AcademicChemistry UNIT 6

MENCLATURE

-I"I. NNilrogÿn

Name:

Class Period: Test Date:

Chemistry Calendar

9

Bill Nye: Atoms andMolecules pg 3Intro: Element orCompound?Page 4

10

Notes #2: ValenceElectrons, Lewis

Dot structures

and IonsP. 5-6

HW: pg 7

11Notes #3: Binary Ioni(Chemical Names andFormulas Pg. 8-9

HW: pg 10

quiz!!

Test

HW: StudyGuide pg 18-19DUETHURSDAY!

Nomenclat2ÿ

17

Notes #5: CovalentMoleculesPg 16

HW: pg 17 ANDStudy GuidePage 18-19

24

Dimensional")Analysis

Poster

16

Mixed Practice PG 15

18

Ionic and CovalentBonding Activity

HW: StudyGuide Page 18-19

25

12

Notes #3: BinaryIonic Compoundswith TransitionMetals Pg. 11

HW: pg 12

19

REVIEWCheck Study Guide

Activity

NO SCHC

26

OL THANKSGIVING

13Notes #4: IonicCompoundswith PolyatomicIons Pg 13

HW: pg 14

2O

DLA!

27

l IREAK!

Nomenclature Test:It

Monday ÿ/27

Bill Nye- Atolns Name:

.

The middJe of the atom is called the

The two particles in the nucleus areandVÿ ÿ/ÿ'ÿfÿ 6

5ÿ

6ÿ

4ÿ

3ÿ The heaviest part of the atom is the

The particles which have a positive charge are

The particleswhich have no charge are Hÿ4ÿ"ÿ'ÿ

The particles which have a negative charge are (ÿ}ÿVlÿ

7. Atoms are mostly

8ÿ

9.

i0.

1.1.

12.

The basic building blocks of aH matter are

Atoms are like letters and molecules are like

All matter is made of ÿlÿqÿ/ÿlÿ and ÿZÿ Vÿq DDL)ÿ

Atoms combine to form C,OÿOOIVÿ4,ÿ / Vvll#t e,04)ÿ-ÿ2ÿ

Water can be broken down by passing an electric, current through it.

produced by the break diown of water?What two gasses are

13, What does the atomic number tell you?

p fGv

14.

1S.

What is the chemical name for:HzO --> NaCI --> CÿHsNsOÿ -->

oms are tOÿ small to be seen, How do scientist study atoms and the particles which make upatoms?

16. Everything in the un, iverse is either or

NOTES 1: Compounds and Their Formulas

Compounds have been defined as matter formed by two or more different elements joined by achemical bond.

Formulas allow scientists to identify the composition of compounds. Every formula contains the symbolsof elements that make up the compound. One example is NaCI, also known as table salt, is formed whensodium (Na) and chlorine (CI) combine in a chemical reaction.Baking soda, or sodium bicarbonate, has a more complicated formulaÿNaHCOÿ Baking soda is formed when

sodium (Na), hydrogen (H), carbon (C), and oxygen (O) combine in a cÿeaction. The small number 3in the formula is called a subscript.A subscript shows the number of atoms of an element in a compound. The subscript always refers tothe symbol just before it in the formula. If there is no subscript following a symbol, it means there isonly one of that kind of atom in the molecule.

Example: Baking soda thus conÿins, 1 atom of sodium,__l atom of hydrogen,____ll atom of carbon, and ÿ atoms of oxygen in each molecule.

A molecule iS the term used for any bonded elements.

Identify the following substances:NaHCO3

Complete ÿ,e chart by first idenI:ifÿ,ing each of ffhe substaaÿc.ea by name. 'Then desÿibe each.substance by placfÿg a check in the appropriate box.

