A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic...

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Page 1: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 2: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

A. Electronegativity - The ability of an atom to attract electrons to itself in a bond

1. Periodic Trends (link to size)Metals – Low ElectronegativityNon- Metals – High Electroneg

The smaller the atom, the higher the electronegativity

Types of Bonds

Page 3: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

a. Molecular Compounds (non-metals)• Sharing of electrons• Covalent or polar covalent bonds• Ex: H2

b. Ionic Compounds (metal + non-metal)• Exchange (stealing) of electrons• Ex: NaCl

Types of Bonds

Page 4: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 5: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 6: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 7: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

3. Types of bondsElectronegatvity Difference

Example: Na-F

Types of Bonds

Page 8: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Are the following bonds ionic, polar covalent or covalent?

Ba – Br C – NBe – F B – HO – H Be – ClP – H C – HO – O

Types of Bonds

Page 9: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Ionic – Electron is completely removed from one atom and goes to another

a. Metal – Low e-neg (loses e-)b. Non-metal – high e-neg (gains e-)

Ionic

Page 10: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 11: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 12: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

IA IIA IIIA IVA VA VIA VIIA

HydrideH-

LithiumLi+

BerylliumBe2+

CarbideC4-

NitrideN3-

OxideO2-

FluorideF-

SodiumNa+

MagnesiumMg2+

AluminumAl3+

PhosphideP3-

SulfideS2-

ChlorideCl-

PotassiumK+

CalciumCa2+

SelenideSe2-

BromideBr-

RubidiumRb+

StrontiumSr2+

TellurideTe2-

IodideI-

CesiumCs+

BariumBa2+

Common Charges

Page 13: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Complete the following chart:Formula Lewis Dot

K and I

Sr and F

Ba and Cl

Sr and N

Ba and O

Page 14: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 15: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Complete the following chart:Formula Lewis Dot

K and S

Al and O

Na and Br

Ca and O

Page 16: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

1. Not Separate molecules2. Crystal Lattice – Regular 3D pattern in an

ionic solid

Ionic Solids

Page 17: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 18: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Ionic Solids

at lattice points ions at lattice points

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1. Water (molecule) dissolves salt (ionic crystal):

Ions in Water

Page 20: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 21: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Molecules

Page 22: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Many ionic compounds are called salts

CaCl2 Calcium Chloride (Quik-Joe)NaHCO3 Sodium bicarbonate(Baking soda)NaF Sodium Fluoride (toothpaste)CaCO3 Calcium Carbonate(Chalk, antacid)NaOH Sodium Hydroxide (Drano)MgSO4 Magnesium Sulfate(Epsom Salts)

All big clumps (crystals) of Ions

Other Salts

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• Group of atoms held together by covalent and polar covalent bonds (SHARING)

• Usually composed of non-metals • Stronger than Ionic bonds• Separate (discrete) groups of

atoms

What is a Molecule?

Page 24: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 25: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

A. Single Bonds (LD and Stick)CH4

H2O

(bonded versus lone pairs)

Old School Lewis Dots

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The Lone Pear(Pair) rides again!

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N and HP and FCl and ONH2CH3

Old School Lewis Dots

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You try:As and HN and BrCH3CH2OH

NH2CH2SiCl3

CH3OCH3

Old School Lewis Dots

Page 29: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

As and ClC and BrCH3CH2NH2

CH3OCH2CH3

Page 30: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

B. Multiple BondsCO2

C2H2

Old School Lewis Dots

Page 31: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

You Try:HCNN2

AlN

O2

Old School Lewis Dots

Page 32: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Rules1. Sum all valence electrons, including

charges2. Single Bonds3. Outer atoms get an octet except H4. Center gets rest even if it violates the octet5. Double/triple bonds if center atom still

does not have an octet

Lewis Dots

Page 33: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

NH3

NCl3

SF6

Br2O

ClF5

Lewis Dots

Page 34: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

You try:SF4

KrF4

Cl2O

ClF3

H2SO4

Page 35: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Warm-Up:

CH3CH2NH2

SeF4

KrCl4

H2O2

BaCl2 (this is an ionic cmpd)

