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Introduction to Chemical Bonding: Ionic, Covalent, and Metallic Bonds, Study notes of Chemistry

Coventry UniversityChemistry

An introduction to chemical bonding, discussing the different types of bonds including ionic, covalent, and metallic bonds. It covers the philosophies of atom to atom interaction, the role of electro-negativity, and the formation of bonds between different elements. It also includes examples and illustrations.

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BONDING
Notes
BONDING
Notes
Mr. BuchananMr. Buchanan
ā€¢ Atoms are generally found in nature in
combination held together by chemical
bonds.
ā€¢ A chemical bond is a mutual electrical
attraction between the nuclei and
valence electrons of different atoms
that binds the atoms together.
ā€¢ There are three main types of
bonding: ionic, metallic and covalent.
ā€¢ Atoms are generally found in nature in
combination held together by chemical
bonds.
ā€¢ A chemical bond is a mutual electrical
attraction between the nuclei and
valence electrons of different atoms
that binds the atoms together.
ā€¢ There are three main types of
bonding: ionic, metallic and covalent.
Introduction to BondingIntroduction to Bonding
ā€¢ Ionic Bonding occurs between a
metal and a nonmetal.
ā€¢ Metallic bonding occurs between
two metals .
ā€¢ Covalent bonding occurs between a
nonmetal and a nonmetal.
ā€¢ A positive ion is called a cation.
ā€¢ A negative ion is called an anion.
ā€¢ Ionic Bonding occurs between a
metal and a nonmetal.
ā€¢ Metallic bonding occurs between
two metals .
ā€¢ Covalent bonding occurs between a
nonmetal and a nonmetal.
ā€¢ A positive ion is called a cation.
ā€¢ A negative ion is called an anion.
Introduction to BondingIntroduction to Bonding
What determines the type of bond
that forms?
ā€¢ The valence electrons of the two atoms
involved are redistributed to the most stable
arrangement.
ā€¢ The interaction and rearrangement of the
valence electrons determines which type of
bond that forms.
ā€¢ Before bonding the atoms are at their
highest possible potential energy
What determines the type of bond
that forms?
ā€¢ The valence electrons of the two atoms
involved are redistributed to the most stable
arrangement.
ā€¢ The interaction and rearrangement of the
valence electrons determines which type of
bond that forms.
ā€¢ Before bonding the atoms are at their
highest possible potential energy
Introduction to BondingIntroduction to Bonding
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BONDING

Notes

BONDING

Notes

Mr. BuchananMr. Buchanan

  • Atoms are generally found in nature in combination held together by chemical bonds.
  • A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
  • There are three main types of bonding: ionic, metallic and covalent.
  • Atoms are generally found in nature in combination held together by chemical bonds.
  • A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
  • There are three main types of bonding: ionic, metallic and covalent.

Introduction to BondingIntroduction to Bonding

  • Ionic Bonding occurs between a metal and a nonmetal.
  • Metallic bonding occurs between two metals.
  • Covalent bonding occurs between a nonmetal and a nonmetal.
  • A positive ion is called a cation.
  • A negative ion is called an anion.
  • Ionic Bonding occurs between a metal and a nonmetal.
  • Metallic bonding occurs between two metals.
  • Covalent bonding occurs between a nonmetal and a nonmetal.
  • A positive ion is called a cation.
  • A negative ion is called an anion.

Introduction to BondingIntroduction to Bonding

What determines the type of bond

that forms?

  • The valence electrons of the two atoms involved are redistributed to the most stable arrangement.
  • The interaction and rearrangement of the valence electrons determines which type of bond that forms.
  • Before bonding the atoms are at their highest possible potential energy

What determines the type of bond

that forms?

  • The valence electrons of the two atoms involved are redistributed to the most stable arrangement.
  • The interaction and rearrangement of the valence electrons determines which type of bond that forms.
  • Before bonding the atoms are at their highest possible potential energy

Introduction to BondingIntroduction to Bonding

  • There are 2 philosophies of atom to atom interaction - One understanding of the formation of a chemical bond deals with balancing the opposing forces of repulsion and attraction
  • Repulsion occurs between the negative e - clouds of each atom
  • Attraction occurs between the positive nuclei and the negative electron clouds
  • There are 2 philosophies of atom to atom interaction - One understanding of the formation of a chemical bond deals with balancing the opposing forces of repulsion and attraction
  • Repulsion occurs between the negative e - clouds of each atom
  • Attraction occurs between the positive nuclei and the negative electron clouds

