Unit 6: Nomenclature.

Unit 6: Nomenclature

This chapter will introduce the chemistry needed to understand how antacids work
Section 1: Identifying Ions Section 2: Naming Ionic Compounds Section 3: Naming Covalent Compounds Section 4: Writing Formulas for Ionic & Covalent compounds Section 5: Percent composition, Empirical formulas, Molecular Formulas

Section 1—Identifying Ions
We need to be able to name the chemicals in the antacids!

The Language of Chemistry
Chemistry has a language all of its own Chemistry English Element Symbols Letters Chemical Formulas Words Chemical Equations Sentences Each element symbol starts with a capital letter

ELEMENTS: made of atoms
An atom consists of subatomic particles There are 3 subatomic particles: protons, electrons and neutrons Neutral atoms have the same number of protons and electrons Atoms can form IONS

IONS An atom or group of atoms with a charge.
The number of protons does not equal the number of electrons. WHY? Atoms can gain or lose electrons to acquire stability like a noble gas element.

The Periodic Table of Elements
Metals form cations Nonmetals form anions H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Lr Rf Db Sg Bh Hs Mt Ds Rg Cn ? Fl Lv Metals Metalloids Non-metals

Monatomic Ions (formed from a single atom) Cations
Cations Positive charge or oxidation number Metal atoms that lose electrons Two types of Metals: Representative & Transition 1. Type I Representative (main group) metals (Group A ) The group # for metals in columns 1A, 2A, & 3A is equal to the charge/oxidation number of the cation Naming them: Take the element name and add the word ion

Monatomic Ions of Group A /Type I Metals
Highlight the periodic table column charges seem below skip Group A Group A Group B

Type II Transition Metals (Group B): usually have more than one charge/oxidation number
You should be familiar with the following transition metals with more than one charge. Fe+2 Fe+3 Sn+2 Sn+4 Pb+2 Pb+4 Co+2 Co+3 Cr Cr+3 Mn+2 Mn+3 Cu Cu+2 Naming them: Take the element name and place in parentheses the charge number as a roman numeral and add the word ion

Three Transition Metals that must be memorized
They only have 1 charge Zinc ion (Zn+2) Cadmium ion (Cd+2) Silver ion (Ag+1)

Monatomic Ions of Transition/Type II Metals
Type II (Group B) Transition Metals +

Monatomic Ions (formed from a single atom) Cu+2, F-1
Anions Negative charge or oxidation number Nonmetals that gain electrons Group A (Representative nonmetals) Subtract the group # in columns 4A, 5A, 6A, and 7A from 8 to get the charge. Naming them: Drop the ending of the element and add –ide and then ion

You Try! Try These: Write the formula for each ion and name it.
Calcium Chromium Chlorine Sulfur

SELF CHECK Write the formula for each ion and name it.
Calcium Ca+2 calcium ion Chromium Cr+2 chromium(II) ion Cr+3 chromium (III) ion Chlorine Cl-1 chloride ion Sulfur S-2 sulfide ion

Self Check Try These: Write the formula for each ion and name it.
Aluminum Zinc Iron Phosphorus Al+3 Aluminum Ion Zn+2 Zinc ion Fe+2 Iron (II) ion or Fe+3 Iron (III) ion P-3 Phosphide ion

Section 2—Naming Ionic Compounds
MAKE SURE YOU HAVE YOUR PERIODIC TABLE IN FRONT OF YOU AT ALL TIMES!

Binary Ionic Compounds
Binary Ionic Compound- compound containing 2 elements—one metal and one non-metal The atoms are held together by Ionic Bonds- bond formed by attraction between + ions and – ions Metal Nonmetal + Cation - Anion Ionic Compound

Metals & Non-Metals Ionic Bonds are between metals(LEFT SIDE) & non-metals (RIGHT SIDE) H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Lr Rf Db Sg Bh Hs Mt Ds Rg Cn ? Fl Lv Metals Metalloids Non-metals

