Unit 2 flashcards (Atomic Theory)

Atoms

The small particles which make up everything and anything.

Subatomic Particles

particles inside the atom. (Smaller than atoms)

Nucleus

In the center of the atom. Contains 2 subatomic particles.

Orbitals/ clouds

circles on the outside of the atom. Contains 1 subatomic particle.

Protons

Positively charged (+1 charge), subatomic particles. Weighs 1 amu. Found in the Nucleus.

Neutrons

Neutrally charged (0 charge), subatomic particles. Weighs 1 amu. Found in the nucleus

Electrons

negatively charged (-1 charge), subatomic particles. Has a negligible mass. Found in the orbitals/ clouds.

amu

atomic mass unit

Negligible

so small we pretend it dosent exist

Atomic Number

number of protons in an atom. Defining characteristic of all elements.

Atomic Mass

Number of protons and neutrons in an atom (Average number of all isotopes of an element)

Isotopes

Atoms that have the same atomic number,but different atomic masses. (The same element but different masses)

Avogadro’s number

A mole, which is like a dozen in real life.

Mole

6.022x10²³

Dalton's theory

Realized that matter had to be made of particles, that could not be broken apart or destroyed. Created the particle model (Just a sphere representing the particle).

Thomson’s Atomic Theory

Used the plum pudding model and found that atoms were negatively charged. Thus finding electrons.

Rutherford's Atomic Theory

Used the gold foil experiment, and figured out there was space in the atom. Made the nuclear model, which showed a nucleus with electrons around it. Figured out protons as well as the nucleus.

Bohr's Atomic theory

Expanded off Rutherford using advanced psychics dealing with electromagnetic energy. Found the electron clouds. Made the planetary model which shows the nucleus and the orbitals which look like planet rings

Schrodinger's model

Expanded off Bohr by making the model 3D. Shows the clouds as expanded balloons and spheres for the nucleus.

Attractive force and distance

The larger, the less attractive force, and vise versa

Attractive force and protons

The more there are, the greater the attractive force.

Ions

Elements or atoms with the wrong number of electrons. (Has a charge). When protons ≠ Electrons

Neutral atom

Protons = Electrons. (Has no charge)

Total charge=

Atomic number or protons - Electrons

Ide

The ending for an element when it is an ion.

Oxide ion

Oxygen as an ion

Light spectra

The color spectrum released by atoms, as the electrons lose energ. Unique for each atom.

Shorter wavelengths

give off colors like: Violet and blue.
Have more energy

Longer wavelengths

Give off colors like: Orange and Red.
Have less energy.

Excited State

When the electrons have more energy and jump up energy levels/ orbitals

Ground State

When the electrons are back to their original orbitals

Photon

Particle of light

Valance Electrons

Electrons on the outside of the atom (farthest orbital/cloud)

Group 1

Group on the periodic table with 1 Valence electrons

Group 2

Group on the periodic table with 2 Valence electrons

Group 13

Group on the periodic table with 3 Valence electrons

Group 15

Group on the periodic table with 5 Valence electrons

Group 18

Group on the periodic table with 8 Valence electrons

Middle groups

Groups on the periodic table that have a random amount of valence electrons.

Orbital S

Orbital that can hold 2 electrons

Orbital P

Orbital that can hold 6 electrons

Orbital d

Orbital that can hold 10 electrons

Orbital f

Orbital that can hold 14 electrons

Energy level 1

Energy level with only orbital S

Energy level 2

Energy level with orbitals S and P

Energy level 3

Energy level with orbitals S, P, and d

Energy level 4+

Energy level with all orbitals S, P, d, and f.

Hydrogen electron notation

1s¹

Lithium electron notation

1s² 2s¹