Motivation THINK

Motivation

T – Is it True?

H – Is it Helpful?

I – Is it Inspiring?

N – Is it Necessary?

K – Is it Kind?

THINK

Do Now: Record and Answer the following questions in your notebook

1. Write down your definition of an ion.

2. What is the difference between an atom, an ion and an excited state atom. Use Calcium as an example and draw pictures.

Aim:?

*Puzzle: Solve the riddle .

“

Aim:?

Do Now: record and answer in your notes

1.Which element would most likely form an ionic bond with Potassium? Explain your reasoning.

a) Sodium b) Neon

c) Bromine

d) Calcium

Recall

• Ionic Bonds form because of a transfer of electrons between a metal and a nonmetal.

• Metals:

– lose valence electrons to form octet or duet – they become positive ions

• Nonmetals:

– gain valence electrons to form octet or duet

– they become negative ions

Show the transfer of electrons to figure out the formula of an ionic compound

Bromine

Magnesium

Show the transfer of electrons to figure out the formula of an ionic compound

Oxygen

Potassium

Show the transfer of electrons to figure out the formula of an ionic compound

Nitrogen

Calcium

Using the Criss-Cross Method, write the formula of the ionic compound

Potassium Oxygen

We need to know the charge of an ion

How do we find the charge on an ion?

We look at how many valence electrons the atom has or at the oxidation state on the periodic table. Non-metals see how many electrons need to form octet.

Group 1 metals +1 Charge Group 2 Metals +2 Charge Transition metals Vary

Group 15 (non-metals) -3 Charge

Group 16 (non-metals) -2 Charge

Group 17 (non-metals) -1 Charge

IN GENERAL USE THE TOP NUMBER CHARGES ONLY

FOR ELEMENTS IN GROUPS 1,2,13-18

CRISS- CROSS METHOD

Al Cl Na ₁ Cl ₃

AlCl ₃

LOOK UP THE CHARGES ON THE REFERENCE TABLE BRING DOWN THE NUMBER DIAGONALLY

KEEP ONLY THE NUMBERS, NOT THE CHARGES

REDUCE THE NUMBERS IF NECESSARY TO THE LOWEST RATIO

+3 -1

Using the Criss-Cross Method, write the formula of the ionic compound

Iodine Strontium

Using the Criss-Cross Method, write the formula of the ionic compound

Phosphorus

Calcium

Using the Criss-Cross Method, write the formula of the ionic compound

Sulfur

Barium

Try This One

• Show using the Criss-Cross Method, the

formula of the compound when a Barium ion reacts with an Selenium ion.

• Then verify this is correct by drawing the

Lewis Dot Structure and showing the electrons

being transferred.

Learning Check

Choose the correct formula for the compounds containing the following ions:

1. Na ⁺ , S ^2-

a) NaS b) Na ₂ S c) NaS ₂ 2. Al ³⁺ , Cl ^-

a) AlCl ₃ b) AlCl c) Al ₃ Cl 3. Mg ²⁺ , N ^3-

a) MgN b) Mg ₂ N ₃ c) Mg ₃ N ₂

Tips when working with Ionic formulas…

1. When writing the formula of an ionic compound, always write the positive ion first and negative ions second.

2. Write the symbols with subscripts so

that the over all compound is neutral.

Regents Practice

Regents Practice 2

Practice

Work on MP 2 Project Questions

Questions due Friday 22 ^nd Nov 2013

Exit Slip:

Please write and answer the aim.

Aim:?

Reflect on todays lesson and develop an aim that can be answered to summarize

the lesson.

Aim:?

Do Now: record and answer in your notes Identify the ionic compound formula

formed from an Aluminum ion and an Oxygen ion.

*Puzzle: Solve the riddle .

“Which element is definitely a male?”

Polyatomic Ions

Memorize these!!! Your next quiz WILL

contain them Where can we find

these on the regents reference

table?

