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Academic Chemistry UNIT 4

NOMENCLATURE

Name:

Class Period: Test Date: Monday 10/27

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Chemistry Calendar

Nomenclature Test: Monday 10/27

Monday Tuesday Wednesday Thursday Friday

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Atomic Structure TEST

10 Bill Nye: Atoms and Molecules Intro: Element or Compound? Page 2

13 Student Holiday

14 Notes #1: Valence Electrons, Lewis Dot structures and Ions P. 4-5 HW: pg 6

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PSAT

16 Notes #2: Binary Ionic Chemical Names and Formulas Pg. 7-8 HW: pg 9

17 Notes #3: Binary Ionic Compounds with Transition Metals Pg. 10 HW: pg 11

20 Notes #4: Ionic Compounds with Polyatomic Ions Pg 12 HW: pg 13

21 Mixed Practice HW: Study Guide pg 19-20 Due Friday

22 Notes #5: Covalent Molecules and Acids Pg 14-15 HW: pg 16 AND Study Guide Page 19-20

23 Polyatomic Ion & Prefix Quiz Assessment:(pg. 17) ALL rules HW: Study Guide Page 19-20

24 Speed Dating Activity

REVIEW Check Study Guide

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Nomenclature

Test

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NOTES 1: Compounds and Their Formulas

Compounds have been defined as matter formed by two or more different elements joined by a

chemical bond.

Formulas allow scientists to identify the composition of compounds. Every formula contains the symbols

of elements that make up the compound. One example is NaCl, also known as table salt, is formed when

sodium (Na) and chlorine (Cl) combine in a chemical reaction.

Baking soda, or sodium bicarbonate, has a more complicated formula, NaHCO3. Baking soda is formed when

sodium (Na), hydrogen (H), carbon (C), and oxygen (O) combine in a chemical reaction. The small number 3

in the formula is called a subscript.

A subscript shows the number of atoms of an element in a compound. The subscript always refers to

the symbol just before it in the formula. If there is no subscript following a symbol, it means there is

only one of that kind of atom in the molecule.

Example: Baking soda thus contains, ____________ atom of sodium, _____ atom of hydrogen,

_____ atom of carbon, and ______ atoms of oxygen in each molecule.

A molecule is the term used for any bonded elements.

Identify the following substances: NaHCO3

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NOTES 2: VALENCE ELECTRONS, LEWIS DOT DIAGRAMS, AND

OXIDATION NUMBERS

Review:

1. How many total electrons are in a neutral atom of Sulfur?

2. How many electrons are in sulfur’s highest energy level (it’s most outer shell) (HINT: use the picture to the right)?

3. How many electrons does sulfur need to gain or lose in order to have 8 valence electrons (electrons in the outermost shell)?

RECAP: BOHR’S ATOMIC MODEL Bohr developed an atomic model in which the electrons are arranged in specific ________________ _______________________. The __________________________________ _ (n=1) is located closest to the nucleus. The highest level is located farther away from the nucleus. *The electrons in the highest (outer most) energy level for any element are known as _________________________ electrons.* *Valence electrons are electrons are involved in chemical bonding. VALENCE ELECTRONS can be easily found by looking at the _________________ ______________________ or “A” number located above the column where the element is located on the periodic table. Examples: Al = Group #_____ and ____ A so it has ____valence electrons. Pb= Group # _____ and ____A so it has ____ valence electrons. Practice: Determine the number of valence electrons for:

1. Phosphorus: ______ 2. Argon: _____ 3. Lead: ______ 4. Barium: _____

**This only works for GROUP A Elements. Another exception is Helium. Who only has ___ valence electrons.

Practice: Label the Valence Electrons for each Group A column on

the periodic table to the right.

The number next to

the A is the valence

Group #

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LEWIS DOT DIAGRAMS: is a diagram in which the chemical symbol of an element represents

the nucleus and the inner energy level and “dots” represent the valence electrons.

There can only be up to 8 valence electrons and thus only 8 dots around a symbol. The first 4 dots are

single and then they pair up as more are added. Octet rule states that all atoms wish to be like the

Nobel gases (group 18) with a full valence of 8 electrons.

How are the dots arranged? Treat the symbol as if it were a square, with 1 dot on each of the 4 sides

before pairing up.

element symbol

one dot for each valence electron

OXIDATION NUMBERS: is the number of electrons an atom gains, loses, or shares when it forms a

chemical bond and achieves the octet rule. This will also be the charge of the ION.

Metals as a rule lose electrons and will have a (+) charge.

