1. Atomic Structure

2. The structure of the atom
The Ancient Greeks used to believe that everything was made up of very small particles. I did some experiments in 1808 that proved this and called these particles ATOMS:
Dalton
ELECTRON – negative, mass nearly nothing
PROTON – positive, same mass as neutron (“1”)
NEUTRON – neutral, same mass as proton (“1”)

3. The Atom
Electron
Nucleus
Shell or Orbit

4. Mass and atomic number 4 He 2 Particle Relative Mass Relative Charge
Proton 1
Neutron
Electron -1
MASS NUMBER = number of protons + number of neutrons He 2 4
SYMBOL
PROTON NUMBER = number of protons

5. How many protons, neutrons and electrons?1 11 16 H B O 1 5 8 23 35
238 Na Cl U 11 17 92

6. Horizontal rows are called PERIODS
Periodic table
Mendeleev
The periodic table arranges all the elements in groups according to their properties.
Vertical columns are called GROUPS
Horizontal rows are called PERIODS

7. Drawing Bohr Models

8. Bohr Models Bohr models are used to predict reactivity in elements.
Reactivity refers to how likely an element is to form a compound with another element.
When looking at Bohr models, we look at its valence electrons (the electrons on the last energy level) to determine reactivity.

9. Drawing Bohr Models Draw the nucleus.
Write the number of neutrons and the number of protons in the nucleus.
Draw the first energy level.
Draw the electrons in the energy levels according to the rules below. Make sure you draw the electrons in pairs.
Keep track of how many electrons are put in each level and the number of electrons left to use.

10. Rules for Energy Levels
Level 1 (closest to the nucleus) can hold a maximum of 2e.
Level 2 can hold a max of 8e.
Level 3 can hold a max of 18e.
Level 4 can hold a max of 32e.
You must fill one level before going on to draw the next level!

11. Guided Practice
In order to draw Bohr models of these elements, you must first determine the number of protons, neutrons, and electrons. Once you have found this information, follow the directions to draw your model. 6 6 6 6 C
Carbon
12.011
Protons: _____ Neutrons: _____ Electrons: ______
How many energy shells will this have? ____
How many valence (outer) electrons does this element have? ____
Bohr Model: 2 4

12. The Periodic Table
Fact 1: Elements in the same group have the same number of electrons in the outer shell (this correspond to their group number) H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg
These elements have __ electrons in their outer shells
These elements have __ electrons in their outer shell
E.g. all group 1 metals have __ electron in their outer shell

13. Quantum Mechanical Model of the Atom
The Quantum Mechanical Model is the current description of electrons in atoms.
- does not describe the electron’s path around the nucleus
The Quantum Mechanical Model is based on several ideas including:
Schrodinger wave equation (1926) treats electrons as waves.
Heisenberg uncertainty principle (1927) states that it is impossible to know both the velocity and position of a particle at the same time.

15. Where do electrons “live”? A. Principal Energy Levels
Principal energy levels n =1 to 7. (Row # on the periodic table)
The electron’s principal energy level is based on its location around the nucleus.
Electrons closer to the nucleus are at a lower energy level and have lower energy than those farther away from the nucleus

16. Energy levels are like rungs of a ladder
Energy levels are like rungs of a ladder. You cannot be in between a rung
Energy levels in an atom’s electron are unequally spaced. The higher energy levels are closer together.

17. B. Atomic Orbitals
An atomic orbital is a region of space in which there is a high probability of finding an electron
assigned letters s, p, d or f (smart people do fine)
Energy sublevels correspond to a shape where the electron is likely to be found.

18. s orbital (1) - spherical

19. p orbitals (3) – dumb-bell shaped

20. d orbitals (5)

21. f-orbitals (7)

22. Energy Levels, Sublevels, and Orbitals
Principal energy levels – n, assigned values 1-7 (Like floors in a hotel)
Energy sublevels- s, p, d, f (Type of suite in a hotel)
s sublevel – 1 orbital
p sublevel – 3 orbitals
d sublevel – 5 orbitals
f sublevel – 7 orbitals
Orbitals – Two electrons per orbital (Two people per room)
(Orbitals are like the number of rooms in a suite)

23. Electron Configurations
Electron configuration – the arrangement of electrons in an atom.
Example Sodium (Na) – 1s22s22p63s1
Three rules determine electron configurations
the Aufbau Principle,
the Pauli Exclusion Principle
Hund’s rule

24. The Aufbau Principle
Each electron occupies the lowest energy orbital available
Like filling the hotel from the bottom up

25. Aufbau Diagram
Which has a lower energy level 4s or 3d orbitals?

26. Filling the Orbitals in the correct order

27. Orbitals in the Periodic Table