How to Identify & Name a Binary Ionic Compound with type I metal
Look for a compound with: 2 elements (“binary”) A Type 1 metal & a non-metal (“ionic”) To name these compounds: Write the name of the type 1 metal (the cation) Write the name of the non-metal (the anion) with the suffix “-ide” The subscripts in the formula do not matter when naming this type

Example #1 NaCl

NaCl Sodium Chloride Cation Anion “Sodium”
“Chlorine” becomes “Chloride” Sodium Chloride

Example #2 CaBr2

CaBr2 Calcium Bromide Cation Anion “Calcium”
“Bromine” becomes “Bromide” Calcium Bromide

Example #3 K2O

“Potassium” Cation K2O Anion “Oxygen” becomes “Oxide” Potassium Oxide

Write the name for the following compounds
Self Check Li2O Sr3P2 MgS BaI2 Example: Write the name for the following compounds

Answers Li2O Sr3P2 MgS BaI2 Lithium oxide Strontium phosphide Magnesium sulfide Barium iodide Example: Write the name for the following compounds

Transition Metals Type II Metals
Transition Metal- group “B” or Type II metal that has the possibility of having more than one cation charge; Common multivalent metals and their charges Cobalt Co Co+3 Copper Cu Cu+2 Iron Fe Fe+3 Manganese Mn+2 Mn+3 Mercury Hg2+2 Hg+2 IMPORTANT: EXCEPTION group B metals, SILVER (+1), CADMIUM (+2), and ZINC (+2) only have 1 charge BEWARE the elements of TIN and LEAD are group A elements, they do have more than one charge Sn(+2 and +4) and Pb(+2 and +4)

How to Identify & Name Ionic Compounds with Type II Transition Metals
Look for: One of the transition metals(group B), excluding Ag, Cd, and Zn To name these compounds: Write the name of the Type II metal element (cation) Write the name of the anion (element name with “-ide”) Determine the charge of the transition metal 1. Determine total negative charge. Multiply subscript by it charge. 2. Total negative charge = total positive charge for all neutral compounds 3. Divide total positive charge by the number of metal atoms 4. Write the charge in roman numerals in parentheses after the Type II metal’s name

Example # 7 CuCl

CuCl Copper Chloride Cation Anion “Copper”
“Chlorine” becomes “Chloride”

CuCl (I) Copper Chloride Cation Anion “Copper”
Chloride has a –1 charge CuCl -1 charge * 1 ion = -1 A –1 charge needs a +1 charge Anion “Chlorine” becomes “Chloride” Therefore, copper must be +1, (I) Copper Chloride (I)

Example # 8 Fe2O3

“Iron” Cation Fe2O3 Iron oxide Anion “oxide”

Fe2O3 Iron oxide (III) Cation Anion “Iron” oxide has a –2 charge
-2 charge * 3 ions = -6 A –6 charge needs a +6 charge and there are 2 iron ions Anion “oxide” Therefore, iron must be +3 (III) Iron oxide (III)

Example # 9 ZnBr2

“Zinc” Cation ZnBr2 Zinc bromide monatomic Anion “bromide”

ZnBr2 Zinc bromide Cation Polyatomic Anion “Zinc”
bromide has a –1 charge ZnBr2 -1 charge * 2 ions = -2 A –2 charge needs a +2 charge and there is 1 zinc ion Polyatomic Anion “bromide” Therefore, zinc must be +2 (not needed) it only has one charge Zinc bromide

Self Check PbCl2 PbCl4 MnO Mn3P2 Example: Write the name for the following compounds

Answers PbCl2 PbCl4 MnO Mn3P2 Lead (II) chloride Lead (IV) chloride Manganese (II) oxide Manganese (II) phosphide Example: Write the name for the following compounds

Ternary Ionic Compounds
Ternary Ionic Compound- a compound containing at least one polyatomic ion Polyatomic Ion- an ion that has more than one atom that together have a single charge - Polyatomic Anion + Cation Ternary Ionic Compound + Polyatomic Cation - Anion