Page 36: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

CO2

HCNCN-

ICl4-

NO+

Lewis Dots

Page 37: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

CO32-

H3O+

NH4+

PO43-

SO2

Page 38: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

• Hydrogenonly makes one bond• Gr I, II and III• Especially if with a halogen

BeCl2 BCl3 AlCl3

Less Than an Octet

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• Non-Metals starting with P

More Than an Octet

P S Cl Ar

As Se Br Kr

Te I Xe

Page 40: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

PCl5

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Warm-Up: O3

Definition – When a molecule can exist in more than one arrangement of electrons1. Atoms don’t move2. Only the electrons (double bonds) move3. Also called “delocalized bonding”

Resonance Structures

Page 42: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Si2H4

AsO43-

CS32-

H3S+

PH4+

Page 43: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

SPECIAL NOTE:

Oxygen rarely makes three bonds for resonance structures. Those structures are not common.

Resonance Structures

Page 44: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

PO3-

HSO3+

Page 45: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Examples1. NO2

-, CO32-, CHO2

-, HNO3

2. Which needs resonance, SO3 or

SO32-

Resonance Structures

Page 46: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

• Valence Shell Electron Pair Repulsion Theory (VSEPR)

• VSEPR – Valence electron pairs on the central atom push as far apart as possible.

Shapes of Molecules

Page 47: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 48: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

1. Linear (180o)BeH2 CO2

Shapes of Molecules

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Shapes of Molecules

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2. Trigonal Planar (120o)NO3

-

Shapes of Molecules

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Shapes of Molecules

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3. Tetrahedral (109.5o)CH4

Shapes of Molecules

Page 53: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Shapes of Molecules

Page 54: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 55: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
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4. Trigonal Pyramidal (~107o)NH3

Shapes of Molecules

Page 57: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Shapes of Molecules

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5. Bent (Type I, ~104.5o)H2O

Shapes of Molecules

Page 59: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Shapes of Molecules

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Shapes of Molecules

OH H

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Shapes of Molecules

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Bent (Type II, 120o)SO2

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•Atoms are bent•Bond angle = 120o

Page 64: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

6. Trigonal Bipyramid (120o, 90o)PCl5

Shapes of Molecules

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Shapes of Molecules

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7. Octahedral (90o)SF6

Shapes of Molecules

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Shapes of Molecules

Page 68: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

DRAW LEWIS DOT STRUCTURES AND PREDICT THE BOND ANGLES FOR:

PH3 GeO2

PCl5 NCl3

H2S SiH4

CF4 SO32-

SeCl6 SO3

Page 69: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Ex: All single bonds:PH3 H2S SiH4

SeCl6 AsF5 BeCl2

CH3F HF BF3

Shapes of Molecules

Page 70: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Ex: Multiple Bonds:N2

HCNCO2

H2CO

Shapes of Molecules

Page 71: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

SO22+ SO2

2- SO2

SO3 SF6

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Shapes of Molecules

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1. Examples:BeH2

H2O

BH3

NH3

2. There is no relationship between formula and shape

Shapes and Formula?

Page 74: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

PO2- PO3

- PO33-

PO43- XeF4

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Household Molecules H2O

HClNH3

H2SO4

Page 79: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

1. Polar molecule – Overall, the electrons are attracted more to one end of an entire molecule

2. Non-Polar Molecule – The electrons are spread out evenly over the entire molecule

-/ + Partial (not full) charges

Polar Molecules

Page 80: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

H2 H2O

CH4 H2CO (C is the center)

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H2 H2O

CH4 H2CO

Page 82: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

BeCl2

NH3

CO2

CSO

HCN (triple bond)

Page 83: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
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CCl4 CH3ClCH2Cl2

CHCl3

HBeClHBr

Page 85: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

CH3Cl CH2Cl2

CHCl3 HBeCl HBr

Polar Molecules

Page 86: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Lewis Dot Shape Polar or Non-polar molecule?

H2O

NH3

CH3Cl

CH3CH2OH

SO2

Page 87: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Hydrogen Bondinga. Water Beadingb. SurfaceTensionc. Iced. DNAe. Miscibility (NH3, ethanol)f. Immiscibility (Water and Oil)

Page 88: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Water Beading

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Surface Tension

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Surface Tension

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Ice

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Ice

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MoleculesBoiling Point• Generally

increases with increasing molar mass

• H2O unusually high - H-bonding

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DNA

Page 98: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

DNA

DNA is TWO molecules

that are hydrogen

bonded (like a zipper)

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DNA

Human Genome Project

Page 100: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

• DNA in one cell = 1 meter• DNA in all your cells = 93,000,000 miles

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Miscibility

•“Like dissolves like.”

