Bonding (Unit 2)

Two Bonds

Linear

Two Bonds (Angle)

180°

Three Bonds

Trigonal Planar

Three Bonds (Angle)

120°

Two Bonds, One Lone Pair

Bent

Two Bonds, One Lone Pair (Angle)

116°

Four Bonds

Tetrahedral

Four Bonds (Angle)

109.5°

Three Bonds, One Lone Pair

Trigonal Pyramidal

Three Bonds, One Lone Pair (Angle)

107°

Two Bonds, Two Lone Pairs

Bent

Two Bonds, Two Lone Pairs (Angle)

104.5°

One/Two Bonds Electron Geometry

Linear

Three Things Electron Geometry

Trigonal Planar

Four Things Electron Geometry

Tetrahedral

P/NP: Linear

Nonpolar

P/NP: Trigonal Planar

Nonpolar

P/NP: Tetrahedral

Nonpolar

P/NP: Bent

Polar

P/NP: Trigonal Pyramidal

Polar

Nonpolar Exception

All nonpolar shapes are polar if the terminal (outside) elements are different elements

Polarity

Bonds are never completely ionic or covalent

Nonpolar Covalent

Electrons are shared equallyN

Nonpolar Covalent Electronegativity Difference

0-0.04

Polar Covalent

Electrons are shared unequally (one atom pulls harder than the other)

Polar Covalent Electronegativity Difference

0.5-1.7

Ionic

Electrons are transferred (one atom pulls on the electrons so much harder than the other that it steals an electron from the other atom (not all metal/nonmetal bonds are ionic)

Ionic Electronegativity Difference

>1.7

Polar Molecule

Electrons are concentrated in one part of the molecule, dipoles DON’T cancel out

Nonpolar Molecule

Electrons are pulled equally in all directions, the bonds in the molecule would be nonpolar too, dipoles DON’T cancel out

One

Mono

Two

Di

Three

Tri

Four

Tetra

Five

Penta

Six

Hexa

Seven

Hepta

Eight

Octa

Nine

Nona

Ten

Deca

Electron Sea Model

Metal atoms in a metallic solid contribute their valence electrons to form a “sea” of delocalized electrons

Delocalized Electrons

Electrons that are free to move from one atom to the next

Metallic Bond

Attraction between a metal cation and delocalized electrons

Properties of Metals

• Delocalized electrons allow metals to conduct electricity (movement of electrons) and heat

• High melting and boiling points (metallic bonds=opposite charges)

• Malleable and ductile

Alloy

Mixture of elements that have metallic properties (stainless steel, brass, cast iron, etc.)

Lattice Energy

• The energy required the separate one mole of the ions of an ionic compound (higher lattice energy → harder to separate ions/more stable crystal)

• Inversely related to the size (radius) of the ions bonded

• The smaller the ions, the closer they are to each other, and the harder they are to separate, so the greater the lattice energy

• The larger the value of the charge, the greater the lattice energy

Physical Property

Something that can be observed without changing the identity of the substance, can use your 5 sense to observe, when you test a physical property, nothing new is made (no chemical reactions occurs)

Magnetism

Physical Property

Conductivity

Physical Property

Melting Point

Physical Property

Boiling Point

Physical Property

Malleability

Physical Property

Intrinsive Property

Independent of the amount of substance present

Scent

Intrinsive (Physical) Property

Density

Intrinsive (Physical) Property

Extensive Property

Depends on the amount of substance present

Mass

Extensive (Physical) Property

Length

Extensive (Physical) Property

Volume

Extensive (Physical) Property

Physical Change

A change in a physical property (appearance or state of matter), the identity of the substance is NOT changedB

Breaking

Physical Change

Cutting

Physical Change

Dissolving

Physical Change

Changing States of Matter

Physical Change

Chemical Property

Ability or inability of a substance to react with another substance, when you test it a reaction happens/something new is made

Chemical Change

When a new substance is made (when a chemical reaction happens)

Ability to Rust

Chemical Property

Ability to Burn

Chemical Property

Acidity

Chemical Property

Flammability

Chemical Property

Burning/Exploding

Chemical Change

Rusting/Tarnishing

Chemical Change

Cooking

Chemical Change

Oxidizing

Chemical Change

Corroding

Chemical Change

Rotting

Chemical Change

Signs of a Chemical Change

Color change, bubbles form (NOT BOILING), heat absorbed/released, NEW odor generated, light emitted (burning), solid (precipitate forms/forming a solid)

Law of Conservation of Mass

Mass is neither created nor destroyed in a chemical reaction, mass of reactants=mass of products

Matter

Any material that has mass/takes up space

Pure Substance

Matter with a fixed composition

Water

Pure Substance

Gold

Pure Substance

CO2

Pure SubstanceE

Elements

Contain only one type of matter

Oxygen

Element

Silver

Element

Atom

The smallest particle of an element that retains the characteristics of that element

Compound

Two or more elements combined with a definite composition

H20

Compound

NaCl

Compound

Molecule

Two or more atoms bonded together, can make up elements or compounds

Mixture

A physical combination of substances that does not change the identities of the mixed substances

Brass

Mixture

Homogeneous

Two or more substances that are uniformly mixed

Bronze salt dissolved in water

Homogeneous

Heterogeneous

Two or more substances that are NOT uniformly mixed

Italian dressing

Heterogeneous

Sigma Bond

Single bond

Pi Bond

Second bond and any other bond after first bondR

Resonance Structures

Drawn when there are multiple correct structures for a molecule or polyatomic ion, only differ in position of electron pairs, not position of atoms, molecules and polyatomic ions that exhibit resonance behave as though there is only structure