Outline of Topics 1. Atomic Radius 2. Electronegativity 3. Ionization Energy 4. Ions 5. Ionic Compounds 6. Covalent Compounds 7. Lewis Structures

Outline of Topics

1.Atomic Radius2.Electronegativity3.Ionization Energy4.Ions5.Ionic Compounds6.Covalent Compounds7.Lewis Structures

Trendy Table

OBJECTIVE: Learn 3 patterns of the Periodic Table

Trendy Table

3 trends/patterns in the PT

1.Atomic Radius2.Ionization Energy3.Electronegativity

Trendy Table

Atomic Radius

Ionization Energy

Electronegativity

Definition

Period INCREASES INCREASES INCREASES

Row INCREASES INCREASES INCREASES

1. Atomic Radius

1st Trend - Atomic Radius

What is it?Size of Atom

1. Atomic Radius

1st Trend - Atomic Radius

As you go down a group, the number of electrons…

So as you go down a group, the size of the atom…

1. Atomic Radius

1s1

1s22s1

1s22s22p63s1

1s22s22p63s23p64s1

1s22s22p63s23p64s23d104p65s1

1s22s22p63s23p64s23d104p65s24d105p66s1

1. Atomic Radius

What do you notice going across periods?

1. Atomic Radius

Atomic Radii – Size of Atom

So, as you go down a period, atomic radius ______.

As you go across a period…wait

WHY?

1. Atomic Radius

1s1 1s2

1s22s1 1s22s2 1s22s22p21s22s22p1

1s22s22p63s1 1s22s22p63s2 1s22s22p63s23p1

1. Atomic Radius

Atomic Radii – Size of AtomNuclear Charge

1. Atomic Radius

NO ENERGY LEVEL added across periods

1. Atomic RadiusAtomic Radius – Size of Atom

1. Atomic Radius

3 Patterns1. Atomic Radius

2. Electronegativity3. Ionization Energy

Atomic Radius

Electronegativity Ionization Energy



1. Trendy Table

Periodic TrendsAtomic Radii – Size of Atom

1. Trendy Table

Periodic TrendsAtomic Radii – Size of Atom

1. Atomic RadiusSummary & Review

1. What is atomic radius?2. What happens to radius going down AND

WHY?3. What happens to radius across from left to

right and WHY?4. Which have smallest and largest radius?5. Arrange by radius from

smallest to largest carbon, cesium, copper, helium, iron, potassium

2. Electronegativity

2nd Trend: Electronegativity

What is this?

electronegativity = wanting/attracting electrons



related to atomic radius

smaller the radius,higher the electronegativityhigher electro = really want/good @

attract e-




Atomic Radius




2. ELECTRONEGATIVITY



2rd Trend: Electronegativity



Fluorine has highest electronegativity

Francium has lowest electronegativity

Noble Gases do not count – why?




2. ElectronegativitySummary & Review

1. What is electronegativity?

2. Which group is on the 0 of the y-axis?

3. Which element has highest electronegativity, and which has lowest?

4. Arrange from lowest to greatest electronegativity

oxygen, cesium, sulfur, potassium, zinc, fluorine

3. Ionization Energy

3rd Trend: Ionization Energy

What is this?energy

needed to remove/steal

an electron from an atom


3nd Trend: Ionization Energy

What is this?Energy needed to remove an electron from

an atom

OPPOSITE of

ATOMIC RADIUS



2. Electronegativity3. Ionization Energy

Atomic Radius






3. Trendy Table

How to tell the difference between the two?

NOBLE GASES do not care about

Electronegativity



Periodic Trends3 Patterns

1. Atomic Radius – size of atom2. Ionization Energy – energy to remove electrons

3. Electronegativity – ability to attract electrons

Atomic Radius

Ionization Energy

Electronegativity

Period INCREASESSmallest: HeLargest: Cs

INCREASESWeakest: Cs

Strongest: He

INCREASESWeakest: CsStrongest: F

Row INCREASESSmallest: HeLargest: Cs

INCREASESWeakest: Cs

Strongest: He

INCREASESWeakest: CsStrongest: F

3. Trendy Table


Summary & Review1. What is ionization energy?

2. What are the relationships between atomic radius, electronegativity, and ionization energy?

3. Arrange from lowest to greatest ionization energy

copper, neon, silicon, cesium, helium,phosphorus, calcium, fluorine,

3. Trendy Table

Periodic Trends3nd Trend: Ionization Energy

What is this?