•Polar dissolves Polar

•Water, ammonia

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Miscibility

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Miscibility

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Miscibility

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Miscibility

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Miscibility

•Water, alcohol

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•Water, alcohol

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•Water, alcohol

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Miscibility

•Water, alcohol

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Miscibility

•Non-Polar dissolves Non-Polar

•oil paint, thinner

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Miscibility

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Would acetone (shown below) dissolve in water?

Acetone

:O: ||CH3CCH3

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MoleculesLondon Dispersion Forces

• Very weak force• Caused by temporary imbalances in electrons

Page 115: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

MoleculesLondon Forces: Inorganic Molecules• More electrons, more chance for temporary

dipole

Boiling Point TableHalogen Molar

MassBP(oC) Noble

GasAtomic Mass

BP(oC)

F2 (g) 38.0 -188 He 4.0 -268

Cl2 (g) 71.0 -35 Ne 20.2 -246

Br2 (l) 159.8 59 Ar 39.9 -186

I2 (s) 253.8 185 Kr 83.8 -152

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Consider the following molecules:

Te2 S2 O2 Se2

a. Rank them from weakest to strongest London forces

b.Which should have the highest boiling point? Which should have the lowest?

c. Would it take more energy to melt a sample of carbon or silicon?

Page 117: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

MoleculesLondon Forces: Organic Compounds• The longer the carbon chain, the higher the

London Dispersion Forces (the higher the melting point and boiling point)

BP(oC)CH4 -161.6C2H6 -88.63C3H8 -42.07C4H10 -0.5

Page 118: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Which should have a higher boiling point:

C6H14 or C12H26

Page 119: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Using you knowledge of “like dissolves like”, explain the following trends in solubility.

Alcohol Solubility in H2O (mol/100 g H2O at 20oC)

CH3OH ∞

CH3CH2OH ∞

CH3CH2CH2OH ∞

CH3CH2CH2CH2OH 0.11

CH3CH2CH2CH2CH2OH 0.030

CH3CH2CH2CH2CH2CH2OH 0.0058

CH3CH2CH2CH2CH2CH2CH2OH 0.0008

Explain the following trends in solubility in water

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Page 121: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Emulsifying agents– Mayonaise– Soap

http://upload.wikimedia.org/wikipedia/commons/a/ae/SDS-2D-skeletal.png
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Page 123: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

The Key to the Universe

Page 124: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

You Try:

CCl4 NO3-

CH3Cl H2COCH2Cl2 H2S

Polar Molecules

Page 125: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

KrCl4 Si2H4

BN CH3SiH2PH2

SiS2 H2SO4

OH O S O H

O

Page 126: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

9. (c) Sc2+ (d) I2- (e) As2- 15. Rb+ Ba2+ Te2- N3-

16. Al3+, Mg2+, Na+, F-, O2-, N3-

20.RbF Rb2Te Rb3P

MgF2 MgTe Mg3P2

CrF3 Cr2Te3 CrP

22. BeS Cs2S Ga2S3 SrS

24.a) Ir8+ b) Sc3+ c) Pt6+ d) Co3+

e) Tc3+ f) Ag+

Page 127: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

27. a) HI b) SeBr2 c) SiBr4 d) H3As

49. a) PC b) Cov c) PC d) Ionic

50. a) PC b) PC d) Ionic d) PC52. a) N-H b) Si-O c) S-F P-Cl

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54.a) trigonal planar b) trigonal pyramidc) linear d) trigonal planare) trigonal planar

56.a) H2O c) NH4+

Page 130: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

a) octahedral h) tetrahedralb) tetrahedral i) trigonal bipyramidc) linear j) trigonal pyramidd) trigonal planar k) octahedrale) bent l) linearf) trigonal planar m) linearg) Linear n) linear

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Assessing the Objectives (page 278)a)2, 3b)Less than 109.5o

c) Trigonal Planard)Bente)Linear, 180o bent, 120o

Page 132: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Questions1. Rank the three liquids from weakest to the

strongest forces between their molecules.2.Discuss how you chose your rankings from the

results of the experiment.3.Is isopropyl alcohol or hexane more like

water? Explain, using the results from the experiments.