Nonmetals will gain electrons and have a ( -) charge

Nobel gases in group 18 will not lose or gain and have a 0

charge

Label the periodic table at right for the ion charge created as

atoms achieve the Octet rule (full valence of 8):

Examples:

Name # Valence

Electrons

Lewis Dot

Diagram

How many electrons are

needed to have a complete

outer shell?

Oxidation number

(Ion charge)

Helium 2

Carbon

Fluorine

Needs to gain 1

Neon

0

X

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Homework:

Element

Name

# of

Valence

Electrons

Lewis Dot Diagram

How many electrons must be

added (- ion) Or

removed(+ ion) to have a

complete outer shell?

Oxidation

Number

(Ion charge)

cation

or

anion

Lithium

Xenon

Phosphorus

Sodium

Oxygen

Add 2 electrons

Hydrogen

1. Name 2 elements that have the same Lewis dot structure as oxygen:

____________________________ and ________________________________

2. How many valence electrons do elements in group 2A have? ___________

3. Besides hydrogen, which other element is an exception to the Octet rule?

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NOTES #2: Binary Ionic Chemical Names and Formulas Quick Review

___________ - atoms that have lost or gained one or more electrons. ________________ – positively charged ion _________________ – negatively charged ion The charge on the ion is known as the _________________________ _________________________ – ion consisting of two or more atoms

Practice - write the ion with the charge for the following elements

* Li * Ca * H

* Be * Si * K

* Al * S * O

* Na * Fr * N

* F * Cl * P

IONIC COMPOUNDS Ionic Compounds are made up of a

___________________+ ___________________ or ___________________ + ___________________

The bond involves the ____________________________ of electrons.

o The electron is transferred from the _______________ to the __________________ so that both atoms have a complete valence shell (usually 8 electrons in valance).

The overall charge of ionic compounds must equal _______________.

Naming Ionic Compounds First name the ____________ and then the ____________. (metal followed by nonmetal) Change the ending of the anion to ___________.

Example:

MgCl2 magnesium chloride

Li2S _________________________ Practice:

MgO ____________________________

K3P ____________________________

CsCl ____________________________

Ba3N2 ____________________________

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DRAWING Lewis Dot Structures for Ionic Compounds • The overall charge on the compound must equal zero, that is, the number of electrons lost by one atom

must equal the number of electrons gained by the other atom. • The Lewis Structure (electron dot diagram) of each ion is used to construct the Lewis Structure (electron

dot diagram) for the ionic compound.

The Lewis Dot structures show the location of the valence electrons after the electrons have been transferred. Examples: Lithium fluoride

• Lithium atom loses one electron to form the cation Li+

• Fluorine atom gains one electron to form the anion F-

• Lithium fluoride compound can be represented as

Draw the Lewis structure of Lithium oxide. What would be the chemical formula for this compound?

Writing Chemical Formulas When given two ions, __________________ the charges and make them the ___________________. Do NOT keep the +/- signs _______________ subscripts if possible

This means we must reduce the subscripts if they have a common denominator.

Example: Ca4F8

A. Using Balanced charges Method: B. Using the Crisscross method: **Sum of charges must equal zero. Example: Li+1 O-2

Ex: a. Na+1 + Cl-1 NaCl (+1 + -1 = 0) b. Mg+2 + O-2 MgO * (+2 + -2 = 0)

* Don’t write this Mg2O2 because it must be reduced.

Now, let’s use the name to write the chemical formula Name cation anion formula Lewis Dot Structure

Lithium oxide _______ _______ ____________________

Magnesium sulfide ______ _______ ____________________

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Your turn: HOMEWORK:

Write the chemical formulas from the ions.

1) Na+1 O-2 _______________

2) Ca+2 F-1 _______________

3) Al+3 Se-2 _______________

4) Mg+2 O-2 _______________

5) K+1 P-3 _______________

Write the chemical formulas from the name:

6) Sodium iodide cation: ______ anion:_______ Formula: ___________________

7) Strontium bromide cation: ______ anion:_______ Formula: ___________________

8) Aluminum oxide cation: ______ anion:_______ Formula: ___________________

9) Barium sulfide cation: ______ anion:_______ Formula: ___________________

Write the name from the formula:

10) NaCl ________________________________________

11) Mg3N2 ________________________________________

12) Na2S ________________________________________

Draw the Lewis Dot structure for numbers 1, 2 & 3 above:

#1) #2) #3)

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NOTES #3: Binary Ionic Compounds with Transition Metals(Cations)

Multivalent Cations are found in the group ______ elements (the middle of the periodic table).

These elements are also known as the ___ metals.

If your cation is a transition metal, then you must specify the charge with a _____________________ ____________________________.