Energy needed to remove an electron from an atom

A filled orbital is a happy and stable orbitalAll elements want to be NOBLE

4. IONS

5 + - 2 = 5 + - 3 =5 + - 4 = 5 + - 6 =

4. IONS

OBJECTIVE: When atoms give away electrons

4. IONS

ION

What is it?An atom that

LOST/GAINEDelectron(s)

4. IONS

How do we know if an atom GAINS or LOSES electrons?

and

How MANY electrons is it going to gain or lose?

4. IONS

Goal is to get to the NEAREST Noble Gas

RULES

1. If you go LEFT, you become POSITIVE.

2. If you go RIGHT, you become NEGATIVE

4. IONS

Ions that LOSE electrons have a

POSTIVE charge

called

cations

pronounced “cat – ions”

4. IONS

All metals become

CATIONS

4. IONS

Transition Metals do not care about being NOBLEThey have their own thing going one.

DO NOT HAVE TO MEMORIZE…kind of

4. IONS

Ions that GAINS electrons have a NEGATIVE

charge

called

anions

pronounced “an – ions”

4. IONS

Ions with at NEGATIVE charge

called

anions

pronounced “an – ions”

4. IONS

Helium

Neon

Argon

Krypton

1. Write the electron configuration for the following elements2. UNDERLINE valence electrons

The S orbital can hold how many electrons MAX?

TWO

The P orbital can hold how many electrons MAX?

SIX

Noble Gases do not become ions because their orbitals are FILLED

THEY have all the VALENCE ELECTRONS THEY NEED

4. IONS

Helium

1s2

Neon

[He]2s22p6

Argon

[Ne]3s23p6

Krypton

[Ar]4s23d104p6

Xenon

[Kr]5s24d105p6

Alkali and Alkali Earth Metals want to be nobleby having the SAME electron configuration as

the nearest noble gas

Non-Metals want to be nobleby having the SAME electron configuration as

the nearest noble gas

4. IONS

So far we learned how a “normal” atom becomes an ion

Li Li+ + 1electronMg Mg2+ + 2electrons

N + 3electrons N3-

O + 2electrons O2-

F + electron F-

4. IONS

Ex: CN-

NH4+

CO32-

Because these ions are made from two or more atoms, they are called

polyatomic ions

Some ions are made from two or more atoms

4. IONS

Because these ions are made from two or more atoms, they are called

polyatomic ions

-ite has less oxygenthan –ate

Memorize? Kind of

4. IONSSummary & Review1. What is an ion?

2. What are the two types of ions?

3. Metals form these types of ions, and non-metals form these types of ions.

4. Why do Noble Gases not become ions?

5. Predict the charge of each atom if it were to become an ion:

Ca, Cl, Cu, F, Fe, Li, Na, N, O

5. Ionic Compounds

4x + -16 = 02x + -8 = 0

3x + -12 = 0

2 + -x = 010 + -2x = 012 + -3x = 0

5. Ionic Compounds

OBJECTIVE: Joining Cations + Anions to make compounds

5. Ionic Compounds

Na+ + Cl- NaCl cation anion ionic compound

forumula

NaCl joined byIONIC BOND

IONIC BOND = giving away/gaining electrons

5. Ionic Compounds

Li+ + Cl-

K+ + Cl-

Ca2+ + Cl-

Li+ + O2-

Ca2+ + O2-

LiCl

KCl

CaCl2

Li2O

CaOCharges must cancel and = 0

1. Separate into cations and anions

2. Separate into Alkali, Alkali Earth, Halogens, Transition Metals, and Polyatomic Ions

3. Make the following compounds

5. Ionic Compounds

H+ + Cl-

Na+ + Cl-

Mg2+ + Cl-

Mg2+ + SO42-

Mg2+ + SO32-

Fe2+ + Cr2O72-

NH4+ + Cl-

Fe2+ + O2-

Na+ + O2-

Na+ + OH-

Fe3+ + OH-

NH4+ + SO4

2-

5. Ionic Compounds

Cu+ + CH3COO-

NH4+ + Cr2O7

-

Mg2+ + OH-

CuCH3COO

NH4Cr2O7

Mg(OH)2

Parenthesis for POLYATOMIC

6. Naming Ionic CompoundsWrite formula for ionic compounds

1. H+ + SO42-

2. Al3+ + O2- 3. Mg2+ + OH- 4. Fe2+ + Cl-

5. Na+ + HCO3-

6. Ca2+ + PO43-

7. Na+ + NO2-

8. Fe3+ + Cl-

9. NH4+ + PO4

3-

Summary & Review

What is the correct formula for magnesium hydroxide: MgOH2, MgO2H2 or Mg(OH)2?

K+ Fe3+ NH4+ Ba2+

Cl- KCl

SO42-

PO43-

NO3-

OH-

Complete table on separate paper

What is the correct formula for magnesium hydroxide: MgOH2, MgO2H2 or Mg(OH)2?

