2.03 Naming/Writing Formulas. Naming and Writing Formulas Formulas Different methods of naming and writing are used depending on the type of bond in the.

Slides:



Advertisements
Similar presentations
Mullis1 Relationship between mass, moles and molecules in a compound Mass (g) Amount (moles) # molecules or Formula units X molar mass (__g__ mole) X
Advertisements

Naming… In case you don’t get it yet. BONDS:  Metal + nonmetal = ionic bond  Metal + metal = metallic bond  Nonmetal + nonmetal = covalent bond.
Chemical Formulas and Compounds. Common Monatomic Ions Chapter 7 Section 1 Chemical Names and Formulas.
Naming Chemical Compounds 1. Ions: Naming and Formulas Cations (positive charge) Single ion formation – Metals in groups 1,2,13 – Element Name + ion –
Naming Ions.
Chapter 7 – Chemical Formulas and Chemical Compounds
Empirical Formulas Empirical – relying on or derived from observation or experiment.
Calculating Empirical and Molecular Formulas
Percentage Composition and Empirical Formula
Section 5: Empirical and Molecular Formulas
Chapter 31 Molecules, Ions, and Their Compounds Chapter 3.
WRITING AND NAMING CHEMICAL FORMULAS. STANDARDS Predict chemical formulas based on the number of valence electrons and oxidation numbers Name and write.
Naming Ionic Compounds and Covalent Molecules
Naming Chemical Compounds Ionic and Covalent Molecules.
Chemical Formulas and Compounds Determining Chemical Formulas.
Empirical and Molecular Formulas
Chapter 7 REALLY Important!!!. 7.1 – Ionic Compounds: Ions for s and p block elements:
Chemical Formulas and equations
Binary Compounds with Multiple Charge Cations
Chapter 9: Chemical Names and Formulae.  Monatomic ions: ionic compounds contain a positive (metal) ion and a negative nonmetal ion in a proportion such.
Chemical Formulas Chemistry 1. Oxidation Numbers  “oxidation states”  The number of electrons that must be added to or removed from an atom in a combined.
Writing Formulas and Naming Compounds. Oxidation Numbers Tells us how many electrons an has gained, lost, or shared to become stable Determined by the.
22.3 Notes Continued. Step By Step – Naming Compounds 1. Write the name of the positive ion 2. Check to see if the positive ion is capable of forming.
Chapter 7 REALLY Important!!!. 7.1 – Ionic Compounds: Ions for s and p block elements:
Naming Chemical Compounds
Chemical Formulas and Chemical Compounds
Chapter #7 Chemical Formulas and Chemical Compounds NearingZero.net.
Formulas and Nomenclature. Charge of Ions called OXIDATION NUMBER Related to the number of electrons that are lost or gained when an atom becomes an ion.
Naming Compounds and Formulas. Naming Ionic Compounds When naming ionic compounds, the cation’s name always comes before the name of the anion – Sodium.
Chapter 19 – Molecules and Compounds Bonding and Molecules Atoms react /combine with other atoms to form molecules. Chemical bonds hold them together.
A. While the _________ formula represents the smallest whole number ratio of elements in a compound, the ___________ formula is the actual formula of.
Determining Chemical Formulas
Chapter 7: Chemical Formulas and Chemical Compounds
Chapter 7 Objectives Explain the significance of a chemical formula. Determine the formula of an ionic compound formed between two given ions. Name an.
Empirical Formula vs. Molecular Formula Empirical formula: the formula for a compound with the smallest whole-number mole ratio of the elements Molecular.
1 Nomenclature Chapter Naming Compounds Many compounds have common names: Ex:H 2 O = water NH 3 = ammonia CH 4 = methane There must be system.
Chapter 7 Chemical Formulas and Chemical Compounds Preview Image Bank Common Monatomic Ions Writing the Formula of an Ionic Compound Polyatomic Ions Naming.
3.4 Empirical and Molecular Formulas. Empirical and Molecular Formulas How do we find a chemical formula for and unknown substance? Identify elements.
Naming Compounds & Writing Formulas
How Do We Make Compounds?
Chemical Formulas & Chemical Compounds Chapter 7.
Friday, April 26 th : “A” Day Monday, April 29 th : “B” Day Agenda  Begin 7.3: “Formulas & Percentage Composition”  In-Class Assignment: Practice.
Learning Objectives Name different types of compounds using IUPAC nomenclature rules – Ionic compounds Containing main group or transition metals – Covalent.
Stoichiometry Chapter 3 Chemical Formulas and Equations.
Chapter 3 Molecules & Compounds. 3.1 Molecules, Compounds and Formulas  Empirical Formulas  Definition: the simplest whole number ratio for the formula.
Chemical Formulas Mrs. Lee Chemical Formulas Mrs. Lee.
CH 7 Chem Formulas and Chem Compounds 7.1 Chemical Names and Formulas Formulas tell the kinds and numbers of atoms Molecular compounds: chemical formula.
Chapter 9: Chemical Formulas and Chemical Compounds.
% Composition, Empirical and Molecular Formulas notes.
Language of Chemistry Unit 4. Ions If a neutral atom loses electrons, then the atom becomes a positively charged particle. If a neutral atom loses electrons,
CHAPTER SEVEN – CHEMICAL FORMULAS SOUTH LAKE HIGH SCHOOL SCIENCE DEPARTMENT MS. SANDERS Chemistry.
Chapter 7 Chemical Formulas & Naming(Nomenclature)
Ionic and covalent compound nomenclature. Naming ionic compounds General rule: 1.State the cation’s element name 2.State the anion’s element name but.
Warm Up  How far was a table moved if 48 N was used to generated 160 J of work?  How many neutrons are in Fe-59?  What is the mass number for an element.
Chemical Formulas and Chemical Compounds Chapter 7.
6.02 Bonding/Nomenclature. Forming Compounds Compounds are formed when two or more elements combine. Compounds are formed when two or more elements combine.
Chapter 7 Objectives Explain the significance of a chemical formula.
Using symbols to write formulas Chapter 7
Ch. 7.4 Determining Chemical Formulas
Empirical Formulas.
7.4 Determining Chemical Formulas
Chemical Formulas and Chemical Compounds
The Structure of matter
Molecular formulas.
Chemical Names and Formulas
Determining Empirical and Molecular Formulas
Section 3: Naming Compounds and Writing Formulas
Chemical Formulas & Mass
Oxidation numbers The number at the top of each column is the most common oxidation number of elements in that group. Copyright © McGraw-Hill Education.
Presentation transcript:

