chemical names, formulas and bonding - … · chemical names, formulas and bonding general chem re:...

Chemical Names,

Formulas and Bonding

General Chem

Re: 10/11 JG

Covalent Naming Nonmetal-nonmetal

Share electrons

No ions- nothing to balance

Name must tell elements and amounts

Rules: Divide formula in half

Name first element

Name second element change the ending to -IDE

Use Greek prefixes to identify subscripts

(Mono is optional for first element, required with second element)

Common Prefixes Common “-Ide” Names

1-mono 6-hexa bromide iodide selenide

2-di 7-hepta hydride carbide

3-tri 8-octa nitride oxide

4-tetra 9-nona fluoride phosphide

5-penta 10-deca sulfide chloride

Sample: CO (mono)carbon monoxide Name:

1. P4O10 tetraphosphorus decaoxide 5. SO3

2. N2H4 dinitrogen tetrahydride 6. N2O6

3. SF6 7. NO

4. C3H8 8. SO2

Write formulas for the following:

9. chlorine dioxide ClO2

10. dichlorine monoxide Cl2O

11. iodine tribromide

12. nitrogen trioxide

13. diphosphorus tetraoxide

14. carbon tetrafluoride

Covalent Formula Writing and Naming

Write the correct name or formula for each of the following:

1. dinitrogen trioxide __________________ 21. P2O5 ________________________

2. sulfur trioxide ______________________ 22. N2S3 _________________________

3. carbon dioxide _____________________ 23. CCl4 _________________________

4. tetraphosphorus decasulfide __________ 24. CO3 __________________________

5. sulfur hexafluoride __________________ 25. PBr3 __________________________

6. oxygen difluoride ____________________ 26. CO ___________________________

7. dinitrogen tetraoxide ___________________ 27. SCl2 __________________________

8. sulfur dioxide _______________________ 28. S2Cl2 _________________________

9. diarsenic trioxide ____________________ 29. N2O4 _________________________

10. disulfur dichloride ___________________ 30. ClF3 __________________________

11. dinitrogen pentoxide __________________ 31. SiCl4 __________________________

12. sulfur diiodide ______________________ 32. SO4 ___________________________

13. nitrogen dioxide ______________________ 33. N2O5 __________________________

14. iodine monochloride ___________________ 34. Cl2O ___________________________

15. silicon tetrabromide __________________ 35. NO ___________________________

16. selenium difluoride __________________ 36. NO2 __________________________

17. carbon disulfide _____________________ 37. ClO6 __________________________

18. dinitrogen trisulfide __________________ 38. N2Cl4 __________________________

19. silicon disulfide _____________________ 39. N2O ___________________________

20. diarsenic trisulfide _________________ 40. PCl5 ___________________________

NOTES:

ELECTRON DOT FORMULA WORKSHEET

Background: Covalent bonding is formed between nonmetals and nonmetals. A covalent bond is a shared pair of electrons. Atoms share electrons to obtain an electron configuration of a noble

gas, this allows the atoms to become more stable. Molecules can be represented by means of

diagrams in which VALENCE electrons are shown as dots around the chemical symbols of the atoms

and bonds are represented as lines. (This is especially useful when diagramming covalent bonds.)

Historical Note: The dot formulas are sometimes referred to as Lewis Dot Structures after the chemist who first introduced them in 1916---G.N. Lewis.

Rules:

1. Determine the total number of valence electrons.

2. Draw a skeleton structure:

Aim for symmetry.

Be sure to include all elements in the formula!!

Do not string out oxygens. Do not make boxes. 3. Each bond - represents 2 electrons

4. Place electrons as dots around atoms to achieve stable octets (8) and

stable duets (2) for hydrogen. Exceptions: 4 for Be and 6 for B

6. Be sure the total number of electrons in the diagram equals the original

number of total valence electrons.

