Chapter 4 Jeopardy Review
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1 Chapter 4 Jeopardy Review Atom Models of the Atom Atomic Theory Calculating Subatomic Particles Isotopes Final Atoms What are the three subatomic particles, and their charges?
2 Atoms Atoms Answer: Protons, +1; Neutrons, 0; Elections, -1 Using the example of the football field, describe the size of an atom. Atoms Answer: If the nucleus of the atom which contains protons and neutron was the size of a golf ball in the center of a football field, the closest electron would be at the goal post. Atoms Use the law of conservation of mass to describe what happens in chemical reactions
3 Atoms Answer: Atoms can be joined, separated, or rearranged in a chemical reaction, but can not be created or destroyed. Atoms A neutral atom contains equal numbers of what two subatomic particles? Atoms Atoms Answer: Protons and Electrons Give the definition of an atom
4 Atoms Models of the Atom The smallest particle of an element that retains the same chemical properties. Describe Thomson s experiment and what he discovered Models of the Atom Answer: Thomson used a cathode ray tube and a magnetic field to determine the presence of electrons and assign a negative charge to the particle. Models of the Atom Describe Millikan s experiment and what he discovered
5 Models of the Atom Answer: Millikan performed the oil drop experiment, and determined the mass and charge on the electron Models of the Atom Describe Rutherford s experiment and what he discovered Models of the Atom Answer: Rutherford performed the gold foil experiment, and determined that there is a small concentrated positive mass at the center of every atom Daily Double
6 Models of the Atom Describe Chadwick s experiment and what he discovered. Models of the Atom Answer: Chadwick discovered the neutron by allowing Polonium to decay, alpha particles hit Beryllium which gave off neutrons. The neutrons hit wax, which gave off atoms. The speed that the atoms hit a receptor allowed Chadwick to calculate the mass of the neutron particle. Models of the Atom Models of the Atom What is the difference between Thomson s and Rutherford s models of the atom? Answer: Thomson did not believe that the protons and electrons were separated by space and Rutherford determined that most of the atom is made up of empty space.
7 Atomic Theory Who was the Greek philosopher that first came up with the idea of the atom? Atomic Theory Answer: Democritus Atomic Theory Atomic Theory Who was the first to propose an atomic theory? Answer: Dalton
8 Atomic Theory Atomic Theory What was the piece of Dalton s atomic theory that was removed in the current theory? Answer: That atoms could not be separated into smaller parts. Atomic Theory Atomic Theory What was changed about the last statement in Dalton s atomic theory? Answer: Atoms of one element can not be changed into atoms of other elements by the result of a chemical reaction.
9 Atomic Theory Atomic Theory What is the relative size of the atom? There are three times as many atoms in a penny as there are people on Earth. Calculating Subatomic Particles Calculating Subatomic Particles What is the formula for calculating the number of neutrons in an atom Answer: mass # - protons = neutrons
10 Calculating Subatomic Particles Calculating Subatomic Particles How many neutrons are in Carbon-13? Answer: 7 Daily Double Calculating Subatomic Particles How many neutrons are in Sodium-23 (atomic number 11)?
11 Calculating Subatomic Particles Calculating Subatomic Particles Answer: 12 How many neutrons are in Lead-207 (atomic number 82)? Calculating Subatomic Particles Calculating Subatomic Particles Answer: 125 How many neutrons are in Ag
12 Calculating Subatomic Particles Isotopes Answer: 61 What is an Isotope? Isotopes Answer: Atoms of the same element that have the same number of protons but different numbers of neutrons Isotopes How do you write an isotope symbol?
13 Isotopes Answer: The mass number is at the top in front of the chemical symbol and the atomic number is below the mass number. Isotopes Give an example of two isotopes. Isotopes Isotopes Answers will vary Copper has two isotopes. Copper- 63, which has an atomic mass of u and copper- 65, which has an atomic mass of u. In any sample of copper atoms, 69.1% will be copper- 63 and 30.9% will be copper- 65. Calculate the average atomic mass of naturally occurring copper.
14 Isotopes Isotopes Answer: amu Isotope mass (u) N % N % N % Isotopes Final Jeopardy Answer: 14.07amu What was the dependent variable in Rutherford s experiment?
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