Name:_______________________________________________ Hour:_______

Guided NotesChapter 5The 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 Number of sublevels Type of sublevel

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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 principleo 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.

Electron Configuration P a g e 3 | 12

↑↓

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Element 1s 2s 2px 2py 2pz 3s Electron ConfigurationHLiOFNeNa

Exceptional Electron Configuration

There are always exceptions to the rules Cr : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 1 Cu :1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1 Exceptions due to subtle electron interactions in orbitals with similar

energies

Light

The study of light led to the quantum mechanical modelo Newton stated: light consists of particleso Huygens stated: light travels in waves

Formula:o C = λ ν

Speed of light (C) Wavelength (λ) Frequency (ν)

Electromagnetic Spectrum

The arrangement of types of radiation from long wavelengths to short wavelengths1. What color in the visible spectrum has the longest wavelength? ______2. Which color in the visible spectrum has the highest energy? _________

Calculation

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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.

Atomic Spectra

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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 = h ν

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

Chapter 6

How did chemists begin to organize the known elements?P a g e 6 | 12

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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 properties3. 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. Metals2. 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. Carbon (C ) ______________2. Boron (B) ________________3. Calcium (Ca) _____________4. Barium (Ba) ______________5. Copper (Cu) ______________

6. Bromine (Br) ______________7. Neon (Ne) ________________8. Silicon (Si) _______________9. 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 metalso Group 2A: alkaline earth metalso Group 7A: halogens

Elements are arranged in families based on electron configuration:

Noble Gases: Elements in group 8A

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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) Written Electron Configuration

Group 4A: four elements in the highest occupied energy level

Element (Symbol) Written Electron ConfigurationP a g e 9 | 12

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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 arrowsindicating the trend:

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

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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 arrowsindicating the trend:

Ionization Energy

Ionization energy is the energy required to __________an electron from an atom.

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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 arrowsindicating 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 arrowsindicating 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 arrowsindicating the trend

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