warm up what are the three types of bonds? determine the type of bond, and how many of each...

Warm Up

What are the three types of bonds? Determine the type of bond, and how

many of each element are present in: Na2O CO2

CuZn

Objectives

Draw the Lewis structures of ionic and covalent structures.

Lewis Structures

Combining of the dot diagrams to show bonding and to predict shape.

Every Element wants 8 electrons. 2 Types- covalent and ionic.

Ionic Lewis Structures

Step 1: Draw the Lewis dot diagrams for each element.

Step 2: Draw an arrow from the metals electrons to the empty spaces around the nonmetal.

Step 3: Redraw the Lewis dot diagrams showing the movement of electrons AND charges.

Example

Draw the Lewis structure for: NaCl

Example

Draw the Lewis structure for: LiF

Example

Draw the Lewis structure for: MgCl2

Example

Draw the Lewis structure for: Na2O

You Try

Draw the Lewis structure for: KI BeI2 SrF2

Covalent Lewis Structures

Show the sharing of electrons. Show bonds as Show the lone pairs as

Steps for Lewis Structures

Step 1: Add up total number of valence electrons.Step 2: Draw a skeleton by connecting each element with a line. (Carbon or the solo element goes in the middle)

★Hydrogen and the Halogens CANNOT be in the center.

Step 3: Distribute the electrons as PAIRS. Start from the outside and move inward. Step 4: Check Ya Self! Count and adjust electrons till each element has 8. (except Hydrogen)

Examples

Draw the lewis structures for the following:

CF4

Examples


H2O

Examples


PH3

Examples


O2

You Try


NH3

F2O CO2

Warm Up

What elements and how many are present in: CO2

PH3

MgBr2

Draw the Lewis structures for: KCl CaF2

Objectives

Draw the Lewis structures for covalent molecules

Predict the shape of a molecule given the formula.

Objectives

Distinguish between a polar and non-polar covalent bond.

Draw Lewis structures of compounds.

Review

Ionic Bond Between a metal and non-metal

Covalent Bond Between a non-metal and another non-

metal Two types: Polar and Non-polar covalent

Metallic Bond Between a metal and a metal

Electronegativity

The attraction an element has to electrons.

Scale of 0-4 Can be used to determine the type of

bond. 0-0.4 = Nonpolar covalent

0.41-1.7 = Polar CovalentGreater than 1.7 is ionic

Example

Identify the following bonds as polar or non-polar covalent:

H bonded to O H bonded to C C bonded to F C bonded to N

Warm Up

What are the three types of bonds? What is electronegativity? Determine the type of bond in:

Na2O CO2

CuZn

Objectives

Determine the type and number of atoms in a compound based on the formula.

Draw Lewis structures of ionic and covalent compounds.

What is a Chemical Formula? Tells you the elements in the compound.

Notated by the atomic symbol of the element.

Tells you the number of each element. Shown by the subscript number. No number

means 1. Note it is always a whole number!

Example

What type of elements and how many are in:

MgCl2

Example


NH3

Example


CF4

Example

Identify each element and amount of each element in the following compounds:

H2O CH4

NaCl Li2O

Lewis Structures

Combining of the dot diagrams to show bonding and to predict shape.

Every Element wants 8 electrons. 2 Types- covalent and ionic.

Ionic Lewis Structures

Step 1: Draw the lewis dot diagrams for each element.

Step 2: Draw an arrow from the metals electrons to the empty spaces around the nonmetal.

Step 3: Redraw the lewis dot diagrams showing the movement of electrons AND charges.

Example

Draw the Lewis structure for: NaCl

Example

Draw the Lewis structure for: LiF

Example

Draw the Lewis structure for: MgCl2

Example

Draw the Lewis structure for: Na2O

You Try

Draw the Lewis structure for: KI BeI2 SrF2

Warm Up

What elements and how many are present in: CO2

PH3

MgBr2

Draw the Lewis structures for: KCl CaF2

Objectives

Draw the Lewis structures for covalent molecules

Predict the shape of a molecule given the formula.