Introduction to BondingIntroduction to Bonding

  • When two atoms approach each other closely enough for their electron clouds to begin to overlap - The electrons of one atom begin to repel the electrons of the other atom - And repulsion occurs between the nuclei of the two atoms
  • When two atoms approach each other closely enough for their electron clouds to begin to overlap - The electrons of one atom begin to repel the electrons of the other atom - And repulsion occurs between the nuclei of the two atoms

Introduction to BondingIntroduction to Bonding

  • As the optimum distance is achieved that balances these forces, there is a release of potential energy - The atoms vibrate within the window of maximum attraction/minimum repulsion
  • The more energy released the stronger the connecting bond between the atoms
  • As the optimum distance is achieved that balances these forces, there is a release of potential energy - The atoms vibrate within the window of maximum attraction/minimum repulsion
  • The more energy released the stronger the connecting bond between the atoms

Introduction to BondingIntroduction to Bonding

  • Another understanding of the form- ation of a chemical bond between two atoms centers on achieving the most stable arrangement of the atomsā€™ valence electrons - By rearranging the electrons so that each atom achieves a noble gas-like arrangement of its electrons creates a pair of stable atoms (only occurs when bonded)
  • Another understanding of the form- ation of a chemical bond between two atoms centers on achieving the most stable arrangement of the atomsā€™ valence electrons - By rearranging the electrons so that each atom achieves a noble gas-like arrangement of its electrons creates a pair of stable atoms (only occurs when bonded)

Introduction to BondingIntroduction to Bonding

  • The take home lesson on electro- negativity and bonding is this: - The closer together the atoms are on the P.T., the more evenly their e- interact, and are therefore more likely to form a covalent bond - The farther apart they are on the P.T., the less evenly their e -^ interact, and are therefore more likely to form an ionic bond.
  • The take home lesson on electro- negativity and bonding is this: - The closer together the atoms are on the P.T., the more evenly their e- interact, and are therefore more likely to form a covalent bond - The farther apart they are on the P.T., the less evenly their e -^ interact, and are therefore more likely to form an ionic bond. (^) metal w/nonmetal = ionicmetal w/nonmetal = ionic nonmetal w/nonmetal = covalentnonmetal w/nonmetal = covalent

Introduction to BondingIntroduction to Bonding

Ionic BondsIonic Bonds

  • Forming ionic bonds can be represented as a transfer of electrons. .. to give Na +^ :Cl: - .. Simply as Na +^ Cl- or NaCl
  • Forming ionic bonds can be represented as a transfer of electrons. .. to give Na +^ :Cl: - .. Simply as Na +^ Cl- or NaCl

Covalent BondingCovalent Bonding

  • In a covalent bond:
    • The electro-negativity difference between the atoms involved is not extreme - So the interaction between the involved electrons is more like a sharing relationship
    • It may not be an equal sharing relationship, but at least the electrons are being ā€œsharedā€.
  • In a covalent bond:
    • The electro-negativity difference between the atoms involved is not extreme - So the interaction between the involved electrons is more like a sharing relationship
    • It may not be an equal sharing relationship, but at least the electrons are being ā€œsharedā€.

Covalent BondingCovalent Bonding

  • Covalent Bonding is between two or more non-metals.
  • Covalent bonds are formed when electrons are shared between two atoms.
  • If they share 2 electrons, they form a single bond; 4 electrons is a double bond;
  • If two atoms share 6 electrons, they form a triple bond.
  • Covalent Bonding is between two or more non-metals.
  • Covalent bonds are formed when electrons are shared between two atoms.
  • If they share 2 electrons, they form a single bond; 4 electrons is a double bond;
  • If two atoms share 6 electrons, they form a triple bond.

Covalent BondingCovalent Bonding

  • Polar bonds usually involve nitrogen, oxygen or fluorine (NOF)
  • Non-Polar bonds usually involve carbon-hydrogen bonds
  • In polar bonds, the electrons are shared unequally
  • In non-polar bonds, the electrons are shared equally.
  • Covalent compounds can exist in any state (solid, liquid or gas). They have low melting and boiling points.
  • Polar bonds usually involve nitrogen, oxygen or fluorine (NOF)
  • Non-Polar bonds usually involve carbon-hydrogen bonds
  • In polar bonds, the electrons are shared unequally
  • In non-polar bonds, the electrons are shared equally.
  • Covalent compounds can exist in any state (solid, liquid or gas). They have low melting and boiling points.

