Chem 103 Chapter 3 and 4 FA19 Suzanne Electron Config, Bonding, Naming, Lewis Dot, VSEPR

A. What is the full electron configuration and shell electrons for the following

elements?

a. Silicon

b. Pd

c. Cr

d. Barium

e. Bromine

f. W

B. Rules of Naming ions Cations

x Which groups/elements can become cations? What suffix do we use?

x Example: Anions

x Which groups/elements will gain electrons? Suffix we use?

x Example:

Use this space for the “staircase” model if it’s helpful for you.

Answer@1s22s22p63s23p42.Q6 1STp6

152252p63s23p64s23db4p65s24d8 §dd7o 4+14¢55 5p°5d" Sfm2,8 , 18,16 , 2 656 p6 led "*18252p63s23p64s23d4-48,13

,I

4s' 3ds ,

152252p63s23p64s2zd'04p65s24d"5p66s'

a' Y YALL I2,8, 18,18 , 8,2

152252p63s•3p6 45 3d '04ps

2,848,7

15252p63s23p64s23d'04p65s24d°5p66s24f'45d418

IT 4£52s w ¥

2,818,32, 13 , iµ÷hfj5d5

13 I

• Both main group and transition metalscan be cations

° We use -ion atthe end ,without changingthe

element's name

Nat , sodium ion

Kt y potassium ion

Nonmetals , we replace the ending of the elementwith - ide

S- 2-0 Sulfide ion G- → Chlorine ion

rosutfurw p Chlorineneutraafom neutral atom CCD

Chem 103 Chapter 3 and 4 FA19 Suzanne Electron Config, Bonding, Naming, Lewis Dot, VSEPR

Types of Chemical Bonds

Ionic Covalent Metallic

Elements Involved

Electron Distribution

Example

Rules of naming binary compounds: (Main Group) Ionic Compounds –

(Transition) Ionic Compounds –

Molecular (Covalent) Compounds – Rules of Drawing Lewis Dot Structure:

Prefixes for Molecular Compound one six

two seven three eight four nine

five ten

metal t nonmetal nonmetal t nonmetal metals( cation t anion) (Anion t Avion)

nonpolar .- equal sharingTransferred pooledPolar-- unequal sharing

LiBr, MGH , NaCl Hao , si Hui , HF copper Wine

no prefixes and no Roman Numerals

• Cation t Anion - ide Example:k At:3 = Kzs

↳ Metals (cations) from group 1,2 ,or 13

↳ Nonmetals(Anions) from group15-17

= Potassium sulfide

✓

use Roman numerals for charge

• Cation- Roman Numeral t Anion - ide Example :charge Fe ,} I -0 Fez 03

2 8

Locations from 3- 12= Iron (HD Oxide

↳ Anions from15-17

Use prefixesmono - hexa -

Prefix - First Element t prefix - Second Element- ide

• use prefixes to indicate thenumber of di - hepta -

atoms of each type inthe molecule

tri - Octa -

• Do not use mono - with the first elementin

the nametetra- nona-

Example: No, = Nitrogen dioxide penta- deca-

-Pyoio = Tetraphosphorus Decaoxide

° Find the total number of valence electrons (ve;)Example: Methane = CH4 Example: Sfa = Sulfur Hexafluoride

E : : : 7:44 .¥: : : : :c:• Put the least electronegative atom inthe center.-

is

o Hydrogen always goes outside. Total Veii 8 Least electronegative

¥:::t:*:::::÷::i::c:*. / . ::¥÷÷÷÷÷÷÷÷ / ."move neurons vom outer atoms t.c.tt '

÷:to form double or triple bonds .% T.gg:p dear

"

H

Chem 103 Chapter 3 and 4 FA19 Suzanne Electron Config, Bonding, Naming, Lewis Dot, VSEPR

Chem 103 Polyatomic Ion – Fill in the missing formulas or names of the polyatomic ions. Pg. 115

Charge Name Formula

+1 Ammonium ion

H O

HCO

Hydrogen sulfate (bisulfate) ion

-1 CH COO or CH CO

Nitrite ion

Nitrate ion

CN

OH

H PO

Permanganate ion

-2 Carbonate

SO

Chromate ion

HPO

C O

Dichromate ion

-3 PO

N Hyt '

Hydronium

Hydrogen carbonate (bicarbonate)

H Sou-

Acetate ion

Noa-

N03-

Cyanide ion

Hydroxide ion

Dihydrogen phosphate ion

Mh04- I

0032-

Sulfate ibn

Croy2-

Hydrogen phosphate ion

Oxalate ionCr 207-2

Phosphate

Chem 103 Chapter 3 and 4 FA19 Suzanne Electron Config, Bonding, Naming, Lewis Dot, VSEPR

1. Draw the Lewis dot structure of the following compounds, determine whether compounds are ionic, polar or non-polar. Also, provide the name or the formula of the compound. How do we know if a compound is polar of nonpolar?

