Chapter 9 Chapter 9 Notes Part INotes Part ICovalent Bonding Covalent Bonding

Obj. 1…Octet RuleObj. 1…Octet Rule• Recall that all elements want 8 valence e-.Recall that all elements want 8 valence e-.• metals will metals will loselose their valence e-. their valence e-.

• non-metals will non-metals will gaingain more valence e-. more valence e-.

- (+) cations- (+) cations

- (-) anions- (-) anions

• noble gases do not gain or lose e-. noble gases do not gain or lose e-.

- happy already!- happy already!

*** atoms need other atoms in order to lose/gain *** atoms need other atoms in order to lose/gain e-.e-. - electronegativity differences determine - electronegativity differences determine

bond.bond. - metals = low / non-metals = high - metals = low / non-metals = high electroneg.electroneg.

Obj. 2…Ionic BondsObj. 2…Ionic Bonds• transfertransfer of e- b/n (+) cation and (-) anion. of e- b/n (+) cation and (-) anion.

- compounds created are neutral- compounds created are neutral

- 10% of all bonds- 10% of all bonds

- - strongeststrongest bond bond

- forms crystalline - forms crystalline solidssolids

- - highesthighest melting/boiling pts. melting/boiling pts.

- can conduct electricity in molten states.- can conduct electricity in molten states.

Obj. 3…Pure Covalent Obj. 3…Pure Covalent BondsBonds

• equal sharingequal sharing of e- b/n non-metals ( of e- b/n non-metals (moleculemolecule))..

- compounds created are neutral- compounds created are neutral

- 2% of all bonds- 2% of all bonds

- - weakestweakest bond bond

- typically form - typically form gasesgases

- - lowestlowest melting/boiling pts. melting/boiling pts.

- do - do NOTNOT conduct electricity! conduct electricity!

Obj. 4…Polar Covalent Obj. 4…Polar Covalent BondsBonds

• un-equal sharingun-equal sharing of e- b/n non-metals of e- b/n non-metals ((moleculemolecule)).. - compounds created are neutral- compounds created are neutral

- 88% of all bonds- 88% of all bonds

- - intermediateintermediate bond strength bond strength

- typically form - typically form soft solids soft solids and and liquidsliquids

- - intermediateintermediate melting/boiling pts. melting/boiling pts.

- - somesome conduct electricity in molten states. conduct electricity in molten states.

Obj. 6…Metallic BondsObj. 6…Metallic Bonds• cations (+) in metals are surrounded by a sea ofcations (+) in metals are surrounded by a sea ofmobile e-…(‘mobile e-…(‘delocalized e-delocalized e-’).’).

• metals held together by attraction b/n e- and metals held together by attraction b/n e- and - cushion b/n cations- cushion b/n cations

cations.cations.

Obj. 6 cont…Obj. 6 cont…

• good conductors of good conductors of electricityelectricity- as e- enter one end, an = - as e- enter one end, an = ## of e- leave the of e- leave the

otherother• ductileductile

- can be drawn into a wire- can be drawn into a wire

• Because of mobile ‘delocalized’ e-, metals are…Because of mobile ‘delocalized’ e-, metals are…

• malleablemalleable- can be hammered- can be hammered

Obj. 7…Bonding Obj. 7…Bonding VocabularyVocabulary• ionion:: atom w/ a charge.atom w/ a charge.

- has lost or gained - has lost or gained e-e-• valence electronvalence electron:: all e- in outer ‘s’ and ‘p’ all e- in outer ‘s’ and ‘p’

orbitals.orbitals.• dipoledipole:: molecule w/ one slightly (-) end and onemolecule w/ one slightly (-) end and oneslightly (+) end.slightly (+) end.

- occurs in polar covalent bonds- occurs in polar covalent bonds• polyatomic ionpolyatomic ion:: a group of atoms (covalentlya group of atoms (covalently

bonded), that act as a single atombonded), that act as a single atom- NH- NH44

+1+1, SO, SO44-2-2, ClO, ClO33

-1-1

• moleculemolecule:: atoms atoms covalentlycovalently bonded together. bonded together.

Covalent BondingCovalent Bonding

A covalent bond occurs A covalent bond occurs between two non-metalsbetween two non-metals

Electrostatic bonding Electrostatic bonding does not occur—in other does not occur—in other words, there is no “give words, there is no “give and take” of electronsand take” of electrons

It ends up being a “tug of It ends up being a “tug of war” of electronswar” of electrons

Where the electrons end up Where the electrons end up somewhere in the middle.somewhere in the middle.