Examples:

1. Nitrogen = N = group 5 (periodic table) = 5 valence electrons

Electron Dot Formula

2. Cl2 = group 7(periodic table)

2 atoms Cl x 7 valence electrons = 14 total valence electrons


3. H2O H = group 1 = 1 valence electron O= group 6 = 6 valence electrons

H = 2 atoms H X 1 valence electron = 2 valence electrons

O = 1 atom O X 6 valence electron = + 6 valence electrons

8 total valence electrons


1. Draw the electron dot structures for the following atoms.

a) F b) Cl c) P d) O

e) C f) N g) H h) Br

2. 1. Name the compound

2.draw the electron dot structures

3.state the geometric shape for the following molecules.

a) Br2 name & shape b) HCl name & shape c)CH4 name & shape

d) NH3 name & shape e) H2S name & shape f) SiF4 name & shape

g) PF3 name & shape h)C2H6 name & shape i)C2Cl2H4

j) N2H4 name k) C5H12 name l) Cl2O name & shape

The Saga Continues

Single Bonds: one pair of electrons shared between bonding atoms

Cl2 14 total valence electrons

Double Bonds: two pairs of electrons shared between bonding atoms

O2 12 total valence electrons

Triple Bonds: Three pairs of electrons shared between bonding atoms

N2 10 total valence electrons

All atoms still need to achieve a stable octet (or duet for H).

Follow all bonding rules.

Draw electron dot structures for the following compounds.

1. CO2 name 2. SiS2 name

3. C2H4 name 4. H2CO

5. H2C2O2 6. NH4+1 shape

7. N2O2 name 8. HCN name

9. C2H2 name 10. C2H5OH

11. C2H3OH 12. C2N2 name

13. OH-1 14. CN-1

More Dot Structures

1. CF4 shape, name 2. CH2Cl2 shape

3. PF3 shape, name 4. H2S shape, name

5. F2 shape , name 6. N2H4 name

7. CH3COOH 8. CH3NH2

9. C3H4 name 10. CCl2O

11. CH3CN 12. P2H2 name

13. CS2 name 14. N2O2 name

15. C2H3O 16. SI2 name, shape

Ionic Compounds

There are four places to find the charge of an ion:

1. The main block elements

2. The Roman numerals

3. The polyatomic ion sheet

4. Determine the charge from the other ions in the compound.

All compounds have a net charge of zero.

How to Write Ionic Formulas

Ex: Determine the chemical formula for magnesium oxide.

1. Always write the cation first then the anion. To find the ionic charge look at your main block elements, the Roman numerals, and/or your polyatomic ion

sheet.

Mg+2 O -2

2.Write the compound using subscripts so that the net charge is equal to

ZERO MgO

Ex : Determine the chemical formula for ammonium carbonate 1. Always write the cation first then the anion. To find the ionic charge look at

your mainblock elements, the Roman numerals, and/or your polyatomic ion

sheet.

(NH4)+1 (CO3)-2

2.NEVER CHANGE THE POLYATOMIC ION.For multiple polyatomic ions use ( ).

The net charge of the compound must equal zero. (NH4)2CO3

How to Name Ionic Compounds. Ex: Write the chemical name for CaCl2

1. Write the cation first calcium

2. If the cation is a transition metal, tin(Sn), lead(Pb), animony(Sb), or

bismuth(Bi). Write the charge as a Roman numeral.

does not apply

3. Write the anion. If the ion is a nonmetal element change the ending to -ide.

calcium chloride

Ex: Write the chemical name for PbO

1. Write the cation first lead

2.If the cation is a transition metal, tin(Sn), lead(Pb), animony(Sb), or

bismuth(Bi). Write the charge as a Roman numeral.

lead(II)


lead(II) oxide

Ex: Write the chemical name for (NH4)2SO4

1. Write the cation first(taken form the polyatomic ion sheet) ammonium

2. If the cation is a transition metal, tin(Sn), or lead(Pb) Write the charge as a

Roman numeral.

does not apply


ammonium sulfate

ex: MgO magnesium oxide

Fe2(CO3)3 iron(III) carbonate

AuN gold(III)nitride

AgC2H3O2 silver acetate

NOTES:

