Chemistry Memorization: Ions, Acids, Bases, and Trends

Flashcards to help memorize key terms, definitions, and chemistry concepts from the lecture notes.

Never hydrogen bond to…

C-H bond groups

London in SEPT

Increase size, electron density, polarizability, temporary dipoles

Bonds in molecular covalent substances

Never break during phase changes

Increasing strengths of IMFs

Increase boiling point, melting point, viscosity, surface temperature

Metallic substances

Conduct electricity as a solid and a liquid,

Ionic substances

Conduct electricity as liquid (often dissolve in water)

Network covalent and molecular covalent

DO NOT conduct electricity

Polyatomic Ion

An ion composed of two or more atoms.

Ammonium

A polyatomic ion with the formula NH4+.

Sulfate

A polyatomic ion with the formula SO4-2.

Hydroxide

A polyatomic ion with the formula OH-.

Solubility Rule 1

Most nitrates are soluble in water.

Ionization Energy Trend

Ionization energy increases from left to right and bottom to top on the periodic table.

Diatomic Elements

Elements that are typically found as pairs of atoms, such as H2, O2, N2.

Strong Acid: Hydrochloric Acid

The chemical formula is HCl.

Tetrahedral Bond Angle

Approximately 109.5°, found in molecules with four bonds and no lone pairs.

Electronegativity Trend

Electronegativity increases from left to right and bottom to top on the periodic table.

Carboxylic Acids

Organic compounds containing the functional group -COOH.

Hydrogen in Metal Hydrides

In metal hydrides, hydrogen has an oxidation state of -1.

Fluorine Oxidation State

Fluorine always has an oxidation state of -1.

Strong Base

Typically hydroxides formed with alkali and alkaline earth metals.

Hydrogen Sulfate Ion

A polyatomic ion with the formula HSO4-.

Chlorate Ion

A polyatomic ion with the formula ClO3-.

Covalent Prefix for 4

The prefix is 'tetra-'.

Atomic Radius Trend

Atomic radius increases from right to left and top to bottom.