Examples

• NaNO ₃

• Al ₂ (SO ₄ ) ₃

Polyatomic Ion

• A group of atoms covalently bonded together, that as a whole have a net (overall) charge

(either – or +).

• We treat the ion as if it were a single element, do not split it apart!

• The entire sulfate ion has a -2 charge

Writing formulas with Polyatomic Ions

Examples:

Calcium and Nitrate

Lithium and Phosphate

You must be able to recognize the name!

a) Ammonium and Chloride b) Sodium and Sulfate

c) Lead and Phosphate d) Sodium and Hydroxide

e) Magnesium and Carbonate

Writing formulas for compounds of

Learning Check

Write the correct formula for the compounds containing the following ions:

1. Na ⁺ , SO ₄ ^2-

a) NaSO ₄ b) Na ₂ S c) Na ₂ SO ₄ 2. Al ³⁺ , OH ^-

a) Al(OH) ₃ b) AlOH ₃ c) Al ₃ OH 3. Mg ²⁺ , NO ₃ ^-

a) Mg(NO ₃ ) ₂ b) Mg ₂ NO ₃ c) Mg ₃ N ₂ 4. Mg ²⁺ , NO ₃ ^-

a) MgNO ₃ b) Mg ₂ NO ₃ c) Mg(NO ₃ ) ₂

More Practice…on a separate sheet of paper

Write the formula for the compound that forms from the following:

1.Magnesium and peroxide 2.Lithium and carbonate 3.Barium and Fluoride

4.Sodium and Sulfide (Ion for Sulfur) 5.Lithium and Sulfate

6.Ammonium and Sulfite 7.Sodium and Nitrate

8.Lithium and Nitrite

9.Lithium and Nitride (Ion for Nitrogen) 10.Potassium and Hydroxide

11.Calcium and Hydroxide

12.Lithium and phosphate

Practice

MP 2 Project Questions

Exit Slip:

Please write and answer the aim.

Aim:?

Reflect on todays lesson and develop an aim that can be answered to summarize

the lesson.

Aim:?

Do Now: record and answer in your notes

*Puzzle: Solve the riddle .

“What do Oxygen and sodium say to each other when they argue?”

Write the formula for:

1. Hydroxide 2. Hydronium 3. Perchlorate 4. Nitride

5. Nitrate

6. Nitrite

1. Naming Simple Ionic Compounds

• Always write the full name of the metal first.

• Then name the nonmetal, but

changing the ending to –ide.

Naming Ionic Compounds

1. Cation (metal ion) = name of the element Ca ²⁺ = calcium ion

2. Anion (nonmetal) = root + -ide Cl ⁻¹ = chloride

3. Name the metal fully then the nonmetal CaCl ₂ = calcium chloride

Procedure and Sample (CaCl ₂ )

NOTE ***

• Name of an nonmetal element ion ends in “-ide”

Fluorine (F ^-1 ) Fluoride

Chlorine (Cl ^-1 ) Chloride Oxygen (O ^-2 ) Oxide

Sulfur (S ^-2 ) Sulfide

Nitrogen (N ^-3 ) Nitride

Bromine (Br ^-1 ) Bromide

Iodine (I ^-1 ) Iodide

Na ₃ N KBr Al ₂ O ₃ MgS Ba ₃ P ₂

Complete the names of the

following ionic compounds:

2. Naming Ionic Compounds containing polyatomics

• Always write the full name of the metal or positive polyatomic first exactly as is.

• Then name the negative

polyatomic exactly how it is

named on Table E.

• Look for 3 different elements at least

• Look at Table E to see if anything matches up

How can you tell if there is a polyatomic present?

Sc(OH) ₃ NH ₄ F CaCO ₃

Sr(C ₂ H ₃ O ₂ ) ₂

1. NaNO ₃ 2. Cs ₃ PO ₄ 3. K ₂ SO ₄

Name the following

• Ca(NO ₃ ) ₂

What about this one?

