Chem Do Now• Hand me all assignments you are submitting• Gather all your materials• Find your name on the seating chart on the

board up front and move your seat.• By the time the timer is up, you should be

seated with your notes pages out.• Anyone not in their assigned seat at the time

of the buzzer must go get a late pass.• Talk to me AFTER CLASS if you have an issue,

I WILL NOT move you today during class.

Ions

Nuclear Charge• In the nucleus there are protons and

neutrons– Protons are positive– Neutrons are neutral

• If the nucleus has 3 protons it has a charge of 3+

Neutral AtomIn a neutral atom, there are

equal numbers of protons and electrons

Each positive is cancelled

by a negative.

Ions• In an ion, there are unequal numbers

of protons and electrons

3 + charge4 – charge1 – charge

Ions• In an ion, there are unequal numbers

of protons and electrons

3 + charge2 – charge1 + charge

What is the charge of an ion that has 12 protons and 13 electrons?

What is the charge of an ion that has 54 protons and 52 electrons?

What is the charge of an ion that has 29 protons and 32 electrons?

What is the charge of a SR ion that loses two electrons?

What is the charge of a Fluorine atom that gains one electron?

What is the charge of an Oxygen ion that gains two electrons?

Now for some practice• Complete the back page of your

notes by your self.• When the timer is up, partner up and

share your answers.• Work together to make sure you and

your partner agree on every answer.• We will go over this as a class

POGIL: Ion Formation• Complete the Ion formation activity

with your group members• Hand in your sheet when completed• If you finish early you may work on

your homework until time is up.

Chemical Bonding

Electron Review• The electron configuration shows the location

of all of the electrons in an atom• Valence electrons are the electrons in the

outer most shell• Valence electrons are represented in Lewis Dot

Structures• The charge of a particular atom can be found

by subtracting the number of electrons (given by the electron configuration) from the number of protons (given by the atomic number)

2-8-8-1

Noble Gas Configuration• Elements will gain

or lose electrons to obtain a noble gas configuration (full outer shell).

• Metals tend to lose electrons

• Nonmetals tend to gain electrons

Current Electron Configuration

After losing an electron

Nobel gas configuration2-8-8

e-

Energetically Stable• By achieving the noble gas

configuration, the atom becomes more energetically stable (reaches a lower energy state).

Gaining or Losing Electrons•When an electron is gained or lost, it isn’t being pulled out of air or released into space. • Electrons are always taken from or given to other atoms.

Bonding• When electrons are transferred,

shared or pooled between atoms, a bond is formed.

• A bond represents increased stability between two atoms.

Spectrum of BondingThere are many different types of bonding.

Electron Transferred

Electron Shared

Electron Attracted

Ionic Bonding

CovalentBonding

IntermolecularBonding

MetallicBonding

Types of Bonding• Ionic Bonding: when electrons are

transferred between atoms (Metal and Nonmetal)

• Metallic Bonding: when electrons are pooled among atoms (all Metal)

• Covalent Bonding: when electrons are shared between two atoms (all Nonmetals)

• Intermolecular bonding: When an atom is attracted to electrons in another molecule (between covalent molecules)

Ions Quick Facts• When do ions gain or lose?

- 1, 2, or 3 valence electrons will lose those electrons - 5, 6, or 7 valence electrons will gain electrons

• Always want to get to a full outer level (usual 8 electrons)

• To find overall charge:– 1. Add the number of protons– 2. Add the number of electrons when in balanced state– 3. Add/sub the number of electrons changing by (lose =

subtract; gain = add).– Remember: electrons are NEGATIVE– Answer should be: -3, -2, -1, 0, +1, +2, +3. Rarely will you

have a charge grater than 3.

Ions Con’t• To write the notation of an ion:

1. write the element symbol2. in the upper right corner write

the chargePractice: Li F O• Atoms that gain electrons are cations• Atoms that lose electrons are anions

Ionic Bonding• In ionic bonding, the electron is

completely transferred from one atom to another.

• Both atoms become charged ions.

Na Cl+ -

Ionic Bonding

MgCl+

-

Cl-2

Positive ions will lose all electrons. Negative ions will gain until they have 8.If need be, an atom will give away electrons to many different atoms

PracticeDraw Lewis Dot diagrams for each

of the following atomic pair and show electrons transferred.