Single BondsSingle Bonds

A single bond occurs A single bond occurs when one pair of when one pair of electrons is shared by electrons is shared by two atoms.two atoms.

This pair of bonded This pair of bonded electrons is called a electrons is called a shared pairshared pair. .

Double and Triple Double and Triple BondsBonds

Double bonds occur Double bonds occur when two atoms have two when two atoms have two shared pair of electronsshared pair of electrons

Triple bonds occur when Triple bonds occur when two atoms share three two atoms share three pair of electronspair of electrons

Sigma and Pi BondsSigma and Pi BondsHow do covalent bonds How do covalent bonds form between two form between two elements?elements?

By the combining of By the combining of their p orbitals.their p orbitals.

Sigma and Pi BondsSigma and Pi BondsThe first bond The first bond between two atoms between two atoms is a sigma bond (is a sigma bond () ) and it forms because and it forms because of end-to-end of end-to-end overlap of p orbitals.overlap of p orbitals.

Sigma and Pi BondsSigma and Pi Bonds

Any other bonds Any other bonds between the same between the same atoms would be a pi atoms would be a pi bond (bond () and they form ) and they form because of side-to-side because of side-to-side overlap of p orbitals.overlap of p orbitals.

Sigma and Pi BondsSigma and Pi BondsSingle bond = 1 sigma Single bond = 1 sigma bondbond

Double bond = 1 sigma+1 Double bond = 1 sigma+1 pi bondpi bond

Triple bond = 1 sigma + 2 Triple bond = 1 sigma + 2 pi pi bondsbonds

Sigma and Pi BondsSigma and Pi BondsHow many sigma and pi How many sigma and pi bonds do the following bonds do the following compounds have?compounds have?NH3 CH2O SiO2

Strength of Covalent Bonds

The strength of a covalent bond depends on how much distance separates the bonded nuclei.

This is known as bond length. Determined by size of the

atoms and how many electrons pairs are shared.

The shorter the bond length, the stronger the bond.

Single bonds, such as F2, are weaker than double bonds, such as those in O2.

Double bonds are weaker than triple bonds, such as N2.

Naming Molecules 9.2Naming Molecules 9.2

Rules to name binary molecular compounds.Rules to name binary molecular compounds. 1. The first element in the formula is always 1. The first element in the formula is always

named first, using the entire element name.named first, using the entire element name. 2. The second element in the formula is 2. The second element in the formula is

named using the root of the element and named using the root of the element and adding the adding the suffix –idesuffix –ide..

3. Prefixes are used to indicate the number 3. Prefixes are used to indicate the number of atoms of each type that are present in the of atoms of each type that are present in the compound. compound.

Prefixes in Covalent Prefixes in Covalent CompoundsCompounds

1 mono-1 mono- 2 di-2 di- 3 tri-3 tri- 4 tetra-4 tetra- 5 penta-5 penta- 6 hexa-6 hexa- 7 hepta-7 hepta- 8 octa-8 octa- 9 non-9 non- 10 deca10 deca One exception – the first element in the One exception – the first element in the

formula never uses the prefix mono-.formula never uses the prefix mono-. When the element name begins with a vowel When the element name begins with a vowel

drop the final letter in the prefix. CO carbon drop the final letter in the prefix. CO carbon monoxide not monocarbon monooxidemonoxide not monocarbon monooxide

Naming AcidsNaming Acidsbinary acidsbinary acids

A binary acid contains hydrogen and A binary acid contains hydrogen and one other element.one other element.

Use the prefix Use the prefix hydro-hydro- to name the to name the hydrogen.hydrogen.

Use the root of the second element Use the root of the second element plus the suffix -ic acid. HBr plus the suffix -ic acid. HBr hydrobromic acidhydrobromic acid

Naming OxyacidsNaming Oxyacids

Contains an oxyanion referred to as Contains an oxyanion referred to as oxyacids.oxyacids.

