Chapter 2: nomenclature

binary acids

Hydrogen + 1 non-metal

• hydro + nonmetal root + ic acid

terenary compounds

3+ different elements

• name cation first then anion

• don’t change polyatomic ion name

• use roman numerals

oxyacids

Hydrogen + oxygen + one other element

• omit “hydro”

• “ate” endings → “ic acid”

• “ite” endings → “ous acid”

atomic mass

• the weighted average of all naturally occuring isotopes of an element

• m₁a₁ + m₂a₂ + m₃a₃ etc…

mass number

• the mass of one specific isotope of an element

• protons + neutrons

halogens

• group 17 on the periodic table

• react easily with other elements

• readily available in nature

organic vs inorganic chemistry

organic: compounds containing carbon-hydrogen bonds

inorganic: compounds that don’t have c-h bonds (salts, minerals, metals, acids)

electronegativity

• how strongly an atom attracts electrons towards itself when it is bonded with another atom

• sometimes one atom attracts the shared electrons in a bond more strongly and pulls it

electron sharing in ionic bonds

• electrons are transferred between two elements, forming oppositely charged ions that attract

• ex: Na loses an electrons to become + (10 electrons now) → Cl gains that electrons to become - (18 electrons now)

• they do this to become stable, and have an equivalent # of electrons to the nearest noble gas

electron sharing in covalent bonds

• atoms share pairs of electrons to fill shells

nonpolar covalent bond

• equal sharing/attraction of electrons

• no positive or negative end forms

• ex: H₂. they are the same element so share equally

polar covalent bond

• uneuqal sharing/attraction of elements, one element has higher electronegativity than another

• creates partial charges

• ex: HCl. Cl has higher electronegativity than H so it becomes slightly more negative