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Examining Isotopes
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100
Write the following number in scientific notation: 640.05
6.4005 x 10^2
100
Write out the Isotope notation for Oxygen with 10 neutrons.
Symbol - O Atomic number (bottom) - 8 Mass number (top) - 18
100
What are the three types of subatomic particles and their charges and masses?
Protons are +, mass of 1 neutrons are neutral, mass of 1 electrons are negative, mass of 0
100
What are the three types of radioactive particles we studied in class?
What are alpha, beta and gamma
100
Name 3 lab safety techniques
Goggles, apron, no gum, no food/drink, safety shower, eye wash, no horseplay, no running, read all directions, no random lab experiments, alert the teacher for all spills and emergencies, close toe shoes, tie up hair, etc.
200
Write the equation for density AND the density equation re-written to solve for V.
D=m/v V=m/D
200
Write out two isotope notations for Carbon, one with 13 neutrons and one with 14 neutrons.
Carbon - 13 and Carbon - 14 both have 6 as their atomic numbers
200
How do you know the number of protons neutrons and electrons in a bohr model?
Protons are the atomic number, neutrons are the mass- protons, and electrons are equal to protons in a neutral atom.
200
Write out an alpha particle and what can be used to block it.
He with atomic number 2 and mass 4, paper can block it.
200
What subatomic particle did Thompson discover? What did his model of the atom look like?
Electrons. Chocolate chip cookie
300
Adding and subtracting in scientific notation the powers must be ___________________ Multiplying and dividing in scientific notation the powers _________________________
the same, added or subtracted
300
What are isotopes?
Two or more atoms of the same element that have different masses.
300
Draw the bohr model for Carbon.
See the board.
300
Why does the mass of the sample not change after it undergoes beta decay?
Beta particles have no mass!
300
What are the three base units we use in the metric system?
Grams (g), Meters (m) and Liters (L)
400
Convert 5g to kg. Show your work!
5g * 1kg/ 10^3g = 5x10^-3kg
400
If you are given a chart of various isotopes for Carbon, how do you find the average atomic mass listed on the periodic table?
Add up the masses of the isotopes and divide by the total number of isotopes. (Find the average!)
400
Draw the Bohr model for Ca.
See the board.
400
In a nuclear power plant, what is the purpose of the uranium decay process?
To produce heat that will heat water to steam, turn a turbine and produce electricity.
400
What are orbitals?
The shapes that the electrons orbit the nucleus in. (Not rings)
500
Which scientist created the atomic theory and what were the three parts?
Dalton. Matter cannot be created, divided or destroyed.
500
In isotopes, what subatomic particle is allowed to change?
What are neutrons.
500
Which atom has 12 electrons? How many rings will its Bohr model have?
Mg, 3
500
Write out a nuclear decay equation for Uranium - 235 as it undergoes beta and gamma decay.
See drawing on board
500
Explain how we figure out the number of rings to draw, and how many electrons can fit on each ring for the bohr model.
The number of electrons is equal to protons for a neutral atom. The rings and placement are based on the periodic table.