History of Chemistry
Parts of an Atom
Atomic Masses
What is Matter?
Periodic Table
100

A Greek philosopher who came up with the idea of "Atomos" and different shapes for different atoms.

Democritus

100
The inner part of an atom that contains the proton and the neutron is called the __________.
Nucleus
100

What atoms are mostly made up of.

Empty space.

100
This is anything that takes up space (has a mass).
matter
100
Atomic numbers of an atom are the same as the number of what in an atom?
protons
200

The person who discovered that atoms can rearrange themselves through chemical reactions

John Dalton

200
These particles have a positive charge and are found inside the nucleus.
proton
200

The atomic weight of Gallium

69.7

200
The smallest pieces of matter are called __________.
atoms
200

The name of the last column of the periodic table

Noble Gases

300

The person who came up with the "cathode ray tube" experiment and made the "plum pudding" model.

JJ Thompson

300
These particles are located within the nucleus, and have no charge.
Neutron
300
A proton has the atomic mass of what?
1
300
What type of particle holds the protons and neutrons together in the nucleus?
mesons
300
What element has a number of 56?
barium
400

The person behind the most recent model of atoms and electrons, with different energy levels of electrons

Niels Bohr

400
These particles are negatively charge and are found outside the nucleus.
electrons
400
A neutron has the atomic mass of what?
1
400

Two different words for the transformation of liquid into gas.

Boiling and evaporation

400
Why does hydrogen have an atomic number of 1?
because it only has one proton
500

The person who used the gold-foil experiment and discovered alpha/beta/gamma rays and discovered that atoms were mostly empty space

Ernest Rutherford

500

Most of the mass of an atom is located here.

nucleus

500
An electron has a mass of what?
1/1836
500

Another name for a part of an energy level of an electron.

orbital

500

Why some atomic masses are not whole numbers.

They are a weighted average of naturally occurring isotopes.

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