Chemistry Essentials Unit 4 · 2020-01-27 · Section 1: Naming Binary Compounds Three types of binary compounds Types I & II –Ionic Contain ions –a cation and an anion Contain

Qualitative Chemistry

Unit 4

Nomenclature

Unit Warm Up1. What is the chemical name for salt? What is the

chemical formula for salt?

2. What is a compound?

3. What are the two types of compounds?

4. How can you tell the difference between them?

5. Using your PT, predict the charge of the

following atoms when they are part of an ionic

compound: Na, K, Ca, O, F, Cl.

Introduction

Nomenclature

Writing formulas for compounds from names

and writing names for compounds from

formulas

Rules set by IUPAC(International Union of

Pure and Applied Chemistry)

We will concern ourselves with any

compound that is not considered organic

(long chains of carbon atoms)

Based on the type of compound

Binary – only two elements in compound

NaCl, CO2

Nonbinary (Complex) – three or more

elements in compound

H2SO4, (NH4)3PO4

Section 1: Naming Binary Compounds

Three types of binary compounds

Types I & II – Ionic

Contain ions – a cation and an anion

Contain a metal and a nonmetal

Type I – cation has only 1 possible charge

Columns 1, 2, 3, and metals in 13 on PT

plus Zn, Ag, Cd, Ta, Zr, and Hf.

Type II – cation has more than 1 possible charge

All other Transition Metals that are not

man-made

Cation

Metal

1st symbol in formula

Anion

Nonmetal

2nd symbol in formula

Covalent (Molecular)

Contain nonmetals only

No ions

Binary Ionic Type I Compounds

Cation has only 1 possible charge

(Check PT)

Naming

ALL IONIC COMPOUNDS:

Name the cation, then name the

anion

Steps in Naming an Ionic

Compound

1) Binary or nonbinary? Why?

2) Ionic or Covalent? Why?

3) If Ionic, Type I or Type II? Why?

4) What is the cation? Symbol and name

5) What is the anion? Symbol and name

6) What is the name of the compound?

Examples

MgCl2

1) Binary or Nonbinary? Why?

Binary --2 different elements ( 2 capital

letters)


Ionic – Mg is a metal(Check PT)

3)Type I or Type II? Why?

Type I --Mg has only 1 possible charge

(check PT)

4) Cation symbol and name:

Mg2+ magnesium

5) Anion symbol and name:

Cl1- chloride

NAME THE CATION, THEN THE ANION

6) Name of compound:

magnesium chloride

ZnF2

1)Binary or nonbinary? Why?

Binary --2 elements

2)Ionic or covalent? Why?

Ionic -- Zn is a metal

3) Type I or Type II? Why?

Type I -- Zn has only 1 possible charge

4) Cation symbol and name

Zn2+ zinc

5) Anion symbol and name

F1- fluoride

6) Name of compound

zinc fluoride

Sr3N2


Binary --2 elements

2) Ionic or covalent? Why?

Ionic-- Sr is a metal


Type I --Sr has only 1 possible charge


Sr2+ strontium


N3- nitride

6) Name of compound

strontium nitride

Li3P


Binary-- 2 elements


Ionic --Li is a metal


Type I --Li has only 1 possible charge


Li+1 lithium


P3- phosphide

6) Name of compound

lithium phosphide

Practice1. Name the following compounds, using

the method taught.

a. KCl

potassium chloride

b. Rb3N

rubidium nitride

c. Ba3P2

barium phosphide

d. Li2O

lithium oxide

e. CaI2

calcium iodide

Binary Ionic Type II Compounds

Cation has more than one possible

charge

(Check PT)

Name the cation,

then name the anion

Steps for Binary Ionic Type II




4) What is the cation? Symbol and name

5) What is the anion? Symbol and name

6) What is the name of the compound?

Naming the cationMust determine the charge on the

cation

Compounds are electrically neutral

Total positive charge = total negative charge

Anions can only have 1 possible

charge

How to determine the charge on the cation:

1. Multiply the charge on the anion (check the PT)

by the subscript for the anion to get the total

negative charge

total negative charge =(charge on anion)X(subscript on anion)

2. Change the sign to positive to get the total

positive charge.Total positive charge = (+)(total negative charge)

3. Divide that answer by the subscript on the

cation. That number is the charge on the cation.Charge on cation = (total positive charge) ÷ (subscript on cation)

4. Write this number as a Roman Numeral

in parenthesis after the name for the

element.

