Enter Title

Scientific notation

100

5.2 x 10³

5200.

200

9.65 x 10^-4

.000965

300

7.1 x 10³

.0071

400

5.02 x 10^-4

.0000502

500

9.77 x 10⁴

97700

Standard notation

100

0.000000234

2.34 x 10^-7

200

456000

4.56 x 10⁵

300

0.069

0.69 x 10^-1

400

44959177

4.4959177 x 10⁷

500

738

7.38 x 10²

Atomic structure

100

The 3 particles and their charges

What is protons, positive, neutrons, neutral, and electrons, negative 

200

The numbers of Protons in one atom of an element determines the atoms ______ and the number of neutrons determines _________ of an element

What is a Atomic number and Mass number 

300

The ______ of an element is the total number of protons and neutrons in the _______ of the atom

What is atomic mass and the nucleus 

400

The outermost electrons are called _____ electrons and can be identified by the elements ______ on the periodic table. For example CI is a halogen and has 17 valence electrons. 

What is valence electrons and group?

500

The ______ rule is an Atoms tendency to gain or lose electrons to achieve a valence shell of 8 electrons 

What is the octave rule?

Periodic table and trends

100

The vertical rows of the periodic table are called.

What are groups?

200

Atomic radius

What is the total distance from an Atoms neleus to the outermost orbital of electron. 

300

The trend of ionization energy 

What is Increases across a period and decreases down a group. 

400

electronegativity 

the tendency of an atom to attract the bonding electrons. 

500

CL electron configuration 

1s², 2s²,2p⁶,3s²,3p⁵

Nuclear

100

Fission plus example 

When a neutron slams into a larger atom. Ex. uranium and plutonium 

200

3 types of nuclear radiation

alpha rays, beta rays, neutron - gamma rays 

300

Fusion plus example 

2 atoms slam together to form a heavier atom ex: 2 hydrogen atom fuse to form a helium atom