Electrons Abd Such Flashcards
Electro magnetic spectrum
Shorter wavelength higher frequency
Electron
Emission of light
Bohr models
Rings 2 8 18 32
Ground state
Lowest state of energy an electron can be at
Most stable
Excited state
State higher than ground state
What does n cloud describe
Energy levels
Larger value of n=more distance from nucleus higher the energy
Quantum number L describes
Types of clouds
Four types of l clouds
S
P
D
F
What four elements have exceptions in electron filling
Cu
Cr
Ag
Au
Pauli exclusion principle
Max of 2 electrons per orbital
Must have different spin
Aufbau principle
Electrons occupy lowest energy orbitals available
And orbital can hold 2 electrons
Hunds rule
Orbitals of equal energy occupied by 1 electron before 2 electrons
All electrons singly occupied must have same spin
Paramagnetic
Attracted to magnets
Contains 1 or more in paired electrons
Diamagnetic
Not attracted to magnets because all electrons are paired
Newlands
First person to use periodic table
16 elements
Organized them by increasing atomic mass
Made law of octaves
Law of octaves
Chemical and physical properties repeated with 8th element
Medelev
63 elements
Left gaps
Mosley
Rearranged table
Increasing atomic number
Made periodic law
Periodic law
Chemical and physical properties of elements periodic functions of their atomic numbers
Alkali metals
React with water to produce basic solutions
First group on the left
Alkaline earth metals
Less reactive than alkali
2nd group to the left
Lanthanides
Color tv
1st group on f block
Actinides
Radioactive
2nd group on f block
Transition metals
D block
Solutions often colored
Halogens
Salt formers
2 group from right
Noble gases
Very stable
Filled outer electron orbitals
1st group to the right
Metals
Conductivity
Shiny
Malleable
Ductile
Alloy
Metal+nonmetal
Stainless steel Fe+cr
Non metals
To the right of metalloids
Metalloids
Semi conductors
Staircase on periodic table
B, si, ge, as, sb, te
Atomic radius
Half he distance between nuclei of adjacent atoms bonded to each other
Vander waals radius
Half the distance between nuclei of adjacent atoms not bonded to each other
Difference between atomic bond radius and vander waals radius
Atomic bond radius smaller than vander waals radius
As you move down a group atomic radius…
Increases
1 energy level is added down each period
Electron sheik ding effect
Electrons in inner energy levels shield outer electrons from full nuclear charge
As you move across a period atomic radius
Decreases
Increasing nuclear charge
Electrons: same energy level
Across a period
Protons added= increased positive charge
Electrons added=same energy level
Ion
Atom with an electrical charge
Positive ion
Loses and electron
Negative ion
Gains an electron
Ionization energy
Energy needed to remove outer electron from and atom
As you love across a period ionization energy
Increases
Electrons held more tightly to nucleus
As you go down a group ionization energy
Decreases
Electrons held less tightly to nucleus
Electron affinity
Energy emitted upon addition of electron to atom