4.What information did the salt experiment provide about the molecules?

Page 133: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

GAK – NEATNESS!!!!!!!1.Glue2.Food coloring3.Borax solution

Page 134: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Formula Lewis Dot

Ca and O

Ca and Br

P and H

C and F

N and F

Page 135: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Consider the following three chemical bonds:

C-O Cl-Br Rb-Cla. Determine the type of bond present in each

situationb.In which bond is an electron transferred?c. Draw the Lewis Dot structure of this ionic

compound.d.In which bond are electrons unequally

shared?e. Identify the element in that bond that the

electron spends more time with.

Page 136: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

The element chlorine forms compounds with both strontium and sulfur.

a. Write the formula of the compound that forms between strontium and chlorine.

b. Draw the Lewis Dot Structure of this compound, indicating whether it is ionic or molecular.

c. Write the formula of the compound that forms between sulfur and chlorine.

d. Draw the Lewis Dot Structure of this compound, indicating whether it is ionic or molecular.

e. Is the structure you drew in (d) linear? Why or why not?

f. State the bond angle of the structure in (d).

Page 137: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.
Page 138: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Draw the Lewis Dot Structure and predict whether it is a polar or non-polar molecule

H2O

CH3CH(OH)CH3

CH3CH2CH2CH2CH2CH3

Page 139: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Water Isopropyl HexaneAlcohol

Page 140: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Draw Lewis Structures (Ionic)

BaF2 Li2O

Draw Lewis Structures (Molecular)

ClF3 SiO32- SO2

Page 141: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

Compound Central Atom

BeH2 Tan

BH3 Tan

CH4, NH3, H2O Black

PCl5 Tan

SF6 Yellow or silver

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7a. Octahedral h. Tetrahedral

b.Tetrahedral i. Trigonal bipyramid

c. Linear j. Trigonal pyramid

d.Trigonal Planar k. Octahedral

e. Bent I l. Linear

f. Trigonal Planar m. Linear

g.Linear n. Linear

Page 149: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

1. Covalent, Ionic or Polar Covalent Bonds?

a. Ionic

b.Covalent

c. Polar Covalent

d.Ionic

e. Ionic

f. Polar Covalent

g.Polar Covalent

h.Ionic

Page 150: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

3a. K+ Br-

b.Al3+ 3Cl-

c. 2Ga3+ 3O2-

d.2Li+ O2-

e. Ca2+ 2Br-

f. Na+ OH-

g.Ca2+ 2NO3-

h.2Na+ CO32-

i. 2Fe3+ 3SO42-

j. Co4+ 4NO2-

Page 151: A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity.

http://www.youtube.com/watch?v=WaPxTAeW5e8

http://www.youtube.com/watch?v=WaPxTAeW5e8
http://www.youtube.com/watch?v=WaPxTAeW5e8

1 5-6Electronegativity Electronegativity is a measure of the relative tendency of an atom to attract electrons to itself when chemically combined with.

1 5-6Electronegativity Electronegativity is a measure of the relative tendency of an atom to attract electrons to itself when chemically combined with.

Starter: Spot the errors. Answers Electronegativity What is electronegativity?

Starter: Spot the errors. Answers Electronegativity What is electronegativity?

Obada Froukh - Doctor 2018 - JU Medicine · 2019-06-14 · 3 | P a g e Important Terms: 1-Electronegativity: the tendency of an atom to attract electrons of the bond. 2- ovalent bonds:

Obada Froukh - Doctor 2018 - JU Medicine · 2019-06-14 · 3 | P a g e Important Terms: 1-Electronegativity: the tendency of an atom to attract electrons of the bond. 2- ovalent bonds:

Esercitazione n° 2 · Electronegativity, symbol χ, is a chemical property that describes the ability of an atom to attract electrons (or electron density) towards itself in a covalent

Esercitazione n° 2 · Electronegativity, symbol χ, is a chemical property that describes the ability of an atom to attract electrons (or electron density) towards itself in a covalent

Periodic Trends Definitions & Trends ELECTRONEGTIVITY Electronegativity is the power of an atom, when in a molecule, to attract electrons to itself.

Periodic Trends Definitions & Trends ELECTRONEGTIVITY Electronegativity is the power of an atom, when in a molecule, to attract electrons to itself.

