1. Chapter 4: Atomic Structure

2. 4.2 – The Structure of an Atom

3. Subatomic Particles
Protons (Rutherford)- a positively charged subatomic particle in the nucleus
Each nucleus must contain at least one particle with a positive charge.

6. Subatomic Particles
Electrons (Thomson)- a negatively charged particle found in the space OUTSIDE the nucleus
Each electron has a charge of –1.

8. Subatomic Particles
Neutrons (Chadwick)- a neutral subatomic particle found in the nucleus
Neutrons have a mass almost exactly equal to that of a proton.
No charge

10. A neutron walked into a bar and asked for the price of a drink
A neutron walked into a bar and asked for the price of a drink. "For you," the bartender replied "no charge." 10

11. Rutherford’s Nuclear Atom
the protons and neutrons are located in the nucleus
The electrons are distributed around the nucleus and occupy almost all the volume of the atom.
the nucleus is tiny compared with the atom as a whole.
If an atom were the size of a football stadium, the nucleus would be about the size of a marble.

12. Comparing Subatomic Particles
Protons, electrons, and neutrons can be distinguished by mass, charge, and location in an atom.
Everything scientists know about the nucleus and subatomic particles is based on how the particles behave.

13. Atomic Number Atomic Number- equals the number of protons in an atom
The atoms of any given element always have the same number of protons.
There is one proton in the nucleus of each and every hydrogen (H) atom…always…no exceptions!
Each element has a unique (different) atomic number
Atoms of different elements have different numbers of protons.

15. Atomic Number
Each positive charge in an atom is balanced by a negative charge because atoms are neutral.
The atomic number of an element also equals the number of electrons in an atom.

17. Mass Number
Mass Number- the sum of the protons and neutrons in the nucleus of an atom
Using the mass number is the only way to find the number of neutrons

19. Atoms of the First Ten Elements

21. Isotopes
Isotopes- atoms of the same element that have different numbers of neutrons and different masses.
Every atom of a given element does have the same number of protons and electrons.
But…every atom of a given element does not have the same number of neutrons.

23. Isotopes
Isotopes of an element have the same atomic number but different mass numbers because they have different numbers of neutrons.
Example: Heavy Water Figure 12, p. 112.

25. Complete Chemical Symbol
The composition of any atom can be represented in shorthand notation using atomic number and mass number
The chemical symbol Au appears with two numbers written to its left.
The atomic number is the subscript.
The mass number is the superscript.
You can also refer to atoms by using the mass number and the name of the element.
For example: gold - 197

26. Calculating Atomic Number
Uranium-238 has a mass number of 238 with 146 neutrons in the nucleus. Uranium-235 (mass of 235) has 143 neutrons in the nucleus.
What is the atomic # of uranium?

27. 4.3 MODERN ATOMIC THEORY Key Concepts:
Electrons move from energy levels when they gains/loses energy
The electron cloud model describes the possible locations of electrons around the nucleus
An electron cloud is a good approximation of how electrons behave in orbitals.
Stable electron configurations

28. Vocabulary: Energy levels Electron Cloud Orbital
Electron Configuration       
Ground State 

29. BOHR’S MODEL 1885-1962 Danish physicist
His model focused on the electrons
Electrons move in orbits around the nucleus
Like planets around the sun

32. ENERGY LEVELS Each electron in orbit has a specific amount of energy.
If the atom gains/loses energy, the energy of the electron changes
Energy levels- the possible energies that electrons in an atom can have
Electrons cannot exist between energy levels
They must be in one energy level
Each step away from the nucleus represents a gain in energy
***An electron can move from one energy level to another when the atom gains or loses energy

34. Question:
What determines the amount of energy gained/lost when an electron moves between energy levels?

35. Answer:
The size of the jump between energy levels

36. EVIDENCE FOR ENERGY LEVELS
Fireworks!!!
Heat produced by the explosion causes e- to move to higher energy levels
When those e- move back to a lower energy level, they emit energy (lose energy).
Some of that energy is released as light
Different elements emit different colors of light because no 2 elements have the same set of energy levels.

39. ELECTRON CLOUD MODEL Out with the old… In with the new…
Bohr was correct in assigning energy levels to electrons.
But incorrect in assuming e- move like planets in a solar system.
In with the new…
Today, we know that e- move in less predictable ways.

40. ELECTRON CLOUD MODEL
Electron Cloud- is a visual model of the most likely locations for electrons in an atom
The cloud is denser at locations where electrons most likely are found.
 Scientists use the electron cloud model to describe the possible locations of electrons around the nucleus.
Example: Propeller blades, page 116, Figure 14.  

47. Atomic Orbitals
The electron cloud represents all the orbitals in an atom.
Orbital- a 3-D region of space around the nucleus where an electron is likely to be found
Example: if you were to put a dot on a map of the school where you were located once every 10 minutes for a week we could see the places you visit the most would have a LOT of dots.

48. Atomic Orbitals The dots on the map would be a model of your “orbital”
They describe your most likely locations.
An electron cloud is a good approximation of how electrons behave in their orbitals.

49. Energy Levels, Orbitals, and Electrons
Number of Orbitals
Maximum # of Electrons 1 2 4 8 3 9 18 16 32

50. Electrons & Energy Levels

51. Question: How many electrons can be in each orbital?
Answer: 2

52. ELECTRON CONFIGURATIONS
Configuration- an arrangement of objects in a given space
Electron configuration- the arrangement of electrons in the orbitals of an atom
The most stable electron configuration is the one in which the electrons are in orbitals with the lowest possible energies

53. ELECTRON CONFIGURATIONS
Ground state- when all the electrons in an atom have the lowest possible energies
Example: Lithium has an atomic number of 3, so it has three electrons
Two electrons are in the orbital of the first energy level, one in the second at its second energy level
If energy is absorbed, one of the e- can move to an orbital with a higher energy level
This is known as an excited state
It is less stable than the ground state

54. Gain Energy…Move to Excited State

55. Lose Energy…Back to Ground State

56. ELECTRON CONFIGURATIONS
Eventually, this e- will lose energy and return to the ground state.
When helium, neon, argon, krypton, and xenon return from an excited state they emit light, neon light!