5. Follow the rest of the steps in naming the

ionic compound.

Name the cation,

then name the anion

Examples

FeCl2


Binary -- only two elements


Ionic -- Fe is a metal


Type II – Fe can have more than 1

possible charge


Determine charge on cation:

Anion is Cl-1

1) Total negative charge =(Charge on anion)X(subscript on anion)

= (-1)X(2)=-2

2) Total positive charge = (+)(total negative charge)

= +2

3) Charge on cation = (total positive charge) ÷ (subscript on cation)

= +2 ÷ 1 = +2

Fe2+ iron(II)


Cl1- chloride

6) Name of compound

iron(II) chloride

Ni2O3


Binary -- only two elements


Ionic– Ni is a metal

3) Type I orType II? Why?

Type II - Ni can have more than 1

possible charge

4)Cation symbol and name

Determine charge on the cation

Anion is O2-

1) Total negative charge = (Charge on anion)(subscript on anion)

= (-2)(3)= -6

2) Total positive charge = (+)(total negative charge) = +6

3) Charge on cation = (total positive charge) ÷ (subscript on cation)

= +6 ÷ 2 = +3

Ni3+ nickel(III)


O2- oxide

6) Name of compound

nickel(III) oxide

PracticeName the following compounds. Show your

work.

a. FeBr3

iron(III) bromide

b. FeBr2

iron(II) bromide

c. Ti2O3

titanium(III) oxide

d. TiO2

titanium(IV) oxide

e. Cr3N2

chromium(II) nitride

f. CrN

chromium(III) nitride

Binary Covalent(Molecular)

Compounds

Compound contains 2 nonmetals

No ions

The two nonmetals may form more than one

different compound

Use prefixes in name to indicate number of each

type of atom

1 = mono 6 = hexa

2 = di 7 = hepta

3 = tri 8 = octa

4 = tetra 9 = nona

5 = penta 10 = deca

Naming Covalent Compounds1) Binary or nonbinary? Why?


3) If covalent: What is the name of the 1st element?

Write the name of the 1st element adding a prefix if the

subscript is not 1.

4) What is the name of the 2nd element?

Write the name of the second element adding a prefix for the

subscript, even if the subscript is 1, and changing the ending

to –ide.

For oxygen: When adding prefixes, omit the ending vowel on

the prefix, if it is an o or a, and would make a double vowel.

5) Write the name of the compound.

Examples

CO


Binary-- contains only 2 elements


Covalent – both elements are nonmetals

3) Name of 1st element?

C (carbon) is the first element, subscript 1, no prefix; carbon

4) Name of 2nd element?

O (oxygen) is the second element, subscript 1, prefix is mono;

monoxide

5) Name of compound

carbon monoxide (no double o)

P2O5


Binary -- contains only 2 elements


Covalent – both elements are nonmetals

3)Name of 1st element?

P (phosphorus) is the first element, subscript 2, prefix is di;

diphosphorus

4) Name of 2nd element?

O (oxygen) is the second element, subscript 5, prefix is

penta; pentoxide

5) Name of compound

diphosphorus pentoxide

Practice

1. Name the following compounds.

a. CO2

carbon dioxide

b. N2H4

dinitrogen tetrahydride

c. B2H6

diboron hexahydride

d. PBr5

phosphorus pentabromide

e. P2S3

diphosphorus trisulfide

Section 2: Naming Nonbinary

Compounds

Nonbinary Ionic compounds

Compounds containing a polyatomic ion. Usually

start with a metal – exception is NH4+ -- the

ammonium cation

Name the cation, then the anion

Treat as a Type I or Type II compound

The ending on the polyatomic ion does

not change

Notice most end in –ite or –ate

Means the polyatomic ion contains oxygen

(oxyions)

-ate contains more oxygen atoms than –ite

Exceptions: –OH1- – called hydroxide

–O22- – called peroxide

Prefixes have meaning, too

hypo- under or less oxygen

per – more or most oxygen

Cl-1 chloride

ClO-1 hypochlorite

ClO2-1 chlorite

ClO3-1 chlorate

ClO4-1 perchlorate

Examples

Na2SO4


Nonbinary– contains more than 2 elements


Ionic– Na is a metal and contains a polyatomic ion


Type I – Na has only 1 possible charge


Na1+sodium


SO42- sulfate

6) Name of compound

sodium sulfate

Co(HCO3)3


Nonbinary– contains more than 2 elements


Ionic– Co is a metal & contains a polyatomic ion


Type II -- Co can have more than 1

possible charge


Determine charge on the cation

Anion is HCO3-1

1) Total negative charge = (Charge on

anion)(subscript on anion)

