Unit 1: Matter & Nomenclature

Unit 1: Matter & Nomenclature

This chapter will introduce the chemistry needed to understand how antacids work
Section 1: Types of Matter Section 2: Properties & Changes of Matter Section 3A: Identifying Ions Section 3B: Naming Ionic Compounds Section 3C: Naming Covalent Compounds Section 4: Writing Formulas for Ionic & Covalent compounds

Section 1—Types of Matter

Matter is…. Anything that takes up space (volume) & has mass
Examples: elements, molecules, cells, people, air, water, paper Non Examples: dreams, energy (light, heat), emotions 3 States of Matter: SOLID, LIQUID, GAS

Atoms & Molecules make up

Pure Substances versus Mixtures
Matter is classified as either a pure substance or a mixture Pure Substances Mixtures Contain only 1 type of particle Elements or Compounds Contain 2 or more different types of particles Homogeneous or Heterogeneous Compounds can be separated by chemical means: heat, light, or electricity Can be separated by physical means: filtration, distillation, evaporation

Pure Substances Elements Compound
2 or more different elements chemically bonded together to form molecules. Each is the same fixed ratio of elements. H2O, NaCl, CO2 Simplest kind of matter Every atom is the same Represented by chemical symbols & found on periodic table Cu, Ag, Fe, Br2

Elements Single Atom Element Every atom is the same

Compounds Single Molecule Compound Every molecule is the same

Diatomic Elements Unique situation 2 identical atoms bonded together
Only 7 exist Br2, I2, N2, Cl2, H2, O2, F2 Mnemonic: ____________

Physical combination of more than 1 type of pure substance
Mixtures More than 1 different type of matter Can be separated physically by Distillation Filtration Chromatography Mixture Not a pure substance Physical combination of more than 1 type of pure substance

Mixtures Homogeneous Heterogeneous (aka “solution”)
Mixtures can be classified as homogeneous or heterogeneous Homogeneous (aka “solution”) Heterogeneous It looks the same throughout; substances evenly dispersed Ex. salt water, alloys, clean air Different substances can be seen (chunks, bubbles, floaties, layers) Ex. salad dressing, fog, chocolate chip cookies, soil

Mixture possibilities
Mixtures can be any combination of solids, liquids and gases: Solid-solid: Medicine tablet Solid-gas: Pop Rocks candy Solid-liquid: Ice water Liquid-liquid: lemon water Gas-Liquid: Carbonated water Gas-Gas: Air

Homogeneous Mixtures Kool-Aid: sugar in water Brass: copper in zinc
Air: oxygen gas in nitrogen gas Milk: fat, proteins, sugar in water

Heterogeneous Mixtures
Oil in water Italian Salad Dressing Chicken Noodle Soup Fruit Salad

True Solutions, Colloids & Suspensions
Homogeneous Heterogeneous Heterogeneous True Solution Colloid Suspension SMALL particles don’t settle out and are too small to scatter light Ex: salt water, air, brass INTERMEDIATE particles don’t settle out but are large enough to scatter light: Ex: fog, foam, jello, paint LARGE particles that settle out over time Ex: oral medicines, italian dressing, paint Dissolved Particle Size Increases

True Solutions

vinegar and oil salad dressing
Suspensions vinegar and oil salad dressing

Particles Scattering Light
If the dissolved particles are large enough to scatter light, we say it exhibits the “Tyndall Effect” Solution Light passes through unchanged Colloids exhibit the Tyndall Effect Light is scattered by larger solute particles

Classification of Matter

Let’s Practice: Not in Notes
Example: Determine if each is element, compound, homogeneous or heterogeneous mixtures Pizza Pure water (H2O) Tap water Mercury (Hg) Sports Drink

Let’s Practice Example:
Determine if each is element, compound, homogeneous or heterogeneous mixtures Pizza Heterogeneous mix Pure water (H2O) Compound Tap Water Homogeneous mix Mercury(Hg) Element Sports drink Homogenous mix

