CP Chemistry - Mr. Potoczak's Science Class



Nomenclature Study Guide

Part 1: Types of Compounds

❑ There are 2 main types of chemical compounds. They are:

1. Molecular - made from 2 different atoms that are both ________________________________.

2. Ionic - made from 2 different ions, one is a _______________ and the other is a ___________________.

An ionic compound can also contain a ___________________________________________.

➢ An atom is ____________________. An ion has a __________________ or __________________ charge.

➢ A polyatomic ion is an ion made from ___________________________________ atoms.

➢ A diatomic molecule is an element that exists as _______ of its atoms combined. (Br2 I2 N2 Cl2 H2 O2 F2)

❑ Examples: Atom Mg Ion Mg+2 Polyatomic ion NO3(1 Diatomic Molecule O2

❑ In order to determine whether a compound is ionic or molecular, you need to determine if the elements in the compound are metals or nonmetals. To do this, look at the element’s position in the Periodic Table.

➢ Metals are to the _______________ of the stair-step line and nonmetals are to the ___________________.

← Are the following compounds ionic or molecular? MgS Ca(OH)2 CO2 NI3 Al2(CO3)3

Part 2: Interpreting Chemical Formulas

➢ A number called a superscript indicates the ________________________ of an ion. For example: Mg+2

➢ If only a + or ( is shown with no number, then the value of the charge is __________.

➢ A number called a

subscript indicates the ____________________ of atoms or ions in a compound. For example: O2

➢ If no subscript is present, then there is only _________ atom or ion.

← How many atoms/ions of each element are in each of the following compounds?

CO2: C_____ O_____ Ca(OH)2: Ca_____ O_____ H_____ Al2(CO3)3: Al_____ C_____ O_____

Part 3: Rules for Naming Ionic Compounds

❑ CO2 is carbon dioxide and CaCl2 is calcium chloride. Why isn’t it calcium dichloride?

➢ The rules for naming ionic compounds are basically the same as for naming molecular compounds

except don’t use ______________________________.

((( If the compound contains a negatively charged polyatomic ion, do not change the ending to “ide”.

Just say the name of the polyatomic ion as it is listed on your “Common Ions” handout.

← What are the names of the following compounds?

K2SO3 ___________________________________ BaO _______________________________________

Ca3N2 ___________________________________ Mg(NO3)2 __________________________________

❑ On your “Common Ions” handout, notice that some ions can have more than one charge. For example, iron can have a +2 or +3 charge. In the compound FeCl3, which iron ion is it and how do you name the compound?

➢ An ionic compound is made from 1 ____________________ ion and 1 _____________________ ion.

The _____________________ ion is written first and the total charge on the compound must be _________.

➢ In FeCl3, the Cl ion’s charge is _______. Since there are three Cl ions, the total amount of negative charge

is _______. Since there is only one iron ion, its charge must be _______ in order to make the charge on the

compound 0. The name of this compound is iron _________ chloride.

← What are the names of the following compounds?

Co2(CO3)3 ________________________________ Fe3P2 ______________________________________

Cu2S ___________________________________ Mn(ClO)3 __________________________________

❑ Common mistake: Cu2S is copper(I) sulfide not copper(II) sulfide.

(((The Roman numeral refers to the ________________________ not the ________________________.

Part 4: Rules for Writing Formulas for Ionic Compounds

❑ How do you know the formula for magnesium chloride is MgCl2 and not MgCl, Mg2Cl or something else?

❑ The rules for writing formulas for ionic compounds are as follows:

1. Write the _____________________ for each ion with its charge.

2. Determine how many of each ion are needed to make the total charge on the compound ______________.

3. Indicate the number of each ion(determined in step #2) with a _________________________.

4. When adding a subscript to a polyatomic ion, put the polyatomic ion in ____________________________

with the new subscript outside.

***Do not change any subscripts already present in the formula of the polyatomic ion.***

5. Erase the ____________________ for the final formula.

← What are the formulas for the following compounds?

magnesium chloride ________________________ copper(II) phosphate _____________________

nickel(III) chlorite__________________________ potassium nitride________________________

lead(IV) acetate ____________________________ sodium sulfate __________________________

Part 5: Rules for Naming Molecular Compounds (text pages 248-251)

❑ You need to learn the prefixes for the following numbers:

Number |Prefix | |Number |Prefix | |Number |Prefix | |Number |Prefix | |1

| | |3 | | |5 | | |7 | | |2

| | |4 | | |6 | | |8 | | |

❑ The rules for naming molecular compounds are as follows:

1. Name the elements in the order they appear.

2. Change the ending of the second element to _____________.

(Drop last 2 letters in C, S, Si, As. Drop last 3 letters in F, Cl, Br, I, Se. Drop last 4 letters in N, O, P)

3. To indicate the number of atoms of each element, add a _________________________ to the beginning

of each element’s name

4. The prefix _________________________ can be dropped if it is on the first element.

← What are the names of the following compounds?

N2O _____________________________________ CS2 ____________________________________

P5Cl4 ____________________________________ S8N7 ____________________________________

← What are the names of the following compounds?

NH4Cl _____________________________________ Al(HSO4)3 _________________________________

CCl4_______________________________________ CoBr3 _____________________________________

Li2S ______________________________________ Cl2O7_____________________________________

NO3_______________________________________ Cr(NO2)2 __________________________________

Fe2(C2O4)3_________________________________ Na3N _____________________________________

Part 6: Rules for Writing Formulas for Molecular Compounds

(text page 250)

❑ The rules for writing formulas for molecular compounds are as follows:

1. Represent each element with its _________________________.

2. To indicate the number of atoms of each element, add a _______________________ after each symbol.

← What are the formulas for the following compounds?

nitrogen trioxide _________________________ tricarbon tetrachloride _____________________

pentasulfur hexafluoride ___________________ dinitrogen heptabromide ___________________

← What are the formulas for the following compounds?

nickel(II) chlorite ________________________ sodium phosphide _____________________________

dinitrogen tetroxide ______________________ manganese(III) chlorate _________________________

potassium nitrate ________________________ tin(IV) oxide _________________________________

aluminum chromate ______________________ tetraphosphorus hexoxide _______________________

sodium hypochlorite ______________________ dinitrogen heptabromide ________________________

pentasulfur octaoxide______________________ iron(III) oxalate _______________________________

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