= (-1)(3)= -3

2) Total positive charge = (+)(total negative

charge) = +3

3) Charge on cation = (total positive charge) ÷

(subscript on cation)

= +3 ÷ 1 = +3

Co3+ cobalt(III)


HCO3-1 bicarbonate

6) Name of compound

cobalt(III) bicarbonate

NH4NO3


Nonbinary – contains more than 2 elements


Ionic – NH41+ is a polyatomic ion


Type I – NH4+1 has only 1 possible charge


NH4+1 ammonium


NO31- nitrate

6) Name of compound

ammonium nitrate

PracticeGive the type and name the following

compounds. Show your work.

a. Na2CO3

sodium carbonate

b. CuSO4

copper(II) sulfate

c. CsClO4

cesium perchlorate

d. Co(NO3)3

cobalt(III) nitrate

e. Au2(SO3)3

gold(III) sulfite

Section 3: Acids

A compound that produces H+1

ions when dissolved in water

Ionic compounds

Cation is the H 1+ ion –

hydrogen acting as a metal

Formulas begin with H

Have subscript (aq) at end

Aq =aqueous = dissolved in water

Two Types

Type depends upon

whether or not the anion

contains oxygen

Binary Acids

Oxyacids

Binary Acids

Cation is H1+

Anion does not contain oxygen

Examples

HCl(aq), HCN(aq), HBr(aq)

(aq) = aqueous -- means dissolved in water

Naming Binary Acids

1) Is it an acid? Why?

2) Is it a binary acid or an oxyacid? Why?

3) Cation Symbol and name?

The H1+ ion is named hydro-

4) Anion symbol and name?

The ending of the anion is changed to –ic;

The word acid is added at the end

5) Name the acid

Binary Acid Anions

F1- fluoric Se2- selenic

Cl1- chloric Te2- telluric

Br1- bromic P3- phosphoric

I1- iodic As3- arsenic

At1- astatic

CN1- cyanic

S2- sulfuric

Example

HCl(aq)


Yes -starts with H, is aqueous

2) Is it a binary acid or oxyacid? Why?

Binary acid – anion does not contain oxygen


H1+ (hydro-)


Cl1- chloric – change ending to –ic; add the word acid

5) Name of acid

hydrochloric acid

If not dissolved in water, name as an ionic compound (HCl

would be hydrogen chloride)

Practice1. Name the following compounds

a. HI(aq)

hydroiodic acid

b. H2S(aq)

hydrosulfuric acid

c. HF(aq)

hydrofluoric acid

OxyacidsCation is still H+

Anion is a polyatomic ion that contains oxygen

Exceptions – hydroxide (OH1-) and peroxide (O22-) do

not make acids.

Examples

HNO3(aq), H2SO3(aq)

Naming Oxyacids



3) Cation symbol

4)Anion symbol and name

The ending changes to -ous if it was –ite

or -ic if it was –ate

Add acid as the second word in the name

5) Name the compound

Funky changes:

sulfite – sulfurous

sulfate – sulfuric

phosphate – phosphoric

Examples

H2SO4(aq)


Yes – starts with H, is aqueous

2) Is it a binary acid or oxyacid? Why?

Oxyacid - anion contains oxygen


H+1( but not in name)


SO42- sulfate changes to sulfuric; add acid

5) Name of acid

sulfuric acid

H2SO3(aq)


– Yes, starts with H, is aqueous


Oxyacid --anion contains oxygen


H+1( but not in name)


SO32- sulfite changes to sulfurous; add acid

5)Name of acid

sulfurous acid

Practice

1. Name the following compounds.

a.HNO3(aq)

nitric acid

b.H2CO3(aq)

carbonic acid

c. HClO(aq)

hypochlorous acid

d. H3AsO4(aq)

arsenic acid

Section 4: Writing Formulas from NamesIonic compounds (review)

Determine the type of compound



3) Type I or II? Why?

4)Write down the symbol and the charge of the cation

5)Write down the symbol and the charge of the anion

6) Continue as taught in Unit 3 – figure out the LCM,

etc.

