Chapter 5
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Chapter 5. Naming Compounds Writing Formulas. Naming Binary Ionic Compounds. Binary Compounds - 2 elements. Ionic - a cation and an anion. To write the names just name the two ions. Easy with Representative elements. Group A NaCl = Na + Cl - = sodium chloride

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Chapter 5

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Chapter 5

Chapter 5

Naming Compounds

Writing Formulas


Naming binary ionic compounds

Naming Binary Ionic Compounds

  • Binary Compounds - 2 elements.

  • Ionic - a cation and an anion.

  • To write the names just name the two ions.

  • Easy with Representative elements.

  • Group A

  • NaCl = Na+ Cl- = sodium chloride

  • MgBr2 = Mg+2 Br- = magnesium bromide


Naming binary ionic compounds1

Naming Binary Ionic Compounds

  • The problem comes with the transition metals.

  • Need to figure out their charges.

  • The compound must be neutral.

  • same number of + and – charges.

  • Use the anion to determine the charge on the positive ion.


Naming binary ionic compounds2

Naming Binary Ionic Compounds

  • Write the name of CuO

  • Need the charge of Cu

  • O is -2

  • copper must be +2

  • Copper (II) chloride

  • Name CoCl3

  • Cl is -1 and there are three of them = -3

  • Co must be +3 Cobalt (III) chloride


Naming binary ionic compounds3

Naming Binary Ionic Compounds

  • Write the name of Cu2S.

  • Since S is -2, the Cu2 must be +2, so each one is +1.

  • copper (I) sulfide

  • Fe2O3

  • Each O is -2 3 x -2 = -6

  • 2 Fe must = +6, so each is +3.

  • iron (III) oxide


Naming binary ionic compounds4

Naming Binary Ionic Compounds

  • Write the names of the following

  • KCl

  • Na3N

  • CrN

  • Sc3P2

  • PbO

  • PbO2

  • Na2Se


Ternary ionic compounds

Ternary Ionic Compounds

  • Will have polyatomic ions

  • At least three elements

  • Just write the name of the element using the front of the periodic table and the polyatomic ion using the chart on the back of the table.

  • Examples of naming ternary ionic compounds:

  • NaNO3 = sodium nitrate

  • (NH4)2O = ammonium oxide


Ternary ionic compounds name these

Ternary Ionic Compoundsname these:

  • LiCN

  • Fe(OH)3

  • (NH4)2CO3

  • NiPO4

  • CaSO4

  • CuSO3


Writing formulas

Writing Formulas

  • The charges have to add up to zero.

  • Get charges for the 2 parts.

  • Cations from location on p. table.

  • Anions from p. table or polyatomic.

  • Balance the charges by putting in subscripts (small #’s on bottom right).

  • Put polyatomic ions in parenthesis before you give them subscripts.


Writing formulas1

Writing Formulas

  • Write the formula for calcium chloride.

  • Calcium is Ca+2

  • Chloride is Cl-1

  • Ca+2 Cl-1 would have a +1 charge.

  • Need another Cl-1

  • Ca+2 Cl2-1

  • CaCl2


Write the formulas for these

Write the formulas for these

  • Lithium sulfide

  • tin (II) oxide

  • tin (IV) oxide

  • Magnesium fluoride

  • Copper (II) sulfate

  • Iron (III) phosphide

  • gallium nitrate

  • Iron (III) sulfide


Write the formulas for these1

Write the formulas for these

  • Ammonium chloride

  • ammonium sulfide

  • barium nitrate


Things to look for

Things to look for

  • If cations have (roman numeral), the number is their charge.

  • If anions end in -ide they are probably off the periodic table (Monoatomic)

  • Exceptions (Hydroxide (OH); Cyanide (CN) are polyatomic.

  • If anion ends in -ate or -ite it is polyatomic.


Molecular compounds

Molecular Compounds

Writing names and Formulas


Molecular compounds1

Molecular compounds

  • made of just nonmetals

  • smallest piece is a molecule

  • can’t be held together because of opposite charges

  • can’t use charges to figure out how many of each atom


Easier

Easier

  • Ionic compounds use charges to determine how many of each.

    • Have to figure out charges.

    • Have to figure out numbers.

  • Molecular compounds name tells you the kind of atoms.

  • Uses prefixes to tell you the number


Prefixes

Prefixes

  • 1 mono-

  • 2 di-

  • 3 tri-

  • 4 tetra-

  • 5 penta-

  • 6 hexa-

  • 7 hepta-

  • 8 octa-

  • 9 nona-

  • 10 deca-


Prefixes1

Prefixes

  • To write the name write two words

Prefix

name

Prefix

name

-ide


Prefixes2

Prefixes

  • To write the name write two words

  • One exception is we don’t write mono- if there is only one of the first element.

Prefix

name

Prefix

name

-ide


Prefixes3

Prefixes

  • To write the name write two words

  • One exception is we don’t write mono- if there is only one of the first element.

  • No double vowels when writing names (oa oo)

Prefix

name

Prefix

name

-ide


Name these

Ex. CO carbon monoxide

CO2 carbon dioxide

P2O5 diphosphorus pentoxide

Name These

  • N2O

  • NO2

  • Cl2O7

  • CBr4

  • BaCl2


Write formulas for these

Write formulas for these

  • diphosphorus pentoxide

  • tetraiodide nonoxide

  • sulfur hexaflouride

  • nitrogen trioxide

  • Carbon tetrahydride

  • phosphorus trifluoride

  • aluminum chloride


Acids

Acids

Writing names and Formulas


Acids1

Acids

  • Compounds that give off hydrogen ions when dissolved in water.

  • Must have H in them.

  • will always be some H next to an anion.

  • The anion determines the name.


Naming acids

Naming acids

  • If the anion attached to hydrogen is ends in -ide, put the prefix hydro- and change -ide to -ic acid

  • HCl - hydrogen ion and chloride ion

  • hydrochloric acid

  • H2S hydrogen ion and sulfide ion

  • hydrosulfuric acid


Naming acids1

Naming Acids

  • If the anion has oxygen in it

  • it ends in -ate or -ite

  • change the suffix -ate to -ic acid

  • HNO3 Hydrogen and nitrate ions

  • Nitric acid

  • change the suffix -ite to -ous acid

  • HNO2 Hydrogen and nitrite ions

  • Nitrous acid


Name these1

Name these

  • HF

  • H3P

  • H2SO4

  • H2SO3

  • HCN

  • H2CrO4


Writing acid formulas naming

Writing Acid Formulas/Naming

  • Hydrogen will always be first

  • name will tell you the anion

  • make the charges cancel out

  • Starts with hydro- if no oxygen in the acid, -ide ending becomes –ic

    Ex. HCl = hydochloric acid

  • no hydro, -ate ending from polyatomic ion becomes -ic, H2SO4 = sulfuric acid

    -ite ending becomes –ous, H2SO3 = sulfurous acid


Write formulas for these1

Write formulas for these

  • hydroiodic acid

  • acetic acid

  • carbonic acid

  • phosphorous acid

  • hydrobromic acid


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