Electrons Electrons are found circling the nucleus at extremely fast speeds. + and – attract. The reason e- are not pulled into the nucleus is because.

Electrons Electrons are found circling the nucleus at extremely fast speeds. + and – attract. The reason e- are not pulled into the nucleus is because.

Bonding – Chapter 7chem.winthrop.edu/faculty/mcintosh/link_to_webpages... · Electronegativity (EN) – attraction for bonding (shared) electrons The difference in EN between the

Bonding – Chapter 7chem.winthrop.edu/faculty/mcintosh/link_to_webpages... · Electronegativity (EN) – attraction for bonding (shared) electrons The difference in EN between the

Periodic Trends We will explain observed trends in Atomic (and Ionic) Radius Ionization Eenergy Electronegativity size lose e – attract e – nuclear.

Periodic Trends We will explain observed trends in Atomic (and Ionic) Radius Ionization Eenergy Electronegativity size lose e – attract e – nuclear.

Chemical Bonding Bonds form in 2 main ways atoms share electrons electrons are transferred between atoms Type of bond depends on the atom’s electronegativity.

Chemical Bonding Bonds form in 2 main ways atoms share electrons electrons are transferred between atoms Type of bond depends on the atom’s electronegativity.

Intro to Bonding Valence Electrons, Lewis Dot Structures, and Electronegativity.

Intro to Bonding Valence Electrons, Lewis Dot Structures, and Electronegativity.

Electronegativity Elements

Electronegativity Elements

tophamscience.weebly.com · 2016-10-06 · Electronegativity is a measure of the ability of an atom's nucleus to attract electrons from a different atom within a covalent bond. A

tophamscience.weebly.com · 2016-10-06 · Electronegativity is a measure of the ability of an atom's nucleus to attract electrons from a different atom within a covalent bond. A

MATERIALS SCIENCE AND ENGINEERING I 3_eng.pdf · 1.3 METALLIC BONDING • Between metal atoms (small difference of electronegativity); • Also through sharing of valency electrons

MATERIALS SCIENCE AND ENGINEERING I 3_eng.pdf · 1.3 METALLIC BONDING • Between metal atoms (small difference of electronegativity); • Also through sharing of valency electrons

Chemistry - · PDF filePeriodic Table of Elements, electrons, atoms, bonds, ions, Dmitri Mendeleev, nucleus, protons, neutrons, Atomic Radii, Ionization Energy, Electronegativity and

Chemistry - · PDF filePeriodic Table of Elements, electrons, atoms, bonds, ions, Dmitri Mendeleev, nucleus, protons, neutrons, Atomic Radii, Ionization Energy, Electronegativity and

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. If the electronegativity of an atom is high, then.

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. If the electronegativity of an atom is high, then.

Lesson #2 Electronegativity & Ionic Bonds...The difference in electronegativity between two atoms, , tells you Electronegativity across a period because: Electronegativity down a group

Lesson #2 Electronegativity & Ionic Bonds...The difference in electronegativity between two atoms, , tells you Electronegativity across a period because: Electronegativity down a group

Polarizability and Electronegativity · Polarizability and Electronegativity ... • Polarizability also depends on electronegativity. Electronegative atoms are not very polarizable.

Polarizability and Electronegativity · Polarizability and Electronegativity ... • Polarizability also depends on electronegativity. Electronegative atoms are not very polarizable.

Chemical Bonding Chemical bond – The attractive force between the protons of one atom for the electrons of another atom Determined by electronegativity.

Chemical Bonding Chemical bond – The attractive force between the protons of one atom for the electrons of another atom Determined by electronegativity.

Chemistry Science Standards Alignment - Amazon Web … · Web viewIonization Energy and Electronegativity Chemical bonds form when electrons are transferred or shared between atoms.

Chemistry Science Standards Alignment - Amazon Web … · Web viewIonization Energy and Electronegativity Chemical bonds form when electrons are transferred or shared between atoms.

Bond Polarity and Electronegativity In a covalent bond, electrons are shared. Equal sharing of electrons to form a covalent bond forms a nonpolar molecule.

Bond Polarity and Electronegativity In a covalent bond, electrons are shared. Equal sharing of electrons to form a covalent bond forms a nonpolar molecule.