AUgh midterm self reflection

Pauli Exclusion Principle

no 2 electrons in an atom can have exactly the same energy

Hund’s Rule

For degenerate orbitals (same energy), the lowest energy is attained when the number of electrons in the same spin direction are maximized

Aufbau Principle

As protons are added one by one to the nucleus to build up the elements, electrons are similarly added to hydrogen-like orbitals

Plum Pudding Model

J.J. Thomson, 1897. All atoms contain electrons. Conducted the cathode-ray experiment and discovered electrons.

John Dalton

1800s

1. All elements consist of atoms

2. All atoms of the same elements are identical

3. Atoms cannot be created or destroyed

Neils Bohr

1913. Explained why atoms only emit light of fixed wavelengths

Rutherford

1911. Conducted the gold foil experiment. Discovered the location of electrons and the existence of the nucleus.

Shrodinger

Electrons paths cannot be predicted. Electron cloud discovery

Hess’s Law

In gaining from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps.

Alkali/Alkaline-Earth metals + H2O →

Metal_Hydroxide (MetalOH) + H2 (g)

Active metals + Acid →

Salt of acid + H2 (g)

Metal_Carbonates + Acid →

CO2, H2O, Salt of acid

Metal_Sulfites + Acid →

SO2 + H2O + Salt of acid

Carbonate Decomposition

Metal_Oxide + CO2

Chlorate decomposition

Metal_Chloride + O2 (g)

Ammonium Hydroxide

NH3 + H2O

Gas Laws: As Temperature Increases,

Volume Increases and Pressure increases

Gas Laws: As particles are added

volume increases and Pressure increases

Gas Laws: As volume increases

pressure decreases

Water vapor eq

P(total) = P(atmosphere) + P(H2O)

Graham’s Law of Effusion

Determines how fast a gas will travel.

Pgas > Patm

Pgas = Patm + H

Pgas < Patm

Pgas = Patm + H

Kinetic Molecular Theory

The ideal gas. These laws are not true when applied to extreme conditions.

1. Gases are tiny gas particles. Their volume is zero

2. Gases always move in straight lines

3. There are no attractive forces

4. Kinetic energy depends on K temp.

Properties of Ionic Compounds

Soluble in water

Charged ions

Not conductible in a solid state

Solid at room temperature (Except Hg)

<= 1.7 electronegativity

High melting points

Metal + Nonmetal

Total transfer electrons

Properties of Covalent Compounds

Polar & Nonpolar determines solubility

Low melting point

No/partial charge

Nonmetal + Nonmetal

Low En difference

Properties of Metallic Substances

Mobile ions

Rigid solids

High boiling point (like, really high.)

Luster

Ductile

Malleable

High Ionization energy

There are 2 bonds and 0 unused e pairs. Qu’est-ce que c’est?

Linear, 180 bond angle, sp hybridization

There are 3 bonds and 0 unused e pairs. Qu’est-ce que c’est?

Trigonal Planar, 120 bond angle, sp2 hybridization

There are 4 bonds and 0 unused e pairs. Qu’est-ce que c’est?

Tetrahedral, 109.5 bond angle, sp3 hybridization

There are 3 bonds and 1 unused e pairs. Qu’est-ce que c’est?

Pyramidal, 90-109.5 bond angle, sp3 hybridization

There are 2 bonds and 2 unused e pairs. Qu’est-ce que c’est?

Angular, 90-109.5 bond angle, sp3 hybridization (like H2O)

There are 5 bonds and 0 unused e pairs. Qu’est-ce que c’est?

Trigonal Bipyramidal, 90 and 120 bond angles, sp3d hybridization

There are 6 bonds and 0 unused e pairs. Qu’est-ce que c’est?

Octrahedral, 90 bond angle, sp3d2 hybridization

Network Covalent Bonds

Insoluble

Hard

High melting point

Arrangement affects properties

Found in large covalent compounds

Poor conductors of heat and energy

Ex. carbon, silicon

Coordinate Covalent Bonding

When two particles, one that is positively charged and one has a lone pair of electrons, bond and one shares both of the lone electron pairs. That’s the best i can explain it.

[NH3-] + [H+]

N has a lone pair of electrons. [H+] has no electrons. N shares both electrons with [H+] to bond.

Sigma Bonds

Single bonds. Stronger than Pi bonds

Pi bonds

Double bonds. Weaker than Sigma Bonds.