Nomenclature lab : will rate answer Nomenclature lab: will choose best answr NM

Question

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Nomenclature lab: will choose best answr

NM

NM

= nonmetal

-3

-2

-1

NM

+1

+2

md

= metalloid

md

NM

NM

NM

NM

NM

+1

+2

+3

md

NM

NM

NM

NM

+1

+2

+2

md

md

NM

NM

NM

+1

+2

+1

md

md

NM

NM

+1

+2

md

NM

+1

+2

Type I Binary Ionic Compounds

Type I binary ionic compounds contain a metal and a nonmetal AND the metal that is present only forms one type of cation. Metals with only one cation(shaded below with charges). Both the metal and the nonmetal form ions, which is why it is called an ionic compound.

From the following list, cross out those compounds that do NOT belong in the category for Type I binary ionic compounds.

NaCl FeCl2 CaCl2 TiO2 MgO AlBr3 KCl K2S BeF2 Cu2O3 AgCl Zn3N2

Formula and name examples for Type I binary ionic compounds:

KI = potassium iodide BaO = barium oxide ZnF2 = zinc fluoride Na2S = sodium sulfide

Ag3N = silver nitride BeCl2 = beryllium chloride

What type of element is always listed first (metal or nonmetal)? ____________ second? ___________

Is the name of the first element in the compound different from the element? (yes/no)

What is the common ending for all the names? ______________

In zinc fluoride, there are 2 fluoride atoms, are they indicated in the name? (yes/no)

What is the charge on the zinc ion? _______

What is the charge on the fluoride ion? _______

Why do you need one zinc ion and two fluoride ions for the formula for zinc fluoride?

Why do you need two sodium ions for every sulfide ion in sodium sulfide?

Try not to look in your book and determine the rules for naming type I binary ionic compound when given the formula.

Try not to look in your book and determine the rules for writing the formula for a type I binary compound when given the name.

Name each of the type I binary ionic compounds listed in Question 1 of the Type I section in words.

Type II Binary Ionic Compounds

Type II binary ionic compounds also contain a metal and a nonmetal however the metal that is present here can form more than one type of cation. Metals with multiple possible charges are listed in the periodic table as blank. Type II metals are NOT Type I metals. Again, both the metal and the nonmetal form ions, and it is still called an ionic compound. These metals usually only form two different ions.

From the following list, cross out those compounds that do NOT belong in the category for Type II binary ionic compounds.

AlP FeCl2 Ag2O VBr5 CoS SnF2 K3N SrF2 CuBr AuCl3 ZnO HgS

Formula and name examples for Type II binary ionic compounds:

Fe2O3 = iron(III) oxide or ferric oxide FeO = iron(II) oxide or ferrous oxide

CuS = copper(II) sulfide or cupric sulfide CuCl = copper(I) chloride or cuprous chloride

MnO2 = manganese(IV) oxide or manganic oxide MnCl2 = manganese(II) chloride or manganous chloride

What type of element is always listed first (metal or nonmetal)? ____________ second? ___________

Is the name of the first element in the compound different from the element? (yes/no)

What is the common ending for the nonmetal portion of the names? ______________

In the compound FeO, what is the charge on iron? _______

In the compound Fe2O3, what is the charge on iron? ________

What does the Roman number after the metal name represent?

Try not to look in your book and determine the rules for naming type II binary ionic compound when given the formula.

Try not to look in your book and determine the rules for writing the formula for a type II binary compound when given the name.

Name each of the type II binary ionic compounds listed in Question 1 of the Type II section in words.

Type III (Nonmetallic) Binary Compounds

Binary compounds that do not contain metals, sometimes referred to as binary molecular compounds, have covalent bonds instead of ionic bonds. A covalent bond is formed by sharing one or more pairs of electrons. The pair of electrons is shared by both atoms. For example, in forming H2, each hydrogen atom contributes one electron to the single bond.

From the following list, cross out those compounds that do NOT belong in the category for binary compounds containing only nonmetals or metalloids.

CCl4 AlCl3 CO SeF6 SiO2 SrI2 P4O10 TiO2 SeO3 IrCl ZrO2 N2O5

Formula and name examples for Type III binary molecular compounds:

CO2 = carbon dioxide H2O = dihydrogen monoxide

IF5 = iodine pentafluoride BF3 = boron trifluoride

Which element is listed first in the name?

Is the name of the first element in the compound different from the element? (yes/no)

What is the common ending for all the names? ______________

What do the prefixes (di-, mono-, penta-, tri-) in the names above mean?

Is the prefix mono- used when there is only one atom of the first element? (yes/no)

Is the prefix mono- used when there is one atom of the second element? (yes/no)

Try not to look at your book and determine the rules for naming type III binary ionic compound when given the formula.

Name each of the type III binary compounds in Question 1 of the Type III section in words.

Compounds Containing Polyatomic Ions

Polyatomic ions are ions that as a group have a set charge. Polyatomic ions are usually recognized in a formula by the grouping of more than one nonmetal elements after a metal. Your book has a table listing polyatomic ions. Use your book’s table to fill in the following table with the appropriate names/formulas of the polyatomic ions.

