SCIENCE 10: Chemical Reactions – Atomic Structure
1.
Terms:
a)
Periodic table:
b)
Atomic #:
c)
Atomic Weight (Mass #):
d)
Ion:
e)
Bohr Diagram:
2. How would you find out the number of ******** in an atom?
a)
Protons:
b)
Electrons:
c)
Neutrons:
3. Bohr Diagrams:
a)
1st orbit = 2 electrons maximum
b)
2nd orbit = 8 electrons maximum
c)
3rd orbit = 8 electrons maximum
d)
A lower orbit must be FULL before electrons can be placed into a
higher orbit
Example:
Carbon:
Magnesium:
4. Atomic Structure Chart: Complete the missing information in the chart



ELEMENT
Atomic #
Mass #
Hydrogen
SYMBOL
#
PROTONS
#
ELECTRONS
#
NEUTRONS
8
8
8
BOHR
DIGRAM
POSSIBLE
ION
Na
Cl1-
Fluorine
S
15
15
16
Li1+
5. Ionic Compounds: (p.192)
a)
Metals:
b)
Non-metals:
c)
Valence #:
Metals & non-metals combine to form ionic compounds.
Metals ions lose electrons to form positive ions.
Non-metals gain electrons to form negative ions.
The resulting compound must be electrically neutral: the positive charges must
equal the negative charges.
Example:
magnesium combines with chlorine to form the ionic compound magnesium chloride




Mg2+



and Cl1each magnesium ion gains 2 electrons
two chlorine ions are needed since each loses only 1 electron
result is MgCl2
2+
1-
?(2+) + ?(1-) = 0
Mg
Cl
1(2+) + 2(1-) = 0
MgCl2
 some metals can form more than one type of ion. A Roman numeral in round
brackets is used to show the charge on the metal ion. (p.195)
Example:
The element copper forms two different compounds with chlorine. Chlorine
always forms a 1- ion. Copper can form either a 1+ ion or a 2+ ion.
CuCl = copper (I) chloride
CuCl2 = copper (II) chloride
 Naming Ionic Compounds: (p.194)
o Metal name first, non-metal name second
o Change the ending of the non-metal to “ide”
6. Polyatomic Compounds: (p.196)
a)
polyatomic ion:
o A table of polyatomic ions can be found on your Periodic Table of Ions.
o If more than one polyatomic ion is needed to balance the positive and
negative charges, then the polyatomic ion is written in brackets and the
number placed after and lower.
o Don’t change the ending of the non-metal polyatomic ions.
Examples:
Calcium ions (Ca2+) combine with Carbonate ions (CO32-) to form
calcium carbonate CaCO3
Sodium ions (Na+) combine with Carbonate ions (CO32-) to form
Sodium carbonate Na2CO3
Calcium ions (Ca2+) combine with Chlorate ions (ClO3-) to form
Calcium chlorate Ca(ClO3)2
7. Molecular Compounds: (p.201)
a)
Ionic compound:
b)
Molecular compound:
c)
Covalent bond:
d)
Diatomic molecules:
 Prefixes are used when different molecular compounds can be formed by the
same elements:
Example:
1 carbon atom combined with 1 oxygen atom = carbon monoxide
1 carbon atom combined with 2 oxygen atoms = carbon dioxide
8. Predict the name and formula for each of the following pairs of elements:
a)
lithium & fluorine
l)
potassium & sulphate
b)
magnesium & chlorine
m)
nickel (II) & silicate
c)
zinc & bromine
n)
ammonium & oxygen
d)
aluminum & oxygen
o)
titanium (IV) & sulphite
e)
iron (III) & chlorine
p)
sodium & dihydrogen phosphate
f)
silver & phosphorus
q)
carbon & 1 oxygen
g)
tin (II) & oxygen
r)
carbon & 2 oxygen
h)
lead (IV) & bromine
s)
carbon & 4 fluorine
i)
copper (I) & sulfur
t)
sulfur & 3 oxygen
j)
sodium & acetate
u)
sodium & nitrate
k)
calcium & hydroxide
v)
sodium & nitrite