Periodic table

Group 1A info

The alkeli metals, +1 charge, they lose electrons to be neutral. They are highly reactive and have a low melting point

Group 2A information

The earth alkali metals, +2 charge, lose 2 electrons to be neutral. Shiny metals that are somewhat reactive

Group 3A info

Composed of 1 metaloid (boron) and 5 post transition metals, have a 3+ charge and require the loss of 3 electrons to be electrivly neutral. The boron family

Group 4A information

1 non metal, 2 metaloids, and 3 metals. Either have a +4 or a -4 charge, +2 and +4 are more common, but -4 is rare.

Group 5A info

2 of each kind. Have a negetive 3 charge and lose 3 electrons to be neutrally charged.

Group 6A info

3 non-metals, 2 metalloids, and 1 metal. All -2 charge, need to lose 2 electrons to become neutral.

Group 7A info

The halogens, all -1 charge and need to lose 1 electron to become neutral. Highly reactive nonmetals.

Group 8A

The Noble gases. All have neutral charge and every other element is trying to get a neutral charge like the noble gases. Colorless and odorless that are highley stable

Transition metals

Distinctive physical strength. Largly random charges and properites.

Element Cs

Censium

Element: Cr

Chromium

Element: Ni

Nickle

Element: Ag

Silver

Element Hg

Mercury

Element:Sn

Tin

Ammonium ion

NH4+

Hydroxide ion

OH –

Cyanide ion

CN –

Acetate Ion

CH3COO – or C2H3O2 –

Nitrite/Nitrate

NO2– / NO3 –

Sulfite/Sulfate

SO3 2- / SO42-

Phosphate

PO4 3-

Carbonate

CO3 2-

Hydrogen sulfite

HSO3 –

Hydrogen sulfate

HSO4 –

Hydrogen carbonate

HCO3 –

Perchlorate

ClO4 –

Chlorate

ClO3 –

Chlorite

ClO2 –

Hypochlorite*

ClO –

Chromate

CrO4 2-

Dichromate

Cr2O7 2-

Permanganate

MnO4 –

Bromate

BrO3-

Bromite

BrO2-

How to name molecular compounds?

Identify the element, and add the latin prefix to the beginning indicating the amount

How to name monoatomic cations?

Identify the cation and add the word ion

ex. Na+ is sodium ion

How to name elements that can form two different charges?

Indicate the charge with roman numeral in parenthesis

ex. Fe2+ Iron (II) and Fe3+ iron (III)

When do you add the suffix -ide?

When naming a monoatomic anion, or a negatively charged ion normally in groups 5-7

When to add the suffix -ate?

When naming an element that can form only one Oxoanion OR element that can form two but is the larger number

One - CO3 -2 is carbonate atom. Two but larger - NO3 - is nitrate ion

When to use the suffix -ite?

When naming an element with two types of oxoanions with the smaller number of oxygen atoms.

ex. Nitrite ion, NO2-

How to name anions that contain hydrogen?

All names will begin with hydrogen, dihydrogen, tetrahydrogen and so on

ex. HSO3- is Hydrogen Sulfite Ion

How to name ionic compounds?

Name the cation first then the anion, use the anion rules

ex. Calcium chloride is CaCl2

When going from formula to name.

Consider the element at hand, weather it is an anion or cation, then applies the rules of naming elements to that.

When going from name to formula

Identify the charge of each of the elements, and balence it out to find the formula

Molecular compound prefixes

mono = 1 di = 2 tri = 3 tetra = 4 hexa = 6 hepta = 7 octa = 8 nona = 9 penta = 5 deca = 10

Empirical Formula

the relative numbers of atoms of each element present in it. For example, the empirical formula of glucose, which is , shows that carbon, hydrogen, and oxygen atoms are present in the ratio 1:2:1

Molecular formula

the actual numbers of atoms of each element in a molecule. The molecular formula for glucose, which is , shows that each glucose molecule consists of 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms (1).

How to find the empirical formula of a compound

First once you have the mass percentage you can multiply each by the total mass, to find the mass of each of the elements. Then you can multiply that mass by the molar mass of the element. This will help you find the relative number of moles of the element within the compound. Finally you compare the number of moles in a ratio to find the empirical formula.

How to find the molecular formula of a compound?

