Chapter 1-8 Chemistry Notes

Vocabulary flashcards covering key terms and concepts from the lecture notes on exam setup, calculations, polyatomic ions, naming conventions, pure substances, and common compounds.

Hydroxide

OH−, a -1 charged polyatomic ion.

Nitrate

NO3−, a -1 charged polyatomic ion.

Nitrite

NO2−, a -1 charged polyatomic ion.

Carbonate

CO3^2−, a -2 charged polyatomic ion.

Sulfate

SO4^2−, a -2 charged polyatomic ion.

Phosphate

PO4^3−, a -3 charged polyatomic ion.

Bicarbonate (hydrogen carbonate)

HCO3−, hydrogen carbonate, a -1 charged polyatomic ion.

Acetate

C2H3O2−, acetate, a -1 charged polyatomic ion.

Ammonium

NH4+, the positively charged polyatomic ion.

Cyanide

CN−, a -1 charged polyatomic ion.

Endings -ite vs -ate

-ite ending is associated with the ion form described in notes as the “individual elements”; -ate ending indicates more oxygenated, polyatomic ions.

Water

H2O, the common name for the molecule; in this course, the formula is used for the compound.

Sucrose

C12H22O11, table sugar; the chemical name for sugar.

Methane

CH4; methane is the molecule also referred to as carbon tetrahydride.

Carbide

A term used here to describe carbon in elemental form; “plain carbon” by itself is referenced as carbide.

Pure substance

A substance that is one element or one compound.

Element

A pure substance consisting of a single type of atom.

Compound

A substance formed when two or more elements chemically combine; has a definite formula.

Mixture

A substance made of two or more elements or compounds that retain their own properties.

Chemical formula

A symbolic representation showing which elements are present and in what ratio.

Polyatomic ion

An ion composed of two or more atoms; examples include hydroxide, nitrate, carbonate, sulfate, phosphate, bicarbonate, acetate, ammonium, and cyanide.