Chemistry Exam

The naming of compounds based on how they bond.

Nomenclature

A bond formed when opposite charged atoms attraction with each other with transfer of valence electrons. (metal to non-metal) or (metal to non-metal group).

ionic bond

an atom with a charge. Cation is positive(loss of valence electrons) and anion is negative(gain of valence electrons.

ion

a single-atom ion. (never a group)

Monatomic ion

ions made up of more then one atom. (group ion)

polyatomic ion

the bond that results from the sharing of valence electrons. (non-metal to non-metal)

covalent bond

how closely an atom lies to a neighboring atom.

Atomic radii

the electrons located in the outermost shell (energy level) of an atom.

valence electrons

the elements are arranged in increasing atomic number order.

periodic law

a chemical rule that atoms tend to lose, gain, or share electrons so that they have exactly eight electrons in their outermost shell.

octet rule

the properties repeat every 8th element.

law of octaves

(series) horizontal rows

period

(families) vertical columns

group

metallic elements occupying Groups 3 through 12 of the periodic table.

transition metals

the six highly reactive, soft, and shiny elements in Group 1.

alkali metals

the six chemical elements that make up Group 2 of the periodic table.

alkaline earth metals

group of highly reactive non-metallic elements found in Group 17.

halogens

group of chemical elements found in Group 18 of the periodic table.

noble gases

father of modern chemistry. (1790)

Lavoisier

arranged elements in atomic mass order. Left blank spaces. (1869)

Menedeleev

atomic #, put the elements in increasing order. (1913)

Mosely

law of octaves - every 8th element. (1864)

Newlands

seven elements that naturally for 2 - atom molecules due to increased stability(need octet).

Diatomic molecules

a pure substance made entirely of a single type of atom, defined by its number of protons.

Elements

metal to non-metal or metal to non-metal group.

ionic compounds

groups of atoms held together by covalent bonds.

covalent molecules

the mass in grams of 1 mol of any pure substance.

molar mass

1 mol Na = 6.02 × 10²³ atoms Na

1 mol FeCl₃ = 6.02 × 10²³ formula unit FeCl₃

1 formula unit FeCl₃ = 4 total atoms = 1 atom Fe = 3 atoms Cl

mole calculation examples. (conversion)

a substance or process that speeds up the reaction. (written above yield arrows).

catalyst

Unexpected color changes, energy changes(cold or hot, no heat source), Odor changes, and Precipitate. Gas produced - bubbles (no heat source), irreversible process, and new properties.

chemical reaction evidence

heat, light, compounds or elements, and aqueous solution.

things used as a catalyst in chemical reactions.

the ratio of the actual and theoretical yield expressed as a percent. 33.4/45.0 × 100 = percent%

percent yield

the max amount of product that can be produced by a given amount of reactant. (the bottom piece of the ratio from your calculation).

theoretical yield

the quantity that is recovered from the lab. (from ex-percent).

actual yield

the study of the quantitative relationships. Balancing (total mass of reactants = total mass of products) Mole ratio.

Stoichiometry