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Chapter 2 Matter is Made up of Atoms

Chapter 2 Matter is Made up of Atoms. Fill in the blanks in your notes with the words or phrases bolded in purple. Warm-up Question 10/19. What is the difference between a theory and a law?. Everything in chemistry comes back to haunt you . Atomic Theory. Greek Philosophers

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Chapter 2 Matter is Made up of Atoms

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  1. Chapter 2Matter 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 Greek Philosophers (about 2,500 years ago) Democritus (460-370 BC) 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) 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. • When a chemical reaction occurs, matter is neither created nor destroyed but only changed. • This became known as the law of conservation of matter.

  5. Atomic Theory • John Dalton(1803)

  6. Atomic Theory

  7. Bench Mark • If you haven’t done so already, you should: • Read pages 51-60 or your text • Complete Homework #1

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

  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 chargesrepel 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 61-68 in the text • Complete homework #2

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

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

  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. 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: Longest wavelength? Highest frequency? Lowest Energy? D A B E C

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