F H O

CHCl SiH

SF Nitrate Ion BF Xenon Hexafluoride Copper (II) Chloride BrF NaCl Hydrogen Fluoride ICl CH

- Difluoride ( Diatomic fluorine - water ID,' hydrogen Monoxide

7×2 - Nws : one. ! : Hel 02=2 tompaifmspoounadkpeolar↳ nonpolar 0=601 - 6 H - O - H

covalent ⑦

Polar covalent

- Chloroform" ti :

- siliconTetrahydrideµ

ftp.makingitpolar414703) ↳ polwauraient I- : ¥+01, ↳ polar - Si - H= 21+44 If I

= 26 ve's l H

i. Cl :- (

- sulfur tetrafluoride Nitrate has 3resonance

=%¥;" ↳ polar covalent No;↳ nonpolar #re= 34ms

←maims.es#aa-eir ¥'m't' f : "I :-.

:i÷÷s÷i÷ : unequal sun's

:# Iii

- Boron Trifluoride:# ⇒ ↳ nonpolar ÷ :

''et. ↳ man Fdn!=24ue's : - B

.

. 8+17.6,I

a. F := 5.One's

✓ d

- Bromine PentafluorideChaz Etta .si ↳ polar

, ;

if.gg?onePoFtespoeoamrMmd"

+z

- '= 42ms I

.

.

↳ ionic :&! - cu-÷ : F - Br - F11

i. f :'I :

O O

"Every

electronegativeSodium chloride HF -- polar aebalent Hat

makingit polar

↳ ionic. .- i Itt - suis

ti

Na .- Cl :• O

- Iodine tetrachloride

I -I ol = 7

"-704--2*2, :c:÷÷÷÷÷÷÷÷÷i÷I. arbontetranaride8ve-s H - C - H

to t't↳ Polar covalent Nonpolar

covalent

Chem 103 Chapter 3 and 4 FA19 Suzanne Electron Config, Bonding, Naming, Lewis Dot, VSEPR

II. Name compounds: BF

C H

ClO

Al O

NaCl

Ir(CN)

Al (SO )

CrO

SF

ICl

Pt(OH)

III. Give molecular or ionic formula:

Arsenic Trihydride

Diphosphorus Hexabromide

Xenon Hexafluoride

Tetraphosphorus Heptachloride

Hydrogen Nitrite (Nitrous Acid)

Iron (III) Iodide Hexahydrate

Palladium (IV) Carbonate

Magnesium Hydroxide

Titanium (II) Bromide

Cobalt (II) Sulfite

Barium Hydroxide

Strontium Phosphate

Sulfuric Acid

Dichromate

Perchlorate

Gold (I) Sulfate

IV. VSEPR Theory

x Explain what the VSEPR theory is. What does it stand for? What we use it for? Why it’s important?

ASH3Boron Trifluoride

P2 Brie

Tetracarbon Decahydride Xe Fee

Pyclg

AN02Chlorine Dioxide

Fetz • 6h20

Pd 3)aAluminum Oxide

Mg@A)aSodium Chloride

Ti Bra

Co 80gIridium 114) cyanide

Ba (OHL

Aluminum Sulfate Srg (Po4) 2

Chromium HD Oxide H soy

Sulfur Hexafluoride Cr207- 2

Iodine Penta chloride cloy- t

Au 2804Platinum 147 Hydroxide

valence- Shell Electron Pair Repulsion theoryto predicts the arrangement of atoms

about central atom in a molecule

to give molecules 3D shapes° important to see that electron sets arrange

themselves as

far away from each other to reduce repulsion

Chem 103 Chapter 3 and 4 FA19 Suzanne Electron Config, Bonding, Naming, Lewis Dot, VSEPR

x List the steps you can take to determine the shape of a molecule:

1. 2. 3. 4. 5.

Fill in the boxes that are empty. Should be in page 123 in your book.

Number of Bonded Atoms

Number of Lone Pairs

Number of Electron Sets

Molecular Shape

Give Example Ball-and-Stick Models (Draw

it) 2 0

Linear

3 3

4 0 4 Tetrahedral

4 Trigonal Pyramidal

2 2 H O

3 Bent

Draw a lewis formula in which a shared electron pair (bonding pair) isindicated bya line . Use dots to show any unsharedpairs I lone pairs of electrons .

To determine shape , count thenumber of electron sets around the

central

atom . Recall that multiple bond counts only as oneelectron set.

Draw a shape as if all the sets were bonding pairs and placethese

electron sets as far as possible .

temp:: Tere:uebiaeemaieinsiidghgasehgroeafnngmpmg satay saaggeegwiene.mewee . It there are

The presence of lone pairs of electrons onthe central atom decreasesthe angles

between the bonds,as cone pairs require more space

than bonding pairs ofelectrons

2 Bella

O Trigonal BF3Planar

CH4

3 I POIz

4 Bent

2 ISO 2