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Compound Name and Formulas Worksheet Answer Key, Exercises of Chemistry

Sacred Heart University (SHU)Chemistry

Answer key for Compound name and formulas worksheet prepared by Dr. Jim Zoval at Saddleback College.

Typology: Exercises

2020/2021

Uploaded on 04/20/2021

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Naming Compounds Tutorial and Worksheet
Since we use different methods in naming binary covalent (molecular)
compounds and ionic compounds, the first step in naming or writing the formula
of a compound is to determine which of the 2 compound classes it belongs. This
can be done as follows:
Binary covalent compounds will contain only two types of non-metal elements.
There may be more than one of each element. For example CO2 contains just two
types of elements, carbon and oxygen. We will discuss naming covalent
compounds that contain more than two types of elements, like glucose C6H12O6,
in later chapters.
Once it is determined that the compound is ionic or covalent, the student can be
asked to do either of the following:
1) Given the name of the compound, write the formula.
Or
2) Given the formula of the compound, write the name.
In this tutorial we will review the process for achieving these 2 objectives and
practice with some worksheet problems. First, we will review and practice how to
write formulas for compounds when given the compound’s name. Second, we
will review and practice how to write the name of a compound when given the
compound’s formula.
Determine if the Compound is Binary Covalent (Molecular) or Ionic:
Does the compound contain only two types of nonmetal elements?
Yes
Binary Covalent
(Molecular) Compound
No
Ionic Compound
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pf13
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Partial preview of the text

Download Compound Name and Formulas Worksheet Answer Key and more Exercises Chemistry in PDF only on Docsity!

Naming Compounds Tutorial and Worksheet

Since we use different methods in naming binary covalent (molecular)

compounds and ionic compounds, the first step in naming or writing the formula

of a compound is to determine which of the 2 compound classes it belongs. This

can be done as follows:

Binary covalent compounds will contain only two types of non-metal elements.

There may be more than one of each element. For example CO 2 contains just two

types of elements, carbon and oxygen. We will discuss naming covalent

compounds that contain more than two types of elements, like glucose C 6 H 12 O 6 ,

in later chapters.

Once it is determined that the compound is ionic or covalent , the student can be

asked to do either of the following:

1) Given the name of the compound, write the formula.

Or

2) Given the formula of the compound, write the name.

In this tutorial we will review the process for achieving these 2 objectives and

practice with some worksheet problems. First, we will review and practice how to

write formulas for compounds when given the compound’s name. Second, we

will review and practice how to write the name of a compound when given the

compound’s formula.

Determine if the Compound is Binary Covalent (Molecular) or Ionic :

Does the compound contain only two types of nonmetal elements?

Yes

Binary Covalent

(Molecular) Compound

No

Ionic Compound

Given the Name of the Compound, Writing Formulas for Compounds Determine if the Compound is Binary Covalent (Molecular) or Ionic : Does the compound contain only two types of nonmetal elements? Yes (^) No Binary Covalent (Molecular) Compound:

1) Write the symbol of the first element in

the compound’s name, then the symbol of

the second element in the compound’s

name.

2) Indicate how many atoms of each element

the molecule contains using subscripts

after the atomic symbol.

  • The numbers of atoms are given in the

molecule’s name in Greek prefixes

  • NOTE: If there is no Greek prefix in

front of the first element in the

name that implies the number is 1.

Ionic Compound:

1) Write the symbol/formula of the first ion

in the compound’s name, then the

symbol/formula of the second ion in the

compound’s name.

2) Indicate the ratio of the ions in the

compound using subscripts after each

ion.

  • The ratio of the ions is deduced by

balancing the charges of the ions.

  • IMPORTANT: When there is more

than one of a polyatomic ion in the

formula unit we use parenthesis.

Example Mg(NO 3 ) 2

Examples: Writing the Formulas of Ionic Compounds

Write the formula for magnesium nitrate.