1) LCM

2) Determine the subscript on the cation:

Cation: ( )(charge on cation) = LCM

3)Determine the subscript on the anion:

Anion: ( )(charge on anion) = -LCM

4) Check: 2+ 3 =0

5)Formula:

Another way -- The “X” maneuver

1) Binary or nonbinary? Why? (only need if want type of compound)



4)Write down the symbol and the charge of the cation

5)Write down the symbol and the charge of the anion

6) Make the superscript (no sign) of the cation into the subscript for the anion.

Make the superscript (no sign) of the anion into the subscript for the cation.

7) Write the formula.

- If a polyatomic is involved, use parenthesis if the

subscript will be anything other than 1.

- If the subscripts have a common factor, reduce –

lowest whole number ratio.

X+2 Y-3

X3Y2

Examples

magnesium chloride


Binary – does not contain a polyatomic


Ionic – contains a metal


Type I – No Roman Numeral

4) Cation is Mg2+

5) Anion is Cl1-

6)Mg2+ Cl1-

7)MgCl2

nickel(III) carbonate


Nonbinary – carbonate is a polyatomic ion


Ionic – contains a metal and a polyatomic


Type II – there’s a Roman Numeral in the name

4) Cation is Ni3+

5) Anion is CO32-

6) Ni3+ CO32-

7) Ni2(CO3)3

lead(IV) oxalate


nonbinary – oxalate is a polyatomic ion


Ionic – contains a metal and a polyatomic

3) Type I or TypeII? Why?

Type II – There’s a Roman Numeral in the name

4) Cation is Pb4+

5) Anion is C2O42-

6) Pb4+ C2O42-

7) Pb2(C2O4)4

- Simplify: Pb(C2O4)2

Practice

1. Write the formula for each of

the following compounds

a. barium hydroxide

Ba(OH)2

b. cobalt(III) sulfate

Co2(SO4)3

c.lithium chloride

LiCl

d.chromium(II) chromate

CrCrO4

Covalent Compounds

1) Binary or nonbinary? Why? ( only need if need type of compound)


3) Write down the symbol for the first element and use the prefix to determine the subscript –remember no “1” subscripts

4) Write down the symbol for the second element and use the prefix to determine the subscript –remember no “1” subscripts

- DO NOT SIMPLIFY

5) Write the formula

Examplescarbon dioxide


Binary – only 2 elements


Covalent -- two nonmetals, prefix in name

3) 1st element is carbon (C) no prefix – so no

subscript

4) 2nd element is oxygen (O) prefix di- so

subscript is 2

5) Formula is CO2

dinitrogen tetroxide1) Binary or nonbinary? Why?

Binary – only two elements


Covalent -- two nonmetals, prefixes in

name

3) 1st element is nitrogen (N), prefix is di- so

subscript is 2

4) 2nd element is oxygen (O), prefix is tetra- so

subscript is 4

5) Formula is N2O4 -- do not simplify

Practice1. Write the formula for each of the following

compounds

a. nitrogen monoxide

NO

b. diphosphorus pentoxide

P2O5

c. carbon disulfide

CS2

Acids1) Is it an acid? Why?


3) Write down H1+ for the cation

4) Write down the symbol and charge for the

anion (watch endings)

binary –ic to –ide

oxyacid -ic to -ate; -ous to -ite

5)Do the “X” thing

6)Add the subscript (aq) at the end

Examplesnitric acid

1) Is it an acid?

Yes, acid in name

2) Binary acid or oxyacid?

oxyacid no “hydro” in name

3)Cation is H+1

4)Anion is nitrate(-ic to –ate) NO3-1

5) H+1 NO3-1

6) HNO3(aq)

hydrobromic acid

1) Is it an acid?

Yes – acid in name

2) binary acid or oxyacid?

Binary – “hydro” in name

3) Cation is H+1

4) Anion is bromide (-ic to –ide)Br-1

5) H+1 Br-1

6) HBr(aq)

Sulfurous acid1) Is it an acid?

Yes – acid in name

2) Binary acid or oxyacid?

oxyacid – no “hydro” in name

3) Cation is H+ 1

4) Anion is sulfite (-ous to –ite) SO32-

5) H+ 1 SO32-

6) H2SO3(aq)

Practice

1. Write the formula for each of the

following compounds

a. phosphoric acid

H3PO4(aq)

b. hydroiodic acid

HI(aq)

c. bromic acid

HBrO3(aq)

d. hydrophosphoric acid

H3P(aq)

Documents

Chemistry Essentials Unit 4 · 2020-01-27 · Section 1: Naming Binary Compounds Three types of binary compounds Types I & II –Ionic Contain ions –a cation and an anion Contain