Example: Iron (III) Sulfide Just like the compounds we looked at yesterday, the sum of charges must equal .

and we can still use the method when writing the chemical formula.

PRACTICE:

Chemical NAME Cation Anion Chemical FORMULA

1. Copper I sulfide

2. Manganese II oxide

3. Tin IV fluoride

4. PbI2

5. Fe2O3

6. PbO2

7. CoP

To figure out the charge of the transition metal, just “uncross the charges”.

EXCEPTIONS!!! These metals do NOT need a roman numeral.

o Zn+2

o Ag+1

o Cd+2

Roman

Numeral

Charge

I

II

III

IV

V

VI

VII

VIII

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HOMEWORK: Binary Ionic Compounds with Transition Metal Cations

Name the compound from just the formula.

To figure out the charge of the transition metal, just “uncross the charges”.

Chemical Formula Name

1. SnF2 ______________________________________________________

2. SnF4 ______________________________________________________

3. PbO2 ______________________________________________________

4. CuO ______________________________________________________

5. Cu2O ______________________________________________________

6. FeCl2 ______________________________________________________

7. Al2S3 ______________________________________________________

Write the chemical formula for the following compounds.

Chemical Name cation anion Chemical Formula

8. copper II chloride _______ _______ ___________________

9. zinc sulfide _______ _______ ___________________

10. tin IV bromide _______ _______ ___________________

11. mercury II iodide _______ _______ ___________________

12. copper II sulfide _______ _______ ___________________

13. nickel III sulfide _______ _______ ___________________

14. iron III oxide _______ _______ ___________________

15. titanium III phosphide _______ _______ ___________________

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NOTES #4: Ionic Compounds with Polyatomic Ions

Polyatomic ions are groups of atoms that behave as one unit.

They are treated like single ions in formulas, but use __________________________________________ when more than one is used in a formula.

NEVER change name or look of polyatomic. If you change the subscripts for any part of the polyatomic, then it is no longer that same polyatomic ion.

Otherwise….Use all the same rules for naming and writing compounds as with any other ionic compound.

PRACTICE:

Practice Formula Name

Al+3 CO3 -2 ____________ ________________________________

Ca+2 NO3 -1 ____________ ________________________________

K+1 ClO3 -1 ____________ ________________________________

Name the following compounds

Ba(OH)2 _____________________________

CaSO4 _____________________________

(NH4)3P _____________________________

Write the formula for the following compounds: cation anion formula

Strontium phosphate _________ __________ ________________________

Lithium acetate _________ __________ ________________________

Sodium sulfate _________ __________ ________________________

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Homework: Ionic Compounds with Polyatomic Ions Identify the polyatomic ion and its charge

Polyatomic Ion Formula of polyatomic ion Ion charge

Acetate

Hydroxide

Ammonium

Sulfate

Sulfite

Carbonate

Phosphate

Name the following compounds (Use Roman numerals and parenthesis as needed)

1. Cr(ClO3)3 ______________________________ 5. Fe3(PO4)2 ______________________________

2. ZnCO3 _______________________________ 6. LiNO2 _______________________________

3. NH4OH _______________________________ 7. Na2SO4 _______________________________

4. Pb(NO3)2 ______________________________ 8. Cu(NO3)2 _______________________________

Write the chemical formula

9. Silver hydroxide ___________________

10. Copper (II) nitrate ___________________

11. Chromium (IV) sulfate ___________________

Mixed-Up Practice ( Give the name or formula)

12. K2CO3 _______________________________________

13. Al2(SO4) 3 _______________________________________

14. FeP _______________________________________

15. Ammonium nitrate ___________________

16. titanium IV sulfide ___________________

17. Copper (II) hydroxide ___________________

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NOTES #6: Naming & Forming Covalent ( Molecular) Compounds

COVALENT (MOLECULAR) COMPOUNDS

Covalent compounds are made up of all ____________________ (also called molecular compounds). To name a covalent compound, name the first element, then name the second one and change its ending

to _______. Use ____________________ to show how many atoms of each element you have. Molecular compounds contain bonds and are formed when elements

________ valence electrons.

The rules for naming and writing covalent molecules are different than those for ionic compounds. NO crisscross NO reducing Prefixes are used in naming to show the number of each element

Prefixes (Memorize these!!!)

nonmetals except Nobel gases (group 18)

*

Examples: P2O5 diphosphorus pentoxide

CCl4 carbon tetrachloride

S2O3 _________________________________

NO2 _________________________________

CO _________________________________

*mono is omitted if on the first element

To write the formula of a covalent compound, simply translate the prefixes and element names.

dinitrogen dioxide ______________

diphosphorus heptoxide ______________

tetrasulfur tetranitride ______________

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ACIDS – special type of covalent compounds Compounds that form _____________ in water.