SOMETIMES YOU WILL SEE

PARENTHESES….

Look inside the

parentheses to find the

correct ion to name.

3. Naming Ionic Compounds containing transition metals

• Always write the full name of the metal with a roman numeral

• Then name the negative ion

using “ide” ending or polyatomic.

• Where are the transition metals located on the periodic table?

• Some transition metals have several (+) charges

Naming with Transition Metals

Transition Metal Naming

Cu Cl

Cu Cl

We use the equivalent roman numeral to distinguish between a transition

metals different oxidation states… lets

look at Cu as an example

Transition Metal Naming Rules

If a particular Transition Metal only has one possible positive charge, it is not necessary to write the roman numeral,

name it as you normally would.

Ag Cl

• Au ₂ O ₃

• FeCl ₂

• CuS

How would you name….

Do Now

1. P ₂ O ₅ a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide

2. Cl ₂ O ₇ a) dichlorine heptoxide b) dichlorine oxide

c) chlorine heptoxide

Naming Molecular Compounds

CH

methane BCl

boron trichloride

CO

Carbon dioxide

All are formed from two or more nonmetals.

Common Names

• A lot of chemicals have common names as well as the proper IUPAC name.

• Chemicals that should always be

named by common name and never named by the IUPAC method are:

– H ₂ O water, not dihydrogen monoxide

– NH ₃ ammonia, not nitrogen

trihydride

Molecular (Covalent) Nomenclature for two nonmetals

Prefix System (binary compounds) 1. Less electronegative atom comes first.

2. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is added on the second

element. Ex. CO (Carbon monoxide)

3. Change the ending of the second element to -ide.

PREFIX mono- di-

tri- tetra- penta- hexa- hepta- octa- nona- deca-

NUMBER 1

2 3 4 5 6 7 8 9 10

Molecular Nomenclature Prefixes

• CCl ₄

• N ₂ O

• SF ₆

• carbon tetrachloride

• dinitrogen monoxide

• sulfur hexafluoride

Molecular Nomenclature: Examples

• arsenic trichloride

• dinitrogen pentoxide

• tetraphosphorus decoxide

• AsCl ₃

• N ₂ O ₅

• P ₄ O ₁₀

More Molecular Examples

What type of bonds exists in compounds that contain

polyatomics? Why?

Choose 1 polyatomic and bond it to a transition metal,

write the formula name it

and answer the question

Exit Slip:

Please write and answer the aim.

Aim: What kind of bonds are in

compounds containing polyatomics and why?

Reflect on todays lesson and develop an aim that can be answered to summarize

the lesson.

Exit Slip:

Please write and answer the aim.

Aim: How do I write and name formulas of ionic and covalent compounds?

Reflect on todays lesson and develop an aim that can be answered to summarize

the lesson.

Rummi with Ions

•Dealer deals 5 cards to each player

•Place left over cards in center as the draw from pile

•Place one card in the center to play from

•Youngest player starts

•You HAVE to make a play! You cant win on your first hand

•Try to make 1 or more compounds with the cards in your hands by using ionic compound rules we have studied in class.

•The first person to use all the cards in their hand wins.

Write the compound you formed on the board.

•If you win, and have written the compound on the board

with the correct name you can get participation points

Do Now

Fill in the blanks to complete the following names of covalent compounds.

CO carbon ______oxide

CO ₂ carbon _______________

PCl ₃ phosphorus _______chloride CCl ₄ carbon ________chloride

N ₂ O _____nitrogen _____oxide

Demo with Salt an Sugar

I am going to place a teaspoon of sugar onto the hot plate at the same time I will place a teaspoon of salt onto the hot plate

Which one do you think is going to melt first?

Try to come up with a an

explanation for your answer.

Ionic Vs. Covalent

Properties of Ionic Compounds

1. Most are crystalline solids at room temperature

Properties of compounds that are bonded differently….