  1. Write the symbol/formula of the first ion in the compound’s name, then the symbol/formula of the second ion in the compound’s name.
  • When you see a polyatomic ion (nitrate), look up the formula and charge in the table of polyatomic ions. Mg NO 3
  1. Indicate the ratio of the ions in the compound using subscripts after each ion. a. This step involves filling in the subscripts boxes as we did in the lecture: Mg NO 3
  • The ratio of the ions is deduced by balancing the charges of the ions.
  • This is done so that the total charge in the crystal, when large numbers of cations and anions combine, is equal to zero.
  • We find the ion’s charge from its position on the periodic table or we look it up in a table in the case of polyatomic ions.
  • Transition metal with varying charges will be written in the compound name in Roman numerals.
  • First, temporarily write the charge of each ion above the ion’s symbol. 2+ 1 - Mg NO 3
  • Next, place numbers in the subscripts such that the total charge of the compound is zero. Note that in this example, we need two nitrate ions, each has a charge of (1-) to cancel the (2+) charge of the magnesium ion:
  • 2(-1) + (+2) = 0 zero total charge. 2+ 1 - Mg 1 NO 3 2
  • We saw a shortcut way to do this called the Criss-Cross Method (see your chapter 3 notes) 2+ 1 - Mg 1 NO 3 2 IMPORTANT: When there is more than one of a polyatomic ion in the formula unit we use parenthesis. There are 2 ions of nitrate in magnesium nitrate Mg 1 NO 3 2 = Mg(NO 3 ) 2 In compound where there is just one formula unit of a polyatomic ion, no parenthesis are needed. An example of this is sodium nitrate: NaNO 3

Examples: Writing the Formulas of Ionic Compounds

Write the formula for iron(II) phosphate.

  1. Write the symbol/formula of the first ion in the compound’s name, then the symbol/formula of the second ion in the compound’s name.
  • When you see a polyatomic ion (phosphate in this case), look up the formula and charge in the table of polyatomic ions. Fe PO 4
  1. Indicate the ratio of the ions in the compound using subscripts after each ion. b. This step involves filling in the subscripts boxes as we did in the lecture: Fe PO 4
  • The ratio of the ions is deduced by balancing the charges of the ions.
  • This is done so that the total charge in the crystal, when large numbers of cations and anions combine, is equal to zero.
  • We find the ion’s charge from its position on the periodic table or we look it up in a table in the case of polyatomic ions.
  • Transition metal with varying charges will be written in the compound name in Roman numerals.
  • In this example, now we know the charge on the Fe ion is 2+
  • First, temporarily write the charge of each ion above the ion’s symbol. 2+ 3 - Fe PO 4
  • Next, place numbers in the subscripts such that the total charge of the compound is zero. Note that in this example, we need two phosphate ions, each has a charge of (3-) and three Fe^2 +^ ions to balance the charge:
  • 2(-3) + 3(+2) = 0 zero total charge. 2+ 3 - Fe 3 PO 4 2
  • We saw a shortcut way to do this called the Criss-Cross Method (see your chapter 3 notes) 2+ 3 - Fe 3 PO 4 2 IMPORTANT: When there is more than one of a polyatomic ion in the formula unit we use parenthesis. There are 2 ions of phosphate in iron(II)phosphate. Fe 3 PO 4 2 = Fe 3 (PO 4 ) 2

Write the formula for the following ionic compounds: (see next page for key)

sodium bicarbonate _________________ sodium fluoride _________________ iron (III) chloride _________________ sodium carbonate _________________ copper (II) sulfate _________________ magnesium hydroxide _________________ barium nitrate _________________ lithium sulfate _________________ magnesium chloride _________________ silver nitrate _________________ aluminum sulfate _________________ calcium hydroxide _________________ calcium sulfate _________________ mercury (II) nitrate _________________ lead (IV) nitrate _________________ magnesium iodide _________________ sodium nitride _________________

Practice Problems KEY

  • sodium bicarbonate NaHCO
  • iron (III) chloride FeCl sodium fluoride NaF
  • sodium carbonate Na 2 CO
  • copper (II) sulfate CuSO
  • magnesium hydroxide Mg(OH)
  • barium nitrate Ba(NO 3 )
  • lithium sulfate Li 2 SO
  • magnesium chloride MgCl
  • silver nitrate AgNO
  • aluminum sulfate Al 2 (SO 4 )
    • calcium hydroxide Ca(OH)
  • calcium sulfate CaSO
  • mercury (II) nitrate Hg(NO 3 )
  • lead (IV) nitrate Pb(NO 3 )
  • magnesium iodide MgI

Write the formulas for the following covalent compounds:

See next page for KEY

a. disulfur tetrafluoride _________________________

b. carbon trioxide _________________________

c. nitrogen pentoxide _________________________

d. nitrogen tribromide _________________________

e. dinitrogen heptachloride _________________________

f. carbon tetrachloride_________________________

g. hydrogen monochloride_________________________

h. trihydrogen monophosphide _________________________

i. dihydrogen monoxide _________________________

KEY

a. disulfur tetrafluoride S 2 F 4

b. carbon trioxide CO 3

c. nitrogen pentoxide NO 5

d. nitrogen tribromide NBr 3

e. dinitrogen heptachloride N 2 Cl 7

f. carbon tetrachloride CCl 4

g. hydrogen monochloride HCl

h. trihydrogen monophosphide H 3 P

i. dihydrogen monoxide H 2 O

Writing the Names of Ionic Compounds

Example: Write the name for CaBr 2

  1. Write the cation name first, then name the anion.
  • monoatomic anions use the “ide” suffix

calcium bromide

  1. If the cation is one of the transition metals with various charges, write the charge using parenthesis and Roman numerals after the metal name.
  • Not necessary here, there is not a transition metal present

Example: Write the name for Mg(NO 3 ) 2

  1. Write the cation name first, then name the anion.
  • monoatomic anions use the “ide” suffix
    • Here we notice that the anion is a polyatomic ion. Get the name from the polyatomic ion table (in your notes or textbook). You will be given a copy of the polyatomic ion table on your exams.
    • Do not change the suffix to “ide” with polyatomic ions:

magnesium nitrate

  1. If the cation is one of the transition metals with various charges, write the charge using parenthesis and Roman numerals after the metal name.
  • Not necessary here, there is not a transition metal present

Writing the Names of Ionic Compounds

Example: Write the name for CuF 2

  1. Write the cation name first, then name the anion.
  • monoatomic anions use the “ide” suffix

copper fluoride

  1. If the cation is one of the transition metals with various charges, write the charge using parenthesis and Roman numerals after the metal name.

copper(?) fluoride

  • We must figure out what the charge is on the copper, we can deduce the charge on the transition metal cations from the charge on the anions - Recall that the total charge for any compound must equal zero. - Since there are two fluorides, each with a charge of (1-) and there is only one copper, we can conclude that the charge on the copper must be (2+). - You can think of this as the reverse criss-cross! See chapter 3 notes for more details.

copper(II) fluoride

write the charge in parenthesis in Roman numerals after the cation name

KEY

NaCl sodium chloride

Fe 2 (CO 3 ) 3 iron(III) carbonate

Cu(OH) 2 copper(II) hydroxide

(NH 4 ) 2 SO 4 ammonium sulfate

LiNO 3 lithium nitrate

BaSO 4 barium sulfate

Mg(NO 3 ) 2 magnesium nitrate

AgCl silver chloride

  • (note: silver is one of the transition metals that only occurs as a (1+) ion)

Al(OH) 3 aluminum hydroxide

CaSO 4 calcium sulfate

FeS Iron(II) sulfide

FeCl 3 iron(III) chloride

NaI sodium iodide

MgCO 3 magnesium carbonate

Writing the Names of Covalent Compounds

  1. List the name of the first element in the formula.
  2. List the second element and add the – ide suffix.
  3. Use Greek prefixes to indicate the number of each atom in the formula.
  • Exception: do not use mono- for the first element in the name.
  • The o or a at the end of the Greek pre-fix is usually dropped when the element name begins with a vowel

Example: Write the name for N 2 S 4

  1. List the name of the first element in the formula.

nitrogen

  1. List the second element and add the – ide suffix.

nitrogen sulfide

  1. Use Greek prefixes to indicate the number of each atom in the formula.
  • See your textbook or lecture notes for a table of the Greek prefixes.

____nitrogen _____sulfide

dinitrogen tetrasulfide

  • Exception: do not use mono- for the first element in the name.
    • Not applicable in this example
  • The o or a at the end of the Greek pre-fix is usually dropped when the element name begins with a vowel - Not applicable in this example

Example: Write the name for SO 3

  1. List the name of the first element in the formula.

sulfur

  1. List the second element and add the – ide suffix.

sulfur oxide

  1. Use Greek prefixes to indicate the number of each atom in the formula.

____ sulfur _____ oxide

sulfur trioxide

  • Exception: do not use mono- for the first element in the name.
    • NOTE, we did not write mono sulfur because of this rule!
  • The o or a at the end of the Greek pre-fix is usually dropped when the element name begins with a vowel - Not applicable in this example

KEY

a. Br 2 I 4 dibromine tetriodide b. P 5 F 8 pentaphosphorus octafluoride c. NO 5 nitrogen pentoxide o The o or a at the end of the Greek pre-fix is usually dropped when the element name begins with a vowel § NOTE, we did not write pentaoxygen because of this rule! d. NBr 3 nitrogen tribromide e. N 2 O 5 dinitrogen pentoxide f. BrCl 3 bromine trichloride g. H 2 S dihydrogen monosulfide h. N 2 O dinitrogen monoxide