If anion suffix is -ate, it is replaced If anion suffix is -ate, it is replaced with the suffix -ic. HNOwith the suffix -ic. HNO33 (nitrate (nitrate ion) nitric acidion) nitric acid

If anion suffix is -ite, it is replaced If anion suffix is -ite, it is replaced with the suffix -ous. HNOwith the suffix -ous. HNO22 (nitrite (nitrite ion) nitrous acidion) nitrous acid

Writing Formulas from Writing Formulas from NamesNames

The name of any binary molecule The name of any binary molecule allows you to write the correct allows you to write the correct formula with ease.formula with ease.

Subscripts are determined from the Subscripts are determined from the prefixes used in the name because prefixes used in the name because the name indicates the exact number the name indicates the exact number of each atom present in the of each atom present in the molecule. Carbon Monoxide COmolecule. Carbon Monoxide CO

Coordinate Covalent Coordinate Covalent BondingBonding

A coordinate covalent A coordinate covalent bond occurs when one bond occurs when one atom gives both atom gives both electrons to a shared electrons to a shared pair between them.pair between them.

Coordinate Covalent Coordinate Covalent BondingBonding

In a line diagram, In a line diagram, instead of a straight instead of a straight line showing a shared line showing a shared pair, the coordinate pair, the coordinate covalent bond is covalent bond is shown as an arrow.shown as an arrow.

ResonanceResonanceIf you draw the covalent If you draw the covalent bonding diagram of some bonding diagram of some compounds there is not only compounds there is not only one way to draw it.one way to draw it.

ResonanceResonance There are two valid ways to show There are two valid ways to show

the structure of nitrite. The real the structure of nitrite. The real structure is an average of the two, structure is an average of the two, and this is called a and this is called a resonance resonance structurestructure. .

Resonance, cont.Resonance, cont.Earlier chemists thought the Earlier chemists thought the compound just quickly compound just quickly flipped back and forth flipped back and forth between the two structures between the two structures (or resonated).(or resonated).

This is proven to be untrue This is proven to be untrue now using bond lengths.now using bond lengths.

An Addendum to Lewis An Addendum to Lewis StructuresStructures

Carbon and silicon Carbon and silicon are exceptions to the are exceptions to the pattern of how to pattern of how to place electrons in a place electrons in a Lewis Dot Structure.Lewis Dot Structure.

An Addendum to Lewis An Addendum to Lewis StructuresStructures

This is because they This is because they have hybrid orbitals have hybrid orbitals (where the s and p (where the s and p sublevels blend sublevels blend together and have four together and have four equal energy orbitals.)equal energy orbitals.)

Drawing Dot DiagramsDrawing Dot Diagrams

A dot diagram shows the valence A dot diagram shows the valence electrons for an atomelectrons for an atom

First, write the symbol for the First, write the symbol for the element.element.

Then, put a dot to show each Then, put a dot to show each electron in the outer shell, in the electron in the outer shell, in the following order:following order:

X 1

285

7

46 3

The reason for this order, The reason for this order, is the first two spots for is the first two spots for electrons represent the electrons represent the

one orbital in the s one orbital in the s sublevel, the last three sublevel, the last three

spots represent the three spots represent the three orbitals of the p sublevel.orbitals of the p sublevel.

Your book’s way to Draw Your book’s way to Draw Lewis Dot StructuresLewis Dot Structures

1. Predict the location of certain atoms.1. Predict the location of certain atoms. a. Hydrogen is always a terminal.a. Hydrogen is always a terminal. b. The atom with the least attraction b. The atom with the least attraction

for shared electrons in the molecule is for shared electrons in the molecule is the central atom.the central atom.

2. Find the total number of electrons 2. Find the total number of electrons available for bonding. This total is the available for bonding. This total is the number of valence electrons in the number of valence electrons in the atoms in the molecule.atoms in the molecule.

3. Determine the number of bonding 3. Determine the number of bonding pairs by dividing the number of pairs by dividing the number of electrons available for electrons available for bonding by two.bonding by two.

4. Place one bonding pair (single bond) 4. Place one bonding pair (single bond) between the central atom and each of between the central atom and each of the terminal atoms.the terminal atoms.

5. Subtract the number of pairs you 5. Subtract the number of pairs you used in step 4 from the number of used in step 4 from the number of bonding pairs you determined in step 3.bonding pairs you determined in step 3.