Ionic Compounds 1.Crystalline solids (made of ions) 2.High melting and boiling points

3.Conduct electricity when melted or dissolved

4.Many soluble in water but not in nonpolar liquid

Covalent Compounds 1.Gases, liquids, or solids (made of

molecules)

2.Low melting and boiling points

3.Poor electrical conductors in all phases 4.Many soluble in nonpolar liquids but not in

water

Exit Slip:

Please write and answer the aim.

Aim: What are the properties of

compounds that are bonded differently?

Reflect on todays lesson and develop an aim that can be answered to summarize

the lesson.

Properties of Ionic Compounds

2. Have High Melting Points and High Boiling Points 3. Very Hard

4. Ionic compounds can conduct an electric current when melted (molten) or dissolved in water

because their ions are free to move, but not in the solid state.

(electrolytes). Inside the beaker is

NaCl dissolved in water

Aim:?

Do Now: Record and answer in your notes

1. How many items do you use daily that are made of metals?

2. List any physical properties these items have

Metallic Bonds Introduction

• How metal atoms are held together in the solid.

• Metal atoms hold on to their valence electrons very weakly.

• Think of metal atoms as positive

ions (cations) floating in a sea of

electrons

Sea of Electrons

+ + + +

+ + + +

+ + + +

• Electrons are free to move through the solid.

• Metals conduct electricity.

Metal Atom

Electron

Metallic Bond

• Since these electrons can move from atom to atom, they are not held tightly, they are often called delocalized electrons.

A metallic bond is the attraction of a metallic

cation for delocalized electrons.

Metal Properties

• Metals are Malleable Hammered into shape (bend).

• Also ductile - drawn into wires.

• Both malleability and ductility

can be explained in terms of the

mobility of the valence electrons

1) Ductility 2) Malleability

Due to the mobility of the

valence electrons, metals have:

and

Notice

that the

ionic

crystal

breaks

due to ion

repulsion!

Malleable

+ + + +

+ + + +

+ + + +

Force

Malleable

+ + + +

+ + + +

+ + + +

• Mobile electrons allow atoms to slide by.

Force

ON THE OTHER HAND Ionic solids are brittle (weak, soft, easy to break)

+ - + - - + - + + - + -

- + - +

Force

Ionic solids are brittle

+ - + - - + - + + - + -

- + - +

• Strong Repulsion breaks a crystal apart, due to similar ions being next to each other.

Force

Chemical Bonds

• There are 3 forms of intramolecular bonding:

_________—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) forming oppositely charged ions that attract one another

_________—some valence electrons shared between atoms

_________ – holds atoms of a metal together

Exit Slip:

Please write and answer the aim.

Aim: What is a metallic bond?

Reflect on todays lesson and develop an aim that can be answered to summarize

the lesson.

Sodium Phosphide Cesium Chloride

Aluminum Selenide Strontium Oxide

Barium Nitride

Write the formulas of the

following ionic compounds

More Practice…

Write the formula for the compound that forms from the following:

1.Magnesium and peroxide 2.Lithium and carbonate 3.Barium and Fluoride

4.Sodium and Sulfide (Ion for Sulfur) 5.Lithium and Sulfate

6.Ammonium and Sulfite 7.Sodium and Nitrate

8.Lithium and Nitrite

9.Lithium and Nitride (Ion for Nitrogen) 10.Potassium and Hydroxide

11.Calcium and Hydroxide

12.Lithium and phosphate

• Matter, bonding, Formulas study guide

Practice

Practice

Orange book

p.33 Q 27 – 29 on a separate sheet of paper or on post its that you

stick into the book.

Regents Question

Bonding/Matter Test Data Analysis for 28 Students

Pass The Test

Fail The Test

Did not receive 100 on study guide

Bonding Test Prep Questions not submitted or incomplete

Got 100 on Test Prep and Study Guide

11 17

You might ask yourself, why so many students failed?

2 2

12

YES !!!!!

5 *Did these 5 students

pass the

test?

What should be on your study

guide?