Na and FAl and ClNa and O

Do Now: Update TOC1. Ion Formation2. POGIL: Ion Formation3. Atoms and Ions HW4. Chemical Bonding5. Chemical bonding

con’t6. Ionic Bonds Activity7. Ionic Bonding

Worksheet8. Naming Ionic

Compounds Notes

9. POGIL: Naming Ionic Compounds

9-a POGIL Con’t10. Ionic Bonding Practice11. Writing Ionic Compounds Guided Practice12. Bond with a classmate13. Chemical Bonding

Ionic Formulas• Formulas represent the

number of ions that are involved in bonding.• In the formula MgCl2, one

magnesium atom is ionically bonded with two atoms of chlorine. • In the formula NaCl, one

sodium atom is ionically bonded with one atom of chlorine.

Formula WritingWhen writing formulas for ionic

systems, always write the cation (positively charged ion) first.

MgCl2 Cl2Mg

Writing Ionic Compound Formulas• Find the two

elements (metal and Non-metal) on the periodic table.

• Write their oxidation numbers above.

• Criss Cross • Reduce

B F3+ 1-

BF3

Boron Fluoride

Nature of ionic Bonds• Charged atoms

are attracted to opposite charges much like magnets are.

• However, nothing more is holding the atoms together.

+

-

Formula Units• Since no ion is

specifically bonded with another ion, we cannot refer to ionic compounds as molecules.

• Instead, we refer to ionic compounds as formula units (the ratio of cations to anions in the solid).

Bonding Basics Activity• One group member come get a

“white board”• One group member get a marker• One group member get counters• Take out the Bonding Basics Sheet• Wait for further instructions

Completing the chart

Completing the Ionic BondsStep 1- Write the Element Symbols on white boardsStep 2- Add counters to create Lewis StructuresStep 3- Move the electron to complete the shellStep 3- Draw a model like the one to the right on your paper that represents what you did on the white boardStep 4- Write the notation for each ionStep 5- Write the equation for the new compound made by the ionic bond

Naming Ionic Compounds

Chloride

Binary Compounds• For ionic compounds consisting

of two types of atoms…

NaClThe cation is given

the element

name

The anion is given the element

name ending in -

ideSodiumChlorine

Common Anions• Sulfur = Sulfide• Oxygen =

Oxide• Phosphorus =

Phosphide• Nitrogen =

Nitride• Fluorine =

Fluoride• Chlorine =

Chloride• Carbon =

Carbide• Arsenic =

Arsenide• Sellenium =

Selenide• Bromine =

Bromide• Iodine = Iodide

What is the name for NaP?

1. Sodium Phosphorus

2.Sodium Phosphide

3.Sodide Phosphide

4.Sodide Phosphorus

What is the name for MgO?

1. Magnesium Oxygen

2.Magenide Oxide

3.Oxygen Magnenide

4.Magnesium Oxide

Polyatomic Ions• Some ions are composed of multiple

atoms covalently bonded together• These groups of ions are called

polyatomic ions[OH]-Hydroxide

Polyatomic Ions

What is the formula for Sodium Hydrogen Carbonate?

1.NaHC2.Na2HCO3

3.NaHCO3

4.NaHCO2

Ions with multiple charge states• Some elements have

multiple charge states possible.

• To designate the charge of these ions in the formula name, we use roman numerals.

Roman Numerals

•1 = I•2 = II•3 = III

•4 = IV•5 = V•6 = VI

Examples Consider the following name:

Copper (II) Chloride

Cu Cl

Consider the following name: Chromium (VI) Oxide

Cr O

Practice

What is the formula for Iron (II) Oxide?

1.Fe2O2.FeO3.FeO2

4.Fe2O2

What is the formula for Vanadium (V) Bromide

1.VBr3

2.V3Br3.VBr5

4.V5Br

Writing Ionic Compounds

Be O2+ 2-

BeO

Beryllium Oxide

SIMPLIFY

Writing Ionic Compounds

Na PO41+ 3-

Na3PO4

Sodium Phosphate

Writing Ionic Compounds

Fe CN2+ 1-

Fe(CN)2

Iron (II) Cyanide

What is the formula for Potassium Hydroxide

1.KH3O2.KH3.KO4.KOH

What is the formula for Dimercury (I) Fluoride

1.HgF2.Hg2F3.HgF2

4.Hg2F2

Do Now- •What is an ionic bond? State 2 key aspects.•When do we use roman numerals?•Why do atoms form bonds?•Why can’t we have negative numbers after criss-crossing?

