1. Atomic Structure
Applied Chemistry

2. Modern Atomic Theory Three subatomic particles:
protons (p+), neutrons (n0), and electrons (e-)
Particles found IN the nucleus:
protons and neutrons
These are called nucleons
Particles found OUTSIDE the nucleus:
electrons in the electron cloud

4. Relative Mass and Charge of Subatomic Particles
Mass (amu)
Charge
Proton
Neutron
Electron 1 +1 1 -1
Note: amu = atomic mass unit (1/12 the mass of a carbon atom)

5. Modern Atomic Theory Atomic Number = # of p+1
ALWAYS equals the number of protons (p+)
Identifies the element
Mass Number = # of p+ + # of n0
Equals the number of protons plus neutrons
Neutral atoms: # of p+ = # of e-
In neutral atoms, the # of protons equals the # of electrons

6. Boxes on the Periodic Table
For Hydrogen with a Mass Number = 1
# of protons = # of neutrons =
# of electrons = 1
1.008
Atomic Mass H
Atomic Number
Hydrogen
Element Name
Element Symbol 1 1

7. Why aren’t atomic masses whole numbers?
Neutral atoms of an element have the same number of protons, but the number of neutrons can vary.
Isotopes: Atoms of an element with the same number of protons, but different number of neutrons. (Atoms of the same element with different masses.)
Atomic Mass is really the average atomic mass of all the isotopes. Mass number and Atomic Mass are NOT the same!!!

8. Isotopes of Hydrogen

9. Isotopic Name – (2 parts)
Sodium - 23
Element
(Name or symbol can be used)
Mass number

10. Example 6 6 6 8 8 8 9 9 10 Element Protons Electrons Neutrons
Carbon-12
Oxygen -16
Fluorine -19 6 6 6 8 8 8 9 9 10

11. How are isotopes expressed?
Isotopic Symbol – shows symbol for an element, the mass number, and the atomic number.
Mass Number
Atomic Number

12. Example of Isotopic Symbol
Element is Neon
Mass number is 20
Atomic Number is 10
# of protons is 10
# of neutrons is 10
# of electrons is 10

13. Example Chart 3 7 3 4 3 17 37 17 20 17 56 137 56 81 56 Isotopic Symbol
Isotopic Name
Atomic Number
Mass Number
# of protons
# of neutrons
# of electrons
Lithium-7
Chlorine-37
Barium-137 3 7 3 4 3 17 37 17 20 17 56
137 56 81 56

14. Are atoms always neutral?
When atoms have a charge, they are called ions.
This charge is due to an UNEQUAL number of protons and electrons.
Charge = protons - electrons

15. Ions (cont.) Metals tend to lose electrons and have a positive charge.
Positive ions are called cations.
The name of the cation is the same name as the element followed by the word ion.
Ex. Sodium ion

16. Ions (cont.)
Nonmetals tend to gain electrons and have a negative charge.
Negative ions are called anions.
The name of an anion uses the element name but the ending is changed to ide.
Example: chloride

17. CATION
Ca†ion
“cat”ion
ANION
anion
“ant”ion

18. Example of Ions Fluorine-19 becomes an ion by gaining 1 electron.
As a result, it will have 9 protons and 10 electrons.

19. IONS
Isotopic Symbol
Proton
Neutron
Electron
Mass #
Charge
Cation or Anion 16 18 28 59 +2 9 10 10 19 -1 A 12 12 10 24 +2 C 32 -2 A 31 26 C

20. Where are the electrons in the electron cloud?
Electrons are in energy levels.
The outermost electrons are called valence electrons. They are in the highest energy level.
The electrons in their lowest energy level are in the ground state. + e-
nucleus

21. Where are the electrons in the electron cloud?
Electrons can absorb energy often from heat or electricity.
When electrons absorb energy, they become excited. They jump up to a higher energy level.
They are not stable at the higher energy level.
This is called the excited state. + e-
absorb energy

22. Where are the electrons in the electron cloud?
Because electrons are not stable, the electrons fall back to a lower energy level, called the ground state.
It releases (or emits) energy, in the form of electromagnetic radiation when it returns to the ground state. + e-
emitted energy

25. electrons fall to n = 1 and give off ultraviolet light.
electrons fall to n = 2 and give off visible light.
electrons fall to n = 3 and give off infrared light.
Hydrogen Atom