Common Polyatomic Ions
You don’t need to memorize them. Look at your reference sheet. COMMON POLYATOMIC IONS Acetate, CH3COO-1 or C2H3O2-1 Ammonium NH4+1 Bromate, BrO3-1 Bromite, BrO2-1 Carbonate, CO3-2 Carbonite, CO2-2 Chlorate, ClO3-1 Chlorite, ClO2-1 Chromate, CrO4-2 Cyanide, CN-1 Dichromate, Cr2O7-2 Dihydrogen phosphate, H2PO4-1 Hydrogen carbonate or bicarbonate, HCO3-1 Hydrogen phosphate or biphosphate, HPO4-2 Hydrogen sulfate or bisulfate, HSO4-1 Hydroxide, OH-1 Hypochlorite, ClO-1 Iodate, IO3-1 Iodite, IO2-1 Nitrate, NO3-1 Nitrite, NO2-1 Oxalate, C2O4-2 Perchlorate, ClO4-1 Permanganate, MnO4-1 Peroxide, O2-2 Phosphate, PO4-3 Phosphite, PO3-3 Silicate, SiO3-1 Sulfate, SO4-2 Sulfite, SO3-2

Identifying Polyatomic Ions: Hints
The only cation (front-half) polyatomic ion is “NH4+” All other polyatomic ions are anions (back-half) The subscripts within the polyatomic ion are important (it must match exactly with the one on your ion list) If there are parentheses, the polyatomic ion is inside (ignore the number outside)

Practice Identifying Polyatomic Ions
NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3 Example: Underline& name the polyatomic ion in each compound

Practice Identifying Polyatomic Ions
NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3 Nitrate Ammonium Hydroxide Ammonium & phosphate Carbonate Example: Identify and name the polyatomic ion in each compound

How to Identify & Name Ternary Ionic Compounds
Look for: More than 2 capital letters next to one another (not starting with H) Contain at least 1 metal & 1 non-metal To name these compounds: Write the name of the cation (either the metal element name or “Ammonium” for “NH4+”) If the anion is a polyatomic ion, write the given polyatomic ion’s name If the anion is a single non-metal element, write its name with the suffix “-ide”

Example # 4 Ca(NO3)2

“Calcium” Cation Ca(NO3)2 Polyatomic Anion “Nitrate” Calcium Nitrate

Example #5 Na3PO4

“Sodium” Cation Na3PO4 Polyatomic Anion “phosphate” Sodium phosphate

Example # 6 Cu2CO3

Cu2CO3 Copper (II) carbonate Cation Polyatomic Anion “copper I”

Self Check Ca(C2H3O2)2 Li2SO3 Sn(OH)2 (NH4)2S Example: Write the name for the following compounds

Answers Ca(C2H3O2)2 Li2SO3 Sn(OH)2 (NH4)2S Calcium acetate Lithium sulfite Tin (II) hydroxide Ammonium Sulfide Example: Write the name for the following compounds

Worksheet 1 (1-10 Answers) 1. Sodium sulfide 6. Silver chloride
2. Aluminum oxide 7. Boron nitride 8. Barium fluoride 3. Sodium chloride 4. Rubidium iodide 9. Strontium nitride 5. Zinc bromide 10. Magnesium chloride

Worksheet 2 (1-10 Answers) 1. copper(I) fluoride 6.chromium (VI) oxide
2. copper (II) fluoride 7. gold(I) bromide 8. nickel(II) oxide 3. chromium (III) oxide 9. vanadium(III) iodide 4. lead (II) iodide 10. tin(IV) oxide 5. lead (IV) chloride

Worksheet 3 (1-10 Answers) 1. vanadium(V) chlorate Gold(I) nitrate
7. iron(III) phosphite 2. rhenium(VI) sulfate 8. nickel(II) bromate 3. osmium(III) iodate 9. lead(IV) sulfide 10. Manganese (VII) dichromate 4. iridium(IV) phosphate 5. palladium(IV) sulfite

Worksheet 4 (1-10 Answers) 1. ammonium chloride 6. ammonium nitrate
2. hydrogen chlorite 7. strontium phosphate 8. zinc chlorate 3. calcium bromate 4. beryllium sulfate 9. silver iodate 5. ammonium nitride 10. potassium dichromate