Name Element Compound

C

G o14

CO

AI

ALl

COÿ

Hÿ

,/Symbol:

Jd

/

,1

/,/

,//

MoleculeAtom

/

/

Oÿ

H

4

NOTES 2: VALENCE ELECTRONS, LEWIS DOT DIAGRAMS, ANDOXIDATION NUMBERS

Review:

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

2. How many electrons are in sulfur'ÿ]ÿghest energy leveJj(it's mostouter shell) (HINT: use the picture to the right)? ---ÿ

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

RECAP: BOHR'S ATOMIC MODELBohfÿ.ÿDed an atomic model in which the electrons are arranged in specific ÿ-'i/ÿtFÿ /

The 10ÿ ÿ _0,ÿ/ÿ. 7 ÿ;ÿ/i (n=l) is located closest to the nucleus. The highestlevel is located farther away from the nucleus.* The electrons in the highest (outer most) energy level for any element are known as

tl Ol t ce,, electrons.**Valence electrons are electrons are involved in chemical bonding.

VALENCE ELECTRONS can be easily found by looking at the Iÿ FUÿ/[ÿ i#iÿ bÿf or"A" number located above the column ÿhere the element is located on

the periodic table.

Examples: If)Ai-- Group # and

electrons.

Pb= Group #ÿand __electrons.

Asoit has ÿ valence

f Asoit has Lÿ valence

[ Group #

The number next tothe A is the valence

**This only works for GROUP A Elements. /3Another exception is Helium. Who only has o/ÿ valence electrons.

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

the periodic table to the right.

Determine the number of valence electrons for:

1. Phosphoÿs:

2. Argon: _ÿ

3. Lead:

4. Barium: _ÿ

I!

PerlodlQ TaMÿ o! Ille [htmentl

' "1 '1"1'1'1 '1' I I'!'"1 1'"1

IIII

Practice:

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

00ÿIj ......... one dot for each valence electron

I

OXIDATION NUMBERS: is the number oj: 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 ÿ/ÿlfÿ ÿ ÿ-vÿ

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

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

It- Metals and Nonmetals

, a IMETALS

0

Examples:

Name

\

Helium

Carbon

#Valence

Electrons

2

Neon

Lewis Dot

Diagram

°

O

F°o o#

u#

How many electrons are

needed to have a complete

outer shell?

0

Needs to gain 1

0

(Ion charge)

0

0

Fluorine

6

Homework:

Element

Name

# ofValence

Electrons

.#,

Lewis Dot Diagram

Phosphorus

t

Sodium

Oxygen

Hydrogen

Xenon

I

Ib

Lithium

"CI..Q,

0

lqCb°o

0°000

How many

electrons must be

added (- ion)Or

removed(+ ion)to have a

complete outershell?

Add 2 electrons

Oxidation

Number

(Ion charge)

0

+1

cation

or

anion

J

,

,

3.

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

How many valence electrons do elements in group 2A have? ¢ÿL

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

7

NOTES #3: Binary Ionic Chemical Names and Formulas

Quick Review• ÿ-ÿ ÿ - atoms that have lost or gained one or more electrons•

• Cÿ!)ÿ ÿVÿv - positively charged ionV%ÿ - negat,vely charged non •• ÿ 1' ' • ÿ

• Thÿakrÿe on the ion is known as the 0ÿ !ÿ/ÿ'ÿ/ÿ [/ÿjÿ/ÿlÿ/ÿ• ÿ* !ÿ'ÿ'ÿIGÿ lgJÿ'ÿ - ion consisting of two or more atoms

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

I"ONI"C COMPOUNb$• Ioÿc CQmpÿunds are made up, of a ,,

"ÿ1

8 in + ÿlÿaÿor

Metals and Nonmetals

• The boÿ/ÿvÿof electrons.

o The electron is transferred from the')1ÿ f/ÿ to the ÿ Vÿ (ÿ i

so that both atoms have a complete valenceshell (usually 8 electrons in valance).

• The overall charge of ionic compounds must equal :

(o).Naming Ionic Compounds (ÿ'ÿt/ (-VÿC/Vÿ 'Vÿ ÿ'ÿ I

• First namethe ÿÿ and then th.e ÿlÿVÿ• Change the ending of the anion to ,4 14 ÿ

W

Example:

• MgCI2 magnesium chloride

• Li2S LH'hlÿfÿ ÿ'ÿ1ÿÿ

• (metal followed by nonmetal)

Na• •

Practice:• MgO

• KÿP

• CsCI

• Ba3N2

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 theelectrons 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

[bi] + r:ÿ':]- i

...................................... .......