Steps for Lewis Structures

Step 1: Add up total number of valence electrons.Step 2: Draw a skeleton by connecting each element with a line. (Carbon, the solo element, or the most electronegative element goes in the middle)★Hydrogen and the Halogens CANNOT be in the center.Step 3: Distribute the electrons as PAIRS. Start from the outside and move inward. Step 4: Count and adjust electrons till each element has 8. (except Hydrogen)

Examples


CF4

Examples


H2O

Examples


PH3

Examples


O2

You Try


NH3

F2O CO2

Exit Card

Identify the type of bond as polar or non-polar:

CCl4 CH4

Identify the elements and their amounts of the compounds above.

Draw the Lewis structures for: NH3

CF4

Warm Up

Classify the following bonds as ionic, polar covalent, or non-polar covalent.

F2

MgI2

NH3

Draw the Lewis structures for the following: F2

MgI2

NH3

Objectives

Predict the shape of a molecule based on the VSEPR theory.

VSEPR

Stands for “Valence shell Electron pair Repulsion”

V-Valence S-Shell E-Electron P-Pair R-Repulsion Basically Electrons don’t like each other

very much!

Steps for predicting shapes

Step 1: Draw the Lewis structures for the compound

Step 2: Draw a box around the central atom/element

Step 3: Predict the shape based on the following.

5 Shapes

Four single bonds-Tetrahedral 3 single bonds and 1 lone pair-Trigonal

Pyramidal 2 single, 1 double-Trigonal planar 2 bonds (any type) and lone pairs-Bent 2 bonds no lone pairs OR just 2 atoms-

Linear

Example

Predict the shape of the following: SO3

Example

Predict the shape of the following: H2O

Example

Predict the shape of the following: NH3

You Try

Predict the shape of the following PF3

MgCl2

SiO2

Exit Card

What does VSEPR stand for? List the five different shapes of

molecules. Predict the shape of the following: H2S O3 CCl4

Warm Up

What does VSEPR stand for? List the 6 different shapes of molecules. Predict the shape of the following: H2S O3 CCl4

Objectives

Predict the polarity of a molecule based on the structure of a molecule.

(Honors) Determine the intermolecular forces between two molecules

Polar and nonpolar…again

Molecules have an overall polarity in addition to polar and nonpolar bonds.

Polar molecules have unequal distribution of electrons.

while Nonpolar molecules have an equal

distribution of electrons.

How do you know if a molecule is polar?

First determine the shape of the molecule in question.

Then Predict the polarity of the molecule based on its shape. Bent, and trigonal pyramidal molecules are

ALWAYS polar. Tetrahedral, trigonal planar, and linear are

ALWAYS nonpolar.

How do you know if a molecule is polar?

Bent, and trigonal pyramidal molecules are ALWAYS polar.

Tetrahedral, trigonal planar, and linear are usually nonpolar. But can be polar, IF and ONLY IF there are 3 or more different elements. Ex. CH4 vs. CH2F2

Examples

Determine if the following molecules are polar or non-polar.

SiBr4

Examples


OI2

Examples


O3

Examples


CO2

Examples


S3O

Examples


CSeF2

You Try


NF3

SO2

H2S

Warm Up


NF3

SiO2

H2S

Objectives

(Honors) Determine the intermolecular forces between two molecules.

Predict the properties of a molecule or compound

May the Forces be with You

Intramolecular forces- Intermolecular forces- the attractions between molecules that account for properties such as BP, MP, viscosity, surface tension, and solubility.

Types of Intermolecular Forces

Three types:

London Dispersion

Also called induced dipole Between non-polar molecules Very very weak

Dipole-Dipole

Between polar molecules Two oppositely charges ends.(one +

and one -)

Hydrogen Bonding

NOT a bond. Between hydrogen of one molecule

and fluorine, oxygen, or nitrogen of ANOTHER molecule.

Extremely strong.

Ranking Intermolecular Forces

The stronger the IM the higher the Bp and Mp.

Hydrogen Bonds >>> Dipole >> London

Example

Rank the following in order of increasing boiling point.

PH3

CH4

CO2

H2O

Example

Which will have a higher Mp? Why? NH3 or PH3

Example

Water boils at 100C and H2S boils at -60C, briefly explain why these two molecules have vastly different boiling points despite having similar structures and polarities.

