Quiz 1 Unit 2 Flashcards
Atom
Smallest unit of an element that retains the properties of that element
Protons
P+, determine the type of atom, +1 charge, 1 amu, inside nucleus, 1 relative mass
Neutrons
n0, change mass in isotopes, 0 charge, 1 amu, inside nucleus, 1 relative mass
Electrons
e-, changes charge for ions, -1 charge, 0 amu, outside nucleus, 1/840 relative mass
Nucleus
Contains almost all the mass of an atom
Electron Cloud
Contains almost all the volume of an atom
Atoms are Measured in
Picometers or 10^-12 meters
Density of Nucleus
Huge
Elements Are
Atoms with the same number of protons, or same atomic number
Atomic Number is Represented By
Z = #p
Hyphen Notation
Element, hyphen, mass number
Charge
Protons minus electrons or
Electrons are Arranged in
Energy levels called shells or orbits
Formula for Bohr Model
2n^2 when n=the shell number
Valence Electrons
Electrons found on the farthest energy level of an atom
Columns in Periodic Table
Also called groups or families, the number of valence electrons
Rows in Periodic Table
Also called periods, the number of energy levels
Phil Model
2, 8, 8, 2 for amount of electrons in energy levels
Duet
Only applies to helium, lithium, hydrogen, and beryllium (he has little booty)
Octet
Electrons are most stable in groups of eight
Atomic Number
Number of protons, number of electrons in a neutral atom
Mass Number
Sum of protons and neutrons
Nuclear/Isotopic Symbol
Mass number on top, atomic number is bottom
Finding Counts
Protons is bottom, electrons is bottom, neutrons is top minus bottom
Using Periodic Table
Whole number is atomic number, decimal is average atomic mass
Average Atomic Mass Rounded
Mass Number
Ions
Changes in charge or electrons
Isotopes
Changes in mass or neutrons
First Number in Hyphen Notation
Atomic Number
John Dalton
1) Number three
2) Tested gasses
3) Father of atomic theory
4) An atom is made of sold, indivisible particles with elements being the same. Compounds are ratios and matter can not be created, destroyed, or changed
5) Ball
Democritus
1) Number one
2) Solid, indivisible particles (atomos)
Aristotle
1) Number two
2) Fire, water, earth, and air
JJ Thompson`
1) Number four
2) Used a cathode ray rube, positive and negative charges or anodes/cathodes, also sued magnetic field
3) Electrons are scattered through an atom in a positively charged cloud, also negatively charged particles in an atom (positive surrounding negative)
4) Cookie
Rutherford
1) Number five
2) Used alpha particles at a thin sheet of gold foil
3) Protons and electrons are not evenly dispersed, protons are in center and electrons are around
4) Big center
Cathode/Anode
Negative/positive electrode
Alpha Particles
Positively charged particles that represent a helium nucleus
Millikan
1) Number six
2) Used a drop of oil and electric field to stop the oil from dropping
3) Determined charge of an electron and smallest quantized charge
Bohr
1) Number seven
2) Electrons orbit around nucleus and do not spiral inward, atoms radiate energy when going to a higher orbit and absorb energy when going to a lower orbit
3) Solar system
Quantum Mechanical Model
1) Particles and waves, no way of knowing how it travels but instead in cloud
2) Mathematical model that predicts the probability of electron locations and paths within an electron cloud