6. If the central atom is not 6. If the central atom is not surrounded by four electron pairs, it surrounded by four electron pairs, it does not have an octet. You does not have an octet. You must must convert one or two of the lone pairs convert one or two of the lone pairs on the terminal atoms to a double on the terminal atoms to a double bond or a triple bond between the bond or a triple bond between the terminal atom and the central atomterminal atom and the central atom

Exceptions to the Octet Exceptions to the Octet RuleRule

Some molecules and ions do not Some molecules and ions do not obey the octet rule. Three reasons obey the octet rule. Three reasons exist for these exceptions.exist for these exceptions.

1. A small group of molecules has 1. A small group of molecules has an odd number of valence electrons an odd number of valence electrons and cannot form an octet around and cannot form an octet around each atom.each atom.

2. Coordinate covalent bond.2. Coordinate covalent bond.

3. The third group of compounds 3. The third group of compounds that does not follow the octet rule that does not follow the octet rule has central atoms that has central atoms that contain more contain more than eight valence. This electron than eight valence. This electron arrangement is referred to as an arrangement is referred to as an expanded octetexpanded octet..

Covalent Bonding and Covalent Bonding and Polyatomic IonsPolyatomic Ions

A polyatomic ion is A polyatomic ion is really just a really just a charged charged moleculemolecule that bonds that bonds ionically.ionically.

The charge signifies The charge signifies how many electrons how many electrons are given/taken away.are given/taken away.

Practice

CN-

SiF4

C2H4

NBr3

Chapter 9 Chapter 9 Notes Part IINotes Part II

VSEPR TheoryVSEPR Theory

The VSEPR TheoryThe VSEPR Theory

VSEPR stands for VSEPR stands for Valence Shell Electron Valence Shell Electron Pair Repulsion theoryPair Repulsion theory

All atoms have electrons All atoms have electrons orbiting the nucleusorbiting the nucleus

The VSEPR TheoryThe VSEPR TheoryThis creates several different This creates several different shapes that molecules can be shapes that molecules can be in.in.

These like charges repel, These like charges repel, causing the atoms bonded to causing the atoms bonded to the central atom to move as the central atom to move as far away from each other as far away from each other as possible.possible.

Shapes not involving Shapes not involving unshared pairs:unshared pairs:

The following shapes The following shapes come about from come about from compounds where the compounds where the central atom does not central atom does not have unshared pairs have unshared pairs of electrons:of electrons:

Shapes not involving Shapes not involving unshared pairs: unshared pairs:

LinearLinearTrigonal PlanarTrigonal PlanarTetrahedralTetrahedralTrigonal BipyramidalTrigonal Bipyramidal

LinearLinear

2 atoms off central, no 2 atoms off central, no unshared pairsunshared pairs

Ex: COEx: CO22

Bond Angle: 180Bond Angle: 180oo

Trigonal PlanarTrigonal Planar3 Atoms off 3 Atoms off central, no central, no unshared pairunshared pair

Ex: BFEx: BF33Bond Angle-120Bond Angle-120oo

TetrahedralTetrahedral4 Atoms off central, 4 Atoms off central, no unshared pairno unshared pair

Ex: CHEx: CH44

Bond Angles—109.5Bond Angles—109.5oo

Trigonal BipyramidalTrigonal Bipyramidal5 Atoms off 5 Atoms off central, no central, no unshared pairunshared pair

Ex: PClEx: PCl55

2 Bond Angles—2 Bond Angles—120120oo and 90 and 90oo

Shapes that involve an Shapes that involve an unshared pair:unshared pair:

These shapes are These shapes are altered by one or altered by one or more unshared pair more unshared pair on the central atom.on the central atom.BentBentPyramidalPyramidal

BentBent

2 Atoms off 2 Atoms off central, 1 or 2 central, 1 or 2 unshared pairunshared pair

Ex: HEx: H22OOBond Angles—Bond Angles—105105oo

PyramidalPyramidal3 Atoms off 3 Atoms off central, 1 central, 1 unshared pairunshared pair

Ex: NHEx: NH33

Bond Angles—107Bond Angles—107oo

Obj. 8…Obj. 8…IntraIntramolecular molecular Bonds vs. Bonds vs. InterIntermolecular molecular

AttractionAttraction• Intramolecular bondsIntramolecular bonds::

- bonds w/in a molecule- bonds w/in a molecule- i.e. holds H and O together in water (H- i.e. holds H and O together in water (H22O)O)

- ionic, covalent, polar covalent and metallic- ionic, covalent, polar covalent and metallic

• Intermolecular attractionIntermolecular attraction::- attraction b/n two or more different - attraction b/n two or more different molecules.molecules.- i.e. holds H- i.e. holds H22O molecules together in a pond.O molecules together in a pond.