Section 3—Naming Covalent Compounds

Binary Covalent (Molecular) Compounds
Binary Molecular Compounds are made from two non-metals that are covalently bonded Covalent bond a bond formed from atoms that share electrons Non metal Non metal Covalent compound

Identifying & Naming Binary Molecular
These compounds have: 2 elements (“binary”) Both non-metals (“covalent”) To name these compounds: Write the name of the first element with the prefix indicating the number of atoms (except don’t use “mono-” if only 1 atom) Write the name of the second element with the prefix indicating the number of atoms (including “mono-”) and the suffix “ide”

PREFIXES USED IN MOLECULAR COMPOUNDS
Covalent Prefixes PREFIXES USED IN MOLECULAR COMPOUNDS mono di- tri- tetra- penta- hexa- hepta- octa- nona- deca-

Example #11 SiF4

SiF4 Silicon tetrafluoride Silicon Fluorine
Don’t use “mono-” on first element Silicon SiF4 Fluorine 4 = “tetra-” “fluoride” Silicon tetrafluoride

Example #10 P2O5

P2O5 Diphosphorus pentoxide Phosphorus Oxygen 2 = “di-” 5 = “penta-”

Self Check SO2 N2Cl4 F4O10 CO Example: Write the name for the following compounds

Answers SO2 N2Cl4 F4O10 CO sulfur dioxide Dinitrogen tetrachloride Tetrafluorine decoxide Carbon monoxide Example: Write the name for the following compounds

Mixed Practice: Determine the type of compound, Ionic (m/nm) or Covalent (nm/nm) & then follow rules Na2O K3PO4 Cu(OH)2 N2S MgCl2 Example: Write the name for the following compounds

Answers Na2O K3PO4 Cu(OH)2 N2S MgCl2 Sodium oxide Potassium phosphate Copper (II) hydroxide Dinitrogen monosulfide Magnesium chloride Example: Write the name for the following compounds

Section 4—Writing Chemical Formulas For Ionic & Covalent Compounds

Reminders Your Reference sheet has a list of:
Common polyatomic ions Use your periodic table is used to determine the charges of common elements when they form ions You must memorize the 10 prefixes for covalent compounds

How to Write Formulas for Binary Ionic Compounds
These compounds: End in “-ide” (except “hydroxide and cyanide”) Do NOT contain covalent prefixes To write these formulas: Write the symbol & charge of the metal, cation) Write the symbol & charge of the non-metal, anion) If total charge is not equal to zero, adjust the # of cations or anions to create a neutral compound. Use subscripts to show how many of each type of ion is there.

Example #1 Sodium chloride

Na+1 Cation Sodium chloride Anion Cl-1 NaCl

NaCl Example #1 Sodium chloride +1 + -1 = 0 Na+1Cl-1 Cation Anion Na+1
The compound is neutral…no subscripts are needed. Cl-1 NaCl

Example #2 Calcium bromide

Example #2 Ca+2 Cation Calcium bromide Anion Br-1

CaBr2 Example #2 Calcium bromide +2 + -1 = +1 Ca+2 Br-1 Cation Anion
Ca+2 Br-1 Br-1 Br-1 = 0 CaBr2 The subscript “2” is used to show that 2 anions are needed.

A Simple Method to Writing Binary Ionic Formulas
The Criss - Cross Method: Write the symbol & charge of the first element (the metal, cation) Write the symbol & charge of the second element (the non-metal, anion) Cross ONLY the charge numbers down diagonally to make subscripts IF they are not equal to each other Simplify subscripts if you can Ca +2 Br-1  Ca1Br2  CaBr2

Write the following chemical formulas
Self Check Cesium chloride Potassium oxide Calcium sulfide Lithium nitride Example: Write the following chemical formulas

Answers Cesium chloride Potassium oxide Calcium sulfide Lithium nitride CsCl K2O CaS Li3N Example: Write the following chemical formulas

Writing Formulas for ionic Compounds with a Transition TYPE II Metal
These compounds: Will have roman numerals To write these formulas: Same as binary ionic or polyatomic ionic. The roman numerals tell the charge of the metal (cation)

