spectrum
ex.
name--> formula
rule
ex.
ex.
ex.
stucture
ex.
ex.
what is a periodic trend?
name--> formula
formula--> name
criss cross
without criss crossing
ex.
what is it?
what is it?
ex.
if there are 8
last shell
represented by
ex.
there are 3 hydrogen atoms
example (product)
example
to indicate the exact state (or phase) the compounds are in before and after the reaction
word equation
ex.
ex.
ex.
ex.
ex.
ex.
has
to
to
ex.
reactants consist of an acid and a base
what tools can we utilize?
why must we balance?
includes
is
example
example
example
the strength of an acid/base can be measured using the
used as tools
can be found on the back of the
may be changed in the balancing of an equation
is determined by
formed by several
form of
is a
bonding
also called multiple oxidation numbers
depend
example (reactants)
produce
also determined by
represented as
is a reaction of this type
if not
is this type of reaction
what do we use to measure?
there are 2 NH3 molecules

C+O2=CO2

Reactions

example

magnesium ribbon when burnt in oxygen is converted into magnesium oxide

occur with

evolution of gas

example

when zinc reacts with hydrochloric acid, hydrogen gas is evolved with formation of zinc chloride

change in color

example

when iron reacts with oxygen and develops an orange-red color from rusting

change in odor/taste

example

rotting food

production of light

example

when oxygen combines with calcium, adenosine triphosphate (ATP) and the chemical luciferin in the presence of luciferase, a bioluminescent enzyme, light is produced.

change in temperature

example

quick lime with water: CaO + H₂0 = Ca(OH)₂ + Heat

change in state

example

Subtopic

Oxidation-Reduction

effect

corrosion

example

rusting

effect

rancidity

example

when butter is kept in the open atmosphere than its smell and taste change

require activation energy for a reaction to occur

Types of Reactions

Double Displacement (AB+CD=AD+CB)

a precipitate must form in order for a reaction to occur

when two elements in different compounds switch places, forming two new compounds

AgNO3 + NaCl → AgCl + NaNO

Synthesis (A+B=AB)

Decomposition (AB=A+B)

when 1 reactant breaks down (decomposes) to form
multiple products

CaCO3→CaO+CO2

Single Displacement (A+BC=AC+B)

when one element displaces another in a compound

2AgNO3(aq)+Cu(s)→Cu(NO3)2(aq)+2Ag(s)

a balanced chemical equation

the number of atoms for each element in the reaction and the total charge is the same for both the reactants and products.

to accurately reflect the law of conservation, that matter is neither created or destroyed

An ERP chart

An ERP chart

reaction will occur when the more active metal displaces the metal that is less active

Combustion (CxHy + O2 = CO2 + H2O + heat energy)

incomplete combustion

when the supply of air or oxygen is poor. H2O is still produced, but carbon monoxide and carbon are produced instead of carbon dioxide.

complete combustion

when a fuel reacts quickly with oxygen (O2) and produces carbon dioxide (CO2) and water (H2O)- when there is a good supply of air.

Precipitation

when an aqueous compound reacts to form an insoluble salt called a precipitate. Whether or not a reaction will form a precipitate is dictated by solubility rules ionic compounds.

Neutralization

Acid + Base = Salt + Water

acids and bases are determined by their pH levels

pH scale

to measure how

acidic

a substance is

basic

ranges from

0.0-6.9

acid

7.0

neutral

can be determined by

indicators

litmus paper

red cabbage water

universal indicator

full color range

< 3

red

strong acid

vinegar (2)

3-6

orange-yellow

weak acid

black coffee (5)

7

green

neutral

pure water (7)

8-11

blue

weak base

baking soda (9)

>11

indigo-violet

strong base

ammonia solution (11)

7.1-14.0

base

very strong acid

very strong base

Acids

Bases

a substance that produces HYDROXIDE IONS (OH⁻) in a solution/take a proton from another compound

physical properties

conduct electricity, slippery touch, water soluble, bitter taste.

chemical properties

corrosive, denature protein and digest fats, react with acids to make neutral solutions.

most bases contain ions/are ionic compounds that contain a metal and a hydroxide polyatomic group

NaOH = sodium hydroxide, Al(OH)3 = aluminum hydroxide

naming rule

"__________hydroxide"

Chemical Equations

include

states

aqueous (aq)

solid (s)

gas (g)

liquid (l)

HCH3CO2(aq)+NaHCO3(s)→CH3CO2Na(aq)+H2O(l)+CO2(g)

Reactants

the substance(s) to the right of the arrow, this is what is produced from the reactants' reaction with each other and is present at the end of the chemical equation.

Fe(s) + S(s) → FeS(s)

Products

the substance(s) to the left of the arrow that is present at the beginning of a chemical reaction

Subscripts

indication to the number of atoms of the preceding element

2NH3

Coefficients

The coefficient tells us how many molecules of a given formula are present and is shown preceding the elements

A word equation should state the reactants (starting materials), products (ending materials), and direction of the reaction in a form that could be used to write a chemical equation.

Iron and sodium nitrate produce iron (II) nitrate and sodium

Fe(s) + NaNO3 (aq) → Fe(NO3)2 (aq) + Na(s)

Periodic Table

Pure Substance

compound

elements

are classified on

periodic table

according to

atomic number

by

Families

Periodic Properties

Submicroscopic

atomic volume

capacity to capture or lose electrons

ions

An ion is a charged atom or molecule. It is charged because the number of electrons do not equal the number of protons in the atom or molecule.

gains an electron

cation

loses an electron

anion

electric conductivity

Macroscopic

melting point

boiling point

density

metallic or non-metallic character

brightness

types of compounds formed

formed by

Atoms

Properties

Models

Lewis Diagram

uses element symbol, shows valence electrons only, valence electrons=electrons in the outermost energy shell.

