Honors Chemistry Unit 4-5 Test WCHS Mrs. Herrick

Dalton’s Atomic Theory

Matter is made of tiny atoms; atoms of the same element are identical, atoms of different elements are different. Atoms combine in whole-number ratios to form compounds, and chemical reactions rearrange atoms without creating or destroying them

Billiard Ball Model

John Dalton’s model of the atom, which describes atoms as solid, indivisible spheres— like tiny billiard balls— that make up matter

What subatomic particle did Thompson discover?

Electron

What subatomic particle did Rutherford discover?

Proton

What subatomic particle did Chadwick discover?

Neutron

Plum Pudding Model

J.J. Thompson’s model of the atom, which describes the atom as a positively charged “pudding” with negatively charged electrons (plums) scattered throughout

Bohr Planetary Model

Niels Bohr’s model of the atom, where electrons orbit the nucleus in fixed energy levels, like planets orbiting the sun

Quantum Mechanical Model (Schrodinger)

The modern atomic model where electrons are found in regions called orbitals, and their positions are based on probabilities rather than fixed paths

Democritus

An ancient Greek philosopher who first proposed that matter is made of tiny, indivisible particles called atoms (no experimental testing)

Aristotle

An ancient Greek philosopher who believed that all matter was made of four elements— earth, water, fire, and air— and rejected the idea of atoms (no experimental testing)

Joseph Priestley

A scientists who discovered oxygen and studied gases, helping to advance chemistry

Antoine Lavoisier

Known as the “Father of Modern Chemistry”, he named oxygen and hydrogen, proved the Law of Conservation of Mass, and helped transform chemistry into a quantitative science

What type of electron configuration is listed?: 1s² 2s² 2p⁴

Full version

What type of electron configuration is listed?: [He] 2s² 2p⁴

Noble Gas (shorthand) version

Label the sublevels

1. S-block

2. D-block

3. P-block

4. F-block

Which sublevel orbital is pictured?

S-block

Which sublevel orbital is pictured?

P-block

Which sublevel orbital is pictured?

D-block

Hund’s Rule

Electrons will fill empty orbitals of the same energy singly before pairing up, and all singly-filled orbitals have parallel spins

Pauli Exclusion Principle

No two electrons in the same atom have the same set of four quantum numbers, meaning each orbital can hold a maximum of two electrons with opposite spins

Aufbau Principle

Electrons fill orbitals starting with the lowest energy level first before moving to higher energy levels 

Heisenberg Uncertainty Principle

It is impossible to know both the exact position and exact momentum of an electron at the same time— the more precisely one is known, the less precisely the other can be known

Excited State

When an electron absorbs energy and moves to a higher energy level than its ground state

Ground State

The lowest energy state of an atom, where all electrons are in their normal, lowest-energy orbitals 

Flame Test

A test where light is emitted when electrons in an atom absorb energy, jump to a higher energy level, and then return to the ground state, producing characteristic colors for different elements

Spectroscopy

A technique that analyzes the light emitted or absorbed by atoms or molecules to identify elements and determine their energy levels

What is represented by this symbol?: λ

Wavelength

Wavelength

The distance between two consecutive peaks or troughs of a wave

What is represented by this symbol?: ν

Frequency

Frequency

The number of wave cycles that pass a point per second 

Planck’s Constant

A fundamental constant that relates to the energy of a photon to its frequency (E=hν)

Speed of Light

The constant c = 3.00 × 10⁸ m/s, which is the speed at which light travels in a vacuum

Emission Spectrum

A spectrum of light emitted by excited electrons as they return to lower energy levels, showing specific colors or lines unique to each element 

Absorption Spectrum

A spectrum showing dark lines where light has been absorbed by electrons, indicating the specific wavelengths absorbed as electrons jump to higher energy levels

Continuous Spectrum

A spectrum that contains all wavelengths of light without gaps, producing a smooth rainbow of colors

The order of all types of waves (longest wavelength, lowest energy →shortest wavelength, highest energy)

1. Radio Waves

2. Microwaves

3. Infrared (IR)

4. Visible Light (red has the longest wavelength, violet has the shortest)

5. Ultraviolet (UV)

6. X-rays

7. Gamma Rays 

Relationship between wavelength, frequency, and energy

1. Wavelength and frequency are inversely proportional: c=λν

2. Energy and frequency are directly proportional to frequency: E=hν

3. Energy is inversely proportional to wavelength: E=hc​/λ

Quantum of Energy

The smallest amount of energy that can be absorbed or emitted by an atom, corresponding to one photon of light

How are isotopes of the same element the same and different?

They have the same protons and are the same element, but have different neutrons and mass 

What is the difference between a cation and an anion?

A cation is a positively charged ion (loses electrons), and an anion is a negatively charged ion (gains electrons)

Which model is shown and who created it?

Billiard ball model created by Dalton

Which model is shown and who created it?

Plum pudding model created by Thompson

Who created this atomic model?

Rutherford

Who created this atomic model?

Chadwick

What is this atomic model and who created it?

Planetary model created by Bohr 

What is this atomic model and who created it?

Quantum mechanical model by Schrodinger

Label the diagram

1. Excited

2. Ground

Which spectrum is pictured?

Emission spectrum

Which spectrum is pictured?

Absorption spectrum

Which spectrum is pictured?

Continuous spectrum

Who created the gold foil experiment?

Rutherford

Who didn’t know position/movement of electrons?

Heisenberg

Who developed the complex math of the motion of electrons?

Schrodinger

What are isotopes?

An element with the same number of protons and a different number of neutrons 

What does “A” mean?

Atomic mass

What does “Z” mean?

Atomic number

What part of the atom is the most dense?

The nucleus

What are valance electrons?

The electrons in the outermost shell of an atom, which are involved in forming chemical bonds 

What is common about the shorten configurations of the elements that are in the same column of the periodic table?

They have the same number of valance electrons

What is an amu?

A unit of mass used for subatomic particles, atoms, and molecules

What parts of the isotope does the amu equal?

The sum of its protons and neutrons