Example #5 Iron (III) oxide

Fe+3 Cation Iron (III) oxide Anion O-2

Fe2O3 +3 + -2 = -1 Iron (III) oxide O-2 Fe+3 Fe+3 O2- Cation Anion
Fe+3 O2- O2- Anion = 0 O-2 The subscript “2” and “3” are used to show the numbers of atoms needed. Fe2O3

Example #6 Copper (II) sulfide

Cu+2 Cation Copper (II) sulfide Anion S-2

Cu+2 Cation Cu+2 S2- = 0 Copper (II) sulfide Anion S-2 CuS

Self Check Iron (II) nitride Copper (I) chloride Silver sulfide Tin (II) oxide Example: Write the following chemical formulas

Answers Iron (II) nitride Copper (I) chloride Silver sulfide Tin (II) oxide Fe3N2 CuCl Ag2S SnO Example: Write the following chemical formulas

Writing Formulas for Ternary Ionic Compounds
These compounds: Do not end with “-ide” (except hydroxide & cyanide) Do not use covalent prefixes To write these formulas: Write the symbol & charge of the cation & anion Add additional cations or anions to have a neutral compound Use subscripts to show the number of ions When using subscripts with a polyatomic ion, you must put the polyatomic ion in a parenthesis with the subscript on the outside

Example #1 Sodium carbonate

Na+1 Cation Sodium carbonate Polyatomic Anion CO3-2

Na2CO3 Sodium carbonate +1 + -2 = -1 Na1+ CO32- Cation Polyatomic
Anion Na+ Na+ CO32- = 0 CO3-2 Na2CO3 The subscript “2” is used to show that 2 cations are needed.

Example #2 Magnesium nitrate

Mg+2 Cation Magnesium nitrate Polyatomic Anion NO3-1

Mg(NO3)2 Mg+2 Magnesium nitrate Mg+2NO31- +2 + -1 = 1 NO3-1 Cation
Polyatomic Anion = 0 NO3-1 The subscript “2” is used to show that 2 anions are needed. Mg(NO3)2 Use parenthesis when adding subscripts to polyatomic ions

Self Check Sodium nitrate Cadmium chlorate Potassium sulfite Iron(III) hydroxide Example: Write the following chemical formulas

Answers Sodium nitrate Cadmium chlorate Potassium sulfite Iron(III) hydroxide NaNO3 Cd(ClO3)2 K2SO3 Fe(OH)3 Example: Write the following chemical formulas

Writing Formulas for Binary Covalent Compounds
These compounds: Use covalent prefixes To write these formulas: Write the symbols of the first and second element Use the covalent prefixes (assume the first element is “1” if there’s no prefix) as the subscripts to show number of atoms. Atoms do not form charges when bonding covalently…you DO NOT need to worry about charges with this type! NOR CRISS CROSS METHOD!

Example #1 Dinitrogen Tetroxide

Dinitrogen Tetraoxide
N2O4

Example #2 Silicon dioxide

Silicon dioxide SiO2 “Di-” = 2 Si O
“Mono-” is not written for the first element Si Silicon dioxide O “Di-” = 2 SiO2

CAUTION!!! “di” and “bi” do not mean the same thing! di- bi-
Stands for “2” in covalent compounds Means there’s a hydrogen in the polyatomic anion Carbon dioxide = CO2 Sodium biphosphate = Na2HPO4

Self Check Carbon monoxide Sulfur tetraiodide Trichlorine pentasulfide Example: Write the following chemical formulas

Answers Carbon monoxide Sulfur tetraiodide Trichlorine pentasulfide CO SI4 Cl3S5 Example: Write the following chemical formulas

Self Check: Mixed Practice
Magnesium hydroxide Copper (II) nitrate Iron (III) oxide Nitrogen dioxide Sodium bicarbonate Example: Write the following chemical formulas

Answers Magnesium hydroxide Copper (II) nitrate Iron (III) oxide Nitrogen dioxide Sodium bicarbonate Mg(OH)2 Cu(NO3)2 Fe2O3 NO2 NaHCO3 Example: Write the following chemical formulas