Bohr Rutherford Diagram

uses element symbol

shows how many protons and neutrons are in the nucleus

shows all electrons in each energy shell (1st energy shell=can hold 2 electrons, 2nd energy shell=can hold 8 electrons, 3rd energy shell=can hold 8 electrons, 4th energy shell=can hold 18 electrons)

electrons space out on the energy shell, and then pair up

Parts

crust

electrons

valence electrons

stable

atoms are at their most stable when their outermost energy level is either empty of electrons or filled with electrons.

negatively charged particles found in the shell of an atom (outside of the nucleus)

nucleus

protons

positively charged particles found in the nucleus of an atom

neutrons

neutral particles found in the nucleus of an atom

Chemical Calculations

Main topic

Solubility

Bronsted-Lowry Theory

when an acid and base are mixed together, the acid will transfer a proton to the base

HCl+NH3=ClNH4

an acid's strength is measured by its ability to donate protons

a base's strength is measured by its ability to receive protons

unstable

instability of an atom's nucleus may result from an excess of either neutrons or protons

different numbers of neutrons in their nuclei

isotope

-Atoms of an element that have the same atomic number but different atomic masses
-Isotopes have the same number of protons, but different numbers of neutrons
-Most elements in nature are a mixture of two or more isotopes, which is why the atomic mass is represented as a weighted average

atoms share electrons to form a stable outer shell of 8

when electrons are

transferred between two or more atoms

ionic

compound

a compound formed between a metal and a non-metal

the

bond

is formed by a transfer of electrons

an attraction that holds two or more
atoms together

the overall charge of an ionic compound is neutral

elements being held together by
a bond in a fixed ratio

formula ---> name

The full name of the metal goes first

The non-metal goes second, and you change the ending to “ide”

Al2O3

aluminum oxide

Name → Formula: CRISS CROSS METHOD

write down both elements and their corresponding charges, then switch their charges

Al3+2-

Al2O3

ionic

multivalent metals

transition metals

capable of having different charges and forming compounds in different proportions are called multivalent metals

rule: roman numerals represent the charge on the multivalent metal ion. Ex Cu⁺² ---> copper (II), can backwards criss cross to find the charge, include roman numerals in word equation and continue to change the ending of the non-metal to "ide"

polyatomic group

when there are more than 2 elements, the compound is polyatomic, have to use the back of the periodic table to identify names, criss cross using brackets

Name the metal normally,
and then use the name from
the polyatomic chart on the
back of the periodic table.

Crisscross the charge of the metal
(found on the periodic table) with
the charge on the polyatomic
(found on the back of the periodic
table). Use brackets when the
number of the polyatomic > 1.

Chemical Formula--> Name

Chemical Formula--> Name

Name-->Chemical Formula

Name-->Chemical Formula

shared between two or more atoms

how to measure?

electronegativity

measure of an atom’s ability to attract a shared
pair of electrons within a molecular bond

trend

electronegativity generally increases as you move from left to right across a period and decreases as you move down a group

how do you find the electronegativity of an element?

the periodic table of elements reveals unique patterns in the properties of chemical elements.

types of trends

difference in electronegativity (∆EN) can be used to determine

bond polarity

non-polar molecule- ∆EN = 0, electrons shared equally

Cl - Cl, N - CL

polar molecule- 0 < ∆EN ≤ 1.7, shared unequally

O - H

molecular polarity

Evaluating all of the bond polarities and overall
shape of the molecule

how do we find the structure?

VSEPR (Valence Shell Electron Pair Repulsion theory)

allows us to predict the geometry (structure) and molecule
polarity of individual molecules based on the number of
electron pairs that surround the central atom

Subtopic

Electron pairs in a valence shell want to stay as FAR
APART from each other as possible, and this affects the shape
of the entire molecule

Molecules have different physical and chemical
properties based on their bond and molecular
polarity.

intermolecular forces

attraction between neighbouring molecules

weaker than molecular bonds

types

London Dispersion

Dipole-Dipole

Hydrogen Bonding

intramolecular forces

molecular bonds within one compound

types

Ionic

Molecular (polar and non-polar)

Partial charges can be assigned to atoms or regions
of the molecule

A molecule can have polar bonds, but be
non-polar overall depending on the shape

If the central atom has any lone pairs (nonbonding), the molecule is POLAR.

Linear and square planar are exceptions.

ionic compound- ∆EN > 1.7, transferred completely

Na - Cl

covalent bonding

hydrogen atoms sharing electrons

hydrogen atoms sharing electrons

molecular compound

compound formed by two non-metals (2 anions)

H2O (water)

write the names of each element in the same order as the chemical formula, change the ending of the second element to "ide.", add prefixes (di, tri, mono, etc...) to match the subscripts for each element, never add MONO to the first name .

Sulfur hexafluoride = SFl₆

The overall charge of a molecular compound
is not always neutral

sodium transfers its electron to chlorine to fill its valence shell

sodium transfers its electron to chlorine to fill its valence shell

visual representations of bonds

visual representations of bonds

"δ" delta symbol signifies a partial charge

Polar molecules will have a slightly negative pole (with higher
density of electrons) and a slightly positive pole

Higher electronegativity = stronger pull on electrons = slightly
negative end

δ+ = partially positive

δ⁻ = partially negative