Gifted Chemistry – Week 13

Monday Chrome Book Activity

TuesdayStudent Presentations: Covalent Bonds; Notes & Guided Practice: Covalent Nomenclature

Wednesday

Lab: Naming Covalent Molecules

Thursday

Quiz: Ionic & Covalent Formulas & Nomenclature;Notes: Lewis Dot Structures for Covalent Molecules

Friday Begin Test Review (Test on Tuesday)Two Quia due on Sunday at 11:59 pmWeek 13: 8-1 and 8-2 & Week 13: Mixed Review

Most Missed Quia – Week 12

Write the formula for the ionic compound created fromaluminum and carbonate

Al2(CO3)3

Most Missed Quia – Week 12

Write the formula for the ionic compound created fromcalcium and chlorate

Ca(ClO3)2

Most Missed Quia – Week 12

Name this compound: Be(ClO2)2

Beryllium DichloriteBeryllium(II) Chlorideberyllium(II) chlorite

beryllium chlorite

Ionic Bonds

• Transferring electrons from one atom to another in order to complete an octet of valence electrons

• Groups 1 and 2 lose electrons…become positive cations

• Chalogens and Halogens gain electrons…become negative anions

• Metal + nonmetal salt• Metal + oxygen oxide

Ionic Bonds

• Formula Writing– Balance charges– Use parentheses, when necessary

Calcium hydroxide Lithium iodate

Ca(OH)2 LiIO3

Ionic Bonds

• Formula Writing– Balance charges– Use parentheses, when necessary

Ammonium sulfate potassium carbonate

(NH4)2SO4 K2CO3

Ionic Bonds – Which one is correct?

(Ca) OH2

(NH4)3PO4

(Fe+2)2(PO3)3

Ca (OH)2

NH12PO4

(Fe+2)3(PO3)2

Ionic Bonds

• Compound Naming– Cations first; anions second– Use roman numerals for transition

metals

Fe(NO2)3

Sn(CO3)2

iron (III) nitrite

tin (IV) carbonate

Properties of Ionic Compounds

• Ionic bonds produce unique physical structures

• Atoms are highly organized with consistent spacing and a uniform pattern

• Crystal lattice – a 3D arrangement of particles

Properties of Ionic Compounds

1. ConductivityIonic solids do not conduct electricity.Melted ionic solids or ionic solids dissolved in a solution will conduct electricity (electrolytes).

Properties of Ionic Compounds

2. High melting points and high boiling points.Ionic bonds are very strong and require a lot of energy to break apart.

Ionic Bonds and Energy

Formation of ionic bonds is always exothermic.

Lattice energy – energy required to separate the ions in an ionic compound

Smaller ions have greater lattice energies.Larger charges also have greater lattice energies.

1

Naming Covalently Bonded Molecules

A binary covalent compound is composed of two different nonmetal elements. There are four rules on naming these molecules.

Rule 1. The element with the lower group number

is written first in the name; the element with the higher group number is written second in the name.

Exception: when the compound contains oxygen and a halogen, the name of the halogen is the first word in the name.

Rule 2. If both elements are in the same group, the element with the higher period number is written first in the name.

Rule 3. The second element in the name is named as if it were an anion, i.e., by adding the suffix -ide to the name of the element.

Naming Covalently Bonded Molecules

Rule 4. Greek prefixes are used to indicate the number of atoms of each nonmetal element in the chemical formula for the compound.

Naming Covalently Bonded Molecules

Prefix Meaning Prefix Meaning

Mono- 1 Hexa- 6

di- 2 Hepta- 7

tri- 3 Octa- 8

Tetra- 4 Nona- 9

Penta- 5 Deca- 10

Practice:

1) SbCl3

2) S2Cl2

3) BF3

4) P4O6

5) Se4S10

Naming Covalently Bonded Molecules

6) phosphorus trichloride7) selenium tetrafluoride8) carbon tetrabromide9) sulfur trioxide10) tetraphosphorus

hexaoxide

Covalent Bond Review

Covalent bond – chemical bond that occurs when valence electrons are shared, not transferred

Molecule – product of a covalent bond

Usually occurs between nonmetals and elements that are close to each other on the periodic table

Covalent Bond Nomenclature Lab

Use your device to download a free dice rolling app

11 Undeca12 Dodeca

Lewis Dot Structure

CH4

Lewis Dot Structure

NH3

1) chlorine monoxide

2) oxygen difluoride

3) boron monophosphide

4) dinitrogen monoxide

5) nitrogen trifluoride

6) sulfur tetrachloride

7) xenon trioxide

8) carbon dioxide

9) diphosphorous pentoxide

Diatomic Molecules

Two atoms of the same element share electrons in order to form a stable molecule

Seven naturally occurring diatomic moleculesH2 O2 F2 Br2 I2 N2 Cl2

“Hof Brincl”

Diatomic Molecules

Diatomic Molecules

More stable than single H atoms due to

full shell

Diatomic Molecules

• When only one pair of electrons is shared, it is a single covalent bond.

Single Bonds

• Draw the Lewis Dot Structure for WaterH2O

Single Bonds

• Draw the Lewis Dot Structure for AmmoniaNH3

Single Bonds

• Draw the Lewis Dot Structure for MethaneCH4

Single Bonds

• Draw the Lewis Dot Structure for MethaneCH4

Double Bonds

Double Bonds

• Draw the Lewis Dot Structure for carbon dioxide CO2

Triple Bonds

Triple Bonds

• Draw the Lewis Dot Structure for acetylene C2H2

Qu

iz R

evie

w:

D

ot

an

d M

ixed

Nom

en

cla

ture

Qu

iz R

evie

w:

D

ot

an

d M

ixed

Nom

en

cla

ture

Qu

iz R

evie

w:

D

ot

an

d M

ixed

Nom

en

cla

ture

Kahoot.it

You must enter your real name

Scores will be part of your classwork grade for today.