ch 7 sec 1 chemical names & formulas pages 219-231 1 modern chemistry chapter 7 chemical...

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

1

Modern ChemistryModern ChemistryChapter 7Chapter 7

Chemical Formulas and Chemical Formulas and Chemical CompoundsChemical Compounds

Sections 1, 3 & 4Chemical Names and Formulas

Using Chemical FormulasDetermining Chemical Formulas


2

Ch

ap

ter

Vocab

ula

ryMonatomic ionBinary compoundNomenclatureOxyanionSaltFormula Mass Percent CompositionEmpirical Formula


3

Section 1

Chemical Namesand Formulas


4

Molecular compounds – for one molecule

Ionic compounds – for one formula unit; the simplest ratio of cations to anions

Chemical Formula

Eight carbon atoms in the

molecule

Eighteen hydrogen atoms in the molecule


5

5 ions – two Al 3+ ions and three (SO4) 2-

ions

Chemical Formula

2 Al atoms

4 O atoms4 SO4 ions


6

• Hydrocarbon – compounds containing hydrogen and carbon

• Binary Compound – compound with only two types of atoms

• Nomenclature – a naming system• Oxyanions – negative polyatomic

ions with oxygen in them

Definitions


7

• Monatomic ions – ions formed from a single atom

• For negative monatomic ions, -ide is added to the root name

Definitions


8

Ionic compounds contain

a metal and/or

a polyatomic ion !!!

How can I tell if the compound is ionic or

covalent ????


9

Ionic Compounds

Writing Fomulas and Naming


10

1+

2+3+ 3-2-1-

Charges on Monatomic Ions


11

Ag 1+Zn 2+Cu 1+ or 2+Fe/Cr2+ or 3+Sn 2+ or 4+Pb 2+ or 4+

Charges on Transition Metals


12

PbO2 and PbOCharges of Metals


13

Polyatomic Ions Page 226


14

Formulas1. Write the symbols2. Determine the charges

1. Monatomic ions from the periodic table

2. Transition metals from a roman numeral

3. Polyatomic ions from a chart on p. 226

3. Cross the charges.4. Reduce to lowest ratio.

Ionic Compounds


15

Names1. Write the cation name.2. Write the anion name.

• Add –ide to the anion if monatomic

3. Add the roman numeral for any transition or group 14 metal.

4. NO PREFIXES!!!!

Ionic Compounds


16

(charge x subscript)+(charge x subscript) = 0

Ionic Binary CompoundsAluminum Oxide

3+ 2-

(3+ x ) + (2- x ) = 02 3

Al2O3

FO

RM

ULA

S


17

Ionic Binary CompoundsAluminum Oxide

3+ 2-

Al2O3

FO

RM

ULA

S


18

Mg3N2

Magnesium

Ionic BinaryCompoundsN

AM

ING

Nitrogen

ide


19

Pra

cti

ce P

ag

e 2

23

1. Write formulas for the binary ionic compounds formed between the following elements:a. potassium and iodineb. magnesium and chlorine c. sodium and sulfurd. aluminum and sulfure. aluminum and nitrogen

2. Name the binary ionic compounds indicated by the following formulas:a. AgCl e. BaOb. ZnO f. CaCl2c. CaBr2

d. SrF2


20

Iron (III) Chloride

3+ 1-

(3+ x ) + (1- x ) = 01 3

FeCl3

Ionic Compounds with Transition MetalsF

OR

MU

LAS


21

Tin (II) Oxide

2+ 2-

(2+ x ) + (2- x ) = 01 1

SnO


OR

MU

LAS


22

Tin (II) Oxide

2+ 2-

SnO


OR

MU

LAS


23

Pra

cti

ce P

ag

e 2

25

1. Write the formula and give the name for the compounds formed between the following ions:a. Cu 2+ and Br − d. Hg 2+ and S 2−

b. Fe 2+ and O 2− e. Sn 2+ and F −

c. Pb 2+ and Cl − f. Fe 3+ and O 2−

2. Give the names for the following compounds:a. CuO c. SnI4b. CoF3 d. FeS


24

PbO

Lead

Ionic Compounds with Transition Metals

NA

MIN

G

OxygenideII

( x 1 ) + ( 2- x 1 ) = 02+


25

Ionic Compounds with Polyatomic Ions

Ammonium Sulfate+ 2-

(1+ x ) + (2- x ) = 02 1

(NH4)2SO4Parenthesis are needed if the p. ion has a subscript from the crossed

charge – outside the ( ).

FO

RM

ULA

S


26

Ca(NO3)2

Calcium

Ionic Compounds with Polyatomic Ions

NA

MIN

G

Nitrate


27

Pra

cti

ce P

ag

e 2

27

1. Write formulas for the following ionic compounds:a. sodium iodide e. copper(II) sulfateb. calcium chloride f. sodium carbonatec. potassium sulfide g. calcium nitrited. lithium nitrate h. potassium perchlorate

2. Give the names for the following compounds:a. Ag2O

b. Ca(OH)2

c. KClO3

d.NH4OH

e. Fe2(CrO4)3

f. KClO


28

Molecular Compounds

Writing Fomulas and Naming


29

Pre

fixes f

or

Covale

nt

p. 228


30

Formulas1. Write the symbols.2. Use prefixes for subscripts.3. DON’T reduce.

Molecular Compound


31

Names1. Write the name of the elements.

– Order: Smaller group number first;– Same group? Greater period

number first.

2. Add –ide to the second element.3. Add prefixes to each element for

the number of atoms.

Molecular Compound


32

Disulfur difluoride

S2F2

Binary Molecular CompoundsF

OR

MU

LAS


33

nitrogen

Binary Molecular CompoundsN

AM

ING

oxygenidedi tetra


34

Pra

cti

ce P

ag

e 2

29

1. Name the following binary molecular compounds:

a. SO3

b. ICl3c. PBr5

2. Write formulas for the following compounds:

a. carbon tetraiodideb. phosphorus trichloridec. dinitrogen trioxide


35

• Acids – Chapter 14• Binary Acids – two elements;

hydrogen and one other element• Oxyacids – contain hydrogen, one

other element and oxygen• Acid – a solution of the compound

in water.

Acids and Salts


36

• Salt – an ionic compound• Made from

– the cation of a base and– the anion of an acid

• Some retain an H in the anion– Example: CO3

2- carbonate

HCO3 1- hydrogen

carbonate or bicarbonate

Acids and Salts


37

Salt

Defi

nit

ion

An

imati

on

p. 230


38

Lis

t of

Acid

s

p. 230


39

Section 1 Homework

Section Review Page 231 #1-5

ch 7 sec 1 chemical names & formulas pages 219-231 1 modern chemistry chapter 7 chemical...

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