Chemistry Honors - Electron Configuration, The Periodic table, The Electron

Like the Bohr model, the quantum mechanical model of the atom _______________

Restricts the energy of electrons to certain values.

The quantum model doesn’t define a _________ an electron takes around the nucleus.

Specific path

The cloud is more dense where the probability of finding the electron is

higher

What is the 2nd Quantum number?

the Azimuthal Quantum number

Azimuthal Quantum number

Symbolized with an “l.” Is expressed with letters: s, p, d, f. Indicates the shape of an orbital.

s orbitals are

Spherical

p orbitals are

Dumb-bell shaped

d orbitals are

mostly clover-leaf shaped

f orbitals are

complex and multi shaped

What is the 1st Quantum number?

The “Principle Quantum Number”

What is the 3rd Quantum Number?

the Orientation/Orbital quantum number

Orientation/Orbital quantum number

Symbolized by m_1. Describes the different orientation on the Cartesian axis (x, y & z). Limits how many electrons that each sub level (s, p, d, f) can hold.

What is the 4th Quantum Number?

Symbolized by m_s. Each orbital can hold at most 2 electrons

The arrangement of electrons in an atom is called the atom’s

Electron configuration

What is the Aufbau Principle?

Electrons fill the lowest energy orbitals first. Always start with 1s. “Lazy Tenant Rule”

What is the Pauli Exclusion Principle?

An orbital can hold a max of 2 electrons. The electrons must spin in opposite directions. Depicted with arrows pointed in opposite directions.

What is Hund’s Rule?

Within a sublevel, place one electron per orbital before pairing them. “Empty Bus Seat Rule.”

What are Orbital Diagrams?

Represent the electrons as arrows drawn in boxes.

What did John Newlands conclude?

(1865) That when elements were arranged in order of increasing atomic mass, the properties of elements repeated every 8 elements.

Mendeleev

(1869) Russian Chemist published the first periodic table and arranged it by atomic mass. Predicted the existence of missing elements.

Henry Moseley

(1913) English chemist who developed the concept of atomic number. The periodic table was then arranged according to atomic number.

Period 1

2 elements: H & He

Periods 2/3

8 elements

Periods 4/5

18 elements

Periods 6/7

32 elements

Decreases in size because when more protons are added to the nucleus, the total positive charge increases which pulls the electron shells inward

Cations (+ion) because it is making the electrons smaller.

Electrons are gained in size as electrons move farther from the nucleus

Anions (-ion) because it is making the electrons bigger.

Atoms want a stable __________, for all elements (except H & He) this means having ___ valence electrons. Is Also called the _______

Electron configuration, 8, Octet Rule.

Atoms with low ionization energies are more likely to _____ and gain a _____

Lose electrons, positive charge

__________ is the energy change that occurs when an atom ____ an extra electron. What ion primarily corresponds with this energy change?

Electron affinity, gains, Anion

__________ is the energy needed to ______ an electron. What ion primarily corresponds with this energy change?

Ionization energy, remove, Cation

The behavior of an electron can be modeled by the behavior of

Light

Light has both ____ and _____ properties.

Wave, particle

Light behaves as a ____ when _________ through space.

Wave, traveling

Light behaves as ________ when interacting with matter.

Particles

Light is a type of ______________ radiation that travels through space as a wave.

Electromagnetic

Other examples of electromagnetic radiation are

X-rays, radio waves, and gamma rays.

All waves can be described in terms of 4 characteristics:

Amplitude, wavelength, frequency, and speed.

Amplitude

Is the ______ of the wave measured from the origin to its crest or peak.

The _______ or _______ depends on amplitude

Brightness, intensity

Wavelength

The distance between equivalent points on a wave. Usually measured from crest to crest or trough to trough.

Frequency

How fast the waves oscillates go up and down.

Frequency is measured by the number of waves that pass a given point ___ ______.

Per second.

Regardless of its wavelength, light moves through space at a ______ _____.

Constant speed

Because light moves at a constant speed there is a _______ between ________ and ________.

Constant speed, frequency, wavelength

What is the unit for the speed of light?

3.00 × 10^8 m/s

What are the common units of wavelength?

m, nm

What is the unit of frequency?

Hz, 1/5

The colors that combine to form light (ROYGBIV) are known as the

visible spectrum

Visible light only constitutes a ____ ______ of the total EM spectrum. The rest of the electromagnetic spectrum is ______ to the naked eye.

tiny portion, invisible

In 1900, the German physicist ________ hypothesized that energy, instead of being given off in continuous waves of energy, is given off in little packets of energy, or quanta.

Max Planck

Used Planck’s equation to explain his work on the photoelectric effect

Albert Einstein

Einstein realized that according to Planck’s equation that the energy (and thus the frequency) of the light determines whether or not it has sufficient _____ to knock an electron from the atom.

Energy

For each metal, a _______ frequency of light is needed to release electrons.

Minimum

When light passes through a prism, it splits into a pattern of individual lines containing only certain colors called a ____ _______

Line spectrum

Each element has its own unique line spectrum known as an ______ _______ ______.

Atomic emission spectrum

In 1911, Danish physicist ____ ____ put Rutherford’s atomic model & Planck’s quantum theory together to begin to explain the line spectra

Niels Bohr

In 1924, a French graduate student in physics named ___________ proposed that all moving particles travel as waves, not in straight-line circular orbits as suggested by Bohr.

Louis de Broglie

In 1926, Austrian physicist ____ ________ furthered the wave-particle theory proposed by de Broglie.

Erwin Schodinger

“It is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.”

Heisenberg Uncertainty Principle