Ionic Formula Writing 1. Al+3 Br-1 _____________ 21. lead(II) chloride ____________

2. Al+3 (C2H3O2)-1 ___________ 22. silver nitrate ____________

3. Ba+2 S-2 ______________ 23. mercury(II) iodide ___________

4. (NH4)+1 (NO3)-1 ___________ 24. strontium nitrite ___________

5. Ca+2 I-1 ______________ 25. barium sulfate ____________

6. Cr+3 F-1 _________ 26. tin(IV) sulfide ___________

7. (NH4)+1 (OH)-1 ________ 27. copper(II) chlorate _________

8. Cu+1 Cl-1 _________ 28. iron(II) oxide ___________

9. H+1 S-2__________ 29. lead(II) bromide ____________

10. K+1 (OH)-1 __________ 30. iron(III) phosphate __________

11. H+1 (CO3)-2 ____________ 31. lead(II) chromate ___________

12. Hg+1 (C2H3O2)-1 ____________ 32. magnesium fluoride __________

13. Cu+1 S-2 ______________ 33. hydrogen bromide ___________

14. Al+3 O-2 _____________ 34. magnesium sulfide __________

15. Sn+2 O-2 _______________ 35. lithium iodide ______________

16. Ag+1 Cl-1 _________ 36. silver carbonate __________

17. Ca+2 (PO4)-3 ____________ 37. zinc sulfite _____________

18. Ba+2 (Cr2O7)-2 ____________ 38. iron(II) chlorate ____________

19. Bi+3 (AsO4)-3 __________ 39. barium oxide _____________

20. Na+1 (ClO)-1 ____________ 40. ammonium phospate __________

Ionic Naming

1. CaCl2 ________________ 21. PbCl2 ________________

2. Al2O3 ________________ 22.Sr(NO3)2_______________

3. Na2S ________________ 23. AuI3 ________________

4. FeS ________________ 24. CuO ________________

5. NH4NO2 ________________ 25. HgBr ________________

6. Ba3N2 ________________ 26. BeSO4 ______________

7. AlF3 ________________ 27. Co3N ________________

8. Ca3P2 ________________ 28. AuI ________________

9. K2CO3 ________________ 29. W2O3 ________________

10. KI ________________ 30. Co(OH)2 ______________

11. Li2C2O4 ________________ 31. SnF4 ________________

12. SrBr2 ________________ 32. AgCl ________________

13. FeCl3 ________________ 33. CuO ________________

14. AgNO3 ________________ 34.Al2(CO3)3_______________

15. MgSO3 ________________ 35. Cu2O ________________

16. CdI2 ________________ 36. AlN ________________

17. BaSO4 ________________ 37. Pb(CO3)2 ______________

18. Fe2S3 ________________ 38. K3N ________________

19. SnO ________________ 39. Au3PO4 ______________

20. Be(C2H3O2)2 ________________ 40. NaCl ________________

Ionic Roman # & Polyatomics

Write the following compounds:

1. beryllium nitrate ___________________________________

2. manganese (II)iodide___________________________________

3. chromium (III) sulfide _________________________________

4. lithium chromate ________________________________

5. ammonium chloride _____________________________

6. copper (I) phosphide _________________________________

7. sodium phosphate _________________________________

8. iron (III) hydroxide___________________________________

9. zinc sulfite _________________________________

10. gold (II) acetate _________________________________

Name the following compounds:

1. FeCl2 ____________________________________

2. CrO ____________________________________

3. Mg(OH)2 ____________________________________

4. Ca(NO2)2 ____________________________________

5. NiBr2 ____________________________________

6. Cu2SO4 ____________________________________

7. HgCO3 ____________________________________

8. K2CO3 ____________________________________

9. (NH4)2O ____________________________________

10. SnI4 ____________________________________

Ionic Naming

Provide the formula for the following:

1. potassium phosphate ______________________ 6. Ca3N2___________

2. iron (III) chloride ______________________ 7. Li2SO4___________

3. mercury (I) oxide ______________________ 8. Ni(CN)2___________

4. aluminum carbonate ______________________ 9. SnF4 ___________

5. sodium chromate ______________________ 10. Sr(NO3)2_________

Each of the following name-formula pairs is incorrect. Determine what is wrong

with the pair, write a sentence explaining what is wrong, and then provide the

correct name or formula as needed.