Carbon Tetrachloride (CCl4) Orange juice(with pulp)
You Try! In Notes Example: Determine if each is element, compound, homogeneous or heterogeneous mixtures Gold Nugget (Au) Carbon Tetrachloride (CCl4) Orange juice(with pulp) Coffee Carbon dioxide(CO2)

Carbon Tetrachloride (CCl4) Orange juice(with pulp)
You Try! Example: Determine if each is element, compound, homogeneous or heterogeneous mixtures Gold Nugget (Au) Element Carbon Tetrachloride (CCl4) Compound Orange juice(with pulp) Heterogeneous mix coffee Homogeneous mix Carbon dioxide(CO2) compound

Section 2—Properties & Changes
We need to be able to name the chemicals in the antacids!

Physical versus Chemical Properties
Physical Property Chemical Property Characteristic that can be determined or measured without changing the substance’s identity Characteristic that can only be determined or measured as the substance changes into different substances

Examples of Physical Properties
COLOR ODOR TEXTURE BOILING POINT DENSITY SOLUBILITY VOLUME MASS HARDNESS MALLEABILITY /BRITTLENESS

Physical Properties of Water

Examples of Chemical Properties
BURNING/COMBUSTING RUSTING ROTTING FLAMMABILITY REACTIVITY NEUTRALIZATION DECOMPOSING

Intensive and Extensive Properties
Intensive Property Extensive Property Size of the sample DOES NOT matter— a big piece & a small piece are the same with respect to the property Size of the sample DOES matter —a big piece & a small piece would be different with respect to the property

Intensive Extensive Melting point/boiling point Mass Volume Density
Color/Smell Conductivity Hardness Extensive Mass Volume Energy Length Shape

Reactivity with oxygen
SELF CHECK-Determine if it’s a physical or chemical property. If physical, is it an intensive or extensive property? Flammability Boiling point Solubility Malleability Reactivity with oxygen

Flammability Boiling point Solubility Malleability Reactivity with oxygen Chemical Physical, Intensive

Physical VS Chemical Changes
Physical Change: the chemical structure of the substances is not changed. H2O(l) H2O(g)

Physical VS Chemical Changes
Chemical Change: the chemical structures of the substances are changed. H2O(l) H2(g) + O2(g) RECALL: Another name for a chemical change is called a CHEMICAL REACTION.

Physical & Chemical Changes
Physical changes do not produce new substances breaking, dissolving, distilling, cutting, Changes in state (boiling, condensing, melting & freezing) Chemical changes do produce new substances rusting, burning, metabolizing food, oxidation or reduction, reacting with oxygen, etc.

Physical & Chemical Changes
Also…if a change can be un-done by a physical change, then the original change was physical as well. If salt is dissolved in water, it seems to disappear… many people think this is a chemical change. But if the water is evaporated (a physical change), the salt is left in the container. Since the original change was un-done with a physical change, then the original change (the dissolving) was a physical change as well.

Possible Signs of a Chemical Change taking place (GOPEC)
Gas production (bubbling) Odor change Formation of a precipitate (an insoluble substance formed from two soluble substances) Energy change (getting hot or cold) Color change

They’re “Possible” signs
Sometimes these “signs” accompany physical changes as well! Gas production (bubbling). Bubbles are formed during boiling (a physical change) Energy change (getting hot or cold). Energy changes accompany changes in state (physical changes) Color change. Color change can occur due to dissolving a substance (a physical change) However, some of these signs also accompany physical changes, so you must take into account many observations to determine if the change was in fact chemical.

Confusing changes People often use the following terms incorrectly.
Definition Type of Change Melting Changes a solid into a liquid Physical Burning Reacting with oxygen to produce CO2 and H2O Chemical Dissolving Adding one substance to another to form a homogeneous mixture Physical Drying Heating a sample to evaporate the water Physical

Section 3A—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 3B—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 3C—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 pentaoxide 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 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!

Dinitrogen Tetraoxide
Example #1 Dinitrogen Tetraoxide

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

Unit 1: Matter & Nomenclature

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