Name:_______________________________________________ Hour:_______
Guided Notes
Chapter 5
The Bohr Model
 Bohr proposed that an electron is found only in __________________ or
orbits around the nucleus.
 Each possible electron orbit has a fixed energy called an ___________
_____________.
Energy Levels
 Fixed energy levels of electrons are similar to rungs of a_____________.
 The lowest possible energy level is called its _____________________.
 Just like a person an electron can ___________ from one rung (energy
level) to another. It ____________ be found in between rungs (energy
levels).
 To move from one level to another an electrons must ________ or
_________ energy.
Quantum
 Amount of energy required to move an electron from one energy level
to another.
 The amount of energy an electron gains or loses in an atom is not
always the ________________.
 The ______________energy levels are ____________together so it
takes less energy to move between levels
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Quantum Mechanical Model
 _______________________________________________
 Determines energies of an electrons
 Electron location is based on how likely it can be found at a particular
location.
Label the model:
Atomic Orbitals
 Region of space in which there is a __________________ of finding an
electron
 Energy levels are labeled by numbers, n= 1, 2, 3, 4, 5, 6 or 7
 Each energy level has ______________________
 Orbitals are labeled by letters and different letters have different shapes
Summary of Principal Energy Levels, Sublevels, and Orbitals
Principal Energy level
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Number of sublevels
Type of sublevel
Name:_______________________________________________ Hour:_______
Maximum number of electrons




n = 1 : ____ electrons
n = 2 : ____ electrons
n = 3 : ____ electrons
n = 4 : ____ electrons
Electron Configuration:
 Arrangement of electrons in orbitals around the nucleus of an atom
 3 rules govern the arrangement:
o Aufbau principle
o Pauli exclusion principle
o Hund’s rule
Aufbau Principle
 Electrons enter the ___________ energy level first.
Pauli Exclusion Principle
 An orbital can hold at most 2 electrons, if 2 electrons are present they must
have opposite spins
 An up or down arrow indicates the electron’s spin ↑ or ↓,
 An orbital with paired electrons is written as
↑↓
Hund’s Rule
 One electron into each orbital until all orbitals have 1, then the second one
can enter.
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Electron Configuration
Element
H
Li
O
F
Ne
Na
1s
2s
2px
2py
2pz
3s
Electron Configuration
Exceptional Electron Configuration




There are always exceptions to the rules
Cr : 1s2 2s2 2p6 3s2 3p6 3d5 4s1
Cu :1s2 2s2 2p6 3s2 3p6 3d10 4s1
Exceptions due to subtle electron interactions in orbitals with similar
energies
Light
 The study of light led to the quantum mechanical model
o Newton stated: light consists of particles
o Huygens stated: light travels in waves
 Formula:
o C=λν
 Speed of light (C)
 Wavelength (λ)
 Frequency (ν)
Electromagnetic Spectrum
 The arrangement of types of radiation from long wavelengths to short
wavelengths
1. What color in the visible spectrum has the longest wavelength? ______
2. Which color in the visible spectrum has the highest energy? _________
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Calculation
Problem: Underline the givens in the problem
Calculate the wavelength of the yellow light emitted by a sodium lamp if the
frequency of the radiation is 5.10 x 1014 Hz (5.10 x 1014 /s) and the speed of light
is 3.00 x 108 m/s.
Step One: Write the Given
Step Two: Write the Equation
Step Three: Substitute in your given(s)
Step Four: Solve
Problem: Try this one on your own. I will come around to check.
Calculate the wavelength of the purple light emitted by a potassium lamp if the
wavelength of the radiation is 4.047 x 10-7 m and the speed of light is 3.00 x 108
m/s.
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Atomic Spectra
 When atoms absorb energy electrons move to higher energy levels
these electrons then lose energy by emitting light when they return to
the lower energy level
 Each discrete line in an emission spectrum correspond to 1 exact
frequency of light emitted by the atom.
 Formula:
o E=hν
 Energy (E)
 Plank’s constant (h)
 Frequency (v)
Quantum Mechanics
Photoelectric effect
 Einstein used Newton idea’s said light could be described as quanta of
energy that behave as particles
 Light quanta  photons
Atomic Spectra
 The motions of subatomic particles and atoms as waves
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Chapter 6
How did chemists begin to organize the known elements?
 Chemists used the properties of elements to sort them into groups
 Chlorine, bromine and iodine have very similar properties
Mendeleev’s Periodic Table
 He arranged the elements in his periodic table in order of _____________
atomic mass.
 The periodic table can be used to predict the properties of undiscovered
elements
Modern Periodic Table Arrangement
 Elements are arranged in order of increasing _____________________
Periodic Law
1. _______________________________________________________
2. There is repeating pattern of their physical and chemical properties
3. The properties of an element within a period change as you move from
left to right
4. The pattern of properties within a period repeats as you move from one
period to the next.
There are 3 broad classes of elements:
1. Metals
2. Nonmetals
3. _____________
Metals:
 Good conductors
 __________________________
 High luster, ductile & malleable
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Non-Metals:
 _____________________
 Dull and brittle
 Most are gases at room temperature
Metalloids:
 ______________________________
 Behavior can be controlled by changing
conditions
Identify the following elements as metals, nonmetals, or metalloids:
1.
2.
3.
4.
5.
Carbon (C ) ______________
Boron (B) ________________
Calcium (Ca) _____________
Barium (Ba) ______________
Copper (Cu) ______________
6.
7.
8.
9.
Bromine (Br) ______________
Neon (Ne) ________________
Silicon (Si) _______________
Iodine (I) _________________
Rows and periods:
 Horizontal rows are called periods. Periods indicates the number of
occupied electron shells
 Vertical columns are called families or groups (elements have similar
properties)
 The background colors in the squares are used to distinguish groups of
elements
o Group 1A: alkali metals
o Group 2A: alkaline earth metals
o Group 7A: halogens
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Elements are arranged in families based on electron configuration:




