FINAL EXAM REVIEW

grrrrr final exam 😡

Oxygen is a pure substance made of one:

molecule

A compound whose name includes prefixes is

molecular

The closer to the bottom right of the periodic table the larger the

atomic radius

acids start with

H

bases end with

OH

aq

dissolved in water

s

solid

l

liquid

g

gas

Combustion

releases heat, light, carbon dioxide, water

valence electrons

Electrons on the outermost energy level of an atom

Single Replacement

one element replaces another element in a compound

double replacement

a chemical reaction where two elements in different compounds trade places

Decomposition

A chemical reaction that breaks down compounds into simpler products.

formation

A chemical reaction where 2 compounds come to make one

neutrilization

the reaction of an acid and a base to form a neutral solution of water and a salt

Precipitation

A chemical reaction where 2 dissolved substances form a solid

precipitate

A solid that forms from a solution during a chemical reaction.

Enthlapy

sum of internal energy - energy change

positive Enthlapy change

increased potential energy of a substance - heat absorbed

Negative Enthlapy change

loss of potential energy - heat released

Exothermic

Chemical Reaction in which energy is primarily given off in the form of heat

Endothermic

Absorbs heat

ionic bond

bond between a metal and a nonmetal - solid at SATP

covanlent bond

bond between 2 non metals - Solid Liquid or Gas at SATP

metallic bond

bond between 2 metals

DURING a phase change temperature is:

the same

John Dalton model of the atom

Billiard ball model

JJ Thomson model of the atom

Plum pudding model - electrons scattered about

Ernest Rutherford model of the atom

Nuclear model - each electron individually orbits nucleus

Niels Bohr model of the atom

Planetary model - Bhor model - electrons have orbitals

De Broglie and Schrodinger model of the atom

quantum model - electrons orbit in a cloud

1s2 2s2 2p6

Neon

Sulfur electron configuration

1s2 2s2 2p6 3s2 3p4

Argon electron configuration

1s2 2s2 2p6 3s2 3p6

how do you simplify electron configuration

go to nearest noble gas and write the rest (1s2 2s2 2p3 -\> [He] 2s2 2p3 -\> nitrogen

\[Kr] 5s2 4d9

Silver

IUPAC non metallic element ending changed to:

ide

IUPAC name of compound does not mention the number of

ions

IUPAC roman numeral indicates

that a metal has two or more ion charges

IUPAC metallic element appears

first

IUPAC nonmetallic element appears

last

IUPAC Ag2S4

disilver tetrasulphide

IUPAC Co2O3

dicobalt trioxide

heterogeneous

different - could see individual particles in solution

homogeneous

of the same kind - solution looks the same all around

molecular compound

non metal and non metal

period

A horizontal row of elements in the periodic table

Group

A column on the periodic table

Bottom left of Periodic Table

Most reactive metal

Top right of periodic table

Most reactive gas

cation

A positively charged ion

Anion

A negatively charged ion

mass of an element

protons + neutrons

atomic number

the number of protons and electrons (if neutrally charge) in the nucleus of an atom

Naming Isotopes

element name followed by mass number

energy level

a region of an atom in which electrons of the same energy are likely to be found

pauli exclusion principle

An atomic orbital may describe at most two electrons, each with opposite spin direction

Aufbau Principle

An electron occupies the lowest-energy orbital that can receive it

Hund's Rule

electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible

Solution

Homogeneous mixture

Solvent

Component of a solution - greater quantity

Solute

Component in a solution - lesser quantity

saturated solution

when a solute dissolves in a solvent until no more will dissolve

Solubulity

the ability of one substance to dissolve in another

When defining solubility you must provide

Solute, amount of solute, solvent, amount of solvent, temp

ionic solution

An ionic compound dissolved in a liquid to form an electrolyte

Electrolyte

An ionic compound whose aqueous solution conducts an electric current

More ions

higher conductivity

If a substance is metal+nonmetal it will form a \_______ solution with water

Ionic

If a substance is nonmetal+nonmetal it will form a \_______ solution with water

Non ionic

Compounds that start with Carbon (organic compounds) don't form ionic solutions in water except:

Organic acids

Metals \_____ \_______

do conduct

Solid non metals \_____ \_________

dont conduct

Acids and Bases \______ \________

do conduct

Ionic compounds \_____ \__________

do conduct

neutral substances \______ \________

dont conduct

Miscible

Describes two liquids that are soluble in each other

Immiscible

liquids that are not soluble in each other

Polar liquids are miscible with

other polar liquids

Nonpolar liquids are miscible with

other nonpolar liquids

ionic compound

A compound that consists of positive and negative ions

Acidic compounds

compounds that have a pH of less than 7 (start with H)

Base Compound

compounds that have a pH of more than 7 (end with OH)

molecular compound

a compound that is composed of molecules

Conductivity

The ability of an object to transfer heat or electricity to another object.

Molarity

the number of moles of solute per liter of solution

C\= n/V

Molar concentration formula

stock solution

a concentrated solution of a substance used to prepare solutions of lower concentration

dilute

To make a liquid less concentrated

concentrated solution

a solution containing a large amount of solute

Cv\=cv

Dilution formula

Lewis acid

an atom, ion, or molecule that accepts an electron pair to form a covalent bond

Lewis base

an atom, ion, or molecule that donates an electron pair to form a covalent bond

Dissociation

when ionic compounds separate into cations and anions

Ionization

any process that results in the formation of an ion

ion concentration

Actual concentrations of ions of a dissolved ionic compound depends upon the stoichiometry of cations and anions

colligative properties

properties that depend on the concentration of solute particles but not on their identity

Precipitation

the process of transforming a dissolved substance into an insoluble solid

precipitate

A solid that forms from a solution during a chemical reaction.