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

Writing Chemical Formulas• When given two ions, /ÿt1ÿ/'1ÿ/ÿ the charges and make them the \ÿÿ/ÿ?ÿ2.• DQNOÿkeeRthe+/-siÿns• gÿ) ÿ./ subscripts if possible

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

Example: Ca4Fs--)

A. Using Balanced charges Method:• **Sum ofcharges must equal zero.

B. Using the Crisÿross method:Example: Li÷1 02

Ex:a. Na+1 + C1-1 -) NaCI (+1+-1= O)

b. Mg+2+ 0-2-)MgO* (+2+-2=0)

* Don't write this Mg202 because it must be reduced.

Now, let's use the name to write the chemical formulaName cation anion

• Lithium oxide LJ_ÿ

formula Lewis Dot Structure

Li,o gij,+Ei :,

Magnesium sulfide

Your turn: HOMEWORK:

Write the chemical formulas from the ions.

=ÿ N%ÿ 02/ Ca÷2 F-1 /ÿ, #ÿ

31 A'÷3 Se-2 ÿ1ÿ ÿ

Chÿ

,,(ÿ, .4- Z.

0

Write the chemical formulas from the name:

6) cation: ÿJÿLÿÿ'ÿ anion: .ÿ

7) cation: ÿ=ÿ anion:__ÿ

8) cation: .ÿa nion:ÿ__ÿI.

9) cation: ÿ ?'ÿanion: .Sÿ'ÿ

Sodium iodide

Strontium bromide

Aluminum oxide

Barium sulfide

Formula:

Formula:

Formula:

Formula:

Write the name from the formula:

10) NaCl 50ÿiI Iljm Cÿ'ÿ ! 0 ifÿ 4-1ÿ

=ÿ =a== ,,!o!IIÿ 5vll&

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

#1) #2) ÿ

oo

'ÿ -77

L-0 0 ÿJ

10

NOTES #4: Binary Ionic Compounds with Transition Metals(Cations)

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

kt. @l@ l [ @@[@@@@ÿlo4g]ÿJÿjÿ

These elements are also known as the %ÿ Iÿihil'ÿ metals.If your cation is a transition metal, then you mÿst speciE/the charge with a.ÿ0ÿqL4ÿq mum ÿ4/_ÿ .

Example: Iron (110 Sulfide

RomanNumeral

I

II

III

IV

V

VI

VII

VIII

Charge

+14-7-

# q-

4 q+f¢

Just like the compounds we looked at yeÿ_fÿaÿ_;ÿhe sum of charges must equaland still the /xJlfÿ ÿ'ÿwe can use ÿ-zÿ, I <," method when writing the chemical

formula.

PRACTICE:

Chemical NAME

1. Copperl sulfide

2. Manganese II oxide

3. Tin IV fluoride

6.

Cation

gn 4+

Anion

0ÿ

Chemical FORMULA

Cu 5

Pblÿ

Fe203

.

• To figure out the charge of the transition metal, just "uncross the charges .

PbOÿ

CoP

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

0 Zn+2 0 Cd+2

o Ag+ÿ

11

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

2. SnF4 ÿ'Iÿfÿ (ÿ) -"'ÿlÿOÿJ['/&

FIuoÿ'IHÿ

Write the chemical formula for the following compounds.

Chemical Name cation anion

8. copper Ilchloride ÿ ÿ

9. zinc sulfide ÿiÿf Sÿ-

10. tin IV bromide ÿ/ÿ ÿt-ÿ- lÿr I-

211. mercury II iodide

12. copper II sulfide ÿ2ÿf Sÿ.-

13. nickel III sulfide ÿI ÿ'ÿ" g ÿ-

rÿ* 0ÿ-14. iron III oxide

.ÿ .itanium.,,..o..hi.e 7ÿ 3ÿ P 3-

Chemical Formula

kJ "

I,P12

NOTES #5: Ionic Compounds with Polyatomic Ions

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

c##2, %coo ....

