Unit 2 Flashcards
fMass of Subatomic Particles
Proton 1 amu
Neutron 1 amu
Electron 0 amu
Elements Have Same
Proton count
Atomic number
Properties
Isotopes
Atoms of the same element with a particular number of neutrons that change the mass
Ions
Atoms of the same element with a particular number of electrons that change the mass
Energy levels
Shells/orbits of crazy shapes where the electrons can be found around the nucleus
Finding Electron Count in Bohr Model
2n^2 when n=shell number
Groups/Families/Colums
Vertical
Number of valence electrons
Rows/Periods
Horizontal
Number of energy levels
Phil Model
2, 8, 8, 2 electrons per energy level
Duet
Applies to hydrogen, heleium, lithium, and berelium
Mass Number
Atomic mass rounded
Sum of protons and neutrons
Measured in amu
Atomic Mass
Weighted average of mass number in all isotopes
Decimal in periodic table
Measured in g/mol or amu
Weighted Average
Takes into account the abundance of each item being averages
Average Atomic Mass Formula
Mass A (%A) + Mass B (%B)
Chemical Reactions
Atoms attain stability by losing, gaining, or sharing electrons
Nuclear Reactions
Atoms attain stability through changes in the nucleus
Radioactivity
Process by which an unstable nucleus spontaneaously emits high energy particles or rays from the nucleus in order to attain a more stable nuclear state
Strong Force
An attractive force that binds protons and neutrons together in the nucleus
Electrostatic Force
Causes protons to repel other protons
Nuclear Force
Created by neutrons to hold the nucleus together
Creates Radioactivity
When there are more neutrons creating nuclear force repelling the electrostatic and strong force
Unstable/Radioactive Elements
Above #83
Beta Particle Protection
Glass, clothing, wood
Neutron/Proton Emission
Neutron 1/0n
Proton 1/1p
Nuclear Symbol Top and Bottom
Top mass
Bottom Charge
Radiation
Emission of particles
Beta Decay Sequence
Electron leaves which adds proton
Opposite of Beta Decay Sequence
Electron capture or positron emission
How Nuclear Electricity is Created
Uranium atoms split producing kinetic energy
Converts water to steam
Rotates turbines
Produces electricities in the generator
First Atomic Weapons
Both fission bombs
How Fusion Bombs Work
Combine two hydrogens to produce helium
How Fission Bombs Work
Neutrons fired at uranium or plutonium atoms
Split causing smaller atoms and energy
Smaller atoms collide with more uranium or plutonium
Artifitial Radioactive Nuclides
Made by artifitial transmutations through bombardments of nuclei with charged and uncharged particles
Transuranium Elements
Above #92
Deuteriium and Tritium
Stable hydrogen isotope with one more neutron
Radioactive isotope of hydrogen with two neutrons
Three Main Sections of a Nuclear Power Plant
Reactor
Generator
Cooling tower
Half-Life Equation
mf = mi/2^n
mf = final mass
mi = initial mass
n = number of half-lives
Conversions
1 mega = 1.0x10^6 base
1 micro = 1.0x10^-6 base
1 nano = 1.0x10^-9 base
1 pico = 1.0x10^-12 base
Complex/Derived Unit
A measurement expressed as a ratio between units
Centimeters to Inch
2.54cm=1in
Meters to Mile
1600m=1mi
Dalton’s Theory
All matter is made of atoms, which are indivisible
All atoms of a given element are identical in mass and properties
Compounds are combinations of two or more different types of atoms
A chemical reaction is a rearrangement of atoms
Tested gases
Democritus’ Theory
Solid, indivisible particles
Divided a seashell
JJ Thomson’s Theory
Negative electrons are scattered throughout a sphere of positive charge
Atom can be broken down
Cathode ray tube
Rutherford’s Theory
Atom is mostly empty space, with nearly all of its mass concentrated in a tiny central nucleus
Alpha particles at gold foil
Milikan’s Theory
Electrons have a negative charge
Charge on a drop of oil and stopped the oil from falling
Quantum Mechanical Model
Electrons exist in an electron cloud, existing as a particle and a wave at the same time
STP
Standard temperature and pressure
Reaction that Requires Critical Mass
Fission and fusion
Liters to Gallon
3.79L=1gal
Meters to Yard
0.91m=1yd
Liters to Cups
0.24L=1cup
Nuclear Versus Chemical Reactions Same
Atoms attain stability, mass and change must be balanced
Nuclear Versus Chemical Reactions Different
Nucleus VS electrons
In nuclear elements change, isotopes matter, spontaneous, can not be sped up/slowed/stopped, decay chain
Chadwick
Positively charged protons and neutral neutrons bound together as the atom’s nucleus
Negatively charged electrons occupying energy levels surrounding the nucleus
Alpha particles bombarding