You Try


SBr2

NH3

SiO2

You Try


F2O Cl2 Br2O

Properties of Ionic Substances Hard Brittle A solid at room temperature Very very high melting and boiling Points Soluble in water Conduct electricity when dissolved in

water or as a liquid.

Properties of Metals

Shiny Solid at room temperature. Very high melting and high boiling points Insoluble in water Conduct electricity Malleable and ductile

Properties of Polar Molecules

Typically a liquid at room temperature. Low melting points and boiling points Soluble in water Not a of conductor electricity

Properties of Non-polar molecules Typically a gas at room temperature. Very low melting and boiling points Insoluble in water Not a conductor of electricity.

Steps for determining properties. Step 1: Draw the Lewis structures of all

compounds involved. Step 2: Predict the shape of all

compounds Step 3: Based on the shape determine

the polarity of the compound Step 4: Once the polarity is determined

look up the properties for that type of compound.

Example

Which of the following will conduct electricity?

NaCl CO2

ZnCu H2O

Example

Which of the following will be a liquid at room temperature?

NaCl CO2

ZnCu H2O

Example

Which of the following will be a gas at room temperature?

NaCl CO2

ZnCu H2O

You Try

Predict the state of matter for each of the following at room temperature.

MgBr2

O3

SO3

HgZn

Exit Card

Determine if the molecule is polar or non-polar and predict the state of matter at room temperature:

NH3

HCl O2

CHF3

OF2

Warm Up

Determine the probable state of matter at room temperature for the following:

CS2

PH3

CBr4

H2O

Objectives

Predict the properties of the compounds based on the type of molecule.

Examples

Predict the state of matter at room temperature of:

CO2

SrF2

PCl3

Exit Card

List one property of ionic compounds, metallic compounds, polar compounds, and non-polar compounds.

Predict the state of matter for the following at room temperature.

H2O NH3

Cu-Zn BaO

Warm Up

What is the typical state of matter for: Ionic substances Polar compounds Non-polar compounds Which of the following would have the

highest boiling point? Lowest? CO2, Na2O, H2O

Warm Up

Determine the polarity of: SO3

H2S

Objectives

Predict the properties of a substance based on the type of compound and its’ polarity.

(Honors) Describe the intermolecular forces present in molecules.

(Honors) Rank molecules based on the intermolecular forces involved.

Properties of Ionic Substances Hard Brittle A solid at room temperature Very high melting points (≈800C) Very high boiling Points Soluble in water Conduct electricity when dissolved in

water or as a liquid.

Properties of Metals

Shiny Solid at room temperature. Very very high melting point (≈1000C) Very Very high boiling point Insoluble in water Conduct electricity Malleable and ductile

Properties of Polar Molecules

Typically a liquid at room temperature. Low melting points (≈20C) Medium boiling points Soluble in water Not a of conductor electricity

Properties of Non-polar molecules Typically a gas at room temperature. Very low melting (≈-100C) Very low boiling points Insoluble in water Not a conductor of electricity.

How to Determine Properties First: Draw the Lewis structures of all

compounds involved. Next: Predict the shape of all compounds Then: Based on the shape determine the

polarity of the compound Finally: Once the polarity is determined

look up the properties for that type of compound.

Example

Which of the following will conduct electricity?

NaCl CO2

ZnCu H2O

Example

Which of the following will be a liquid at room temperature?

NaCl CO2

ZnCu H2O

Example

Which of the following will be a gas at room temperature?

NaCl CO2

ZnCu H2O

You Try

Predict the state of matter for each of the following at room temperature.

MgBr2

O3

SO3

HgZn

Exit Card

Which of the following would dissolve in water: NaCl CH4

NH3

Rank the following in order of increasing boiling point:

NH3

CO2

CSF2

Warm Up

Identify the type of compounds as ionic, covalent, metalic:

CaS BrF Draw the Lewis Structure for AsI3, predict

the shape, determine its polarity, and predict its’ state of matter at room temperature.

warm up what are the three types of bonds? determine the type of bond, and how many of each...

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