Name

Formula

Name

Formula

hydronium

chlorite

phosphate

C2H3O2-1

SO3-2

ClO4-1

OH-1

carbonate

cyanide

NO2-1

Polyatomic ions containing oxygen (oxyanions or oxoanions) are somewhat special.

carbonate = CO3-2

Match the location of carbon on the periodic table with the two figures on the right.

What number is in the carbon location on the left figure? To what does this number refer?

What number is the carbon location on the right figure? To what does this number refer?

What element must all oxyanions contain?

What is the ending of the name of the ion determined from these tables?

Determine the formula for the following oxyanions using the figures above. Phosphate _________ Silicate ________ Bromate ________ Iodate ________ Sulfate ________ Nitrate ________

Review Table

Use your knowledge of Type I and Type II metals as well as the appropriate polyatomic name/formula to fill in the following table.

Name

Formula

Name

Formula

sodium phosphate

Cu(ClO)2

tin (II) nitrate

calcium sulfate

KCN

ammonium nitrate

Sr(MnO4)2

MnSO4

Acids

Acids are compounds that when dissolved in water, produce hydrogen ions (H+). Naming acids can be tricky. Use the following figure to determine how to name an acid.

FG02_27

Given that the ion formula is NO2-1, how can one determine the name of the ion, acid formula, and acid name?

Ion name:

What is the formula for nitrate?

Is NO2-1 the nitrate ion or the nitrite ion?

Acid formula:

According to the figure above, what ion must be added to create an acid? What is the charge of that ion?

How many of the hydrogen ions must be added to NO2-1 to make a neutral acid (zero charge)?

What is the chemical formula for the acid created when hydrogen ion(s) are added to NO2-1?

Acid name:

Based on your answer to Question 1 above, does the name for the NO2-1 ion end in –ite or –ate?

Name the acid, HNO2.

Fill in the following acid table:

Acid Formula

Acid Name

Anion Formula

Anion Name

HCl

hydrochloric acid

Cl¯

chloride

ClO3¯

sulfuric acid

bromate

PO4-3

HF

H2CO3

C2H3O2 ¯

NM

NM

= nonmetal

-3

-2

-1

NM

+1

+2

md

= metalloid

md

NM

NM

NM

NM

NM

+1

+2

+3

md

NM

NM

NM

NM

+1

+2

+2

md

md

NM

NM

NM

+1

+2

+1

md

md

NM

NM

+1

+2

md

NM

+1

+2

Explanation / Answer

1.) Compounds not belonging to Type 1 ionic compounds

FeCl2 , TiO2 , Cu2O3 , AgCl , Zn3N2

2.) Metal is always listed first; nonmetal listed second.

3.) Name of the first element in the compound is not different from that element

4.) Common ending for all the names: "IDE" like Chloride, Bromide, Sulfide

5.) No, the 2 fluoride atoms, are not indicated in the name

6.) The charge on the zinc ion is +2

7.) The charge on the fluoride ion is -1

8.) Zinc ion has charge +2 and Floride ions have charge of -1 each. So, to balance the charges in the compound, two fluoride ions are required per zinc ion for the formula for zinc fluoride.

9.) Sodium ion has charge +1 and sulfide ions have charge of -2 each. So, to balance the charges in the compound, two sodium ions are required per sulfide ion for the formula in sodium sulfide

10.) Rules for naming type I binary ionic compound when given the formula:

a) Name of metal is written first, followed by name of non-metal as in the formula

b) The name of metal is written as such; the name of nonmetal is written by adding "ide" as suffix like, Cl=Chloride, S=Sulfide, F=Fluoride

11.) Rules for writing the formula for a type I binary compound when given the name:

a) In the formula, abbreviation name for element is used

b) Firstly the metal is written, then non metal

c) balancing of valencies accoding to charge: Suppose A is metal with valency 2, and B is non metal with valency 1

So formula will be written by crossing the valency: i.e. in this formula would be A3B2

d) If the valencies of both are same, then the elements are written in formula as such.

12.) NaCl = Soudium chloride, CaCl2 = Calcium chloride, MgO = Magnesium oxide, AlBr3 = Aluminium bromide,

KCl = Potasium chloride, K2S = Potassium sulfide, BeF2 = Beryllium Fluoride

13.)AlP, K3N, SrF2

14.) Metal is always listed first; nonmetal listed second.

