AP Chem Module 2 + 3 Assessment

Democritus and Leucippus Theory

indivisible particles, different sizes and shapes, iron had hooks, salt was sharp, etc.

Dalton’s Theory

indivisible and invisible, arrange in different combinations to make compounds,

Thompson’s Theory

Overall neutral charge (electrons in a positively charged field (plum pudding)), first person to say there are smaller parts

Rutherford’s Theory

gold foil experiment, determined nucleus is in the middle and is positively charged

Bohr Theory

electron spins around nucleus in orbits, rings with different amounts of electrons

Quantum Theory

hyperactive electrons in differently shaped orbitals which says the probability of electrons, neutrons in the center

Atomic Radius trend

smaller on the right because more protons = more pull

bigger as you go down because there’s more rings

Ionic Radius trend

In an ion, the greater the number of electrons, the larger its radius will be.

First Ionization Energy trend

How hard is it to lose an electron

increases as it goes up and right (toward fluorine) because it’s tough to lose an electron because they want to gain one. Also, it increases as it goes up because the lower elements = bigger radius = easier to take an electron.

Electron Affinity trend

How easy it is to gain an electron

also grows toward fluorine because halogens and higher elements want to gain an electron, and it’s easy for them to.

Electronegativity

more likely to gain and electron (F has the highest EN and noble gases don’t have a value)

What are photons?

Packs or “quanta” of energy that are released if a certain frequency of light is used

Energy formula for wavelengths

E = hc/λ

h = planck’s constant

c = speed of light

λ = wavelength

Rydberg Equation

Change in Energy = (-2.18 × 10^-18 J) (1/f² - 1/i²)

Hybridization Steric Numbers

2 - sp

3 - sp²

4 - sp³

5 - sp³d

6 - sp³d²