2.03 Naming/Writing Formulas

Naming and Writing Formulas Formulas Different methods of naming and writing are used depending on the type of bond in the compound. Different methods of naming and writing are used depending on the type of bond in the compound. Ionically bonded compounds are named and written using the Stock method. Ionically bonded compounds are named and written using the Stock method. Covalently bonded compounds are named and written using the Greek prefix method. Covalently bonded compounds are named and written using the Greek prefix method.

Stock System Naming Write the full name of the cation first. Write the full name of the cation first. Write the root of the anion followed by an –ide ending. Write the root of the anion followed by an –ide ending. If a transition element is used, a charge must be assigned and written in parenthesis as a roman numeral. If a transition element is used, a charge must be assigned and written in parenthesis as a roman numeral. The charge is determined by finding out what is need to neutralize the compound or create its overall charge. The charge is determined by finding out what is need to neutralize the compound or create its overall charge.

Stock System Writing Write the symbol of the cation, followed by anion Write the symbol of the cation, followed by anion Find their oxidation charges on the periodic table and cross the absolute values of each to get the subscripts. Find their oxidation charges on the periodic table and cross the absolute values of each to get the subscripts.

Greek System Naming Write the full name of the least electronegative (bottom left) element first. Write the full name of the least electronegative (bottom left) element first. Write the root of the most electronegative element (top right) second, followed by an –ide ending. Write the root of the most electronegative element (top right) second, followed by an –ide ending. Write a prefix for each element name based on the subscript number. Write a prefix for each element name based on the subscript number. If the prefix for the first element is mono, it does not have to be included in the name. If the prefix for the first element is mono, it does not have to be included in the name.

Greek System Writing Write the symbol for the least electronegative element first followed by the most. Write the symbol for the least electronegative element first followed by the most. Write in subscripts by looking at prefixes for each element. Write in subscripts by looking at prefixes for each element.