NHÿ"

CO23-

Acetate

Ammonium

Carbonate

Chlorate

Chlorite

Chromate

Cyanide

Dichromate

aoÿ7

aoÿ 77

CrO2-

CN" ÿiii

%oÿ,- i',

Hydrogen carbonate HCOÿ"

Hydroxide OH-

Hypochlorite CIO-

Nitrate NO7

Nitrite NO2

Perch Iorate CI 04

Permanganate MnOÿ

Phosphate POÿ-

Su Ifate SO2-

Sulfite SO21

• They are treated like single ions in formulas, butuse Pÿlllf'ÿ/il'+ÿiÿl-ÿ ( )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 ioniccompound.

PRACTICE:

Practice

AI+3

Ca+2

K+I

Formula Name

CIO3' ÿ' ÿiIt0 ÿ Po-l-4#lUÿ CA Io<f6

Name the following compÿfl L)

• Ba(OH,2 ÿ "t"ÿOI Iÿ14-g• CaS04 ÿlclum <..CO I,.P--4P6• (NH4).P tÿ'ÿFilf'lq0V!!0ÿ(Vÿ Phoÿ-pÿi4&,

Write the formula for the following compounds:

Strontium phosphate

• Lithium acetate

• Sodium sulfate

cation anion

Li* &&4-+ <7ou. z- rd z,5oq-

13

Homework:Identif the polyatomic ion and its charge

Polyatomic IonAcetate

Hydroxide

Ammonium

Sulfate

Sulfite

Carbonate

Phosphate

Ionic Compounds with Polyatomic Ions

Formula of polyatomic ion

OI

SOÿv

poi

Ion charge

[4

+?/

Zÿ5-

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

1. Cr(CIOÿ)3

2. ZnC03

3. NH40H

4. Pb(NOÿ)2

.ÿÿ.o.ÿ @c4ÿxÿ4ÿ6. LiNO2

7. Na2SO4

8. Cu(NO3)2

Write the chemical formula

9. Silver hydroxide .

10. Copper (II) nitrate _

Or uÿ ,,704ÿ11. Chromium (IV) sulfate

Mixed-Up Practice ( Give the name or formula)

16.

17.

ra ÿ (qTiT) P'TI oÿbll <'JlsT,'0-nitraTEÿ Nÿ ÿx]Oÿ

12. K2C03

13. AI2(SO4) 3

14. FeP

15. Ammonium

titanium IV sulfide

Co pCÿe rÿ(lÿl)hydrÿgxide

]4

MIXED PRACTICE

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

,

2.

3.

4.

5.

6.

7.

8.

9.

i0.

11.

12.

13.

14.

15.

NAMEcalcium carbonate

nickel II chlorate

zinc hydroxide

barium sulfate

mercury II chloride

silver carbonate

copper I sulfate

ammonium chloride

Zn(N03)2

NaC2H302

FeCI3

CuCI

N H4CI

AgBr

Sn(OH)4

15

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

COVALENT (MOLECULAR) COMPOUNDS i i• Covalent compounds are made up of all ÿ0ÿ1ÿ ('ÿ (also called molecular compounds).• To name a covalent compound, name the first element, then name the second one and change its ending

toÿ. Use ÿ-[1'ÿ ÿ,ÿo ÿ ,ÿ ÿo slÿow how many atoms of each element you have.

• M olecularcompoundscontain (ÿ(ÿ,;ÿ ÿ'ÿt" bonds and are formed when elements .• ÿ-ÿ/ÿ ÿI ÿI'ÿ 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 theseH !)

nÿbeÿPre&x

indicated

133.OI10- 1

di- 2

tri- 3

tetra- 4

penta- 5

hexa- 6

hepta- 7

oc, ta- 8

I1Onÿ- 9

deca- t 0

A

g

.ÿetals exceptNobel gases(group 18)

P20sExamples:

diphosphorus pentoxide

CCIÿ

SÿOÿ

NOÿ

CO

carbon tetrachloride

s 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

16

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.

