Chemistry Unit 2

H⁺

Li⁺

Na⁺

K⁺

Rb⁺

Cs⁺

Ag⁺

Mg²⁺

Ca²⁺

Sr²⁺

Ba²⁺

Zn²⁺

Fe²⁺

Fe³⁺

Al³⁺

NH₄⁺

F^-

Cl^-

Br^-

I^-

O^2-

S^2-

N^3-

P^3-

OH^-

CN^-

NO₃^-

C₂H₃O₂^-

SO₄^2-

HSO₄^-

CO₃^2-

HCO₃^-

PO₄^3-

Mass (or matter) is not created or destroyed in chemical reactions. The total mass of all products equals the total mass of all reactants.

Compounds consist of elements combined in definite proportions by mass

1.007 amu

1.008 amu

0.000549 amu

the number of protons = the number of electrons

superscript on top

subscript lower number

Groups of bonded atoms with a net charge

Ions derived from single atoms

positive ion

negative ion

how electrons are distributed in the cloud

wavelength X frequency = C

• Inversely. 
• short wavelength-----high frequency
• long wavelength------low frequency

• m
• cm
• micrometers
• nm
• Angstroms

• s^-1
• Hz
• kHz
• MHz

• E= h x frequency
• h=plank's constant

only certain discrete values are allowed

• wavelength = 
• h= plank's constant

a branch of physics that deals with light and subatomic particles that exhibit wave-particle duality

• 1- principal quantum number (n)
• 2- angular momentum quantum number (l)
• 3- magnetic quantum number (ml)

• n
• the quantum number most directly related to the size. Associated with shells of electrons.

• l
• aka secondary quantum number or azimuthal quantum number
• related to the shape of the orbital's electron density map (electron cloud)
• has a range of 0 up to n-1
• associated with a subshell

• Spherical
• known as the s orbital

regions of zero electron density within an s orbital.

• dumbell
• known as the p orbital

• It's complicated
• can be 2 different shapes like a flat four leaf clover or a baby pacifier
• known as the d orbital

f orbital

• m_l
• related to how an orbital is aligned in 3-dimensional space
• ranges from -l to l

-1, 0, 1

1

3

-2, -1, 0, 1, or 2

5

-3, -2, -1, 0, 1, 2, or 3

7

• spin quantum number
• can be either +1/2 or - 1/2

no two electrons in an atom can have the same values for all 4 quantum numbers

Chromium and Copper

Atoms tend to lose, gain, or share valence electrons in order to be left with or to reach that ns²p⁶ configuration

the highest numbered shell

• the energy required to remove an electron from a gas phase atom
• X(g) + energy = X⁺(g) + e

From left to right

• the energy change occurring when an electron is added to a gas phase atom
• X(g) + e^- = X^-(g) + energy

As you move to the right and up

As you move down and left

the bigger the atomic size

smaller

bigger

A set of ions and atoms that all have the same number of electrons (and therefore the same electron configuration)

The higher the atomic number, the smaller the ion or atom is

Aluminum, Zinc, Silver, and Cadmium

-ide

• group of atoms with an overall net ionic charge
• have special names

• zero net charge
• total positive charge = total negative charge

simplest combination of ions that gives a charge balance in an ionic compound

When you have two even charges

• sodium chloride
• NaCl

• sodium hypochlorite
• NaClO

• sodium bicarbonate
• NaHCO₃