1. Atomic Structure
Advanced Chemistry
By PresenterMedia.com

2. Elements and Compounds
Simplest form of matter
Cannot be broken down into smaller stable state of matter
Compounds
Combination of elements in whole number ratios
Can be broken down into smaller components

3. Every substance has unique physical and chemical properties
Properties of Matter
Physical Properties
Chemical Properties
Can be observed/measured without changing the composition.
Examples are density, solubility and state of matter
Intensive do not depend on amount (density and boiling point)
Extensive do depend on amount (mass, volume)
Can only be observed with a change in the composition
Examples are rusting and flammability
Every substance has unique physical and chemical properties

4. Changes in Matter Physical changes
Change in a substance that results in different appearance but not composition
Examples are bending and change in state of matter
States of matter
All particles in constant motion
Solids have a definite shape and volume
Liquids have a definite volume but not a definite shape
Gases have neither a definite shape nor a definite volume
Chemical changes (chemical reactions)
Change in a substance that results in one or more new substances
Indicators are smoke, heat, light, odor
Initial materials are reactants; final materials are products

5. Laws of Chemistry
These laws help to explain the behavior of atoms during chemical reactions (changes)
Law of Conservation of Mass
Matter cannot be created or destroyed but can change forms
Law of Definite Proportions
A chemical always has the same whole number ratio of elements to one another
Law of Multiple Proportions
Elements can combine in different whole number ratios to make different chemicals

6. Dalton’s Atomic Model True False
All matter is composed of extremely small particles called atoms
All atoms of a given element are identical, having the same size, mass and chemical properties. Atoms of specific elements are different from any other element
Atoms cannot be created, divided, or destroyed
Different atoms combine in small whole number ratios to form compounds
Atoms are separated, combined, and rearranged in reactions
True
False

7. Atomic Structure Discovery
Early experiments
Thompson
Cathode ray tube
Discovered electrons (1st subatomic particle)
Plum pudding model/chocolate chip cookie dough ice cream
Rutherford
Gold foil experiment
Discovered nucleus
Later discovered protons

8. Basic Atomic Structure
Nucleus
Central dense region of an atom with two subatomic particles
Positively charge subatomic particle
Protons
Neutrons
Subatomic particle without a charge
Empty space surrounding the nucleus of an atom
Electron cloud
Electrons
Negatively charged subatomic particle

9. Atomic Differences Atomic number
Identifies the atom as a specific element
Indicates the number of protons
In a neutral atom, protons = electrons
Mass number
Indicates the number of protons and neutrons
Atoms with same number of protons but different number of neutrons are isotopes
Atomic mass number
Weighted average of mass of all isotopes

10. Radioactivity Nuclear reaction involving a change to the atom
Atom becomes more stable/less energy
Radiation is emitted
Alpha (a) particle– Helium nucleus
Beta (b) particle – neutron splits
Gamma (g) ray – energy released usually with an alpha or beta particle

11. Bohr Proposed energy states are involved with atoms
Ground state is lowest energy for an atom
Excited state is energy is gained by the atom
Also proposed atomic orbitals
Electrons travel around the nucleus
Assigned quantum numbers to each energy level
One is closest to the nucleus, then two, etc
Electrons can move from energy level to energy level
de Broglie – Wave Particle Duality
Heisenberg Uncertainty Principle
Impossible to know velocity and location of an electron at the same time

12. Atomic Orbitals Area around nucleus indicating location of electrons
Principal quantum numbers/Energy levels
Indicate size and energy of atomic orbitals
Numbered from 1 to 7
Energy sublevels are found in the energy levels
Are s, p, d, or f as determined by their shape (p. 133)
Each sublevel has orbitals holding two electrons each
s has one orbital
p has three orbitals
d has five orbitals
f has seven orbitals
Energy level 1 has 1 sublevel, 2 has 2 sublevels, 3 has three sublevels, 4 has 4 sublevels

13. Electron Configurations
Arrangement of electrons in an atom
Three rules define location
Aufbau principle
Electrons occupy lowest energy position (p. 138)
Each orbital in a sublevel has the same energy
Orbitals of different energy levels can overlap
Pauli exclusion principle
Electrons spin and in an orbital they are opposite
Hund’s rule
Negative charge plays a role in location
One electron per orbital before a second one fills
Exceptions are possible (d block)

14. Electron Configurations (cont)
Notations
Electron configuration notation
Uses energy level, sublevel and number of electrons
1s2 2s2 2p3 is nitrogen
Orbital diagram
Box represents each orbital with energy level and sublevel written below it
Electrons are represented with opposite arrows

15. Valence Electrons Electrons in the outermost energy level
Determine the properties of an atom
Determine position on periodic table
Noble gases have full outer energy levels (most stable elements)
Electron Dot Structures
One dot for each valence electron
Fill on sublevel at a time

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