5.2 The Structure of the Atom

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Presentation transcript:

5.2 The Structure of the Atom

The Atom Protons (p+) Electrons (e-) Neutrons (no) The atom is made up of three subatomic particles: Protons (p+) Electrons (e-) Neutrons (no)

The protons and neutrons are found in the nucleus at the centre of the atom. The electrons are found “orbiting” around the nucleus in specific energy levels.

The Subatomic Particles Location Charge Mass Proton nucleus +1 1 Electrons outer shells -1 Neutrons

Standard Atomic Notation Shows: Atomic number the number of protons in the nucleus of an atom The atomic number identifies the atom as a particular element Mass Number The number of protons and neutrons in an atom

Uses a standard symbol to represent the element (ex Uses a standard symbol to represent the element (ex. H for hydrogen, Li for lithium)

The Atom Calculating the Number of Subatomic Particles: Atomic number = number of protons Mass number = number of protons + number of neutrons Number of neutrons = mass number – atomic number Number of protons = number of electrons (neutral atom)

Activity 5-4, p. 189 Read the activity and complete #1-4 NOTE: for number 3, do not use Appendix A, instead use the periodic table on p. 197, the mass number is the number under the symbol, rounded. Ex. zinc 65.4 = 65.

Answers to Activity 5-4 1. carbon = C, hydrogen = H, nitrogen = N Rule: use the first letter (capital) of each element 2. a. Calcium = Ca, use the first two letters, first letter only capitalized. b. C cannot be used as it is already used for carbon 3. silver (argentum) = Ag, gold (aurum) = Au, copper (cuprum) = Cu, iron (ferrum) = Fe, mercury (hydrargyrum) = Hg, lead (plumbum) = Pb, tin (stannum) = Sn Identify rules…. 4. Next slide…

Name of Element Atomic Number Mass Number 126C Carbon 6 12 6530Zn zinc Standard Atomic Notation Name of Element Atomic Number Mass Number Number of Electrons Number of Protons Number of Neutrons 126C Carbon 6 12 6530Zn zinc 30 65 35 Sulfur 16 Calcium 40 20 nitrogen 7 14

Bohr Rutherford Diagrams Show the quantities and locations of protons, electrons and neutrons in an atom (used for the 1st 20 elements) Atomic Number = # of protons # of neutrons = Mass Number – Atomic Number # of electrons = # of protons in a neutral atom For an atom of Helium: Atomic # = # of protons = 2 = 4 - 2 = 2 # of electrons = # of protons = 2

Bohr-Rutherford Diagram for He helium 2e- # of electrons in 1st orbital (energy level) Max = 2 2p+ 2n° # of protons (p) # of neutrons (n) Nucleus

Bohr-Rutherford Diagram for K Potassium 1e- # of electrons in 4th orbital (energy level) Max = 8 8e- # of electrons in 3rd orbital (energy level) Max = 8 8e- # of electrons in 2nd orbital (energy level) Max = 8 2e- # of electrons in 1st orbital (energy level) Max = 2 19p+ 20n° # of protons (p) # of neutrons (n) Nucleus

Isotopes Most atoms of an element have the same number of neutrons A few will have a different number of neutrons Ex. Most Li atoms have 3 protons and 4 neutrons Mass Number = 7 Some have only 3 neutrons Mass Number = 6 Atoms that have the same number of protons but different numbers of neutrons are called isotopes.