1. Chapter 2 Matter is Made up of Atoms
Fill in the blanks in your notes with the words or phrases bolded in purple.

2. Warm-up Question 10/19
What is the difference between a theory and a law?
Everything in chemistry comes back to haunt you

3. Atomic Theory
Democritus
( BC)
Greek Philosophers
(about 2,500 years ago)
Atoms are the smallest particles of matter and different types of atoms exist for every type of matter.
The idea that matter is made up of fundamental particles called atoms is known as the atomic theory of matter.

4. Atomic Theory
Antoine Lavoisier
(1782)
Joseph Proust
(1799)
When a chemical reaction occurs, matter is neither created nor destroyed but only changed.
This became known as the law of conservation of matter.
The elements that compose a compound are always in a certain proportion by mass.
This principle is now referred to as the law of definite proportions.

5. Atomic Theory
John Dalton (1803)

6. Atomic Theory

7. Bench Mark If you haven’t done so already, you should:
Read pages or your text
Complete Homework #1

8. Exit Question 50.0g + ____g = 80.0g + 25.0g
What mass of NaOH must have been used in the following reaction?
50.0g ____g = g g

9. Warm-up Question 2/22 Examine the two magnets:
What ends of each magnet must be placed next to each other for the magnets to be attracted to one another?

10. Atomic Particles J.J. Thomson (1897)
Discovered that Dalton’s solid ball model was not accurate.

11. Atomic Particles

12. Atomic Particles Conclusion…
The rays bent toward a positively charged plate and away from a negatively charged plate.
Objects with like charges repel each other, and objects with unlike charges attract each other.
Cathode rays are made up of invisible, negatively charged particles referred to as electrons.

13. Atomic Particles
J.J. Thomson (1910)
The “Plum Pudding” Model

14. Exit Question 10/22
If an electrical field was applied to the cathode ray tube below. Which direction (up or down) would the beam of light be bent ?

15. Warm-up Questions 10/23
Why is the path of the red ball to the right when it gets hit by the white cue ball?

16. Atomic Particles Ernest Rutherford (1909)
Revealed that Thomson’s plum pudding model was not accurate.

17. Atomic Particles Conclusion…
Because most of the particles passed through the foil, they concluded that the atom is nearly all empty space.
Because a few particles were deflected, they proposed that the atom has a small, dense, positively charged central core, called a nucleus.

18. Atomic Particles Rutherford’s Nuclear Model
Consisting of a nucleus and electrons

19. Further Atomic Developments
Scientists also determined that the rays in the cathode ray tube were also composed of positively charged subatomic particles called protons.
Atoms of an element that are chemically alike but differ in mass are called isotopes of an element.
The existence of a neutral particle, called a neutron, was confirmed in the early 1930s.

20. Exit Question 10/23 What keeps the electrons from leaving the atom?
Bonus: What keeps the electrons in motion away from the nucleus?

21. Warm-up Question 10/26
Examine the picture below. What percentage of all the fruit pictured is bananas?

22. Atomic Particles

23. Atomic Particles
The atomic number of an element is the number of protons in the nucleus of an atom of that element.
It is the number of protons that determines the identity of an element, as well as many of its chemical and physical properties.
The sum of the protons and neutrons in the nucleus is the mass number of that particular atom.
Isotopes of an element have different mass numbers because they have different numbers of neutrons, but they all have the same atomic number.

24. Atomic Particles
The number at the bottom of each box is the average atomic mass of that element.
This number is the weighted average mass of all the naturally occurring isotopes of that element.

25. Benchmark If you haven’t done so already, you should:
Read pages in the text
Complete homework #2

26. Exit Question 10/26
What are the similarities and differences between these 3 diagrams? e e e

27. Warm-up Question 10/30 Order these nesting dolls from the inside out.B C D E F
Russian Matryoshka Dolls

28. Electron Configuration
Niels Bohr (1913)
He proposed that atoms have only certain allowable energy states
Ground state
Excited state
Electrons move around the nucleus in only certain allowed circular orbits.

