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Atomic Theories and Models
The Story of the Atom
The physical theory
of the _________,
__________, and
__________ of the
atom
John Dalton
Law of Conservation of Mass
Subatomic Particles
(Protons, Neutrons, and Electrons)
Subatomic Particles
Name
Symbol
Relative Mass
(Atomic Mass Unit, AMU)
Electric
Charge
Location in
the Atom
Note: 1 atomic mass unit = 1.66053886 × 10-27 kg = one-twelfth of the mass of the nucleus of a
carbon-12 atom.
Atomic Number (Z)
Proton number
• The number of __________ found in the nucleus of an atom
• Atoms have no overall electric charge (i.e. charge of atom is zero)
Atomic Number=
=
• If a proton (
) is added to an element’s nucleus, a _______
element will be produced.
• e.g.
1
19
+ 1

9
F
p
Mass Number (A)
Atomic mass number or nucleon number
• The number of nucleons (________________________) in an
atomic nucleus
Mass Number=
Atomic Mass
Average mass of an element’s isotopes
•
Since most of the mass of an atom is concentrated in the
__________ and ___________ located in the nucleus, the atomic
mass is ________________ to the mass number.
• Recall, mass number =
• Atomic Mass  Mass Number


# of neutrons =
• If a neutron (
) is added to an element’s nucleus, a heavier
version of the _________ element (isotope) will be produced.
• e.g.
19
+ 1

9
0
F
n
Isotopes
• Atoms having the same _________________ but different
_______________ (because different number of __________).
• E.g. Hydrogen isotopes
Hydrogen-1 (hydrogen)
Hydrogen-2 (deuterium)
Hydrogen-3 (tritium)
Ions
• Most atoms are capable of either _________ or ________ electrons.
• A few elements, like hydrogen, are able to do both!
• They can do this by ____________ electrons from, or ________
electrons to, other atoms.
• Atoms that have gained or lost electrons are called ______.
Ions (continued…)
An ion is an electrically __________ atom (or groups of atoms):
i) ____________ - charged ion: when electron(s) is/are added to a
neutral atom (i.e. there are _______ electrons than protons).
_____________ tend to gain electrons and become negatively
charged.
ii) ___________ - charged ion: when electron(s) is/are removed to a
neutral atom (i.e. there are ________ electrons than protons).
________ tend to gain electrons and become negatively charged.
Ions (continued…)
Chemical Equations
Depict the kind of _________ and ________ and their relative
amounts in a reaction.
2 Al(s) + 3 Br2(l)  Al2Br6(s)
The numbers in the front are called _____________.
The letters (s), (g), and (l) are the physical states of
compounds.
Chemical Equations
Symbolic equation:
2 Al(s) + 3 Br2(l) ---> Al2Br6(s)
Balancing Chemical Equations
Example: CH4
+
O2

CO2
+
H2O
Example: CH4
+
O2

CO2
+
H 2O
The chemical equation for the reaction of methane and oxygen
is ______ yet properly balanced because the atoms of the
elements on the product side do not ______ the atoms of each
element on the reactant side of the equation. The
_________________________, which states that matter can
neither be ________ nor __________ in an ordinary chemical
reaction, must be upheld when writing a chemical equation. This
chemical equation is ___________.
Balancing Chemical Equations
Example: CH4
+
O2

CO2
+
Rewrite and balance the equation below.
H2O
Balancing Chemical Equations
Balancing the following equations using atomic models.
1. K+ Cl2  KCl (draw)
2. N2 + H2  NH3 (draw)
3. Fe + Cl2  FeCl3 (draw)
4. Zn + HCl  ZnCl2 + H2 (draw)
Balancing Chemical Equations
1. K+ Cl2  KCl
2. Ba + Br2  BaBr2
3. N2 + H2  NH3
4. H2 + O2  H2O
5. Na + N2  Na3N
6. NaCl + F2  NaF + Cl2
7. AgNO3 + MgCl2  AgCl + Mg(NO3)2
8. CH4 + O2  CO2 + H2O
9. ZnO + HCl  ZnCl2 + H2O
10. I2 + NaBr  NaI + Br2
Write the word equations below as chemical equations and balance.
1. Zinc and lead (II) nitrate yield zinc nitrate and lead.
2. Potassium chlorate when heated yields potassium chloride and
oxygen gas.
3. Copper and sulfuric acid yield copper (II) sulfate and water and
sulfur dioxide.
4. magnesium chloride + ammonium nitrate  magnesium nitrate +
ammonium chloride
5. iron (III) chloride + potassium hydroxide  potassium chloride +
Iron (III) hydroxide
6. sodium nitrate (heated)  sodium nitrite + oxygen
7. potassium phosphate + magnesium chloride  magnesium
phosphate + potassium chloride
8. mercury (II) hydroxide + hydrogen phosphate (phosphoric acid)
 mercury (II) phosphate + water
9. carbon dioxide + carbon  carbon monoxide
10. ammonium chloride + sodium nitrite sodium chloride +
nitrogen + water
On a separate piece of paper, write the following equations and balance them.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
zinc + hydrochloric acid (HCl)  zinc chloride + hydrogen
calcium oxide + water  calcium hydroxide
mercury (II) oxide  mercury + oxygen
hydrogen + chlorine  hydrogen chloride
aluminum + chlorine  aluminum chloride
iron (II) oxide + carbon  iron + carbon monoxide
aluminum + copper (II) sulphate  aluminum sulphate + copper
aluminum + tin (IV) chloride  aluminum chloride + tin (II) chloride
sodium hydroxide + hydrogen bromide  sodium bromide + water
sulphuric acid + sodium hydroxide  sodium sulphate + water
silver nitrate + sodium chloride  silver chloride + sodium nitrate
12. calcium hydroxide + nitric acid  calcium nitrate + water
13. hydrochloric acid (HCl) + magnesium hydroxide  magnesium chloride +
water
14. phosphoric acid (H3PO4) + magnesium hydroxide  magnesium phosphate +
water
15. carbon dioxide + calcium hydroxide  calcium carbonate + water
16. hydrochloric acid (HCl) + magnesium oxide  magnesium chloride + water
17. hydrochloric acid (HCl) + magnesium  magnesium chloride + hydrogen
18. carbon + oxygen  carbon dioxide