15.) Name of the first element in the compound is different from that element, like cuprous/ cupric for copper

16.) Common ending for all the names: "IDE" like Chloride, Bromide, oxide

17.) In the compound FeO, the charge on iron is +2_______

18.) In the compound Fe2O3, the charge on iron is +3 ________

19.) Roman number after the metal name represent the oxidation state of metal in the compound

20.) Rules for naming type II binary ionic compound when given the formula:

a) Name of metal is written first, followed by the oxidation state in roman numeral, followed by the name of non-metal as in the formula

b) The name of metal is written according to oxidation state, as given below; the name of nonmetal is written by adding "ide" as suffix like, Cl=Chloride, S=Sulfide, F=Fluoride

Formula and name examples for Type II binary ionic compounds:

Fe2O3 = iron(III) oxide or ferric oxide FeO = iron(II) oxide or ferrous oxide

CuS = copper(II) sulfide or cupric sulfide CuCl = copper(I) chloride or cuprous chloride

MnO2 = manganese(IV) oxide or manganic oxide MnCl2 = manganese(II) chloride or manganous chloride

21.) Rules for writing the formula for a type II binary compound when given the name:

a) In the formula, abbreviation name for element is used

b) Firstly the metal is written, then non metal

c) balancing of valencies accoding to charge: Suppose A is metal with valency 2, and B is non metal with valency 1

So formula will be written by crossing the valency: i.e. in this formula would be A3B2

d) If the valencies of both are same, then the elements are written in formula as such.

22.) FeCl2 = Ferrous (II) chloride, Ag2O = silver (II) oxide, VBr5 = Vanadium (II) bromide, CoS= Cobalt (II) Sulfide, SnF2= Tin (II) Fluoride, CuBr = Cuprous (II) Bromide, AuCl3 = Gold (III) Chloride, ZnO = Zinc (II) Oxide, HgS = Mercury (II) Sulphide

23.) CCl4, CO , SeF6, SiO2 , P4O10 , SeO3, N2O5

24.) The element which donates electron for sharing is listed first in the name

25.) Name of the first element in the compound is not different from the element

26.) Common ending for all the names: "IDE" like Chloride, Bromide, oxide

27.) The prefixes (di-, mono-, penta-, tri-) in the names above mean that number of atoms present in the compound

like di-hydrogen means 2 hydrogen atoms are present

28.) No, prefix mono- is not used when there is only one atom of the first element.

29.) Yes, the prefix mono- is used when there is one atom of the second element

30.) Rules for naming type II binary ionic compound when given the formula:

a) Name of first lement is written first, followed by the name of other as in the formula

b) The name of first element as such, with prefix di-, tri- for 2 or more atoms; the name of second element is written by adding prefix mono-, di-, tri-, as per the number of atoms and "ide" as suffix like, Cl=Chloride, S=Sulfide, F=Fluoride

Formula and name examples for Type III binary molecular compounds:

CO2 = carbon dioxide H2O = dihydrogen monoxide

IF5 = iodine pentafluoride BF3 = boron trifluoride

31.) CCl4 =carbon tetrachloride, CO = carbon monoxide, SeF6= selenium fluoride, SiO2= silicon dioxide , P4O10= phosphorus pentaoxide, SeO3 = selenium trioxide, ZrO2= zirconium dioxide, N2O5=dinitrogen pentaoxide

32.)

Name

Formula

Name

Formula

hydronium

chlorite

phosphate

C2H3O2-1

SO3-2

ClO4-1

OH-1

carbonate

cyanide

NO2-1

33.) all oxyanions MUST contain oxygen

34.) The ending of the name of the ion is "ITE" or "ATE"

35.) Phosphate = PO43- Silicate = SiO44- Bromate = BrO3- Iodate = IO3- Sulfate = SO42- Nitrate = NO3-

36.)

Name

Formula

Name

Formula

sodium phosphate

Cu(ClO)2

tin (II) nitrate  

calcium sulfate

KCN

ammonium nitrate

Sr(MnO4)2

MnSO4

37.) Acids are compounds that when dissolved in water, produce hydrogen ions (H+). Naming acids can be tricky. Use the following figure to determine how to name an acid.

Figure not present

38.) Given that the ion formula is NO2-1, how can one determine the name of the ion, acid formula, and acid name?

Ion name: Nitrite ion

Since charge is -1, so it gives one H+ ion, Formula of acid would be HNO2, name would be Nitrous acid

39.) The formula for nitrate is NO3-

40.) NO2-1 is the nitrite ion

41.) Acid formula: Nitrous acid

42.) According to the figure above, what ion must be added to create an acid? What is the charge of that ion?

43.) H+ ion (Hydronium ion) is required, it has charge of +1

44.) How many of the hydrogen ions must be added to NO2-1 to make a neutral acid (zero charge)?

One H+ ion is required

45.) What is the chemical formula for the acid created when hydrogen ion(s) are added to NO2-1?

HNO2

46.) Acid name: Nitrous acid

47.) Based on your answer to Question 1 above, does the name for the NO2-1 ion end in –ite or –ate?

It ends in -ITE

48.) Name the acid, HNO2 = Nitrous acid

49.) Fill in the following acid table:

Acid Formula

Acid Name

Anion Formula

Anion Name

HCl

hydrochloric acid

Cl¯

chloride

ClO3¯

sulfuric acid

bromate

PO4-3

HF

H2CO3

C2H3O2 ¯

Name

Formula

Name

Formula

hydronium

H+

chlorite

ClO-

phosphate

PO43- Acetate

C2H3O2-1

sulphite

SO3-2

perchlorate

ClO4-1

hydroxyl

OH-1

carbonate

CO32-

cyanide

CN- Nitrite

NO2-1

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