K+ Fe3+ NH4+ Ba2+

Cl- KCl FeCl3 NH4Cl BaCl2

SO42- K2SO4

Fe2(SO4)3 (NH4)2SO4 BaSO4

PO43- K3PO4

FePO4 (NH4)3PO4 Ba3(PO4)2

NO3- KNO3

Fe(NO3)3 NH4NO3Ba(NO3)2

OH-

KOHFe(OH)3 NH4OH Ba(OH)2

Complete table on separte paper

? mols ? grams

K+ Fe3+ NH4+ Ba2+

Cl- 12g 3.27 mol

SO42- 79.3g 65.30 mol

PO43- 123.4g 2.31 mol

NO3- 423.1g 3.27 mol

OH- 1.497g 1.985 mol

7. Lewis Structures

How many valence electrons do the each of the Noble Gases

have?

HeNe Ar KrXe Rn

7. Lewis Structures

OBJECTIVE:How bonds are made

7. Lewis Structures

Most elements want 8 valence electrons

Octet Rule

7. Lewis Structures

dot = valence electron

7. Lewis Structures

blue line = bond

7. Lewis Structures

Elements that do not want 8 dots

Group 1H, Li, Na, K, etc.

Only wants 2 dotsmore exceptions later

7. Lewis Structures

Draw the following Lewis Structures

H2 Cl2H2S HBrOF2 H2O

NH3 CH4

CH2F2 C2H6

6. Covalent Bonds & Compounds

Most compounds = covalent bonds

7. Lewis Structures

Draw the following structures

O2 N2

CO CO2

HCN SO3

C2Cl4 COCl2

7. Lewis Structures

1.Write elements 2. Count total number of valence

e3. LEAST electronegative is in

the center (usually CARBON)4.Draw bond5.Then draw dots until you run

out6.Make double/triple bonds if

necessary

7. Lewis Structures

Summary & Review1. What element goes in the middle of a

Lewis Structure?

2. Which group does not need 8 dots?

3. Which element is NEVER in the center

4. Lewis Dot Structures

What are the two poles of a magnet called?

What do these poles mean/tell you?

When do you use this diagram in your other classes?


OBJECTIVE: When atoms SHARE

electrons


co-valentSo which electrons are the atoms sharing??

sharing VALENCE electrons

Difference between Ionic & Covalent

IONIC BONDIONIC COMPOUND

Covalent BondCovalent Compound

Atoms

GAIN or LOSE electrons

Atoms

SHAREelectrons

Na+ + Cl- NaCl


C + Cl CCl4


Covalent Bond/Compounds =

when atoms SHARE valence

electronsvideo

6. Covalent Bonds & CompoundsSome examples of covalent compounds


Some example of covalent compounds

6. Covalent Bonds

2 types

Nonpolar Covalentvalence electrons EQUALLY shared

Polar Covalentvalence electrons NOT equally shared

6. Covalent Bonds

Electronegativity determines type

0 – 0.49Nonpolar

C

0.50 – 2.0Polar C

above 2.0Ionic

6. Covalent Bonds

H2, Cl2, F2, N2, NO

1. Draw Lewis Structure

2. Subtract electronegativity values to determine bond type.

3. All have values less than 0.49, so all the above share electrons

equally

6. Covalent Bonds

HBr, NaCl, OF2, NH3, KCl

1. Draw Lewis Structure

2. Subtract electronegativity values to determine bond type

6. Covalent Bonds

HBr, NaCl, OF2, NH3, KCl

What does it mean for HBr, OF2, and NH3 to be polar?

Means shared electron spends more time with…

the element with higher electronegativity

6. Covalent BondsIf polar you use the signs

d- and d+What do these signs mean???

Means shared electron spends more time on the d- side, so d- side has a

small negative charge

So how do you know which side is d-?

the element with higher electronegativity

6. Covalent BondsIf Ionic, we just use

- and +

What do these signs mean???Minus side has a negative charge because it gained and electron

So how do you know which side is -?anion is the minus side

3. Types of Covalent Bonds

Difference > 0.5 Difference > 2.1Polar Ionic

Least Ionic Most Ionic


Summary & Review

1. How is an ionic bond/compound different from a covalent bond/compound?

2. What is shared in a covalent bond/compound?

3. How can you tell if bond is nonpolar, polar, or ionic?

4. If a bond is polar, what are the two signs you use?

5. How do you know where put the signs?

6. What do those signs mean?

Documents

Outline of Topics 1. Atomic Radius 2. Electronegativity 3. Ionization Energy 4. Ions 5. Ionic Compounds 6. Covalent Compounds 7. Lewis Structures