"AP Chemistry - Electronic Structure of Atoms and Quantum Theory Review"

Wavelength

Wavelength

Distance between two points on a wave. The unit of measurement is METERS (but can be measured in cm and nm)

Frequency

Number of complete waves that pass a point each second. The unit of measurement is Hz (1/s)/

Speed of light = wavelength x frequency

c = λv

Inverse

Frequency and wavelength are what proportion?

Long wavelength

Low energy and frequency gives what type of wavelength?

Short Wavelegth

High energy and frequency gives what type of wavelength?

Speed of light constant

3.00 x 10^8 m/s

Wavelength and frequency

Each type of energy has a different what?

Energy = Planck's constant x frequency

E = hv

Planck's constant

6.626 x 10^-34 J/s

Photoelectric effect

When light shines on a metal surface causes the electrons to be ejected from the metal.

Photons

Einstein said that light travels in energy packets or what?

Planck's theory

Energy absorbed/released from atoms in certain minimum amounts (quanta). This is assumed.

Electromagnetic Spectrum

Continuous Spectrum

Spectrums from light containing all wavelengths.

Line Spectrum

A spectrum containing radiation of only specific wavelengths.

Ground state

The lowest energy state of an atom (n=1)

Excited state

When the electron is in a higher energy level.

Orbitals

The allowed wave functions of the hydrogen atom.

Electron configuration

A simple way of writing down the locations of all of the electrons in an atom. It describes the distance, energy, and size of orbitals.

Principal quantum number (n)

Represents the distance from the nucleus. Energy levels. (1-7)

Angular quantum number (l)

Represents the shape of the orbital. Sublevels. (0=s, 1=p, 2=d, 3=f).

Magnetic quantum number (ml)

Represents the orientation in space. Axis orientation. (-3, -2, -1, 0, 1, 2, 3)

Spin quantum number (Ms)

Represents the electron spin. Arrow direction. (+1/2 or -1/2).

Aufbau Principle

Electrons fill the orbitals in order of increasing energy.

Spinning change.

What produces a magnetic field?

Diamagnetic

Occurs when all e- are paired.

Paramagnetic

Has one or more unpaired e-.

Pauli Exclusion Principle

Two electrons occupying the same orbital must have opposite spins.

Hund's Rule

Single electrons with the same spin will occupy each orbital with equal energy before pairing.

Orbital Notation

This image represents?

Electron Configuration

This image represents?

Noble Gas Notation

This image represents?

Dimitri Mendeleev

The first scientist to create a periodic table of the elements in order of increasing atomic mass.

Henry Mosley

Rearranged the periodic table to be in order of increasing atomic number.

Periodic Law

When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical and physical properties.

Nanometer (nm)

10^-9

Megameter (Mm)

10^6

Heisenberg Uncertainty Principle

It is impossible for us to simultaneously know both the exact momentum and location. It can only discuss the probability of an electron's position in space.

Higher energy

Lower energy further from nucleus equals what?

De Brogile

Suggested that electrons could behave as waves with a characteristic wavelength.

Effective nuclear charge

The attractive force felt from the nucleus by electrons It depends on the distance from the nucleus and the number of inner electrons. (Result of Coulomb's law)

Down a group

Increase of shielding occurs ONLY when?

Shielding effect

The decrease in attraction between an electron and the nucleus of an atom.
-Atomic radius increases.
-Ionization Energy decreases.
-Electronegativity decreases.
-Zeff (effective nuclear charge) decreases.
-Harder to remove electrons.

Atomic Radius

Half the distance between the nuclei in covalently bonded atoms.
-Decreases left to right
-Increases downward.

Ionization Energy

The energy required to remove electrons.
-Increases left to right.
-Decreases downward.

Electronegativity

Measure of an atom's bond to another atom.
-Increases left to right.
-Decreases downward.

Electron Affinity

The energy change that results in the addition of electrons
-Increases left to right.
-Decreases downward.

The force of attraction of the nucleus is greater than the ground state.

Why is there a huge jump between n=1 and n=2?

Isoelectronic

When a group of ions have the same number of electrons.

Metallic charcter

An element that has the physical and chemical properties of metals.
-Decreases left to right.
-Increases downward.

The attraction of an extra proton.

The distance from the S to P orbital out weighs what?

Repulsion of paired electrons.

As the e- moves to enter an orbital already having 1e- they
pair with opposite spins so the IE drops.
-Outweighs the increased attraction from the nucleus so less energy to remove the e-.

Electron givers

The most reactive metals are the largest since they are the best what?

Electron takers

The most reactive nonmetals are the smallest ones, the best what?

Paramagnetism

The magnetic state of an atom with one or more unpaired electrons.

Diamagnetism

The magnetic state of an atom with paired electrons with no magnetic attraction.

Coulomb’s Law

The strength of the interaction between two electrical charges depends on the magnitudes of the charges and on the distance between them.