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chem
test unit 2
| Question | Answer |
|---|---|
| Which scientist concluded that atoms contain negatively charged particles scattered evenly throughout the atom with positively charged matter between them? | J.J. Thomson (Plum Pudding Model) |
| Q: Whose experiments led to the identification of the nucleus of the atom? | A: Ernest Rutherford (Gold Foil Experiment) |
| Q: How did John Dalton describe his model of the atom? | A: As a tiny, indivisible, solid sphere (like a billiard ball). |
| Q: According to the Bohr model, how does the single electron in a hydrogen atom move around the nucleus? | A: In specific, fixed circular orbits or energy levels. |
| Q: During Rutherford’s gold foil experiment, what was the behavior of most alpha particles as they passed through the foil? | A: They passed straight through with no deflection. |
| Q: Niels Bohr was the first scientist to consider electrons in terms of what property? | A: Energy Levels (or Quantized Energy) |
| Q: When does radiation occur according to Niels Bohr’s explanation of electron behavior? | A: When an electron falls from a higher energy level to a lower one. |
| Q: What is a cathode ray, and which British scientist discovered the electron using cathode rays? | A: A cathode ray is a stream of electrons. It was discovered by J.J. Thomson. |
| Q: Which atomic model is most closely associated with Niels Bohr? | A: The Planetary Model (or Bohr Model) |
| Q: Who isolated the nucleus of the atom using the gold foil experiment in 1911? | A: Ernest Rutherford |
| Q: Identify the scientist associated with the Rutherford model of the atom. | A: Ernest Rutherford |
| Q: Which scientist is credited with creating the atomic model shown in the provided image? | Solid Sphere = Dalton Plum Pudding = Thomson Nuclear Model = Rutherford Planetary Model = Bohr |
| Q: Which thinkers believed the atom looked like the models shown in the timeline of atomic theory? | A: Match the model to the scientist from the list in Card 12. |
| Q: Who was the early philosopher (460 B.C.–370 B.C.) who first suggested the concept of atoms? | Democritus |
| Q: What subatomic particle was discovered through cathode ray tube experiments in the late 1800s? | A: The Electron |
| Q: What conclusion did Rutherford make about the structure of the atom? | A: The atom has a small, dense, positively charged nucleus and is mostly empty space. |
| Q: What are the equations to find the following? a. Protons b. Neutrons c. Electrons (in a neutral atom) d. Mass number e. Atomic number | A: a. p⁺ = Atomic Number (Z) b. n⁰ = Mass Number (A) - Atomic Number (Z) c. e⁻ = Atomic Number (Z) d. A = p⁺ + n⁰ e. Z = number of protons |
| Q: What are protons? | A: Positively charged subatomic particles found in the nucleus. |
| Q: What are electrons? | A: Negatively charged subatomic particles found outside the nucleus. |
| Q: What are neutrons? | A: Neutral (no charge) subatomic particles found in the nucleus. |
| Q: PRACTICE ELECTRON CONFIGURATION What is the electron configuration for Oxygen (Atomic # 8)? What is the electron configuration for Sodium (Atomic # 11)? | A: Oxygen: 2-6 (2 electrons in 1st shell, 6 in 2nd shell) Sodium: 2-8-1 (2 in 1st, 8 in 2nd, 1 in 3rd shell) |
| Q: When an electron absorbs energy, from which state to which state does it transition? | A: From a lower energy level (ground state) to a higher energy level (excited state). |
| Q: Does the speed of light change across the electromagnetic spectrum, or is it constant? | A: It is constant (3.00 x 10⁸ m/s). |
| Q: What is another name commonly used for electromagnetic radiation? | A: Light (or radiant energy). |
| Q: How are wavelength and frequency related mathematically? | A: They are inversely proportional. c = λν (speed of light = wavelength x frequency). |
| Q: What is the name of the unique pattern of lines produced when light from an atom passes through a prism? | A: Atomic Emission Spectrum (or Line Spectrum) |
| Q: What kind of light (in terms of frequency or wavelength) is produced when there is a large jump between energy levels? | A: High frequency, short wavelength light (e.g., UV, X-rays). |
| Q: Which electron transition involves the greatest energy of emitted light: from n = 4 to 5, n = 2 to 5, n = 5 to 1, or n = 5 to 4? | A: n = 5 to n = 1 (The biggest drop releases the most energy). |
| Q: What happens to an electron’s energy when it moves from a lower energy level to a higher energy level? | A: Its energy INCREASES. It must absorb energy to make this jump. |
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