ionic bond:
a) Mg, O _________________________________________________________________________________
b) Zn, Cl _________________________________________________________________________________
c) C, F ___________________________________________________________________________________
d) H, F ___________________________________________________________________________________
3. This type of bonding involves the _______________________ of electrons from one atom to another.
4. A ________________________ion is made up of more than one atom that acts as a single particle.
5. Write the chemical formula for each of the polyatomic ions in the table below:
Phosphate
Carbonate
Chlorate
Sulfate
Hydroxide
Nitrate
Molecular (Covalent) Bonding
1. This type of bonding involves the ____________________________ of electrons between two or more atoms.
2. A molecular bond forms between a _________________________ and a ________________________________.
3. Molecular compounds are made of ____________________________ that are joined by covalent bonds.
4. Molecule consisting of only two atoms of the same or different elements is called _________________________.
5. List the diatomic molecules: ______________________________________________________________________________________.
Let’s Put it All Together Now!!!
1. Identify each of the compounds as one of the categories below, and write its chemical name:
A) Simple Ionic Compound
B) Tricky Metal Ionic Compound
C) Polyatomic Ionic Compound
Chemical Formula
Ba(OH)2
N2 (g)
Fe(OH)3
MgCl2
AlF3
NI3
Li2(C03)
PbO2
NaOH
Br2(g)
Sn(NO3)2
CaCO3
FeCl3
Category (A-F)
D) Polyatomic IC with a Tricky Metal
E) Molecular Compound
F) Diatomic Molecular Compound
Chemical Name
Sr(ClO3)2
2. Identify each of the compounds as one of the categories above, and write its chemical formula:
Chemical Name
Lithium oxide
Carbon tetrabromide
Hydrogen sulphide
Calcium nitrate
Diboron hexahydride
Nitrogen gas
Potassium chloride
Calcium carbonate
Silver carbonate
Ammonium nitrate
Nitrogen monoxide
Potassium carbonate
Silver bromide
Calcium iodide
Barium hydroxide
Sodium bicarbonate
Iron (II) sulfate
Carbon tetrafluoride
Lead (II) phosphate
Sulphur hexachloride
Category (A-F)
Chemical Formula
Carbon monoxide