CHAPTER 4 Atomic Structure. Atoms An atom is the smallest particle of an element that retains its...
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Transcript of CHAPTER 4 Atomic Structure. Atoms An atom is the smallest particle of an element that retains its...
CHAPTER 4
Atomic Structure
Atoms
An atom is the smallest particle of an element that retains its identity in a chemical reaction.
History
Democritus (460-370BC): first suggested the existence of the atom
History
John Dalton (1766-1844): proposed the Atomic Theory: 1. All elements are made of atoms 2. Atoms of the same element are identical 3. Atoms of different elements can combine
to form compounds 4. Chemical reactions occur when atoms are
separated, joined, or rearranged
Size of the atom
One penny contains 2.4x1022 atoms of copper100,000,000 atoms in a row would be 1 cm
longAtoms can be seen with special microscopes
called scanning tunneling microscopes
Atomic Structure
An atom can be broken down into subatomic particles: protons, neutrons, and electrons.
Parts of an atom
The nucleus is the tiny central core of an atom containing protons and neutrons
Surrounding the nucleus is the electron field where electrons are located.
If an atom was the size of a football field, the nucleus would be the size of a marble located on the 50 yard line.
Subatomic Particles
Particle Symbol Location Charge Mass (g)
Electron e- orbital - 9.11 x 10-
28
Proton p+ nucleus + 1.67 x 10-
24
Neutron n0 nucleus 0 1.67 x 10-
24
Protons
Protons are positively charged subatomic particles located in the nucleus
Neutrons
Neutrons are subatomic particles with no charge, equal in size to protons, and found in the nucleus.
Electrons
Electrons are negatively charged subatomic particles, which are very small, and orbit the nucleus.
Important Scientists
J.J. Thomson (1897) discovered electrons using a cathode ray tube.
Cathode Ray Experiment
Important Scientists
Ernest Rutherford (1911) discovered protons through his gold foil experiment.
Gold Foil Experiment Animation
Reading and Writing in Science
1. Read pages 100-108 in the red textbook
2. Answer questions 1-14 on pages 103 and 108. Write and answer these questions in your notebooks.
Next notebook collection date is October 30.
Distinguishing Among Atoms
Atoms of an element are different because they contain different numbers of protons.
The atomic number of an element is the number of protons an atom of that element has.
Practice
How many protons does each element have?
Hydrogen CarbonNitrogenPotassiumGold
Practice
How many protons does each element have?
Hydrogen = 1 Carbon = 6Nitrogen = 7Potassium = 19Gold = 79
Mass Number
The other number on the periodic table is an atom’s mass number which is the sum of protons and neutrons.
What is the mass number of:Hydrogen Carbon NitrogenPotassiumGold
Mass Number
The other number on the periodic table is an atom’s mass number which is the sum of protons and neutrons.
What is the mass number of:Hydrogen (1.0079) Carbon (12.011)Nitrogen (14.007)Potassium (39.098)Gold (196.97)
Neutrons
To determine the number of neutrons an atom has, you subtract the atomic number from the mass number, then round to the nearest whole number.
How many neutrons are found in:HydrogenCarbonNitrogenPotassiumGold
Neutrons
To determine the number of neutrons an atom has, you subtract the atomic number from the mass number, then round to the nearest whole number.
How many neutrons are found in:Hydrogen = 0Carbon = 6Nitrogen = 7Potassium = 20Gold = 118
Electrons
In a neutral atom, the number of electrons is equal to the number of protons, which is equal to the atomic number.
How many electrons does each atom have?HydrogenCarbonNitrogenPotassiumGold
Electrons
In a neutral atom, the number of electrons is equal to the number of protons, which is equal to the atomic number.
How many electrons does each atom have?Hydrogen = 1Carbon = 6Nitrogen = 7Potassium = 19Gold =79
Determining subatomic particles
Particle Number
Protons Atomic Number
Electrons
Atomic Number
Neutrons
Atomic mass – atomic number
Isotopes
Isotopes are atoms that have the same number of protons but different numbers of neutrons (and therefore different mass numbers).
Isotopes
The most well known isotope is Carbon-14. Regular Carbon is called Carbon-12, because
its mass number is 12, and it has 6 neutrons.Carbon 14 has 8 neutrons (14-6).It is used for radioactive dating of fossils.
Getting to know the Periodic Table
You should memorize the names and symbols of common elements on the periodic table.
Complete the activity to help you get to know the elements of the periodic table.
History of Atomic Models
Over time, scientists proposed different models of atoms, each better than the last.
Rutherford said that positive protons were in the nucleus, and electrons orbited it.
Atomic Models
Bohr stated that the nucleus had positive protons, and electrons orbited in fixed shells.
Atomic Models
Schrodinger proposed the quantum mechanical model, which is still used today.
It states that there are protons and neutrons in the nucleus, which is surrounded by an electron cloud showing the probability of electron location.
Electrons
Electrons are found outside the nucleus in shells/orbitals/energy levels.
Energy Levels
The number of electrons allowed in each energy level is:
Energy Level (n) Maximum Number of Electrons
1 2
2 8
3 18
4 32
Placing electrons
Each energy level must be full before electrons can be placed in the next level up.
Example: Draw an atom of Lithium
Lithium
Practice
Draw an atom of Sodium.
Sodium
Practice
In your notebooks, draw the first 30 atoms. Name each one, and place the correct numbers of protons, neutrons, and electrons in each.
This is what your quiz will be like (Tuesday for periods 5 and 7, Wednesday for period 2)