Formulas usually begin with ‘________’.

Examples: HCl- Hydrochloric acid H2SO4-Sulfuric acid

Compounds that usually begin with and have low pH are acids. Rules for naming and writing formulas are similar to those for ionic compounds with the following

exceptions:

ION TYPE ION

ENDING ACID NAME BEGINNING

ACID ENDING

Polyatomic -ite NO hydro- beginning -ous -ate NO hydro- beginning -ic

Monatomic -ide hydro- beginning -ic

HINT: ate-ic-ite-ous ide-ic PRACTICE:

Chemical NAME Hydrogen Nonmetal/Poly Chemical FORMULA

1) Hydrophosphoric acid H+

2) Perchloric acid

3) Dichromic acid

4) HCl

5) HNO2

6) HC2H3O2

7) H2S

8) H2SO4

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HOMEWORK: Naming & Forming Covalent / Molecular Compounds

Covalent compounds using Prefixes: **Do NOT reduce subscripts for covalent compounds **Be careful that you do NOT use prefixes for ionic compounds. Practice – Write the formula or the name for the following Molecular compounds.

1. Nitrogen trihydride ________________

2. Sulfur hexafluoride ________________

3. Dinitrogen pentoxide ________________

4. Nitrogen monoxide ________________

5. SiCl4 ___________________________________

6. C3H8 ___________________________________

7. OF2 ___________________________________

8. NBr3 ___________________________________

Naming and Writing formulas for acids Practice – Write the formula or the name for the following Acids

ION TYPE ION

ENDING ACID NAME BEGINNING

ACID ENDING

Polyatomic -ite NO hydro- beginning -ous -ate NO hydro- beginning -ic

Monatomic -ide hydro- beginning -ic

9. HCl ____________________________

10. H2S ____________________________

11. HClO3 ____________________________

12. H3PO3____________________________

13. H3P____________________________

14. Acetic acid____________________________

15. Sulfurous acid____________________________

16. Phosphoric acid____________________________

17. Nitric acid____________________________

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Assessment: Names and Formulas using ALL Rules

DIRECTIONS: For each of the following write the correct formula/name and state the type of bond that holds the elements together.

NAME FORMULA Ionic, Covalent, or Acid?

1. calcium carbonate

2. nickel II chlorate

3. zinc hydroxide

4. barium sulfate

5. hypochlorous acid

6. carbon tetrachloride

7. nitrogen monoxide

8. silver carbonate

9. mercury II chloride

10. disphosphorus pentoxide

11. copper I sulfate

12. copper II sulfate

13. nitric acid

14. ammonium chloride

15. H3PO3

16. Zn(NO3)2

17. NaC2H3O2

18. FeCl3

19. CuCl

20. P2O5

21. NH4Cl

22. AgBr

23. Sn(OH)4

24. H3P

25. PF5

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Academic Chemistry Nomenclature Study Guide

Nomenclature TEST on

1. Define the following: a. Octet Rule

b. Ionic Bond

c. Valence electron

d. Lewis Dot Structure

e. What’s a polyatomic ion

2. When Group 1A elements form ions, when they (transfer/share)_electrons.

3. Where are metals found on the periodic table?

4. Where are nonmetals found on the periodic table?

5. Do Nobel gases in group 18 form compounds?_____ Why or why not? (Hint: octet rule)

6. How many valence electrons are in an atom of nitrogen? ____ How many are in calcium?____

7. How does magnesium obey the octet rule when reacting to form compounds? (lose or gain or share electrons)

8. Covalent bonds (share/transfer) electrons between ________________ and ______________.

9. Ionic bonds (share/transfer) electrons between __________________ and ________________.

10. Cations have a (positive/negative) charge because they have (lost/gained) electrons.

11. Anions have a (positive/negative) charge because they have (lost/gained) electrons.

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12. Fill in the following chart with the correct information:

CHEMICAL NAME Ions (If applicable)

CHEMICAL FORMULA

TYPE OF BOND Ionic/Covalent

IF IONIC, DRAW LEWIS STRUCTURE

Lithium fluoride

Lead II oxide

Acetic acid

Sulfur hexafluoride

Trichlorine heptaoxide

Silver carbonate

Mercury I oxide

LiBr

Al2O3

NaNO2

HCl

HBrO3

HNO2

FeO

SnBr4

N2O5

NaOH

HBr

SCl2

HOH

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