29. Electron Configuration
Bohr’s planetary model was found to be inaccurate.
The electron cloud model shows that electrons are most likely to be found in certain spherical regions of space around the nucleus.
The space around the nucleus of an atom where the atom’s electrons are found is called the electron cloud.

30. Electron Configuration
A three-dimensional region around the nucleus called an atomic orbital describes the electron’s probable location.

31. Electron Configuration
The arrangement of electrons in an atom is called the atom’s electron configuration.
Principle energy level (1, 2, 3, 4, etc…)
Energy sublevel (s, p, d, or f)
Atomic orbital
The number of electrons in those orbitals
Energy Level
Sublevel
Atomic Orbitals
Number of Electrons 1 s 2
s, p
1, 3
2, 6 3
s, p, d
1, 3, 5
2, 6, 10 4
s, p, d, f
1, 3, 5, 7
2, 6, 10, 14

32. Electron Configuration
Aufbau Diagram
Example
Write the electron configuration of neon.
Electrons? _____
Electron configuration?
__________________

33. Electron Configuration

34. Electron Configuration
The electrons in the outermost energy level are called valence electrons.
When atoms come near each other, it is these electrons that interact with one another.
Many of the chemical and physical properties of an element are directly related to the number and arrangement of valence electrons.
A Lewis dot diagram illustrates valence electrons as dots around the chemical symbol of the element.
Each dot represents one valence electron, and the element’s symbol represents the core of the atom (the nucleus plus all the inner electrons.

35. Electron Configuration
Example…
Write the electron configuration and Lewis dot diagram for an atom of boron.
ELECTRONS _____
ELECTRON CONFIGURATION ______________
VALENCE ELECTRONS _____
SYMBOL _____
LEWIS DOT DIAGRAM

36. Benchmark If you haven’t done so already, you should:
Review your notes on electron configuration
Do homework #3

37. Exit Question 10/30
Why does the Lewis dot diagram for helium look different than the diagrams for the other noble gases?

38. How are the bright lights in the signs below generated?
Warm-up Question 10/31
How are the bright lights in the signs below generated?

39. Electromagnetic Spectrum
Electromagnetic radiation is a form of energy that exhibits wavelike behavior as it travels through space.
All of the forms of radiant energy are parts of a whole range of electromagnetic radiation called the electromagnetic spectrum.
All waves can be described by several characteristics…
Wavelength (λ) is the shortest distance between equivalent points on a continuous wave (m, cm, or nm).
Frequency (ν) is the number of waves that pass a given point per second (1/s, s-1, or Hz).
Amplitude is the wave’s height from the origin to a crest (or to a trough).
All waves travel at the speed of light (3.00x108 m/s).

40. Electromagnetic Spectrum

41. Electromagnetic Spectrum

42. Electromagnetic Spectrum
Example…
What is the wavelength of a microwave having a frequency of 3.44x109 Hz?
KNOWNS & UNKNOWNS
FORMULA __________
REARRANGED FORMULA __________
PLUG-IN NUMBERS ____________________
ANSWER (with unit) __________

43. Electromagnetic Spectrum
Matter can gain or lose energy in only small, specific amounts called quanta.
A quantum is the minimum amount of energy that can be gained or lost by an atom.
E = energy in Joules (J)
h = Planck’s constant = 6.626x10-34 (Js)
ν = frequency in Hertz (Hz)

44. Electromagnetic Spectrum
Example…
Tiny water drops in the air disperse the white light of the sun into a rainbow. What is the energy of a photon from the violet portion of the rainbow if it has a frequency of 7.23x1014 Hz?
KNOWNS & UNKNOWNS
FORMULA __________
REARRANGED FORMULA __________
PLUG-IN NUMBERS ____________________
ANSWER (with unit) __________

45. Electromagnetic Spectrum
The atomic emission spectrum of an element is the set of frequencies of the electromagnetic waves emitted by atoms of the element.

46. Benchmark If you haven’t done so already, you should: Read pages 69-79
Complete Homework #4

47. Exit Question 10/31 Which of the following waves has the: A C B E D
Longest wavelength?
Highest frequency?
Lowest Energy?