Chemistry Grade 11 Exam Review

All things grade 11 chemistry! Includes math parts with stoichiometry

Nomenclature

IUPAC system for naming chemical compounds.

Binary Acids

using “H” plus another element (ex. H2S, H3P)

Ionization energy

the minimum energy needed to remove an electron from a gaseous atom or ion

ionization energy - periodic trend

ionization energy increases down a group and increases left to right across periods

atomic number

number of protons and electrons (unless its an ion), identifies the element

mass number

sum of protons and neutrons

isotope

atoms with the same number of protons but different number of neutrons

ion

atom with lost or gained electrons

AAM

average atomic mass.

atomic radius periodic trend

radius increases down groups and left to right across periods

electron affinity

a measure of the attraction between the incoming electron and the nucleus

empirical formula

formula of a compound in the simplest terms

total ionic equation

all reactants and products separated from each other in the equation, with the exception of solids.

net ionic equation

chemical equation without the spectator ions

spectator ion

ion present in a reaction that does not change during the reaction

synthesis

two elements combine to form a new compound (A + B → AB)

decomposition

a compound is broken down into the elements that make it up (AB → A + B)

single displacement

a compound and a single element react to form a new compound and a different single element (AB + C → AC + B)

double displacement

two compounds react to form two new compounds (AB + CD → AD + CB)

% yield

found by dividing the actual yield (AY) by the theoretical yield (TY)

theoretical yield (TY)

the maximum amount of product produced by a chemical reaction, depending on the amounts of reactants present

actual yield (AY)

the amount of product that is actually obtained or isolated from a chemical reaction

linear molecular shape

can be either polar or nonpolar. symmetrical. shaped like a line.

tetrahedral

can be either polar or nonpolar. symmetrical. 3 molecules at the bottom, one in the middle, and one up top of the middle molecule.

trigonal pyramidal

polar. asymmetrical. one molecule in the middle, three at the bottom. shaped like a pyramid but with 3 corners not 4.

trigonal planar

can be polar or nonpolar. symmetrical. shaped like a collapsed 3 corner pyramid.

bent

polar. asymmetrical. shaped like a boomerang.

molecular polarity

the overall polarity or nonpolarity of a molecule. depends on the individual bond polarities and the molecule’s geometry

bond polarity

the uneven sharing of electrons in a chemical bond between two atoms, resulting a partial positive and partial negative charge on the bonded atoms

intramolecular forces

forces that hold atoms together within a molecule. stronger than intermolecular forces

intermolecular forces

attractive or repulsive forces that exist between molecules/atoms.

hydrogen bonding

a type of attraction between molecules. occurs when an already covalently bonded hydrogen atom is attracted to another electronegative atom (ex. nitrogen, oxygen, fluorine). the strongest intermolecular force

dipole-dipole forces

attractive forces existing between polar molecules. the partially positive portion of one molecule is attracted to the partially negative portion of another molecule.

london dispersion forces

the weakest attractive force that are formed due to temporary dipoles induced in nonpolar molecules.

ion dipole forces

exist in the attraction between a charged particle (ion: cation or anion) and a polar.

dipole induced forces

when a nonpolar molecule approaches a polar molecule (with a permanent dipole), a dipole will be induced in the nonpolar molecule

electronegativity

a measure of an atom’s ability to attract electrons in a chemical bond

C1V1 = C2V2

formula used for finding concentration or volume of two substances by comparison

limting reactant

the reactant in a reaction that is completely used up, thus limiting the amount of product that can be formed

excess reactant

a reactant present in a chemical reaction where there is a greater amount than what is needed to completely react with the limiting reactant

acids

sour in taste, react with metals to produce hydrogen gas

bases

bitter in taste, react with acids to produce salt and water

neutralization

an acid and base react to form a salt and water, bringing the pH closer to 7 (reducing the acidity and basicity)

complete combustion

a fuel reacts rapidly with oxygen, producing carbon dioxide and water as the main products, along with energy in the form of heat and sometimes light. products change depending on the fuel and amount of oxygen present

complete combustion formula

C_xH_y + O2 → CO2 + H2O

incomplete combustion

occurs when a fuel does not burn fully due to insufficient oxygen, producing harmful substances such as CO and unburnt fuel

incomplete combustion formula

ex. CH4 + O2 → CO + O + H2O

molarity

a common way to describe the concentration of a solution. it is the concentration expressed in moles per litre.

electronegativity differences

help you find the type of chemical bond between two atoms and predict the polarity of the bond.