Covalent BondingCovalent Bonding

Lets look at the molecule ClLets look at the molecule Cl (^2 )

Covalent BondsCovalent Bonds

ClCl

Shared Electrons

Shared Electrons

ClCl ClCl ClCl

Valence electrons for ElementsValence electrons for Elements

Recall that the valence electrons for the elements can be determined based on the elements position on the periodic table. Examples of Lewis Dot Symbol

Recall that the valence electrons for the elements can be determined based on the elements position on the periodic table. Examples of Lewis Dot Symbol

BondsBonds

  • Atoms can share more than one electron pair.
  • They may double or triple up pairs of electrons to satisfy the octet rule.
  • A Single bond is the sharing of one pair of electrons between two atoms.
  • A Double bond is the sharing of two pairs of electrons between two atoms.
  • A Triple bond is the sharing of three pairs of electrons between two atoms.

Valence electrons and number of bondsValence electrons and number of bonds Number of bonds element can form depends on the number of valence electrons. Number of bonds element can form depends on the number of valence electrons.

X

Fam i l y (^) ļ‚® # C ov al en t Bon d s* H al ogen s F, B r, C l , I C al cogen s O , S N i tr ogen N , P C arb on C , Si ļ‚®

O

N

C

ļ‚®

ļ‚®

ļ‚® 1 bond often

2 bond often

3 bond often

4 bond always The above chart is a guide on the number of bonds formed by these atoms.

In general -

BondsBonds

4 bonds 3 bonds 2 bonds 1 bond O=C=O Nļ‚ŗļ€ N O = O :F ā€“ F:

4 bonds 3 bonds 2 bonds 1 bond O=C=O ::Nļ‚ŗļ€ N :: O = O :F ā€“ F:::

Rules for Writing Lewis StructuresRules for Writing Lewis Structures

  1. Determine whether the compound is covalent or ionic. If covalent, treat the entire molecule. If ionic, treat each ion separately.
  2. Determine the total number of valence electrons available to the molecule or ion by summing the valence electrons of all the atoms in the unit.
  3. Organize the atoms so there is a central atom (usually the least electronegative) surrounded by ligand (outer) atoms. Hydrogen is never the central atom.
  4. Determine whether the compound is covalent or ionic. If covalent, treat the entire molecule. If ionic, treat each ion separately.
  5. Determine the total number of valence electrons available to the molecule or ion by summing the valence electrons of all the atoms in the unit.
  6. Organize the atoms so there is a central atom (usually the least electronegative) surrounded by ligand (outer) atoms. Hydrogen is never the central atom.

BondsBonds

  • So forming covalent bonds can be shown as
  • So forming covalent bonds can be shown as

To be stable the two atoms

involved in the covalent bond

share their electrons in order

to achieve the arrangement

of a noble gas.

To be stable the two atoms

involved in the covalent bond

share their electrons in order

to achieve the arrangement

of a noble gas.

So whatā€™s the bottom line? Ionic BondingIonic Bonding

**-

  • -**^ **- -
  • -**

- -^ - -

- -^

-^ -

-

Notice 8 e -^ in each valence shell!!!

Both atoms are happy, they both achieve the electron arrangement of a noble gas.

Both atoms are happy, they both achieve the electron arrangement of a noble gas.

Very Strong Electrostatic attraction establishedā€¦

IONIC BONDS

To be stable the two atoms

involved in the ionic bond will

either lose or gain their valence

electrons in order to achieve a

stable octet arrangement of

electrons.

To be stable the two atoms

involved in the ionic bond will

either lose or gain their valence

electrons in order to achieve a

stable octet arrangement of

electrons.

So whatā€™s the bottom line?

Metallic BondingMetallic Bonding

Metallic BondingMetallic Bonding

  • The metallic bond consists of

positively charged metallic cations

that donate electrons to the sea.

  • The sea of electrons are shared by

all atoms and can move throughout

the structure.

  • The metallic bond consists of

positively charged metallic cations

that donate electrons to the sea.

  • The sea of electrons are shared by

all atoms and can move throughout

the structure.

Metallic BondingMetallic Bonding Metallic BondingMetallic Bonding

  • In a metallic bond:
    • The resulting bond is a cross between covalent and ionic bonding - Valence electrons are transferred from one metal atom to the surrounding metal atoms - But none of the involved metal atoms want the electrons from the original atom, nor their own so they pass them on
  • In a metallic bond:
    • The resulting bond is a cross between covalent and ionic bonding - Valence electrons are transferred from one metal atom to the surrounding metal atoms - But none of the involved metal atoms want the electrons from the original atom, nor their own so they pass them on