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Atomic Theory of Matter
Chemical Analysis
The Shell Model
Periodicity
Quantum Mechanical Model
100
These small particles are the fundamental units of matter.
What are atoms.
100
This formula is the lowest whole number ratio of atoms in a compound.
What is an empirical formula.
100
The minimum energy needed to remove the least tightly held electron from an atom or ion.
What is first ionization energy.
100

Elements display periodicity in their properties when organized by….

Increasing atomic number.

100

The most probable location of an electron.

The Orbital.

200
Particles that are identical in mass and fundamental chemical properties, make up these substances.
What are Elements.
200
This is the term for the concentration of an element in a compound or a component in a mixture.
What is mass percent.
200
The farther an electron is from the nucleus, the ________ its ionization energy.
What is lower.
200

As you travel left to right across the table, electronegativity ….

As you travel from the top to the bottom of the table, electronegativity….

Increases, Decreases
200

The intrinsic electron property responsible for magnetic moments.

Spin.

300
This theory says that matter cannot be created or destroyed.
What is Law of Conservation of Matter.
300
The fundamental scientific unit for measuring large quantities of very small entities such as atoms, molecules, or other specified particles.
What is the Mole.
300

Shells are formed by groups of electrons with __________ ionization energies.

What is relatively close.

300

This is the reason for the noble gases’ very high ionization energies.

Full valence shells.

300

There are 18 electrons required to fill this energy level.

3rd PEL.

400
A substance that always contains the same atoms in the same ratio.
What is a chemical compound.
400
Name one purpose of calculating mass percent.
To test the purity of a compound OR determine its identity.
400
This law is the basis for the shell model. Explain it.
What is Coulomb's Law. The force between two charged particles is proportional to the magnitude of each of the two charges and inversely proportional to the square of the distance between them.
400

Atomic radius decreases as you travel left to right across the table. Why?

Greater Effective Nuclear Charge.

400

Valence electrons are located in the last of these 2 orbitals.

S and P
500
John Dalton said that atoms are in_______ and          in______.
What is Indivisible and Indestructable
500
The name for the number of constituent particles, usually atoms or molecules, that are contained in the amount of substance given by one mole.
What is Avogadro's number.

Bonus: Add $150 to your total if correct

Q: What is Avogadro's number?

A: 6.022140857 x 10^23

500
The energy measurement of electrons emitted from solids, gases, or liquids by the photoelectric effect, in order to determine the binding energies of electrons in a substance
What is photoelectron spectroscopy.


Bonus:Add $150 to your score if correct.

Q: Define the photoelectric effect

A: When high energy photons hit an atom, molecule, or solid surface  an electron can be emitted if the energy of the photon is greater than the ionization energy of the matter.

500

The ability of an atom's inner electrons to shield its positively-charged nucleus from

its valence electrons.

Electron Shielding.

500

The principle that states that in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels

The Aufbau Principle