Section 5 Formula Calculations
Percent Composition, Empirical Formulas & Molecular Formulas

Percent Composition by Mass of Air

Percent Composition Defined as the percent by mass of each element in a compound Steps to Finding Percent Composition Add up the mass of each element within the compound to get the mass of the compound. Divide each element’s mass by the mass of the compound. Multiply by 100 % composition= mass of element x 100 mass of compound

Example: Calculate the % composition of each element in calcium carbonate.
CaCO3 Molar mass = g % C = 12.01/ x 100 = % %Ca = 40.08/ x 100 = 40.04% %O = 48.00/ x 100 = 47.96%

Example: What is the % of each element in a compound that contains 29
Example: What is the % of each element in a compound that contains 29.00g Ag and 4.30g S only? Total mass of compound = g % Ag = 29.00/33.30 x 100 = % %S = 4.30/33.30 x 100 = 12.9%

Hydrates A HYDRATE is an ionic compound with water trapped
in its crystal. Examples are: CuSO4 5H2O MgSO4 7 H2O CoCl2 6 H2O Heating a hydrate removes the water and leaves behind just the salt which is called the anhydrate.

Example: What is the % water in the hydrate, CuCl2  2H2O
Molar mass of hydrate = g % water = 36.04/ x 100 = 21.14%

Heating of A Hydrate Animation
Calculating the experimental % composition of water in a hydrate.

Empirical Formula A chemical formula showing the simplest whole number ratio of moles of elements (subscripts) May or may not be the same as the ACTUAL molecular formula Hydrogen Peroxide has an actual formula (molecular formula) of H2O2 but an empirical formula of HO

How to Calculate Empirical Formula
RHYME: Percent to Mass Mass to Mole Divide by Small Multiply till Whole Assume 100 grams of the sample of compound. Switch the percent sign to grams 2. Convert each element’s mass into moles. 3. Divide each element’s mole amount by the smallest mole amount in the entire problem. The answer is the subscript of the element within the compound. 4. OPTIONAL: If mole ratio is not within .1 of a whole number, multiply each amount by the smallest whole number that will produce either a whole number itself or a number within .1 of a whole number.

Example: What is the empirical formula for 40.05% S and 59.95% O?
Switch the percent sign to grams & convert each element’s mass into moles 40.05 g S / 32.07g = mol S 59.95 g O / g = mol O Divide each element’s mole amount by the smallest mole amount in the entire problem. 1.250 mol S = mol O = 2.99 = 3 1.250 mole mol S1O3  SO3

Example: What is the empirical formula for 43.64% P and 56.36% O?
Switch the percent sign to grams & convert each element’s mass into moles 43.64 g P / 30.97g = mol S 56.36 g O / g = mol O Divide each element’s mole amount by the smallest mole amount in the entire problem. 1.409 mol S = mol O = 2.49 ≠ 3 1.409 mole mol If mole ratio is not within .1 of a whole number, multiply each amount by the smallest whole number that will produce either a whole number itself or a number within .1 of a whole number. 1 x 2 = x 2 = = 5 P2O5

Molecular Formula Is the ACTUAL, true formula of the compound.
They are usually multiples of their empirical formula N2O4 is the molecular formula; the empirical formula is NO2 Notice that the molecular formula is 2 times larger than the empirical formula

Molecular Formula

How to Calculate Molecular Formula
1. You need to find the empirical formula and calculate its molar mass. Call this empirical formula mass EFM. 2. Find the mass of the actual formula which will most likely be given to you in grams. Call this molecular formula mass MFM. 3. Divide the MFM by the EFM to get a factor. 4. Multiply the factor by the empirical formula to get the MOLECULAR FORMULA Factor x (Empirical Formula) = Molecular Formula

Example: What is the molecular formula of a compound whose empirical formula is CH4N and the molecular mass is g/mol? 1. Empirical Formula Mass (EFM) = = g 2. Molecular Formula Mass (MFM) = g / = 2 4. 2(CH4N) = C2H8N2

Unit 6: Nomenclature.

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