** always weaker than intramolecular ** always weaker than intramolecular bonds.bonds.- strength indicates solid, liquid or gas.- strength indicates solid, liquid or gas.

Obj. 9-10…Intermolecular Obj. 9-10…Intermolecular AttractionsAttractions

• three types…three types…

- dispersion forces- dispersion forces- dipole interactions- dipole interactions

- Hydrogen bonds- Hydrogen bonds

van der Waals forcesvan der Waals forces((weakestweakest))

(strongest)(strongest)

• dispersion forces (DF)dispersion forces (DF)……

- seen in Halogen diatomic molecules - seen in Halogen diatomic molecules (Z(Z22))- strength of force as - strength of force as ## of e- in of e- in molecules molecules - F and Cl have few e- = weak DF (gases)- F and Cl have few e- = weak DF (gases) - Br has more e- = stronger DF (liquid)- Br has more e- = stronger DF (liquid) - I has most e- = strongest DF (solid)- I has most e- = strongest DF (solid)

Obj. 9-10 cont…Obj. 9-10 cont…• dipole interactionsdipole interactions……

- slightly (-) pole attracted to (+) pole of - slightly (-) pole attracted to (+) pole of anotheranothermolecule.molecule.- similar to but much weaker than ionic bonds- similar to but much weaker than ionic bonds

Obj. 9-10 cont…Obj. 9-10 cont…• Hydrogen bondsHydrogen bonds……

- strong attraction b/n H on one polar molecule- strong attraction b/n H on one polar moleculeand the e- of an electronegative atom (N,O, or F)and the e- of an electronegative atom (N,O, or F)from a different molecule.from a different molecule.- H atom is forced to share its only e-- H atom is forced to share its only e-- H is therefore very attracted to pair of e- in- H is therefore very attracted to pair of e- inneighboring molecule.neighboring molecule.

Obj. 9-10 cont…Obj. 9-10 cont…• bond strengths…bond strengths…

dispersion forcesdispersion forces

dipole interactionsdipole interactions

Hydrogen bondsHydrogen bonds

Covalent bondsCovalent bonds

Metallic bondsMetallic bonds

Ionic bondsIonic bonds

van der Waalsvan der Waals interintermolecularmolecular

intraintramolecularmolecular

WEAKESTWEAKEST

STRONGESTSTRONGEST

(Pure and Polar)(Pure and Polar)

Chapter 9 Notes, Chapter 9 Notes, part IIIpart III

Bond Polarity and Bond Polarity and Molecular PolarityMolecular Polarity

Types of BondsTypes of Bonds

Up until now, we have Up until now, we have assumed that there are two assumed that there are two types of bonds: Covalent and types of bonds: Covalent and Ionic.Ionic.

This is true, but covalent This is true, but covalent bonds can be broken into bonds can be broken into two categoriestwo categories

Nonpolar CovalentNonpolar CovalentIn nonpolar covalent bonding In nonpolar covalent bonding electrons are shared electrons are shared equallyequally..

Electrons spend an equal Electrons spend an equal amount of time with both amount of time with both elements in the bond.elements in the bond.

Typical in diatomic elements:Typical in diatomic elements:

BrBr22, I, I22, N, N22, Cl, Cl22, H, H22 O O22, F, F22, ,

Polar CovalentPolar Covalent In polar covalent bonding, In polar covalent bonding, electrons are still shared, but they electrons are still shared, but they are shared are shared unequallyunequally..

This is due to one nucleus pulling This is due to one nucleus pulling the shared pair harder than the the shared pair harder than the other.other.

This creates a This creates a dipoledipole—a bond —a bond where one side is slightly positive where one side is slightly positive and the other is slightly negative.and the other is slightly negative.

A dipole is caused A dipole is caused because the electron because the electron spends more time on one spends more time on one side than the other.side than the other.

The polarity of the bond The polarity of the bond is shown like:is shown like:

Polar CovalentPolar Covalent

H—Cl H—Cl + -

OR

Ionic BondsIonic BondsIn an ionic bond, In an ionic bond, electrons are electrons are transferredtransferred..

