Chapter 9 Chemical Bonding

Electronegativity

A measure of the ability of an atom in a bond to attract electrons.

Metallic Bond

The interaction that holds metal atoms together, resulting from a 'sea of electrons' shared by all metal atoms.

Ionic Bond

Formed when there is a complete transfer of electrons from one atom to another, resulting in electrostatic attraction between oppositely charged ions.

Covalent Bond

A bond formed by the sharing of valence electrons between two nonmetal atoms.

Polar Covalent Bond

A type of bond where electrons are shared unequally between two atoms, resulting in partial charges.

Nonpolar Covalent Bond

A bond in which electrons are shared equally between two atoms, resulting in no significant charge separation.

Lewis Dot Diagrams

Diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory that predicts the three-dimensional shape of molecules based on electron pair repulsion.

Bond Length

The distance between the nuclei of two bonded atoms, usually measured in picometers.

Bond Angle

The angle formed between three atoms in a molecule, typically centered on a central atom.

Core Electrons

Electrons located in energy levels below the outermost energy level.

Valence Electrons

The electrons in the outer energy level that are involved in chemical bonding.

Shielding Effect

The phenomenon where inner electrons block the attraction between the nucleus and the valence electrons.

A decrease in the attraction exerted by the atomic nucleus on valence electrons

Noble Gas Configuration

A stable electron arrangement resembling that of noble gases, typically having eight electrons in the outer shell.

Periodic Trends

Patterns observed in the properties of elements, including electronegativity, atomic radius, and ionization energy.

Ionic Character

The degree to which a chemical bond is ionic in nature, often determined by the difference in electronegativity.

Hybridization

The concept of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds.

partial charge

symbolized by δ- δ+

ductility

ability to be drawn into a thin wire

malleability

the ability of a material to deform under compressive stress, often resulting in a change in shape without breaking. OFTEN ROLLED INTO A THIN SHEET

conductivity

the ability of a material to conduct electric current or heat.

LINEAR SHAPE

• 180

• 2 total electron pairs

• 2 bonded

• 0 lone pairs

TRIGONAL PLANAR

• 3 total electron pairs

• 3 shared pairs

• 0 lone pairs

• 120*

BENT (<120)

• 3 total electron pairs

• 2 shared pairs

• 1 lone pair

• (<120*)

Tetraherdal

• 4 electron pairs

• 4 shared pairs

• 0 lone pairs

• 109.5*

Triginal Pyramidal

• 4 total electron pairs

• 3 shared pairs

• 1 lone pair

• 107*

Bent

• 4 electron pairs

• 2 shared pairs

• 2 long pairs

• 104.5

A vaule of 0.3 for ΔEN of atoms of two elements suggest that the bond between them is ____________

NONPOLAR COVALENT BOND

a bond is considered to be ionic if the differnece in electornegtaivities between the two atoms of which is formed: ____________

GREATER THEN 2.0

In ΔEN the greek symbol Δ represnets

DIFFERENCE

The valence electrons in a metal………..

are shared among other electorns

diatomic molecules of elements always have:

NONPOLAR COVALENT BONDS

In moving from left to right in a row of the perodic table, electronegativties tend to: 1. _______ and the sheilding effect tends to 2.______________

1. increase

2. stay the same

In moving from top to bottom, in a column near the right edge of the periodic table electronegativities tend to 1. and the shield effect tends to 2.

1. decrease

2. increase

The bond in a nitrogen molecule is:

nonpolar covalent bond

hydrogen chloride is a(n) ________ substance

polar

in a water molecule the two colevents bonds are are in _________a straight line

at 105* to each other

of the four pairs of valence electrons in the water molecule, how mnay pairs are in the bonding?

two pairs

of the four pairs of valence electrons, how many pairs contribute to the shape?

FOUR

the relatively high boiling point of water is due to

the polarity of the water molecule

the presence of of a double bond in a molecule that

two pairs of electrons are shared