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Transcript of Formulas use chemical symbols and numbers for qualitative and quantitative information Symbol =...
![Page 1: Formulas use chemical symbols and numbers for qualitative and quantitative information Symbol = qualitative (element) Example, CO Subscript =](https://reader035.fdocuments.in/reader035/viewer/2022062322/56649ea85503460f94bab765/html5/thumbnails/1.jpg)
CHEMICAL FORMULAS AND
EQUATIONS
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CHEMICAL FORMULAS Formulas use chemical symbols and
numbers for qualitative and quantitative information
Symbol = qualitative (element)Example, CO
Subscript = quantitative (amount) Example, CO2
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TYPES OF FORMULAS There are two types of formulas,
empirical and molecular. The empirical formula represents the
simplest integer ratio in which atoms combine to form a compound.
Ionic compounds do not form molecules, so ionic formulas indicate a ratio of ions. Example, NaCl (1 sodium and 1 chlorine ion)Example, MgCl2 (1 magnesium and 2
chlorine ions) Formulas of ionic substance are
empirical
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TYPES OF FORMULAS Molecular formulas may be a multiple of
the empirical formula. Covalently bonded substances form
molecules. A molecular formulas represents the
actual ratio of atoms in a molecule. Example, glucose is C6H12O6, but that
formula can be reduced to CH2O
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ATOMS, COMPOUNDS, AND IONS Atoms and compound are electrically
neutral. In an atom protons = electrons In a compound the charges balance out. Ions are not neutral and may be either
positive or negative (cations and anions) An ionic charge is indicated by a
superscript. A sodium ion with a charge of 1+ is written
as Na+ (this is known as the oxidation state) Some atoms have more than one oxidation
state
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POLYATOMIC IONS A polyatomic ion is a group of atoms
covalently bonded together possessing a charge.
Parentheses are used to enclose polyatomic ions when there is more than one of the ions in a compound.
A subscript after the parentheses tells how many polyatomic ions are present.
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COEFFICIENTS A coefficient written in front of a formula
tells how many units of the formula are present and it applies to the entire formula
Example, 2H2O The elements present are: hydrogen and oxygen In water there are two hydrogens for every one
oxygen In 2H2O there are actually 4 hydrogen atoms and
2 oxygen atoms
How many of each atom in: 4 Ca(NO3)2
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WHAT IS A HYDRATE A hydrate is formed when water gets
trapped with in the crystal lattice structure of an ionic compound.
These crystals have a definite number of water molecules for each unit of the compound
An anhydrous (opposite of hydrated) compound can be obtained by heating the crystals to drive off water.
In a chemical reactions, the water in the hydrate does not react, but it adds mass to the compound.
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WRITING FORMULAS AND
NAMING COMPOUNDS
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EQUALIZING CHARGES Compound are considered neutral by
having an equal number of positive and negative charges.
The criss-cross method is used to help figure out the correct formula when equalizing charges. Remember to transfer only the number and
not the sign and do not write the number 1
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NAMING COMPOUNDS Compounds are named based on the
types of elements that form them. Ionic compounds are named by one
method. Covalent compounds that contain only
nonmetals are named differently.
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BINARY IONIC COMPOUNDS The names of binary ionic compounds
come directly from the elements in the compound.
The positive particle (the metal) is placed first.
The negatively charged ion will end the formula.
The metal’s name remains the same and the nonmetal gets an –ide ending. Example, NaCl is sodium chlorideExample, CaBr2 is calcium bromide
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IONIC COMPOUNDS WITH POLYATOMIC IONS Naming these kinds of compounds is
simple, just simple use the metal’s name and the polyatomic ions name.
Nothing needs to modified. Example: NaOH is sodium hydroxide
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BINARY COVALENT COMPOUNDS A binary compound that contains two nonmetals
is arranged by electronegativity values. The element with the lower electronegative
value is written first. The name of the compound will end in –ide. These elements can often form more than one
compound, so a prefix is used to tell the reader how many atoms of each element are present. Example, CO is carbon monoxide Example, CO2 is carbon dioxide
If there is only one atom of the first element in the compound a prefix is not needed
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THE STOCK SYSTEM Some metals (transition metals) have
more than one oxidation state. The stock system solves this problem by
simply stating the oxidation number by using Roman numerals after the name of the metal. Example, Iron (II) chloride tells the reader
that the iron has an oxidation number of +2 and the formula would be FeCl2
What would Iron (III) chloride look like?
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CHEMICAL REACTIONSPhysical Change A change in the
appearance of the starting material
Phase changes are physical changes
Ex, melting, freezing, boiling
Chemical Change A change in which
the products are a different material than the reactants
Chemical reactions are chemical changes
Ex, burning, rusting
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CHEMICAL EQUATIONS A chemical equation is used to show
what takes place during a chemical reaction.
The starting substance is called the reactant (located on the left side of the arrow)
The substance produced is called the product (located on the right side of the arrow)
H2 (g) + O2 (g) 2H2O (g)
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ENDOTHERMIC AND EXOTHERMIC Chemical and physical changes involve
the loss or gain of energy. Endothermic – heat is absorbed during
the reaction Exothermic – heat is released during the
reaction
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Type of reaction
Surrounding temperature
Potential Energy of the Reactants
Potential Energy of the Products
Value of Delta H
Endothermic Decreases Less More Positive
Exothermic Increases More Less Negative
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ENDOTHERMIC Process that requires energy in order for
a chemical reaction to occur. Physical change – ice melting Chemical change – food cooking The reactants absorb energy as they
become products. The products have more potential
energy than the reactants.
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EXOTHERMIC Process that release energy when a
chemical reaction occurs. Physical change – water freezing Chemical change – combustion The reactants release energy as they
become products. The products have less potential energy
than the reactants.
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BALANCING CHEMICAL REACTIONS The Law of Conservation of Mass: mass
of the products = the mass of the reactants
There also has to be conservation of atoms
Coefficients in equations tells us how many atoms or molecules are present (Moles)
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TYPES OF REACTIONS Synthesis reactions Decomposition reactions Single replacement reactions Double replacement reactions
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SYNTHESIS REACTIONS When two or more reactants combine to
form a single product
A + B AB
A and B represent either elements or compounds and AB represents a compound
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DECOMPOSITION REACTION The reverse of a synthesis reaction in
that a single compound is broken into tow or more simpler substances
AB A + B
A and B represent either elements or compounds and AB represents a compound
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SINGLE REPLACEMENT REACTIONS A type of reaction where one element replaces
another element in a compound. This type of reaction always involves an
element and a compound.
A + BC B + AC
One can predict whether a reaction will happen or not using the Activity Series
A metal listed on the table will react with the compound of a metal below it.
A nonmetal will replace a less active nonmetal in a compound
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DOUBLE REPLACEMENT REACTION These reactions generally involve two
soluble ionic compounds that react in solution to produce a precipitate, a gas, or a molecular compound
AB + CD AD + CB
There are three ways to determine if a double replacement reaction will occur
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DOUBLE REPLACEMENT REACTION1) The reaction will occur if one of the
products is a solid. If one product is insoluble then the reaction will occur.
2) The reaction will occur if one of the products is a gas.
3) The reaction will occur if one of the products is water.