Atomic Structure: Protons and Neutrons
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| What did J.J Thompson calculate? | Charge to mass ratio- (e/m = 1.758820x10^8 C/g)
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| What did Millikan calculate? | The charge of an electron.
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| What did J.J Thompson's cathode ray experiment prove? | atoms give off negatively charged electrons. Also, those atoms must contain positively charged particles to balance the charge.
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| What is significant about J.J Thompson's Plum Pudding Model? | He proposed that electrons "corpuscles" were surrounded by a positively charged soup, like a blueberry muffin.
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| What is significant about Rutherford? | He created a Gold foil experiment that debunked Thompson's plum pudding model.
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| What is significant about Rutherford's gold foil experiment? | It used alpha particles- a type of emission given off by some naturally occurring radioactive elements.
When he aimed a stream of alpha particles at the foil, he noticed almost all went through the foil without being deflected.
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| What did Rutherford take away from his Gold Foil Experiment? | A metal atom is mostly empty space and the mass is concentrated in a tiny central core that he calls the nucleus.
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| What two particles is the nucleus composed of? | protons and neutrons
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| What makes one atom different than another? | The atomic number
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| What do protons and electrons have in common? | they equal each other
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| Neutrons? | neutrons are uncharged, but they add up to an atom's mass number
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| Mass Number | protons plus neutrons
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| Isotopes | Isotopes of an atom have the same atomic number but different mass numbers
Isotopes of the same element have the same number
of protons but different number of neutrons
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| Atomic Mass | a weighted average of isotopic
masses of an elements naturally occurring isotopes.
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| Using AMU as a conversion factor | If a diamond has a mass of 1.00 grams, how many atoms does the diamond contain?
1.00g (1amu/1.6605x10-24grams)(1carbonatom/12.011amu) = 5.02x10^22 c atoms
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| what is Avogadro's number? | it is a quantity, just like a dozen that we use to count atoms and molecules. one mole of carbon atoms equals 6.022x10^22 c atoms
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| Using Avogadro's number as conversion factor | how many moles of carbon atoms are in the diamond? 5.02x10^22 C atoms (1mole/6.022x10^23 atoms) =0.0834 mol C
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| Molar Mass | mass in grams of one mole of any element. units are g/mol
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| What does Avogadro's number tell us? | How many atoms are in a mole.
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| What do we use Avogadro's number to convert between? | atoms and moles 1mole= 6.022x10^22
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| What is Nuclear Chemistry? | the study of properties and changes of atomic nuclei
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| Nuclear Reaction | involves a change in the atom's nucleus, usually producing a different element.
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| Radioactive Isotopes | undergo spontaneous decomposition (decay)and emit some form of radiation.
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| Radiation | The emission of energy as electromagnetic waves or moving subatomic particles. there are three types found by Rutherford, alpha, beta, and gamma!
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| Alpha Radiation | is attracted/deflected to a negative electrode
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| Beta radiation | is attracted/deflected to a positive electrode
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| Gamma | unaffected by magnetic and electric fields
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| What are the two other radioactive decay processes in addition to alpha and beta? | Positron Emission and Electron Capture.
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| Positron Emission | occurs when a proton in a nucleus changes to a neutron and ejects a positron.
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| What is a positron | thought of as a positive electron, same mass of electron but opposite charge.
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| what is electron capture? | happens when a proton in the nucleus an electron and turns into a neutron.
The atomic number will decrease (one fewer proton) and mass number is unchanged.
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| How can we think of electromagnetic energy? | As Waves
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| What is electromagnetic energy characterized by? | frequency, wavelength, and amplitude.
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| Wavelength x Frequency equals? | Speed
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| What is Frequency? | the number of wave peaks to pass a given point per unit of time.
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