Covalent

Bonding

http://www.chemistrydaily.com/chemistry/Double_bond

Shared ElectronsCovalent bonds are about sharing electrons.

*Also called molecular bonds*

Shared Electrons• Atoms share electrons to

have access to electrons to achieve a noble gas configuration.

• Neither atom wants to lose its electrons.

• They engage in a “tug of war” over the electrons.

F

He-

Drawing Bonds• When two electrons are shared between

two atoms, this bond is represented as a line.

FHe-

e-

e-e-e-

e-e-

e-Hydrogen wants to gain 1Fluorine wants to gain 1

Non-bonding Electrons

FH

Electrons not involved in bonding are referred

to as Lone Pairs of Electrons

Drawing Covalent Molecules• Drawing covalent molecules are

a bit more complicated than ionic formula units.

• Atoms are now bonded to specific atoms within the system.

• We can represent these bonded systems through Lewis Dot Diagrams.

Lewis Dot Diagrams

O OFirst, draw the valence electrons

Second, connect the single electrons

Lewis Dot Diagram

O OThird, put bonds directly between atoms

Lewis Dot Diagram

NCl

ClCl

Lewis Dot Diagram

CO ClH

Independent Practice• Draw Lewis Dot diagrams and bonds

for the following molecules.

CH4NF3 H2O CO2

Do Now-Update TOC14. SH1015. Ionic Bonding Overview16. Review Naming Ionic Compounds17. Covalent Bonds Notes18.Venn-Diagram and Vocab19.Bonding Basics- Covalent Bonds20.Bonding Basics Packet21.Molecular Geometry22.Covalent Bonding Practice

Homework Check

Molecular Geometry

Electron Repulsion• When we draw structural

formulas using Lewis Dot diagrams, we can’t always see the exact angles of the bonds.

• However, what we know is that the electrons want to be as spaced out around the center atom as much as possible.

CO

Cl

H

Geometries In order for the electrons to

get as far apart as possible, the

atom’s orbitals adopt a geometry that

minimizes their interaction

But how do you know?By drawing Lewis Dot

Diagrams, you can predict

the geometry of a molecule.

CTetrahedral

Molecular GeometryThere are four basic

geometries.

Linear

Pyramidal

Tetrahedral

Bent

Example with Oxygen

O Bent

Example with Chlorine

ClLinear

Check your work on the geometry notes page

Bond Energy

Bond Energy• Each level of electrons have energy• Levels closer to the nucleus have less

energy than the levels further away• When atoms form bonds, the atoms

become more energetically stable. • The energy required to make or this

bond is referred to as the Bond Energy.

Bonds and Energy• By forming this

bond, the atoms become more energetically stable.

• Energy is released. • The atoms get

their “stable 8” configuration and can relax.2Mg + O2 2MgO

Bonds and Energy• When a bond is broken,

energy is absorbed.• The energy required to

break this bond is referred to as the Bond Energy.

• When atoms are separated, they lose their “stable 8” electrons.

• The potential energy of each atom is decreased.

http://durangotexas.blogspot.com/2010/06/crowley-texas-school-bunsen-burner-gas.html

H Cl

Do Now- Use your notes if need be. Remember to check to see if these are

ionic or covalent!• Write the name of the following:1. NH3

2. FeSO4

3. CoBr2

• Write the formula for the following:1. Vanadium (V) Oxide2. Aluminum hydroxide3. Silver Phosphate

Polarity

Molecular Geometries and Sharing Electrons

• In a covalent bond, two atoms are sharing electrons. • Just like in the real world, they don’t

always share equally. • Electronegativity: The attraction that

an atom has for electrons in a bond• Electrons spend more time with the

greater electronegative atom

Consider Hydrogen Fluoride (HF)

H FWhat is the electronegativity of

each atom? Check Table S in your NYS Reference Tables

2.1 4.0e-e- δ-δ+

Polar Bonds• Where one atom has a higher

electronegativity than the other, there is an unequal sharing of electrons.

• The unequal sharing of electrons in a covalent bond will result in the formation of a polar bond.

• Polar bonds have partial positive (δ+) and partial negative (δ-) charges.