Nitrogen trihydride

Sulfur hexafluoride

Dinitrogen pentoxide

Nitrogen monoxide

carbon tetrachloride

nitrogen monoxide

disphosphorus pentoxide

NBr3

OH8

OF2

P205

PFs

SiCl4

17

Academic Chemistry Nomenclature Study GuideNomenclature TEST on

1. Define the following:a. Octet Rule

,

c. Valence electron -- ÿ ÿ ÿ) Cÿ/ÿ/ÿ/ÿ ÿ/ÿ ,ÿ ÿ ÿ L)ÿ'ÿ,,Y WVÿ ÿ,Cf ÿv'ÿ'ÿ ÿ,/

i v?dd. Lewis Dot Structure ÿ-ÿ'ÿVÿiiÿ, A/,}ÿ -ÿ ÿ/ÿt,/ÿ'ÿ'x7ÿ/ÿL" ÿJltÿ/'ÿ'//gÿ C'ÿIÿÿQÿ

e. What's a poIÿomtc ion

When Group 1A elements form ions, when they ÿshare) electrons.

3. Where are metals found on the periodic table?

4. Where are nonmeÿms Touncl on the perioaic ÿable.

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

6. How many valence electrons are in an atom of nitrogen? ÿ 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 ÿtransfer> electrons between ÿ!ÿ/ÿmÿiand m[ÿ'ÿQÿV3,ÿIÿI

9. Ionic bonds (shaÿ electrons between Vÿ ÿ-ÿ, \ and ÿ ÿ)ÿ 'I/ÿ #ÿ.f-ÿ i

10. Cations haven ÿ/negative)charge because they haveÿosÿ#ÿained)electrons.----'ÿ they have (Iost/6electrons.

11. Anions have a (positive/ÿeÿcharge because

18

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

t

..So4ÿ

Pl30ÿ5u

CHEMICAL NAME

Lithium fluoride

Lead II oxide

Sulfur hexafluoride

Trichlorine heptaoxide

Silveÿrr ca rboÿnnatÿe in/]

Mercury I oxide

Ions(If applicable)

Li 'ÿ Fiÿpbÿ Oz-

<ÿr rF'l Zo

L!L) z-

A.I ÿiO ÿ---

Faroÿ°

( I ÿ;t,s2,' I/II

m4oÿÿ ulff-,//////

0 0 ,

70 r:-o/L €,o __1

CHEMICALFORMULA

LiBr

Li F

0m R ÿYÿ.t-6

o1ÿ0,7

HOH

NAN02

FeO

SnBr4

N20s

NaOH

SCI2

TYPE OF BONDIonic/Covalent

;ÿql cCÿvaiD'ÿOowatÿq-

17641uCÿv'41ÿf

7ÿot,,l t cÿ

7>'mtc,

oÿfliu%ÿt0

IF IONIC, DRAW LEWISSTRUCTURE

L"+ÿ,ÿ}-I-I f2ÿ,ÿ

Li %r;I i

19

i .............

E

o,,0

o E

IN

w

........ 'ÿ ........ ÿ ÿii ...........................

.:t

Z ÿ ÿ , ÿ.iÿ-' ÿ .n

g

rÿ

_

,-I

- ÿ

,,,,,i,. • ,,,,,,,, , ,,, , ,

........ ,,.,,,, ....

,iÿ ÿ_ ÿo.

oa

ca

1ÿ ÿ ÿ ÿ "t:ÿ "

Z

kÿ U

Z

,ÿ'

2 ..... .,,÷,

o

20

x" h'.¸ .i

o,oooÿou, !

uÿ.J

' .g g .r

ggNÿ

EEEÿ

N ÿ N N N ÿ

8u8ÿ

U

o i: 8

I i

U uÿ

21