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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
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
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
2. Electronegativity
2nd Trend: Electronegativity
related to atomic radius
smaller the radius,higher the electronegativityhigher electro = really want/good @
attract e-
2. Electronegativity
3 Patterns1. Atomic Radius
2. Electronegativity
Atomic Radius
Electronegativity Ionization Energy
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
2. ELECTRONEGATIVITY
2nd Trend: Electronegativity
2. Electronegativity
2rd Trend: Electronegativity
2. Electronegativity
2rd Trend: Electronegativity
Fluorine has highest electronegativity
Francium has lowest electronegativity
Noble Gases do not count – why?
3rd Trend: Electronegativity
2. Electronegativity
3rd Trend: Electronegativity
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
3. Ionization Energy
3nd Trend: Ionization Energy
What is this?Energy needed to remove an electron from
an atom
OPPOSITE of
ATOMIC RADIUS
3. Ionization Energy
3 Patterns1. Atomic Radius
2. Electronegativity3. Ionization Energy
Atomic Radius
Electronegativity Ionization Energy
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Ionization Energy
3nd Trend: Ionization Energy
3. Trendy Table
How to tell the difference between the two?
NOBLE GASES do not care about
Electronegativity
3. Ionization Energy
3nd Trend: Ionization Energy
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
3. Ionization Energy
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?
6. Covalent Bonds & Compounds
OBJECTIVE: When atoms SHARE
electrons
6. Covalent Bonds & Compounds
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
6. Covalent Bonds & Compounds
C + Cl CCl4
6. Covalent Bonds & Compounds
Covalent Bond/Compounds =
when atoms SHARE valence
electronsvideo
6. Covalent Bonds & CompoundsSome examples of covalent compounds
6. Covalent Bonds & 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
6. Covalent Bonds & Compounds
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?
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