The nucleus of one The nucleus of one element pulls hard element pulls hard enough to take electrons enough to take electrons away completely.away completely.

How can you tell what How can you tell what kind of bond there is?kind of bond there is?

By looking at the difference in By looking at the difference in electronegativity!electronegativity!

Remember, electronegativity Remember, electronegativity is the tendency of an atom to is the tendency of an atom to attract an electron when attract an electron when bonding.bonding.

The more electronegative, the The more electronegative, the more it will pull electrons.more it will pull electrons.

- highest electronegativity diff. (ED - highest electronegativity diff. (ED 1.67) 1.67)Ionic BondsIonic Bonds

Ex…Ex… NaCl:NaCl: NaNa++ = 0.9 = 0.9 ClCl-- = 3.0 = 3.0 3.0 – 0.9 = 3.0 – 0.9 = 2.12.1

KBr:KBr: KK++ = 0.8 = 0.8 BrBr-- = 2.8 = 2.8 2.8 – 0.8 = 2.8 – 0.8 = 2.02.0

Polar Covalent BondsPolar Covalent Bonds - lowest electronegativity diff. (ED - lowest electronegativity diff. (ED 0.4) 0.4)

Ex…Ex… HH22:: HH++ = 2.1 = 2.1 HH++ = 2.1 = 2.1 2.1 – 2.1 = 2.1 – 2.1 = 00

CHCH44:: C = 2.5C = 2.5 HH++ = 2.1 = 2.1 2.5 – 2.1 = 2.5 – 2.1 = 0.40.4

Nonpolar Covalent BondsNonpolar Covalent Bonds - int. electronegativity diff. (ED 0.41 - 1.66)- int. electronegativity diff. (ED 0.41 - 1.66)

Ex…Ex… HH22O:O: H = 2.1H = 2.1 O = 3.5O = 3.5 3.5 – 2.1 = 3.5 – 2.1 = 1.41.4

COCO22:: C = 2.5C = 2.5 O = 3.5O = 3.5 3.5 – 2.5 = 3.5 – 2.5 = 1.01.0

Nonpolar Bonds:

EN Diff ≤ 0.4Polar Bonds:

0.4 < EN Diff ≤ 1.7 Ionic Bonds:

EN Diff > 1.7

PracticePractice

• Identify bond Identify bond types…types… HBrHBr

KClKCl

COCO22

2.8 – 2.1 =2.8 – 2.1 =0.70.7PCPC

3.0 – 0.8 =3.0 – 0.8 = 2.22.2II

3.5 – 2.5 =3.5 – 2.5 = 1.01.0PCPC

LiLi22OO 3.5 – 1.0 =3.5 – 1.0 =2.52.5II

BrBr22 2.8 – 2.8 =2.8 – 2.8 = 00

• Rank polarities… Rank polarities… 11 = least polar… = least polar…55 = most polar = most polar

11

22

33

44

55

CC

What type of bond is What type of bond is between:between:

H and ClH and ClLi and ClLi and ClC and SC and SF and OF and O

What type of bond is What type of bond is between:between:

N and Br N and Br Na and FNa and FC and OC and O

Polar MoleculesPolar MoleculesIf the slightly positive If the slightly positive and slightly negative and slightly negative ends of polar bonds can ends of polar bonds can collect on two different collect on two different sides of a molecule, it sides of a molecule, it can make an entire can make an entire molecule polar.molecule polar.

Polar MoleculesPolar Molecules

If bonds are If bonds are nonpolar, a molecule nonpolar, a molecule will always be will always be nonpolar.nonpolar.

Polar MoleculesPolar Molecules If bonds are polar and the shape of a If bonds are polar and the shape of a

molecule is symmetrical, the molecule is symmetrical, the molecule will be nonpolar because molecule will be nonpolar because the charges cancel out.the charges cancel out.

(Linear, trigonal planar, tetrahedral (Linear, trigonal planar, tetrahedral and trigonal bipyramidal are the and trigonal bipyramidal are the symmetrical shapes we talked about.)symmetrical shapes we talked about.)

Polar MoleculesPolar MoleculesIf bonds are polar and the If bonds are polar and the molecule is asymmetrical, molecule is asymmetrical, the molecule will be polar!the molecule will be polar!

(Bent and pyramidal (Bent and pyramidal molecules are molecules are asymmetrical)asymmetrical)