Is the bond between Carbon and Hydrogen polar?

Is the bond between Hydrogen and Hydrogen polar?

Is the bond between Hydrogen and Tellurium polar?

Which bond is more polar, N-H or C-H?

Which bond is more polar, O-N or H-O

Practice• Let’s consider….

Si – O δ-δ+

Intermolecular Forces

Polar Molecules• Within a molecule, each bond can be

polar or nonpolar.

CH

H

H

H

Molecular Polarity• The net polarity of a molecule is

dependent upon the orientation of the polar bonds.

CH

H

H

H

In the case of CH4, each bond is polar. Because methane has a tetrahedral geometry, each polar bond cancels out the adjacent bond.

Non-polar MoleculesWhere all polar bonds cancel

out, the molecule is considered

non-polar.

CH

H

H

H

Polar Molecules

Where the polar bonds don’t cancel

each other out, the molecule

becomes polar.

N HHH

δ-

δ+δ+

δ+

Consider…H2S

δ-

δ+δ+

Consider…CO2

Non-Polar

How does a bond’s polarity impact a molecule and its

behavior?

H

HOSi

δ+

δ+

δ-

Intermolecular Forces

Intermolecular ForcesThe presence of partial positive

and partial negative

charges allow for the

interaction of molecules.

δ-δ+

Intermolecular ForcesThe partial positive and

negative charges are called dipoles.

Molecules with dipoles can experience dipole-dipole

attractions.

Dipole-Dipole Interactions In solution, these molecules will orient themselves so that the

positive dipole is near the negative dipole of another molecule.

Hydrogen BondingWithin dipole-dipole

interactions there is a subset of stronger

interactions called hydrogen bonds.

Intermolecular bonds between hydrogen and F, O,

N, Cl.

What about Non-polar molecules?

H

H

H

H

Van der Waals/London Dispersion Forces

The molecule is surrounded by the electron cloud.

+-

--

Molecules can now be attracted to one another temporarily

Van der Waals/London Dispersion ForcesJust like a real cloud, the electron cloud moves around the molecule.

Van der Waals Forces• What would increase the

strength of Van der Waals forces?–The size of the electron cloud–The size of the molecule–The composition of the molecule

Boiling Point and Van der Waals Forces

C5H12 C6H14 C7H16

C8H18

What type of intermolecular forces best describes NH3?

1. Dipole-Dipole Interactions

2. Van der Waals Forces

3. Covalent Bonds4. Ionic Bonds

What type of intermolecular forces best describes CH3CH3?

1. Dipole-Dipole Interactions

2. Van der Waals Forces

3. Covalent Bonds4. Ionic Bonds

What type of intermolecular forces best describes PCl3?

1. Dipole-Dipole Interactions

2. Van der Waals Forces

3. Covalent Bonds4. Ionic Bonds

What type of intermolecular forces best describes CH3OH?

1. Dipole-Dipole Interactions

2. Van der Waals Forces

3. Covalent Bonds4. Ionic Bonds

Hydrogen

Hydrogen BondingBecause the polarity of bonds

between hydrogen and F, O, N, (Cl) is so great, the attraction between these dipoles is more intense.

Hydrogen Bonding and Boiling Point

The Special Nature of Water• The difference between water as a

bent structure and water as a linear structure is the difference between life and death on the planet.

What we know about water…

• It has a bent geometry. • It is a polar molecule. • It experiences dipole-dipole/hydrogen bonding.

Giver of Life• The human body is approximately 60% water. • If water didn’t hydrogen bond, what would be the consequences for life?

Modern Marvels: Water

Start at 15:23

Crystal Structure of Water• Because of hydrogen bonding, the

water molecules arrange into a specific geometry.

Crystal Structure of Water

• The orientation of water molecules in a solid form take up more space than the liquid form.

• Solid is less dense.

Thus, ice floats.

Walking on WaterThe ability for

water molecules to hold

together, seemingly

forming a skin is referred to as

surface tension.

Surface Tension The molecules on

the surface of water feel the pull back into the liquid and

the pull of their neighbors, creating

a “skin” on the water.

How would life be different?• If water was non-polar…–Grab a large whiteboard, make a

poster that describes how life would be different if water was a linear, non-polar molecule. –These are predictions based on

what you know and what you see in the Modern Marvels' video