Noble Gases: Elements in group 8A
Representative Elements: Elements in groups 1A – 7A
Transition Elements: Elements in Group B in main part of periodic table
Inner transition metals: The elements below the main body of the
periodic table
Noble Gases
 Noble gases are elements in Group 8A
 The highest energy level is filled.
Element (Symbol)
Written Electron Configuration
The Representative Element:
 Elements in groups 1A through 7A are often referred to as
representative elements because they display a wide range of physical
and chemical properties.
 The s and p sublevels of the highest occupied energy level are not filled
 The group number equals the number of electrons in the highest
occupied energy level
Group 1A: one electron in the highest occupied energy level
Element (Symbol)
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Written Electron Configuration
Name:_______________________________________________ Hour:_______
Group 4A: four elements in the highest occupied energy level
Element (Symbol)
Written Electron Configuration
Transition Elements:
 There are two types of transition elements – transitions metals and
inner transition metals.
 They are classified based on their electron configurations
 In atoms of a transition metal, the highest occupied s sublevel and
nearby d sublevel contain electrons
 In atoms of an inner transition metal, the highest occupied s sublevel
and a nearby f sublevel generally contain electrons
Atomic Size
 The atomic radius is one half of the distance between the nuclei of two
atoms of the same element when the atoms are joined.
 In general, atomic size increases from top to bottom within a group and
decreases from left to right across a period.
Draw arrows
indicating the
trend:
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Ions
 During reactions between metals and nonmetals, metal ions tend to lose
electrons and nonmetals tend to gain electron
o ____________ are positive ions, they lose electrons
o __________ are negative ions and they gain electrons
Ionic Size
 Cations are smaller than the atoms and anions are larger than the atoms
 In general, ionic size of cations and anions decrease from left to right
across periods and increase from top to bottom within groups.
Draw arrows
indicating the
trend:
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Name:_______________________________________________ Hour:_______
Ionization Energy
 Ionization energy is the energy required to __________an electron from an
atom.
 In general the ionization energy tends to increase from left to right across a
period and decrease from top to bottom within a group.
Draw arrows
indicating the
trend:
Electron Affinity
 The energy change involved when a electron is added to a gaseous
atom
 In general, the electron affinity increases from left to right across a
period and decrease from top to bottom within a group.
Draw arrows
indicating the
trend:
Electronegativity
 Electronegativity is the ability of an atom to attract electrons to itself
when bonded to another atom
 In general, electronegativity decreases for top to bottom within a group
and increase from left to right
Draw arrows
indicating the
trend
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