Electron Arrangement: CH 6
Electromagnetic radiation is all ______that exhibits wavelike behavior and travels through space.
Examples are: ______
Speed of light
equals 3.0 x 108 m/s
all ______travel at this speed
Electromagnetic Spectrum (EM spectrum)
Identifies all forms of electromagnetic radiation
Notice that as frequency increases, the amount of energy ______. This is a ______proportional relationship.
______is a small region within the spectrum that has wavelengths/frequencies that are eyes can detect.
ROY G BIV is a mnemonic to help you remember the colors of the spectrum. Red is near ______and violet is near ultra violet.
Continuous Spectrum vs. Line Spectrum
Continuous Spectrum: Sunlight (or white light) will produces a ______of color because there are no ______wavelengths.
Line Spectrum is when ______atoms emit light of only certain______. Each element has its own line spectrum.
Review of Models
Greek/Dalton view Plum Pudding model Rutherford Model
Bohr Model
Why don’t electrons fall into the nucleus?
Electrons thought to move like ______around the sun in circular orbit at different levels (energy levels)
There are amounts of ______that separate 1 level from another.
Think of the energy levels as rungs of a ______.
There is no in-between energy!
The farther away an energy level is from the nucleus,
the more ______it attains!
Ground state: lowest energy level state
Excited state: a higher state
Electrons can move from a ground state to an excited state by ______energy whereas they ______energy when moving from the excited state to a ground state.
Quantum Mechanical Model(Modern view of the atom)
Electrons have both particle & ______like behavior.
They exist in ______.
Electrons do not have ______. They only can have a probability of being located in a certain place but its position cannot be described exactly. Their energy & positions are described by ______.
Electrons can be found in a blurry ______.
Quanta: amount of energy an electron can ______as it moves higher or release when it moves ______.
Where are the electrons?
- Within the atom are “Energy Levels”
There are ______on the periodic table.
The period number on the periodic table corresponds to the energy level.
Energy levels are also called ______.
Ca is in energy level ______Cl is in energy level ______
- Within each energy level are “Sublevels”
Sublevels are like ______of space
“s” sublevel
______shaped
there is only ______orientation (position) = orbital
represented in the periodic table as
groups 1A and 2A + helium
first seen in the 1st energy level
maximum ______electrons
“p” sublevel
______shaped
there are ______orientations(positions) = orbitals
represented in the periodic table
as groups 3A- 8A
first seen in the 2nd energy level
maximum ____ electrons
“d” sublevel
______shaped
there are ______orientations(positions)= orbitals
represented in the periodic table as the transition metals, group 3B – 2B
first seen in the 3rd energy level
maximum ____ electrons
“f” sublevel
______shaped
there are ______orientations(positions)= orbitals
represented in the periodic table as
the inner transition metals, lower block
first seen in the 4th energy level
maximum ____ electrons
- Within each sublevel are “Orbitals”
An orbital is defined as the ______where there is a high probability of finding an ______.
Each orbital holds ______electrons
To calculate the total number of electrons in an energy level, use 2(n2)
Summary
n2 2(n2)
Energy Level / # of sublevels / Type of sublevel / Total # of orbitals / Total # of electronsAs seen in the chart above, 1st energy level has a maximum of _____ electrons, 2nd energy level has a maximum of ______electrons, 3rd energy level has a maximum of ____ electrons, and 4th energy level has _____ electrons
When drawing simple Bohr models, when you get the 3rd energy level, place 8 in the 3rd energy level first, then 2 in the 4th energy level, the remainder of the 18 are placed into the 3rd. Then place in the 4th if needed.
Valence electrons are the electrons found in the ______shell (energy level) They are not very ______.
Examples
H O Cl
Short cut to determine valence electrons
The group # next to the letter A represents the valence electrons.
Electron Dot notation
Valence electrons are represented by dots around the element symbol
Li Be C N Ne
Electron Configuration
Is an ______of an electron
Electrons must be placed in the ______
possible energy levels first (ground state)
3 rules that govern electron configuration
- Aufbau Principle: electrons must be placed in ______of lowest energy levels first
Can use the periodic table as a guide or use diagram below; If you use the periodic table, need to make 2 modifications:
Transition metals: period # -1 is the energy level
Inner transition metals: period # - 2 is the energy level
Sequence of energy level is ______
Sequence of sublevels is ______
An orbital can ______within different energy levels
______is lower in energy than 3d
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p
- Pauli Exclusion Principle: electrons in the same orbital must have opposite ______.
- Hund’s rule: When electrons occupy orbitals of the ______energy , 1 electron enters each orbital first until they are all ______filled. Then and only then can a second electron be added to those orbitals.
______
You Try !
Electron Configuration
H
He
Li
B
N
Ne
Mg
Ca
Fe
As
Orbital Notation
Shows the spin of the electron
Uses ______( )to display electrons moving in ______directions to prevent repulsion
______or represents an orbital
Example: Orbital 1s 2s 2px 2py 2pz
H
He
Li
N
O
Noble Gas Configuration
also known as ______configuration
Place the ______that comes before the element in brackets and then start your configuration from that point
The brackets represent the ______electrons
Example: Full electron configuration vs. shorthand configuration
Al
Ge
Hf
Exceptional (special) Configurations
Elements up to vanadium (V) follow Aufbau principle
After that, there are lots of exceptions to the rule
****Reasons for exceptional configuration
- Completely filled orbitals are more ______than half filled or partially filled orbitals.
- ______orbitals are more stable than partially filled orbitals.
**Exceptions you need to know are Cu Cr Mo Ag
Cr
Ag
Electron Configurations for Ions
Representative Ions have a ______configuration
Cations: removal of 1 or more ______electrons from highest energy level and sublevel; for transition metals, always remove electrons from ______sublevel before the d sublevel
Sodium atom: Na
Sodium ion: Na+1
Titanium: Ti
Titanium(II) ion: Ti+2
Anions: ______of 1 or more valence electrons to the highest energy level and sublevel
Chloride ion : Cl-1
You Try:
Write the electron configuration for the following ions:
S-2
**Cu+1
**Cu+2
Flame Tests
______can be identified by the ______of light they emit.
When metals absorb energy from a flame, the ______absorb energy and are raised to a
higher ______. When they return to their______, they release
the energy they absorbed in the form of ______. The wavelength of light of some
metals fall in the ______light portion of the spectrum. This allows us to see their color.
Representation of the process described above