The first step is to multiply the amount of atoms per element given by the empirical formula by the molar mass of each of those elements. Then you add all of them up to find the total mass of the empirical formula. Then you divide the total mass of the compound by the total mass of the empirical formula. That will give you a number, and that number you multiply by the number of atoms in the empirical formula to finally find the molecular formula.

Mole

numbers of atoms, ions, and molecules in terms of a unit called a mole

Avogadros constant

6.0221 × 10 23 mol -1

Used to convert between chemical amount and the number of atoms, ions, or molecules in that amount

How to find the number of objects in chemistry?

Amount in moles X number of objects per mol

Molar mass

The mass per mole of particles: “The molar mass of an element is the mass per mole of its atoms

How to find mass of sample in chemistry?

Amount in moles X mass per mole OR m = nM

How are molar masses determined?

using mass spectrometry to measure the masses of the individual isotopes and their abundances

How to find the average atom mass?

Calculating the weighted average, the sum of the produce of the mass of each isotope multiplies by its functional abundance OR Theata Isotopes FisotopeMisotope

Atomic Weight

element is the numerical value of its molar mass.

Molecular weight

ionic compound is the numerical value of its molar mass.

Physical property

substance is a characteristic that can be observed or measured without changing the identity of the substance.

Common SI prefixes

Kilo 10 3

Centi 10 -2

Milli 10 -3

Micro 10 -6

nano 10 -9

Systematic vs random error

A systematic error is an error that is present in every one of a series of repeated measurements. A random error is an error that varies in both sign and magnitude and can average to zero over a series of observations.

Coulomb potential energy

particle of charge at a distance r from another particle of charge is proportional to the two charges and inversely proportional to the distance between them:

Allotrope

a different structural form of the same chemical element in the same physical state

Isotopes

variants of a chemical element that have the same number of protons but a different number of neutrons in their nuclei

  Ion

an atom or molecule that carries a net positive or negative electrical charge

Ionic compound

a chemical substance made of oppositely charged ions held together by strong electrostatic forces called ionic bonds

Oxoanion

oxygen combined with another element

Monatomic

consisting of a single atom rather than molecules bound together by chemical bonds

Stoichiometric coefficient

the numbers written directly in front of chemical formulas in a balanced equation to show the proportion of reactants and products involved

Soluable

Able to disolve in water and denoted by (aq) at the end of a compound

Electrolyte

Molecule that conducts electricity through the unequal distribution of water atoms

Strong vs weak electrolytes

A strong electrolyte completely breaks apart (100% ionizes) into ions in water, while a weak electrolyte

Nonelectrolytes

a substance that dissolves in water as intact neutral molecules rather than ions, denoted by (s)

Mobile charge carriers

any free particle or quasiparticle that can move through a material and transport an electric charge to form an electric current

Precipitates

a solid substance that separates from a liquid solution, usually during a chemical reaction or due to a change in temperature, pH, or concentration

-          Skeletal equation

an unbalanced chemical equation that uses chemical formulas and physical state symbols to show the reactants and products of a reaction without indicating their relative stoichiometric amounts

Complete vs net ionic equation

Complete ionic equations show all the ions within the equation, net ionic equations remove the spectator ions from the complete ionic equations

  Spectator ions

an ion that exists in the same form on both the reactant and product

Procedure for finding net ionic equation from reactants

o   1: Identify the compounds of the reactants

o   2: Split the compounds into ions

o   3: Connect negatively and positively charged ions

o   4: Balance the equation

o   5: identify and remove the spectator ions

Mole ratio

the proportional relationship between the number of moles of any two substances (reactants or products) in a balanced chemical equation

Dependent on the coefficient of the molcules

How to make mass to mass prediction

o   Identify the mole ratio with reactants and products

o   Convert grams to moles of element

o   Covert moles of element to moles of compound

o   Multiply the moles by the molar mass

o   Find the grams

-          Stoichiometric point

the theoretical stage in a chemical reaction where reactants have been mixed in exact stoichiometric proportions according to a balanced chemical equation

-   Theoritical vs actual yield

-          Theoritical yields the amount of product you expect based on the balanced equation

o   Actual yiels is the amount of the pure substance

Percentage yield

o   Percentage yield equals actual yield/theoretical yield x 100

How to find the percentage yield

o   Identify the balanced equation

o   Find the atomic mass to convert grams to moles

o   Find mole ratio

o   Convert moles to grams then kg to find actual yield