Tertiary Compounds Compounds that consist of only two elements are called binary. Compounds that consist of only two elements are called binary. Compounds containing three or more elements are called tertiary. Compounds containing three or more elements are called tertiary. Tertiary compounds can only be formed when a metal bonds with a polyatomic ion. Tertiary compounds can only be formed when a metal bonds with a polyatomic ion. A polyatomic ion is two or more nonmetals that are already bonded covalently to one another. A polyatomic ion is two or more nonmetals that are already bonded covalently to one another. The polyatomic ion has an overall charge therefore allowing it to bond to a metal to form the tertiary compound. The polyatomic ion has an overall charge therefore allowing it to bond to a metal to form the tertiary compound.

Polyatomic ions These are some common polyatomic ions and their charges. They need to be memorized. These are some common polyatomic ions and their charges. They need to be memorized. NitrateNO 3 1- NitrateNO 3 1- AcetateCH 3 COO 1- SulfateSO 4 2- CarbonateCO 3 2- HydroxideOH 1- AmmoniumNH 4 1-

Naming/Writing with Polyatomic Endings of polyatomic ions cannot be changed when naming. Endings of polyatomic ions cannot be changed when naming. When determining subscripts in formulas, the charge on the overall polyatomic ion is what is used when crossing. When determining subscripts in formulas, the charge on the overall polyatomic ion is what is used when crossing. If more than one polyatomic ion is used, parenthesis must be added around it before any subscripts can be added. If more than one polyatomic ion is used, parenthesis must be added around it before any subscripts can be added. All other rules remain. All other rules remain.

Mole Relationships in Compounds In a formula, the subscripts represent the amount of moles of that element in the substance. In a formula, the subscripts represent the amount of moles of that element in the substance. H 2 O contains two moles of hydrogen and one mole of oxygen. H 2 O contains two moles of hydrogen and one mole of oxygen. Subscripts must be multiplied by coefficients to get correct mole counts. Subscripts must be multiplied by coefficients to get correct mole counts. 2H 2 O contains two moles of water, four moles of hydrogen and two moles of oxygen. 2H 2 O contains two moles of water, four moles of hydrogen and two moles of oxygen.

Percent Composition Percent composition is the percentage by mass of a particular element in a compound. Percent composition is the percentage by mass of a particular element in a compound. Percent composition Percent composition To find percent composition, the total mass of the element within a compound must be known. To find percent composition, the total mass of the element within a compound must be known. This is done by multiplying the atomic mass of the element by its total number of moles. This is done by multiplying the atomic mass of the element by its total number of moles. By dividing this total mass of the element by the formula mass of the compound, you are able to get the percentage of that element within the total compound. By dividing this total mass of the element by the formula mass of the compound, you are able to get the percentage of that element within the total compound.

Empirical Formulas Empirical formula is the formula showing the smallest whole-number mole ratio of the atoms in the compound. Empirical formula is the formula showing the smallest whole-number mole ratio of the atoms in the compound. H 4 O 2 could be reduced to an empirical formula of H 2 O. H 4 O 2 could be reduced to an empirical formula of H 2 O.

Writing Empirical Formulas To write an empirical formula, the smallest whole number ratio of atoms must be found. To write an empirical formula, the smallest whole number ratio of atoms must be found. This is done by converting the mass of all elements in the compound to moles and then dividing by the smallest mole. This is done by converting the mass of all elements in the compound to moles and then dividing by the smallest mole.

Molecular Formulas Unlike empirical formula which is the smallest whole number ratio of moles of atoms, the molecular formula is the actual ratio. Unlike empirical formula which is the smallest whole number ratio of moles of atoms, the molecular formula is the actual ratio. H 2 O could have the molecular formula H 4 O 2 or even H 6 O 3. H 2 O could have the molecular formula H 4 O 2 or even H 6 O 3.

Writing Molecular Formulas The empirical formula must be multiplied by an x factor to go from the smallest ratio to the actual ratio. The empirical formula must be multiplied by an x factor to go from the smallest ratio to the actual ratio. That x factor is found by dividing the given experimental formula mass by the calculated empirical formula mass. That x factor is found by dividing the given experimental formula mass by the calculated empirical formula mass. Formula mass is found by adding the mass of all elements together. Formula mass is found by adding the mass of all elements together.