11. PbCl2 – lead chloride

12. CuO – copper (I) oxide

13. Co3(PO4)2 – carbonate phosphate

14. CdI2 – cadmium (II) iodide

15. NH4NO2 – nitrogen tetrahydride mono nitrogen dioxide

16. copper (II) chlorate – Cu2ClO3

17. lithium iodide – LiIO3

18. barium oxide – BaO2

19. lead (III) sulfide – Pb2(SO4)2

20. hydrogen bromide – H2Br

Mixed Practice

Ionic vs. Covalent Compounds

Is the compound ionic or covalent? Name the following compounds:

1. CO _______________________ _______________________

2. BaI2 _______________________ _______________________

3. CrF3 _______________________ _______________________

4. CaCrO4 _______________________ _______________________

5. Cu(OH)2 _______________________ _______________________

6. N2O3 _______________________ _______________________

7. SrO _______________________ _______________________

8. NH4Br _______________________ _______________________

9. PF3 _______________________ _______________________

10. CoCl3 _______________________ _______________________

11. Al2O3 _______________________ _______________________

12. Mg(NO3)2______________________ _______________________

13. NaCl _______________________ _______________________

14. K2SO4 _______________________ _______________________

15. P2O3 _______________________ _______________________

Is the compound covalent or ionic? Write the correct formula.

1. aluminum chloride ________________ _______________________

2. calcium oxide ________________ _______________________

3. lithium hydroxide ________________ _______________________

4. diphosphorous tetraoxide __________ _______________________

5. cobalt (II) sulfate ________________ _______________________

6. ammonium iodide ________________ _______________________

7. sodium phosphate ________________ _______________________

8. iron (III) oxide ________________ _______________________

9. sulfur trioxide ________________ _______________________

10. nickel (II) acetate ________________ _______________________

11. carbon tetrachloride ______________ _______________________

12. potassium sulfide ________________ _______________________

13. dinitrogen pentoxide ______________ _______________________

14. magnesium nitride ________________ _______________________

15. barium phosphate ________________ _______________________

Mixed practice

Mixed Practice Writing and Naming Name the following compounds: Write the following formulas:

1. C2H6 ______________________________ 21. copper (II) nitrate ___________

2. CaBr2 ______________________________ 22. dinitrogen trioxide __________

3. LiMnO4 __________________________ 23. lead (IV) chloride ___________

4. H2O _________________________ 24. aluminum hydroxide ________

5. HF ____________________________________ 25. ammonium acetate __________

6. P4O10 _____________________________ 26. silicon disulfide _____________

7. Al2O3 __________________________ 27. sulfur dioxide ______________

8. Na2SO3 _____________________________ 28. copper (I) oxide _____________

9. BaO _______________________________ 29. diphosphorus pentasulfide _____

10. H3PO4 _______________________________ 30. carbon tetrafluoride __________

11. Na2O ________________________________ 31. zinc permanganate __________

12. Hg(OH)2 ____________________________ 32. tin (II) phosphate ___________

13. SO3 ________________________________ 33. iron (III) carbonate __________

14. NI3 ______________________________ 34. silver phosphide ____________

15. Cu2CO3 ______________________________ 35. silicon tetraiodide ___________

16. NO ___________________________ 36. strontium fluoride __________

17. P2S5 ____________________________ 37. cadmium hydroxide _________

18. Co3PO4 __________________________ 38. iron (III) chromate __________

19. CS2 ___________________________ 39. ammonium sulfide _________

20. SF2 ____________________________ 40. lithium oxide ___________

Electronegativity Values

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